Bonding

Question 1

Mass number =

Answer 1

Top number

Total number of protons and neutrons

Question 2

Atomic number

Answer 2

Bottom number

Number of protons

Question 3

How are compounds formed

Answer 3

Two or more elements chemically joined together

Question 4

What are isotapes

Answer 4

Different atomic forms of the same element, which have the SAME number of PROTONS but DIFFERENT number of NEUTRONS

Question 5

Ionic bonding

Answer 5

Atoms LOSE or GAIN electrons to form CHARGED particles (called ions)

Question 6

Ionic compounds

Answer 6

• Have regular ionic lattices
• Form a closely packed regular lattice arrangement
• Similar properties

Question 7

Ionic compounds properties

Answer 7

• high melting & boiling points (strong attraction)
• melt -> free to move
• carry electrical current
• dissolve easily

Question 8

Which groups are most likely to form ions

Answer 8

Groups
1 & 2
6 & 7

Question 9

Ions have the electronic structure of a

Answer 9

Noble gas

Question 10

What happens to group 1 and 2 elements

Answer 10

They lose electrons to form positive ions

Question 11

What happened to group 6 and 7

Answer 11

The gain elections to form negative ions

Question 12

What forms an ionic compound

Answer 12

Positive ions combine with negative ions to form ionic compounds

Question 13

Wha is the overall charge of any compound

Answer 13

Zero

Question 14

The negative charges ——- the positive charges

Answer 14

Balance

E.g. Na+ and Cl- = +1 + -1 = 0 The charges are balanced to for NaCl

Question 15

What is covalent bonding

Answer 15

Sharing electrons with other atoms

Both atoms have a full outer shell

Question 16

Substances with covalent bonds can either be —–

Answer 16

Simple molecules or giant structures

Question 17

Explain a simple molecular structure

Answer 17

• Atoms have strong bonds
• Forces of attraction are weak
• Melting & boiling points are low (easily parted)
• Don’t conduct electricity
• No ions or electrical charge

Question 18

Giant covalent structures are

Answer 18

Macromolecules

Question 19

Giant covalent structures

Answer 19

• Atoms are bonded by strong covalent bonds
• High melting and boiling points
• Don’t conduct electricity
• Example - diamond

Question 20

Metallic structures

Answer 20

• Consists of giant structures
• Have free electrons -> good heat and electricity conductors
• Allow layers to slide over each other/bent/shaped

Question 21

Alloys are harder than

Answer 21

Pure metals

Question 22

Pure metals

Answer 22

• Have different sized atoms
• Distort the layers
• More difficult for layers to slide over each other

Question 23

Draw the ionic structure of Sodium Chloride

Answer 23

Na+ Cl-

Question 24

Draw the ionic structure of calcium oxide

Answer 24

Cl- Ca2+ Cl-

Question 25

Draw the covalent bond of Hydrogen and Chlorine

Answer 25

H-H Cl-Cl

Question 26

Simple molecules definition

Answer 26

A few atoms held together by strong covalent bonds. An example is carbon dioxide (CO2), the molecules of which contain one atom of carbon bonded with two atoms of oxygen.

Question 27

Properties of simple molecular substances | Low melting and boiling points

Answer 27

This is because the weak intermolecular forces break down easily.

Question 28

Properties of simple molecular substances | Non-conductive

Answer 28

they do not have any free electrons or an overall electric charge.

Question 29

Giant covalent structures definition

Answer 29

- Contain a lot of NON- METAL ATOMS joined to adjacent atoms by covalent bonds. - Atoms are arranged into giant regular lattices - extremely STRONG STRUCTURES because of the many bonds involved.

Question 30

Properties of giant covalent structures | Very high melting points

Answer 30

a lot of strong covalent bonds must be broken. Graphite, for example, has a melting point of more than 3,600ºC.

Question 31

Properties of giant covalent structures | Variable conductivity

Answer 31

Diamond does not conduct electricity. Graphite contains FREE ELECTRONS , so it DOESN'T conduct electricity. Silicon is semi-conductive - that is, midway between non-conductive and conductive.

Question 32

Metals have a

Answer 32

Giant structure

Question 33

Why do metallic bonds have free electrons

Answer 33

Produce all the properties of metals

Question 34

Where do free electrons come from

Answer 34

The outer shell of every atom in the structure

Question 35

Metals are

Answer 35

good conductors of HEAT and ELECTRICITY

Question 36

How do electrons hold atoms together

Answer 36

They have strong forces of electrostatic attraction between positive metal ions and negative electrons