2 - Periodic Table

Question 1

Why do Group 8/0 inert?

Answer 1

• they don’t react because they have a full outer shell

Question 2

What is the charge for a nitrate (NO3)?

Answer 2

-1

Question 3

What is the charge of a sulphate (SO4)?

Answer 3

-2

Question 4

What is the charge of a carbonate (CO3)?

Answer 4

-2

Question 5

What is the charge of ammonium (NH4)?

Answer 5

+1

Question 6

What is the charge of a hydroxide (OH)?

Answer 6

-1

Question 7

What is the charge of silver (Ag)?

Answer 7

+1

Question 8

What is the charge of copper (Cu)?

Answer 8

+2

Question 9

What is the charge of iron (Fe)?

Answer 9

+2/+3

Question 10

What is the charge of lead (Pb)?

Answer 10

+2

Question 11

What is the charge of zinc (Zn)?

Answer 11

+2

Question 12

What happens when an electron is transferred?

Answer 12

• the element has a charge of +1

Question 13

What happens to the charge when an electron is gained?

Answer 13

• negative charge

Question 14

What is an ionic bond?

Answer 14

Oppositely charged ions that are electrostatically attracted to each other

Question 15

What charge does group 1 have?

Answer 15

+1

Question 16

What charge does group 2 have?

Answer 16

+2

Question 17

What charge does group 3 have?

Answer 17

+3

Question 18

What charge does group 5 have?

Answer 18

-3

Question 19

What charge does group 6 have?

Answer 19

-2

Question 20

What charge does group 7 have?

Answer 20

-1

Question 21

What is the ionic formula for Aluminium oxide?

Answer 21

“Al2O3”

Question 22

What is the ionic formula for Lithium iodide?

Answer 22

Li I

Question 23

What is the ionic formula for Copper (II) fluoride?

Answer 23

CuF2

Question 24

When does an ionic bond happen?

Answer 24

non-metal + metal

Question 25

What do ionic bonds create?

Answer 25

- giant ionic lattices

Question 26

What is a giant ionic lattices?

Answer 26

Lots of very strong electrostatic attractions that take a lot of energy to break

Question 27

Equation to calculate moles:

Answer 27

mol = mass/mr

Question 28

What type of melting point do ionic compounds have?

Answer 28

- high melting point | - requires lots of energy to overcome electrostatic attractions

Question 29

Are ionic compounds soluble?

Answer 29

- yes

Question 30

Are ionic compounds conductive?

Answer 30

- if ionic compound is solid, they do not conduct electricity or thermal - if ionic compound is dissolved/melted they can conduct electricity because ions are free to move and therefore carry charge

Question 31

What is a covalent bond?

Answer 31

Strong electrostatic attraction between (a) shared pair(s) of electrons and the posistive nuclei of the atoms

Question 32

When does a covalent bond form?

Answer 32

non-metal + non-metal

Question 33

What does a covalent bonds form?

Answer 33

- simple molecular | - giant covalent

Question 34

What is a simple molecular:

Answer 34

- carbon dioxide, ethane, water | - weak intermolecular bonds that do not need much energy to break

Question 35

What type of melting and boiling points do simple moleculars have? Why?

Answer 35

- low melting and boiling points | - weak intermolecular forces so requires less energy to seperate the ions in the ionic compounds, or atoms in metals

Question 36

Do simple molecular substances conduct?

Answer 36

- they do not have any delocalised electrons  - they do not have any ions either - does not conduct as solids, liquids or aqueous

Question 37

What are 3 examples of giant covalent structures?

Answer 37

- diamond - graphite - buckminsterfullerene (C60)

Question 38

Describe the carbon bonds of diamond:

Answer 38

- covalent  | - each carbon makes 4 bonds

Question 39

Describe the carbon bonds of graphite:

Answer 39

- covalent - covalently bonded to 3 other carbon atoms in a layer - unbonded electrons from each carbon are delocalised

Question 40

Define delocalised

Answer 40

- free to move around

Question 41

Describe the carbon bonds of buckminsterfullerene

Answer 41

- covalent - each carbon makes 3 bonds - unbonded electrons are in and outside the sphere - 20 hexagons and 12 pentagons

Question 42

Shape of diamond:

Answer 42

"- tetrahedral | "

Question 43

Shape of graphite:

Answer 43

"- layers of hexagons | "

Question 44

Shape of buckminsterfullerene:

Answer 44

"- fixed structure with 20 hexagons and 12 pentagons | "

Question 45

Properties + explanation of diamond:

Answer 45

- hard  - strong - high melting/boiling points  - does not conduct electricity  - covalent bonds are strong - many covalent bonds so it takes a lot of energy to break - no delocalised electrons

Question 46

Properties and explanation of graphite:

Answer 46

- conducts electricity - has delocalised electrons - slippery - layers can slide off each other

Question 47

Properties and explanation of buckminsterfulleren:

Answer 47

- low melting/boiling point - limited size of structure - individual molecules

Question 48

What are examples of simple molecular?

Answer 48

- gases or liquids | - hydrogen