Trends

Question 1

Atomic radius of an atom

Answer 1

Half the distance between the nuclei of 2 atoms of the same element that are joined together by a single covalent bond

Question 2

First ionisation energy

Answer 2

Minimum energy required to completely remove the most loosely bound e from a neutral atom in its ground state
Eg NA(g) ->NA+(g) + e

Question 3

Second ionisation energy

Answer 3

Energy required to completely remove an electron from an ion with 1 positive charge in the gaseous state
Eg Ca+ -> Ca+2 (g) + e

Question 4

Exceptions of first ionisation energy

Answer 4

Any sub level that is completely or half filled has extra stability therefore it is harder to remove the electrons leading to a higher ionisation energy

Question 5

Explain why x has a higher ionisation energy than y

Answer 5

Write e configuration of both
Compare e configuration
sublevels that are half filled or full have more stability

Question 6

Why is second ionisation energy always bigger than the first

Answer 6

The e is removed from a positively charged ion
There is a greater attraction between the nucleus and the e being removed
thus more energy is require to move the e-

Question 7

How does atomic radius differ down a group

Answer 7

Increases

Question 8

Why does atomic radius increase down a group

Answer 8

Electrons are going into a new energy level
Increased shielding effect by inner e

Question 9

How does atomic radius differ across a period

Answer 9

Decreases

Question 10

Why does atomic radius decrease across a period

Answer 10

Increase in effective nuclear charge
No increase in shielding

Question 11

How does first ionisation energy differ down a group

Answer 11

Decreases

Question 12

Why does first ionisation energy decrease down a group

Answer 12

Increasing atomic radius
Increased shielding by inner electrons

Question 13

How does first ionisation energy differ across a period

Answer 13

Increases

Question 14

Why does first ionisation energy increase across a period

Answer 14

Increasing effective nuclear charge
Decreasing atomic radius

Question 15

How does electronegativity differ down a group

Answer 15

Decreases

Question 16

Why does electronegativity decrease down a group

Answer 16

Increasing atomic radius
Increased shielding by inner electrons

Question 17

Why does electronegativity increase across a period

Answer 17

Increasing effective nuclear charge
Decreasing atomic radius

Question 18

How does electronegativity differ across a period

Answer 18

Increases

Question 19

why does x have an exceptionally high first ionisation energy?

Answer 19

write e- configuration

sublevels that are half full or full have extra stability
this makes it much harder to remove the most loosely bound e- and it requires much more energy

Question 20

how do group 1 elements react?

Answer 20

by donating 1 e-

Question 21

how do group 2 elements react

Answer 21

by donating 2 e-

Question 22

how does reactivity differ down group 1 and 2

Answer 22

it increases

Question 23

is it easier to remove e- when an element is more or less reactive

Answer 23

more

Question 24

why does reactivity increase down group 1 of the periodic table

Answer 24

increasing atomic radius
increased shielding by inner e-

Question 25

what is produced when a group 1 reacts with O2

Answer 25

a metal oxide

Question 26

write the balanced equation of a metal oxide reaction in group 1

Answer 26

2(metal) + 1/2 O2 ------->metal2O

Question 27

write the balanced equation of a metal hydroxide reaction in group 1

Answer 27

metal + H20 ---->(metal)OH + 1/2 H2

Question 28

why are group 1 metals stored in oil

Answer 28

to prevent the metals from reacting with oxygen in the air

Question 29

what is formed when a group 1 reacts with water

Answer 29

metal hydroxides

Question 30

how do group ones react with water

Answer 30

vigorously/ violently the metal floats on the surface of water lots of fizzing is observed as H2 gas is produced as the reactivity increases down the group, potassium is so reactive the hydrogen gas actually ignites and a lilac flame is observed

Question 31

what is formed when group one metals react with HCL

Answer 31

metal chloride salt and h gas

Question 32

write the balanced equation of a HCL reaction with group 1

Answer 32

metal + HCl --> metalCl + 1/2 H2

Question 33

how does a group 1 react with HCl

Answer 33

explosively

Question 34

which group are the most electronegative on the periodic table

Answer 34

halogens (group 7/17)

Question 35

how do group 7 react

Answer 35

by accepting 1 e- to have a stable outer octet

Question 36

what happens to reactivity down group 7

Answer 36

decreases

Question 37

why does reactivity decrease down group 7

Answer 37

decreasing electronegativity increasing atomic radius

Question 38

what is used to show that reactivity decreases down group 7

Answer 38

displacement reactions

Question 39

what does displacement mean

Answer 39

element is replaced with a more reactive element

Question 40

what is the only element in group 7 that will displace everything in the group and why

Answer 40

flourine has the highest electronegativity value

Question 41

describe the experiment carried out to show that reactivity decreases down group 7

Answer 41

bubble chlorine gas through a solution that contains bromide ions. (BrCl) the Cl is more reactive and takes 1e- from the Br- ion forming a Br atom 2 Br atoms join to form Br2 this is visualised from a colour change of colourless to red

Question 42

what is the colour change shown in the experiment carried out to show that reactivity decreases down group 7

Answer 42

colourless to red

Question 43

does boiling point increase or decrease down group 7?

Answer 43

increases

Question 44

why does does boiling point increase down group 7

Answer 44

as you go down the electron cloud gets larger thus the van der waals interactions between halogen molecules get stronger and more energy is needed to overcome the force of attraction

Question 45

what is the appearance of flourine at room temp

Answer 45

pale yellow gas

Question 46

what is the appearance of chlorine at room temp

Answer 46

greenish-yellow gas

Question 47

what is the appearance of bromine at room temp

Answer 47

red-brown liquid

Question 48

what is the appearance of iodine at room temp

Answer 48

grey solid

Question 49

what is the balanced equation of the displacement reaction that is carried out to show that reactivity decreases down group 7

Answer 49

Cl2 + 2NaBr --> 2NaCl + Br2

Question 50

what is the balanced equation that shows the colour change of the displacement reaction that is carried out to show that reactivity decreases down group 7

Answer 50

Cl2 + 2e- --> 2Cl- 2Br- ----> Br2 + 2e-