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Chemistry revision > Year 11 Mock > Flashcards

Year 11 Mock Flashcards

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1
Q

What is covalent bonding

A

Non metals combined together by sharing electrons. The shared pair of electrons holds the 2 atoms together.

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2
Q

Why are covalent bonds strong

A

there is a strong electrostatic force of attraction between the positive nuclei of the atoms and the negative electrons in each shared pair

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3
Q

What do we use to show covalent bonds

A

dot and cross diagrams

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4
Q

What are simple molecular substances

A

Formed by covalent bonds with simple molecular structures such as CO2 and H20.

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5
Q

Properties of simple molecular structures

A

Held together by strong covalent bonds
Force of attraction between the molecules are weak
Melting and boiling points are very low because the molecules are easily parted from each other.
Gases or liquids at room temperature and don’t conduct electricity because they don’t have free electrons or ions.

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6
Q

Properties of Giant covalent structures

A

Atoms are bonded to each other by strong covalent bonds
Very high melting and boiling points
Don’t conduct electricity

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7
Q

What are giant covalent bonds

A

Similar to a giant ionic lattice except that there are NO charged ions

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8
Q

Properties of Diamond

A

each carbon atoms forms 4 covalent bonds in a very rigid giant covalent structure.
Hard, takes a lot of energy to break
High melting and boiling point
Doesn’t conduct electricity because it has no free electrons.

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9
Q

Properties of Graphite

A

Black, opaque and shiny
Each carbon atom forms 3 covalent bonds, creating sheets of carbon atoms which are free to slide over eachother.
High melting point, need loads of energy to break.
Conducts electricity

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10
Q

How does graphite conduct electricity

A

Only 3 out of 4 of carbons 4 outer electrons are used in bonds, there are lots of delocalised electrons that can move = electricity.

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11
Q

Uses of Graphite

A

a lubricating material and electrodes as the layers are held together weakly so they are slippery and can be rubbed off on paper= pencil.

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12
Q

Uses of diamonds

A

cutting tools

jewelry

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13
Q

What are fullerenes

A

Another form of carbon , large molecules shaped like hollow balls or tubes, atoms arranged in rings and have free electrons so can conduct electricity

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14
Q

What is Graphene

A

A single sheet of graphite, strong covalent bonds, free electrons can conduct electricity better than graphite

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15
Q

What is ionic bonding

A

Form between positive and negative ions, which attract each other and bind together by gaining or losing electrons to form ionic compounds (full outer shell) eg- Sodium.

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16
Q

What happens to metals and non metals in ionic bonding

A

Metals can lose electrons to form a positively charges ion and the non metal can gain electrons to form a negatively charged ion.

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17
Q

What are oppositely charged ions strongly attracted to one another by

A

electrostatic force of attraction

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18
Q

How do you find the formula of an ionic compound

A

balance the positive and negative charges

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19
Q

What do we use to show ionic bonding

A

Dot and Cross diagram

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20
Q

What happens in the ionic bond of sodium chloride (NaCl)

A

Sodium atom has a electronic configuration of 2,8,1 therefore needs to lose its outer electron to have a full shell. The Chlorine atom has an electronic configuration of 2,8,7 therefore needs to gain an electron to have a full outer shell. Sodium gives up its outer electron and Chlorine gains it. This gives Na a + charge and Cl a - charge.

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21
Q

What structure do Ionic compounds have

A

Giant ionic lattice structure, ions form a closely packed regular lattice. There are very strong electrostatic forces of attraction between oppositely charged ions, in all directions.

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22
Q

What are the properties of Ionic compounds

A

High melting and boiling points due to strong attraction between ions, takes a large amount of energy to overcome it.
Don’t conduct electricity because the ions are fixed in place and can’t move
DISSOLVE EASILY IN WATER.

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23
Q

What happens when ions dissolve in water or become molten

A

The ions separate and are all free to move in the solution, so they’ll carry an electric current.

