Science Chemistry revision

Question 1

What are the 5 structures types?

Answer 1

Ionic
Simple molecular
Metallic
Monoatomic
Giant Covalent

Question 2

True or false, ionic has a giant lattice structure

Answer 2

True

Question 3

Describe simple molecular?

Answer 3

It has a covalent bond, and it is between non metals only and it has low melting and boiling point due to weak intermolecualr forces

Question 4

Describe giant covalent?

Answer 4

It has covalent bonding giant lattice structure and high melting and boiling point

Question 5

Why does ionic have a high melting and boiling point

Answer 5

the reason is because they have strong electrostatic attraction.

Question 6

Describe ionic bonding?

Answer 6

ionic bonding between a metal and a non metal, it has a high melting point and boiling point, it has a giant lattice structure and it has got strong electrostatic attraction

Question 7

Describe metallic bonding?

Answer 7

bonding between metals only, it has a giant lattice structure and it has got a high melting point and boiling point

Question 8

Do non metal ions lose or gain electrons?

Answer 8

they gain electrons

Question 9

What are group 7 elements called?

Answer 9

Halogens

Question 10

What are group 0 elements called?

Answer 10

Noble gases

Question 11

What are group 1 elements called?

Answer 11

Alkaline metals

Question 12

What is the overall charge of non metals and metals when they combine together?

Answer 12

Zero

Question 13

What is electronegativity?

Answer 13

The tendency to attract the bonding pair of electrons

Question 14

What is the equation to calculate the relative formula mass

Answer 14

Mass= Mr x Moles

Question 15

What is Hunds rule

Answer 15

Electrons prefer to occupy orbitals on their own, and only pair when no orbitals of the same energy are available

Question 16

what is attenuation

Answer 16

the loss of a signal

Question 17

what process do the pulses undergo in fibre optics

Answer 17

total internal reflection

Question 18

what does first ionisation mean

Answer 18

energy required to remove one electron from each atom in a moles of gaseous atoms producing one mole of first gaseous ions

Question 19

Which metal is the most reactive metal

Answer 19

Potassium

Question 20

What is oxidation

Answer 20

The loss of electrons

Question 21

What is reduction

Answer 21

The gain of electrons

Question 22

what is a temporary dipole

Answer 22

they are weak intermolecular forces present between non polar covalent forces

Question 23

what term describes the electrical distribution in a molecule

Answer 23

Non symmetrical

Question 24

what happens when the electrons are non symmetrical

Answer 24

there are more electrons at one end of the molecule than the other

Question 25

What happens to the molecule with the temporary dipole and the molecule with the induced dipole

Answer 25

they attract each other and pull the molecules together

Question 26

What are Van der waals forces

Answer 26

They are permanent forces between polar molecules.

Question 27

What does the negative and the positive charge disturb

Answer 27

They disturb the electrons and cause an induced dipole

Question 28

In Van der waals forces, what happens to the polar molecules that have a permanent negative end and a permanent positive end

Answer 28

They attract each other

Question 29

What is the strongest type of intermolecular force

Answer 29

Hydrogen bonding

Question 30

Which three atoms does hydrogen form a compound with

Answer 30

nitrogen, oxygen and fluorine

Question 31

what is the reason for this

Answer 31

becuase of large differences in eletronegativity

Question 32

What is the trend with electronegativity across the period?

Answer 32

great number of protons
same amount of shielding
more attraction between nucleus and bonding pair of electrons

Question 33

what is the trend with electronegativity down the group?

Answer 33

number of inner electrons increase
atoms get larger
great amount of shielding
weaker attractions between nucleus and boding pair of electrons

Question 34

What is the trend with ionisation energy across the period?

Answer 34

great number of protons
same amount of shielding
more attractions between nucleus and outermost electrons
more energy needed to remove the outermost electron

Question 35

What is the trend with ionisation energy down the group?

Answer 35

atoms get larger
number of inner electrons increase
great amount of shielding
less energy needed to remove the outermost electron

Question 36

What is the trend with the atomic radius across the period?

Answer 36

It decreases because:
great number of protons
same amount of shielding
more attractions between the nucleus and the outermost electron

Question 37

What is the trend with the atomic radius down the group?

Answer 37

It increases because:
atoms get larger
number of inner electrons increase
great amount of shielding
weaker attractions from the nucleus and outer shell electrons

Question 38

What is the trend with the ionic radius across the period

Answer 38

It gets smaller because
the number of protons increase and the electrons stays the same

Question 39

why is the ionic radius larger across the group?

Answer 39

number of electrons increase and the are the same number of protons

Question 40

What is the reactivity series down group 1?

Answer 40

the reactivity series increases down the group because:
the distance from the nucleus to the outer electron gets bigger
This means the electrostatic attraction decreases between the nucleus and the outer electron.

Question 41

What is the reactivity series down group 7?

Answer 41

It increases as you go down the group because:
the distance from the nucleus and the outermost electron gets bigger.
This means the electrostatic attraction decreases between the nucleus and the outermost electron