2. bonding and structure (as)

Question 1

ionic bonding

Answer 1

strong electrostatic attraction between oppositely charged ions

Question 2

ionic bonding involves

Answer 2

the transfer of electrons from a metallic element to a non metallic element

Question 3

ionic solids structure

Answer 3

ions in a lattice are arranged in a regular repeating pattern

Question 4

ionic radius def

Answer 4

measure of the size of an ion

Question 5

ionic radii increases with
ionic radii decreases with

Answer 5

increasing negative charge
increasing positive charge

Question 6

negative ions formed by

Answer 6

atoms gaining electrons

Question 7

isoelectronic ions

Answer 7

ions that have the same electronic configuration

Question 8

the type of lattice formed depends on

Answer 8

the sizes of positive and negative ions which are arranged in alternating fashion

Question 9

why are most ionic compounds are solids at room temp

Answer 9

there isn’t enough energy to overcome the strong electrostatic forces of attraction between oppositely charged ions that make up the lattice

Question 10

ionic compounds require to melt

Answer 10

high temperatures required to make an ionic compound melt or boil

Question 11

electrical conductivity of ionic compounds

Answer 11

in solid they cannot conduct electricity

but molten or aqueous ions they have ions that can move and carry charge

Question 12

things that affect the strength of an ionic bond

Answer 12

ionic charge
ionic radii increases

Question 13

ionic charges affects ionic bond how

Answer 13

greater charge of ion stronger the ionic bond ,, higher mp/bp

Question 14

ionic radii explain how it affects ionic bond

Answer 14

smaller ions can be packed closer together than larger ions electrostatic attraction gets weaker with distance ,, small, closely packed ions have stronger ionic bonding

Question 15

what happens to ionic radii down a group

Answer 15

ionic radii increases

Question 16

what happens when isoelectronic ions ionic radii as atomic number increases

Answer 16

ionic radii decreases

Question 17

physical properties of ionic compounds

Answer 17

• high mps-
• soluble in water but not in non polar solvents
• don’t conduct electricity when solid
• brittle

Question 18

migration of ions evidence for charged particles

Answer 18

• copper (II) chromate (VI) solution is green on a piece of filter paper
• cathode- filter paper is blue because copper ions- pos ions
• anode- filter paper is yellow because of chromate ions- neg ions

Question 19

covalent bonds

Answer 19

strong electrostatic attraction between two positive nuclei and the shared electrons in the bond

Question 20

bond length

Answer 20

distance between the attractive and repulsive forces that balance each other between two nuclei

Question 21

relation between bond enthalpy and bond length

Answer 21

the greater the bond enthalpy the shorter the bond

Question 22

dative covalent bonding

Answer 22

one atom donates both electrons to a bond

Question 23

structure of diamond and silicon (IV) dioxide

Answer 23

each carbon atom bonded to 4 other and silicon is similar but has oxygen atoms between silicon

Question 24

properties of giant structure w covalent bonds

Answer 24

high mp
hard
good thermal conductors
insoluble-
can’t conduct electricity-

Question 25

why can graphite conduct electricity

Answer 25

3 carbon atoms covalently bonded ,, one free electron ,, carry charge

Question 26

graphene structure

Answer 26

- sheet of graphite - joined together hexagonal - one atom thick - two dimensional - conducts electricity - strong - transparent - light

Question 27

metallic bonding

Answer 27

positive metal ions electrostatically attracted to the delocalised negative electrons forming a lattice of closely packed ions in a sea of delocalised electrons

Question 28

metals structure

Answer 28

- high melting point - malleable/ ductile - good thermal conductors- - good electrical conductors- - insoluble

Question 29

what affects metallic bond

Answer 29

- number of electrons - size of metal ions - charge of metal ions

Question 30

electronegativity def

Answer 30

the ability of an atom to attract the bonding electrons in a covalent bond

Question 31

most electronegative element

Answer 31

fluorine

Question 32

do ionic compounds have high mp? and why

Answer 32

strong attraction between ions

Question 33

are ionic compounds soluble and why

Answer 33

soluble in water but not non polar solvents-tells you that particles are charges ions pulled apart by polar molecules like water

Question 34

do ionic compounds conduct electricity

Answer 34

- don’t conduct electricity when solid- ions not free to move

Question 35

are ionic compounds brittle and why

Answer 35

yes they are brittle bcs if layers pulled same charged ions could be above each other ,, repulsion would be strong

Question 36

does giant structure w covalent bond have high mp + explain

Answer 36

require a lot of energy to break bonds

Question 37

giant structure w covalent bond hard+ explain

Answer 37

strong bonds through lattice

Question 38

is giant structure w covalent bond good thermal conductors + explain

Answer 38

vibrations travel easily through lattice

Question 39

are giant structure w covalent bond insoluble + explain

Answer 39

covalent bonds are more attracted to their neighbours in lattice than solvent molecules. don’t have ions bcs insoluble in polar solvents

Question 40

does giant structure w covalent bond conduct electricity + explain

Answer 40

no charged ions/ free electrons

Question 41

does metal structure have high melting point + explain

Answer 41

- strong metallic bonds

Question 41

is metal structure malleable/ ductile + explain

Answer 41

metal ions can slide over each other without disrupting attraction between pos ions + e

Question 42

is metal structure a good thermal conductors/electrical conductors + explain

Answer 42

delocalised e can pass KE to each other

Question 43

is metal structure insoluble + explain

Answer 43

strength of metallic bonds