Inorganic: periodicity

Question 1

Which groups are contained in S, D, P and F block

Answer 1

S-1,2
D-transition metals
P-3-8
F-bottom groups

Question 2

how is the periodic table separated into groups, explain why they are seperated

Answer 2

s d p f blocks
each element in each block will contain electrons only up to that shell , determined by proton number
s- electrons only fill s outer shell
p- electrons will fill at least one p electron in outer shell
d- will have at least one electron in d outer shell, no f or p fill in shell
f- electron will fill at least one f outer shell, no d or p electrons

Question 3

explain the properties of elements in same shell

Answer 3

Elements in the same group show similar properties, and properties change gradually as you go across a period

Question 4

explain the reactivity of s group metals

Answer 4

elements become more reactive going down the group

Question 5

what is atomic radius

Answer 5

atomic radius is the distance between the nucleus and the outermost electron of an atom

Question 6

explain atomic radius across the period

Answer 6

across will decrease, due to proton number increasing/ nuclear charge meaning number of electrons also increases by one each element, so greater attraction from the nucleus to the outermost electron pulling closer together, shielding will stay the same

Question 7

explain the properties of the elements in period 3

Answer 7

Na, Mg, Al, Si, P, S, Cl, Ar = period 3
group 1,2,3 metals have giant structures, they lose outer e- to form ionic compound
group 4 Si is non metal, forming 4 covalent bond, a macromolecular (giant covalent) with high m/bp
group 5,6,7 are molecular structures P4, S8, Cl2 non metals either accept e- to form ionic or share outer to form covalent compounds
group 8 Ar is full outer shell so unreactive

Question 8

explain the m/bp trend in period 3

Answer 8

Na, Mg, Al, Si, P, S, Cl, Ar
giant structures to have a high m/bp
molecular structures have low m/bp
NA-Al, mp increases due to stronger metalic bonds and higher ionic charge/ number of valence e- so more delocalised e- holding giant metalic lattice (na+1,, Mg+2, Al+3) so Al has stronger electrostatic force between delocalised e- and +v ion
Si has giant covalent structure with highest m/bp
P-Ar, mp decreases though covalent bonds within the molecules are strong, between the molecules are weak instantaneous dipole-induced dipole/ VdW forces, less energy required to break forces
(melting point of S is higher than that of P as sulphur exists as larger S8 molecules compared to the smaller P4 molecule)

Question 9

explain trend of atomic radii down a group

Answer 9

it decreases down a group since there is an increase in proton/ nuclear charge number so more e- , the nucleus will have a stronger attraction to outermost e- so stronger pull decreasing the atomic radii

Question 10

definition of first ionisation energy and its equation

Answer 10

The first ionisation energy (IE1) is the energy required to remove one mole of electrons from one mole of atoms of an element in the gaseous state to form one mole of gaseous ions
Na (g) → Na+ (g) + e-

Question 11

explain trend in first ionisation energy in p3

Answer 11

There is a general increase in IE1 across a period
-The nuclear charge increases
-The atomic radius decreases
There are stronger attractive forces between the nucleus and outer electrons
It therefore gets harder to remove any electrons

Question 12

what are the outliers of this trend, explain why

Answer 12

Mg - Al and P - S
al fills 3p orbital which has higher energy level so it is easily removed and further from nucleus so less attraction
S fills 3p orbitals but 11 repels e- theory so easier to lose
less energy required