2.1.1 & 2.1.2: Periodicity and the periodic table

Question 1

Elements

Answer 1

Arranged in order of proton number

Question 2

Groups

Answer 2

Columns
Often have very similar properties and and have their e-s in similar orbitals
group n = n valence e-s

Question 3

Periods

Answer 3

Row

Elements in the same period have the same number of electron shells

Question 4

Blocks

Answer 4

S,P,D,F

valence electrons in n orbital in n block

Question 5

Name of F block

Answer 5

Lathanides and Actinides

Question 6

Atomic radius

period trend and why

Answer 6

decreases along a period

(as) proton number increases and extra electrons are added to the same shell
(so) the electrons have more attraction to the nucleus - held closer

Question 7

Atomic radius

group trend and why

Answer 7

increases down a group
(as) no. of electrons increases down a group, outweighs the effect of the proton no.
each electron shell is further from further from the nucleus

Question 8

Ionisation energy

period trend and why

Answer 8

increases along a period
as electrostatic attraction increases of each electron to nucleus and the proton number increases
more energy is needed to remove an electron

Question 9

Ionisation energy

group trend and why

Answer 9

Decreases down a group
(as) the outer electrons are further from the nucleus
the electrostatic attraction of the outer electrons decreases down the group

Question 10

Melting point

period trend and why

Answer 10

along a period:
metals - giant cov - molecular solids
increase - sharp peak - decrease

Question 11

Melting point

Covalent structures

Answer 11

giant covalent = relatively high mps.

molecular solids = low mps.

Question 12

Melting point

Metals

Answer 12

the more valence electrons = the higher mp.