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Chemistry > Definitions > Flashcards

Definitions Flashcards

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
Q

Giant metallic lattice

A

3D structure of positive ions and delocalised electrons bonded together by strong metallic bonds

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26
Q

Hydrogen bond

A

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.

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27
Q

Acid

A

A chemical that is a proton donor and releases H+ into solution

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28
Q

Intermolecular force

A

An attractive force between neighbouring molecules of atoms.

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29
Q

Ion

A

A positively or negatively charged atom or covalently bonded group of atoms molecular ion.

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30
Q

Ionic bond

A

Electrostatic attraction between oppositely charged ions.

31
Q

Ionisation

A

The process of an atom becoming an ion.

32
Q

Isotopes

A

Atoms of the same element with different numbers of neutrons.

33
Q

London (dispersion) forces

A

Attractive forces between induced dipoles in neighbouring molecules.

34
Q

Lone pair

A

An outer shell pair of electrons that is not involved in chemical bonding.

35
Q

Mass number

A

The number of particles, protons and neutrons in the nucleus.

36
Q

Mass spectrometry

A

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
Q

Metallic bonding

A

Electrostatic attraction between positive metal ions and delocalised electrons.

38
Q

Molar gas volume

A

Volume per mole of a gas. Units are dm3mol-1.

At room temperature and pressure the molar gas volume is approximately 24dm3mol-1.

39
Q

Molar mass

A

M

Mass per mole of a substance g mol-1.

40
Q

Molar volume

A

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
Q

Mole

A

The amount of any substance containing as many particles as there are carbon atoms in exactly 12g of carbon 12 isotope.

42
Q

Neutralisation

A

The reaction of an acid with a base

43
Q

Neutron

A

A particle found in the nucleus of an atom. It is almost identical in mass to a proton but has no charge.

44
Q

Oxidation

A

Loss or electrons, loss of hydrogen, gain of oxygen or increase in oxidation number.

45
Q

Oxidising agent

A

A reagent that oxidises (takes electrons from) another species.

46
Q

Percentage yield

A

Actual amount in mol of a product divided by theoretical amount of product multiplied by 100.

47
Q

Period

A

A horizontal row of elements in the periodic table.

48
Q

Periodic table

A

A tabular arrangement of the chemical elements organised on the basis of their atomic number, electron configurations and recurring chemical properties.

49
Q

Periodicity

A

A regular periodic variation of properties of elements with atomic number and position in the periodic table.

50
Q

Permanent dipole

A

A small charge difference across a bond that results from a difference in electronegativities of the bonded atoms.

51
Q

Permanent dipole-dipole interaction

A

A weak attractive force between permanent dipoles and permanent dipoles or induced dipoles in neighbouring polar molecules.

52
Q

Polar covalent bond

A

A covalent bond that has a permanent dipole

53
Q

Pressure

A

A measure of the force applied over a unit area

54
Q

Principal quantum number

A

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
Q

Redox reaction

A

A reaction in which both reduction and oxidation take place.

56
Q

Reducing agent

A

A reagent that reduces (adds electrons) to another species.

57
Q

Reduction

A

Gain of electrons, gain of hydrogen, loss of oxygen or a decrease in oxidation number.

58
Q

Relative atomic mass

A

The weighted mean mass of an atom of an element compared with one twelfth of the mass of carbon 12.

59
Q

Relative isotopic mass

A

The mass of an atom of an isotope compared with 1/12th of the mass of an atom of carbon-12.

60
Q

s-orbital

A

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
Q

P-orbital

A

A region within an atom that can hold up to 2 electrons with opposite spins.

62
Q

d-orbital

A

A region within an atom that can hold up to 2 electrons with opposite spin.

63
Q

Shell

A

A group of atomic orbitals with the same principal quantum number. Also known as energy level.

64
Q

Single covalent bonds

A

Where atoms are bonded by one shared pair of electrons between nuclei.

65
Q

Simple molecular lattice

A

A 3D structure of molecules held together by simple molecular forces.

66
Q

Standard condition

A

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
Q

Standard solution

A

A solution of known concentration. Usually used in titrations to determine unknown information about another substance.

68
Q

Stoichiometry

A

A molar relationship between the relative quantities of substances taking part in a reaction.

69
Q

Sub-shell

A

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
Q

Successive ionisation

A

Value that are a measurement of the energy required to remove each electron in turn.

71
Q

Titrations

A

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
Q

Van der waals forces

A

A type of intermolecular bonding that includes permanent dipole-dipole bonding and induced dipole-dipole interactions (London) interactions.

73
Q

Volume

A

The quantity of 3D space occupied by a solid liquid or gas.

74
Q

Water of crystallisation

A

Water molecules that form an essential part of the crystalline structure of a compound.

Chemistry (7 decks)

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