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88 Cards in this Set
- Front
- Back
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Atomic Structure Describe the charges of protons, neutrons and electrons. |
Protons: Positively charged Neutrons: No charge Electrons: Negatively charged |
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Atomic Structure Describe the basic composition of an atom. |
- Electron shells: negative charge, negligible mass - Nucleus: protons (positive charge, mass of 1 a.m.u), neutrons (no charge, mass of 1 a.m.u) |
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Atomic Structure What is the maximum number of electrons per electron shell? |
- In the first, there can be a maximum of 2 - The others have a maximum of 8 |
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Atomic Structure What is the number shown at the top of an element on the periodic table? |
- R.A.M: Relative Atomic Mass - Mass number |
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Atomic Structure What is the number shown at the bottom of an element on the periodic table? |
- Atomic number - Proton number |
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Atomic Structure Which out of the atomic number and R.A.M has the higher value? |
- R.A.M: larger value - Atomic number: smaller value |
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Atomic Structure What does the R.A.M/mass number tell us? |
The number of protons and neutrons |
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Atomic Structure What does the atomic number tell us? |
The number of protons (and electrons) |
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Atomic Structure How would you find out the number of neutrons in an atom? |
Subtract the atomic number (the number of PROTONS) from the R.A.M (leaving only the number of NEUTRONS) |
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Periodic Table What are groups and periods? |
- Groups: Columns - Periods: Rows |
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Periodic Table What things are in Group 1? |
Alkali metals |
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Periodic Table What things are in Group 2? |
Alkaline earth metals |
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Periodic Table What things are in Group 7? |
Halogens |
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Periodic Table What things are in Group 8/0? |
Noble Gases |
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Periodic Table How do you determine the group of an element? |
It's the number of electrons on its outer shell |
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Periodic Table How do you determine the period of an element? |
It's the number of electron shells
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Atomic Structure How can you determine an element's 'number' (e.g. 2.8.1)? |
The numbers must add to the atomic number, and these numbers represent the number of electrons. There can be a maximum of 2 in the first electron shell and a maximum of 8 in the other shells. |
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Relative Atomic Mass What is everything measured relative to? |
Carbon -12 |
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Isotopes Give an example of an element that exists as 2 isotopes. |
Chlorine |
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Isotopes The R.A.M of chlorine is 35.5. Why is this? |
- 75% of Chlorine on Earth is Cl 35 - 25% of Chlorine on Earth is Cl 37 |
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Isotopes How is the atomic mass of Chlorine calculated? (Words) |
- Multiply the % by the R.A.M - Add it with the % of the other multiplied by the other R.A.M - Divide by the %s added together |
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Isotopes How is the atomic mass of Chlorine calculated? (Numbers) |
[(75x35) + (25x37)] / (75+25) = 35.5 R.A.M = 35.5 |
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Ions and Ionic Bonding What is an ion? |
An electrically charged particle |
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Ions and Ionic Bonding How are ions formed? |
Electron Transfer: the addition or removal of electrons |
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Ions and Ionic Bonding Why do atoms bond together to form compounds? |
To make an outer shell to make it more stable |
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Ions and Ionic Bonding What is one way for atoms to bond? |
Forming an ionic particle. |
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Ions and Ionic Bonding What are cations? |
Positively charged ions |
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Ions and Ionic Bonding What are anions? |
Negatively charged ions |
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Ions and Ionic Bonding Let's say A transfers an electron to B. What happens to the two of them? |
- A gains a positive charge as there are now more protons than electrons, so it's a cation. - B gains a negative charge as there are now more electrons than protons, so it's an anion. |
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Ions and Ionic Bonding What is an ionic bond? |
When metal cations are electrostatically attracted to non-metal anions |
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Ions and Ionic Bonding How is it determined as to whether or not an atom gains or loses electrons? |
It does whatever is easiest - it's easier to gain 1 than lose 7 (to form 8 electrons). |
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Ions and Ionic Bonding What do metals become when they lose electrons? |
Metal cations |
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Ions and Ionic Bonding What do non-metals become when they lose electrons? |
