Bonding

Question 1

What do metal do?

Answer 1

Lose electrons to become +

Question 2

What do non-metals do?

Answer 2

Gain electrons -

Question 3

When is ionic bonding stronger?

Answer 3

When ions are smaller and have higher charges

Question 4

Define covalent bond

Answer 4

A shared pair of electrons

Question 5

When do dative covalent bonds form?

Answer 5

The shared electrons in a covalent bond come from one of the bonding atoms

Question 6

What is a dative covalent bond also called?

Answer 6

Co-ordinate bonding

Question 7

Define metallic bond

Answer 7

An electrostatic force of attraction between positive metal ions and delocalised electrons

Question 8

What affects the strength of metallic bonds?

Answer 8

1) number of protons/ strength of nuclear attraction
2) number of delocalised electrons per atom
3) size of ion

Question 9

Define ionic bond?

Answer 9

Electrostatic force of attraction between oppositely charged ions formed at energy transfer

Question 10

Electro negativity

Answer 10

Relative tendency of an atom in a molecule to attract electrons to itself

Question 11

Name the four structures you need to know.

Answer 11

Giant ionic lattice
Simple molecular
Macromolecular
Giant metallic lattice

Question 12

Bonding for Giant ionic lattice?

Answer 12

Ionic

Question 13

Bonding for Simple molecular?

Answer 13

Covalent

van der waals, dipole-dipole, hydrogen bonding

Question 14

Bonding for macromolecular?

Answer 14

Covalent

Question 15

Bonding for giant metallic lattice

Answer 15

Metallic

Question 16

Example of Giant ionic lattice?

Answer 16

Sodium chloride

Magnesium oxide

Question 17

Example of Simple molecular?

Answer 17

Iodine, ice, carbon dioxide, water, methane

Question 18

Example of Macromolecular?

Answer 18

Diamond, graphite, silicon dioxide, silicon

Question 19

Examples for giant metallic lattice?

Answer 19

Magnesium sodium (all metals)

Question 20

Giant ionic lattice boiling and melting point?

Answer 20

High because of ions with electrostatic forces between oppositely charged ions

Question 21

Simple molecular boiling and melting point?

Answer 21

Low because of weak intermolecular forces between molecules

Question 22

Macromolecular boiling and melting point?

Answer 22

High because of many strong covalent bonds in the macromolecular structure.

Question 23

Giant metallic lattice melting and boiling points?

Answer 23

High

Strong electrostatic forces between positive charge ions and sea of delocalised electrons

Question 24

Solubility in water

Answer 24

Giant Ionic lattice- generally good
Simple Molecular- generally poor
Macromolecular- insoluble
Giant metallic lattice-insoluble

Question 25

Conductivity when solid

Answer 25

Giant Ionic lattice- poor can’t move
Simple Molecular- no ions to conduct and electrons are localised
Macromolecular- diamond and sand poor electrons can’t move, graphite good as free delocalised electrons between layers
Giant metallic lattice- good delocalised electrons can move through

Question 26

General description Giant Ionic lattice?

Answer 26

Crystalline solid

Question 27

General description Simple Molecular

Answer 27

Mostly gases or liquid

Question 28

General description Macromolecular?

Answer 28

Solids

Question 29

General description Giant metallic lattice?

Answer 29

Shiny metal
Malleable as positive ions in the lattice are all identical. So planes of ions can slide over each other easily.
Attractive forces in lattice are same whichever ions are adjacent.