1.2 Bonding

Question 1

Ammonium

Answer 1

NH4 +

Question 2

Hydroxide

Answer 2

OH-

Question 3

Nitrate

Answer 3

NO3 -

Question 4

Nitrite

Answer 4

NO2 -

Question 5

Hydrogencarbonate

Answer 5

HCO3 -

Question 6

Chlorate (I)

Answer 6

ClO-

Question 7

Chlorate (V)

Answer 7

ClO3 -

Question 8

Carbonate

Answer 8

CO3 2-

Question 9

Sulfate

Answer 9

SO4 2-

Question 10

Sulfite

Answer 10

SO3 2-

Question 11

Dichromate

Answer 11

Cr2O7 2-

Question 12

Sulfide

Answer 12

S2-

Question 13

Phosphate

Answer 13

PO4 3-

Question 14

Nitride

Answer 14

N3-

Question 15

Linear

Answer 15

180°

Question 16

Trigonal planar

Answer 16

120°

Question 17

Tetrahedral

Answer 17

109.5°

Question 17

Tetrahedral

Answer 17

109.5°

Question 18

Trigonal bipyramidal

Answer 18

120°
90°

Question 19

Octahedral

Answer 19

90°

Question 20

V-shape

Answer 20

2 bonding
1 lone
117.5°

Question 21

Pyramidal

Answer 21

3 bonding
1 lone
107°

Question 22

See-saw

Answer 22

4 bonding
1 lone
119
89

Question 23

Square pyramidal

Answer 23

5 bonding
1 lone
89

Question 24

V-shape

Answer 24

2 bonding
2 lone
104.5

Question 25

T-shape

Answer 25

3 bonding
2 lone
89

Question 26

Square Planar

Answer 26

4 bonding
2 lone
90

Question 27

Describe the structure and particles of metallic bonding

Answer 27

Structure: giant metallic lattice
Particles: positive metal ions
delocalised electrons

Question 28

Describe the structure and particles within ionic bonding

Answer 28

Structure: giant ionic lattice
Particles: negative and positive ions

Question 29

Describe the structure and particles of macromolecular covalent bonding

Answer 29

Structure: macromolecular
Particles: atoms

Question 30

Describe the structure and particles of simple molecular covalent bonding

Answer 30

Structure: simple molecular
Particles: molecules

Question 31

Metallic bonding definition

Answer 31

The strong electrostatic forces of attraction between positive metal ions and a sea of delocalised electrons

Question 32

Properties of metals

Answer 32

Conductivity: good electrical and thermal conductors
Strength: very strong
Malleable: highly malleable
Melting point: stronger the metallic bonds, the higher the melting or boiling point

Question 33

Why are metals good conductors?

Answer 33

The electrical current can be transferred through the delocalised electrons

Question 34

Why are most metals strong?

Answer 34

There is strong electrostatic forces of attraction between the metal ions and delocalised electrons

Question 35

Why are metals malleable?

Answer 35

The layers of metal ions can slide over each other

Question 36

What are the two types of covalent bonds?

Answer 36

Macromolecular
SImple molecular

Question 37

Covalent bond definition

Answer 37

A shared pair of electrons between two atoms

Question 38

Examples of macromolecular structures

Answer 38

Carbon
Silicon
Silicon oxide

Question 39

Ionic bonding definition

Answer 39

The strong electrostatic attraction between two oppositely charged ions

Question 40

How do you know what forms the positive or negative ion?

Answer 40

Electrons are transferred from the metal to the non metal
The metal will therefore always form the positive ion and the non metal will be negative

Question 41

Properties of ionic compounds

Answer 41

High melting point and boiling point
Electrical conductivity
Brittle

Question 42

Coordinate bond definition

Answer 42

A shared electron pair which both have come from there same atom

Question 43

How do you represent a covalent bond?

Answer 43

An arrow

Question 44

Electronegativity definition

Answer 44

The power of an atom to attract the pair of electrons in a covalent bond

Question 45

How does electronegativity change across the periodic table

Answer 45

Increases

Question 46

How does electronegativity change as you go down the periodic table

Answer 46

Decreases

Question 47

Why does the electronegativity change as you go across the periodic table?

Answer 47

The number of protons increases
Shielding stays the same
The ability to attract electrons in a covalent bond increases

Question 48

What are the types of intermolecular forces?

Answer 48

Induced dipole dipole
Permanent dipole dipole
Hydrogen bonding

Question 49

What type of IMF does a molecule have if it is polar?

Answer 49

Permanent dipole dipole

Question 50

What type of IMF does a molecule have if it isn’t polar?

Answer 50

Induced dipole dipole

Question 51

What does polar mean?

Question 52

What type of IMF is the strongest?

Answer 52

Hydrogen

Question 53

When does hydrogen bonding occur?

Answer 53

Between a H bonded to an O, N or F

Question 54

How does hydrogen bonding arise?

Answer 54

Large difference in electronegativity between the oxygen and hydrogen
This creates a dipole on the O-H
The lone pair on the oxygen atom in one molecule strongly attracts the partially positive hydrogen atom in another molecule

Question 55

When does PDD occur?

Answer 55

Between two polar molecules

Question 56

How does PDD arise?

Answer 56

Difference in electronegativity leads to bond polarity
Dipoles don’t cancel out therefore the molecule has an overall permanent dipole
There is an attraction between the delta positive on one molecule and the delta negative on another molecule

Question 57

When does IDD occur?

Answer 57

Between all molecules but generally non polar molecules

Question 58

How does IDD arise?

Answer 58

Random movement of electrons in one molecule leads to an
Uneven distribution of electrons creating a
Temporary dipole in one atom, this
Induces a dipole in a neighbouring molecule and
Dipoles attract

Question 59

When is hydrogen bonding used?

Answer 59

Ice
Proteins
DNA