GC

SE SC

IEN

CE

: Chem

istry 2. Structure, Bonding &

the Properties of Matter

Section 1: Ions & Ionic Bonding

1 What charge do electrons have? -1

2What charge will an ion of lithium take? 1+ (one electron in the outer shell, needs to

lose it)

3What charge will an ion of beryllium take? 2+ (two electrons in the outer shell, needs to

lose them both)

4What charge will an ion of barium take? 2+ (group 2 so two electrons in the outer shell,

needs to lose them both)

5 What charge will an ion of fluorine take? 1- (7 electrons in the outer shell, needs to gain one)

6If something has gained electrons, what charge will it have?

Negative

7If something has lost electrons, what charge will it have?

Positive (because they have lost a negative!)

8 What charge will an ion of oxygen take? 2- (6 electrons in outer shell so needs to gain two)

9What charge will an ion of Selenium take? 2- (group 6, so has 6 electrons in the outer shell

and needs to gain two)

10Explain in terms of electrons what occurs when lithium bonds with chlorine

One electron transferred from lithium to chlorine

11 Why do atoms transfer electrons in ionic bonding?

So that they can have full outer shells

12Explain in terms of electrons what occurs when lithium bonds with fluorine

One electron transferred from lithium to fluorine

13Explain in terms of electrons what occurs when magnesium bonds with oxygen

Two electrons transferred from magnesium to oxygen

14Explain in terms of electrons what occurs when beryllium bonds with oxygen (3 marks)

Two electrons transferred from beryllium to oxygen

15 Explain in terms of electrons what occurs when magnesium bonds with chlorine

One electron transferred from magnesium to two different chlorine atoms

16Explain in terms of electrons what occurs when sodium bonds with oxygen

Two electrons transferred to an oxygen atom from two different sodium atoms

17Why do sodium ions and chlorine ions form an ionic bond?

There is an electrostatic force of attraction between oppositely charged ions

18 Why don't sulphur ions and oxygen ions form ionic bonds with each other?

Both have negative charges so would repel

GC

SE SC

IEN

CE

: Chem

istry 2. Structure, Bonding &

the Properties of Matter

Section 1: Ions & Ionic Bonding continued

19What is the name for a substance made of billions of oppositely charged ions joined together?

Giant ionic lattice

20 Define giant ionic lattice A huge 3D network of ions

21 State the melting points of ionic substances High

22Explain why ionic substances have high melting points.

Strong bonds between oppositely charged ions are hard to break

23Will NaCl(s) conduct electricity? No

24Will NaCl (aq) conduct electricity? Yes (aq stands for aqueous which means it is

dissolved in water)

25 Will NaCl (l) conduct electricity? Yes

26 What does molten mean? Melted

27Explain why ionic compounds do not conduct electricity when solid

Because the ions are not free to move

28Explain why ionic compounds conduct electricity in solution

Because the ions are free to move

29Explain why ionic compounds conduct electricity when molten

Because the ions are free to move

30 What does soluble mean? Dissolves in water

31 What does insoluble mean? Does not dissolve in water

32Magnesium carbonate is insoluble. What do you need to do before it will conduct electricity?

Melt it

33Sodium fluoride is soluble. Explain what the easiest way for it to conduct electricity is

Dissolve it in water because this does not require high temperatures

GC

SE SC

IEN

CE

: Chem

istry 2. Structure, Bonding &

the Properties of Matter

Section 2: Covalent Bonding

34 Explain why chlorine and fluorine form covalent bonds

They are both non-metals

35 Complete the sentence: In covalent bonds, electrons are _______________________

Shared

36 In ionic bonds, electrons are ___________________

Transferred

37 What is the name given to the structure of diamond, graphite and silicon dioxide?

Giant covalent

38 How many bonds does each carbon have in diamond?

4

39 Explain why diamond has a high melting point

Giant structure, Strong covalent bonds between the atoms, requires a lot of energy to break

40 Explain why most giant covalent substances do not conduct electricity (3 marks)

There are no electrons/ions/charged particles that are free to move

41 Explain why graphite conducts electricity Has delocalised electrons between the layers that can move through the graphite

42Making full reference to structure and bonding in graphite, explain how it conducts electricity

Each carbon has 3 bonds, 1 electron is delocalised, free to carry charge through the graphite

43 Explain why graphite can act as a lubricant Weak forces between layers which are free to slide over each other

44 What is graphene? One layer of graphite

45 What is a fullerene? Substance made of carbon atoms arranged in a cage

46 What type of substance are methane and water?

Simple molecular (or simple molecules)

47 What is a molecule? A group of atoms chemically bonded together

48 Describe the structure of simple covalent molecules

Strong covalent bonds between atoms, weak forces holding the molecules together

49 What are intermolecular forces? Weak forces between molecules which hold them together

50Explain why methane has a low melting point

It is a simple molecular substance with weak forces between the molecules (which are easy to break)

51 What is a polymer? Millions of small molecules joined together in a chain to form a large molecule

Silica has a giant covalent structure containing silicon atoms (grey) and oxygen atoms (red)

Carbon atoms in diamond form a tetrahedral arrangement

GC

SE SC

IEN

CE

: Chem

istry 2. Structure, Bonding &

the Properties of Matter

Section 3. Metals & Alloys

52 Describe the main features of metals in terms of their structure

Positive metal ions arranged in layers with delocalised electrons

53 Explain why metals can conduct electricity Delocalised electrons are free to carry charge

54 Explain why pure metals are soft Layers of metal ions are free to slide over each other

55 What is an alloy? A mixture of two or more elements, at least one of which is a metal

56 Give a reason for alloying a metal To make it harder, to make it less reactive

57 Explain why alloys can be harder than pure metals

Different size of atoms disturb the layers to stop them sliding over each other

Section 4. Nanoparticles

58 How big are nanoparticles? 1-100nm, a few hundred atoms

59 Why do nanoparticles have different properties to bulk materials?

Because of their high SA:V ratio

60 Give two examples of what nanoparticles can be used for

Medical applications, sun creams, catalysts, deoderants, cosmetics, electronics