Bonding

Question 1

2 main types of bonding in compounds

Answer 1

Ionic
Covalent

Question 2

sulfate ion

Answer 2

SO4^2-

Question 3

hydroxide ion

Answer 3

OH-

Question 4

nitrate ion

Answer 4

NO3- (3 IS below)

Question 5

carbonate ion

Answer 5

CO3 ^2-

Question 6

ammonium ion

Answer 6

NH4^+

Question 7

what struc does sodium chloride have

Answer 7

giant ionic lattice

Question 8

Sodium azide has a high melting point.
Predict the type of bonding in a crystal of sodium azide.
Suggest why its melting point is high.

Answer 8

Ionic
Oppositely charged ions / Na+
and N3 ions
Strong attraction between (oppositely charged) ions / lots of energy needed to
overcome (strong) attractions (between ions) - mark scheme ans

Question 9

3 features of ionic compounds

Answer 9

1) conduct electrivcity when molten or dissolved - free moving ions that can carry charge
2) ionic compound have high melting points - strong electrostatic attraction bet oppositely charged ions that take alot of energy to overcome
3)ionic compounds tend to dissolve in water - water mol are polar
charged parts pull ions away from lattice

Question 10

what is covalent bonding

Answer 10

atoms have a shared pair of electrons

Question 11

what struc has huge network of covalently bonded atoms

Answer 11

giant covalent stuc
macromolecular struc

Question 12

What is a dative covalent bond?

Answer 12

2 electrons are donated from one atom to another / a lone pair of electrons rather than one from each

Question 13

2 types of covalent structures

Answer 13

Simple molecular I simple covalent
Macro molecular/giant covalent structures

Question 14

Examples of simple covalent

Answer 14

Co2 Ch4 Cl2

Question 15

What is broken when boiling covalent structures

Answer 15

IMF’s not the strong covalent bonds

Question 16

Examples of giant covalent struc

Answer 16

Diamond, graphite, silicon dioxide

Question 17

Describe diamonds structure and its properties

Answer 17

Each carbon atoms makes 4 bonds sono free electrons to form used of delocalised electrons to carry charge or conduct electricity thus diamond cannot conduct.
Diamond is hard with a high melting point due to strong covalent bands that take a lot of energy to break
Diamond is insoluble in water

Question 18

Describe graphite structure and its properties

Answer 18

Giant covalent structure
Can conduct electricity as each carbon atom makes 3 bonds so there is one free delocalised electron per carbon atom forming sea of delocalised elections that can more throughout structure and conduct electricity.
Graphite is soft BCD weak IMF’s I vow between layers d’atoms allowing them to slide over eachother
Has high melting point due to strong covalent bands within mol

Question 19

Where are covalent bands and imfs found

Answer 19

Covalent - within
IMF’s found between

Question 20

What is metallic banding ?

Answer 20

Lattice of positive ions surrounded by sea of delocalised_ electrons
There are electrostatic attractions

Question 21

Properties of metals

Answer 21

Good conductors due to sea of delocalised electrons
High melting and boiling point do to strong bands due to strong attraction

Question 22

Properties of metals going down a group

Answer 22

Usually looking @ groups 123 - all ions have same charge so this factor not important instead looking at increasing atomic radius so delocalised e-further away from metalions so weaker attraction = weaker metallic bond and so lower boiling point

Question 23

Properties of metals across a period

Answer 23

Increase in melting point due to increasing charge so stronger attraction between the positive ions and e-so stronger metallic bonds so higher melting point

Question 24

Why does boron trichlovide have tribunal planar shape?

Answer 24

3 bonds that repel equally to get as for away from eachother as possible lo minimise repulsion.

Question 25

2BP?

Answer 25

Linear 180°

Question 26

3BP

Answer 26

trigonal planar 120°

Question 27

4 bp

Answer 27

Tetrahedral 109.5°

Question 28

2 bp +2LP

Answer 28

Bent/v -shaped 104. 5°

Question 29

3BP + one lp

Answer 29

Trigonal pyramidal 107.5°

Question 30

5 bp

Answer 30

Tribunal bipyramidal 120° + 90°

Question 31

6 bp

Answer 31

Octahedral 90°

Question 32

4BP+2LP

Answer 32

Square planar 90°

Question 33

4BP and one lone pair

Answer 33

See- saw 102° +87°

Question 34

3 bp t2LP

Answer 34

T-shaped 88°

Question 35

How to find shape of mol

Answer 35

Determine group no of central. Add one to it for each band it makes. Add one for each negative charge and subtract are for each positive charge. Men divide by 2 to give you number of banding pairs.

Question 36

Order of now much lone pairs t banding pairs repel

Answer 36

Lone pair 2x) then /lp + 1BP then 2 bp

Question 37

Define electronegativty

Answer 37

Power of an atom to attract banding pair A electrons in covalent bond

Question 38

How is polar band formed in h-cl band

Answer 38

Chlorine is mare electronic so attracts banding pair of electrons more strongly giving it a deltanegative charge whilst hydrogen has delta positive. Creates a dipole.

Question 39

When can something with dipole not be polar

Answer 39

Dipoles cancel out due to symmetrical bonds

Question 40

3 things that determine it polar on non polar.

Answer 40

If it has delta neg t pos charge = polar Lone pair = polar all same atom on outside than nan polar

Question 41

3 types of intermole ocular forces from highest to lowest strength

Answer 41

Hydrogen bonding Dipole-dipole interactions (permanent) Van her walls

Question 42

Describe vdw

Answer 42

All mol have this IMF E more within e-cloud e same point there will be more e-on one side than the other creating , induced temporary dipole Dipole influences another nearby mol inducing a dipole in that Dipoles only temporary bc e are constantly moving

Question 43

What molecules * only * contain van her Walls

Answer 43

Non polar

Question 44

Boiling points and van den walls

Answer 44

Increaesd molecular weight = increased e = stronger V

Question 45

Van her walls in hydrocarbons

Answer 45

1) chain length increase means more e- so stronger van so higher bp 2) branching of 2 alkanes with same molecular weight, branching decreases chairs length so lower electron su weaker van per Walls so less ar surface areal points of contact

Question 46

Describe permanent dipole

Answer 46

Eg band h-cl Large difference in electronegativity

Question 47

Hydrogen banding occurs between hydrogen and...

Answer 47

Nitrogen, oxygen and fluorine

Question 48

Solubility of non polar and polar mo)

Answer 48

Polar mol dissolve in polar solvents and non polar md dissolve in non polar solvents Bc mol dissolved has to form intermolecular forces with solvent, if these stranger than forces broken it will be dissolved su

Question 49

A mol can dissolve in water it...

Answer 49

It is able to form hydrogen bonds with it.