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GCSE AQA Chemistry > Topic 2- Bonding > Flashcards

Topic 2- Bonding Flashcards

1
Q

Define Ion

A

Charged particles of either single atoms or a group of atoms

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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)

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3
Q

When metals form ions they?

A

Lose electrons to form positive ions

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4
Q

When non-metals form ions they?

A

Gain electrons to form negative ions

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5
Q

The charge on the ion =

A

Number of electrons lost or gained

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

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6
Q

Ionic Bonding

A

A metal and a non-metal transferring electrons

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7
Q

Oppositely charged ions are…

A

Strongly attracted to eachother by electrostatic forces

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8
Q

Group 1 and 2 metals (ionic bonding)

A

Lose electrons to form positive ions(cations)

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9
Q

Group 6 and 7 elements… (ionic bonding)

A

Gain electrons to form negative ions (anions)

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10
Q

Ionic compounds are arranged in…

A

Giant Ionic Lattice

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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

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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

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13
Q

Calculate Empirical Formula from ions

A

Ensure total ionic charge is zero

Eg. Ca2+ + Cl- > CaCl2

2+ + (2)- > 0

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14
Q

Covalent Bonding

A

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

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15
Q

Why are Covalent Bonds strong?

A

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

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16
Q

Where are the electrons in covalent bonding shared?

A

In the outer shell where there are the highest energy levels

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17
Q

Why do atoms make covalent bonds

A

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

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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
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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

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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
Properties of polymers
- intermolecular forces larger than of simple covalent molecules, solid at room temp - weaker than of covalent bonds, lower melting and boiling points
26
Giant Covalent Structures
All atoms bonded by covalent bonds
27
Properties of a Giant Covalent Structure
-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
Diamond
Each carbon atom forms four covalent bonds in a rigid giant covalent structure
29
Graphite
Each carbon atom forms three covalent bonds to create layers of hexagons. Each carbon atom has one delocalised electron
30
Properties of Diamond
-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
Properties of Graphite
``` -soft (Weak intermolecular forces between layers) -high melting point (Lots of energy to break cb) -conducts electrical and thermal energy (One delocalised electron) ```
32
Graphene
A sheet of carbon atoms joined together in hexagons, one atom thick
33
Properties of Graphene
``` -strong (Held together by cb) -light (One atoms thick) -conducts electricity (Has one delocalised electron) ```
34
Fullerenes
Molecules of carbon shaped like closed tubes or hollow balls. They’re made up of carbon atoms arranged in hexagons, pentagons or heptagons
35
Uses of Fullerenes
Can be used to deliver drugs Can be used as industrial catalysts Can be used as a lubricant Can form nanotubes
36
Metallic Bonding
Strong forces of electrostatic attraction hold positive metal ions with the shared negative electrons in a regular structure
37
Properties of Metals
``` -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
Solids > Liquids
particles gain energy, vibrate more which weakens forces and eventually have enough energy to break free from positions into a liquid
39
Liquid > Gas
Particles gain more energy, move faster which weakens bonds until eventually they have enough energy to break their bonds
40
Gas > Liquid
As gas cools, particles don’t have enough energy to overcome forces of attraction between them, bonds form
41
Liquid > Solid
Particles have less energy after cooling, move less, cannot overcome forces of attraction so more bonds form until they’re held in place
42
State Symbols
(s) - solid (l) - liquid (g) - gas (aq) - aqueous (dissolved in water)
43
If the temperatures below the melting point it’s
A solid
44
If the temperatures above the boiling point it’s
A gas
45
Nanoparticles
Really small particles Diameter between 1nm and 100nm
46
1nm =
0.000 000 001m
47
Calculate SA:V
Surface area/volume
48
Thermosoftening polymer
Softens and melts on heating -due to the weak intermolecular forces between the layers
49
Thermosetting polymer
Does not soften or melt on heating -due to strong cross links between layers

GCSE AQA Chemistry (5 decks)

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