C3: Structure and Bonding

Question 1

Covalent Bonding vs Ionic Bonding

Answer 1

Sharing electrons vs transferring electrons.

Question 2

Giant Ionic Lattice

Answer 2

A huge 3D network of ions, held together by electrostatic attraction (ionic bonding).

Question 3

Group 1 Ionic Charge

Answer 3

1+

Question 4

Group 2 Ionic Charge

Answer 4

2+

Question 5

Group 3 Ionic Charge

Answer 5

3+

Question 6

Group 4 Ionic Charge

Answer 6

Group 4 don’t form Ions.

Question 7

Group 5 Ionic Charge

Answer 7

3-

Question 8

Group 6 Ionic Charge

Answer 8

2-

Question 9

Group 7 Ionic Charge

Answer 9

1-

Question 10

Group 0 Ionic Charge

Answer 10

Group 0 never form ions.

Question 11

Electrostatic Attraction

Answer 11

The force of attraction between positively and negatively charged ions. Act in all directions.

Question 12

Giant Ionic Structure Facts.

Answer 12

Held together by strong electrostatic attraction.

Very high melting and boiling points because of this.

Question 13

What happens when an ionic solid melts and becomes a liquid?

Answer 13

The ions are free to move anywhere in the liquid.
Attracted to oppositely charged electrodes dipped into the liquid.
Therefore, they carry their electrical charge through the liquid.
Conduct Electricity.
Water also separates many ionic solids and allows them to conduct electricity.

Question 14

Covalent Bonds

Answer 14

The bonds between two atoms that share one or more pairs of electrons.

Question 15

Example of a Macromolecule.

Answer 15

Diamond.
Each carbon atom forms four covalent bonds with its neighbours.
This results in a rigid giant covalent lattice.

Question 16

Covalent Bond Facts

Answer 16

Covalent bonds are very strong, so the two atoms it joins are very tightly bonded.
However, their intermolecular forces are very weak. Overcoming them is relatively easy and requires little energy.

Question 17

Do covalently bonded substances conduct electricity?

Answer 17

No.

Question 18

Giant Covalent Structures/ Macromolecules

Answer 18

STRONG covalent bonds
High melting and boiling points
Insoluble in water
Hard, do not conduct electricity (except for graphite)

Question 19

Graphite

Answer 19

> Carbon atoms bond to three other carbon atoms.
Form hexagons which are arranged in giant layers.
Layers can slide over each other easily.
Graphite is soft and slippery- Easily malleable.
The fourth electron in Carbon’s outer shell becomes a DELOCALISED ELECTRON- These allow graphite to conduct electricity.

Question 20

Fullerenes

Answer 20

Form of the element carbon that can exist as large cage-like structures, based on hexagonal rings of carbon atoms.

Question 21

Nanoscience

Answer 21

The study of particles that are between 1 and 100 nanometres in size.

Question 22

How do nanoparticles behave?

Answer 22

Differently to their larger scale counterparts.