Q1

Q2

Draw the electronic structure of the ions in Sodium chloride

Q4

Fill in the blanks Charge

Relative mass

proton electron neutron

Q7 Draw out the electron structure to show the covalent bonding in Methane CH4

Draw the electronic structure of the ions in Magnesium oxide

Q5 What type of bonding is present in Water (H2O), Hydrogen (H2), Ammonia (NH3), Hydrogen Chloride (HCl), Methane (CH4) and Oxygen (O2)?

Q8 Draw out the electron structure to show the covalent bonding in Water H2O

Q3 Draw the electronic structure of the ions in Calcium chloride

Q6 Draw out the electron structure to show the covalent bonding in Hydrogen H2

Q9 Draw out the electron structure to show the covalent bonding in Oxygen O2

A3

A6

A9

A2

A1

A5

A4 A4

Charge

Relative mass

proton

+1

1

electron

-1

Almost 0

neutron

0

1

Covalent bonding (sharing electrons). This is because they are all molecules of non-metals

A8

A7

Q10 What is chemical bonding?

Q13 What is the structure of an Ionic compound

Q11 What type of bonding involves transferring electrons (gaining or losing electrons)

Q14 Some covalent substances (H2, CO2, H2O, CH4) make simple molecules. What are the properties of simple molecules?

Q16

Q17 HT only

What is the structure of Metals?

How are metal atoms held together in a metallic structure?

Q12 What type of bonding involves sharing of electrons?

Q15 Give two examples of giant covalent structures (macromolecules)

Q18 HT only Why do simple covalent molecules have low melting and boiling points?

A12

Covalent bonding.

Compounds made from nonmetals make molecules by sharing electrons.

A15 Diamond and Silicon dioxide (also Graphite)

A18 The only forces to overcome on heating are the weak intermolecular forces between the covalent molecules.

A11

Ionic bonding.

Metal atoms lose electrons to make positive ions. Non-metal atoms gain electrons to make negative ions.

A14 Simple molecules make solids, liquids or gases with low melting and low boiling points

A17

The electrons in the outer

energy levels of the metal atoms are delocalised and free to move. There is then a strong electrostatic attraction between the positive metal ions and the negative electrons.

A10

Chemical bonding is

transferring or sharing electrons to get a stable electron structure (like the noble gases)

A13 Ionic compounds are giant structures (lattice) of ions held together by strong electrostatic forces between oppositely charged ions

A16 Metals consist of a giant structures, with atoms arranged in a regular pattern.

Q19

Q20

How do you find Ar and Mr for a substance

Q22

HT

What is the empirical formula?

Q23

HT

What is a mole (in chemistry)? How do you work out percentage yield?

Q25 What are reversible reactions?

Q26 What is nanoscience?

Q21 How do you calculate the percentage of an element in a compound?

Q24 Why is it important to achieve a high yield in industry?

Q27 What is a shape memory alloy?

A21 Ar of element x 100 Mr of compound The percentage of Na in NaOH is: 23 (Ar of Na) x 100 = 57.5% 40 (Mr of NaOH)

A19

A20 The formula showing the simplest ratio of elements present in a compound.

A24

A23

This minimises energy wasted, conserves Earth’s resources, reduces pollution and makes a greater profit.

Mass of chemical obtained

Ar (relative atomic

mass) can be read from the periodic table for any element. The Mr (relative molecular mass) is the sum of Ar in a formula: NaOH = 23+16+1 = 40

A22

A mole of any substance is

The maximum mass possible is calculated from the reaction equation.

its relative formula mass (Mr) in grams. Mass (g) Moles = Ar or Mr

A27

A26

A25

If a shape memory alloy is deformed, it returns to its original shape on heating.

Nanoscience is the study of small particles that are between 1 and 100 nanometres in size

In reversible reactions the products can react again to make the original reactants. These are shown with a double arrow 

x 100

Maximum mass of chemical possible

e.g. NH4Cl  NH3 + HCl

Q28

HT

Why are metals such good conductors of heat?

Q31 What are food additives?

Q34 What two instruments or techniques are needed to analyse compounds in a sample mixture?

Q29

Q30

What affects the properties of polymers?

What is the difference between thermo-setting and thermo-softening polymers?

Q32 How can we detect artificial food colourings?

Q33 What are the advantages of instrumental methods of analysis?

Q35

Q36

What is the equation to work out the rate of reaction?

What are the 4 main things affecting the rate of a reaction?

A30

The properties are affected by the monomers used and the reaction conditions

HT Thermosetting polymers have strong cross links (covalent bonds).

A33 Modern instrumental techniques are: faster, more accurate and more sensitive.

A36   



Temperature Surface area Concentration (of solutions) or Pressure (of gases) Presence of a catalyst

A28

A29

Thermo-softening polymers are softened or melt easily when heated. Thermo-setting polymers will not soften on heating and will char.

Delocalised electrons can flow through the metal lattice allowing electrical current and heat energy to be transferred quickly.

A32

A31

Paper chromatography .

Food additives are added to food to improve flavour, appearance and shelf life.

A35 Rate of reaction = or Rate of reaction =

amount of reactant used time amount of product formed time

A34 1) Gas chromatography which separates the compounds 2) Mass spectrometer that identifies compounds based on their relative molecular mass (Mr)

Q37

Q38

Q39

What is collision theory?

Explain how surface area affects the rate of a reaction.

Explain how temperature affects the rate of a reaction.

Q40

Q41

Explain how concentration affects the rate of a reaction.

Explain how pressure affects the rate of a reaction (in gases)

Q43 What are the advantages and disadvantages of using catalysts in industry?

Q44 What is an exothermic reaction?

Q42 What do catalysts do to the rate of a reaction?

Q45 What is an endothermic reaction?

A39 The higher the temperature, the faster the rate of reaction. (pattern) This is because the frequency and energy of collisions is increased between reacting particles. More collisions are successful as they have exceeded activation energy. (reason)

A42 Catalysts speed up the rate of reaction, but they are not used up in the reaction. Different catalysts are needed for different reactions.

A45 A reaction which absorbs heat energy from its surroundings .

A38 The larger the surface area, the faster the rate of reaction (pattern) This is because the frequency of collisions is increased between reacting particles (reason)

A41 The greater the pressure, the faster the rate of reaction. (pattern) This is because the frequency of collisions increases between reacting particles. (reason)

A44 A reaction which releases heat energy to its surroundings.

A37

Particles must collide

before they can react. Not all collisions cause a reaction. The minimum energy the particles must have in order to react is called Activation energy.

A40 The greater the concentration, the faster the rate of reaction. (pattern) This is because the frequency of collisions increases between reacting particles. (reason)

A43

Advantages: faster reactions

and reduced energy costs. Modern catalysts (nanoparticles) have less waste and are more efficient Disadvantages: catalysts are often harmful transition metals or their compounds which can be toxic in the environment

Q46

Q47

How is energy transferred in a reversible reaction?

What products use the energy from exothermic reactions?

Q49

Q50

What is an acid?

What are bases and alkalis?

Q48 What products use the cooling effect of endothermic reactions?

Q51

Making salts 1

What salts can we make from hydrochloric, sulphuric and nitric acids?

Q52

Making salts 2

What happens when a metal and acid react?

Q53

Making salts 3

How do we make a salt from an acid and insoluble base?

Q54

Making salts 4

What happens when an acid and alkali react?

A48

A47

Instant cold packs for sports injuries or burns.

Hand warmers and self-heating cans.

A50

A51 Acid

Formula

Type of salt

Hydrochloric acid

HCl

chlorides

Sulphuric acid

H2SO4

sulphates

Nitric acid

HNO3

nitrates

A54 acid + alkali a salt + water

A base is a substance that

can neutralise an acid. Bases that are soluble in water and are called alkalis, they produce OH- ions. The pH of alkalis are more than 7 (pH from 7-14, a pH of 14 is more alkaline than a pH of 8)

A53

1) add acid to insoluble base

2) heat gently and then filter off the excess (un-reacted) base 3) evaporate the water from the solution to make crystals of the salt acid + base salt + water H2SO4 + CuO  CuSO4 + H20

A46

The amount of energy

released when the reaction goes in one direction is exactly the same as the amount of energy absorbed when it goes in the other direction.

A49

A substance that produc-

es H+ ions when it is dissolved in water. The pH of acids is less than 7 (pH from 0-7, a pH of 2 is more acidic than a pH of 5)

A52 Metal + Acid a Salt + Hydrogen (MASH)

Q55

Making salts 5

How do we make insoluble salts?

Q56 What is electrolysis and what type of substances can we electrolyse?

Q58

Q59

How does water affect electrolysis?

How is aluminium extracted from aluminium oxide (ore)?

Q61 What is produced when we electrolyse brine (sodium chloride solution)?

Q62 What are the products of brine electrolysis used for?

Q57 What happens to the ions in electrolysis?

Q60 What happens at the electrodes during aluminium oxide electrolysis?

Q63 How do we electroplate objects?

A57

Positive (usually metal) ions

move to the negative electrodes. Negative ions move to the positive electrodes. Negative ions are oxidised, positive ions are reduced. Oxidation Is Loss of electrons, Reduction Is Gain of electrons (OILRIG)

A60 Negative electrode: Al3+ ions gain 3 electrons and become aluminium atoms, molten aluminium is tapped off. Positive electrode: O2- ions lose 2 electrons and become oxygen atoms which pair off to give molecules of oxygen gas (O2)

A63 The metal object to be plated is placed at the negative electrode in an electrolysis cell. The metal to coat the object with is placed at the positive electrode.

A56

Electrolysis is where a

A55

substance is broken down using electricity. Ionic compounds which are in solution or are molten can be used as their ions are free to move.

A59

Insoluble salts are made

when two solutions react to produce a precipitate. This can be used to remove unwanted ions from solution, e.g from industrial waste water.

A58

The aluminium oxide is

Hydrogen and metal ions both go to the negative electrode, the less reactive element is made there. (look at the reactivity series on the data sheet in the exam)

mixed with molten cryolite, and extracted by electrolysis. Cryolite is essential to reduce the melting point.

A62

A61

Chlorine: to make bleach and plastics Hydrogen: to make margarine Sodium hydroxide: to make bleach, paper and soap

  

Chlorine gas Hydrogen gas Sodium hydroxide solution