Atomic Structure - Types Of Bonding

Question 1

Atomic number

Answer 1

No. of protons

Question 2

Atomic mass number

Answer 2

No. Of protons + neutrons

Question 3

Relative mass of protons neutrons and electrons

Answer 3

1 1 and 1/1840

Question 4

Relative charge protons neutrons and electrons

Answer 4

+1 0 -1

Question 5

Position of protons neutrons and electrons

Answer 5

Nucleus , nucleus, shell

Question 6

Who discovered the plum pudding model

Answer 6

JJ Thompson - 1897

Question 7

Who did the gold foil experiment? When?

Answer 7

Rutherford - 1911

Question 8

Who discovered the neutron? When?

Answer 8

Chadwick- 1932

Question 9

Ions are?

Answer 9

Charged particles
Positive ions formed when atoms lose electrons
Negative ions formed when atoms gain electrons

Question 10

Size of the atom

Answer 10

Atoms have a radius of 0.1 nanometres (nm) or 1 x 10 to the power of -10m

Question 11

What are isotopes

Answer 11

Atoms of the same element which have the same number of protons but different numbers of neutrons

Question 12

How to find relative atomic mass - R.A.M

Answer 12

R.A.M = (Mass Number 1 x abundance) + ( Mass number 2 x abundance) / total abundance

Question 13

What is ionic bonding and what is it called?

Answer 13

Giant ionic lattice

Occurs in metal ions when reacting with non-metal ions.

The positive metal ion transfers one or more electrons to the negative non-metal ion that both end up with full outer shells.

They are attracted by electrostatic attractions.

Question 14

Properties of Ionic bonds

Answer 14

Strong and lots of heat energy needed to break

Question 15

Cations and anions

Answer 15

Lose electrons- cations
Gains electrons- anions

Question 16

What is covalent bonding and what is it called with atoms and then with molecules?

Answer 16

A shared pair of electrons. A molecule is 2 or more atoms covalently bonded together.

Two non metals

Molecular covalent bonding is 2 molecules sharing electrons
Giant covalent lattice bonding is 2 atoms sharing electrons

Question 17

Properties of ionic bonding/ Giant ionic lattice

Answer 17

High melting and boiling point as strong ionic bonds requires a lot of heat energy to break

Conducts electricity when molten as free electrons to move and carry a charge

Soluble in water

Brittle

Question 18

Diatomic molecules are?

Answer 18

When 2 of the same atom are covalently bonded together e.g chlorine

Question 19

Properties of covalent molecules

Answer 19

There are weak forces of attraction - van der waals

Do not conduct electricity as they have no free electrons

Have low solubility in water

Have low melting and boiling points

Question 20

Allotropes are

Answer 20

Different forms of the same element in the same physical state e.g diamond, graphite and graphene

Question 21

Metallic bonding and what is it called

Answer 21

Metallic Lattice

The electrostatic attraction between the positive metal ions and delocalised electrons

Only between metals

Question 22

Diagrams for bonding

Answer 22

Look in book

Question 23

Properties of metallic bonding

Answer 23

High melting and boiling points- strong attraction
Conducts heat and electricity- delocalised electrons
Strong malleable and ductile - layers of metal ions can Slide Over each other

Question 24

Flame test colour for -
lithium
sodium
potassium
calcium
copper

Answer 24

Crimson red
orange
lilac
brick red
green-blue

Question 25

An alloy is?

Answer 25

A mixture of a least two elements one of which is metal

Question 26

To find percentage of gold -

Answer 26

No. Of carats/ 24 x 100

Question 27

Why is an alloy a better material than the metal element in terms of structure?

Answer 27

As an alloy has different sizes of atoms . This makes it difficult for the layers to slide and the alloy to break.

Question 28

What is meant by the term relative atomic mass?

Answer 28

The average atomic mass of an isotope compared to the C-12 isotope

Question 29

What elements have a double covalent bond and which one has a triple covalent bond

Answer 29

Double - Oxygen, Carbon dioxide Triple - Nitrogen

Question 30

What are the allotropes of Carbon?

Answer 30

Diamond, Graphite and Graphene

Question 31

What is the structure of diamond?

Answer 31

Each carbon atom is covalently bonded to four others in a tetrahedral three-dimensional structure

Question 32

What are the properties of diamond?

Answer 32

High melting and boiling points Does not conduct heat or electricity as it has no free ions Hard due to tetrahedral structure

Question 33

What are the uses of diamond?

Answer 33

As a cutting tool for hard rock, metals and glass

Question 34

What is the structure of Graphite

Answer 34

Layer of carbon atoms are arranged in hexagons with weak covalent bonds and forces. Each atoms is bonded to 3 others so one electron is free and it is 3-dimensional

Question 35

What are the properties of graphite

Answer 35

High melting and boiling points Good conducteur of heat and electricity as it has a free atom Soft due to the weak forces between layers

Question 36

What are the uses for graphite

Answer 36

Lubricants for machinery and pencil leads

Question 37

What is the structure of Graphene

Answer 37

A single-atom thick layer of graphite with strong covalent bonds between each carbon atom. The atoms are arranged in hexagons 2-dimensional

Question 38

What are Properties of Graphene

Answer 38

High melting and boiling points Good conductor as one electron is unbonded Very strong as it has strong covalent bonds - 100 times stronger than steel Light

Question 39

What are Uses of Graphene

Answer 39

As a strong light and relatively cheap conductor in solar cells and batteries