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59 Cards in this Set
- Front
- Back
- 3rd side (hint)
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How is an atom placed in the periodic table? |
An atom is placed in the periodic table according to its number of protons |
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How did Mendeleev use his table to predict the existence and properties of other elements? |
By using the gaps between already discovered elements |
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The mass number is... |
The number of protons added to the number of neutrons - the bigger number |
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Why do atoms bond together to form compounds? |
So that they have full outer shells so they are more stable |
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What is an ion? |
Ions are electrically charged particles, formed from atoms by the addition or removal of e- |
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Which ions are attracted to each other? |
Positive cations are attracted to negatively charged anions |
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How do metals become ions? |
Metals lose e- to become metal cations |
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How do non-metals become ions? |
Non-metals gain e- to become non-metal anions |
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Define an ionic bond |
The electrostatic attraction between oppositely charged metal cations and non-metal anions |
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Compounds ending with "ide" contain... |
Two elements |
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Compounds ending with "ate" contain... |
Both named elements and oxgyen |
e.g. Calcium carbonate |
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What charge do ionic compounds have? |
Ionic compounds are neutral |
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Describe the electron configuration and ion formed of an alkali metal |
All have 1 e- in their outer shell, therefore forming a metal cation with a charge of 1+ |
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Describe the electron configuration and ion formed of an alkaline Earth metal |
All have 2 e- in their outer shell, so they all form metal cations with 2+ charge |
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Describe the charge of the following ions: - Cu(i) - Cu(ii) - Fe(ii) - Fe(iii) - Zn(ii) |
- Cu(i) = Cu + - Cu(ii) = Cu + - Fe(ii) = Fe 2+ - Fe(iii) = Fe 3+ - Zn(ii) = Zn 2+ |
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Name the compounds: - CO3 - SO4 - NO3 - OH |
- CO3 = Carbonate (2-) - SO4 = Sulphate (2-) - NO3 = Nitrate (-) - OH = Hydroxide (-) |
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Sheet C2.6e Ionic compounds |
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Define lattice |
A regular arrangement of billions of ions in a 3D structure |
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Give one example of a giant ionic lattice |
NaCl |
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Do ionic solids conduct electricity and why? |
Ionic solids don't conduct electricity as the ions cannot move |
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How can one enable ionic compounds to conduct electricity? |
If ionic compounds are dissolved in water (aqueous) or melted (molten) then they can conduct electricity |
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Why can molten or aqueous ionic compounds conduct electricity? |
As in both the ions can move so the flow of charged particles (current) occurs |
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Define a precipitate |
An insoluble solid formed from the reaction between two soluble substances |
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Define a covalent bond |
A single covalent bond is a shared pair of e- between two non-metals. A double covalent bond would be two shared pairs of e- between 2 non-metals |
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In a covalent bond, how is the number of shared e- determined? |
By the number of e- in the outer shell of the element |
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Name the two main types of covalent bonds |
- Simple molecular covalent substance - Giant molecular covalent substance |
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Do covalent substances conduct electricity? |
No, bar graphite, as they have no charged particles |
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Simple molecular covalents are usually... |
Gases at room temperature
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low melting and boiling points |
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Simple molecular covalents exist as... |
Discrete molecules (e.g. CO2, O2, CO, NH3) |
Weak inter-molecular forces, strong intra-molecular forces |
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Define electronegativity |
The property which mans something draws e- to it |
Water |
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Giant molecular covalent substances are... |
Solids at room temperature |
High melting and boiling points |
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Give three examples of giant molecular covalents |
Diamond, graphite (both allatropes of carbon) and sand (SiO2) |
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Why doesn't diamond conduct electricity? |
As there are no free e- as each carbon atom is bonded to 4 other carbon atoms ---> no free e- |
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Why does graphite conduct electricty? |
As each carbon is bonded to 3 other carbon atoms so there is 1 delocalized e-, meaning they are free to move between layers when p.d. is applied |
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Give a use of graphite |
Lubricant as layers slide over eachother |
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Give a use of diamond |
Drill as extremely strong and durable |
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Soluble substances are usually... |
ionic substances, bar sucrose, which is a covalent |
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Why are ionic substances usually soluble? |
As water possesses hydrogen bonding so there is a polarity - a slight positive charge on the hydrogen and a slight negative charge on the oxygen |
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Is ethanol attracted to water? |
Yes |
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Why? |
Because ethanol contains O, H and C atoms so there is delta charge and will be attracted to water |
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Is oil immiscible or miscible? |
Immiscible |
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Why? |
As it doesn't have oxygen so it's neutral |
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What is the energy change when bonds are formed? |
Energy is released into the surroundings from the system (exothermic) |
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Name 5 ways which can be used to separate mixtures |
-Fractional distillation -Centrifuge -Filtering -Evaporating -Chromotography |
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What is distillation? |
When a solution is evaporated and then condensed so miscible substances are separated |
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What is a separating funnel used for? |
Separating immiscible mixtures |
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How can distillation be used to separate ethanol and water? |
The mixture is evaporated then condensed. The temp. must be between the boiling point of two of the liquids - ethanol will evaporate, water won't. Ethanol gas condenses in Leiberg condenser, comes out in beaker |
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Why does the round-bottomed flask have bump granules? |
So that SA is increased for bubbles to form |
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How can a separating funnel be used to separate oil and water? |
Densities of two are different - denser of two will sink to bottom, so it can be let out |
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Name the flame colors for potassium, calcium, sodium and copper |
K - lilac Ca - red Na - yellow Cu - blue/green |
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How does one test for a halide ion? |
Add nitric acid and silver nitrate to solution. If halide ions are present the silver halide will precipitate |
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What are the colours of the possible silver halide precipitates formed? |
AgCl - white precipitate AgBr - cream precipitate AgI - yellow precipitate |
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What is the test for sulfate ions? |
Add sulfate ions to barium chloride and HCl. If sulfate ions present, barium sulfate will precipitate |
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How would one tell if barium sulfate is present? |
It is a white precipitate |
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Describe the test for carbonate ions |
Acid is added to carbonate, if carbonate is present CO2 released in effervescence, which turns lime water cloudy when bubbled through |
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What is the use of chromatography? |
Separating out different compounds in a mixture |
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Where must the water level be in order for chromatography to work? |
The water level must be below the test samples and pencil line |
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What will affect how far the samples move? |
The particle size/mass and the solubility |
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How is the Rf value found? |
distance moved by compound --------------------------------------------- distance moved by solvent |
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