IQR 3

Question 1

Atomic radius: Left to right across a period

Answer 1

Moving left to right across a period the atomic radius decreases: The number of protons increase, causing a stronger pull in the outer electron towards the nucleus resulting in a smaller radius.

Question 2

Atomic radius: Moving down a group

Answer 2

The atomic radius increases. More shells create screening effect as the increased shells block force of attraction towards nucleus resulting in larger radius.

Question 3

Ionisation energy definition

Answer 3

Amount of energy required to remove the most loosely bound electron from an atom or ion in the gaseous state.

Question 4

Ionisation energy: Moving from left to right

Answer 4

Ionisation energy increases: With a smaller atomic radius (Number of shells remain but increased number of protons). Causes stronger force of attraction, hence more energy is required to remove the valence electron.

Question 5

Moving down a group

Answer 5

Ionisation energy decreases: Although number of protons increases the number of shells also increases. Therefore, less energy is required to remove it.

Question 6

Factors affecting the magnitude of ionisation energy:

Answer 6

Nuclear charge: The higher the charge the higher the energy
Shielding effect: more shells= less energy.
Radius: More distance between nucleus and outer electrons= reduced ionisation energy.
Sublevel: Electron from full or half sublevels requires more energy.

Question 7

Relationship between atomic radius and ionisation energy

Answer 7

Inversely proportional

Question 8

MP/BP: going down groups 1,2,13, 14

Answer 8

Decreases: As atoms get bigger the nuclei get further away from the outside electron. The attraction falls and the metallic bonds weakens. hence, atoms are more easily pulled apart.

Question 9

MP/BP going down groups: 15, 16, 17, 18

Answer 9

Attraction between molecules called van der waals dispersion forces. As molecules get bigger dispersion forces gets bigger so there melting and boiling forces rise.

Question 10

Two elements liquid at room temperature

Answer 10

Mercury and Bromine

Question 11

Electronegativity: Left to right

Answer 11

Increases: Atomic radius decreases, ability of nucleus to attract increases.

Question 12

Electronegativity: Top to bottom

Answer 12

Decreases: More shells causes the shield effect. Which means it can’t pull electrons as well

Question 13

Electronegativity and ionisation energy relationship

Answer 13

Directly proportional

Question 14

Metallic character: Left to right

Answer 14

Decreases: As there is decreasing atomic radius, the valence electron become more closely bound to the nucleus resulting in decreasing electrical and thermal conductivities.

Question 15

Metallic character: Top to bottom

Answer 15

Metallic character increases. As atomic radius increases the valence electron become more loosely bound and thus more electrical and thermal conductivity.

Question 16

Reactivity with water

Answer 16

metals may react with water to produce hydrogen gas and metal

Question 17

Reactivity with water trend group 1

Answer 17

Atomic radius increases and number of shells, meaning less ionisaton energy. The electron is more easily able to be get rid of and thus reactivity increases.

Question 18

Reactivity with water group 2

Answer 18

Group 2 elements react at varying temperatures, in comparison to group 1 the atomic radius is less so reactivity decreases.

Question 19

Reactivity in general from left to right

Answer 19

Reactive metal (Incomplete valence shell to unreactive noble gas (Full valence shell

Question 20

Reactivity in general down groups 1 and 2

Answer 20

Electronegativity energy decreases and radius incerases so high reactivity as going down.

Question 21

Reactivity in general going down groups 5

Answer 21

15-17
Non metals. More attarctive and lower radius poorer tendency to gain electrons.

Question 22

Periodicity

Answer 22

Regular recurrence of events or properties