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Definitions Flashcards

1
Q

Average bond enthalpy

A

The energy at standard conditions required to break 1 mole of a bond in a gaseous molecules (data taken over a range of similar compounds).

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1
Q

Atomic number (Z)

A

Number of protons in an atom, which equals the number of electrons and is used to define which element the atom belongs to.

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1
Q

Activation energy

A

The minimum energy required for a reaction to occur

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1
Q

Aufbau principle

A

Electrons enter the lowest energy orbit available.

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1
Q

Bronsted-Lowry acid

A

Proton donor

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1
Q

Buffer solution

A

A solution which resists change in pH when small amounts of acid or base are added.

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2
Q

Concentration

A

Amount of solute per unit solvent, measured in g dm-3 or mol dm-3

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3
Q

Continuous spectrum vs line spectrum

A

Continuous made up of all the frequencies, while line spectra contain only certain distinct frequencies.

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3
Q

Conditions for the Haber process

A

Fe catalyst, 450˚C, 200atm

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3
Q

Conditions for the Contact process

A

V2O5 catalyst, 250˚C, 2atm.

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4
Q

Covalent Bond

A

Electrostatic attraction between an electron pair and nuclei, formed when atoms share electrons.

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5
Q

Electron affinity

A

The energy released when 1 mole of gaseous atoms each acquire an electron to form 1 mole of gaseous 1- ions.

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5
Q

Electrolyte

A

A substance which is an insulator when solid but a conductor when liquid or aqueous, and is decomposed by electricity.

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6
Q

Electron arrangement copper

A

4s13d10

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7
Q

Electron relative mass

A

5x10^(-4)

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8
Q

Allotropes

A

Different physical forms of an element

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8
Q

Electronegativity

A

Relative measure of the attraction an atom has for a shared pair of electrons when it’s covalently bonded to another atom.

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9
Q

Empirical formula

A

The simplest whole number ratio of atoms of each element in a particle of the substance.

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11
Q

Endothermic reactions

A

Reactions in which heat is absorbed from the surroundings, temperature decreases and positive delta H

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11
Q

Enthalpy of vaporisation

A

The energy absorbed when 1 mole of gas is made from 1 mole of liquid.

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12
Q

Example of a catalyst in biology

A

Cobalt-57 for vitamin B12 uptake

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13
Q

Exothermic reactions

A

Reactions in which heat is given out to surroundings, causing temperature to increase (delta H is negative)

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14
Q

Factors affecting Kc

A

TEMPERATURE ONLY.

15
Q

First ionisation energy

A

The minimum energy required to remove one electron from a gaseous atom

16
Hybridisation
Mixing of atomic orbitals to form new orbitals with intermediate properties
16
Hund's rule
Electrons prefer to occupy orbitals on their own, and only pair up when no empty orbitals of the same level are available.
17
Ionic bond
Electrostatic attraction between oppositely charged ions, formed when atoms transfer electrons
18
Isotopes
Atoms of the same element with the same atomic number but different mass numbers.
19
Lattice enthalpy
Enthalpy change when one mole of solid crystal is formed from scattered gaseous ions
20
Lewis acid
Electron pair acceptor
22
Ligand
A species that can donate a lone electron pair to a central transition atom/ion, forming a dative covalent bond.
23
Mass number (A)
The number of protons and neutrons in the nucleus
24
Medical use for isotope
Radiotherapy (Cobalt 60), medical tracers (Iodine 125,131).
26
Molar mass
The mass of one mole of a substance
28
Molecular formula
The actual number of atoms of each element in a particle of the substance
29
Molecularity
The number of species taking part in the rate determining step
29
Moles of electron that have passed through the circuit:
n=It/96485
30
Object to be electroplated is placed at the...
cathode
31
pi bonds
Covalent bonding which results from the sideways overlap of parallel p orbitals
34
Rate determining step
The slowest step of the reaction with the highest activation energy
36
Rate of reaction
Increase in concentration of products per unit time
38
Relative atomic mass (Ar)
The weighted mean mass of all the naturally occurring isotopes of an element relative to one twelfth the mass of a 12C atom.
40
Relative molecular mass (Mr)
Sum of relative atomic masses of constituent atoms of a molecule
42
sigma bonds
Covalent bonding which results from the axial overlap of orbitals
43
Solute
A substance which is dissolved in a solvent
44
Solution
A mixture made by dissolving a solute in a solvent.
45
Solvent
A liquid in which something else is dissolved
46
Stages of mass spectrometry
Vapourisation, Ionisation, Accelerration, Deflection, Detection.
48
Standard electrode potential
Voltage obtained when the half cell is connected to the standard hydrogen electrode under standard contions of 298K with 1M solutions.
49
Standard enthalpy change
The heat energy transferred under standard conditions - pressure 101.3kPa, T=298K
50
Standard enthalpy change of formation (delta Hf)
The enthalpy change when one mole of a compound is form from its elements in standard state under standard conditions.
51
Standard enthalpy of combustion
Enthalpy change when one mole of an element/compound is completely burned in excess oxygen under standard conditions.
52
Standard state
The pure form of the substance at T=298K, P=101.3kPa
54
Structural formula
Unambiguously shows arrangement and bonding of atoms in a molecule.
55
Where does oxidation occur?
Oxidation at the anode, reduction at the cathode.

Chemistry (5 decks)

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