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prelim Flashcards

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1
Q

relative abundance

A

the percentage of that isotope in the naturally occurring element

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2
Q

Isotopes

A

Atoms of the one element that have different numbers of neutrons in their nuclei. Named by mass number

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3
Q

Prefixes

A 
one - mono
two - di
three - tri
four - tetra
five - pent
six - hex
seven - hept
eight - oct
nine - non
ten - dec
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4
Q

Nomenclature of Covalent Compounds

A
  1. more electronegative element last
  2. last element has suffix -ide
  3. prefix denoting number of atoms
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5
Q

Nomenclature of Ionic Compounds

A
  1. Cation first, anion second
  2. Monoatomic anions
    - suffix ide
    Polyatomic anions
    - unique names
  3. Cations
    - oxidation state for atoms that may have several
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6
Q

Non-metal properties

A
  • solid or gas at room temp
  • dull/non-lustrous
  • poor conductors
  • neither malleable nor ductile
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7
Q

Properties of Metals

A
  • solid at room temp
  • shiny, lustrous
  • good conductors of heat/electricity
  • malleable and ductile
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8
Q

Gravimetric Analysis

A
  • analysis by mass
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9
Q

Heterogenous mixture

A

composition varies throughout mixture

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10
Q

Emission Spectrum

A

when an atom has electrons in higher levels that can move down to lower levels, they emit photons with an energy based on the difference in electron levels
- as electrons move, excess energy is emitted as light

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11
Q

Ionisation Energy

A

The energy required to remove an electron and form an ion

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12
Q

Homogenous mixture

A

uniform in composition

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13
Q

physical properties - definition

A

characteristics of a substance that can be observed without changing it into a different substance

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14
Q

Flame Test colours

A 
copper - green
calcium - red
strontium - red
barium - green
potassium - purple
sodium - yellow
(cations cause colour)
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15
Q

Sulphate

A

(SO4)2-

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16
Q

Hydroxide

A

(OH)-

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17
Q

Carbonate

A

(CO3)2-

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18
Q

Sulphite

A

(SO3)2-

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19
Q

State of Matter - periodicity

A

solid to gas across a period

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20
Q

Unstable Isotopes

A

release radiation to become more stable. Atomic number >83

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21
Q

Physical properties to separate mixtures

A
  • filtration
  • solubility
  • boiling point
    • evaporation
    • distillation
  • density
    • sedimentation
    • decanting
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22
Q

Characteristics Used to identify substances

A
  • colour
  • magnetism
  • melting and boiling points
  • density
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23
Q

Nitrate

A

(NO3)-

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24
Q

Nitrite

A

(NO2)-

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25
Q

Alpha

A
  • helium nucleus
  • low penetrative ability
  • decays as there are too few neutrons to be stable
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26
Q

Detoxifying Poisonous Foods

A 
Cycad Fruit
- leaching
- fermentation
Black Beans
- heat seeds
- scrape into finer portions
- soak in water
- mash then bake
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27
Q

Leaching

A
  • grind/pound kernels
  • soak in water
  • ground then bake
  • salt sometimes used
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28
Q

Fermentation

A

Stored for months in a moist environment

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29
Q

Beta

A
  • electron
  • medium penetrative ability
  • decays as there are too many neutrons to be stable
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30
Q

Gamma

A
  • no particle is released, instead electromagnetic radiation
  • high penetrative ability
  • decays from an unstable atom releasing energy
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31
Q

Phosphate

A

(PO4)3-

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32
Q

Intermolecular forces

A

forces that act between molecules

  • dipole-dipole
  • dispersion
  • hydrogen bonding
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33
Q

Intramolecular forces

A
  • forces that act within the molecule
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34
Q

ionic bonding

A
  • atoms exchange electrons to achieve noble gas configuration
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35
Q

covalent bonding

A

atoms share electrons to gain noble gas configuration

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36
Q

ionic substance properties

A
  • solids at room temp
  • high melting and boiling points
  • hard and brittle
  • don’t conduct electricity as solids
  • when molten or in aqueous solution, they do conduct electricity
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37
Q

Covalent molecular substance properties

A
  • generally gases or liquid at room temp
  • low melting and boiling points
  • soft as solids
  • pure covalent don’t conduct electricity
  • in aqueous solution do conduct electricity
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38
Q

why do ionic substances have those properties?

