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Chemistry definitions > Unit 2 Chemistry definitions > Flashcards

Unit 2 Chemistry definitions Flashcards

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1
Q

Empirical formula

A

Shows the simplest whole number ratio of atoms of each element in compound

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2
Q

Molecular formula

A

Shows the actual number of atoms of each element in one molecule of a substance

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3
Q

molar gas volume

A

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

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4
Q

ty

A

max amount of mass of a product that could theoretically be obtained in a chemical reaction

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5
Q

Actual yield

A

The actual mass of a product

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6
Q

functional group

A

the part of a structure that determine the characteristics of a compound

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7
Q

homologous series

A

series of compounds that have the same general formula and similar chemical properties

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8
Q

hydrocarbon

A

contains only carbon and hydrogen atoms

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9
Q

saturated hydrocarbon

A

contains no c=c bonds

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10
Q

substitution

A

replacing one atom or group with another

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11
Q

radical

A

particle with unpaired electron

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12
Q

homolytic fission

A

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

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13
Q

unsaturated hydrocarbons

A

contains at least one c=c bond

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14
Q

sigma bond

A

covalent bond formed by the linear overlap of atomic orbitals which allows rotation along the bond axis

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15
Q

bond length

A

distance between the nuclei of 2 covalently bonded atoms

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16
Q

pi bond

A

covalent bond formed by the sideways over lap of p orbitals which restricts rotation along the bond axis

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17
Q

addition reaction

A

the pi bond of a double covalent bond is broken and 2 species add on across the double bond

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18
Q

electrophile

A

ion or molecule that attacks regions of high electron density

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19
Q

heterolytic fission

A

bond breaking in which both electrons in the shared pair go to a single action

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20
Q

primary carbo cat ion

A

has 1 carbon directly attached to the positively charged carbon

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21
Q

hydrogenation

A

addition of a hydrogen molecule across a c=c bond

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22
Q

Polymerisation

A

joining together of small molecules to form a large molecule

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23
Q

monomer

A

small molecules whichjoin together to form a polymer

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24
Q

polymer

A

large molecules which formed when monomers join together

25
Q

primary halogenoalkane

A

a halogenalkane that has one carbon directly bonded to the carbon ayom that is bonded to the halogen

26
Q

nucleophile

A

ion or molecule with a lone pair of electrons that attacks regions of low electron density

27
Q

py

A

ay/tyx100

28
Q

atom economy

A

m of desired of products/total mass of products x 100

29
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 bond

30
Q

reflux

A

repeated boiling and condensing of a mixture

31
Q

structural formula

A

shows the bonding between all the atoms

32
Q

Hydrolysis

A

Breaking up molecules by reaction with water

33
Q

Nucleophile

A

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

34
Q

Elimination

A

A reaction in which a small molecule is removed from a larger
molecul

35
Q

primary alcohol

A

An alcohol which has 1 carbon directly bonded to the carbon atom which is directly bonded to the oh group

36
Q

Ground state
(infrared
spectroscopy)

A

A molecular vibration which is in the lowest possible energy

state

37
Q

Wavenumber

A

The reciprocal of the wavelength and it is measured in cm-1

.

38
Q

Endothermic

A

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

39
Q

Exothermic

A

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

40
Q

Standard

conditions

A

298K and 100kPa

41
Q

Standard

enthalpy change

A

Change in heat energy at constant pressure, measured at

standard conditions.

42
Q

Standard enthalpy

of combustion

A

The enthalpy change when one mole of a substance is

completely burnt in oxygen under standard conditions.

43
Q

Standard enthalpy

of formation

A

The enthalpy change when one mole of a compound is formed

from its elements under standard conditions

44
Q

Standard enthalpy

of neutralisation

A

The enthalpy change when one mole of water is produced in a

neutralisation reaction under standard conditions.

45
Q

Conservation of

energy

A

Energy cannot be created or destroyed but it can change from

one form to another.

46
Q

Hess’s Law

A

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

47
Q

Average bond

enthalpy

A

The energy required to break one mole of a given bond

averaged over many compounds.

48
Q

Reaction rate

A

The change of the concentration (amount) of a reactant or

product with respect to time.

49
Q

Catalyst

A

A substance which increases the rate of a chemical reaction but
does not get used up.

50
Q

Activation energy

A

The minimum amount of energy required for a reaction to

occur.

51
Q

Reversible

A

A reaction which goes in both the forward and backward

directions.

52
Q

Dynamic

equilibria

A

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

53
Q

Equilibrium

A

A reversible reaction in which the amount of each reactant /

product remains constant.

54
Q

Homogeneous

A

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

55
Q

Heterogeneous

equilibria

A

A reaction in which all the reactants and products are not in the
same physical state

56
Q

Kc

A 
KC =
[C]
c
[D]
d
[A]
a
[B]
b
for a reaction in the format
aA + bB ⇌ cC + dD
57
Q

Heterogeneous

catalyst

A

The catalyst is in a different phase from the reactants

58
Q

s-block element

A

An element which has an atom with highest energy/outer

electron in an s-subshell (orbital).

59
Q

Solubility

A

The maximum mass of solute that will dissolve in 100 g of

solvent at a stated temperature.

Chemistry definitions (2 decks)

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