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Chemistry > Unit 2 Definitions > Flashcards

Unit 2 Definitions Flashcards

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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
Q

Polymerisation

A

Joining together of small molecules to form a large molecule

26
Q

Nucleophile

A

An ion or molecule, with a lone pair of electrons, that attacks an area of low electron density

27
Q

Miscibility

A

Liquids which mix in all proportions. Ie: form a single layer

28
Q

Hydrolysis

A

Breaking up molecules by reaction with water

29
Q

Ground state

A

A molecular vibration which is in its lowest possible energy state

30
Q

Wave number

A

The reciprocal of wavelength (measured in cm/1

31
Q

Endothermic

A

A reaction in which the enthalpy of the products is greater than the enthalpy of the reactants

32
Q

Endothermic

A

A reaction in which t he enthalpy of the products is less than the enthalpy of the reactants

33
Q

Activation energy

A

The minimum amount of energy required for a reaction to occur

34
Q

Standard enthalpy change

A

Change in heat energy at constant constant pressure, measured at standard conditions

35
Q

Enthalpy of formation

A

The enthalpy change when one mole of a compound is formed from its elements under standard conditions

36
Q

Enthalpy of combustion

A

The enthalpy change when one mole of a substance is completely burnt in oxygen under standard conditions

37
Q

Enthalpy of neutralisation

A

The enthalpy change when one mole of water is produced in a neutralisation reaction under standard conditions

38
Q

Conservation of energy

A

Energy cannot be created or destroyed but it can change from one form to another

39
Q

Hess’s law

A

The enthalpy change for a reaction is independent of the route taken, provided the i rial and final conditions are the same

40
Q

Average bond enthalpy

A

The energy required to break one mole of a given bond, averaged over many compounds

41
Q

Rate of reaction

A

The change in concentration of a reactant or product with respect to time

42
Q

Catalyst

A

A substance which increases the rate of reaction without being used up itself

43
Q

Activation energy

A

The minimum amount of energy required for a reaction to occur

44
Q

Maxwell Boltzmann Distribution

A

The distribution of energies of molecules at a particular temperature, often shown on a graph.

45
Q

Reversible

A

A reaction which goes in both the forward and backward directions

46
Q

Dynamic

A

The rate of the forward reaction is equal to the rate of the backward reaction

47
Q

Equilibrium

A

A reversible reaction in which the amount of each reactant/product remains constant

48
Q

Homogeneous

A

A reaction in which all the reactants and products are in the same physical state

49
Q

Heterogeneous

A

A reaction in which all the reactants and products aren’t in the same physical state

50
Q

Le Chatilier’s principle

A

For a system to be at dynamic equilibrium, the system will move in the direction to oppose any external change imposed upon it

51
Q

Heterogeneous catalyst

A

The catalyst is in a different phase from the reactants

52
Q

S block element

A

An element which has an atom with the highest energy/outer electron in an s sub shell

53
Q

Solubility

A

The maximum mass of solute that will dissolve in 100g of solvent at a stated temperature

Chemistry (11 decks)

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