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305 Cards in this Set
- Front
- Back
- 3rd side (hint)
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What happens when a solid melts? |
Its particles gain enough energy to overcome the weak forces of attraction between them. |
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Why do mixtures melt over a range of temperatures whilst pure substances have precise melting points? |
Pure substances have properties that are constant throughout meaning they have a sharp melting a boiling point whilst mixtures do not have constant properties. |
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What is crystallisation? |
When solutes (dissolved substances) are separated from a solution by evaporating the solvent to leave solutes behind. |
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What is solution mining? |
This is when water is pumped into layers of salt underground. That solution is then heated which evaporates the solvent and is filtered until salt residue is left that can be collected. |
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How does filtration and crystallisation work in a lab? |
First a filter funnel is lined with filter paper that is fine holes in it. The solutes pass through them, but the minuscule particles that don’t remain in the filter paper. A bunsen burner is then used to gently heat and evaporate the filtrate until residue that can become crystals is left. |
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What can chromatography be used for? |
It can be used to find out the different coloured compounds a mixture contains. |
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Why do solvents move at different speeds along a strip of paper? |
Each solvent carries different substances which is why they’re separated |
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State the equation used to find the Rf value |
Distance moved by the spot Rf = ———————————— Distance moved by the solvent |
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What can paper chromatography be used for? |
Distinguishing pure/impure substances Identifying substances by comparing different patterns Identifying substances by calculating their Rf values |
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If two dyes have the same Rf value, are they the same? |
They are likely but not necessarily the same compound. |
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Z |
Z |
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Describe the process of distillation |
When water evaporates in a mixture, only the liquid turns into a gas and the solid minerals are left behind. The condensed water is now pure. |
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Describe the process of distillation |
When water evaporates in a mixture, only the liquid turns into a gas and the solid minerals are left behind. The condensed water is now pure. |
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Why is a simple still not efficient? |
A lot of vapour is lost in the delivery tube |
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What can fractional distillation be used for? |
To separate the products in crude oil To make a alcoholic drinks To separate gases in the air after it’s been cooled |
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What can fractional distillation be used for? |
To separate the products in crude oil To make a alcoholic drinks To separate gases in the air after it’s been cooled |
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What is desalination and how can it be done? |
Producing pure water from sea water. It can be achieved using simple distillation |
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Describe the process of simple distillation |
Sea water is heated so that vapour leaves it quickly and then vapour is then cooled and condensed forming pure water |
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What is a downside of simple distillation? |
It requires a lot of energy so it’s not applicable to large amounts of drinking water. |
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What is a downside of simple distillation? |
It requires a lot of energy so it’s not applicable to large amounts of drinking water. |
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What is chemical analysis? |
This involves using chemical reactions or sensitive machines to identify and measure the substances in a sample |
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What is a downside of simple distillation? |
It requires a lot of energy so it’s not applicable to large amounts of drinking water. |
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What is chemical analysis? |
This involves using chemical reactions or sensitive machines to identify and measure the substances in a sample |
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Describe the process of sedimentation |
Fresh water with objects in it such as leaves, twigs and other minuscule particles are put into a sedimentation tank where they’re filtered through sand and gravel. This is where small particles my settle out. Chlorine is then added to kill bacteria. That drinking water is finally stored in a tower and can be used in homes and industries. |
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Suggest two reasons why samples of treated water is tested regularly |
To ensure water is suitable for the intended use and to determine how effective the treatment system they’ve used is. |
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Suggest two reasons why samples of treated water is tested regularly |
To ensure water is suitable for the intended use and to determine how effective the treatment system they’ve used is. |
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How did Ernest Rutherford prove that atoms are mostly empty space and that the nucleus in an atom carries the most mass? |
Positive particles were fired at thin gold foil and most of them passed straight through the foil. Very few were deflected or bounced back. |
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Suggest two reasons why samples of treated water is tested regularly |
To ensure water is suitable for the intended use and to determine how effective the treatment system they’ve used is. |
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How did Ernest Rutherford prove that atoms are mostly empty space and that the nucleus in an atom carries the most mass? |
Positive particles were fired at thin gold foil and most of them passed straight through the foil. Very few were deflected or bounced back. |
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How was nuclear energy discovered? |
By firing neutrons at uranium-235 it was discovered that a nucleus can be split (nuclear fission) which produces new elements and transfers large amounts of energy. |
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Suggest two reasons why samples of treated water is tested regularly |
To ensure water is suitable for the intended use and to determine how effective the treatment system they’ve used is. |
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How did Ernest Rutherford prove that atoms are mostly empty space and that the nucleus in an atom carries the most mass? |
Positive particles were fired at thin gold foil and most of them passed straight through the foil. Very few were deflected or bounced back. |
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How was nuclear energy discovered? |
By firing neutrons at uranium-235 it was discovered that a nucleus can be split (nuclear fission) which produces new elements and transfers large amounts of energy. |
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State the formula for relative atomic mass |
total mass of atoms Ar = ————————— no. of atoms |
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Suggest two reasons why samples of treated water is tested regularly |
To ensure water is suitable for the intended use and to determine how effective the treatment system they’ve used is. |
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How did Ernest Rutherford prove that atoms are mostly empty space and that the nucleus in an atom carries the most mass? |
Positive particles were fired at thin gold foil and most of them passed straight through the foil. Very few were deflected or bounced back. |
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How was nuclear energy discovered? |
By firing neutrons at uranium-235 it was discovered that a nucleus can be split (nuclear fission) which produces new elements and transfers large amounts of energy. |
