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Chemistry > glossary f-n > Flashcards

glossary f-n Flashcards

1
Q

fermentation

A

a natural process that uses yeast enzymes to convert glucose to ethanol and carbon dioxide

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2
Q

filtrate

A

the purified liquid that collects in a flask when a mixture is filtered.

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3
Q

filtration

A

the process of removing solids from a liquid or gas by passing the mixture through a mesh or filter.

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4
Q

first ionization energy

A

the energy required to remove one electron from an atom of an element in the gas phase

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5
Q

flame test

A

determination of the metallic elements present in a compound by inserting a sample of the compound into a non-luminous bunsen burner flame.
Some metals produce a particular colours when heated.

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6
Q

formula

A

a representation of an element or compound using symbols for its constituent elements. It shows the RATIO of atoms in a compound or the number of atoms in a molecule.

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7
Q

fractional distillation

A

A form of distillation that separates solutions of liquids according to their boiling points.

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8
Q

fuel

A

substances that have chemical energy stored with them that can be released relatively easily.

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9
Q

full equation

A

a representation of a reaction that uses the formulae of all reactants and products in a chemical reaction.

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10
Q

fullerene

A

a molecule composed entirely of carbon, in the form of a hollow sphere or tube.
Each carbon is bonded to 3 other carbon atoms

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11
Q

gas chromatography GC

A

a very sensitive form of chromatography in which the mobile phase is a gas
(inert like N Ar etc )

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12
Q

geometric isomer

A

a type of stereoisomer that can occur when there is restricted rotation of a molecule ( = bond or ring ).
cis , trans used.

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13
Q

graphene

A

a form of carbon consisting of planar sheets one atom thick in which each carbon atom is bonded to 3 neighbouring atoms.

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14
Q

graphite

A

a form of carbon in which the carbon is arranged in layers.

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15
Q

ground state

A

a term used to describe an atom in which the electrons occupy the lowest possible energy levels.

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16
Q

group

A

A vertical column of elements in the periodic table.

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17
Q

Heat capacity

A

A measure of a substance’s capacity to absorb and store heat energy.
For water heat cap = 4.18 J C-1
or 1g of water given 4.18 J of energy will inc temp by 1 degree.

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18
Q

Heat of Combustion

A

The enthalpy change that occurs when a specific amount of a fuel burns completely in oxygen

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19
Q

Heat of Reaction

A

The exchange of heat between a system and its surroundings during a chemical reaction under constant pressure.
Symbol = ^H.
Also known as enthalpy change.

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20
Q

Heat treatment

A

Heating a metal in different ways to alter its structure and physical properties.

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21
Q

Heavy metal

A

A metal with high density, usually used to describe a metal that poses a threat to health.

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22
Q

Heterogenous

A

Different. A heterogenous substance or solution possesses two or more different types of phases in the one sample e.g. a suspension

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23
Q

High performance or High Pressure Liquid Chromatography HPLC

A

A very sensitive technique used to separate the components in a mixture, to identify each component and to measure the concentrations of the components.

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24
Q

Homogenous

A

Uniform, the same throughout.
The components of a homogenous substance are uniformly distributed throughout the substance
e.g. a solution

