Bonding

Question 1

what is an ionic bond ?

Answer 1

a bond between a metal and a non metal where an electrostatic force of attraction occurs between oppositely charged ions

Question 2

state the charges on :
group 1
group2
group6
group7

Answer 2

+
2+
2-
-

Question 3

what is a structure of an ionic bond ?

Answer 3

each ion attracts to opposiute charges - forms giant ionic lattice containing billions of ions (lattice structure)

Question 4

what is formula for :
sulfate
hydroxide
nitrate
carbonate
ammonium

Answer 4

so42-
oh-
no3-
co32-
nh4+

Question 5

ionic bonding properties :nacl
melting and boiling point

Answer 5

high MP &BP as a lot of energy is needed to overcome strong force of electrostatic force of attraction (the higher the charge of the ionic compound the higher the mp and bp - e.g mgo and nacl )

Question 6

ionic bonding strength :nacl

Answer 6

when size of ions decrease , strength increases( . e.g fluoride ions are smaller than chloride ions so calcium fluoride has higher melting point then calcium chloride )
hard and brittle

Question 7

ionic bonding solubility : nacl

Answer 7

they are soluble - but ionic lattice must be broken and water molecules attract and surround ions
as ionic charge increases - solubility decreases

Question 8

ionic bonding electricity nacl

Answer 8

can conduct electricity when molten or in aqueous solution as ions are free to move and conduct electricity . in solid ions cannot move = not conduct electricity

Question 9

when can ionic compounds split ?

Answer 9

if pressure / forces cause ions to one closer to each other , some charged ions may repel causing it to split .

Question 10

what is a covalent bond ?

Answer 10

electrostatic force of attraction between a shared pair of electrons and nuclei of bonded atoms - when atoms are combined by covalent bionds they form molecules

Question 11

what is the difference between multiple and single covalent bonds ?

Answer 11

single = shaired pair of electrons
multiple bonds = multiple pairs of electrons

Question 12

what is a coordinate covalent bond

Answer 12

it is a covalent bond which includes a shaired pair of electrons from 1 atom

Question 13

simple molecular properties iodine MP & BP

Answer 13

low as there are weak forces of attraction

Question 14

simple molecular properties iodine electrical conductivity

Answer 14

doesn’t as no charged particles free to move

Question 15

simple molecular properties iodine strength - brittle

Answer 15

weak intermolecular forces

Question 16

simple molecular properties iodine solubility

Answer 16

depending on intermolecular forces (slightly )

Question 17

giant covalent (diamond ) properties (MP AND BP

Answer 17

high as lots of strong covalent bonds (electrostatic forces of attraction ) between atoms

Question 18

giant covalent (diamond ) properties electrical conductivity ?

Answer 18

cannot as no delocalised electrons around it

Question 19

giant covalent (diamond ) properties strength ?

Answer 19

very strong due top strong force of attraction between carbon atoms - rigid arrangement of atoms held y covalent bonds

Question 20

giant covalent (diamond ) properties solubility ?

Answer 20

insoluble

Question 21

what is metallic bonding ?

Answer 21

sea of delocalised electrons surrounding by poitive ions arranged in a lattice

Question 22

metallic bonding properties - melting point and boiling point

Answer 22

high MP AND BP as high metallic attraction as strong bonds =strong metallic bond between the -ve and +ve charge

Question 23

what is metallic bonding ? strength

Answer 23

strong as force of electrostatic attraction between opposite charges = high metallic bond as layers can slide while maintaining metallic bond

Question 24

what is metallic bonding ? electrical conductivity

Answer 24

high as surrounded by sea od delocalised electrons = conduct electricity

Question 25

what is metallic bonding ? solubility

Answer 25

insoluble

Question 26

graphite + graphene properties MP + BP

Answer 26

high MP AND BP as a lot of energy needed to break all strong covalent bonds

Question 27

graphite + graphene properties electrical conductivity

Answer 27

yes as 1 delocalised electron free per carbon atom = can conduct electricity

Question 28

graphite + graphene properties strength

Answer 28

brittle as weak forces between layers = easy for layers to slide

Question 29

graphite + graphene properties solubility

Answer 29

insoluble

Question 30

ICE properties : MP +BP

Answer 30

low mp amnd bp as there are weak froces of attraction between molecules

Question 31

ICE properties : electrical conductivity

Answer 31

doesn’t conduct as there are no mobile charged particles surrounding it

Question 32

density of ice versus water ?

Answer 32

ice is less dense then water as ice molecules are arranged in a lattice structure due to hydrogen bonds - liquid molecules are closer but not in a lattice

Question 33

electronegativity ?

Answer 33

relative ability of an atom to attract pairs of electrons in covalent bonds

Question 34

electronegativity down a group

Answer 34

electronehativity decreases

Question 35

electronegativity across a period ?

Answer 35

electronegativity increases

Question 36

factors effecting electronegativity

Answer 36

atomic radius - closer to nucleus = stronger attraction between nucleus and bonding pair of electrons
shielding - less shells of electrons between nuclei and the electrons = less shielding = less repulsion = stronger attraction between nucleus and outer bonding electrons
nuclear charge - more protons , stronger attraction between nucleus and bonding pairs of electrons

Question 37

a bond will be non polar when

Answer 37

bonded atoms are the same
bonded atoms have same or similar electronegativity