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State the formula for relative atomic mass |
total mass of atoms Ar = ————————— no. of atoms |
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What does the electronic configuration show? |
How many electrons occupy a shell |
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How do bonds make atoms stable? |
Energy is released from the atoms when they bond making them more stable and less reactive |
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How do bonds make atoms stable? |
Energy is released from the atoms when they bond making them more stable and less reactive |
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How are ions formed? |
The transfer of electrons between atoms formed charged particles called ions |
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How do bonds make atoms stable? |
Energy is released from the atoms when they bond making them more stable and less reactive |
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How are ions formed? |
The transfer of electrons between atoms formed charged particles called ions |
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Describe how cations and anions are formed |
Cations are formed when metal atoms lose electrons and form positive ions. Anions are formed when non-metal gain electrons and form negative ions. |
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How do bonds make atoms stable? |
Energy is released from the atoms when they bond making them more stable and less reactive |
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How are ions formed? |
The transfer of electrons between atoms formed charged particles called ions |
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Describe how cations and anions are formed |
Cations are formed when metal atoms lose electrons and form positive ions. Anions are formed when non-metal gain electrons and form negative ions. |
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What holds ions together in an ionic bond? |
Electrostatic forces that hold the oppositely charged ions together |
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How do bonds make atoms stable? |
Energy is released from the atoms when they bond making them more stable and less reactive |
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How are ions formed? |
The transfer of electrons between atoms formed charged particles called ions |
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Describe how cations and anions are formed |
Cations are formed when metal atoms lose electrons and form positive ions. Anions are formed when non-metal gain electrons and form negative ions. |
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What holds ions together in an ionic bond? |
Electrostatic forces that hold the oppositely charged ions together |
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True or false? Atoms that easily form ions will either have a nearly full or nearly empty electron shell. |
True |
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How do bonds make atoms stable? |
Energy is released from the atoms when they bond making them more stable and less reactive |
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How are ions formed? |
The transfer of electrons between atoms formed charged particles called ions |
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Describe how cations and anions are formed |
Cations are formed when metal atoms lose electrons and form positive ions. Anions are formed when non-metal gain electrons and form negative ions. |
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What holds ions together in an ionic bond? |
Electrostatic forces that hold the oppositely charged ions together |
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True or false? Atoms that easily form ions will either have a nearly full or nearly empty electron shell. |
True |
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Provide the outer electrons, the electrons lost of gained, and the charge on an ion for group 1, 2, 6 and 7 of the periodic table. |
Group 1 - 1 outer electron, 1 lost electron, 1+ charge on an ion. Group 2 - 2 outer electrons, 2 lost electrons, 2+ charge on an ion Group 6 - 6 outer electrons, 2 gained electrons, 2- charge on an ion Group 7 - 7 outer electrons, 1 gained electron and 1- charge on an ion |
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What is a lattice? |
The huge number of ions that are arranged in giant structures within ionic compounds. |
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How do bonds make atoms stable? |
Energy is released from the atoms when they bond making them more stable and less reactive |
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How are ions formed? |
The transfer of electrons between atoms formed charged particles called ions |
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Describe how cations and anions are formed |
Cations are formed when metal atoms lose electrons and form positive ions. Anions are formed when non-metal gain electrons and form negative ions. |
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What holds ions together in an ionic bond? |
Electrostatic forces that hold the oppositely charged ions together |
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True or false? Atoms that easily form ions will either have a nearly full or nearly empty electron shell. |
True |
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Provide the outer electrons, the electrons lost of gained, and the charge on an ion for group 1, 2, 6 and 7 of the periodic table. |
Group 1 - 1 outer electron, 1 lost electron, 1+ charge on an ion. Group 2 - 2 outer electrons, 2 lost electrons, 2+ charge on an ion Group 6 - 6 outer electrons, 2 gained electrons, 2- charge on an ion Group 7 - 7 outer electrons, 1 gained electron and 1- charge on an ion |
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What is a lattice? |
The huge number of ions that are arranged in giant structures within ionic compounds. |
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Explain why ionic compounds have high melting points. |
Some ions have more than one charge and those ions will attract others more strongly compared to an ion with one charge. More energy will be needed to overcome the electrostatic forces which is why they have higher melting points. |
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How do bonds make atoms stable? |
Energy is released from the atoms when they bond making them more stable and less reactive |
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How are ions formed? |
The transfer of electrons between atoms formed charged particles called ions |
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Describe how cations and anions are formed |
Cations are formed when metal atoms lose electrons and form positive ions. Anions are formed when non-metal gain electrons and form negative ions. |
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What holds ions together in an ionic bond? |
Electrostatic forces that hold the oppositely charged ions together |
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True or false? Atoms that easily form ions will either have a nearly full or nearly empty electron shell. |
True |
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Provide the outer electrons, the electrons lost of gained, and the charge on an ion for group 1, 2, 6 and 7 of the periodic table. |
Group 1 - 1 outer electron, 1 lost electron, 1+ charge on an ion. Group 2 - 2 outer electrons, 2 lost electrons, 2+ charge on an ion Group 6 - 6 outer electrons, 2 gained electrons, 2- charge on an ion Group 7 - 7 outer electrons, 1 gained electron and 1- charge on an ion |
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What is a lattice? |
The huge number of ions that are arranged in giant structures within ionic compounds. |
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Explain why ionic compounds have high melting points. |
Some ions have more than one charge and those ions will attract others more strongly compared to an ion with one charge. More energy will be needed to overcome the electrostatic forces which is why they have higher melting points. |
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How do ionic compounds conduct electricity and what are the two conditions that must be met so that a substance can conduct electricity? |
They can only conduct electricity when they are molten or dissolved in water. A substance must contain charged particles and they need to be able to move freely. |
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How do bonds make atoms stable? |
