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Chemistry Year 12/13 > Module 2 - Keywords > Flashcards

Module 2 - Keywords Flashcards

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1
Q

Isotopes

A

Atoms of the same element with different numbers of nuetrons and different masses but the same number of protons and electrons

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2
Q

Relative isotopic mass

A

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

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3
Q

Relative atomic mass

A

Weighted mean mass of an atom compared with 1/12 the mass of carbon-12

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4
Q

Relative molecular mass, Mr

A

Mass of a molecule compared with 1/12th the mass of carbon-12

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5
Q

Mole

A

The unit for an amount of substance (6.02x1023 mol-1)

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6
Q

Avogadro constant

A

The number of particles per mole, 6.02x1023 mol-1

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7
Q

Molar mass

A

Mass per mole, units: gmol-1

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8
Q

Mass spectrometry

A

Method used to determine the relative abundances of different isotopes

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9
Q

Empirical formula

A

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

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10
Q

Molecular formula

A

Number and type of atoms of each element in a molecule

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11
Q

Anhydrous

A

Contains no water

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12
Q

Hydrated

A

Contains water of crystallisation

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13
Q

Ideal gas equation

A

pV=nRT

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14
Q

Stoichiometric relationships

A

The whole number relationships between particles of reactants and products

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15
Q

Percentage yield

A

actual yield/expected yield x100

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16
Q

Atom economy

A

Useful products/total product x100

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17
Q

Acid

A

Proton donor, release H+ in aqueous solution

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18
Q

Base

A

Proton acceptor

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19
Q

Alkalis

A

A substance that releases OH- ions in aqueous solution

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20
Q

Neutralisation reaction

A

A reaction of H+(aq) + OH-(aq) → H2O(l)

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21
Q

Titration

A

The slow addition of one solution of a known concentration to a known volume of another solution of unknown concentration until the end point

22
Q

Strong acid

A

An acid that completely dissociates in water HA → H+ + A-

23
Q

Weak acid

A

An acid that only partially dissociates in water HA ⇌ H+ + A-

24
Q

Dilute acid

A

An acid with only a few particles dissolved per litre (e.g. 0.01 moldm-3)

25
Q

Concentrated acid

A

An acid with lots of particles dissolved per litre (e.g. 50 moldm-3)

26
Q

Oxidation number

A

A measure of the number of electrons involved in bonding. Used to work out what has been oxidised/reduced

27
Q

Oxidation

A

Loss of electrons, increase in oxidation mumber, adding oxygen

28
Q

Reduction

A

Gain of electrons, decrease in oxidation number, removing oxygen

29
Q

Redox

A

A reaction in which one substance is oxidised and another reduced

30
Q

Salt

A

A compound formed when the hydrogen in an acid is replaced by a metal

31
Q

Orbital

A

A region around the nucleus that can hold up to 2 electrons, with opposite spins

32
Q

Subshell

A

Orbitals which have the equivalent energy levels. s subshells contain 1 orbital, p subshells contain 3 orbitals, d subshells contain 5 orbitals

33
Q

Electron configuration

A

Shows how the electrons are arranged in the subshells

34
Q

Ionic bond

A

Electrostatic attraction between positive and negative ions

35
Q

Giant ionic lattices

A

Structure resulting from oppsoitely charges ions strongly attracted in all directions e.g. NaCl

36
Q

Covalent bond

A

The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

37
Q

Dative covalent bond

A

A shared pair of electrons where both electrons originated from the same atom

38
Q

Average bond enthalpy

A

A measurement of covalent bond strength. It’s the energy changes associated with breaking 1 mole of bonds in gaseous molecules

39
Q

Electron pair repulsion theory

A

The idea that electron pairs repel and so affect the shape of the particles. Non bonding pairs (lone pairs) repel more than bonded pairs

40
Q

Linear

A

Shapes caused by having 2 bonding pairs and 0 non bonding electron pairs, which repel as far as possible. Bond angle: 180°

41
Q

Non linear

A

Shape caused by having 2 bonding and 1/2 non bonding electron pairs which repel as far as possible. The non bonding pairs repel more than bonding pairs. Bond angle: 118°/104.5°

42
Q

Trigonal planar

A

Shape caused by having 3 bonding and 0 non bonding electron pairs which repel as far as possible. Bond angle: 120°

43
Q

Pyramidal

A

Shape caused by having 3 bonding and 1 non bonding electron pairs which repel as far as possible. The non bonding pairs repel more than bonding pairs. Bond angle: 107°

44
Q

Tetrahedral

A

Shape caused by having 4 bonding and 0 non bonding electron pairs which repel as far as possible. Bond angle: 109.5°

45
Q

Octahedral

A

Shape caused by having 6 bonding and 0 non bonding electron pairs which repel as far as possible. Bond angle: 90°

46
Q

Electronegativity

A

The ability of an atom to attract the bonding electrons in a covalent bond

47
Q

Polar bond

A

A covalent bond in which there is a permanent dipole due to different electronegativites of the bonded atoms

48
Q

Dipole

A

Having a positive and a negative end

49
Q

Induced dipole

A

An instantaneous dipole caused by dipoles on neighbouring molecules

50
Q

London forces

A

Induced dipole-dipole interactions between molecules

51
Q

Hydrogen bond

A

Intermolecular bonding between molecules containing N, O or F and the H atom of -NH, -OH or HF

Chemistry Year 12/13 (18 decks)

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