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AS Chemistry > Definitions 101 > Flashcards

Definitions 101 Flashcards

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1
Q

Acid

A

Proton donor.

Species that releases H+ ions in aqueous solution

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2
Q

Bases

A

Proton acceptors.

Compound that neutralises an acid to form a salt.

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3
Q

Alkali

A

Soluble base that releases OH- ions in water.

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4
Q

Isotope

A

Atoms of the same element with different number of neutrons and different masses.

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5
Q

Relative isotopic mass

A

Mass of an isotope compared with 1/12 mass of a carbon -12 atom

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6
Q

Relative atomic mass

A

The weighted mean mass of an atom of an element compared with 1/12 mass of a carbon-12 atom

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7
Q

First ionisation energy

A

Energy required to remove 1 electron from each atom in 1 mol of gaseous atoms.

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8
Q

Atomic orbital

A

A region around the nucleus that can hold up to two electrons with opposite spins.

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9
Q

Mole

A

The amount of any substance containing as many elementary particles as there are carbon atoms in exactly 12g of the carbon-12 isotope.

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10
Q

Avogadro constant

A

Number of particles per mole, 6.02 X 10^23

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11
Q

Molar mass

A

Mass per mile of a substance (gmol^-1)

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12
Q

Molar gas volume

A

Gas volumes per mole (dm^3mol^-1)

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13
Q

Empirical formula

A

The simplest whole number ratio of atoms of each element present in a compound

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14
Q

Molecular formula

A

The actual number of atoms of each element in a molecule

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15
Q

Anhydrous

A

Containing no water molecules

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16
Q

Hydrated

A

Containing water of crystallisation

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17
Q

Water of crystallisation

A

Water molecules that are bonded into the crystalline structure of a compound.

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18
Q

Ionic bonding

A

Electrostatic attraction between oppositely charged ions.

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19
Q

Covalent bond

A

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

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20
Q

Electronegativity

A

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

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21
Q

Hydrogen bonding

A

Intermolecular bonding between molecules containing N, O or F and the H atom of -NH, -OH or HF

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22
Q

Metallic bonding

A

Strong electrostatic attraction between cations and delocalised electrons

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23
Q

Solid giant covalent lattices

A

Networks of atoms bonded by strong covalent bonds

24
Q

Periodic table

A

Arrangement of elements:
By increasing atomic number
In periods showing repeating trends in physical and chemical properties
In groups having similar chemical properties.

25
Q

Disproportionation

A

Oxidation and reduction of the same species in the same reaction

26
Q

Activations energy

A

Minimum energy required to start a reaction by the breaking of bonds

27
Q

Enthrall chance of reaction

A

The enthalpy chance associated with a stated equation.

28
Q

Enthalpy change of formation

A

Enthalpy change that takes place when one mole of a compound is formed from its constituent elements in their standard states under standard conditions.

29
Q

Enthalpy change of combustion

A

The enthalpy change that occurs when one mole of a substance reacts completely with oxygen, under standard conditions, all reactants and products in their standard states.

30
Q

Enthalpy change of neutralisation

A

The enthalpy change that occurs when one mole of water is formed from a reaction of an acid and a base, under standard conditions with everything in standard states

31
Q

Average bond enthalpy

A

The average enthalpy change when one mole of bonds is broken into gaseous molecules.

32
Q

General formula

A

Simplest algebraic formula of a member of a homologous series

33
Q

Structural formula

A

The minimal detail that shows the arrangement of atoms ins molecule

34
Q

Displayed formula

A

Relative position of atoms and the bonds between them is shown

35
Q

Skeletal formula

A

Simplified ordains formula shown by removing hydrogen atoms, leaving just a carbon skeleton with associated functional groups.

36
Q

Homologous series

A

A series of organic compounds, each with the same general formula, but each successive member differing by CH2.

37
Q

Functional group

A

Group of atoms responsible for the characteristic reactions of a compound

38
Q

Aliphatic

A

Compound containing hydrogen and carbon joined together in straight chains, branched chains or non aromatic rings

39
Q

Alicyclic

A

An aliphatic compound arranged in non aromatic rings

40
Q

Aromatic

A

A compound containing a benzene ring.

41
Q

Saturated

A

Containing single carbon-carbon bonds only

42
Q

Structural isomers

A

Compounds with the same molecular formula but a different structural formula

43
Q

Homolytic fission

A

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

44
Q

Heterocyclic fission

A

One bonding pair receiving both electrons from the bonding pair.

45
Q

Radical

A

A species with an unpaired electron

46
Q

Alkanes

A

Saturated hydrocarbons containing single C-C bonds only.

47
Q

Sigma bonds

A

Direct overlap of orbitals between bonding atoms

48
Q

Pi orbitals

A

Sideways overlap of adjacent p orbitals above and below the plane of the molecule.

49
Q

Stereoisomers

A

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

50
Q

E/Z isomerism

A

An example of Stereoisomerism, where rotation is restricted by a double bond with two different groups attached to each carbon in double bond.

51
Q

Cis-trans isomerism

A

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

52
Q

Electrophile

A

An electron pair acceptor

53
Q

Nucleophile

A

An electron pair donor

54
Q

Addition polymerisation

A

Formation of a very long molecular chain by repeated addition reactions of many unsaturated alkene molecules (monomers).

55
Q

Dative covalent

A

A shared pair of electrons in which the bonded pair has been provided by one if the bonding atoms only.

AS Chemistry (6 decks)

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