Energy is released from the atoms when they bond making them more stable and less reactive |
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How are ions formed? |
The transfer of electrons between atoms formed charged particles called ions |
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Describe how cations and anions are formed |
Cations are formed when metal atoms lose electrons and form positive ions. Anions are formed when non-metal gain electrons and form negative ions. |
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What holds ions together in an ionic bond? |
Electrostatic forces that hold the oppositely charged ions together |
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True or false? Atoms that easily form ions will either have a nearly full or nearly empty electron shell. |
True |
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Provide the outer electrons, the electrons lost of gained, and the charge on an ion for group 1, 2, 6 and 7 of the periodic table. |
Group 1 - 1 outer electron, 1 lost electron, 1+ charge on an ion. Group 2 - 2 outer electrons, 2 lost electrons, 2+ charge on an ion Group 6 - 6 outer electrons, 2 gained electrons, 2- charge on an ion Group 7 - 7 outer electrons, 1 gained electron and 1- charge on an ion |
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What is a lattice? |
The huge number of ions that are arranged in giant structures within ionic compounds. |
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Explain why ionic compounds have high melting points. |
Some ions have more than one charge and those ions will attract others more strongly compared to an ion with one charge. More energy will be needed to overcome the electrostatic forces which is why they have higher melting points. |
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How do ionic compounds conduct electricity and what are the two conditions that must be met so that a substance can conduct electricity? |
They can only conduct electricity when they are molten or dissolved in water. A substance must contain charged particles and they need to be able to move freely. |
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State the melting and boiling points of sodium bromide, sodium chloride and magnesium oxide. (Degrees C) |
Sodium bromide: MP: 747 BP: 1390 Sodium chloride: MP: 801 BP: 1413 Magnesium oxide: MP: 2852 BP: 3600 |
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How do bonds make atoms stable? |
Energy is released from the atoms when they bond making them more stable and less reactive |
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What are anodes and cathodes? |
Anodes: Anions (negative ions) are attracted to anodes. Cathodes: cations (positive ions) are attracted to cathodes. |
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How are ions formed? |
The transfer of electrons between atoms formed charged particles called ions |
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Describe how cations and anions are formed |
Cations are formed when metal atoms lose electrons and form positive ions. Anions are formed when non-metal gain electrons and form negative ions. |
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What holds ions together in an ionic bond? |
Electrostatic forces that hold the oppositely charged ions together |
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True or false? Atoms that easily form ions will either have a nearly full or nearly empty electron shell. |
True |
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Provide the outer electrons, the electrons lost of gained, and the charge on an ion for group 1, 2, 6 and 7 of the periodic table. |
Group 1 - 1 outer electron, 1 lost electron, 1+ charge on an ion. Group 2 - 2 outer electrons, 2 lost electrons, 2+ charge on an ion Group 6 - 6 outer electrons, 2 gained electrons, 2- charge on an ion Group 7 - 7 outer electrons, 1 gained electron and 1- charge on an ion |
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What is a lattice? |
The huge number of ions that are arranged in giant structures within ionic compounds. |
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Explain why ionic compounds have high melting points. |
Some ions have more than one charge and those ions will attract others more strongly compared to an ion with one charge. More energy will be needed to overcome the electrostatic forces which is why they have higher melting points. |
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How do ionic compounds conduct electricity and what are the two conditions that must be met so that a substance can conduct electricity? |
They can only conduct electricity when they are molten or dissolved in water. A substance must contain charged particles and they need to be able to move freely. |
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State the melting and boiling points of sodium bromide, sodium chloride and magnesium oxide. (Degrees C) |
Sodium bromide: MP: 747 BP: 1390 Sodium chloride: MP: 801 BP: 1413 Magnesium oxide: MP: 2852 BP: 3600 |
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How do bonds make atoms stable? |
Energy is released from the atoms when they bond making them more stable and less reactive |
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What are anodes and cathodes? |
Anodes: Anions (negative ions) are attracted to anodes. Cathodes: cations (positive ions) are attracted to cathodes. |
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How do ionic compounds conduct electricity when dissolved in water? |
Ionic compounds, that carry the current, can only conduct electricity when in a molten state because of the particle arrangement. |
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How are ions formed? |
The transfer of electrons between atoms formed charged particles called ions |
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Describe how cations and anions are formed |
Cations are formed when metal atoms lose electrons and form positive ions. Anions are formed when non-metal gain electrons and form negative ions. |
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What holds ions together in an ionic bond? |
Electrostatic forces that hold the oppositely charged ions together |
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True or false? Atoms that easily form ions will either have a nearly full or nearly empty electron shell. |
True |
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Provide the outer electrons, the electrons lost of gained, and the charge on an ion for group 1, 2, 6 and 7 of the periodic table. |
Group 1 - 1 outer electron, 1 lost electron, 1+ charge on an ion. Group 2 - 2 outer electrons, 2 lost electrons, 2+ charge on an ion Group 6 - 6 outer electrons, 2 gained electrons, 2- charge on an ion Group 7 - 7 outer electrons, 1 gained electron and 1- charge on an ion |
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What is a lattice? |
The huge number of ions that are arranged in giant structures within ionic compounds. |
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Explain why ionic compounds have high melting points. |
Some ions have more than one charge and those ions will attract others more strongly compared to an ion with one charge. More energy will be needed to overcome the electrostatic forces which is why they have higher melting points. |
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How do ionic compounds conduct electricity and what are the two conditions that must be met so that a substance can conduct electricity? |
They can only conduct electricity when they are molten or dissolved in water. A substance must contain charged particles and they need to be able to move freely. |
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State the melting and boiling points of sodium bromide, sodium chloride and magnesium oxide. (Degrees C) |
Sodium bromide: MP: 747 BP: 1390 Sodium chloride: MP: 801 BP: 1413 Magnesium oxide: MP: 2852 BP: 3600 |
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Define covalent and ionic bonds |
Covalent bond - when two non-metal atoms share a pair of electrons. Ionic bond - when a metal donates its electron to a non metal |
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Define covalent and ionic bonds |
Covalent bond - when two non-metal atoms share a pair of electrons. Ionic bond - when a metal donates its electron to a non metal |
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What substances share double bonds? |
Oxygen and carbon dioxide |
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Define valency |
The number of covalent bonds formed by atoms of different elements. |