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25
Homogenous catalyst
A catalyst that has the same physical state as the reactants and products.
26
Homologous Series
A series of compounds with similar properties and the same general formula, in which each member contains one CH2 unit more than the previous member.
27
Hydrated
An ion surrounded by water molecules. | Hydrated ions can be found in aqueous solution or crystalline solids.
28
Hydride
A compound in which hydrogen is bonded to another element. | HF, HCl, HI are hydrides of group 17 elements.
29
Hydrocarbon
A compound that contains carbon and hydrogen only. | e.g. alkanes, alkenes, alkynes
30
Hydrogen bonds
A type of inter-molecular, dipole-dipole force where a hydrogen atom is covalently bonded to a highly electronegative atom such as F, O, N. The hydrogen develops a positive charge and bonds to another lone pair.
31
Hydronium ion
The H3O+ (aq) ion.
32
hydroxide ion
the OH - ion.
33
Hypothesis
A prediction based on previous knowledge, a possible outcome of an experiment
34
Ideal gas
A gas that obeys the gas equation at all temperatures and pressures. An ideal gas is a theoretical gas in which there are no intermolecular attractive forces and the gas particles have no volume.
35
Incomplete combustion
Combustion that takes place when the oxygen supply is limited. Products are carbon monoxide or carbon and water.
36
Independent Variable
A variable that is controlled by the researcher
37
Indicator
A substance that is different colours in acid and base forms
38
Inert
not chemically reactive
39
Injection Port
Opening through which the sample is injected into the gas chromatograph.
40
Instantaneous dipole
A net dipole formed in a molecule due to temporary fluctuations in the electron density in the molecule.
41
Intermolecular Force
An electrostatic force of attraction between molecules | including dipole-dipole, hydrogen bonding and dispersion forces.
42
intramolecular bond
A force that holds the atoms within a molecule together.
43
ion
A positively or negatively charged atom or group of atoms.
44
ion-dipole attraction
The attraction that forms between dissociated ions and polar water molecules when an ionic solid dissolves in water.
45
ionic bonding
A type of chemical bonding that involves the electrostatic attraction between oppositely charged ions.
46
ionic compound
A type of chemical compound that involves the electrostatic attraction between oppositely charged ions.
47
Ionic equation
An equation for a reaction that shows only the species that are involved in the reaction
48
Ionisation
i) The removal of one or more electrons from an atom or ion. | ii) The reaction of a molecular substance with a solvent to form ions in solution.
49
Ionisation energy
The energy required to remove ONE electron from an atom of an element in the gas phase.
50
Isotope
Each of the two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons in their nucleii. e.g. C12 C13 C14
51
Kinetic energy
The energy that a particle has due to its motion.
52
kinetic energy distribution diagram
Maxwell Boltzmann distribution graph A graph showing the range of kinetic energy of particles in a sample.
53
Kinetic Molecular Theory
A theory that aims to explain the behavior of gases by assuming gases are composed of larger number of particles in random motion, these particles move in straight lines and have elastic collisions, the gas particles are very small. There is no attraction between the particles. The temperature is related to the average kinetic energy.
54
Latent heat
The heat energy required to change the state of a substance at a constant temperature.
55
Latent Heat of Fusion
The energy required to change a fixed amount of solid to liquid at its melting temperature.
56
Latent heat of Vaporisation
The energy required to change a fixed amount of liquid to a gas at its boiling temperature.
57
Lattice
A regular arrangement of large numbers of atoms, ions or molecules.
58
Law of conservation of energy
A scientific law that states energy cannot be created or destroyed, it can only be transformed from one type of energy to another.
59
Lewis structure diagram
A representation of the electron arrangement in a molecule in which outer-shell electrons are represented by dots or crosses, also called electron dot diagrams.
60
Limewater test
A test for carbon dioxide gas. | Bubble gas through limewater - calcium hydroxide. CO2 turns it milky.
61
Limiting reagent
A reactant that is completely consumed in a reaction and which determines the amount of products formed
62
Lone electron pair
An outer-shell electron pair that does not form a bond with other atoms
63
Main group element
An element in group 1,2 or 13-18 in the periodic table
64
Malleable
Able to be bent or beaten into sheets
65
Mass Number
The number of protons and neutrons in the nucleus of an atom.
66
Material
a substance that can be used to make objects
67
Mass spectrum
A graph of the isotopic mass (relative to c12) against the relative abundance of each isotope in the sample.
68
Matter
Anything that has mass and takes up space
69
Maxwell-Boltzmann distribution graph
A graph showing the range of kinetic energies of particles in a sample, also called a kinetic energy distribution diagram
70
Metallic bonding
The electrostatic attractive forces between delocalised valence electrons and positively charged metal ions.
71
Metallic character
Describes how closely an element exhibits the properties commonly associated with metals, namely, that it readily loses an electron to form a cation. This is closely related to ionisation energy
72
Metallic lattice
Tightly packed arrangement of metal atoms in a "sea" of electrons.
73
Metalloid
An element that displays both metallic and non-metallic properties, e.g. germanium, silicon, arsenic, tellurium
74
Mineral
A naturally occurring inorganic substance that is solid and can be represented as a chemical formula.
75
Miscible
Liquids that can be mixed in any ratio to form a homologous solution.
76
Mobile Phase
The phase that moves over the stationary phase in a chromatographic separation.
77
Molar mass
The mass of one mole of a substance measured in g/mol (M)
78
Molarity
The amount of solute, in moles, dissolved in one litre of solution.
79
Molar volume
The volume occupied by one mole of gas at a specified set of conditions. At STP the molar volume of a gas is 22.7 L /mol
80
mole
The amount of a substance that contains the same number of fundamental particles as there are atoms in 12 g of carbon - 12
81
Mole ratio
The ratio of a species involved in a chemical reaction, based on the ratio of their coefficients in the reaction equation.
82
Molecular formula
A formula of a compound that gives the actual number and type of atoms present in a molecule.
83
Molecule
A group of two or more atoms covalently bonded together.
84
Molten
materials that are normally solids but are liquid, melted due to increased temperature.
85
Monoprotic acid
An acid molecule that generates only one hydrogen ion when ionized in water

Chemistry (15 decks)

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