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Chemistry > Unit 2 Definitions > Flashcards

Unit 2 Definitions Flashcards

1
Q

Empirical formula

A

A formula which shows the simplest whole number ratios of each element in a compound

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2
Q

Molecular formula

A

A formula which shows the actual number of atoms of each element in a molecule

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3
Q

Molar gas volume

A

The volume of one mole of gas under specified conditions of temperature and pressure

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4
Q

Avogadro’s law

A

The volume of one mole of gas is exactly 24dm^3 if measured at one atmospheric pressure and 20°C

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5
Q

Hydrocarbon

A

A compound that is made of carbon and hydrogen only

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6
Q

Saturated

A

A compound with no C=C bonds

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7
Q

Unsaturated

A

A compound with one or more C=C bonds

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8
Q

Homologous series

A

Compounds that have the same general formula, similar chemical properties, show a graduation in physical properties and successive numbers differ by a CH2 unit

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9
Q

Functional groups

A

The reactive group within a compound

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10
Q

Structural isomers

A

Molecules with the same molecular formula but with different structural formula

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11
Q

Functional isomers

A

Compounds that have the same molecular formula but a different structural formula with different functional groups

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12
Q

Geometric isomers

A

Molecules with the same structural formula, but different arrangement of atoms due to the presence of one or more C=C bonds

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13
Q

Substitution

A

Replacing one atom/group with a different atom/group

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14
Q

Radical

A

A particle with an unpaired electron

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15
Q

Homolytic fission

A

Bond breaking in which one of the shared electrons goes to each atom

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16
Q

Heterolytic fission

A

Bond breaking in which both of the electrons in the shared pair go to a single atom

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17
Q

Sigma bond

A

A covalent bond formed by the linear overlap of atomic orbitals

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18
Q

Pi bond

A

A covalent bond formed by the sideways overlap of p orbitals

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19
Q

Bond length

A

The distance between the nuclei of two covalently bonded atoms

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20
Q

Hydrogenation

A

Addition of a hydrogen molecule across a C=C bond

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21
Q

Electrophile

A

An ion or molecule that attacks a region of high electron density

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22
Q

Heterolytic fission

A

Bond breaking in which both electrons in the shared pair go to a single atom

23
Q

Monomers

A

Many small molecules which can join together to form a polymer

24
Q

Polymer

A

Large molecule formed when monomers join together

25
Polymerisation
Joining together of small molecules to form a large molecule
26
Nucleophile
An ion or molecule, with a lone pair of electrons, that attacks an area of low electron density
27
Miscibility
Liquids which mix in all proportions. Ie: form a single layer
28
Hydrolysis
Breaking up molecules by reaction with water
29
Ground state
A molecular vibration which is in its lowest possible energy state
30
Wave number
The reciprocal of wavelength (measured in cm/1
31
Endothermic
A reaction in which the enthalpy of the products is greater than the enthalpy of the reactants
32
Endothermic
A reaction in which t he enthalpy of the products is less than the enthalpy of the reactants
33
Activation energy
The minimum amount of energy required for a reaction to occur
34
Standard enthalpy change
Change in heat energy at constant constant pressure, measured at standard conditions
35
Enthalpy of formation
The enthalpy change when one mole of a compound is formed from its elements under standard conditions
36
Enthalpy of combustion
The enthalpy change when one mole of a substance is completely burnt in oxygen under standard conditions
37
Enthalpy of neutralisation
The enthalpy change when one mole of water is produced in a neutralisation reaction under standard conditions
38
Conservation of energy
Energy cannot be created or destroyed but it can change from one form to another
39
Hess’s law
The enthalpy change for a reaction is independent of the route taken, provided the i rial and final conditions are the same
40
Average bond enthalpy
The energy required to break one mole of a given bond, averaged over many compounds
41
Rate of reaction
The change in concentration of a reactant or product with respect to time
42
Catalyst
A substance which increases the rate of reaction without being used up itself
43
Activation energy
The minimum amount of energy required for a reaction to occur
44
Maxwell Boltzmann Distribution
The distribution of energies of molecules at a particular temperature, often shown on a graph.
45
Reversible
A reaction which goes in both the forward and backward directions
46
Dynamic
The rate of the forward reaction is equal to the rate of the backward reaction
47
Equilibrium
A reversible reaction in which the amount of each reactant/product remains constant
48
Homogeneous
A reaction in which all the reactants and products are in the same physical state
49
Heterogeneous
A reaction in which all the reactants and products aren’t in the same physical state
50
Le Chatilier’s principle
For a system to be at dynamic equilibrium, the system will move in the direction to oppose any external change imposed upon it
51
Heterogeneous catalyst
The catalyst is in a different phase from the reactants
52
S block element
An element which has an atom with the highest energy/outer electron in an s sub shell
53
Solubility
The maximum mass of solute that will dissolve in 100g of solvent at a stated temperature

Chemistry (11 decks)

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