B2 - redox and periodicity

Question 1

Why does the first ionisation energy increase along a period

Answer 1

Atomic radius decreases
Nuclear charge increases
Nuclear attraction increases
Harder to remove the furthest electron

Question 2

What is the 1st ionisation energy

Answer 2

Energy neeed to remove 1 mole of electrons from 1 mole of gaseous atoms

Question 3

Why does first ionisation energy decrease down a group

Answer 3

Atom radius increases
Shielding increases
Nuclear attraction decreases
Easier to remove electrons

Question 4

Why does ionisation energy decrease between Mg and Al

Answer 4

Al outer shell electron is in a P subshell rather then Mg in an S subshell. This means less energy is needed to remove it

Question 5

Why does ionisation energy decrease between P and S

Answer 5

In sulfur one of the electron orbitals have paired electrons compared to phosphorus which doesn’t have any paired electrons. The paired electrons in sulfur repel which makes it easier to lose an electron

Question 6

Why does melting point between Na and Mg increase

Answer 6

Nuclear charge increases
Number of delocalised electrons increase
Strength of metallic bonds increase

Question 7

What is the order of increasing melting point between P,S,Cl,Ar

Answer 7

S8,P4,Cl2,Ar