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Chemistry > Definitions > Flashcards

Definitions Flashcards

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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
Q

Hybridisation

A

Mixing of atomic orbitals to form new orbitals with intermediate properties

16
Q

Hund’s rule

A

Electrons prefer to occupy orbitals on their own, and only pair up when no empty orbitals of the same level are available.

17
Q

Ionic bond

A

Electrostatic attraction between oppositely charged ions, formed when atoms transfer electrons

18
Q

Isotopes

A

Atoms of the same element with the same atomic number but different mass numbers.

19
Q

Lattice enthalpy

A

Enthalpy change when one mole of solid crystal is formed from scattered gaseous ions

20
Q

Lewis acid

A

Electron pair acceptor

22
Q

Ligand

A

A species that can donate a lone electron pair to a central transition atom/ion, forming a dative covalent bond.

23
Q

Mass number (A)

A

The number of protons and neutrons in the nucleus

24
Q

Medical use for isotope

A

Radiotherapy (Cobalt 60), medical tracers (Iodine 125,131).

26
Q

Molar mass

A

The mass of one mole of a substance

28
Q

Molecular formula

A

The actual number of atoms of each element in a particle of the substance

29
Q

Molecularity

A

The number of species taking part in the rate determining step

29
Q

Moles of electron that have passed through the circuit:

A

n=It/96485

30
Q

Object to be electroplated is placed at the…

A

cathode

31
Q

pi bonds

A

Covalent bonding which results from the sideways overlap of parallel p orbitals

34
Q

Rate determining step

A

The slowest step of the reaction with the highest activation energy

36
Q

Rate of reaction

A

Increase in concentration of products per unit time

38
Q

Relative atomic mass (Ar)

A

The weighted mean mass of all the naturally occurring isotopes of an element relative to one twelfth the mass of a 12C atom.

40
Q

Relative molecular mass (Mr)

A

Sum of relative atomic masses of constituent atoms of a molecule

42
Q

sigma bonds

A

Covalent bonding which results from the axial overlap of orbitals

43
Q

Solute

A

A substance which is dissolved in a solvent

44
Q

Solution

A

A mixture made by dissolving a solute in a solvent.

45
Q

Solvent

A

A liquid in which something else is dissolved

46
Q

Stages of mass spectrometry

A

Vapourisation, Ionisation, Accelerration, Deflection, Detection.

48
Q

Standard electrode potential

A

Voltage obtained when the half cell is connected to the standard hydrogen electrode under standard contions of 298K with 1M solutions.

49
Q

Standard enthalpy change

A

The heat energy transferred under standard conditions - pressure 101.3kPa, T=298K

50
Q

Standard enthalpy change of formation (delta Hf)

A

The enthalpy change when one mole of a compound is form from its elements in standard state under standard conditions.

51
Q

Standard enthalpy of combustion

A

Enthalpy change when one mole of an element/compound is completely burned in excess oxygen under standard conditions.

52
Q

Standard state

A

The pure form of the substance at T=298K, P=101.3kPa

54
Q

Structural formula

A

Unambiguously shows arrangement and bonding of atoms in a molecule.

55
Q

Where does oxidation occur?

A

Oxidation at the anode, reduction at the cathode.

Chemistry (5 decks)

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