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chemistry textbook knowledge > LEARN BEFORE EXAM > Flashcards

LEARN BEFORE EXAM Flashcards

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1
Q

v (3+)

A

GREEN

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2
Q

mno4-

A

purple

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3
Q

mno4 (2-)

A

green

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4
Q

cr2o7 2-

A

orange

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5
Q

vo2 (+)

A

yellow

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6
Q

vo (2+)

A

blue

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7
Q

ti (3+)

A

purple

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8
Q

v (3+ )

A

green

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9
Q

cr (3+)

A

violet

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10
Q

fe (3+)

A

yellow

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11
Q

ti (2+)

A

violet

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12
Q

v (2+)

A

violet

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13
Q

mn (2+)

A

PALE pink

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14
Q

fe(2+)

A

PALE green

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15
Q

co (2+)

A

pink

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16
Q

ni (2+)

A

green

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17
Q

cu (2+)

A

PALE blue

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18
Q

interconversion between fe2+ and fe 3+

A

fe 2+ ( pale green) oxidised to fe 3+ (yellow) by ACIDIFIED POTTASIUM MANGANATE SOLUTION

fe 3+ reduced to fe 2+ by IODIDE IONS

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19
Q

interconversion between cr 3+ and cr2o7 2-

A

cr 3+ in (cr(oh)6) 3- DARK GREEN) oxidisied to cro4 2- (YELLOW) by WARMING with HYDROGEN PEROXIDE solution in ALKALINE conditions

add dilute sulfuric acid to chromate solution—> orange dichromate solution (cro4(2-) + 2h(+) –> cr2o7 (2-) + h2o

cr2o7(-) (orange) REDUCED to cr (3+) by ACIDIFIED zince

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20
Q

reduction of cu 2+ and disproportionation of cu+

A

cu(2+) (pale blue) reduced to white CUI precipitate by IODIDE IONS .(2cu (2+) + 4I- —> 2cui + i2

NOTE: precips are ALWAYS SOLid

cu+ is unstable and disporportionates to cu and cu 2+

2cu + (aq)—> cu (s) + cu (2+)

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21
Q

test for co3 2-

A

add nitric acid , bubble gas released through limwewater, cloudy in presence of co2

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22
Q

test for so4 2-

A

add barium nitrate or baroium chloride, white precip formes ( baso4)

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23
Q

test for nh4+

A

cold naoh to compound and warm. hold damp red litmus paper over, red litmus–> blue `

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24
Q

transition metals as catalysts

A

fe- haber process
v2o5- contact process ( 2so2(g) + o2 reversible sign 2o3)

NOTE : HABER AND CONTACT ARE REVERSIBLE REACTIONS

hydrogenation o vegetable fats- nickle catalyst

decomposition of hydrogen peroxide to water and oxygen- mno2 catalyst (manganese V) oxide)

reaction of zinc with acids- cu2+ catalysts

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25
Q

pyramidal bond angle

A

107 (1 lone pair, and 3 ligands)

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26
Q

non linear bond anglw

A

104.5 ( two lone pairs and 2 ligands

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27
Q

trigonal planar

A

120

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28
Q

otctahedral

A

90

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29
Q

ammonium ion shape

A

tetrahedral- 109.5

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30
Q

co3 2- ion shape

A

trigonal planar (120)

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31
Q

no3 - ion shape

A

trigonal planar (120)

32
Q

so4 2- ion shape

A

tetrahedral (109.5)

s

33
Q

formation of idnuced dipols

A

movemment of e- produces changong dipole ,and instantaneous dipole is made, this induces dipole on neighbouring molecule, induced dipole induces more dipoles on neighbouring molecuels

34
Q

how does something dissolve

A

intermolecular forces between the water and the lattice is stronger than intermolecular forces within the lattice so intermolecular forces between lattice break

polar substance have polar bonds (eg oh) so they dissolve In polar substances. cant dissolve in non polar as the intermolecular forces within lattice are too strong.

ONLY SIMPLE MOLECULAR SUBSTANCES ARE SOLUBLE (EG H20, H2 , CO2 , NE )

35
Q

why water has high bp

A

hydrogen bonds , lots of energy needed

36
Q

water high surface tension and viscosity

A

insects can walk

37
Q

factors affectiing ionisation energy

A

atomic radius, nuclear charge, electron shielding ( inner electron repel outer)

38
Q

ionisation energy acros period

A

increased nuclear charge, same shell= similar shielding, nuclear attraction incerease, atomic radius decrease, first ionisation energy increases

39
Q

berylium and boron

A

2p subshell filling . 2p in boron has higher energy than 2 in beryllium o 2p easier to remove than 2s

40
Q

nitrogen and oxygen

A

oxyen has 1 pair of electrons in 2p subshell, repulion= easier to remove

41
Q

giant covalent lattice

A

non soluble in solvents

42
Q

fall in melting points across period 3 at group 15

A

giant structures to simple

43
Q

group 2oxides + water

A

oh- ions released (cao +h2o–> ca 2+ + 2oh-) alkaline SOLUTION FORMED

.group 2 hydoxides only slightly soluble in water , saturation causes precipitate.