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Define covalent and ionic bonds |
Covalent bond - when two non-metal atoms share a pair of electrons. Ionic bond - when a metal donates its electron to a non metal |
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What substances share double bonds? |
Oxygen and carbon dioxide |
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Define valency |
The number of covalent bonds formed by atoms of different elements. |
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Define intermolecular forces |
A weak attraction between molecules |
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Define covalent and ionic bonds |
Covalent bond - when two non-metal atoms share a pair of electrons. Ionic bond - when a metal donates its electron to a non metal |
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What substances share double bonds? |
Oxygen and carbon dioxide |
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Define valency |
The number of covalent bonds formed by atoms of different elements. |
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Define intermolecular forces |
A weak attraction between molecules |
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Why do smaller and simpler molecules have lower boiling and melting points? |
Because it doesn’t require a lot of energy to break intermolecular forces since they’re weak. |
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Define covalent and ionic bonds |
Covalent bond - when two non-metal atoms share a pair of electrons. Ionic bond - when a metal donates its electron to a non metal |
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What substances share double bonds? |
Oxygen and carbon dioxide |
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Define valency |
The number of covalent bonds formed by atoms of different elements. |
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Define intermolecular forces |
A weak attraction between molecules |
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Why do smaller and simpler molecules have lower boiling and melting points? |
Because it doesn’t require a lot of energy to break intermolecular forces since they’re weak. |
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What are monomers and polymers? |
Monomers - small simple molecules that can be joined in a chain to form a polymer. Polymer - chains of ethane monomers that come in different lengths |
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Define covalent and ionic bonds |
Covalent bond - when two non-metal atoms share a pair of electrons. Ionic bond - when a metal donates its electron to a non metal |
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What substances share double bonds? |
Oxygen and carbon dioxide |
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Define valency |
The number of covalent bonds formed by atoms of different elements. |
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Define intermolecular forces |
A weak attraction between molecules |
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Why do smaller and simpler molecules have lower boiling and melting points? |
Because it doesn’t require a lot of energy to break intermolecular forces since they’re weak. |
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What are monomers and polymers? |
Monomers - small simple molecules that can be joined in a chain to form a polymer. Polymer - chains of ethane monomers that come in different lengths |
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What are allotropes? |
Different structural forms of the same element. The structure and bonding in different allotropes influence their properties and uses. |
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What are allotropes? |
Different structural forms of the same element. The structure and bonding in different allotropes influence their properties and uses. |
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What are fullerenes? |
Fullerenes are spherical carbon molecules that have been covalently bonded to three other carbon atoms. |
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What are allotropes? |
Different structural forms of the same element. The structure and bonding in different allotropes influence their properties and uses. |
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What are fullerenes? |
Fullerenes are spherical carbon molecules that have been covalently bonded to three other carbon atoms. |
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Describe the attributes of fullerenes. |
Weak intermolecular forces and therefore have low melting points. Are physically soft and slippery. Molecules themselves are very strong due to covalent bonding. Are presented in a tube like structure. |
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What is graphene? |
They are similar to fullerenes, but are simple sheets of carbon atoms with no fixed formula |
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Describe the attributes of graphene |
One sheet of graphene is one atom thick making it the lightest known material, its covalent bond makes it extremely strong, is a good electrical conductor because electrons move freely on its surface. |
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Name and describe two giant structures of carbon |
Diamond and graphite. They are both allotropes of carbon and have huge three dimensional networks of carbon atoms linked by covalent bonds. |
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Describe the attributes of graphene |
One sheet of graphene is one atom thick making it the lightest known material, its covalent bond makes it extremely strong, is a good electrical conductor because electrons move freely on its surface. |
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Name and describe two giant structures of carbon |
Diamond and graphite. They are both allotropes of carbon and have huge three dimensional networks of carbon atoms linked by covalent bonds. |
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Do diamond and graphite have high or low boiling points? |
Diamond and graphite have high boiling points because lots of energy is required to break their strong three dimensional bonds. |
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Describe the attributes of graphene |
One sheet of graphene is one atom thick making it the lightest known material, its covalent bond makes it extremely strong, is a good electrical conductor because electrons move freely on its surface. |
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Name and describe two giant structures of carbon |
Diamond and graphite. They are both allotropes of carbon and have huge three dimensional networks of carbon atoms linked by covalent bonds. |
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Do diamond and graphite have high or low boiling points? |
Diamond and graphite have high boiling points because lots of energy is required to break their strong three dimensional bonds. |
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How are graphite and diamond different? |
Graphite has three covalent bonds whereas diamond has four. This is because graphite’s electrons are delocalised and are free to move around and carry electric currents. This is why graphite can conduct electricity and be used for electrolysis, but diamond cannot. |
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Why can graphite be used as a lubricant? |
It has weak forces of attraction between which allow its layers to slide past each other making it soft. |
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Why can graphite be used as a lubricant? |
It has weak forces of attraction between which allow its layers to slide past each other making it soft. |
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Why is diamond an electric insulator and why is it useful for cutting tools? |
Diamond is hard because it has a rigid network of carbon atoms joined by strong covalent bonds making it useful for cutting tools. It has no freely-charged particles making it a good insulator for electricity. |
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Why can graphite be used as a lubricant? |
It has weak forces of attraction between which allow its layers to slide past each other making it soft. |
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Why is diamond an electric insulator and why is it useful for cutting tools? |
Diamond is hard because it has a rigid network of carbon atoms joined by strong covalent bonds making it useful for cutting tools. It has no freely-charged particles making it a good insulator for electricity. |