A
  • much energy is needed to break up electrostatic forces between ions
  • ions are tightly bound and unable to move towards a charged electrode, therefore do not conduct electricity
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39
Q

why do covalent molecular substances have those properties?

A
  • bonding forces holding the atoms together within the molecule are very strong, but intermolecular forces are easily broken, hence lower boiling and melting points
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40
Q

covalent network solids

A
  • covalent bonding extends indefinitely throughout

- don’t conduct electricity except graphite

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41
Q

metallic bonding

A
  • metals all have a common structure

- 3D array of positive ions held together by a mobile ‘sea’ of delocalised electrons

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42
Q

polar covalent bonds

A

electrons are unequally shared

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43
Q

dipole-dipole forces

A

the attractive electrostatic forces between polar molecules

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44
Q

dispersion forces

A

weak intermolecular forces that arise from electrostatic attractions between instantaneous dipoles in neighbouring molecules

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45
Q

hydrogen bonding

A

type of intermolecular force that involves a hydrogen atom bonded to an O, N or F atom in one molecule becoming attached to an O, N or F atom in a different molecule

46
Q

Strength of bonds

A
  1. intramolecular forces
  2. hydrogen bonding
  3. dipole-dipole+dispersion
  4. dispersion
47
Q

allotropes

A

forms of one element that have distinctly different physical properties

48
Q

law of conservation of mass

A

matter cannot be created or destroyed, but merely changed from one form to another

49
Q

relative atomic mass

A

average mass of the atoms present in the naturally occurring element, relative to the mass of an atom of the carbon-12 isotope

50
Q

mole

A

the amount of a substance that contains exactly 6.022x10^23 atoms, molecules or ions

51
Q

converting between mass and moles

A

n=m/MM

52
Q

moles to number of atoms or molecules

A

N=nxNA

53
Q

percentage composition in a compound

A

%A in a compound = mass of A in one mole of compound/mass of one mole of compound

54
Q

calculating formulae from experimental data

A
  1. write down masses of all present elements
  2. convert masses to moles
  3. divide by smallest number of moles to get simple ratio
55
Q

limiting reagent calculations

A

compare quantities to determine which is in short supply

56
Q

accuracy of measuring equipment

A
  • measuring cylinders +- 5%
  • pipettes and burettes +- 0.2 to 0.5%
  • volumetric flasks +- 0.2 to 0.5%
57
Q

concentration formula

A

c=n/v

58
Q

dilution formula

A

c2v2=c1v1

59
Q

combined gas law

A

PV=nRT

60
Q

gas law assumption 1

A

gases contain a large number of molecules in random and rapid motion, moving in a straight line until they hit the wall of a container from which they bounce off

61
Q

gas law assumption 2

A

the molecules of gas occupy a negligible volume of the container which they are in

62
Q

gas law assumption 3

A

the molecules of a gas experience no forces except when they collide with each other and the walls of the container

63
Q

Gay-Lussac’s Law

A

P1/T1=P2/T2

64
Q

Boyle’s Law

A

P1V1=P2V2

65
Q

Charles’ Law

A

V1/T1 = V2/T2

66
Q

Avogadro’s Law

A

V1/n1 = V2/n2

67
Q

indicators of a chemical change

A
  • gas is evolved
  • precipitate is formed
  • colour change
  • significant temperature change
  • solid disappears
  • an odour is produced
68
Q

synthesis reaction

A

A+B –> AB

69
Q

decomposition

A

AB –> A+B

70
Q

combustion

A

A + O2 –> H2O + CO2

71
Q

precipitation reaction

A

A + Soluble Salt B –> Precipitate + Soluble Salt C

72
Q

Acid Base reaction

A

Acid + Base –> salt + water

73
Q

acid carbonate reaction

A

acid + metal carbonate –> salt + water + carbon dioxide

74
Q

atomic radius - reactivity

A

reactivity increases as atomic radius increases

75
Q

electronegativity - reactivity

A

reactivity increases as electronegativity decreases

76
Q

oxidation

A

the loss of electrons

77
Q

reduction

A

the gain of electrons

78
Q

half equations

A

describes the oxidation and reduction processes separately in terms of electrons lost or gains