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24
Q

What structure do metals have

A

Crystal

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25
Q

Properties of the structure of metals

A

Outer electrons are free

Atoms become positive ions in a sea of delocalised electrons

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26
Q

What is metallic bonding

A

The electrostatic attraction between these ions and electrons in metals

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27
Q

Which side of the periodic table are metals found

A

left hand side

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28
Q

Properties of METALS THEMSELVES and their abilities

A

High melting and boiling points because of strong metallic bonds
High densities
High tensile shape- Hard to break
Malleable (can be hammered into different shapes)
Conduct head and electricity through free electrons

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29
Q

What happens when metals react with oxygen and when they dissolve in water

A

Form metal oxides

Most metal oxides are solid at room temperature and form basic solutions when you dissolve them in water

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30
Q

What are alloys

A

Changing a metals properties by mixing it with other elements (metals or non metals) to change their structure to make them more; strong, malleable or more corrosion resistant

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31
Q

Properties of non metals

A

Low melting and boiling point, when solid they tend to be weak and brittle. Low density and dont conduct electricity.
Gas or solid at RT

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32
Q

What is neutralization

A

A reaction in which acidity or alkalinity is removed

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33
Q

What does a A neutralization involving an acid and a base (or alkali) always produce?

A

Salt and water

34
Q

What do all acids contain

A

Hydrogen H+ ions, the greater the concentration of these the lower the pH.

35
Q

What base forms if hydrochloric acid is used

A

Chloride

36
Q

What base forms if Nitric acid is used

A

Nitrate

37
Q

What base forms if Sulfuric acid is used

A

Sulfate

38
Q

What base forms if phosphoric acid is used

A

Phosphate

39
Q

If the acid hyrdochloric acid is used with the base copper oxide, what salt will be formed?

A

copper chloride + water

40
Q

Test for hydrogen

A

A lighted wooden splint that makes a squeaky pop

41
Q

Test for Oxygen

A

A glowing wooden splint relights in a test tube of O

42
Q

Test for Carbon Dioxide

A

Lighted splint goes out or Bubble test through limewater (calcium hydroxide solution) CO2 will turn lime water a cloudy white.

43
Q

Test for Ammonia

A

Sharp, choking smell. Turns damp red litmus paper blue

44
Q

Test for chlorine

A

Sharp, choking smell. Turns damp blue litmus paper red and then bleaches it white

45
Q

What do Titrations allow us to do

A

Used to find out concentrations, Find out exactly how much acid is needed to neutralize a given quantity of alkali (or vice versa)

46
Q

Describe the experiment of a titration

A

Measure out a set volume of alkali into a flask with a pipette. Add drops of indicator.
Fill a burette with a standard solution (a known concentration of acid)
Use the burette to add the acid to the alkali bit at a time. Swirl the flask regularly. Slowly (drop at a time) when the alkali’s almost neutralized.
The indicator changes colour when all the alkali is neutralized (end point).
Record the volume of acid used to neutralize the alkali (titrate)
Repeat process to get concordant results (WITHIN 0.2)

47
Q

Why can’t you use a universal indicator

A

It changed colour gradually and you need a single colour change

48
Q

What should you remember to do first in a titration

A

Do a rough one first to rinse out the equipment.

49
Q

Indicators used and what colours they should turn

A

Phenolphthalein- colourless in acids and pink in alkali

Methyl orange- yellow/peach in alkali but red in acids

50
Q

what are the 2 techniques for the Production of ethanol

A

Fermentation of glucose and hydration of ethene

51
Q

Describe Fermentation

A

Sugars from plant material is converted into ethanol and CO2. The enzymes found in single celled fungi YEAST are the natural catalysts for this process. Temperatures required are 30-40*, with 1 atmosphere pressure and rate is slow. Thank

52
Q

What needs to happen after fermentation process

A

To purify it, it needs to be fractionally distilled to concentrate the ethanol.

53
Q

Describe hydration of ethene

A

Reacting ethene from crude oils with steam, a catalyst of phosphoric acid is used to ensure a fast reaction. Non renewable, works at temperatures of 300* and 65 atmospheric pressure, highly pure product

54
Q

How are soluble salts made

A

Soluble salts can be made from acids by reacting them with solid insoluble substances, such as metals, metal oxides, hydroxides or carbonates.

55
Q

Practical for making insoluble salts

A

Using precipitation reactions where you pick 2 soluble salts, they react and you get your insoluble salt eg- mix lead nitrate and sodium chloride to make lead chloride

56
Q

What is atom economy

A

A way to measure the atoms wasted to make a chemical. The higher atom economy the “greener” the process.