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Name three properties of metals and non-metals. |
Metals - shiny, good electricity conductors and have high densities. Non-metals - not usually shiny as solids, low densities, brittle solids. |
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Why can graphite be used as a lubricant? |
It has weak forces of attraction between which allow its layers to slide past each other making it soft. |
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Why is diamond an electric insulator and why is it useful for cutting tools? |
Diamond is hard because it has a rigid network of carbon atoms joined by strong covalent bonds making it useful for cutting tools. It has no freely-charged particles making it a good insulator for electricity. |
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Name three properties of metals and non-metals. |
Metals - shiny, good electricity conductors and have high densities. Non-metals - not usually shiny as solids, low densities, brittle solids. |
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What is metallic bonding? |
A strong electrostatic attraction between positive metal ions and negative delocalised electrons. |
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Why can graphite be used as a lubricant? |
It has weak forces of attraction between which allow its layers to slide past each other making it soft. |
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Why is diamond an electric insulator and why is it useful for cutting tools? |
Diamond is hard because it has a rigid network of carbon atoms joined by strong covalent bonds making it useful for cutting tools. It has no freely-charged particles making it a good insulator for electricity. |
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Name three properties of metals and non-metals. |
Metals - shiny, good electricity conductors and have high densities. Non-metals - not usually shiny as solids, low densities, brittle solids. |
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What is metallic bonding? |
A strong electrostatic attraction between positive metal ions and negative delocalised electrons. |
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Define malleable |
Substances or objects that can be hammered or rolled into shape without shattering. |
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Why can graphite be used as a lubricant? |
It has weak forces of attraction between which allow its layers to slide past each other making it soft. |
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Why is diamond an electric insulator and why is it useful for cutting tools? |
Diamond is hard because it has a rigid network of carbon atoms joined by strong covalent bonds making it useful for cutting tools. It has no freely-charged particles making it a good insulator for electricity. |
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Name three properties of metals and non-metals. |
Metals - shiny, good electricity conductors and have high densities. Non-metals - not usually shiny as solids, low densities, brittle solids. |
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What is metallic bonding? |
A strong electrostatic attraction between positive metal ions and negative delocalised electrons. |
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Define malleable |
Substances or objects that can be hammered or rolled into shape without shattering. |
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How come metals don’t break and merely change shape when hit? |
When you hit a metal, layers of ions slide over each other. The sea of electrons hold the ions together. So the metal changes shape instead of breaking. |
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Why can graphite be used as a lubricant? |
It has weak forces of attraction between which allow its layers to slide past each other making it soft. |
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Why is diamond an electric insulator and why is it useful for cutting tools? |
Diamond is hard because it has a rigid network of carbon atoms joined by strong covalent bonds making it useful for cutting tools. It has no freely-charged particles making it a good insulator for electricity. |
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Name three properties of metals and non-metals. |
Metals - shiny, good electricity conductors and have high densities. Non-metals - not usually shiny as solids, low densities, brittle solids. |
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What is metallic bonding? |
A strong electrostatic attraction between positive metal ions and negative delocalised electrons. |
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Define malleable |
Substances or objects that can be hammered or rolled into shape without shattering. |
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How come metals don’t break and merely change shape when hit? |
When you hit a metal, layers of ions slide over each other. The sea of electrons hold the ions together. So the metal changes shape instead of breaking. |
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How is an electrical current formed in a metal? |
Delocalised electrons randomly move between positive metal ions in all directions. When a voltage is applied on a piece of metal, the electrons flow towards the positive side which transfers energy and forms a current. |
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What does the electrical conductivity of metals depend on? |
The electrical conductivity of metals increase as the number of delocalised electrons increase. |
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Why can graphite be used as a lubricant? |
It has weak forces of attraction between which allow its layers to slide past each other making it soft. |
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Why is diamond an electric insulator and why is it useful for cutting tools? |
Diamond is hard because it has a rigid network of carbon atoms joined by strong covalent bonds making it useful for cutting tools. It has no freely-charged particles making it a good insulator for electricity. |
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Name three properties of metals and non-metals. |
Metals - shiny, good electricity conductors and have high densities. Non-metals - not usually shiny as solids, low densities, brittle solids. |
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What is metallic bonding? |
A strong electrostatic attraction between positive metal ions and negative delocalised electrons. |
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Define malleable |
Substances or objects that can be hammered or rolled into shape without shattering. |
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How come metals don’t break and merely change shape when hit? |
When you hit a metal, layers of ions slide over each other. The sea of electrons hold the ions together. So the metal changes shape instead of breaking. |
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How is an electrical current formed in a metal? |
Delocalised electrons randomly move between positive metal ions in all directions. When a voltage is applied on a piece of metal, the electrons flow towards the positive side which transfers energy and forms a current. |
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What does the electrical conductivity of metals depend on? |
The electrical conductivity of metals increase as the number of delocalised electrons increase. |
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State the four different chemical bonds and structures. |
Ionic, covalent, giant covalent and metallic. |
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Why can graphite be used as a lubricant? |
It has weak forces of attraction between which allow its layers to slide past each other making it soft. |
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Describe issues with bonding models |
Dot and cross diagrams suggests that each electron is different and do not show the structure formed. Metallic models don’t show that ions are constantly vibrating. Ball and stick model depict the atoms as too far apart and there aren’t actually sticks that hold atoms together. |
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Name two acids and alkalis used in the home. |
Acids - vinegar and citrus fruits Alkalis - bleach and baking soda |
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How do you know if a substance is acidic, alkaline or neutral? |
On a pH scale, neutral substances have a pH of 7, acids have a pH lower than 7 and alkaline a have a pH higher than 7. |
