exam Flashcards

1
Q

primary standard solution

A

a solution containing one solute, prepared by dissolving a known mass of that solute in a known volume of water. As a result the concentration is known accurately

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2
Q

primary standard

A

a substance that can be prepared pure and dissolved in water to make a solution whose concentration is accurately known

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3
Q

where are the strongest oxidants on the electrochemical series

A

top left (at cathode)

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4
Q

rules for ox number

A

F = -1
H to non-metals is +1, H to metals is -1
Oxygen in peroxides is -1

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5
Q

salt bridge function

A

contain free-moving unreactive ions that keep polarity/charge constant

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6
Q

cell potential

A

E (cathode) - E (anode)

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7
Q

water properties

A

high latent heat
high specific heat capacity
high melting and boiling point
universal sovent

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8
Q

why does water expand upon freezing

A

as cools, molecules slow down and water adopts more regular lattice bc rigid H bonds bw molecules
this -> hexagonal lattice as ice pushes molecules further apart vs liquid form, expanding liquid water
tf same no of molecules occupy larger space and ice has a lower density

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9
Q

latent heat of fusion

A

nrg required to convert 1 mol of substance from s to l at its melting point

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10
Q

latent heat of vaporisation

A

nrg required to convert 1 mol of substance from l to g as it’s boiling point

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11
Q

specific heat capacity

A

amount of nrg required to raise the temp of 1g of substance by 1 degree C
Q=mcAT

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12
Q

process of dissolving

A

forces being formed need to be approximately the same strength or stronger than forces being broken
“bonds being formed are weaker than those that were broken tf immiscible”

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13
Q

insoluble ions

A

halides w Ag, Pb, Hg
SO4 w Pb or Ba
O, S, CO3, PO4 except for G1
OH except G1, Ba or Ca

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14
Q

ppm

A

mg/L or ug/g

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15
Q

w/w%
w/v%
v/v%

A

g/g
g/mL
mL/mL

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16
Q

crystallisation

A

solid crystals form as temp decreases and the solute can no longer remain dissolved. the slower the cooling, the bigger the crystals

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17
Q

Kw - ionic product of water

A

[OH][H3O] = 10 ^-14

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18
Q

ph

A

-log [H]; 14 + log[OH]
10 ^-pH; 10 ^pH-14

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19
Q

assumption with diprotic acids

A

assume all molecules eg H2SO4 dissociate and all hydrogen ions contribute to pH

20
Q

Ka (weak acids)

A

[H+]^2 / [acid]

21
Q

collision theory

A

for a chemical reaction to occur, reactant particles need to collide with sufficient nrg and the correct orientation

22
Q

factors affecting the rate of reaction

A

increase fq of successful collision:
SA of solid
concentration of solution
pressure (by decreasing volume)(Boyle’s law)
increase proportion w nrg > = Ea
temperature
catalysts (reduce Ea)

23
Q

dynamic equilibrium

A

rate of forward reaction = rate of reverse reaction

24
Q

Le Chatelier’s Principle

A

system at equilibrium has a tendency to partially oppose a change

25
orbital
region of space in which up to 2 e are likely to be located. Orbitals may also be empty
26
Pauli's Exclusive Principal
a max of 2 e in a given orbital of opposite spins
27
Hund's Rule of Maximum Multiplicity
every orbital in a sub shell is half-filled before any orbital in that subshell is filled
28
Aufbai=u Principal
subshells are filled in order from lowest to highest nrg
29
electron configuration exceptions
Chromium and Copper
30
cc
measure of net attractive force felt by valence e towards the nucleus protons- inner shell e
31
electronegativity
strength with which atoms of an element attract electrons when they are chemically combined with another element
32
ionisation nrg
amount of nrg required to remove an electron from 1 mol of a gaseous atom
33
mettalic bonding
electrostatic force of attraction in lattice between sea of delocalised e and positively charged cations
34
covalent bonding
shared pair of e bw two non-metal ions
35
dative covalent bond
both of shared electrons are contributed by one atom only
36
fuel
substance that burns in air or oxygen to release a usable amount of nrg
37
substitution reaction (alkanes)
UV light
38
haloalkane + OH -->
alcohols
39
alkene + hydrogen
Ni catalyst + 150C
40
alkene + water
(steam) H3PO4, 300C, 60-70atm
41
thermoplastic
no cross-links chains loosely tangled together low mp can be remoulded eg plastic bags/cling wrap
42
thermosetting
cross-link bw chains rigid and inflexible X be remoulded eg kitchen bench cover
43
elastomers
can be stretched/deformed retain their shape few cross-links
44
polymerisation
under pressure w catalyst
45
LDPE
Low density polyethene: high temp and pressure amorphous (branched chains that don't fit well) low mp soft and flexible eg carrier bags, plastic wrap
46
HDPE
high density polyethene: cataylst at lower temp unbranched chains that fit together more cyrstalline and less amorphous eg wheelie bins. classroom chairs