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a level chemistry > module two > Flashcards

module two Flashcards

1
Q

what does an atom consist of?

A

a nucleus containing protons and neutrons
electrons orbiting the nucleus in shells

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2
Q

relative mass and charge of sub-atomic particles

A

proton mass = 1 charge = +1
neutron mass = 1 charge = 0
electron mass = 1/2000 charge = -1

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3
Q

atomic number

A

number of protons in an atom

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4
Q

mass number

A

number of protons and neutrons in an atom

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5
Q

isotopes

A

atoms of the same element with different number of neutrons

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6
Q

relative isotopic mass

A

mass of an atom of an isotope relative to 1/12th the mass of an atom of carbon-12

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7
Q

relative atomic mass

A

weighted mean mass of an atom of an element relative to 1/12th the mass of an atom of carbon-12

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8
Q

equation for relative atomic mass

A

Ar = (% abundance of isotope 1 x mass) + (% abundance of isotope 2 x mass) / 100

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9
Q

atomic orbital

A

a region within an atom, around the nucleus, that contains up to two electrons with opposite spins

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10
Q

shell

A

a group of orbitals with the same principle quantum number

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11
Q

sub-shell

A

a group of the same type of orbitals in a shell

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12
Q

s sub-shell

A

orbital is spherical
consists of one orbital
can hold up to 2 electrons

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13
Q

p sub-shell

A

orbital is dumbell shaped
consists of 3 orbitals
can hold up to 6 electrons

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14
Q

d sub-shell

A

consists of 5 orbitals
can hold up to 10 electrons

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15
Q

f sub-shell

A

consists of 7 orbitals
can hold up to 14 electrons

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16
Q

aufbau (building-up) principle

A

electrons fill orbitals of lowest energy first
order of filling: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 4d10 4f14

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17
Q

why does 4s fill before 3d?

A

4s sub-shell has a lower energy than 3d sub-shell

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18
Q

blocks of the periodic table linking to electron structure

A

eg elements in s-block have their highest energy electron in an s sub-shell

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19
Q

common acid-base reactions

A

metal + acid -> salt + hydrogen
metal oxide + acid -> salt + water
metal hydroxide + acid -> salt + water
metal carbonate + acid -> salt + water + CO2
ammonia + acid -> ammonium salt

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20
Q

acid

A

proton (H+) donor

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21
Q

strong vs weak acids

A

a strong acid completely dissociates into its ions in aqueous solution
a weak acid partially dissociates into its ions in aqueous solution

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22
Q

base

A

proton (H+) acceptor

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23
Q

alkali

A

soluble base that releases OH- ions in aqueous solution

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24
Q

salt

A

produced when the H+ of an acid is replaced by metal or ammonium ions

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25
Q

mole

A

the amount of a substance containing as many particles as there are carbon atoms in 12g of carbon-12

26
Q

standard moles equation

A

moles (mol) = mass (g) / Mr (gmol-1)

27
Q

equation for number of particles

A

no. of particles = Na x moles
Na = avogadro’s constant 6.02 x 10^23

28
Q

percentage yield equation

A

% yield = actual yield / theoretical yield x 100

29
Q

atom economy equation

A

atom economy = Mr of desired product / total Mr of all products x 100

30
Q

concentration equation

A

moles (mol) = concentration (moldm-3) x volume (cm3) / 1000

31
Q

percentage uncertainty equation

A

% uncertainty = uncertainty / measurement x 100

32
Q

preparing a standard solution

A

1 - weigh the solid
2 - dissolve in a small amount of distilled water
3 - transfer the solution to a volumetric flask, rinse the beaker and add to the flask
4 - fill the flask with distilled water to the graduation mark
5 - invert the flask several times

33
Q

gas equation at RTP

A

moles (mol) = volume, v / molar gas volume, Vm
Vm = 24 in dm3 or 24000 in cm3

34
Q

ideal gas equation

A

pV = nRT
p = pressure (Pa)
V = volume (m3)
n = moles (mol)
R = 8.314
T = temperature (K)

35
Q

empirical formula

A

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

36
Q

molecular formula

A

actual number of atoms of each element present in a compound

37
Q

hydrated

A

when water of crystallisation is present in a crystal compound

38
Q

anhydrous

A

when all the waters of crystallisation have been removed from a compound

39
Q

oxidation

A

loss of electrons/increase in oxidation state

40
Q

reduction

A

gain of electrons/decrease in oxidation state

41
Q

oxidising agent

A

a reagent that oxidises (takes electrons from) another species, and is reduced itself

42
Q

reducing agent

A

a reagent that reduces (adds electrons to) another species, and is oxidised itself

43
Q

disproportionation

A

a reaction in which one element is both oxidised and reduced

44
Q

ionic bonding

A

electrostatic attraction between oppositely charged ions

45
Q

covalent bonding

A

strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonding atoms

46
Q

metallic bonding

A

strong electrostatic attraction between a lattice of cations and a sea of delocalised electrons

47
Q

properties of ionic compounds

A

high melting/boiling points
conduct electricity when molten or aqueous as the ions are free to move and carry charge
soluble in water

48
Q

dative covalent bond

A

a covalent bond where one atom supplies both of the electrons shared

49
Q

electron pair repulsion

A

electron pairs repel each other to get as far apart as possible
lone pairs repel more strongly than bonding pairs

50
Q

molecule with 2 bond pairs and 0 lone pairs

A

180°
linear

51
Q

molecule with 3 bond pairs and 0 lone pairs

A

120°
trigonal planar

52
Q

molecule with 4 bond pairs and 0 lone pairs

A

109.5°
tetrahedral

53
Q

molecule with 6 bond pairs and 0 lone pairs

A

90°
octahedral

54
Q

molecule with 3 bond pairs and 1 lone pair

A

107°
pyramidal

55
Q

molecule with 2 bond pairs and 2 lone pairs

A

104.5°
non-linear

56
Q

molecule with 2 bond pairs and 1 lone pair

A

117.5°
non-linear

57
Q

electronegativity

A

ability of an atom to attract the bonding pair of electrons towards itself in a covalent bond
most electronegative element is fluorine

58
Q

what are intermolecular forces?

A

attractive forces between molecules

59
Q

induced dipole-dipole forces

A

very weak intermolecular forces between molecules
exist in all molecules

60
Q

permanent dipole-dipole forces

A

weak attractive forces between polar molecules
stronger than induced dipole-dipole forces

61
Q

hydrogen bonds

A

exists between a Hδ+ atom in one molecule and a lone pair on a highly electronegative atom (O, N or F) on another molecule

62
Q

anomalous properties of water

A

ice is less dense than water as hydrogen bonds hold the H2O molecules apart in an open lattice structure
water has relatively high melting/boiling point due to strong hydrogen bonds between molecules

a level chemistry (19 decks)

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