Bonding

Question 1

What is ionic bonding?

Answer 1

Its the electrostatic attraction between oppositely charged ions in a lattic.

Question 2

What is formula of the compound ions?

Answer 2

Sulfate: SO-4
Hydroxide: OH-
Nitrate: NO3-
Carbonate: CO3-2
Ammonium: NH4+

Question 3

What is the structure of an ionic compound?

Answer 3

A giant ionic lattice with alternating positive and negative ions.

Question 4

What is metallic bonding?

Answer 4

The attraction between delocalised electrons and positive ions arranged in a lattice

Question 5

What is a covalent bond?

Answer 5

chemical bond where two atoms share electrons to achieve a stable, full outer electron shell

Question 6

what is a mutliple bond

Answer 6

A bond containing more than one shared pair of electrons

Question 7

What is a coordinate bond?

Answer 7

A covalent bond where the shared pair of electrons comes from only one atom.

Question 8

How is a coordinate bond represented in diagrams?

Answer 8

With an arrow (→) pointing from the donor atom to the acceptor atom

Question 9

Give an example of a coordinate bond in a molecule.

Answer 9

NH₄⁺ (formed when NH₃ donates a lone pair to H⁺).

Question 10

what is metallic bonding

Answer 10

attraction between delocalised electrons and positive ions arranged in a lattice.

Question 11

what are the 4 types of crystals

Answer 11

Ionic, metallic, macromolecular and molecular

Question 12

Melting/boiling points of ionic crystals?

Answer 12

High — strong ionic bonds require lots of energy to break.

Question 13

electrical conductivity of ionic crystals?

Answer 13

Conduct when molten or dissolved (ions free to move), not when solid.

Question 14

Melting points of metallic crystals?

Answer 14

High — strong metallic bonds, especially in small, highly charged ions like Mg²⁺.

Question 15

Electrical conductivity of metals?

Answer 15

Conduct when solid and liquid — delocalised electrons move freely.

Question 16

What bonding is present in diamond?

Answer 16

Each carbon covalently bonded to 4 others in a tetrahedral 3D structure.

Question 17

Properties of diamond?

Answer 17

Very high melting point, hard, doesn’t conduct electricity

Question 18

What bonding is present in graphite?

Answer 18

Each carbon covalently bonded to 3 others in layers with delocalised electrons between layers.

Question 19

Properties of graphite?

Answer 19

High melting point, conducts electricity (delocalised electrons), layers slide due to weak intermolecular forces.

Question 20

What bonding is present in iodine crystals?

Answer 20

van der Waals’ forces.

Question 21

Properties of iodine crystals?

Answer 21

Low melting point, do not conduct electricity.

Question 22

What bonding is present in ice?

Answer 22

Water molecules held by hydrogen bonding in an open lattice.

Question 23

Properties of ice?

Answer 23

Low melting point, less dense than water due to hydrogen bonds being more spread

Question 24

What type of crystals have the highest melting points?

Answer 24

ionic and macro

Question 25

How are bonding and lone pairs of electrons represented?

Answer 25

As charge clouds that repel each other.

Question 26

What determines the shape of a molecule?

Answer 26

The number of bonding and lone pairs of electrons around the central atom.

Question 27

Order of electron pair repulsion strength?

Answer 27

Lone pair–lone pair > lone pair–bond pair > bond pair–bond pair.

Question 28

What happens to bond angles as lone pairs are added?

Answer 28

Bond angles decrease because lone pairs repel more strongly.

Question 29

2 bonding pairs

Answer 29

Shape: Linear Bond angle: 180° Example: BeCl₂, CO₂

Question 30

what is electronegativity

Answer 30

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

Question 31

3 bonding pairs

Question 32

How do polar bonds share electrons

Answer 32

share electrons unequally

Question 33

how do non polar bonds share electrons

Answer 33

share electrons equally

Question 34

What is a permanent dipole?

Answer 34

A separation of charge in a molecule where one end is always slightly negative and the other slightly positive.

Question 35

Why do some molecules with polar bonds not have a permanent dipole?

Answer 35

Because the molecular shape is symmetrical, so the bond dipoles cancel each other out.

Question 36

Which type of intermolecular force is present in all molecules

Answer 36

Induced dipole–dipole (London/dispersion) forces.

Question 37

how does the strength of metallic bonds change across the period.

Answer 37

increases higher MP,BP greater charge on ion more delocalised electron per ion stronger forces of atrraction

Question 38

describe van der waal forces

Answer 38

temp dipoles are created by random movement of electrons induces dipole in neighbouring mole temp induced dipole dipole ineraction made

Question 39

which experiences more replusion bp or lp

Answer 39

LP -LP BP-LP BP-BP

Question 40

what is the shape 2 bond pair 0 lone pairs

Answer 40

linear 180

Question 41

what is the shape 3 bond pairs 0 lone pairs

Answer 41

trigonal planar 120

Question 42

what is the shape 4 bond pairs 0 lone pairs

Answer 42

tetrahedral 109.5

Question 43

what is the shape 5 bond pairs 0 lone pairs

Answer 43

trigonal bypyramid 90 and 120

Question 44

what is the shape 6 bond pairs 0 lone pairs

Answer 44

octahedral 90

Question 45

what is the shape 3 bonding pairs + 1 lone pair

Answer 45

trigonal pydramidal 107

Question 46

what is the shape 2 bond pair 2 lone pais

Answer 46

v shaped/ bent 104.5