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Definitions Flashcards

(74 cards)

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1
Q

Alkali

A

A chemical that reacts with an acid and is soluble in water releasing hydroxide ions, OH-.

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2
Q

Amount of substance

A

The quantity whose unit is mole. Chemists use it as a means of counting atoms.

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3
Q

Amphoteric

A

Substances that can react as both acids and bases

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4
Q

Anhydrous

A

A substance containing no water molecules

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5
Q

Anion

A

Negatively charged ion

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6
Q

Aqueous

A

A solution in which the solvent is water

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7
Q

Atomic orbital

A

A region of space where it is likely you will find electrons. Each can hold up to two electrons, with opposite spins.

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8
Q

Atomic radius

A

A measure of size of atom, usually distance from nucleus to boundary of the surrounding sea of electrons

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9
Q

Avogadros constant

A

The number of atoms pet mole of the carbon-12 isotope 6.02x10^23mol-1

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10
Q

Base

A

Chemical that reacts with acids and is a proton acceptor

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11
Q

Bond angle

A

The angle that is formed by two adjacent bonds on the same atom

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12
Q

Bonded pair

A

A pair of electrons that have been shared between two chemically bonded atoms

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13
Q

Bonding region

A

The space an electron can be found In a bond

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14
Q

Concentration

A

The amount of solute in mol dissolved per 1dm3 of a solution

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15
Q

Covalent bond

A

A bond formed by a shared pair of electrons between nuclei

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16
Q

Dative covalent bond

A

A bond formed by a shared pair of electrons that have been provided by one of the bonding atoms only.

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17
Q

Dilute

A

To add more solute without the addition of more solvent. Decreasing the concentration.

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18
Q

Dot formulae

A

Gives the ratio between the number of compound molecules and the number of water molecules within a crystalline structure.

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19
Q

Electron shielding

A

Repulsion between electrons in different inner shells. Reduces the net attraction force from the positive nucleus to the negative outer shell electrons.

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20
Q

Electronegativity

A

A measure of the attraction of an electron in a covalent bond

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21
Q

Empirical formula

A

Simplest whole number ratio of atoms of each element present in a compound

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22
Q

First ionisation energy

A

Energy required to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions.

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23
Q

Giant covalent lattice

A

3D structure of atoms that are all bonded by strong covalent bonds.

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24
Q

Giant ionic lattice

A

3D structure of oppositely charged ions, held together by strong electrostatic forces of attraction.

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25
Giant metallic lattice
3D structure of positive ions and delocalised electrons bonded together by strong metallic bonds
26
Hydrogen bond
A strong permanent dipole, between electron defficient hydrogen one one molecule and a lone pair of electrons on a highly electronegative atom on a different molecule.
27
Acid
A chemical that is a proton donor and releases H+ into solution
28
Intermolecular force
An attractive force between neighbouring molecules of atoms.
29
Ion
A positively or negatively charged atom or covalently bonded group of atoms molecular ion.
30
Ionic bond
Electrostatic attraction between oppositely charged ions.
31
Ionisation
The process of an atom becoming an ion.
32
Isotopes
Atoms of the same element with different numbers of neutrons.
33
London (dispersion) forces
Attractive forces between induced dipoles in neighbouring molecules.
34
Lone pair
An outer shell pair of electrons that is not involved in chemical bonding.
35
Mass number
The number of particles, protons and neutrons in the nucleus.
36
Mass spectrometry
An analytical chemical technique that helps identify the amount and type of chemicals present in a sample by measuring the mass to charge ratio and abundance of gas phase ions.
37
Metallic bonding
Electrostatic attraction between positive metal ions and delocalised electrons.
38
Molar gas volume
Volume per mole of a gas. Units are dm3mol-1. | At room temperature and pressure the molar gas volume is approximately 24dm3mol-1.
39
Molar mass
M | Mass per mole of a substance g mol-1.
40
Molar volume
The volume per mole of a gas. The units of molar volume are dm3mol-1. At room temperature and pressure the molar volume is approximately dm3mol-1.
41
Mole
The amount of any substance containing as many particles as there are carbon atoms in exactly 12g of carbon 12 isotope.
42
Neutralisation
The reaction of an acid with a base
43
Neutron
A particle found in the nucleus of an atom. It is almost identical in mass to a proton but has no charge.
44
Oxidation
Loss or electrons, loss of hydrogen, gain of oxygen or increase in oxidation number.
45
Oxidising agent
A reagent that oxidises (takes electrons from) another species.
46
Percentage yield
Actual amount in mol of a product divided by theoretical amount of product multiplied by 100.
47
Period
A horizontal row of elements in the periodic table.
48
Periodic table
A tabular arrangement of the chemical elements organised on the basis of their atomic number, electron configurations and recurring chemical properties.
49
Periodicity
A regular periodic variation of properties of elements with atomic number and position in the periodic table.
50
Permanent dipole
A small charge difference across a bond that results from a difference in electronegativities of the bonded atoms.
51
Permanent dipole-dipole interaction
A weak attractive force between permanent dipoles and permanent dipoles or induced dipoles in neighbouring polar molecules.
52
Polar covalent bond
A covalent bond that has a permanent dipole
53
Pressure
A measure of the force applied over a unit area
54
Principal quantum number
A number representing the relative overall energy of each orbital, which increases with distance from the nucleus. The sets of orbitals with the same n (principal quantum number) value are referred to as electron shells or energy levels.
55
Redox reaction
A reaction in which both reduction and oxidation take place.
56
Reducing agent
A reagent that reduces (adds electrons) to another species.
57
Reduction
Gain of electrons, gain of hydrogen, loss of oxygen or a decrease in oxidation number.
58
Relative atomic mass
The weighted mean mass of an atom of an element compared with one twelfth of the mass of carbon 12.
59
Relative isotopic mass
The mass of an atom of an isotope compared with 1/12th of the mass of an atom of carbon-12.
60
s-orbital
A spherical shaped region within an atom that can hold up to two electrons with opposite spins found at the n=1 level and above.
61
P-orbital
A region within an atom that can hold up to 2 electrons with opposite spins.
62
d-orbital
A region within an atom that can hold up to 2 electrons with opposite spin.
63
Shell
A group of atomic orbitals with the same principal quantum number. Also known as energy level.
64
Single covalent bonds
Where atoms are bonded by one shared pair of electrons between nuclei.
65
Simple molecular lattice
A 3D structure of molecules held together by simple molecular forces.
66
Standard condition
Standard set of conditions, temperature and pressure, for experimental measurements established to allow comparisons to be made between different sets of data. This is usually set at 100kPa 298 K and all solutions have a concentration of 1moldm-3.
67
Standard solution
A solution of known concentration. Usually used in titrations to determine unknown information about another substance.
68
Stoichiometry
A molar relationship between the relative quantities of substances taking part in a reaction.
69
Sub-shell
A group of the same type of atomic orbitals (S, P, D, F) within an shell. S subshell can hold 2 electrons, a P subshell can hold 6 electrons and a d subshell can hold a maximum of 10 electrons.
70
Successive ionisation
Value that are a measurement of the energy required to remove each electron in turn.
71
Titrations
The slow addition of one solution of a known concentration, to a known volume of another solution of unknown concentration until the reaction changes, an end point. which is often indicated by a colour change.
72
Van der waals forces
A type of intermolecular bonding that includes permanent dipole-dipole bonding and induced dipole-dipole interactions (London) interactions.
73
Volume
The quantity of 3D space occupied by a solid liquid or gas.
74
Water of crystallisation
Water molecules that form an essential part of the crystalline structure of a compound.

Chemistry (7 decks)

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