Unit 1-periodicity

Question 1

what does the position of elements allow?

Answer 1

The position of elements on the Periodic Table allow us to make predications of their physical properties and chemical behaviour.

Question 2

What is the same going down a group?

Answer 2

Going down a group in the periodic table the elements contain the same number of outer electrons but an extra outer shell each time.

Question 3

What is the trend along a period?

Answer 3

Going along a period elements move from metallic to non-metallic and add an outer electron each time.

Question 4

What structure/bonding occurs in Lithium

Answer 4

Metallic lattice

Question 5

What are the names of all the metallic lattices?

Answer 5

Lithium, Beryllium, Sodium, Magnesium, aluminium, potassium and calcium

Question 6

What bonding/ structure occurs in Boron, Carbon (diamond and graphite) and silicon

Answer 6

Covalent network

Question 7

What Bonding occurs in Noble gases?

Answer 7

Monatomic

Question 8

What elements are covalent molecular

Answer 8

Hydrogen, Nitrogen, Oxygen, Fluorine, chlorine, Phosphorus, sulphur, and fullerenes (eg C60)

Question 9

What is the covalent Radius?

Answer 9

The covalent radius is a measure of the size of an atom.

Question 10

What happens to the covalent radius across a period?

Answer 10

Across a period, the covalent radius decreases as the nuclear charge increases (higher nuclear charge pulls the outer electrons in closer).

Question 11

What happens to a covalent radius going down a group?

Answer 11

Going down a group the covalent radius increases as the number of occupied shells increase (more shells = bigger atom).

Question 12

What is the definition of the first ionisation energy?

Answer 12

First ionisation energy is the energy required to remove one mole of electrons from one mole of gaseous atoms.

Question 13

What is the definition of the second ionisation energy?

Answer 13

Second ionisation energy is the energy required to remove the 2nd mole of electrons.

Question 14

What is the trend of the ionisation energy a long a period?

Answer 14

Across a period, the ionisation energy tends to increase as the nuclear charge increases.

Question 15

What is the trend of the ionisation energy down a group?

Answer 15

Down a group the ionisation energy decreases as there are more shells, which means there is an increased screening effect due to the inner electrons (making it easier to remove the outer ones).

Question 16

What does the term electronegativity mean?

Answer 16

Electronegativity is a measure of the attraction which an atom (involved in a bond) has for the electrons in the bond.

Question 17

Trends in electronegativity along a period?

Answer 17

Across a period the electronegativity values increase due to the nuclear charge increasing (higher positive nuclear charge will mean the negative electrons will be more attracted).

Question 18

Trends of electronegativity down a group?

Answer 18

Going down a group the electronegativity decreases, this is due to the screening effect (of the inner shell electrons) – they will ‘shield’ the nuclear charge.