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What colours do alkalis and acids make litmus, methyl orange and phenolphthalein? |
Alkalis - Litmus: blue, methyl orange: yellow, phenolphthalein: pink. Acids - Litmus: red, methyl orange: red, phenolphthalein: colourless. |
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How are polyatomic ions formed? |
They’re formed when small groups of atoms held together by covalent bonds lose or gain electrons. |
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How is hydrochloric acid made? |
It is formed hydrogen chloride gas dissolves in water and splits into H+ and Cl- ions. |
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True or false. The higher number of hydrogen ions in a certain volume, the lower their concentration. |
False. The higher number of hydrogen ions in a certain volume, the higher their concentration. |
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What are bases? |
Substances that neutralise acids to form a salt and water base only. |
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Name the basic word equation for all neutralisation reactions. |
metal oxide + acid —> salt + water |
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How are salts produced? |
Metal ions replace the hydrogen ions. |
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Why is diamond an electric insulator and why is it useful for cutting tools? |
Diamond is hard because it has a rigid network of carbon atoms joined by strong covalent bonds making it useful for cutting tools. It has no freely-charged particles making it a good insulator for electricity. |
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What is the symbol for sulfuric acid and hydrochloric acid? |
Sulfuric acid: H2SO4 (aq) Hydrochloric acid: 2HCL (aq) |
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Describe the process to make tin chloride, a soluble salt. |
Step 1 - add excess tin (II) oxide to a beaker of hydrochloric acid. Step 2 - gently warm the mixture using a water bath to speed the reaction. Step 3 - filter to remove the unreacted solid from the solution. Step 4 - heat with a Bunsen burner to evaporate water and concentrate the salt solution. Step 5 - leave to evaporate water slowly for crystallisation to occur. |
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What makes a base an alkali? |
Most bases don’t dissolve in water, but a base that can dissolve in water, a soluble base, is considered an alkali |
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State two examples each of insoluble and soluble bases (alkalis) |
Insoluble: Copper (II) hydroxide and most other metal hydroxides. Soluble: sodium hydroxide and calcium hydroxide |
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What is titration? |
This is where acid is added from burette to a fixed volume of alkali in a conical flask. |
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What substance react and do not react with dilute acids. |
Copper and silver do not react with dilute acids whilst metals such as potassium and sodium react explosively with dilute acids. |
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What is the general reaction that produces salt? |
metal + acid —> salt + hydrogen |
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What is oxidation and reduction? |
Oxidation reaction: A loss of electrons. Reduction reaction: A gain of electrons. |
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Describe pure carbon dioxide and describe the experiment you can do to test for its presence. |
Carbon dioxide is a colourless and outer less gas. To test for it, bubble the gas through lime water. It will turn a milky white if carbon dioxide is present. |
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How do you test for hydrogen? |
The squeaky pop test. Light a splint until it glows after trapping hydrogen in a test tube. Then, hold the glowing splint inside the test tube and if a squeaky pop sound emits, hydrogen is present. |
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Name three properties of metals and non-metals. |
Metals - shiny, good electricity conductors and have high densities. Non-metals - not usually shiny as solids, low densities, brittle solids. |
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What is metallic bonding? |
A strong electrostatic attraction between positive metal ions and negative delocalised electrons. |
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Define malleable |
Substances or objects that can be hammered or rolled into shape without shattering. |
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|
How come metals don’t break and merely change shape when hit? |
When you hit a metal, layers of ions slide over each other. The sea of electrons hold the ions together. So the metal changes shape instead of breaking. |
|
|
|
How is an electrical current formed in a metal? |
Delocalised electrons randomly move between positive metal ions in all directions. When a voltage is applied on a piece of metal, the electrons flow towards the positive side which transfers energy and forms a current. |
|
|
|
What does the electrical conductivity of metals depend on? |
The electrical conductivity of metals increase as the number of delocalised electrons increase. |
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State the four different chemical bonds and structures. |
Ionic, covalent, giant covalent and metallic. |
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C |
C |
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Why can graphite be used as a lubricant? |
It has weak forces of attraction between which allow its layers to slide past each other making it soft. |
|
|
|
Describe issues with bonding models |
Dot and cross diagrams suggests that each electron is different and do not show the structure formed. Metallic models don’t show that ions are constantly vibrating. Ball and stick model depict the atoms as too far apart and there aren’t actually sticks that hold atoms together. |
|
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|
Name two acids and alkalis used in the home. |
Acids - vinegar and citrus fruits Alkalis - bleach and baking soda |
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|
How do you know if a substance is acidic, alkaline or neutral? |
On a pH scale, neutral substances have a pH of 7, acids have a pH lower than 7 and alkaline a have a pH higher than 7. |
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What colours do alkalis and acids make litmus, methyl orange and phenolphthalein? |
Alkalis - Litmus: blue, methyl orange: yellow, phenolphthalein: pink. Acids - Litmus: red, methyl orange: red, phenolphthalein: colourless. |
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How are polyatomic ions formed? |
They’re formed when small groups of atoms held together by covalent bonds lose or gain electrons. |
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How is hydrochloric acid made? |
It is formed hydrogen chloride gas dissolves in water and splits into H+ and Cl- ions. |
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True or false. The higher number of hydrogen ions in a certain volume, the lower their concentration. |
False. The higher number of hydrogen ions in a certain volume, the higher their concentration. |
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What are bases? |
Substances that neutralise acids to form a salt and water base only. |
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Name the basic word equation for all neutralisation reactions. |
metal oxide + acid —> salt + water |
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How are salts produced? |
Metal ions replace the hydrogen ions. |
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|
Why is diamond an electric insulator and why is it useful for cutting tools? |
Diamond is hard because it has a rigid network of carbon atoms joined by strong covalent bonds making it useful for cutting tools. It has no freely-charged particles making it a good insulator for electricity. |
|
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|
What is the symbol for sulfuric acid and hydrochloric acid? |
Sulfuric acid: H2SO4 (aq) Hydrochloric acid: 2HCL (aq) |
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Describe the process to make tin chloride, a soluble salt. |
Step 1 - add excess tin (II) oxide to a beaker of hydrochloric acid. Step 2 - gently warm the mixture using a water bath to speed the reaction. Step 3 - filter to remove the unreacted solid from the solution. Step 4 - heat with a Bunsen burner to evaporate water and concentrate the salt solution. Step 5 - leave to evaporate water slowly for crystallisation to occur. |
