Chemistry Paper 1 Revision

Knowledge Questions

Topic 1- Atomic Structure

and the periodic Table

Topic 2- Bonding, Structure

and Properties of Matter

Why am I doing this?

To answer exam questions you need to understand the basic knowledge first.

These questions are designed to help you understand the basics, before moving

on to exam style questions.

Resources to help:

• Electronic Revision Guide (ask your teacher if you have forgotten your

code)

• GCSE Bitesize Chemistry (AQA)

• Resources on singhscience.co.uk

• Focus E-Learning

What if I finish these and want to try some

exam questions?

Go onto www.singhscience.co.uk and answer the

exam questions on these two topics.

A. Atoms, Elements, Compounds and Mixtures part 1 – Atoms, Elements, Compounds, Word and Symbol Equations

1. How many different types of atoms are there?

2. What does it mean if a compound ends in –ide?

3. What does it mean if a compound ends in –ate?

4. What does a chemical reaction involve?

5. Name the following substances:

• NaCl

• NaSO4

6. Why is it useful to have symbols for atoms of different elements?

7. What is the difference between an element and a compound?

8. Why is it difficult to separate a compound?

9. Solid sodium reacts with water to form a sodium hydroxide (NaOH) solution and hydrogen gas.

a) Write a word equation to represent this reaction.

b) Give the balance symbol equation for the reaction.

10. Higher Tier only:

When magnesium reacts with sulfuric acid, the hydrogen ions in the acid will be displaced from the solution by magnesium.

Balance the following ionic equation:

Mg(s) + H+(aq) → Mg2+(aq) + H2(g)

B. Atoms, Elements, Compounds and Mixtures part 2 – Separating Techniques

1. What is the difference between a compound and a mixture?

2. Describe the method used to collect the salt from a mixture of sand and salt.

3. What process is used to purify seawater to obtain usable water?

4. Describe how the following equipment is used to separate water and ethanol.

5. A mixture and six colours are tested using chromatography. The following chromatogram was produced:

a) What can you conclude about the mixture?

b) Why do the inks separate?

C. Atomic Model part 1 – History of the Atom

1. What was the earliest model of the atom?

2. Which subatomic particle did JJ. Thomson discover?

3. Which early atomic model does the following diagram show:

4. Name Rutherford’s experiment.

5. State two ways in which Rutherford changed Thomson’s model of the atom.

6. How did Bohr adapt the nuclear model?

7. Explain why Bohr revised Rutherford’s model of the atom.

D. Atomic Model part 2 – Size and Mass of Atoms and Atomic Structure

1. Name three subatomic particles and their charges.

2. Complete the sentence ‘All atoms of one type of element have the same number of…’

3. What does the atomic number tell us about an atom?

4. What does the mass number tell us about an atom?

5. How is an isotope different to an atom?

6. What is the electron configuration for sodium?

7. Why is the overall charge of an atom zero?

8. Draw the electron configuration for a chlorine atom.

9. Write the electron configuration for potassium.

10. How many electrons does potassium have on its highest energy level?

11. Calculate how many protons, electrons and neutrons there are in: a) A silver atom with atomic number 47 and mass number 108

b)

12. The atomic radius of a bromine atom is 9 x 10 -11m.

a) Give its atomic radius in nanometres.

b) Calculate the radius of the nucleus (in nm), given that it will be about 1/10,000 the radius of

the atom. Give your answer in standard form.

