1.1 Periodicity

Question 1

Groups

Answer 1

vertical columns within the table contain elements with similar chemical properties resulting from a common number of electrons in the outer shell

Question 2

Periods

Answer 2

Rows of elements arranged with increasing atomic number, demonstrating an increasing number of outer electrons and a move from metallic to non-metallic characteristics

Question 3

Metallic elements

Answer 3

Li, Be, Na, Mg, Al, K, Ca

Question 4

Covalent molecular elements

Answer 4

H2, N2, O2, F2, Cl2, P4, S8 and fullerenes (eg C60)

Question 5

Covalent network elements

Answer 5

B, C (diamond, graphite), Si

Question 6

Monatomic elements

Answer 6

Noble gases

Question 7

Covalent radius

Answer 7

A measure of the size of an atom. The trends in covalent radius across periods and down groups can be explained in terms of the number of occupied shells, and nuclear charge.

Question 8

First ionisation energy

Answer 8

The energy required to remove one mole of electrons from one mole of gaseous atoms. The second and subsequent ionisation energies refer to the energies required to remove further moles of electrons

Question 9

Trends in ionisation energies

Answer 9

Trends in ionisation energies across periods and down groups can be explained in terms of the atomic size, nuclear charge and the screening effect due to inner shell electrons

Question 10

Electronegativity

Answer 10

Atoms of different elements have different attractions for bonding electrons. Electronegativity is a measure of the attraction an atom involved in a bond has for the electrons of the bond

Question 11

Trends in electronegativity

Answer 11

The trends in electronegativity across periods and down can be rationalised in terms of covalent radius, nuclear charge and the screening effect due to inner shell electrons.