Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

IGCSE CHEMISTRY MATS > 2 - Periodic Table > Flashcards

2 - Periodic Table Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

Why do Group 8/0 inert?

A
  • they don’t react because they have a full outer shell
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is the charge for a nitrate (NO3)?

A

-1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is the charge of a sulphate (SO4)?

A

-2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is the charge of a carbonate (CO3)?

A

-2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What is the charge of ammonium (NH4)?

A

+1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is the charge of a hydroxide (OH)?

A

-1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What is the charge of silver (Ag)?

A

+1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What is the charge of copper (Cu)?

A

+2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What is the charge of iron (Fe)?

A

+2/+3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is the charge of lead (Pb)?

A

+2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is the charge of zinc (Zn)?

A

+2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What happens when an electron is transferred?

A
  • the element has a charge of +1
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What happens to the charge when an electron is gained?

A
  • negative charge
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What is an ionic bond?

A

Oppositely charged ions that are electrostatically attracted to each other

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What charge does group 1 have?

A

+1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What charge does group 2 have?

A

+2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What charge does group 3 have?

A

+3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What charge does group 5 have?

A

-3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What charge does group 6 have?

A

-2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What charge does group 7 have?

A

-1

21
Q

What is the ionic formula for Aluminium oxide?

A

“Al2O3”

22
Q

What is the ionic formula for Lithium iodide?

A

Li I

23
Q

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

A

CuF2

24
Q

When does an ionic bond happen?

A

non-metal + metal

25
Q

What do ionic bonds create?

A
  • giant ionic lattices
26
Q

What is a giant ionic lattices?

A

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

27
Q

Equation to calculate moles:

A

mol = mass/mr

28
Q

What type of melting point do ionic compounds have?

A
  • high melting point

- requires lots of energy to overcome electrostatic attractions

29
Q

Are ionic compounds soluble?

A
  • yes
30
Q

Are ionic compounds conductive?

A
  • 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
31
Q

What is a covalent bond?

A

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

32
Q

When does a covalent bond form?

A

non-metal + non-metal

33
Q

What does a covalent bonds form?

A
  • simple molecular

- giant covalent

34
Q

What is a simple molecular:

A
  • carbon dioxide, ethane, water

- weak intermolecular bonds that do not need much energy to break

35
Q

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

A
  • low melting and boiling points

- weak intermolecular forces so requires less energy to seperate the ions in the ionic compounds, or atoms in metals

36
Q

Do simple molecular substances conduct?

A
  • they do not have any delocalised electrons
  • they do not have any ions either
  • does not conduct as solids, liquids or aqueous
37
Q

What are 3 examples of giant covalent structures?

A
  • diamond
  • graphite
  • buckminsterfullerene (C60)
38
Q

Describe the carbon bonds of diamond:

A
  • covalent

- each carbon makes 4 bonds

39
Q

Describe the carbon bonds of graphite:

A
  • covalent
  • covalently bonded to 3 other carbon atoms in a layer
  • unbonded electrons from each carbon are delocalised
40
Q

Define delocalised

A
  • free to move around
41
Q

Describe the carbon bonds of buckminsterfullerene

A
  • covalent
  • each carbon makes 3 bonds
  • unbonded electrons are in and outside the sphere
  • 20 hexagons and 12 pentagons
42
Q

Shape of diamond:

A

”- tetrahedral

“

43
Q

Shape of graphite:

A

”- layers of hexagons

“

44
Q

Shape of buckminsterfullerene:

A

”- fixed structure with 20 hexagons and 12 pentagons

“

45
Q

Properties + explanation of diamond:

A
  • 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
46
Q

Properties and explanation of graphite:

A
  • conducts electricity
  • has delocalised electrons
  • slippery
  • layers can slide off each other
47
Q

Properties and explanation of buckminsterfulleren:

A
  • low melting/boiling point
  • limited size of structure
  • individual molecules
48
Q

What are examples of simple molecular?

A
  • gases or liquids

- hydrogen

IGCSE CHEMISTRY MATS (7 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions