Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

atomic number

A

number of protons in an atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

mass number

A

number of protons and neutrons in an atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

isotopes

A

atoms of the same element with different number of neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

equation for relative atomic mass

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

atomic orbital

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

shell

A

a group of orbitals with the same principle quantum number

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

sub-shell

A

a group of the same type of orbitals in a shell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

s sub-shell

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

p sub-shell

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

d sub-shell

A

consists of 5 orbitals
can hold up to 10 electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

f sub-shell

A

consists of 7 orbitals
can hold up to 14 electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

why does 4s fill before 3d?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

acid

A

proton (H+) donor

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

base

A

proton (H+) acceptor

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

alkali

A

soluble base that releases OH- ions in aqueous solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

salt

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
mole
the amount of a substance containing as many particles as there are carbon atoms in 12g of carbon-12
26
standard moles equation
moles (mol) = mass (g) / Mr (gmol-1)
27
equation for number of particles
no. of particles = Na x moles Na = avogadro's constant 6.02 x 10^23
28
percentage yield equation
% yield = actual yield / theoretical yield x 100
29
atom economy equation
atom economy = Mr of desired product / total Mr of all products x 100
30
concentration equation
moles (mol) = concentration (moldm-3) x volume (cm3) / 1000
31
percentage uncertainty equation
% uncertainty = uncertainty / measurement x 100
32
preparing a standard solution
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
gas equation at RTP
moles (mol) = volume, v / molar gas volume, Vm Vm = 24 in dm3 or 24000 in cm3
34
ideal gas equation
pV = nRT p = pressure (Pa) V = volume (m3) n = moles (mol) R = 8.314 T = temperature (K)
35
empirical formula
simplest whole number ratio of atoms of each element present in a compound
36
molecular formula
actual number of atoms of each element present in a compound
37
hydrated
when water of crystallisation is present in a crystal compound
38
anhydrous
when all the waters of crystallisation have been removed from a compound
39
oxidation
loss of electrons/increase in oxidation state
40
reduction
gain of electrons/decrease in oxidation state
41
oxidising agent
a reagent that oxidises (takes electrons from) another species, and is reduced itself
42
reducing agent
a reagent that reduces (adds electrons to) another species, and is oxidised itself
43
disproportionation
a reaction in which one element is both oxidised and reduced
44
ionic bonding
electrostatic attraction between oppositely charged ions
45
covalent bonding
strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonding atoms
46
metallic bonding
strong electrostatic attraction between a lattice of cations and a sea of delocalised electrons
47
properties of ionic compounds
high melting/boiling points conduct electricity when molten or aqueous as the ions are free to move and carry charge soluble in water
48
dative covalent bond
a covalent bond where one atom supplies both of the electrons shared
49
electron pair repulsion
electron pairs repel each other to get as far apart as possible lone pairs repel more strongly than bonding pairs
50
molecule with 2 bond pairs and 0 lone pairs
180° linear
51
molecule with 3 bond pairs and 0 lone pairs
120° trigonal planar
52
molecule with 4 bond pairs and 0 lone pairs
109.5° tetrahedral
53
molecule with 6 bond pairs and 0 lone pairs
90° octahedral
54
molecule with 3 bond pairs and 1 lone pair
107° pyramidal
55
molecule with 2 bond pairs and 2 lone pairs
104.5° non-linear
56
molecule with 2 bond pairs and 1 lone pair
117.5° non-linear
57
electronegativity
ability of an atom to attract the bonding pair of electrons towards itself in a covalent bond most electronegative element is fluorine
58
what are intermolecular forces?
attractive forces between molecules
59
induced dipole-dipole forces
very weak intermolecular forces between molecules exist in all molecules
60
permanent dipole-dipole forces
weak attractive forces between polar molecules stronger than induced dipole-dipole forces
61
hydrogen bonds
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
anomalous properties of water
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)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions