Paper 1 practice questions

Question 1

Why is graphite used for the electrodes?

Answer 1

Graphite has delocalised electrons to carry charge
graphite is inert

Question 2

A student is trying to measure the mass of copper he has how would he measure it?

Answer 2

filter the mixture
wash and dry the reisdue
weight the mass of copper collected
add to the mass of the electrode

Question 3

suggest why the blue of copper nitrate solution fades during electrolysis

Answer 3

The copper ions are discharged

Question 4

give two differences between the physical properties of the elements between group 1 and transition elements

Answer 4

Transition metals are much stronger
Group 1 is softer then transition
transition metals are more dense

Question 5

describe how metals conduct electricity anwser in terms of electrons

Answer 5

metals conduct electricity with it’s delocalised electrons, metals are very dense so charge easily flows through the structure

Question 6

name the type of bonding in between metals and non-metals

Answer 6

IONIC

Question 7

In a reaction profile graph what does the Y axis and X axis measure?

Answer 7

Y = overall energy change
X = energy

Question 8

describe the structure and bonding of diamond

Answer 8

Diamond has 4 covalent bonds with carbon
which are very strong
because it is a giant covalent structure

Question 9

Why are fullerenes used to move medicines inside of the body?

Answer 9

Fullerenes usually have a spherical shape that is hollow (easy to put medicine inside of it)

Question 10

predict one observation you would see that shows that rubidium is more reactive then sodium

Answer 10

A more violent reaction

Question 11

is it true that all noble gases have eight electrons on it’s outer shell?

Answer 11

No, because helium only has 2

Question 12

why should the products of electrolysis be kept apart?

Answer 12

Prevents an irreverisble reaction e.g when it is a solid it is much harder to react with

Question 13

explain why aluminium is more reactive then carbon?

Answer 13

As alumium is always found as a compound which means electrolysis is needed to extract it.
electroylsis requires high temperatures and energy to extract it.

Question 14

explain why the pH of an acid depends on the strength of the acid
the concentration of the acid

Answer 14

pH depends on the H+ ion concentration the higher the concentration means the lower the pH
a strong acid will fully ionise in water while a weak acid will only partially ionise which lowers the pH

Question 15

explain why the electrical conductivity of an ionic solution is zero when it has been neutralised

Answer 15

No ions are free to move, as neutralisation makes a salt which is a solid.
And all of the OH- and H+ ions have fully reacted

Question 16

explain why adding an alkali to a solution will increases it’s electrical conductivity

Answer 16

more delocalised ions in the solution

Question 17

In the modern periodic table, the elements are arranged in order of ?

Answer 17

by there atomic number

Question 18

Sodium is in group one
describe what you would see when sodium reacts with chlorine

Answer 18

Coloured gas from the chlorine
white solid forming
flame/effervesence

Question 19

Evidence from the alpha scattering experiment led to a change in the model of the atom from the plum pudding model
explain how

Answer 19

most of the alpha particles passed straight through
so the mass of the atom is concentrated at the centre
some were deflected so it has a charged nucleus in the centre

Question 20

suggest why the student used a polystyrene cup rather than a glass beaker for a reaction

Answer 20

Is a better thermal insulator
so reduces energy exchange

Question 21

The products of electrolysis are lead and bromine why should the teacher do the demonstration in a fume cupboard?

Answer 21

a lead is toxic/poisonous

Question 22

Methane is a gas at room temperature but poly ethene is a solid at room temperature
explain why they exist in different states at room temp

Answer 22

Methane is a small molecule
with weak intermolecular forces
which need little energy to over come them
resulting in a lower melting/boiling point

Question 23

Explain how oxygen was formed from water during electrolysis of this aqueous solution

Answer 23

the water molecules break down
into H+ and OH-
the OH- is attracted to the positive electrode
where the OH- is discharged to give oxygen

Question 24

explain why hydrogen chloride is a gas at room temperature

Answer 24

Hydrogen chloride is made of small molecules
so has weak intermolecular forces
require little energy to overcome

Question 25

Explain why a student should use a pipette to measure the dilute sulfuric acid and a burette to measure the sodium hydroxide solution

Answer 25

Pipette measures a fixed volume accurately
burette measures variable volume