79
Q

oxidant

A
  • substance that brings about oxidation of another substance

- oxidant gets reduced

80
Q

reductant

A
  • substance that brings about reduction of another substance

- reductant gets oxidised

81
Q

oxidation numbers

A

the oxidation of an element in a molecule or ion is the charge the atom of that element would carry if the molecule or ion were completely ionic

82
Q

oxidation state - substance in elemental state

A

oxidation number of zero, regardless of the formula of the molecule

83
Q

oxidation state - monatomic ion

A

simply the charge on the ion

84
Q

oxidation state - fluorine

A

-1

85
Q

oxidation state - hydrogen

A

hydrogen has an oxidation state of +1 except where it is -1

86
Q

oxidation state - oxygen

A

oxygen has an oxidation of -2 unless the other rules dictate that it have a different value

87
Q

oxidation state - chlorine, bromine, iodine

A

-1 unless other rules require them to have a different value

88
Q

oxidation state - molecule or ion

A

the algebraic sum of the oxidation numbers of the elements in a molecule or ion must equal the net charge on the species

89
Q

increase in oxidation number

A

corresponds to oxidation

90
Q

decrease oxidation number

A

corresponds to reduction

91
Q

Galvanic cell

A

a device in which a chemical reaction (redox reaction) occurs in such a way that it generates electricity

92
Q

electrode

A

the conductor that connects the external electrical circuit to the solution of the galvanic cell (the pieces of metal)

93
Q

electrolyte

A

a substance that in solution or in the molten state conducts electricity (the solution/liquid)

94
Q

salt bridge

A

a device that provides electrical contact between solutions in a galvanic cell. allows the migration of ions between two electrolytes in a galvanic cell to maintain electrical neutrality in the cell solutions

95
Q

Reaction Spontaneity

A
  • if the overall voltage is positive the reaction is spontaneous
  • if negative, the reaction is not spontaneous
96
Q

rate of reaction

A

the rate at which reactants are used up or the rate at which products form in a chemical reaction

97
Q

factors influencing the rate of a reaction

A
  • concentration
  • temperature
  • catalyst
  • surface area
98
Q

factors influencing the rate of a reaction - temp

A

increasing temperature increases rate of reaction

99
Q

factors influencing the rate of a reaction - concentration

A

increasing the concentration increases the rate of reaction

100
Q

factors influencing the rate of a reaction - catalyst

A

a substance that increases the rate of reaction without undergoing permanent chemical change in the reaction. catalyst provides alternate lower activation energy

101
Q

factors influencing the rate of a reaction - surface area

A

increasing surface area of reactant increases rate of reaction

102
Q

Activation energy

A
  • an energy barrier between reactants and products

- the higher it is, the harder it is for reactants to get over it and form products, so the slower, the reaction is

103
Q

collision theory

A

collision theory proposes that, for a chemical reaction to occur, the reactant particles must

  • collide
  • have more than a certain minimum amount of kinetic energy
  • be correctly orientated
104
Q

Permanganate

A

(MnO4)-

105
Q

Hydrogencarbonate

A

(HCO3)-

106
Q

Dichromate

A

(Cr2O7)2-

107
Q

Chromate

A

(CrO4)2-

108
Q

Ammonium

A

(NH4)+

109
Q

Cyanide

A

(CN)-

110
Q

peroxide

A

O2 2-

111
Q

methane

A

CH4

Prelim Chemistry (1 decks)

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