Bonding structure and properties of matter

Question 1

What type of ion do elements from the following groups form:
Group 1
Group 7

Answer 1

Group 1 = +1 ions (positive)

Group 7= -1 ions(negative)

Question 2

Describe how ionic bonds form

Answer 2

When a metal and non-metal react together the metal atom loses electrons to form a positively charged ion and the non-metal gains these electrons to form a negatively charged ion. These oppositely charged ions are strongly attracted to one another by electrostatic forces. This is called an ionic bond.

Question 3

Describe the structure of a crystal of sodium chloride

Answer 3

The sodium atom gives up its outer electron, becoming an Na+ ion. The chloride atom picks up the electron, becoming a Cl- (chloride) ion.

Question 4

List the main properties of ionic compounds

Answer 4

high melting points and high boiling points.

Question 5

Describe how covalent bonds form

Answer 5

When non-metal atoms bond together, they share pairs of electrons to make covalent bonds.

Question 6

Explain why simple molecular compounds typically have low melting and boiling points.

Answer 6

Simple molecular substances are made up of molecules containing a few atoms joined together by covalent bonds; to melt or Bol these substances you only have to break these feeble intermolecular forces not the covalent bonds. So the molecules are easily parted.

Question 7

Describe the structure of a polymer

Answer 7

Small units are linked together to make a long molecule. All of the atoms are joined by covalent bonds.

Question 8

Give three examples of giant covalent substances

Answer 8

Diamond
Graphite
Silicon dioxide

Question 9

Explain why graphite can conduct electricity

Answer 9

It has one delocalised (free) electron which can move.

Question 10

Explain how fullerenes could be used to deliver drugs into the body

Answer 10

Fullerenes can be used to cage other molecules. This fullerene structure forms around another atom or molecule which is then trapped inside. This could be used to deliver a drug into the body.

Question 11

What is metallic bonding?

Answer 11

The electrons on the outer shell of the metal atoms are delocalised. There are strong forces of electrostatic attraction between the positive metal ions and the negative electrons. These forces of attraction hold the atoms together in a regular structure and are known as metallic bonding.

Question 12

List three properties of metals and explain how metallic structure causes each property.

Answer 12

• Malleable as the layers of atoms in a metal can slide over each other.
• Good conductors of electricity/heat as they have delocalised electrons which carry electrical current and thermal energy through the whole structure.

Question 13

Explain why alloys are harder than pure metals

Answer 13

Different elements have different sized atoms so when another element is mixed with a pure metal, the new metal atoms will distort the layers of metal atoms making it more difficult for them to slide over each other.

Question 14

Name the three states of matter

Answer 14

Solid, Liquid and gas.

Question 15

What is the state symbol of an aqueous substance?

Answer 15

aq

Question 16

What is the name of the temperature at which a liquid becomes a gas?

Answer 16

the boiling point

Question 17

How does the strength of the forces between particles influence the temperature at which a substance changes state?

Answer 17

The stronger the forces the more energy is needed to break them and therefore the higher the melting and boiling points of the substance.