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Chemistry > 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 neutrons and different masses

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2
Q

Relative Isotopic Mass

A

Mass of an isotope compared to 1/12th of the mass of carbon-12

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3
Q

Relative Atomic Mass

A

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

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4
Q

Relative Molecular Mass, Mr

A

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

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5
Q

Mole

A
  • The unit for an amount of substance (6.02 x 10^23 particles)
  • The amount of substance containing as many particles as there are carbon atoms in exactly 12g of the carbon-12 isotope
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6
Q

Avogadro Constant

A

The number of particles per mole, (6.02 x 10^23 mol^-1)

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7
Q

Molar Mass

A

Mass per mole, g mol^-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 the particles of reactants and products

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15
Q

Percentage Yield

A

actual yield / expected yield x 100

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16
Q

Atom Economy

A

useful products / total product x 100

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17
Q

Acid

A

Proton donor, release H+ ions in aqueous solution

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18
Q

Base

A

Proton acceptor

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19
Q

Alkali

A

A soluble base that releases OH- ions in aqueous solution

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20
Q

Neutralisation

A

A reaction of H+ + OH- –> H2O

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21
Q

Titration

A

The slow addition of one solution ok 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 mol dm^-3)

25
Q

Concentrated Acid

A

An acid with lots of particles dissolved per litre (e.g. 50.01 mol dm^-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 number
  • 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

The 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 two electrons, with opposite spins

32
Q

Subshell

A

Orbitals which have the equivalent energy levels. S subshell contains 1 orbital, p subshell contains 3 orbitals, d subshell contains 5 orbitals

33
Q

Electron Configuration

A

Shows how many electrons are arranged in the subshells. e.g. oxygen: 1s22s22p4

34
Q

Ionic Bond

A

Electrostatic forces of attraction between positive and negative ions

35
Q

Giant Ionic Lattices

A

Structure resulting from oppositely charged ions in all directions e.g. NaCl

36
Q

Covalent Bond

A

A shared pair of electrons

37
Q

Dative Covalent Bond

A

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

38
Q

Average Bond Enthalpy

A

A measurement of covalent bond strength. It is the energy change associated with breaking 1 mol 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 bonded pairs repel more than bonded pairs

40
Q

Linear

A

Shape caused by having 2 bonded pairs and 0 non-bonding electron pairs - which repel as far as possible. The bond angle is 180º

41
Q

Non-linear

A

Shape caused by having 2 bonding and one or two non-bonding electron pairs which repel as far as possible . The bond angle will be 118º or 104.5º

42
Q

Trigonal Planar

A

Shape caused by having 3 bonding and 0 non bonding electron pairs which repel as far as possible. The bond angle will be 120º

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. The bond angle will be 107º

44
Q

Tetrahedral

A

Shape caused by having 4 bonding and 0 non bonding electron pairs which repel as far as possible. The bond angle will be 109.5º

45
Q

Octahedral

A

Shape caused by having 6 bonding and 0 non bonding electron pairs which repel as far as possible. The bond angle will be 90º

46
Q

Electronegativity

A

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

47
Q

Polar Bond

A

A covalent bond in which there is a permanent dipole due to differing electronegativities 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 (13 decks)

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