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VCE Chemistry 1&2 > Glossary > Flashcards

Glossary Flashcards

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1
Q

absolute zero

A

273C or 0 K. Molecules and atoms have minimum kinetic energy at this temperature.

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2
Q

acid

A

Substance capable of donating a hydrogen ion (proton).

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3
Q

acid rain

A

Rainwater that has reacted with acidic emissions from industry and has a pH less than 5.5.

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4
Q

acidic oxide

A

an oxide generally of a nonmetal that either reacts with water to form an acid or reacts with a base. acidic solution An aqueous solution in which [H+] > [OH]. At 25C the pH

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5
Q

actinides

A

The set of elements with atomic number between 90 and 103 in which the 5fsubshell is progressively filled.

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6
Q

addition reaction

A

A reaction in which a molecule binds to an unsaturated hydrocarbon forming a single carbontocarbon bond. In this process two reactant molecules become one.

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7
Q

aliquot

A

A volume of liquid measured by a pipette. alkali A soluble base.

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8
Q

alkali metals

A

Group 1 metals.

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9
Q

alkanes

A

Hydrocarbons with only single bonds between carbon atoms; general formula CnH2n+2.

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10
Q

alkenes

A

Hydrocarbons with one double bond between two carbon atoms; general formula CnH2n.

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11
Q

alkyl group

A

A group obtained by removing a hydrogen atom from an alkane with general formula CnH2n+1 e.g. methyl (CH3).

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12
Q

allotropes

A

Different physical forms of the same element.

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13
Q

alloy

A

A substance formed when other materials (e.g. carbon other metals) are mixed with a metal.

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14
Q

alpha particle

A

A 42He nucleus emitted from the nucleus of an atom during radioactive decay.

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15
Q

amorphous

A

Without structure.

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16
Q

amount of substance

A

A measure used by chemists for counting particles; the unit is the mole.

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17
Q

amphiprotic

A

The ability to act as an acid or a base.

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18
Q

anion

A

A negatively charged ion.

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19
Q

annealing

A

Heating a metal to a moderate temperature and then allowing it to cool slowly to make it softer and more ductile.

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20
Q

anode

A

An electrode at which an oxidation reaction occurs.

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21
Q

atom

A

The smallest part of an element that can take part in a chemical reaction.

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22
Q

atom economy

A

A method of tracking the atoms in a reaction equation to calculate the mass of the atoms of reactants actually used to form product as a percentage of the total mass of reactants.

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23
Q

atomic number

A

The number of protons in the nucleus of an atom.

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24
Q

atomic radius

A

Half the distance between the nuclei in a molecule consisting of identical atoms.

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25
Q

Avogadros number (NA)

A
  • NA the number of particles in a mole;
  • NA = 6.023 1023 mol1.
  • NA is the number of elementary particles (atoms) in exactly 12 g of carbon-12. is number is equal to 6.02 × 1023.
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26
Q

Avogadros law

A

At the same temperature and pressure equal volumes of all gases contain the same number of molecules.

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27
Q

base

A

A substance capable of accepting a hydrogen ion (proton).

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28
Q

basic oxide

A

An oxide of a metal which either reacts with water to form hydroxide ions or reacts with H3O+ ions.

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29
Q

basic solution

A

A solution where [H3O+] 7.

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30
Q

biosphere

A

That part of the Earths environment that supports life.

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31
Q

bonding electrons

A

Outershell electrons involved in covalent bonding.

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32
Q

Boyles law

A

P V1 at constant temperature.

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33
Q

brittle

A

Shatters when given a sharp tap.

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34
Q

BrnstedLowry theory

A

A theory that defines an acid as a proton (hydrogen ion) donor and a base as a proton acceptor.

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35
Q

carbonoxygen cycle

A

The path taken by carbon and oxygen atoms as they react to form new compounds and move around the biosphere.

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36
Q

catalyst

A

A substance that increases the rate of a reaction but are not consumed in the reaction. cathode An electrode at which a reduction reaction occurs.

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37
Q

cation

A

A positively charged ion.

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38
Q

Charles law

A

V T at constant pressure.

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39
Q

chlorination

A

Reaction with chlorine.

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40
Q

chlorofluorocarbons

A

Synthetic compounds containing chlorine fluorine and carbon atoms e.g. CF2Cl2.

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41
Q

colloids

A

Very small particles spread throughout a liquid solid or gas. These particles are bigger than single molecules but so small that they do not settle on standing.

