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Chemistry > Glossary a-e > Flashcards

Glossary a-e Flashcards

1
Q

absorbance

A

the ability of a substance to absorb a certain wavelength of light

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2
Q

absorption line

A

The black lines found in a continuous spectrum of light

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3
Q

accuracy

A

how close to the real value a measurement is

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4
Q

acid (Arrhenius)

A

a substance that can make hydrogen ions in solution

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5
Q

acid (Bronsted-Lowry)

A

a substance that can donate a hydrogen ion (proton)

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6
Q

acid - base reaction

A
  • when and acid reacts with a base.

* may be called Neutralization when in correct proportion.

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7
Q

acid rain

A

rainwater that reacted with acidic gases in the atmosphere to make water with a pH of less than 5.5

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8
Q

acidic solution

A

a solution which has more hydrogen ions than hydroxide ions.

pH is < 7

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9
Q

acidity

A

the concentration of H+ ions in a solution.

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10
Q

What scale measured the acidity of a solution?

A

pH scale

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11
Q

activation energy

A

the minimum energy the reactants require for the reaction to occur.

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12
Q

What is the symbol for activation energy?

A

Ea.

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13
Q

What is the activation energy needed for?

A

To break the bonds between atoms in the reactants

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14
Q

active site

A

the specific part of an enzyme molecule where the reactant can interact

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15
Q

addition reaction

A

a reaction in which a molecule binds to an unsaturated hydrocarbon (alkene, alkyne) to form a single carbon bond.

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16
Q

How many products are formed in an addition reaction?

A

1

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17
Q

adsorption

A

when a substance sticks to the surface of a liquid or a solid

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18
Q

alkali

A

a soluble base

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19
Q

alkali metal

A

a group 1 metal.

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20
Q

alkane

A

a saturated hydrocarbon with all single bonds

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21
Q

What is the general formula for a straight alkane

A

Cn H(2n+2)

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22
Q

alkene

A

an unsaturated hydrocarbon with a double bond between carbons.

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23
Q

alkyl group

A

a hyrdocarbon group on main carbon chain

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24
Q

alkyne

A

an unsaturated hydrocarbon with a triple bond between .carbons.

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25
Q

allotrope

A

different forms of the same element in which the atoms are bonded in different ways

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26
Q

Allotropes of carbon

A

graphite, diamond

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27
Q

Allotropes of oxygen

A

oxygen gas, ozone gas.

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28
Q

alloy

A

a mixture of a metal an another substance like C or another metal/s.

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29
Q

An alloy of copper and tin

A

bronze

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30
Q

An alloy of copper and zinc

A

brass

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31
Q

An alloy of iron and carbon

A

steel

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32
Q

alpha particle

A

a positively charged particle in radiation, similar to a helium nucleus

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33
Q

amorphous

A

a substance with no consistant structure

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34
Q

anion

A

a negatively charged ion

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35
Q

annealing

A

heating a metal to a moderate temperature and letting it cool slowly. This makes the metal softer and more ductile.

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36
Q

What effect does annealing have on a metal?

A

It makes it softer and more ductile.

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37
Q

aqueous (aq)

A

A substance is dissolved in water.

i.e. water is the solvent.

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38
Q

Arrhenius model - acid

A

It defines an acid as a substance that ionizes in water to produce hydrogen ions (H+) or protons.

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39
Q

Arrhenius model - base

A

It defines a base as a substance that dissociates in water to form hydroxide OH- ions

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40
Q

artesian basin

A

an underground area of porous rock that stores water.

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41
Q

asymmetrical molecule

A

a molecule in which the polar bonds are unevenly distributed.

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42
Q

asymmetrical molecule 2

dipoles

A

the bond dipoles do not cancel and and overall dipole is created.

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43
Q

atom

A

The basic building block of matter.

Smallest particle of an element.

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44
Q

What particles make up an atom?

A

Made of protons and neutrons in the nucleus.

