Chapter 7

Question 1

first ionisation energy

Answer 1

the energy required to move one electron from each atom in one mole of gaseous atoms of an element

Question 2

unit for first ionisation energy

Answer 2

kJmol-1

Question 3

general equation for first ionisation energy

Answer 3

X(g) -> X+(g)+e-

Question 4

first ionisation energy trends-group

Answer 4

-decreases down a group because the atomic radius increases= more inner shells= more shielding= attraction decreases

Question 5

first ionisation energy- periods

Answer 5

increase across a period= nuclear charge increases= shielding is the same= atom radius decreases= attraction increases

Question 6

why are there falls in graph of ionisation energy

Answer 6

sub shells- their energies and how orbitals fill with electrons

Question 7

reasons for fall between Be and B

Answer 7

Be=2s, B=2p
2p has higher energy= easier to remove= ionisation energy is less

Question 8

reasons for fall between N and O

Answer 8

N=2p3, O=2p4
easier to remove electron pair from O= ionisation energy is lower

Question 9

atomic radius on IE

Answer 9

greater distance between nucleus and outer shell electrons= weaker nuclear attraction= lower IE

Question 10

increased nuclear charge on IE

Answer 10

more protons in the nucleus= greater attraction between nucleus and outer shell electrons= increased

Question 11

inner shell shielding on IE

Answer 11

inner shell repels outer shell, this repulsion reduces attraction between the nucleus and outer shell resulting in a lower IE

Question 12

in successive ionisation energies

Answer 12

an elements ionisation energies= number of electrons
no of ionisation energies= charge on ion produced

Question 13

metals and non metals on period table

Answer 13

divide starts at the top of group 3 and finishes at the bottom of group 7
left=metals. right=non metals

Question 14

what are the elements immediately adjacent to the divide called

Answer 14

metalloids/semi-metals

Question 15

metallic bonding

Answer 15

strong electrostatic attraction between metal cations held in fixed positions and delocalised electrons which are free to move through the whole structure

Question 16

metal properties- electrical conductivity

Answer 16

all are electrically conductive
delocalised electrons move and carry a charge with them

Question 17

metal properties- high melting and boiling points

Answer 17

most besides mercury have high mp and bp, depends on strength of bonds- metal bonds need large energy to break

Question 18

metal properties- solubility

Answer 18

all are insoluble

Question 19

giant covalent structures

Answer 19

atoms are held together by a network of strong covalent bonds to form a lattice

Question 20

diamond structure

Answer 20

tetrahedral structure
uses 4 outershell electrons to form covalent bonds to other carbon

Question 21

diamond features

Answer 21

very high mp and bp, insoluble, electrically nonconductive

Question 22

graphite structure

Answer 22

planar hexagonal layers held by london forces
uses 3/4 outershell electrons to form covalent bonds to others, remaining is released into pool of delocalised electrons

Question 23

graphite feature

Answer 23

very high mp and bp, insoluble, electrically conductive

Question 24

graphene

Answer 24

single graphite layer, same conductivity as copper, thinnest and strongest metal ever made

Question 25

metallic melting point trends

Answer 25

increases from group 1-4 sharp decrease between 4-5( goes from giant to simple molecular comparatively low from 5-8