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What makes a base an alkali? |
Most bases don’t dissolve in water, but a base that can dissolve in water, a soluble base, is considered an alkali |
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State two examples each of insoluble and soluble bases (alkalis) |
Insoluble: Copper (II) hydroxide and most other metal hydroxides. Soluble: sodium hydroxide and calcium hydroxide |
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What is titration? |
This is where acid is added from burette to a fixed volume of alkali in a conical flask. |
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What substance react and do not react with dilute acids. |
Copper and silver do not react with dilute acids whilst metals such as potassium and sodium react explosively with dilute acids. |
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What is the general reaction that produces salt? |
metal + acid —> salt + hydrogen |
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What is oxidation and reduction? |
Oxidation reaction: A loss of electrons. Reduction reaction: A gain of electrons. |
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Describe pure carbon dioxide and describe the experiment you can do to test for its presence. |
Carbon dioxide is a colourless and outer less gas. To test for it, bubble the gas through lime water. It will turn a milky white if carbon dioxide is present. |
|
|
|
How do you test for hydrogen? |
The squeaky pop test. Light a splint until it glows after trapping hydrogen in a test tube. Then, hold the glowing splint inside the test tube and if a squeaky pop sound emits, hydrogen is present. |
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Name three properties of metals and non-metals. |
Metals - shiny, good electricity conductors and have high densities. Non-metals - not usually shiny as solids, low densities, brittle solids. |
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|
What is metallic bonding? |
A strong electrostatic attraction between positive metal ions and negative delocalised electrons. |
|
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|
Define malleable |
Substances or objects that can be hammered or rolled into shape without shattering. |
|
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|
How come metals don’t break and merely change shape when hit? |
When you hit a metal, layers of ions slide over each other. The sea of electrons hold the ions together. So the metal changes shape instead of breaking. |
|
|
|
How is an electrical current formed in a metal? |
Delocalised electrons randomly move between positive metal ions in all directions. When a voltage is applied on a piece of metal, the electrons flow towards the positive side which transfers energy and forms a current. |
|
|
|
What does the electrical conductivity of metals depend on? |
The electrical conductivity of metals increase as the number of delocalised electrons increase. |
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State the four different chemical bonds and structures. |
Ionic, covalent, giant covalent and metallic. |
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C |
C |
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What is a precipitation reactions? |
A reaction where soluble substances in a solution cause an insoluble precipitate to form. |
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What is a precipitation reactions? |
A reaction where soluble substances in a solution cause an insoluble precipitate to form. |
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Why is the limewater test for carbon dioxide a precipitation reaction? |
The test is a precipitation reaction because the precipitate calcium carbonate is formed when the test is done. |
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What is a precipitation reactions? |
A reaction where soluble substances in a solution cause an insoluble precipitate to form. |
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Why is the limewater test for carbon dioxide a precipitation reaction? |
The test is a precipitation reaction because the precipitate calcium carbonate is formed when the test is done. |
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What happens when two solutions that contain soluble salts swap? |
The ions from each salt swap. |
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What is a precipitation reactions? |
A reaction where soluble substances in a solution cause an insoluble precipitate to form. |
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Why is the limewater test for carbon dioxide a precipitation reaction? |
The test is a precipitation reaction because the precipitate calcium carbonate is formed when the test is done. |
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What happens when two solutions that contain soluble salts swap? |
The ions from each salt swap. |
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Magnesium sulfate solution reacts with barium chloride solution. Predict the name of the participates. |
Magnesium chloride and barium sulfate |
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What is a precipitation reactions? |
A reaction where soluble substances in a solution cause an insoluble precipitate to form. |
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Why is the limewater test for carbon dioxide a precipitation reaction? |
The test is a precipitation reaction because the precipitate calcium carbonate is formed when the test is done. |
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What happens when two solutions that contain soluble salts swap? |
The ions from each salt swap. |
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Magnesium sulfate solution reacts with barium chloride solution. Predict the name of the participates. |
Magnesium chloride and barium sulfate |
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Describe the process you can use to prepare insoluble salts. |
Wear eye protection, mix two soluble solutions in a beaker and filter it. Rinse the beaker with distilled water and pour this through the funnel. There should be a precipitate in the funnel; pour a little distilled water over it. Remove the filter paper containing the precipitate and dry it in an oven. |
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What is an empirical formula? |
The simplest whole number ratio of atoms or ions of each element in a substance. |
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What is a precipitation reactions? |
A reaction where soluble substances in a solution cause an insoluble precipitate to form. |
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Why is the limewater test for carbon dioxide a precipitation reaction? |
The test is a precipitation reaction because the precipitate calcium carbonate is formed when the test is done. |
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What happens when two solutions that contain soluble salts swap? |
The ions from each salt swap. |
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Magnesium sulfate solution reacts with barium chloride solution. Predict the name of the participates. |
Magnesium chloride and barium sulfate |
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Describe the process you can use to prepare insoluble salts. |
Wear eye protection, mix two soluble solutions in a beaker and filter it. Rinse the beaker with distilled water and pour this through the funnel. There should be a precipitate in the funnel; pour a little distilled water over it. Remove the filter paper containing the precipitate and dry it in an oven. |
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What is an empirical formula? |
The simplest whole number ratio of atoms or ions of each element in a substance. |
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What is a molecular formula? |
The actual number of atoms of each element in one molecule. |
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What is a precipitation reactions? |
A reaction where soluble substances in a solution cause an insoluble precipitate to form. |
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True or false. When a solute is dissolved in a solvent to make a solution, the mass of the solution is equal to the mass of the solvent and the mass of the solute. |
True. |
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What is a concentration and state the equation used to find it. |
Concentration is the amount of solute dissolved in a stated volume of a solution.