Surrounded by electrons in shells.

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45
Q

atomic absorption spectroscopy (AAS)

A

A technique that uses light absorption to measure the amount of metal in a sample.

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46
Q

atomic number

A

The number of protons in the nucleus of an atom.

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47
Q

What is the symbol of the atomic number?

A

Z

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48
Q

atomic radius

A

A measurement of the size of an atom, half the distance between adjacent atoms in a molecule

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49
Q

atomic theory of matter

A

states all matter is made up of atoms.

Atoms are indivisible and elements are made of identical atoms.

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50
Q

Avogadro’s Law

A

At the same temperature and pressure equal volumes of all gases contain equal numbers of particles.

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51
Q

Avogadro’s number

A

the number of particles in a mole.

6.023 x 10 23

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52
Q

bar

A

unit of pressure

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53
Q

base (Arrhenius)

A

a substance capable of producing hydroxide ions.

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54
Q

base (Bronsted-Lowry)

A

a substance capable of accepting a proton.

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55
Q

a basic solution

A

an aqueous solution with more hydroxide ions than hydrogen ions.

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56
Q

What is the pH of a basic solution?

A

pH is greater than 7

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57
Q

bias

A

values skewed in one direction from the true value.

e.g. too high or too low.

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58
Q

biodegradable

A

capable of being broken down by bacteria

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59
Q

biofuel

A

fuel made from plants such as grains, sugar or vegetable wastes and oils.

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60
Q

bohr diagram

A

a simple diagram that shows the arrangement of electrons around the nucleus.

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61
Q

Bohr Model of the Atom

A

a theory of the atom by Niels Bohr where electrons occupy fixed, circular orbits.

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62
Q

bore water

A

water that comes from underground

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63
Q

brittle

A

shatters when given a sharp tap.

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64
Q

buckyball

A

a ball like structure of carbon atoms.

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65
Q

calibrate

A

to check the scale of an instrument

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66
Q

calibration curve

A

a graph of two variables that can be used to determine the true value of one of the variables

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67
Q

carbon-12

A

the isotopes of carbon that has a mass number of 12,

6 protons and 6 neutrons.

68
Q

What is carbon - 12 used to standardize?

A

one twelfth of the mass of a carbon -12 atom is used to calculate the mass of other atoms.
It makes one atomic mass unit.

69
Q

carbon nanotube

A

a tube shaped nanoparticle made of carbon atoms

70
Q

catalyst

A

a substance that increases the rate of a reaction but is not consumed in the reaction.

71
Q

catalysis

A

the increase in the rate of a reaction due to the presence of a catalyst

72
Q

How does a catalyst work?

A

By offering a lower energy pathway with a lower activation energy.

73
Q

cation

A

a positively charged ion

74
Q

centrifugation

A

a physical separation technique which uses rapid rotation

75
Q

ceramic

A

material made by the firing of clay.

76
Q

chemical energy

A

form of energy stored in the chemical bonds between atoms and molecules.

77
Q

What makes chemical energy?

A

electrostatic forces of repulsion and attraction between the protons and electrons, movement of electrons, rotation and vibration around bonds

78
Q

chemical formula

A

a representation of a substance using symbols of the elements and showing the ratio between them

79
Q

chemical symbol

A

A symbolic representation of an element with one or two letters (usually). The first is a capital.

80
Q

chemiluminescence

A

the light emitted by a chemical reaction (does not produce a significant amount of heat)

81
Q

chlorination

A

adding chlorine to drinking water to purify it.

82
Q

chromatography

A

a way of separating a mixture with a moving phase (solvent) over a stationary phase (paper).

83
Q

collision theory

A

a theoretical model that accounts for the rates of chemical reactions in terms of collisions between particles in a chemical reaction.

84
Q

colloid

A

a mixture in which very small particles are spread throughout a liquid, solid or gas.

85
Q

how big are the particles in a colloid?

