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Chemistry Y9 > EOY Exam > Flashcards

EOY Exam Flashcards

1
Q

Ion

A

An atom that has lost or gained electrons.
* Metals loose electrons and form positive ions.
* Non metals gain electrons and form negative ions.
(And atom that has become charged)

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2
Q

Bond

A

A force of attraction that holds atoms/ions together.

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3
Q

Electrostatic force

A

The strong force of attraction between positive and negative ions.

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4
Q

Cations

A

Positive ions

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5
Q

Anions

A

Negative ions

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6
Q

Ionic bonding

A

The strong electromagnetic force of attraction between cations (+) and anions (-).

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7
Q

Atomic number

A

Number of protons / electrons

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8
Q

Atomic mass number

A

Number of neutrons and protons.

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9
Q

Ionic lattices

A

Ionic compounds are made up of ions arranged in regular structures tightly packed with a repeating pattern or alternating (+) and (-) ions.

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10
Q

No oxygen present

A

‘ide’

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11
Q

Oxygen present

A

‘ate’

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12
Q

Ammonium (ion formula)

A

NH₄⁺

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13
Q

Carbonate (ion formula)

A

CO₃²⁻

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14
Q

Sulphate (ion formula)

A

SO₄²⁻

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15
Q

Nitrate

A

NO₃4⁻

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16
Q

Fluoride

A

F⁻

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17
Q

Chloride

A

Cl⁻

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18
Q

Bromide

A

Br⁻

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19
Q

Oxide

A

O²⁻

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20
Q

Sulphide

A

S²⁻

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21
Q
A
22
Q

Phosphide

A

P3⁻

23
Q

Properties of ionic compounds
(Ionic lattice)

A
  • High melting and boiling points.
  • Not conducting electricity or heat.
  • Brittle
  • Soluble in water
24
Q

Brittle ionic lattice

A

The ionic lattice breaks when force is applied, because the arrangement of positive and negative ions changes and the positive and negative ions repel each other.

25
Q

Soluble in water
(ionic lattice)

A

(Dissolves in water)
When ionic compounds are dissolved (in solution) the ions can move and conduct electricity.

26
Q

Where do covalent bonds exist?

A

Between non-metals
e.g. C, H, O, N, S, halogens

27
Q

Covalent compounds

A

Molecular substances.
Groups of atoms:
* That don’t form lattices
* Are held together by covalent bonds.

28
Q

How are covalent bonds formed?

A

They are formed by atoms of non-metals sharing electrons from their outer shells.

29
Q

1 covalent bond =

A

= 1 pair of shared electrons

30
Q

What do group 7 form

A

The halogens form di-atomic molecules.

31
Q

What is a molecule

A

A group of atoms bonded by covalent bonds.

32
Q

Monomers

A

Simple molecules that can be joined in a chain.

33
Q

Polymer

A

A chain of repeating units, all chemically bonded.

34
Q

What are the forces between simple molecules?

A

Weak intermolecular forces of attraction.

35
Q

What are the forces between the molecules of polymer chains?

A

Many weak inter-molecular forces of attraction along the length of the molecules.

36
Q

What are the properties of simple molecules?

A
  • low melting and boiling points
  • poor conductor of electricity
  • often a gas or liquid at room temperature
37
Q

What are the properties of polymer chains?

A
  • poor conductor of electricity
  • solid at room temperature
38
Q

Why are both simple molecules and polymers poor conductors of electricity?

A

There are no charge carriers (electrons) that are free to move.

39
Q

Examples of simple molecules

A
  • CO2
  • H2O
  • CH4
  • H2
  • O2
  • Halogens
40
Q

Example of polymer

A

Plastic

41
Q

Where is the word allotropes from?

A

The Greek word for “other forms”

42
Q

What are allotropes of carbon?

A

Different arrangements of large numbers of atoms covalently bonded to each other

43
Q

What happens to carbon atoms in graphite?

A
  • They form 3 covalent bonds
  • Arranged in hexagons
  • In parallel layers
44
Q

How many bonds are there in diamonds?

A

4

45
Q

Nanotubes

A
  • Carbon atoms with 3 covalent bonds
  • they form a cylinder (tube shape)
  • resistant
  • high melting and boiling points
  • conducts electricity
46
Q

Buckminster fullerenes

A
  • carbon atoms with 3 covalent bonds
  • they form a sphere (small radius)
  • formula = C60
  • low melting and boiling point due to weak intermolecular forces
47
Q

Graphine

A

Consists of carbon atoms in a single layer forming large sheets
* one atom thick = light weight
* free (delocalised) electrons (conduct electricity)

48
Q

Properties of metals

A
  • Solids
  • Malleable
  • Good conductors of electricity
  • High density
  • High melting and boiling points
  • Shiny and grey (except copper)
49
Q

Properties of non-metals

A
  • Mainly gases
  • Brittle
  • Usually don’t conduct electricity
  • Low density
  • Low melting and boiling points
  • Dull (not shiny, colour varies)
50
Q

Metallic bonding

A

The strong electrostatic force of attraction between the positive metal ions and the negative delocalised ions.

51
Q
A

Chemistry Y9 (2 decks)

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