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Alevel > Y12 Definitions > Flashcards

Y12 Definitions Flashcards

1
Q

Relative isotopic mass

A

The mass of an isotope relative to 1/12 of the mass of carbon 12

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2
Q

Relative atomic mass

A

The weighted mean mass of an element relative to 1/12 of the mass of carbon 12

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3
Q

Ammonium

A

NH4+

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4
Q

Hydroxide

A

Oh-

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5
Q

Nitrate

A

NO3-

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6
Q

Nitrite

A

NO2-

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7
Q

Hydrogen carbonate

A

HCO3-

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8
Q

Manganite VII

A

MnO4-

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9
Q

Carbonate

A

CO32-

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10
Q

Sulphate

A

SO42-

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11
Q

Sulfite

A

SO32-

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12
Q

Dichromate VI

A

Cr2O72-

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13
Q

Phosphate

A

PO43-

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14
Q

Polyatomic molecules

A

N2 P4 S8

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15
Q

Mole

A

The amount of substance that contains 6.02 x10^23 particles

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16
Q

Molar mass

A

Mass per mole of a substance units are gmol^-1

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17
Q

Molecular formula

A

The actual number of atoms of each element in a molecule

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18
Q

Empirical formula

A

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

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19
Q

Relative molecular mass

A

Compares the mass of the molecule with the mass of an atom of carbon 12 calculated by adding atomic masses together

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20
Q

Relative formula mass

A

Compares the mass of the formula unit with the mass of an atom of carbon 12 calculated by adding together the relative atomic masses of the elements in the empirical formula

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21
Q

Molecular formula

A

Molecular mass divided by empirical formula mass

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22
Q

Room temperature and pressure

A

20°C 101KPA or one atmosphere

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23
Q

Ideal gas equation

A 
PV= nRT
P= pressure Pa
V= volume m^3= 1000dm^3
n= moles
R= gas constant= 8.31j/mol/k
T=temp= K
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24
Q

Assumptions real gas equation

A

Random motion elastic collisions negligible size no intermolecular forces

25
Q

Stoichiometry

A

The ratio balancing an equation

26
Q

Atom economy

A

A measure of how well the atoms have been utilised

Reactions with high at McConomy is produced a large proportion of desired product few unwonted waste products they are important the sustainability and make the best use of natural resources based on balanced chemical equations assume 100% yield atom economy equals some of mola masses of desired Products divided by some of mola masses of all products times 100

27
Q

Bases

A

Metal oxides metal hydroxide metal carbonate and ammonia NH3

28
Q

Alkalis

A

A base the dissolves in water releasing hydroxide ions into the solution

29
Q

Acid plus base

A

Salt and water

30
Q

Dissociation of sulphuric acid

A

Only one of the two hydrogen atoms is a strong acid’s are only partially dissociates to form HSO4-
This then disassociates to form SO42-

31
Q

Titrations

A

Technique used to accurately measure the volume of one solution that reacts with another solution

32
Q

Ox number F

A

-1

33
Q

Special cases oxidation number is

A

H in metal hydrides(NaH)= -1
O in peroxide = -1
O bonded to F= +2

34
Q

Max no of electrons in a shell

A

2n^2

35
Q

Atomic orbitals

A

A region around the nucleus that can hold up to 2 electrons with opposite spins

36
Q

Patterns of 4S and 3-D subs shells

A

4S fills before 3-D and empties before as once fills 3-D energy levels fall below 4S energy levels

37
Q

Covalent bond

A

Strong electrostatic attraction between shared pair of electrons and the nuclei of the bonded atoms

38
Q

Boron bond forming

A

Boring has three electrons in outershell when all three are bonded in covalent bonding only six electrons are in its outer shell

39
Q

Expanding the octad

A

Occurs after the third shell depends how many unpaired electrons

40
Q

Dative covalent bonds

A

Form when there is originally a lone pair of electrons on one of the bonded atoms for example ammonium is formed when an ammonia and hydrogen ions react

41
Q

2 electron regions

A

Linear bond angle 180° example CO2

42
Q

Three electron regions

A

Trogonal planar Bond angle 120° example BF3

43
Q

4 electronic regions

A

Tetrahedral bond angle 109.5°CH4

44
Q

Six electron regions

A

Octahedral 90° SF6

45
Q

Electronegativity

A

The attraction of a bonded atoms for the pair of electrons in a covalent bond

46
Q

Intermolecular forces

A

Week interactions between dipoles of different molecules

47
Q

London forces

A

Induced dipole dipole interactions

48
Q

Simple molecular substance

A

Made up of simple molecules small units containing definite number of atoms with a definite molecular formula such as H2O CO2 H2

49
Q

Hydrogen bonds can form with

A

Oxygen nitrogen fluorine

50
Q

Percentage error

A

Error/amount x100

51
Q

Dipole

A

A difference in charge between two atoms caused by shift in electron density in the bond

52
Q

Entropy units

A

J/K/mol

53
Q

Standard entropy

A

The entropy of one mole of a substance understand his condition always positive

54
Q

Catalyst for breakdown of hydrogen peroxide

A

Magnesium oxide MNO2

55
Q

entropy

A

A term used for the dispersal of energy within the chemicals making up the chemical system

56
Q

Free energy change Delta G

A

The overall change in energy during a chemical reaction

57
Q

Enthalpy

A

The measure of the heat energy in a chemical system

58
Q

Ethanolic acid

A

CH3COOH

Alevel (8 decks)

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