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Chemistry Facts > Equations and Definitions > Flashcards

Equations and Definitions Flashcards

1
Q

Ideal gas equation

A

P (kPa) x V (m^3) = n x R x T (K)

PV=nRT

R = 8.314

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2
Q

Define relative isotopic mass

A

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

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3
Q

Define relative atomic mass

A

The weighted mean mass compared with 1/12th the mass of carbon-12

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4
Q

Charge of nitrate?

A

1-

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5
Q

Charge of carbonate?

A

2-

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6
Q

Charge of sulphate

A

2-

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7
Q

Charge of OH

A

1-

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8
Q

Charge of ammonium

A

1+

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9
Q

Charge of zinc ion

A

2+

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10
Q

Charge of silver ion

A

1+

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11
Q

What does a Roman numeral indicate in terms of oxidation?

A

The magnitude of the oxidation number when an element may have compounds/ions with different oxidation numbers

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12
Q

Define electronegativity

A

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

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13
Q

Define first ionisation energy

A

The energy required to remove 1 mol of electrons from 1 mol of gaseous atoms

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14
Q

Define an ionic bond

A

The electrostatic attraction between positive and negative ions

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15
Q

Define a covalent bond

A

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

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16
Q

Define disproportionation

A

The oxidation and reduction of the same element

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17
Q

Define activation energy

A

The minimum energy required for a reaction to take place

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18
Q

What are standard conditions in terms of enthalpy changes

A

101kPa and a stated temperature, 298K

19
Q

Define the enthalpy change of formation

A

The formation of 1 mol of a compound from its elements

20
Q

Define the enthalpy change of combustion

A

The complete combustion of 1 mol of a substance

21
Q

Define the enthalpy change of neutralisation

A

The formation of 1 mol of water from neutralisation

22
Q

Equation for enthalpy change

A

q = m (g) x c x change in temp (K)

23
Q

Define a homologous series

A

A series of organic compounds having the same functional group but with each successive member differing by CH2.

24
Q

Define aliphatic

A

A compound containing C and H joined together in straight chains, branched chains, or non-aromatic rings.

25
Q

Define alicyclic

A

An aliphatic compound arranged in non-aromatic rings with or without side chains

26
Q

Define aromatic

A

A compound containing a benzene ring

27
Q

Define structural isomer

A

Compounds with the same molecular formula but different structural formula

28
Q

Define homolytic fission

A

Each bonding atom receiving one electron from the bonded pair, forming two radicals

29
Q

Define heterolytic fission

A

One bonding atom receiving both electrons from the bonded pair

30
Q

Define radical

A

A species with an unpaired electron

31
Q

Define stereoisomers

A

Compounds with the same structural formula but different arrangement in space

32
Q

Define E/Z isomerism

A

An example of stereoisomerism, in terms of restricted rotation about a double bond and the requirement for two different groups to be attached to each carbon atom of the C=C group.

33
Q

Define cis-trans isomerism

A

A special case of E/Z isomerism in which two of the substituent groups attached to each carbon atom of the C=C group are the same.

34
Q

Define an electrophile

A

An electron pair acceptor

35
Q

Define nucleophile

A

An electron pair donor

36
Q

Formula for atom economy?

A

Mr of desired product / sum of total Mr for all products

x 100

37
Q

Formula for percentage yield

A

Actual amount / theoretic amount

38
Q

Enthalpy of solution

A

The enthalpy change when 1 mol of an ionic solid dissolves in water

39
Q

Enthalpy of hydration

A

When one mol of a gaseous ion is completely hydrated by water

40
Q

Lattice enthalpy

A

Energy released when one mol of a Crystal is formed from ions of its constituents in gaseous state

41
Q

Enthalpy of atomisation

A

When one mol of gaseous atoms is formed from the element in its natural state

42
Q

Ionisation energy

A

The energy required to remove one mol of electrons from one mol of gaseous atoms

43
Q

Electron affinity

A

Enthakpy change when one mol of gaseous atoms gains one mol of electrons

44
Q

define average bond enthalpy

A

the enthalpy change when 1 mol of a specific type of bond breaks in a gaseous molecule

Chemistry Facts (11 decks)

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