Topic 2 - The Periodic Table

Question 1

Periods

Answer 1

Horizontal Rows
- number of shells

Question 2

Groups

Answer 2

Vertical Columns
- number of electrons in outer shell

Question 3

Noble Gases

Answer 3

have a full outer shell
- therefore, inert

Question 4

Electrons

Answer 4

Negatively charged subatomic particles which orbit the nucleus of an atom in shells

Question 5

Loss of electrons

Answer 5

Positively charged

Question 6

Gain of electrons

Answer 6

Negatively Charged

Question 7

Metals always form

Answer 7

CATIONS

Question 8

Properties of Metals

Answer 8

• good heat conductors
• good electrical conductors
• malleable
• ductile
• sonorous (ring when struck)
• held together by metallic bonds

Question 9

Transition Metals

Answer 9

• used as catalysts
• share metal properties
• form different coloured solutions
• create ions of different charges

Question 10

Groups 1,2,6,7

Answer 10

Form ions EASILY

only need to gain/lose a small number of electrons

Question 11

Groups 3,4,5

Answer 11

Do NOT form ions easily

need to gain/lose a large number of electrons

Question 12

Magnesium ionisation equation

Answer 12

Mg -> Mg2+ + 2e-

Question 13

Ionic Bonding

Answer 13

electrostatic forces of attraction between oppositely charged ions

• dot and cross diagrams

Question 14

Ionic Compounds

Answer 14

• many ionic bonds
• regular 3D lattice structure

Question 15

Properties of Ionic Compounds

Answer 15

• high melting and boiling points (strong bonds require lots of heat energy)
• conduct electricity when molten or in aqueous solution (free moving ions can carry)

Question 16

Polyatomic Ions

Answer 16

Hydroxide (OH -)
Sulphate (SO4 2-)
Nitrate (NO3 -)
Carbonate (CO3 2-)
Ammonium (NH4 +)

Question 17

Covalent Bonding

Answer 17

electrostatic forces of attraction between a shared pair of electrona and the nuclei of atoms involved.

Question 18

Simple Covalent Substances

Answer 18

• weak intermolecular forces, strong covalent bonds
• low melting and boiling points
• cannot conduct electricity

Question 19

Characteristics of Diamond

Answer 19

• All four valence electrons used
• Hard
• High melting & boiling point
• Does not conduct electricity
• Used for jewelry and cutting tools

Question 20

Characteristics of Fullerene C60

Answer 20

• Only 3 valence elecctrons used
• soft
• low melting and boiling point
• conducts electricity (delocalised electrons)
• used for lubricant and drug delivery system in body

Question 21

Characteristics of Graphite

Answer 21

• only 3 valence electrons used
• soft
• high melting & boiling point
• conducts electricity (delocalised electrons)
• used for lubricant and electrodes
• weak intermolecular forces between layers -> slide over each other

Question 22

Metal & Nonmetal

Answer 22

Ionic Bonding

Question 23

Nonmetal & Nonmetal

Answer 23

Covalent Bonding

Question 24

Metal & Metal

Answer 24

Metallic Bonding

Question 25

Malleable

Answer 25

Can be bent or hammered into shape

Question 26

Ductile

Answer 26

Can be pulled into strings/wires

Question 27

Alloy

Answer 27

Metal made by combining two or more metallic elements

Question 28

Why are alloys stronger than pure metals?

Answer 28

Particles of different sizes are unable to slide over each other, making them harder.

Question 29

Metallic Bonding

Answer 29

electrostatic forces of attraction between metal cations and a sea of delocalised electrons

Question 30

Why do metals conduct electricity

Answer 30

sea of delocalised electrons

Question 31

Reactivity in Group 7 (Halogens)

Answer 31

Decreases as you go down

Question 32

States & Colours of Halogens at room temp

Answer 32

chlorine - yellow gas bromine - orange liquid iodine - blue black solid