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AS Inorganic Chemistry > AS Chemistry > Flashcards

AS Chemistry Flashcards

1
Q

isotope

A

each atom of element has same no of protons, different number of neutrons

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2
Q

mass number

A

total number of protons and neutrons

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3
Q

atomic number

A

number of protons,

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4
Q

ammonium

A

nh+4

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5
Q

hydrogencarbonate

A

hco3-

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6
Q

manganate

A

mno4-

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7
Q

dichromate

A

cr2o7-2

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8
Q

phosphate

A

PO4-3

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9
Q

relative isotopic mass

A

the mass of an atom of an element relative to one twelfth of the mass of an atom of carbon-12

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10
Q

one mole

A

amount of substance, contain same no of particles as 12g of carbon 12.

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11
Q

no of moles

A

no of things/6.02x10^24

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12
Q

yield

A

actual/max theroticaly

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13
Q

why is yield never 100%

A

side reactions can occur
reactions may not be complete
reaction can be reversible.

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14
Q

atom economy

A

desired product mR/sum of Mr of all

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15
Q

gases at room temp

A

mol x 24dm^3

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16
Q

if not at room temp

A

pV=nRT

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17
Q

standard solution

A

solution of known concentratiion, made in voncial flasks

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18
Q

how do you prepare a standard solution?

A

1)zero balance and weigh mass to small beaker
2)dissolve in small amount of distilled water.
3)using funnel, transfer to volumetric flask,
4)rinse with distilled water, and make it to the line.

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19
Q

concentration

A

moles/volume of solution.

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20
Q

acids

A

proton donors
can be strong/weak depending on dissociation.

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21
Q

bases

A

protons acceptors
some are soluble, and release OH

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22
Q

acid+metal

A

salt+water

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23
Q

acid+metal hydroxide

A

salt+water

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24
Q

acid+metal carbonate

A

salt+water+co2

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25
Q

hydrous salt

A

salt containing water, which is heated to release.

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26
Q

oxidiation number

A

pure elements=0
flurione=-1, O=+2
oxygen=.2, peroxides=-1
Cl=-1, Fl or O=1

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27
Q

disproportion reaction

A

same reaction is oxidised and reduced

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28
Q

oxdising agent

A

gets reduced
electron acceptors

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29
Q

reducing agent

A

gets oxidised
reduction of others

30
Q

ionic bonding

A

metals and non mentasl

31
Q

structure of ionic

A

giant ionic lattice need large amount of energy to overcome electrostatic forces.
electron conductivty as can conduct when molten as particles are mobile.

32
Q

covalent bonding

A

happens between non metals
electrostatic attraction between shared pair of electrons and nuceli of bonded atoms.

33
Q

dalative covalent

A

involve share pair of electrons, where only one pair supplies electrons.

34
Q

linear

A

2 bond pairs=180

35
Q

trignoal planer

A

3 bond pairs=120

36
Q

bent

A

2 bond, and 1 lone-117.5

37
Q

tetracadal

A

4 bond paairs=109.5

38
Q

pyramdial

A

3 bond and 1 lone=107

39
Q

octacherdal

A

6 bond=90

40
Q

london forces

A

electron density is uneven, so temp dipole. more electrons=stronger induced dipole so is stronger.
happens in all molecules, only intermolecular between non polar.

41
Q

permanent dipole

A

occur between polar molecules
opposite ends of each pole attract each other.

42
Q

hydrogen bonds

A

lone pair attracted to H+

43
Q

polar

A

different electronegativty, +-more share.

44
Q

polar-has to be any of these

A

different molecules
central has a lone pair.

45
Q

polar

A

not symmetrical
bonds dont cancel.

46
Q

first ionisation energy

A

energy required to remove any electron from each atom in mole of gaseous to form +1 ions.
x->x+e

47
Q

nuclear charge

A

more protons, more attraction so electron removed

48
Q

atomic radius

A

larger atomic weaker nucleus attraction

49
Q

electron shielding

A

electrons

50
Q

ionisation energy increases due to

A

large atomic
greater shielding
Higher nuclear(this is outweighed by other 2)

51
Q

dips in Al and P

A

due to change in subshell.
and less energy, as due to less repulsion, from orbital of 2 then one.

52
Q

period 2 is higher ionisation energy

A

dip for boron=higher sub shell
0=first paired electron

53
Q

period 2 melting points

A

Li and Be
decrease in ionic radius
more delocalised electrons
B and C
b=3 covalent bonds
c=4 covalent
N, O, F, Ne needs less energy to break forces

54
Q

group 2

A

lose electrons to form 2+
reducing agents
reactivity increases as go down
antacids
neutralise soils

55
Q

group 2=reactivity increases as go down

A

increase of atomic
more shielding
less attraction
electrons lost easily

56
Q

halogens

A

solid=simple covalent lattices
f2=pale yellow
c2=pale green
br2=red brown
i2=shiny gra

57
Q

why does oxidising decrease as you go down

A

higher atomic
higher shielding
weaker attraction

58
Q

test of chlorine

A

add small of dilute nitric acid, to remove carbonate. add silver nitrate=white
bromine-cream
iodine=yellow

59
Q

bond enthalpy

A

one mole of covalent bond broken in gas state.

60
Q

enthalpy change

A

bonds broken-bonds formed

61
Q

hess law

A

if reaction can take place by two routes, enthalpy is same.
Formation=products-reactants
Combustion=reactants-products.

62
Q

enthalpy change of neutrallisation

A

enthalpy change for reaction between acid and base to produce one mole of water under standard conditions.

63
Q

enthalpy change

A

heat change at constant pressure
One mole of covalent bonds broken in gas state

64
Q

formation

A

one mole of compound formed from constituent elements in standard states and conditions.

65
Q

combustion

A

one mole of substance in standard states burned in excess of O2 under standard conditions.

66
Q

collision theroy

A

particles must collide for reactions to occur.
need
=correct oreniation
sufficent energy

67
Q

dynamic equillbrium

A

reactants to products
closed
same concentration
factors = pressure, temperature, and concentration

68
Q

temperatyre

A

+ endothermic=increase temp favours
- exothermic=decrease temp favours

69
Q

test for ammonium

A

add NaOH=warm
test with damp red litmus should go blue

70
Q

test for carbonate

A

add dilute acid, should be efferceveness

71
Q

test for sulfate

A

add barium nitrate, and white

72
Q

order for tests

A

carbonate, sulfide, halidie

AS Inorganic Chemistry (1 decks)

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