Atomic Structure And Bonding

Question 1

Element

Answer 1

Made up of only one type of atom

Question 2

Compound

Answer 2

Contains more than one type of atom held together by bonds

Question 3

Proton

Answer 3

+1
1
Nucleus

Question 4

Neutron

Answer 4

0
1
Nucleus

Question 5

Electron

Answer 5

-1
1/1836
Shells

Question 6

Mass number

Answer 6

Protons and neutrons

Question 7

Atomic number

Answer 7

Protons

Question 8

Isotope

Answer 8

Atoms of the same element which have the same atomic number but a different mass number

Question 9

Relative atomic mass

Answer 9

The average mass of an atom of an element compared to 1/12 of the mass of a carbon -12 atom

Question 10

Ar

Answer 10

(Mass of atom 1 x%) + (mass of atom 2 x%)
Divided by
Total number of atoms

Question 11

Noble gases

Answer 11

They are unreactive because they have full outer shells

Question 12

Ionic bonding

Answer 12

Metal and non metal react
Metals form positive ions
Non metals form negative ions
Opposite charged ions are electrostatically attracted to each other
Giant lattice is formed

Question 13

Covalent bonding

Answer 13

Atoms share a pair of electrons and the shared electrons are attracted to both nuclei

Question 14

When can ionic compounds conduct electricity

Answer 14

Cannot conduct electricity when solid because ions are fixed
Can conduct electricity when in aqueous or molten solution because ions are free to move and carry charge

Question 15

Why do ionic compounds have high melting and boiling points

Answer 15

They have strong electrostatic attraction between the ions and a lot of energy is required to break them apart

Question 16

Why do simple covalent molecules have low melting and boiling points

Answer 16

They have weak intermolecular forces and not a lot of energy is needed to overcome these forces

Question 17

Why do simple covalent molecules not conduct electricity

Answer 17

They have no charged particles free to move

Question 18

Diamond

Answer 18

Giant covalent structure
Each carbon atom is bonded to 4 other carbon atoms
Tetrahedral shape

Question 19

Why does diamond have a high melting and boiling point

Answer 19

It has many strong covalent bonds and a lot of energy is required to break these bonds

Question 20

Why does diamond not conduct electricity

Answer 20

It has no free charged particles

Question 21

Why is diamond very hard

Answer 21

It is a giant covalent lattice

Question 22

What is diamond used for

Answer 22

Cutting tools
Jewellery

Question 23

Graphite

Answer 23

Giant covalent structure
Each carbon atom is bonded to 3 other carbon atoms
Layers of hexagon

Question 24

Why does graphite have a high melting and boiling point

Answer 24

It has many strong covalent bonds and lots of energy is needed to break these bonds

Question 25

Why does graphite conduct electricity

Answer 25

The free delocalised electrons are free to move

Question 26

Why is graphite quite soft

Answer 26

There are weak forces of attraction between layers of carbon atoms

Question 27

What is graphite used for

Answer 27

Lubricant Pencil The free electrons allow the layers to slide over each other

Question 28

C60 Fullerene

Answer 28

Simple molecule Each carbon atoms is bonded to 3 other carbon atoms Spherical molecule with 60 carbons

Question 29

Why does C60 Fullerene have a low melting and boiling point

Answer 29

There are weak intermolecular forces so it does need much energy to break these forces

Question 30

Why does C60 Fullerene not conduct electricity

Answer 30

The delocalised electrons have to stay within the molecule and cannot move from one molecule to the other

Question 31

Metal definition

Answer 31

Strong electrostatic attraction between positive metal ions and a sea of delocalised electrons Giant metallic lattice

Question 32

Why do metals have a very high melting and boiling point

Answer 32

It is a giant lattice with strong electrostatic attraction between the positive metal ions and sea of delocalised electrons and a lot of energy is needed to break bonds and overcome forces

Question 33

Why are metals malleable

Answer 33

The delocalised electrons allow the layers of metal ions to slide over each other

Question 34

Alloy

Answer 34

Mixture or atleast 2 elements where one of these is a metal