A

bigger than a molecule but small enough not to settle on standing

86
Q

column chromatography

A

chromatography technique in which the stationary phase is a column

87
Q

combustion

A

a rapid reaction with oxygen with the release of a large amount of heat.

88
Q

another name for combustion

A

burning

89
Q

complete combustion

A

only products of burning are carbon dioxide and water

90
Q

incomplete combustion

A

burning leaves other products like carbon and carbon monoxide as well as carbon dioxide and water

91
Q

components

A

chemicals in a mixture

92
Q

composite material

A

made up of two or more materials with different properties

93
Q

compounds

A

a substance made up of two or more types of atoms in a fixed ratio

94
Q

concentrated solution

A

a solution with a relatively high ratio of solute to solvent

95
Q

concentration

A

a measure of how much solute is dissolved in a specific volume of solvent ( mole per litre)

96
Q

condensed structural formula

A

a simple representation of the structural formula of an organic molecule. CH3 .CH3

97
Q

conductivity

A

permitting the flow of electric charges

98
Q

conductor

A

an object or type of material that can let electricity pass through

99
Q

control experiment

A

an experiment carried out in which the independent variable is NOT changed

100
Q

controlled variable

A

a variable that is kept constant

101
Q

core charge or effective nuclear charge

A

the effective nuclear charge experienced by the outer shell electrons in an atom.
It indicates the attractive forces felt by the valence electrons.

102
Q

covalent bond

A

the force of attraction formed when one or more pairs of electrons are shared between two nucleii

103
Q

covalent layer lattice

A

an arrangement of atoms in a lattice in which there are strong covalent bonds between the atoms that have formed in a layer

104
Q

covalent network lattice

A

an arrangement of atoms in a lattice in which there are strong covalent bonds between the atoms in all three dimensions

105
Q

cracking

A

a chemical process during which carbon-carbon bonds in alkanes are broken to form smaller molecules and some unsaturated molecules.

106
Q

credible

A

reliable and can be backed up with evidence;

a credible source provides information that one can believe to be true.

107
Q

crude oil

A

a mixture of hydrocarbons that originates from the remains of prehistoric marine micro-organisms.
These have been broken down by heat and pressure over millions of years.

108
Q

crystal

A

a solid made up of atoms or molecules arranged in a repeating 3D pattern.

109
Q

crystal lattice

A

the symmetrical 3D arrangement of atoms or ions inside a crystal.

110
Q

crystallisation

A

the process in which solid crystals are deposited when the concentration of a solute in a solution increases past the point of saturation.

111
Q

crystallise

A

form solid crystals.

112
Q

decantation

A

a separation process in which a layer of liquid is separated from the solid that has settled at the bottom of the liquid.

113
Q

decomposition

A

a reaction in which a compound is broken down into smaller parts.

114
Q

delocalise

A

spread out

115
Q

delocalised electron

A

an electron that is not restricted to the region between two atoms.

116
Q

density

A

mass per unit volume kg/m-3 or g/cm-3 or g/mL

117
Q

dependent variable

A

the variable that is measured or observed to determine the effect of changes in the independent variable

118
Q

desalinated seawater

A

fresh water made by removing salt from sea water

119
Q

desalination

A

the removal of salts from seawater to obtain fresh water

120
Q

desorption

A

the breaking of the attraction between a substance and the surface to which the substance is adsorbed.

121
Q

diamond

A

a form of pure carbon that is hardest naturally occurring substance

122
Q

diatomic molecule

A

a molecule formed from two atoms only.

123
Q

diffusion

A

all the gases in a gas mixture spread to fill the available space

124
Q

dilute solution

A

a solution that has a relatively low ratio of solute to solvent.

125
Q

dilution

A

the addition of a solvent to a solution to reduce its concentration.

126
Q

dipole

A

the separation of areas of positive and negative charge in a molecule.

127
Q

dipole-dipole force

A

a form of intermolecular force that occurs between polar molecules.