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42
Q

combined gas equation

A

P1V1 = P2V2 n1T1 n2T2

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43
Q

combustion

A

Reaction with oxygen.

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44
Q

compound

A

A pure substance composed of atoms of two or more elements which have chemically combined in fixed proportions.

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45
Q

concentration

A

A measure of the amount of solute dissolved in a given quantity of solvent or solution.

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46
Q

conductivity of electricity

A

Allows an electric current to pass through.

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47
Q

conjugate acid

A

The conjugate acid of a base contains one more hydrogen ion (proton) than the base.

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48
Q

conjugate base

A

The conjugate base of an acid contains one less hydrogen ion (proton) than the acid.

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49
Q

conservation of mass

A

see law of conservation of mass.

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50
Q

core charge

A

the attraction felt by the outershell electrons to the nuclear charge. Core charge can be calculated as atomic number all electrons except those in the outer shell.

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51
Q

corrosion

A

The reaction of a metal with oxygen and other substances in its environment.

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52
Q

covalency

A

The number of electrons an element shares in a covalent molecular compound.

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53
Q

covalent bond

A

The force of attraction formed when one or more pairs of electrons are shared between two nuclei.

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54
Q

covalent layer lattice

A

A twodimensional array of atoms held together by covalent bonds. Weak forces operate between the layers.

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55
Q

covalent molecular lattice

A

An arrangement of molecules into a lattice; the attractive forces between the molecules are weak. covalent network lattice An arrangement of atoms into a lattice in which there are strong covalent bonds between the atoms in all three dimensions.

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56
Q

crosslinks

A

Covalent links between polymer chains. The extent of crosslinking varies depending on use.

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57
Q

crystalline solid

A

A solid with a regular arrangement of particles.

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58
Q

crystallisation

A

Some solute comes out of solution to form crystals.

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59
Q

customised

A

Manufactured with specific properties to meet a need.

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60
Q

dblock

A

A block of elements in the periodic table known as the transition metals; the atoms of these metals have outershell electron configurations of d1s2 to d10s2.

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61
Q

decomposition

A

The breaking down of a compound to form two or more other compounds or elements.

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62
Q

delocalised electrons

A

Electrons that are not restricted to a region between two atoms.

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63
Q

desalination

A

The removal of salts from seawater to obtain fresh water.

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64
Q

dilute

A

A dilute solution is one in which the ratio of amount of solute to solvent or solution is low. dilution The addition of solvent to a solution to reduce its concentration.

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65
Q

dipole

A

A molecule that has two oppositely charged poles or ends.

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66
Q

dipoledipole interaction

A

Attractions between dipoles.

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67
Q

diprotic

A

A diprotic acid is capable of donating two hydrogen ions (protons); e.g. H2SO4.

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68
Q

dispersion force

A

The attraction that exists between molecules because of the instantaneous dipoles that form as electrons move randomly.

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69
Q

displacement

A

A process in which one substance replaces another.

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70
Q

dissociation

A

The separation of positive and negative ions as an ionic lattice melts or dissolves.

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71
Q

distillation

A

The separation of a liquid from a solid or other liquid by heating to cause evaporation followed by cooling to cause condensation.

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72
Q

dry ice

A

Solid carbon dioxide.

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73
Q

ductile

A

Able to be drawn into a thread.

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74
Q

elastic

A

Able to be stretched and then return to original shape when stretching force is removed.

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75
Q

elastomer

A

A material that returns to its original position after contraction or expansion.

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76
Q

electrochemical cell

A

A device that converts chemical energy into electrical energy.

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77
Q

electrochemical series

A

A list of chemical species arranged in order of their strength as oxidants.

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78
Q

electrolytic conductor or electrolyte

A

A solution or molten substance that conducts electricity by means of the movement of

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79
Q

electronegativity

A

The ability of an atom that is bonded to another atom to attract the bonding electrons towards itself.

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80
Q

electrovalency

A

The charge on an ion.

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81
Q

element

A

A substance composed of atoms with the same atomic number.

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82
Q

emission spectrum

A

A set of coloured lines on a black background obtained when light emitted by excited electrons as they move to a lower energy state is passed through a prism in a spectroscope.

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83
Q

empirical formula

A

A formula of a compound that shows the elements present and their ratio.

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84
Q

enhanced greenhouse effect

A

An increase in the temperature of the atmosphere due to an increased concentration of greenhouse gases such as carbon dioxide and water vapour.

