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Chemistry > Definitions > Flashcards

Definitions Flashcards

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1
Q

Disproportion

A

When the same element has been oxidised and reduced.

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2
Q

Isotope

A

Atoms of an element with same number of protons but different number of neutrons.

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3
Q

Relative atomic mass

A

the weighted mean mass of an element compared with 1/12 of the mass of an atom Carbon-12

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4
Q

Relative isotopic mass

A

the mass of an atom of an isotope compared with 1/12 of the mass of an atom of Carbon-12

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5
Q

First Ionisation Energy

A

the energy needed to remove one electron from each atom in one mole of gaseous atoms to form one mol of gaseous 1+ ions.

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6
Q

Periodicity

A

The repeating trend in properties of elements across a period

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7
Q

Ionic Bonding

A

The electrostatic force of attraction between +ions and -ions

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8
Q

Covalent Bonding

A

The electrostatic force of attraction between a shared pair of electrons and the nuclei of the bonded atom.

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9
Q

Dative Covalent bond

A

A covalent bond in which the shared pair of electrons have been supplied by only one of the bonded atoms

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10
Q

Metallic Bonding

A

The strong electrostatic force of attraction between cations and delocalised sea of electrons

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11
Q

Electron pair

A

One or more electrons involved in a covalent bond.

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12
Q

Lone pair

A

A pair of electrons not involved in a covalent bond

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13
Q

Electronegativity

A

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

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14
Q

Acids

A

Contain hydrogen and when dissolved in water hydrogen dissociates and releases H+ ions

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15
Q

Base

A

Substances that react with acids to neutralise them

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16
Q

Hydrocarbons

A

Compounds containing only Carbon and Hydrogen

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17
Q

Saturated

A

Single bonds

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18
Q

Unsaturated

A

More than one bond (double bond)

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19
Q

Functional Group

A

The part that’s responsible for the chemical properties

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20
Q

Aliphatic

A

Carbons joined in a branched or unbranched chain

21
Q

Alicyclic

A

Carbons joined to each other in a ring

22
Q

Aromantic

A

Some or all Carbons found in Benzene ring

23
Q

Molecular formula

A

The exact number of atoms of each element present in the molecule

24
Q

Empirical formula

A

Simplest whole number ratio of atoms in molecule

25
Q

Structural formula

A

The minimal detail using conventional groups for an unambiguous structure

26
Q

Displayed Formula

A

Shows both relative placing of atoms and the number of bonds between them.

27
Q

Skeletal Formula

A

Simplified organic formula by removing Hydrogen atoms from alkyl chain leaving just a Carbon skeleton and associated functional group.

28
Q

General Formula

A

Represents any member of a homologous series

29
Q

Isomer

A

Same molecular formula but different structural formula

30
Q

Radical

A

An extra electron that is unpaired

31
Q

Homolytic fission

A

When bond breaks each bonded atom takes one of the shaired pair of electrons

32
Q

Heterolytic fission

A

One of the bonded atoms takes both of the shaired pair of electrons.

33
Q

Stereoisomer

A

Have the same structural formula but a different arrangement of the atoms in space

34
Q

Electrophile

A

Electron pair acceptor

35
Q

Nucleophile

A

Electron pair donor

36
Q

Carbocation

A

positively charged Carbon

37
Q

Curly arrow

A

Shows the movement of electron pair

38
Q

Activation energy

A

The energy input required to break existing bonds and the minimum energy required to start the reaction.

39
Q

Standard enthalpy change of formation

A

The enthalpy change that takes place when one mole of a compound is formed from its elements

40
Q

Standard enthalpy change of combustion

A

The enthalpy change that takes place when one mole of a substance reacts completely with oxygen

41
Q

Standard enthalpy change of neutralisation

A

The energy change that accompanies the reaction of an acid by a base to form one mol of water.

42
Q

Average Bond enthalpy

A

The energy required to break one mole of a specified type of bond in a gaseous molecule

43
Q

Catalyst

A

Provides an alternative pathway with a lower activation energy without being used up or damaged.

44
Q

ideal gas equation

A

PV=nRT

45
Q

in the ideal gas equation what does the P stand for and what unit

A

pressure

Pa

46
Q

in the ideal gas equation what does V stand for and what is the units

A

volume
m^3
cm^3 x 10^-6
m^3 x10^-3

47
Q

what is n stand for

A

moles

48
Q

in the ideal gas equation what does R stand for

A

8.31 gas constant

49
Q

in the ideal gas equation what does T stand for and what unit

A

temperatures
kelvin
+273

Chemistry (6 decks)

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