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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

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A

Networks of atoms bonded by strong covalent bonds

24
Q

Periodic table

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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
Disproportionation
Oxidation and reduction of the same species in the same reaction
26
Activations energy
Minimum energy required to start a reaction by the breaking of bonds
27
Enthrall chance of reaction
The enthalpy chance associated with a stated equation.
28
Enthalpy change of formation
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
Enthalpy change of combustion
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
Enthalpy change of neutralisation
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
Average bond enthalpy
The average enthalpy change when one mole of bonds is broken into gaseous molecules.
32
General formula
Simplest algebraic formula of a member of a homologous series
33
Structural formula
The minimal detail that shows the arrangement of atoms ins molecule
34
Displayed formula
Relative position of atoms and the bonds between them is shown
35
Skeletal formula
Simplified ordains formula shown by removing hydrogen atoms, leaving just a carbon skeleton with associated functional groups.
36
Homologous series
A series of organic compounds, each with the same general formula, but each successive member differing by CH2.
37
Functional group
Group of atoms responsible for the characteristic reactions of a compound
38
Aliphatic
Compound containing hydrogen and carbon joined together in straight chains, branched chains or non aromatic rings
39
Alicyclic
An aliphatic compound arranged in non aromatic rings
40
Aromatic
A compound containing a benzene ring.
41
Saturated
Containing single carbon-carbon bonds only
42
Structural isomers
Compounds with the same molecular formula but a different structural formula
43
Homolytic fission
Each bonding atom receiving one electron from the bonding pair, forming two radicals.
44
Heterocyclic fission
One bonding pair receiving both electrons from the bonding pair.
45
Radical
A species with an unpaired electron
46
Alkanes
Saturated hydrocarbons containing single C-C bonds only.
47
Sigma bonds
Direct overlap of orbitals between bonding atoms
48
Pi orbitals
Sideways overlap of adjacent p orbitals above and below the plane of the molecule.
49
Stereoisomers
Compounds with the same structural formula but a different arrangement of atoms in space
50
E/Z isomerism
An example of Stereoisomerism, where rotation is restricted by a double bond with two different groups attached to each carbon in double bond.
51
Cis-trans isomerism
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
Electrophile
An electron pair acceptor
53
Nucleophile
An electron pair donor
54
Addition polymerisation
Formation of a very long molecular chain by repeated addition reactions of many unsaturated alkene molecules (monomers).
55
Dative covalent
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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