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85
Q

equivalence point

A

The point in a titration when the reactants have reacted in their correct mole ratios.

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86
Q

excess reagent

A

Reagent that is present in an amount greater than that required in a reaction.

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87
Q

excited state

A

The state of an atom ion; etc. in which one or more electrons have absorbed energy and are not in their lowest energy levels.

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88
Q

fblock

A

A block of metallic elements in the periodic table; known as the lanthanides and actinides; in which the 4f and 5fsubshells are progressively being filled.

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89
Q

fermentation

A

The conversion of sugar solutions; in the presence of yeast to form ethanol and carbon dioxide.

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90
Q

filtrate

A

The liquid that passes through a filter.

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91
Q

first ionisation energy

A

The minimum amount of energy that is required to remove the highest energy electron from an atom; in the gaseous state.

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92
Q

flocculation

A

Small suspended particles come together to form larger heavier particles which are usually insoluble.

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93
Q

fossil fuels

A

Coal oil and natural gas; fuels derived from the remains of animal and plant matter.

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94
Q

fractional distillation

A

The separation of a mixture into different fractions; each containing a number of gases with similar boiling temperatures.

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95
Q

galvanic cell

A

A device that converts chemical energy into electrical energy.

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96
Q

galvanometer

A

A device used to detect the movement of charge.

97
Q

general gas equation

A

The equation that describes the behaviour of a gas: pV = nRT.

98
Q

global warming

A

The gradual increase of Earths temperature.

99
Q

green chemistry

A

A set of principles and practices that aim to reduce generation and use of hazardous materials in chemical products.

100
Q

greenhouse effect

A

A warming of the Earths atmosphere due to the absorption of infrared radiation by gases such as carbon dioxide and water vapour.

101
Q

greenhouse gases

A

Gases which are able to absorb infrared radiation coming from the Earths surface; e.g. carbon dioxide and methane.

102
Q

ground state

A

A term used to describe atoms in which the electrons are in their lowest possible energy levels. group A vertical column of elements in the periodic table.

103
Q

haemoglobin

A

A protein in blood that transports oxygen around the body to the cells.

104
Q

half equation

A

An equation involving either an oxidation or a reduction process. The electrons lost or gained in this process are shown in the equation.

105
Q

halogens

A

Elements of group 17 of the periodic table.

106
Q

halons

A

Synthetic compounds containing chlorine bromine and carbon atoms.

107
Q

homologous series

A

A series of organic compounds with similar chemical properties (same functional group) and in which each member differs by a CH2 group from the previous member.

108
Q

hydrated ions

A

Ions surrounded by water molecules in aqueous solution or crystalline solids.

109
Q

hydrocarbon

A

A compound of carbon and hydrogen.

110
Q

hydrogen bond

A

A strong dipoledipole attraction that forms between molecules in which hydrogen is bonded to one of the electronegative elements nitrogen oxygen and fluorine.

111
Q

hydronium ion

A

The H3O+ ion.

112
Q

hydrophilic

A

Waterloving substances; i.e. they are attracted to water.

113
Q

hydrophobic

A

Waterfearing substances; their attraction to water molecules is too weak for them to dissolve.

114
Q

ideal gas

A

A gas that obeys the general gas equation at all temperatures and pressures.

115
Q

impressed current

A

A lowvoltage power supply that is used to force electrons on to an electrode to ensure that a reduction reaction occurs at its surface.

116
Q

indicator

A

A substance that has different colours in its acid and base forms.

117
Q

interstitial alloy

A

Alloy made by adding smaller atoms to a metal.

118
Q

ion

A

A positively or negatively charged atom or group of atoms.

119
Q

iondipole attraction

A

The force of attraction between an ion and a polar molecule.

120
Q

ion exchange

A

A process in which ions are removed from a solution by adsorption onto the surface of a resin. The resin releases other ions (usually H+ or OH) into the solution in exchange.

121
Q

ionic bond

A

The electrostatic attraction between oppositely charged ions.

122
Q

ionic equation

A

An equation that includes only the ions involved in the reaction.

123
Q

ionic product of water

A

The product of the hydrogen ion concentration and hydroxide ion concentration.

124
Q

ionisation

A

(i) The reaction of a molecular substance with a solvent to form ions in solution; (ii) the removal of one or more electrons from an atom or ion.

125
Q

ionisation energy

A

The minimum amount of energy that is required to remove an electron from an atom or ion, in the gaseous state.

126
Q

isomers (structural isomers)

A

Molecules with the same molecular formula but different structures. isotope An atom with a specific atomic and mass number.