mass of solute conc. = ——————— volume of solution in dm3 |
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How do you convert cm3 to dm3? |
Divide by 1000 |
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Closed system - where an experiment’s environment doesn’t allow any substances, such as gases, escape. Non-enclosed system - where substances such as gas |
Closed system - where an experiment’s environment doesn’t allow any substances, such as gases, escape. Non-enclosed system - an environment where substances, such as gases, can easily escape. |
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True or false? The mass of the products is always the same as the mass of the reactants. |
True |
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State the Avogadro constant |
6.02 x 10 (to the power 23) |
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State the equation for moles |
mass of a substance moles = ——————————— Ar |
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What is a limiting reactant? |
The reactant that is totally consumed when the chemical reaction is completed. The amount of product formed is limited by this substance since the reaction can’t continue without it. |
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What is electrolysis? |
Electrolysis is a process that uses energy transferred by electricity to decompose electrolytes. |
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What are cations and anions? |
Cations are positive ions and are attracted to the negative cathode. Anions and negative ions and are attracted to the positive anode |
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Why is the limewater test for carbon dioxide a precipitation reaction? |
The test is a precipitation reaction because the precipitate calcium carbonate is formed when the test is done. |
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What are cathodes and anodes? |
Cathodes are the positive electrodes Anodes are the negative electrodes. |
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What happens to negative and positive ions and the anodes and cathodes? |
At the anode, negative ions lose electrons. At the cathode, electrons are transferred from the electrode to the positive ions. |
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Define oxidation and reduction |
Oxidation is the loss of electrons. Reduction is the gain of electrons. |
OIL RIG |
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Where does reduction and oxidation take place? |
Reduction takes place at the cathode. Oxidation takes place at the anode. |
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What are inert electrodes and what are they usually made from? |
Inert electrodes are unreactive electrodes and they’re usually made from graphite or platinum. |
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What happens when a molten salt is electrolysed? |
Ions are discharged as atoms or molecules at the electrodes. |
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How come you can always predict the electrolysis products of any molten salt? What happens when molten lead bromide is electrolysed? |
The salt always decomposes into its elements. The metal is produced at the cathode and the non-metal is produced at the anode. Lead is produced at the cathode because it is a metal and bromine is produced at the anode because it is a non-metal. |
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What is the reactivity series? |
A list of metals in order of reactivity, with the most reactive metals at the top. |
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What happens when two solutions that contain soluble salts swap? |
The ions from each salt swap. |
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Magnesium sulfate solution reacts with barium chloride solution. Predict the name of the participates. |
Magnesium chloride and barium sulfate |
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Describe the process you can use to prepare insoluble salts. |
Wear eye protection, mix two soluble solutions in a beaker and filter it. Rinse the beaker with distilled water and pour this through the funnel. There should be a precipitate in the funnel; pour a little distilled water over it. Remove the filter paper containing the precipitate and dry it in an oven. |
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What is an empirical formula? |
The simplest whole number ratio of atoms or ions of each element in a substance. |
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What is a molecular formula? |
The actual number of atoms of each element in one molecule. |
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Describe how to convert the molecular formula to empirical formula. |
Find what each of the numbers given are divisible by and divide them to get the lowest possible values. |
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Describe how the empirical formula of a compound can be calculated when given the masses of the elements used to make it. |
First, divide each mass given by their atomic masses. Then, divide your answers by the smallest answer to find the simplest ratio. Lastly, write your formula using the elements. |
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Describe how you’d find the molecular formula from the empirical formula when the question gives you the relative formula mass and a compound. |
Multiply each element from the compound by its atomic mass and add your answers together. Divide your relative formula mass by your final answer.
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List the reactivity series from the least to most reactive |
gold, silver, copper, iron, zinc, aluminium, magnesium, calcium, sodium, potassium |
G S C I Z A M C S P |
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List the reactivity series from the least to most reactive |
gold, silver, copper, iron, zinc, aluminium, magnesium, calcium, sodium, potassium |
G S C I Z A M C S P |
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What is a redox reaction? |
A reaction in which one substance is oxidised and another is reduced. |
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What is extraction? |
The process of obtaining a metal from a compound. |
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