57
Q

what does 100% atom economy mean

A

all the atoms in the reactants have been converted to the desired product.

58
Q

How to calculate atom economy

A

Mr of desired products∕sum of Mr of all products × 100

59
Q

What does poly(ethene) show

A

Simple polymers consist of large molecules containing chains of carbon atoms

60
Q

limitations of particular representations and
models, to include dot and cross, ball and stick models and
two- and three-dimensional representations

A 
Mainly applies well to the smaller class of solids composed of group 1 and 2 elements with the highly electronegative elements such as halogens- can't show large molecules 
In covalent molecular, the dot-cross diagrams don’t show the relative attraction of shared electrons due to electronegativity
61
Q

What is the molar volume of any gas at room temperature and pressure

A

24dm3 or 24000cm3

62
Q

What do chemical cells do

A

produce a voltage until one of the reactants is used up

63
Q

What is used in a hydrogen-oxygen fuel cell to produce a voltage

A

hydrogen and oxygen are used to produce a voltage and water is the only product

64
Q

Evaluate the strengths and weaknesses of fuel cells for given uses

A

Environmental benefit – only water produced
Overall has a greater efficiency
Rechargeable
Expensive
Difficulties of transportation and storage of hydrogen

65
Q

How did Mendeleev arrange his periodic table

A

In order of relative atomic mass

66
Q

What are the steps for finding percentage yield

A

1- Ar Mr find number of moles
2- Use balance equation DP TR
3-Find mass —> KG
4- Percentage yield equation

= actual yield/ theoretical yield * 100

67
Q

How to convert gdm3 to moldm3

A

Divide conc in gdm3 by MR of solute

68
Q

Steps for finding concentration from titrations

A

Find moles of acid or alkali (opposite from question)
Use equation to find ratios- Multiply to make same if not already
Use formula triangle to find conc of acid or alkali (what question asks)

69
Q

How to find number of protons, neutrons and electrons

A

Protons and electrons are the same and are the bottom number= atomic number
Neutrons and protons are in the top number= mass number

70
Q

Where does oxidation occur

A

At the anode

71
Q

Where does reduction occur

A

At the cathode

72
Q

How do we know what group ma elements in

A

The amount of electrons it has on its outer she

P

73
Q

How do we know what period an elements in

A

How many shells of electrons it has

74
Q

Explain the practical for making soluble salts

A

Measure required volume of acid with measuring cylinder and add the weighed solid (insoluble metal, oxide, hydroxide or carbonate) in small portions with stirring.
Safety goggles required- the mixture may be heated to speed up the reaction. When no more of the solid dissolves, it means all the acid is neaturalised and there should be a little excess solid. Filter the solution to remove the excess solid into evaporating fish. On filtration, only a solution of the salt is left. Then hot concentrated solution is left to cool and crystallise. After crystallisation, you collect and dry the crystals with a filter paper. If the solution is heated, the solvent will evaporate faster. Heating a solution until all the solvent has evaporated is known as heating to dryness

75
Q

What are soluble

A 
All nitrates 
All common sodium, potassium and ammonium salts 
Most chlorides 
Most sulfates
Sodium potassium and ammonium carbonates
Sodium potassium and ammonium hydroxides
76
Q

What are insoluble

A

Silver chloride and lead chloride
Lead sulfate, barium sulfate and calcium sulfates
Most carbonates
Most hydroxides

77
Q

Practical for making insoluble salts

A

Mix together solutions of soluble salts
Insoluble salt will form a precipitate in the solution
Filter off the precipitate and wash several times with pure water
Dry precipitate in an oven

78
Q

What’s the definition of an alkali

A

Example of a soluble base

79
Q

What is a base

A

Any substance that reacts with an acid to form salt and water only

80
Q

What’s the general equation for a reaction between acids and metal oxides

A

Acid + metal oxide —salt +water

81
Q

What’s the general equation for a reaction between acids and metal hydroxides

A

Acid + metal hydroxide — salt + water

82
Q

What’s the general equation for a reaction between acids and metal carbonates

A

Acid + metal carbonate — salt+ water + carbonate

Chemistry revision (10 decks)

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