Bonding

Question 0

What’s the mass number?

Answer 0

The total number of protons and neutrons.

Question 1

What is the Atomic Number?

Answer 1

The Number of Protons.

Question 2

Whats the relative mass of a proton neutron and electron?

Answer 2

1) Proton and Neutron = 1

2) Electron = 0

Question 3

Why do we not include the mass of electrons in the mass number?

Answer 3

Their relative mass is very small.

Question 4

What is an Isotope?

Answer 4

Different Atomic form of the same element - which have the same number of protons but different number of neutrons.

Question 5

What is ionic bonding?

Answer 5

The transferring of electrons.

Question 6

If an element loses one electron what will its overall charge be?

Answer 6

+

Question 7

What are the characteristics of Ionic Compounds?

Answer 7

1) Giant Ionic Lattice
2) Very strong electrostatic forces of attraction between oppositely charged ions.
3) High Melting/Boiling Point
4) Carry Electric Current

Question 8

Why do ionic Compounds Conduct Electricity When Dissolved?

Answer 8

Ions are separated and free to move and carry current.

Question 9

Why do Ionic compounds have high Melting/Boiling Points?

Answer 9

Strong attractions between ions take large amounts of energy to overcome.

Question 10

What Are The Characteristics Of Simple Molecular Substances?

Answer 10

1) Very strong covalent bonds
2) Very weak intermolecular forces
3) Very low Melting/Boiling Points

Question 11

What are the characteristics of Giant Covalent Structures (Macromolecules)?

Answer 11

1) No charged ions
2) All atoms strong covalent bonds
3) Very High Melting/Boiling Points

Question 12

Give examples of Giant Covalent Structures…

Answer 12

1) Diamond - Carbon

2) Graphite - Silicon Dioxide

Question 13

Describe the Structure of Diamond…

Answer 13

1) Each atom forms 4 Covalent Bonds

2) Very Rigid

Question 14

Describe the structure of Graphite…

Answer 14

1) Forms 3 Covalent Bonds creating Layers that are free to slide over each other. It’s soft and slippery.
2) Layers loose - rubbed off - weak intermolecular forces.
3) Good conductor
4) Each carbon atom has one delocalised electron

Question 15

Describe metallic bonds…

Answer 15

1) Free delocalised electrons on the outer shell of every atom.
2) Strong electrostatic attraction between positive metal ions and negative electrons.
3) Slide over each other to be bent and shaped.

Question 16

Why are alloys harder than pure metals?

Answer 16

Different elements gave different sized atoms so when they’re mixed layers are distorted making it difficult for them to slide over each other.

Question 17

What type of structures are there?

Answer 17

1) Giant Ionic
2) Simple Covalent
3) Giant Covalent
4) Giant Metallic