E. Periodic Table part 1 – History of the Periodic Table

1. How are elements arranged in the periodic table?

2. What are the columns of the periodic table called?

3. What are the rows of a periodic table called?

4. What does the column an element is in tell you about the atoms?

5. What does the row an element is in tell you about the atoms?

6. Which side of the periodic table are the non-metals found?

7. How were elements classified before the discovery of subatomic particles?

8. What was the problem with early periodic tables?

9. How did Mendeleev overcome these problems?

10. Why is the order based on atomic masses not always correct?

11. What do we call elements that tend to form positive ions?

F. Periodic Table part 2 – Group 0, group 1 and group 7

1. What are the elements in Group 0 called?

2. What are the elements in Group 1 called?

3. What are the elements in Group 7 called?

4. What happens to the boiling point of elements in Group 0 as you go down the group?

5. Why are the elements in Group 0 so unreactive?

6. Why do all elements in Group 1 react in a similar way to each other?

7. What happens to the reactivity of the elements as you go down Group 1?

8. Write a word equation for the reaction between sodium and oxygen.

9. Why do all the elements in Group 7 react in a similar way to each other?

10. Halogens are diatomic. What does the word ‘diatomic’ mean?

11. What happens to the reactivity as you go down Group 7?

12. What happens to the melting point and boiling point as you go down Group 7?

13. Write a word equation for the reaction between lithium and chlorine.

14. Write a balanced chemical equation for the reaction between lithium and chlorine gas.

A. Changes of State – States of matter

1. What are the three types of strong chemical bond?

2. What particles are found in:

a) Ionic bonding

b) Covalent bonding

c) Metallic bonding?

3. Which type of bonds occurs when metals combine with non-metals?

4. What type of bonding occurs in carbon dioxide? Why?

5. What type of bonding occurs in alloys?

6. What happens to the electrons in ionic bonding?

5. What is the link between the charge number on the ions in groups 1, 2 and 3 and their group number ?

7. What is the link between the charge number on the ions in Groups 1, 2, 6 and 7 and their group?

8. What is an ionic compound?

9. How are ionic compounds held together?

10. Why is the ball and stick model not an accurate representation of the structure of an ionic

compound?

11. Draw a diagram to show how potassium and chlorine atoms join together to form ions.

12. Explain how you can use the following model of sodium chloride to work out the empirical formula.

B. Bonding part 2 – Covalent bonding, metallic bonding

1. How are strong covalent bonds formed?

2. What are the three types of structure that can be formed by covalent bonding?

3. What are polymers an example of?

4. What type of structure do the following covalently bonded substances have?

a) Water H2O

b) Silicon dioxide SO2

c) Diamond

d) Poly(ethene)

5. What are the limitations of using dot and cross diagrams to represent covalent bonds?

6. How are atoms arranged in a metal?

7. Why are metallic bonds so strong?

8. What is the formula of the following model?

9. Draw a dot and cross diagram for water.

10. Describe the arrangement of particles in a metal.

11. Why are the particles that make up a metal described as positively charged?

12. What are delocalised electrons?

C. Properties of substances part 1 – states of matter, state symbols

1. What are the three states of matter?

2. What is used to represent particles in the simple particle model?

3. What takes place at the melting point?

4. What takes place at the boiling point?

5. What factor affects the amount of energy needed to change state?

6. In chemical equations what symbols are used to show the states of matter?

7. In what state of matter do particles have the most energy?

8. What would eventually happen to a gas if pressure is increased?

9. HT ONLY: Explain the limitations of the particle model.

10. The following represents the heating of ice:

a. What change in state happens at stage 2? b. What change in state happens at stage 4?

D. Properties of substances part 2 – Ionic compounds, small molecules, polymers, giant covalent structures, metals and alloys

1. Describe the structure of ionic compounds.

2. Why do ionic compounds have high melting and boiling points?

3. Why can ionic compounds conduct electricity when melted or dissolved in water?

4. What state of matter are small molecules normally found in?

5. Why do small molecules have low melting and boiling points?

6. What happens to the melting and boiling points as small molecules get bigger? Why?

7. Why don’t small molecules conduct electricity?

8. What are polymers?

9. How are the atoms in a polymer linked together?

10. Why are polymers normally solid at room temperature?

11. Give an example of a giant covalent structure.

12. Why do giant covalent structures have very high melting and boiling points?

13. Why do most metals have high melting and boiling points?

14. How are atoms arranged in pure metals?

15. What is an alloy?

16. Why do we use alloys, rather than pure metals, for many uses?

17. Why are metals good conductors of electricity?

18. What is thermal energy?

19. Why are metals good conductors of thermal energy?

E. Properties of substances part 3 – Diamond, graphite, graphene and fullerenes

1. In a diamond, how many covalent bonds does each carbon make?

2. Diamond does not conduct electricity. Why?

3. Name 2 other properties of diamond.

4. In graphite, how many covalent bonds does each carbon make?

5. Describe the structure of graphite.

6. Why is graphite soft?

7. Why does graphite conduct electricity?

8. How is graphite similar to metals?

9. What is graphene?

10. What are fullerenes?

11. What was the first fullerene to be discovered?

12. What are carbon nanotubes?

13. What are carbon nanotubes useful for?