44
Q

group 2 hydroxides and water

A

precipitate forms, ca 2+ + oh- –> ca(oh)2 (s)

45
Q

bromine, iodine, chlorine

A

orange, purple , pale green (dissolve in cyclohexane as its easier to see )

46
Q

outer shell of halogens

A

s2p5

47
Q

cl2 + h2o

A

hclo + hcl

48
Q

cl2 + 2Naoh

A

naclo + nacl + h2o (naclo is bleach)

49
Q

agx

A

SOLID

50
Q

Carbonate + acid

A

co2 in LIMEWATER

51
Q

Sequence of halide tests

A

carbonate, sulfate, halide

carbonate ions present in halide tet; ag2 co3

sulfate; ag2so4 precipitate

52
Q

test for a mixture of ion

A

carbonate test, see bubbles, continue adding dilute nitrc acid until bubbling tops , all carbonate ions removed, move to next test (use nitric acid as sulfuric acid and hcl contain sulfate and cl- which interfere )

.sulfate test: to soluton left, add excesss ba (no3)3 , barium suflate precip formes, filter and remove

halide test: to solution left from sulfate test, ad silver nitrate , carbonate nad sulfate ions revmoved so no wrong precip fomred,

,add nh3 to confirm halide ( differentiate colours )

53
Q

enthaloy change of reaction

A

enthalpy change that accompanies reaction in olar qiuantities shown in chemical equation under standard conditions

54
Q

enthalpy of combustion

A

enthalpy change takes place when 1 mol of substance reacts COMPLETELY with oxygen UNDER STANDARD CONDITIONS

55
Q

nthapy of foormation balancing

A

balance so that ONE MOLE of product present

56
Q

enthalpy of neutralisation

A

energy change that accompanies reaction of acid by base to form ONE MOLE of water under standard conditions

57
Q

accuracy of experimental value of combustion

A

heat loss
to surroundings

.incomplete meth combustion, evaporation of meth from wick

. non standard condition

58
Q

average bond enthalpy

A

energy required to break of bonds in a gaseous molecule

59
Q

altering rate of reaction by

A

changing surface area of solid reactants

60
Q

catalyst

A

not used up in chemical reaction , forms intermediate, regenerated

61
Q

heterogenous catalysts

A

differnet physical state, adsorbed, solids, work b adsorption and desorption

62
Q

catalysts, sustainability and economic importance

A

indrease rate of reactions by lowring activation energy

.decreases temp needed

.less electricity or fossil fuel used

.allows operating processes with high atom economies and fewer pollutants

63
Q

boltzmann

A

orgin, end doesnt meet x axis as no max energy, area under curve remains same as no of molecules is same .

use “ molecules” NOT “particles !”

64
Q

catalyst in boltzmann

A

reduces ea but DONT draw two curves

65
Q

explanation of dynamic equillibrium

A

exists
in a closed system when the rate of the forward
reacton is equal to the rate of the reverse
reacton and the concentratons of reactants and
products do not change

66
Q

investigating eq with concentration

A

(yellow) 2cro4 (2-) + 2H+ (reversible sign) cr2o72- + h2 (orange)

add acid- eq shifts right

add base, eq shifts left, yellow colour

(SAME AS ACID BASE EQUILLIBRIUM !!)

67
Q

Investigating eq with temp

A

. dissolve cobalt chlriide in water ,add hcl , plaec in iced water, pink colour

.set up boiling awter, add the boiling tube , solution = blue colour

. put solution back, solution= pink colour

(reaction is co(h2o)6 complex wiht 4 cl-, cocl4 2- is blue!)

68
Q

kc of 1, less than 1, more than 1

A

eq , more than 1, eqi shifted to produces, eq less than 1 eq shift to reactants

69
Q

increasing temperature

A

increases the rate constant

70
Q

pv= nrt UNITS

A

Pressure=pa , volume= M3 , ideal gas constant = 8.32 jmol-1 k-1, temperature is in KELVIN, amount of gas is in MOLES

71
Q

percentage yield is in… and atom economy in…

A

moles, molar mass of product/ reactamts

72
Q

rate constant

A

derived from GRADIENT of a rate/ concentration graph

73
Q

balancing equations for enthalpy of formation

A

make sure that it FORMS ONE MOLE

note: metals are in solid state !!!!!!!!!!!!!!!!!!!

74
Q

enthalpy of formation of element

A

formation of one mole of element from its element

75
Q

standard enthalpy of reaction, formation, combustion and neutralisation

A

. enthalpy change that accompanies a reaction in molar quantitites shown in a chemical equation under standard condition with all reatants and products in standard states

.enthalpy change takes palce when 1 mole of compound is formed from its elements udner standard conditions with all reactants and products in standard tates

..enhtalpy change that takes place when one mole of substance react completely with oxygen under standard condition with all reactants and products in standard states

.enthalpy chnage that ACCOMPANIES reaction of acid by base to form one mple pf h2o under standard condtitions with all reactants and prdoucts n standard states

76
Q

advantages and disadvantages of fuel cells

A

advantages:
only H2O formed/ non-polluting
greater efficiency (1) EMPHASIS ON GREATER EFFICIENCY

disadvantages:
H2 difficult to store (1)
H2 difficult to manufactured initially /
limited life cycle of H2 adsorber/absorber

77
Q

homogenous equillibria

A

include h2o

DO NOT INCLUDE IN HETERO!

chemistry textbook knowledge (8 decks)

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