127
Q

isotopes

A

Atoms with the same atomic number but different mass numbers.

128
Q

kelvin scale

A

The absolute temperature scale (K = oC + 273).

129
Q

kinetic energy

A

The energy that a particle or body has because of its motion.

130
Q

lanthanides

A

The set of elements with atomic numbers between 58 and 71, in which the 4fsubshells are progressively being filled.

131
Q

latent heat

A

The energy needed to change the state of a substance at its melting or boiling temperature.

132
Q

latent heat of fusion

A

The energy required to change a fixed amount of solid to liquid at its melting temperature.

133
Q

latent heat of vaporisation

A

The energy required to change a fixed amount of liquid to a gas at its boiling temperature.

134
Q

lattice

A

A regular arrangement of large numbers of atoms, ions or molecules.

135
Q

law of conservation of mass

A

During a chemical reaction the total mass of the reactants is equal to the total mass of the products.

136
Q

limiting reagent

A

The reagent in a chemical reaction that determines the amounts of products formed. lone pair A pair of outershell or valence electrons that is not involved in bonding.

137
Q

main group elements

A

Elements in groups 1, 2 and 1318.

138
Q

malleable

A

Able to be bent or beaten into sheets.

139
Q

mass number

A

The number of protons and neutrons in the nucleus of an atom.

140
Q

mass spectrometer

A

An instrument designed to measure the masstocharge ratio of particles.

141
Q

mass spectrum

A

A plot of the isotopic mass, relative to 12C, against the relative abundance of each isotope present in a sample.

142
Q

metalloids

A

Elements, such as germanium, silicon, arsenic and tellurium, that display both metallic and nonmetallic properties.

143
Q

molar mass

A

The mass of a mole of a substance, measured in g mol1.

144
Q

molar volume

A

The volume occupied by 1 mole of gas at a specified set of conditions. At SLC, the molar volume of gases is 24.5 L mol1.

145
Q

molarity

A

The amount of solute (mole) dissolved in 1 litre of solution.

146
Q

mole

A

The amount of substance that contains the same number of fundamental particles as there are atoms in 12 g of 126C; symbol n.

147
Q

mole ratio

A

The ratio of moles of one substance to moles of another substance in a chemical equation.

148
Q

molecular formula

A

Indicates the actual number of atoms of each element in a molecule.

149
Q

molecule

A

Two or more atoms held together by covalent bonds.

150
Q

monomer

A

A compound made up of small molecules that are able to bond to form longchain molecules.

151
Q

monoprotic

A

An acid capable of donating only one hydrogen ion (proton).nanoparticle Extremely small particles that have a diameter ranging typically from 1 nm (109 m) to about 100 nm.

152
Q

nano science

A

The study of nanoparticles and their properties

153
Q

nanotechnology

A

The application of nanoscience to make useful devices.

154
Q

neutral solution

A

A solution in which the concentration of H3O+(aq) ions equals the concentration of OH(aq) ions. neutralise To react an acid with a base to form a solution of a salt and water.

155
Q

neutron

A

A neutral particle found in the nucleus of an atom.

156
Q

nitrogenfixing bacteria

A

Bacteria that are able to convert atmospheric nitrogen into nitrate and ammonium ions. They are usually found in the nodules that are present in the roots of legumes, such as peas, beans, clover and lucerne.

157
Q

nitrogenoxygen cycle

A

The path taken by nitrogen and oxygen atoms as they react to form new compounds and move around the biosphere.

158
Q

noble gas

A

The unreactive gaseous elements of group 18 of the periodic table.

159
Q

nonbonding electrons

A

Outer shell or valence electrons which are not involved in bonding; also called lone pairs. nucleus The small, very dense centre of an atom, composed of protons and neutrons.

160
Q

octet

A

Group of eight.

161
Q

orbit

A

The path that an electron was thought to take as it moved around the nucleus.

162
Q

orbital

A

Regions of space in which electrons move. carbonates.

163
Q

oxidant

A

A substance that causes another substance to undergo an oxidation reaction; an oxidant accepts one or more electrons from the substance it oxidises.

164
Q

oxidation

A

A reaction in which a substance loses one or more electrons or undergoes an increase in oxidation number.

165
Q

oxidation number

A

Numbers that are assigned to elements to determine if a reaction can be classified as a redox reaction. Although they have no physical meaning, the numbers are assigned on the basis of a set of rules that assumes that all covalent bonds, except those between like atoms, are polar.

