3.1.1

Question 1

What is periodicity?

Answer 1

regular repeating pattern
in the properties of elements

Question 2

What is ionisation energy?

Answer 2

energy needed to remove 1 mole of electrons from a mole of gaseous atoms

Question 3

What is the trend? As ionisation energy inc,

Answer 3

nuclear attraction inc

Question 4

What is the general trend of I.E across period 2?

Answer 4

inc in 1st I.E

Question 5

What happens to nuclear charge as we go across a period?

Answer 5

increases

Question 6

What happens to sheilding as we go across a period

Answer 6

stays constant
stays same

Question 7

What happens to atomic radius as we go across a period

Answer 7

decreases as nucleus pulls electrons in more

Question 8

When does the trend of ionisation across a period go against the trend?

Answer 8

Boron and Oxygen

Question 9

Why does Boron go against the trend?

Answer 9

2p subshell is higher than 2s

so it requires less energy to remove electron from 2p

Question 10

What makes the trend return to increasing after Boron across a period?

Answer 10

Carbon
inc nuclear charge
smaller atomic radius

Question 11

Why does oxygen not follow the trend?

Answer 11

has the first paired electrons in the orbital so the electron experiences repulsion

so it is easier to remove the electron

so IE decreases

Question 12

What causes the trend to pick up again after oxygen?

Answer 12

extra proton in nucleus
dec atomic radius

Question 13

What is the trend across period 3?

Answer 13

inc in IE

Question 14

What elements dont go with the general trend in period 3?

Answer 14

Aluminium and Sulfur

Question 15

Why doesnt Aluminium not go with the general trend?

Answer 15

3p is higher in energy than 3s

so less energy is required to remove the outer electron

so slight dip in energy

Question 16

Why does sulfur not o with the period 3 trend in IE?

Answer 16

1st paired electron in the orbital

so there is repulsion

so makes it easier to remove the outer electron

Question 17

What is the general increase in ionisation energy of a period due to?

Answer 17

inc nuclear charge
constant sheilding
dec in atomic radius
stronger attraction between nucleus and outer electron

Question 18

What 2 groups have dips in ionisation energy>

Answer 18

3 and 6

Question 19

What are the metals in period 3?

Answer 19

Na
Mg
Al

Question 20

What is the giant covalent structure in period 3?

Answer 20

Silicon

Question 21

What are the simple covalent structures?

Answer 21

P, S, Cl, Ar

Question 22

Why does mp inc like Na<Mg<Al?

Answer 22

charge increases so stronger metallic bond
higher charge reduces radius
inc attraction between positive metal ions and delocalised electrons

Question 24

Why does Silicon have such a high melting point?

Answer 24

lots of energy needed to break the many covalent bonds between atoms

Question 25

Why is the melting points for simple molecular low?

Answer 25

weak intermolecular forces of attraction require very little energy to be overcome

Question 26

Why do metals have a high melting point?

Answer 26

strong forces of attraction between positive metal ions and delocalised electrons

Question 27

Why does S8 have a higher melting point than the other simple molecular?

Answer 27

most electrons so more / stronger london forces require lots of energy to be overcome

Question 28

What is first ionisation energy?

Answer 28

energy needed to remove 1 electron from each atom in a mole of gaseous atoms to form one mole of gaseous 1+ ions

Question 29

Why does first ionisation energy decrease down the group?

Answer 29

despite elements having more protons as you go down groups so inc nuclear charge atomic radius gets larger more sheilding so weaker attraction

Question 30

How do you test for sulphate?

Answer 30

Add barium chloride white ppt

Question 31

How do you test for carbonates?

Answer 31

add acid observe fizzing bubble gas through lime water limewater goes cloudy

Question 32

How do you test for the ammonium ion?

Answer 32

add OH- to sample heat to produce NH3 hold damp red litmus paper in mouth of the test tube litmus paper goes blue

Question 33

What is the result when silver chloride is added to dilute aqeous ammonia?

Answer 33

soluble

Question 34

What is the result when silver bromide is added to dilute aqeous ammonia?

Answer 34

soluble1

Question 35

What is the result when silver bromide is added to aqueous dilute ammonia?

Answer 35

sparingly soluble

Question 36

What is the result when silver iodide is added to dilute aqeuous ammonia?

Answer 36

insoluble

Question 37

What happens when Cl2 and iodide ions react?

Answer 37

chlorine displaces iodine

Question 38

What happens when bromine is added to iodide ions?

Answer 38

Bromine displaces iodine by reduction

Question 39

What happens when iodine is added to chloride ions?

Answer 39

no reaction

Question 40

What is an oxidising agent?

Answer 40

electron pair acceptor

Question 41

What group describes halogens?

Answer 41

simple covalent structures

Question 42

where are the halogens?

Answer 42

p5

Question 43

Why do halogens have low boiling pointsd?

Answer 43

weak intermolecular forces require very little energy to be overcome

Question 45

What does chlorine do to water?

Answer 45

kill bacteriaq

Question 46

What is chlorine suspected of doing?

Answer 46

reacting with organic compounds to form halogenated organic molecules Carcinogenic

Question 47

What products do group 2 oxides and hydroxides form when reacted with acid?

Answer 47

Salt and water

Question 48

What is an obsv of group 2 oxides and hydroxides reqacting with acid?

Answer 48

solid dissolvs

Question 49

What happens when oxides react with water?

Answer 49

hydroxides form

Question 50

What happens when hydroxides react with water?

Answer 50

dissociates into ions

Question 51

What is the trend of solubility down group 2?

Answer 51

more soluble down group 2 solutions become more alkaline as there are higher concentrations of OH-

Question 52

What happens when group 2 carbonates react with acid?

Answer 52

salt water CO2

Question 53

What are the observations of group 2 carbonates reacting with acids?

Answer 53

solid dissolved effervesence

Question 54

What is the trend of thermal decomposition as you go down the group?

Answer 54

more difficult to decompose due to inc ionic chara cter

Question 55

What are the uses of group 2 oxides and hydroxides?

Answer 55

neutralising acids / alkalis

Question 56

What agents are group 2 metals?

Answer 56

reducing

Question 57

What are reducing agents?

Answer 57

electron donor

Question 58

What happens whena group 2 metal reacts with water?

Answer 58

hydrogen gas salt formed

Question 59

What happens when group 2 metals react with oxygen?

Answer 59

salt formed

Question 60

What is the trend in reactivity down the group?

Answer 60

more reactivity down group

Question 61

Why does reactivity increase down the group?

Answer 61

increasing atomic radius increasing sheilding dec in attraction between nucleus and outer electrons outer electrons lost more readily

Question 62

What is an orbital?

Answer 62

region of space where 2 electrons of opposite spins are found

Question 63

What is meant by 1 mole of substance?

Answer 63

amount of susbtance that contains the same number of particles as there are carbon atoms in 12g of carbon-12

Question 64

Why is there a dec in 1st IE between Ne and Na?

Answer 64

Na has extra shell so more sheilding so weaker nuclear attraction