Non-metal anions |
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Naming Compounds What does the suffix -ide mean? |
Only two elements are present e.g. sodium chloride |
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Naming Compounds What does the suffix -ate mean? |
Two elements AND oxygen are present |
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Ions and Ionic Bonding True or false: Ionic compounds are neutral overall |
TRUE |
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Ions and Ionic Bonding How is the charge (shown as subscript) determined? |
The group determines it. e.g. Aluminium is in Group 3 and forms a 3[+] charge. |
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Naming Compounds Which compounds have the ending -ite and what does it mean? |
- Iron suplhite and nitrogen oxite - It means they have one less oxygen than the previous one - there are only two and they're anions (?) |
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Properties of Ionic Compounds What is an ionic compound? |
When you have an ionic lattice |
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Properties of Ionic Compounds What is a lattice? |
A regular cuboid arrangement of billions of ions |
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Properties of Ionic Compounds When something becomes an ion, what suffix does it get? |
-ide e.g. Chlorine ---> Chloride |
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Properties of Ionic Compounds What is the melting point of a lattice and why is it like this? |
- It has a very HIGH melting point - There are too many strong ionic bonds for it to be low |
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Properties of Ionic Compounds In order for an ionic compound to conduct electricity, what type of charges must it have? |
Mobile charges (charged particles that are free to flow and therefore can move) |
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Properties of Ionic Compounds Why can't ionic solids conduct? |
While they do contain ions, they can't move and therefore can't conduct. |
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Properties of Ionic Compounds What properties must an ionic compound have to conduct electricity and how can these properties be attained? |
- Aqueous: dissolve them in water OR - Molten: melt them |
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Properties of Ionic Compounds Define electricity. |
The flow of electrons |
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Soluble and Insoluble Salts Which salts are soluble? |
- All common sodium, potassium and ammonium salts - Nitrates - Most chlorides - Most sulphates - Sodium, potassium and ammonium carbonate - Sodium, potassium and ammonium hydroxide |
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Soluble and Insoluble Salts Which salts are insoluble? |
- Silver and lead chloride - Lead, barium and calcium suplhate - Most carbonates - Most hyrdroxidesq |
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Soluble and Insoluble Salts What can Barium Sulphate be used in? |
X-Ray machines |
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Covalent Bonding What is a single covalent bond? |
A shared pair of electrons between two non-metals |
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Covalent Bonding What is a double covalent bond? |
Two shared pairs of electrons between two non-metals |
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Covalent Bonding What is the outcome of double and single covalent bonds? |
Both elements have a full outer shell |
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Covalent Bonding How is the number of shared electrons determined? |
The numbers of electrons in the outer shell in the atom of an element e.g. Carbon: Group 4 -> 4e[-] in the outer shell (needs to share 4e[-] to make 8e[-] in total) |
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Covalent Bonding What must each individual element's outer shell add up to? What is the exception to this? |
- 8e[-] - Hydrogen: only 2e[-] on the outer shell |
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Properties of Covalent Substances Why can't covalent substances conduct electricity? |
They have no charged particles. |
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Properties of Covalent Substances What are SMCS? |
Simple Molecular Covalent Substances |
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Properties of Covalent Substances List the properties of SMCS. |
- Usually gas at room temp. - Include molecules e.g. CO(2), NH(3), O(2), CO... - Low boiling and melting points - Exist as discreet molecules (e.g. a carbon atom joined to two oxygen atoms), i.e. individual molecules - Strong bonds in the intramolecular covalent bonds - Weak forces of attraction between molecules (intermolecular) |
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Properties of Covalent Substances Describe the strength of the bonds in intramolecular and intermolecular forces. |
- Intermolecular forces: Weak forces of attraction between molecules - Intramolecular forces: Strong covalent bonds within the molecule |
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Properties of Covalent Substances Define intramolecular forces. |
Bonds within the molecule |
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Properties of Covalent Substances Define intermolecular forces. |
Forces of attraction between molecules |
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Properties of Covalent Substances What are GMCs? |
- Giant Molecular Covalent - Structures with thousands of covalent bonds - Solid at room temp. - High boiling/melting points |
