Brainscape's Knowledge GenomeTM

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


See full index

GCSE AQA Chemistry > Topic 2- Bonding > Flashcards

Topic 2- Bonding Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards GCSE Religious Studies - Edexcel Route A flashcards GCSE Religious Studies - Eduqas Route A flashcards GCSE Geography - AQA flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards GCSE Religious Studies - Edexcel Route B flashcards GCSE Religious Studies - Eduqas Route B flashcards
1
Q

Define Ion

A

Charged particles of either single atoms or a group of atoms

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

Why do atoms form ions?

A

They’re attempting to gain a full outer shell to mimic a noble gas (stable electronic structure)

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

When metals form ions they?

A

Lose electrons to form positive ions

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

When non-metals form ions they?

A

Gain electrons to form negative ions

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

The charge on the ion =

A

Number of electrons lost or gained

eg. 2+ loses 2 electrons, 3- gains 3 electrons

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

Ionic Bonding

A

A metal and a non-metal transferring electrons

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

Oppositely charged ions are…

A

Strongly attracted to eachother by electrostatic forces

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

Group 1 and 2 metals (ionic bonding)

A

Lose electrons to form positive ions(cations)

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

Group 6 and 7 elements… (ionic bonding)

A

Gain electrons to form negative ions (anions)

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

Ionic compounds are arranged in…

A

Giant Ionic Lattice

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

Giant Ionic Lattice

A

Ions closely packed in a regular lattice arrangement held together by strong electrostatic forces of attraction between oppositely charged ions in all directions in the lattice

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

Properties of ionic compounds

A

-high melting points
-high boiling points
(Due to the many strong bonds that take a lot of energy to overcome)
-not conductors of electricity(solid)
(The ions are held in place)
-conductors of electricity(liquid)
(The ions are free to move and carry charge)
-dissolve easily in water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Calculate Empirical Formula from ions

A

Ensure total ionic charge is zero

Eg. Ca2+ + Cl- > CaCl2

2+ + (2)- > 0

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

Covalent Bonding

A

Non metals bond together, sharing pairs of electrons to complete shells.

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

Why are Covalent Bonds strong?

A

The positively charged nuclei of each atoms are attracted to the shared electrons by electrostatic forces

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

Where are the electrons in covalent bonding shared?

A

In the outer shell where there are the highest energy levels

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

Why do atoms make covalent bonds

A

To complete its outer shell to provide an electronic structure that is stable

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

How are Covalent Bonds drawn?

A
  • Using a dot-and-cross diagram, the shared electrons drawn in the overlap between the outer shells of two atoms
  • Using a displayed formula, the Covalent bonds drawn as single lines between atoms
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

How do you find the molecular formula from a covalent bond diagram?

A

Counting up the number of each atom present in the diagram

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

Simple Molecular Substances

A

Made up of molecules containing a few atoms joined together by Covalent Bonds

Eg. HCl, CH4, O2

21
Q

Properties of Simple Molecular Substances

A
  • contain covalent bonds
  • weak forces of attraction between molecules
  • low melting and boiling points, only need to break weak intermolecular forces instead of covalent bonds
  • most are gases or liquids at room temp
  • the larger they are, the stronger the forces, the higher the melting and boiling points
  • don’t conduct electricity (no charge)
22
Q

Polymer

A

Many small units linked together to form a long molecule with repeating sections, joined together by strong covalent bonds

23
Q

Drawing polymers

A

Draw the shortest repeating section in brackets, with an “n” on the outside to represent the units repeated multiple times

24
Q

Writing molecular formula of a polymer

A

Write the molecular formula in brackets and place an “n” outside

Eg. (C2H4)n

25
Q

Properties of polymers

A
  • intermolecular forces larger than of simple covalent molecules, solid at room temp
  • weaker than of covalent bonds, lower melting and boiling points
26
Q

Giant Covalent Structures

A

All atoms bonded by covalent bonds

27
Q

Properties of a Giant Covalent Structure

A

-very high melting and boiling points
(Strong covalent bonds require a lot of energy to break)
-don’t conduct electricity
(No charged particles, except Graphite)

28
Q

Diamond

A

Each carbon atom forms four covalent bonds in a rigid giant covalent structure

29
Q

Graphite

A

Each carbon atom forms three covalent bonds to create layers of hexagons. Each carbon atom has one delocalised electron

30
Q

Properties of Diamond

A

-very hard
(Each carbon atom forms four covalent bonds)
-very high melting points
(Takes a lot of energy to break covalent bonds)
-doesn’t conduct electricity
(No free electrons or ions)

31
Q

Properties of Graphite

A 
-soft
(Weak intermolecular forces between layers)
-high melting point
(Lots of energy to break cb)
-conducts electrical and thermal energy
(One delocalised electron)
32
Q

Graphene

A

A sheet of carbon atoms joined together in hexagons, one atom thick

33
Q

Properties of Graphene

A 
-strong
(Held together by cb)
-light
(One atoms thick)
-conducts electricity
(Has one delocalised electron)
34
Q

Fullerenes

A

Molecules of carbon shaped like closed tubes or hollow balls. They’re made up of carbon atoms arranged in hexagons, pentagons or heptagons

35
Q

Uses of Fullerenes

A

Can be used to deliver drugs
Can be used as industrial catalysts
Can be used as a lubricant
Can form nanotubes

36
Q

Metallic Bonding

A

Strong forces of electrostatic attraction hold positive metal ions with the shared negative electrons in a regular structure

37
Q

Properties of Metals

A 
-Solid at room temp
(Strong electrostatic forces)
-Good conductors of electricity and heat
(Delocalised electrons)
-Malleable
(Layers of atoms slide over eachother)
>> alloys are stronger as they don’t have layers
38
Q

Solids > Liquids

A

particles gain energy, vibrate more which weakens forces and eventually have enough energy to break free from positions into a liquid

39
Q

Liquid > Gas

A

Particles gain more energy, move faster which weakens bonds until eventually they have enough energy to break their bonds

40
Q

Gas > Liquid

A

As gas cools, particles don’t have enough energy to overcome forces of attraction between them, bonds form

41
Q

Liquid > Solid

A

Particles have less energy after cooling, move less, cannot overcome forces of attraction so more bonds form until they’re held in place

42
Q

State Symbols

A

(s) - solid
(l) - liquid
(g) - gas
(aq) - aqueous (dissolved in water)

43
Q

If the temperatures below the melting point it’s

A

A solid

44
Q

If the temperatures above the boiling point it’s

A

A gas

45
Q

Nanoparticles

A

Really small particles

Diameter between 1nm and 100nm

46
Q

1nm =

A

0.000 000 001m

47
Q

Calculate SA:V

A

Surface area/volume

48
Q

Thermosoftening polymer

A

Softens and melts on heating

-due to the weak intermolecular forces between the layers

49
Q

Thermosetting polymer

A

Does not soften or melt on heating

-due to strong cross links between layers

GCSE AQA Chemistry (5 decks)

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