166
Q

oxidised

A

When a substance has lost one or more electrons.

167
Q

ozone layer

A

A region in the stratosphere, 1030 km above the Earths surface, with a higher concentration of ozone than other regions of the atmosphere.

168
Q

partial pressure

A

The pressure exerted by one component of a mixture of gases.

169
Q

Pauli exclusion principle

A

The principle that states that an atomic orbital can hold 0, 1 or 2 electrons.

170
Q

pblock

A

The block containing the groups 1318 elements in the periodic table, which has atoms with outershell electron configurations of s2p1 to s2p6.

171
Q

percentage by mass of an element

A

The mass of individual elements in a compound expressed as a percentage of the mass of the compound.

172
Q

period

A

A horizontal row of elements in the periodic table.

173
Q

periodic law

A

The properties of elements vary periodically with their atomic number.

174
Q

periodic table

A

An arrangement of elements in order of increasing atomic number; the start of a new period corresponds to the outer electron of that element beginning a new shell.

175
Q

pH

A

A measure of acidity; pH = log10[H3O+(aq)].

176
Q

photochemical smog

A

Air pollution produced through the action of sunlight on oxides of nitrogen and unburnt hydrocarbons to form ozone and other pollutants.

177
Q

photon

A

A small packet of energy that has a particular wavelength. A light beam is made up of photons.

178
Q

photosynthesis

A

The reaction that occurs in the leaves of plants between carbon dioxide and water, in the presence of sunlight and chlorophyll, to form glucose and oxygen.

179
Q

polarised bond

A

A covalent bond in which the electrons are not shared equally between the two atoms.

180
Q

polar molecule

A

A molecule that acts as a dipole; it has one or more polar covalent bonds, with the charge being distributed asymmetrically.

181
Q

polymer

A

Very large covalent molecules which are composed of repeating units, usually longchain molecules. polymerisation Reaction in which many small molecules join to form a large molecule.

182
Q

polyprotic

A

An acid capable of donating more than one hydrogen ion (proton) to a base.

183
Q

precipitate

A

A solid formed during a reaction in which two or more solutions are mixed.

184
Q

precipitation reaction

A

Reaction between substances in solution in which one of the products are insoluble. pressure The force exerted per unit area of a surface.

185
Q

propellant

A

An unreactive gas that is compressed and used to disperse liquids.

186
Q

proton

A

A positively charged particle found in the nucleus of an atom.

187
Q

quanta

A

Photons.

188
Q

quenching

A

Heating a metal to a moderate temperature and then cooling it rapidly to make it harder and more brittle.

189
Q

organic

A

Relating to organisms, living things

190
Q

organic chemistry

A

Chemistry of carboncontaining compounds with the exception of compounds such as oxides of carbon and carbonates

191
Q

redox reaction

A

A reaction that involves both oxidation and reduction.

192
Q

reductant

A

A substance that causes another substance to undergo a reduction reaction; a reductant donates one or more electrons to the substance it reduces.

193
Q

reduction

A

A reaction in which a substance gains one or more electrons or undergoes a decrease in oxidation number.

194
Q

relative atomic mass

A

The weighted mean of the relative isotopic masses of an element on the scale where 12C is 12 exactly; symbol Ar.

195
Q

relative formula mass

A

The mass of a formula unit relative to the mass of an atom of 12C taken as 12 units exactly. It is numerically equal to the sum of the relative atomic masses of the atoms making up the formula.

196
Q

relative isotopic mass

A

The mass of an atom of the isotope relative to the mass of an atom of 12C taken as 12 units exactly. relative molecular mass The mass of a molecule relative to the mass of an atom of 12C taken as 12 units exactly. It is numerically equal to the sum of the relative atomic masses of the atoms making up the molecule.

197
Q

renewable energy sources

A

Sources of energy that do not use finite resources, e.g. wind power.

198
Q

respiration

A

A biological process in which nutrients are broken down to simpler molecules with the release of energy.

199
Q

reverse osmosis

A

A process by which pure water can be obtained from salt water. Pressure is applied to the salt water, causing a net flow of water molecules away from the solution through a semipermeable membrane.

200
Q

sacrificial protection

A

Protecting a metal from corrosion by coating it with a more reactive metal that will be preferentially oxidised.

201
Q

salinity

A

The presence of levels of salt in water and soil that can damage plants or inhibit their growth.

202
Q

salt

A

A substance formed from a metal (or ammonium) cation and an anion.

203
Q

salt bridge

A

Part of the internal circuit of an electrochemical cell; it allows anions to migrate to the half cell that contains the anode, and cations to migrate to the half cell that contains the cathode.

204
Q

saturated

A

Carbonbased compounds containing only single bonds between carbon atoms.

205
Q

saturated solution

A

A solution that cannot dissolve any more solute at the given temperature.

206
Q

sblock

A

The block of groups 1 and 2 elements in the periodic table, which has atoms with outershell electron configurations of s1 or s2.

207
Q

semistructural formula

A

A formula that summarises the structural formula without giving the arrangement of atoms in space. shell A region in which a group of electrons of similar energies moves around the nucleus.

208
Q

solubility

A

A measure of the amount of solute dissolved in a given amount of solvent or solution, at a given temperature. solubility curve A plot of solubility versus temperature for a particular solute dissolved in a particular solvent.

209
Q

solute

A

A substance that dissolves in a solvent, e.g. sugar.

210
Q

solution

A

A homogeneous mixture of a solute dissolved in a solvent.

211
Q

solvent

A

A substance, usually a liquid, which is able to dissolve a solute, e.g. water.

212
Q

specific heat capacity

A

The amount of energy required to raise the temperature of an amount of substance, usually 1 gram, by 1C.

213
Q

spectator ions

A

Ions that remain in a solution and are unchanged in the course of a reaction. Spectator ions are not included in ionic equations.

214
Q

standard laboratory conditions (SLC)

A

Defined as 25oC (or 298 K) and 101.3 kPa pressure.

215
Q

standard temperature and pressure (STP)

A

Defined as 0oC (or 273 K) and 101.3 kPa pressure. standard solution A solution of known concentration.

216
Q

stratosphere

A

A region in the atmosphere beyond the troposphere where the temperature ranges from 25C to 25C.

217
Q

strong acid

A

An acid that readily donates a hydrogen ion (proton) to water acting as a base.

218
Q

strong base

A

A base that readily accepts a hydrogen ion (proton) from water acting as an acid.

219
Q

structural formula

A

A formula that represents the threedimensional arrangement of atoms in a molecule.

220
Q

sublimation

A

A process by which a substance goes directly from the solid phase to the gaseous phase without passing through a liquid phase.

221
Q

substitutional alloy

A

Alloy made from elements of similar chemical properties and size.

222
Q

supercritical fluid

A

A vapour which is heated above a certain critical temperature so that it cannot be liquefied no matter what pressure is applied. It has properties similar to those of gases in that it expands to fill any available space but it also has properties similar to those of liquids and can be used as a solvent.

223
Q

supersaturated solution

A

An unstable solution that has more solute dissolved at that temperature than a saturated solution. surface energy The energy required to increase the surface area by a unit amount.

224
Q

surface/interface

A

The boundary between two substances.

225
Q

surface tension

A

The resistance of a liquid to increase its surface area.

226
Q

tempering

A

After a metal has been quenched it is warmed again to a lower temperature to reduce its brittleness but to retain its hardness.

227
Q

thermoplastic polymer

A

A polymer that will soften and can be moulded when heated but will become harder again when cooled.

228
Q

titre

A

The volume of liquid, measured by a burette, used in a titration.

229
Q

transition metals

A

The dblock of elements in the periodic table, which has atoms with outershell electron configurations of d1s2 to d10s2.

230
Q

triprotic

A

An acid capable of donating three hydrogen ions (protons) to a base.

231
Q

troposphere

A

A region in the inner atmosphere where the temperature ranges from 25C to 25C.

232
Q

ultraviolet radiation

A

A form of highenergy radiation coming from the sun.

233
Q

unsaturated

A

Carbonbased compounds containing double or triple bonds between carbon atoms.

234
Q

unsaturated solution

A

A solution that contains less solute dissolved at that temperature than a saturated solution.

235
Q

valence structure

A

A formula that depicts the shape of a molecule and in which lines are used to represent pairs of electrons. volume The amount of space that a substance occupies.

236
Q

volumetric analysis

A

Analysis using measurement of volumes, e.g. titration.

237
Q

water cycle

A

Continual cycling of solid, liquid and gaseous water in the biosphere.

238
Q

weak acid

A

An acid that donates protons to a limited extent when water is the base.

239
Q

weak base

A

A base that accepts hydrogen ions to a limited extent when water is the acid.

VCE Chemistry 1&2 (20 decks)

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