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s4 chemistry > Definitions > Flashcards

Definitions Flashcards

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1
Q

Ion

A

Atom which has lost or gained electrons

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2
Q

isomer

A

Same molecular formula Different structural formula

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3
Q

Hydrocarbon

A

Compound containing only C and H

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4
Q

Acid

A

Solution containing a higher number of H+ aqueous ions than OH- aqueous ions

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5
Q

Molecule

A

2 or more atoms joined together by covalent bonds

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6
Q

Covalent bond

A

A shared pair of electrons

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7
Q

Isotope

A

Same atomic number Different mass number

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8
Q

Alkali

A

Solution with higher numbers of OH- aqueous ions than H+ aqueous ions

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9
Q

Atomic number

A

Number of protons in an atom

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10
Q

Fuel

A

A substance that burns to release energy

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11
Q

Combustion

A

Combining with oxygen to release energy

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12
Q

Valency

A

The number of unpaired of outer electrons

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13
Q

Element

A

Substance containing only one type of atom

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14
Q

Mass number

A

The sum of the number of protons and neutrons in an element

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15
Q

Solute

A

A substance that will dissolve in a liquid (water)

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16
Q

Diatomic

A

A molecule containing two atoms

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17
Q

What are the 7 diatomic elements

A

Iodine Hydrogen Nitrogen Bromine Oxygen Chlorine Fluorine

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18
Q

Electrolyte

A

An ionic solution used to complete an electrochemical cell

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19
Q

Exothermic

A

A reaction that releases energy

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20
Q

Endothermic

A

Reaction in which heat energy is taken in

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21
Q

What are the properties of protons

A

Charge : 1+ Mass: 1 a.m.u Found: in the nucleus

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22
Q

What are the properties of neutrons

A

Charge: 0 Mass: 1 a.m.u Found: in the nucleus

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23
Q

What are the properties of electrons

A

Charge: 1- Mass: 0 Found : in shells around nucleus

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24
Q

Period

A

Horizontal row of elements in the periodic table

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25
Q

Electricity

A

The flow of charged particles(electrons and ions)

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26
Q

Solvent

A

A liquid into which a substence will dissolve

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27
Q

Homologous series

A

Compounds with Same general formula Similar chemical properties

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28
Q

Lattice

A

A regular, repeating 3-D structure

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29
Q

Saturated

A

A substance where all C to C bonds are single

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30
Q

Unsaturated

A

A substance contains (at least) on C=C bond

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31
Q

Monomer

A

Small unsaturated molecule that takes part in addition polymerisation

32
Q

Halogen

A

Any of the group 7 elements

33
Q

Alkali metal

A

Any of the group 1 metals

34
Q

Salt

A

When the H+ aqueous ions of an acid are replaced by metal (or ammonium) ions

  1. sulphuric acid gives sulphate salts
  2. hydrochloric acid gives chloride salts
  3. nitric acid gives nitrate salts
35
Q

Neutralisation of acids

A

Removing excess H+ aqueous ions from a solution

36
Q

Base

A

A substance that neutralises an acid

37
Q

What are the 4 types of base

A

Metal Metal Hydroxide Metal Carbonate Metal Oxide

38
Q

Pollution

A

The introduction of harmful substances into the environment

39
Q

Haber Process

A

Industrial process used to manufacture ammonia

40
Q

Fertiliser

A

A soluble salt containing N, P, or K

41
Q

Spectator ion

A

An ion that doesn’t take part in a reaction Reactions of acids Displacement reactions

42
Q

Catalyst

A

A substance that increases the rate of a reaction

43
Q

What are the ideal conditions for Haber Process?

A

Temperature: around 450 degrees Pressure: 200 atmospheres Catalyst: Iron

44
Q

Indicator

A

A substance that changes colour when something is added to it

45
Q

Solution

A

A mixture of a solvent and a solute

46
Q

Electrolysis

A

Breaking apart a compound using electricity

47
Q

What is an ion bridge?

A

Used to complete the circuit

48
Q

Why are some nuclei unstable?

A

The neutron to proton ratio is outwith band of stability

49
Q

Noble gases

A

Unreactive group 8 elements

50
Q

Ion migration

A

Movement of ions to opposite charged terminal

51
Q

A mole

A

The gram formula mass of a substance

52
Q

Relative atomic mass (RAM)

A

The average mass of an element taking into account the relative abundance of each isotope

53
Q

Density

A

Mass divided by volume

54
Q

Electrostatic attraction

A

Attraction between oppositely charged particles

55
Q

Thermoplastic polymer

A

Can be reshaped upon heating

56
Q

Thermosetting polymer

A

Is decomposed upon heating

57
Q

Biodegradable

A

Broken down by the action of bacteria

58
Q

Nitrogen fixing

A

Turning nitrogen into a soluble form (nitrates!!)that plants can take in through their roots

59
Q

Acid rain

A

Rain with pH below 5.5

60
Q

Acidic oxide

A

Non metal oxide that is soluble in water

61
Q

Basic oxide

A

Metal oxide that is soluble in water

62
Q

Corrosion

A

The changing of the surface of a metal from an element into a compound

63
Q

Oxidation

A

The loss of electrons

64
Q

Reduction

A

The gain of electrons

65
Q

Functional Group

A

The part of a molecule that is responsible for its chemical (and sometimes physical) properties.

66
Q

Why are atoms neutral

A

They contain equal numbers of positive charges (protons) and negative charges (electrons)

67
Q

Qualitative Analysis

A

Used to determine what substances are present. A flame test for example

68
Q

Quantitative Analysis

A

Used to determine the quantity of a substance in a sample. A titration is used for quantitative analysis

69
Q

What are the steps in the nitrogen cycle?

A
70
Q

Eutrophication

A

Water systems enriched become by nutrients from fertliser run-off

71
Q

What are the steps in eutrophication?

A
  1. Excess nutrients from fertilisers get into water systems (lakes etc) by natural run off or rainfall
  2. High levels of nitrates cause excess algal growth.
  3. Algal growth blocks out sunlight needed by plants below water
  4. Bacteria use oxygen as they feed on dead plants
  5. Reduced O2 levels kills off marine creatures
72
Q

Nitrates and blue baby syndrome

A
73
Q

Nitrate effect on human health

A
74
Q

What are P K and N needed for and what problems can deficiency cause?

A
75
Q

Why can alkalis never have zero H+ ions present

A

Because alkalis are aqueous solutions and the dissociation of water means some H+ ions must be present

76
Q

Why can acids never have zero OH- ions present

A

Because acids are aqueous solutions and the dissociation of water means some OH- ions must be present

77
Q

Give 2 advantages of neutralising with a metal carbonate instead of a metal oxide

A
  1. Reaction rate is high enough that acid doesn’t need to be heated
  2. Easier end point detection due to evolution of CO2

s4 chemistry (26 decks)

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