128
Q

diprotic acid

A

an acid that can ionise in water to give 2 hydrogen ions.

129
Q

discrete

A

a separate or particle

130
Q

dispersion forces

A

force of attraction between molecules due to temporary dipoles induced in the molecules.

131
Q

temporary dipoles

A

result of fluctuations (quick changes) in the electron density ( where the electrons are at any one time)

132
Q

dissociate

A

break apart

133
Q

dissociation

A

process in which molecules or ionic compound separate into atoms or ions.

134
Q

dissolution

A

the process of dissolving a solute in a solvent to form a solution.

135
Q

dissolve

A

to incorporate (mix in) a solid or gas into a liquid to form a solution.

136
Q

distillation

A

the process of separating a solution by evaporating, condensing and collecting the component of the solution with the lowest boiling point.
e.g. in a mixture of water and alcohol, the alcohol will evaporate off first.

137
Q

double covalent bond

A

a covalent bond in which 4 electrons are shared

138
Q

ductile

A

able to be drawn into a wire.

139
Q

elastic collision

A

collision between particles where kinetic energy is conserved.

140
Q

electrical conductivity

A

the degree to which a specified material or solution conducts an electric current.

141
Q

electrolyte

A

a solution or molten substance that conducts electricity by means of the movement of ions.

142
Q

electromagnetic radiation

A

a form of energy that moves through space.

e.g. vis light, radio waves, X rays.

143
Q

electromagnetic spectrum

A

all possible frequencies of electromagnetic radiation shown in order of their wavelength or frequencies.

144
Q

electron

A

a negatively charged, subatomic particle that occupies the region around the nucleus of an atom

145
Q

subatomic particle

A

a particle that makes up an atom.

e.g. electron, neutron, proton.

146
Q

electron configuration

A

means of representing the number of electrons in each shell

147
Q

electron density

A

the concentration of electrons that usually refer to the areas around an atom or molecule.

148
Q

electron dot diagram/Lewis structure

A

a representation of the electron arrangement in a molecule in which the outer-shell electrons are represented by dots or crosses.

149
Q

electron shell

A

a fixed energy level that corresponds to a circular orbit of the electrons.

150
Q

electron transfer diagram

A

a diagram that shows how electrons move from a metal atom to a non-metal to form an ion.

151
Q

electronegativity

A

the ability of an atom to attract electrons in a covalent bond toward itself.

152
Q

electrostatic attraction

A

the force of attraction between a positively charged particle and a negatively charged particle

153
Q

element

A

a substance made up of atoms with the same atomic number.

154
Q

elemental analysis

A

a process that determines the mass of each element in a sample of a compound.

155
Q

eluent

A

the solvent that carries the components and passes through a chromatography column

156
Q

emission spectrum

A

A spectrum produced when an element is excited by heat or radiation. It appears as distinct lines characteristic of the element

157
Q

empirical formula

A

a formula that shows the simplest whole number ratio of the elements in a compound.
e.g C3H6 = CH2

158
Q

endothermic

A

a reaction that absorbs energy from the surroundings

^H is positive.

159
Q

energy content

A

the chemical energy of a substance

160
Q

energy level

A

One of the different shells of an atom in which an electron can be found

161
Q

energy profile diagram

A

The energy changes that occur during the course of a reaction

162
Q

enthalpy

A

heat content
The sum of the chemical potential and kinetic energies in a substance.
Symbol ^H

163
Q

enthalpy change

A

The difference in the total enthalpy of the products and the total enthalpy of the reactants
^H
Also known as heat of reaction

164
Q

enzyme

A

biological catalyst

165
Q

excess reactant

A

a reactant that is not completely consumed in a chemical reaction

166
Q

excited state

A

a term used t describe an atom in which electrons occupy higher energy levels than the lowest possible ones

167
Q

exothermic

A

a reaction that releases energy into the surroundings.

^H is negative

Chemistry (15 decks)

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