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Properties of Covalent Substances Give three examples of GMCs. |
- Diamonds - allotropes of carbon - Graphite - allotropes of carbon - Sand - silicon oxide |
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Properties of Covalent Substances What arrangement does a diamond have? |
Tetrahedral arrangement |
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Properties of Covalent Substances Why is the maximum number of bonds carbon make to other carbon atoms 4? |
Carbon is in Group 4 and therefore can make a maximum of 4 bonds. |
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Properties of Covalent Substances Why can't carbon conduct electricity? |
Because it can make a maximum of 4 bonds, there are no free electrons as they're all in covalent bonds. No electrons, no conduction of electricity. |
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Properties of Covalent Substances Describe the structure of graphite. |
Flat sheets of hexagons. |
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Properties of Covalent Substances How can graphite, unlike other carbon substances, conduct electricity? |
- There's one free electron (localised electron) per carbon atom, meaning that the electrons can move between the layers - Potential difference, or voltage, is applied - This allows graphite to conduct electricity |
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Properties of Covalent Substances Why does graphite have one free electron? |
Because it's carbon, it's in Group 4 and therefore has four electrons. Graphite only uses three for covalent bonding, so there's one left over. |
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Properties of Covalent Substances How can graphite be used as a lubricant? |
- There are weak forces of attraction between the layers - So the layers can easily slide over each other - Graphite can be used as a lubricant |
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Ion Tests What can metal cations be tested with? |
Flame tests |
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Ion Tests What colours will sodium, calcium, potassium and copper go in the flame tests? |
- Sodium: Yellow - Calcium: Red - Potassium: Lilac - Copper: Green-blue or blue-green |
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Ion Tests What are halide ions? |
Ions of halogens |
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Ion Tests Give three examples of halide ions. |
- Silver Chloride (AgCl) - Silver Bromide (AgBr) - Silver Iodide (AgI) |
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Ion Tests To test non-metal anions, which in this case are halide ions, what do you add to the halide ion? What does this create? |
1) Add HNO(3) (Nitric Acid) 2) Add AgNO(3) (Silver Nitrate) This creates a silver halide precipitate. |
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Ion Tests After adding the substances to the halide ions, what colour precipitates will be formed with AgCl, AgBr and AgI? |
- AgCl: White precipitate - AgBr: Cream precipitate - AgI: Yellow precipitate |
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Ion Tests What do you do to find suplhate ions? |
1) Add HCl 2) Add BaCl(2) (Barium Chloride) This forms a white precipitate of barium chloride |
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Classifying Substances True or false: Ionic compounds dissolve in water |
TRUE |
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Miscible and Immiscible What do miscible and immiscible mean? |
- Miscible: Completely mixes - Immiscible: Doesn't completely mix |
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Miscible and Immiscible Give an example of a miscible substance. |
Ethanol |
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Miscible and Immiscible Give an example of an immiscible substance and explain why it is immiscible in water. |
- Oil - Water is electronegative, so it attracts ions and electrons. Oil isn't attracted to it so it doesn't mix |
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Miscible and Immiscible List 7 ways of separating mixtures |
- Distillation - Fractional distillation - Filtering - Centrifuge - Evaporation - Chromatography - Separating funnel |
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Miscible and Immiscible True or false: distillation and separating funnels both separate miscible substances. |
FALSE Distillation separates miscible substances Separating funnels separate immiscible substances |
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Miscible and Immiscible What do anti-bumping granules do and when might they be used? |
- They'd be used in distillation - There are imperfections in the glass of the round bottom flask, which creates bubbles, so the anti-bumping granules reduce pressure |
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Miscible and Immiscible Why does the water separate from the oil in a separation funnel? |
The water is denser than the water so it goes to the bottom. |
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Chromatography What does chromatography do? |
It separates compounds from a mixture |
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Chromatography When is chromatography used? |
- To separate paint - Food testing - To use in criminal investigations e.g. car paint |
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Chromatography Which things affect how far the compounds move on the chromatography paper? |
- The size/mass of particles - Solubility |
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Chromatography What is the Rf value? |
The distance a compound has risen divided by the distance the solvent has risen |
