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P Block > Group 16: Calcogens > Flashcards

Group 16: Calcogens Flashcards

1
Q

compare I.E. group 16 and group 15 (group 16)

A

group 16 < group 15

half filled

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2
Q

minimum EA (group 16)

A

O

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3
Q

maximum EA (group 16)

A

S

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4
Q

highest catenation (group 16)

A

S

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5
Q

minimum oxidation state (group 16)

A

-2

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6
Q

maximum oxidation state (group 16)

A

+6

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7
Q

stability of which OS decreases down the group due to inert pair effect? (group 16)

A

+6 decreases and +4 increases

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8
Q

allotropes of oxygen(group 16)

A

ozone

oxygen

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9
Q

allotropes of sulphur (group 16)

A 
rhombic sulphur(alpha)
monoclinic sulphur (beta)
plastic sulphur (delta)
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10
Q

general molecule on reaction with H2(group 16)

A

H2E

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11
Q

trend of BP on H2E (group 16)

A

H2S< H2Se < H2Te < H2O (H- bonding)

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12
Q

acidic strength of H2E (group 16)

A

increases down the group

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13
Q

bond energy H2E (group 16)

A

decreases down the group

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14
Q

Bond angle H2E (group 16)

A

decreases down the group due to Drago’s rule

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15
Q

thermal stability of H2E (group 16)

A

decreases down the group

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16
Q

general compound with oxygen (group 16)

A

EO3 and EO2
oxidation state directly proportional to acidic nature
EO3 > EO2

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17
Q

reducing nature of oxide(Group 16)

A

decreases down the group

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18
Q

General compound with halides (Group 16)

A

EX2 / EX4 / EX6

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19
Q

stability of halide (Group 16)

A

F > Cl> Br > I

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20
Q

only __ hexa halide is stable and exist in gaseous state (Group 16)

A

Flourids

due to bulkiness

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21
Q

Se2Cl2 show disproportionation like (Group 16)

A

SeCl4 + Se

other dimer also show such reaction

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22
Q

preparation of dioxygen (Group 16)

A
  1. factional distillation
  2. electrolysis of acidified water
  3. decomposition of oxides
  4. photosynthesis
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23
Q

catalyst in decomposition of H2O2 (Group 16)

A

MnO

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24
Q

chlorate (Group 16)

A

ClO3-

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25
Q

catalyst for deacon’s process (Group 16)

A

CuCl2

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26
Q

catalyst for contact process (Group 16)

A

V2O5

27
Q

neutral oxides (Group 16)

A

NO N2O CO H2O

28
Q

metals that form amphoteric oxides (Group 16)

A

Al , Sn , Ga, Be , Sb , Pb, Cr

29
Q

example of acidic oxides that are formed by metals (Group 16)

A

Mn2O7, CrO3, V2O5

metal with high OS

30
Q

suboxide (Group 16)

A

-2

carbon suboxide C3O2

31
Q

colour of O3(Group 16)

A

Gas : pale blue
liquid : dark blue
solid : violet-blue

32
Q

condition for preparation of O3 from O2 (Group 16)

A

silent electric discharge

33
Q

ozone show bleaching property by (Group 16)

A

oxidation

34
Q

fuel used by supersonic jets (Group 16)

A

NO

35
Q

NO +O3 (Group 16)

A

NO2 +O2

36
Q

structure of S8 (Group 16)

A

crown like (W)

37
Q

alpha and beta sulphur is soluble and insoluble in (Group 16)

A

soluble in CS2 and insoluble in H2O

38
Q

alpha stable under _ C (Group 16)

A

96

39
Q

beta stable above _ C(Group 16)

A

96

40
Q

at high temperature sulphur exist as (Group 16)

A

S6 and in vapour state even at S2

41
Q

sulphite(SO3 2-) salt + H2SO4 (Group 16)

A

SO2 + H2O

42
Q

FeS2 + O2(Group 16)

A

Fe2O3 + SO2

43
Q

why do lime water turns milky on adding CO2 to it

A

CaCO3

44
Q

on adding excess CO2 to calcium carbonate

A

Ca(HCO3)2 colourless

45
Q

sodium bisulphide(Group 16)

A

NaHSO3

formed on passing excess CO2 to sodium suphide

46
Q

SO2 show bleaching property by (Group 16)

A

reducing nature

47
Q

SO2+ Cl2 (Group 16)

A

SO2Cl2

48
Q

SO2Cl2 (Group 16)

A

sulphuryl chloride

49
Q

preparation method for H2SO4(Group 16)

A

Contact process

50
Q

catalytic oxidation of SO2 is favored by (Group 16)

A

low temperature

51
Q

S +O2 (Group 16)

A

SO2

52
Q

SO2 + O2 (Group 16)

A

in presence of V2O5

SO3

53
Q

fuming sulphuric acid

A

oleum H2S2O7

54
Q

chemical reactions ofH2SO4(Group 16)

A
  1. low volatility
  2. dehydrating agent
  3. oxidizing agent
  4. acid- base
55
Q

structure of peroxodisulphuric acid (group 16)

A

H2S2O8

56
Q

structure of pyrosulphuric acid (group 16)

A

H2S2O7

57
Q

structure of thiosulphuric acid (group 16)

A

H2S2O3

58
Q

structure of peroxomonosulphuric acid (group 16)

A

H2SO5

59
Q

structure of pyrosulphurous acid (group 16)

A

H2S2O5

60
Q

structure of dithionic acid (group 16)

A

H2S2O6

61
Q

structure of dithionus acid (group 16)

A

H2S2O4

62
Q

structure of polythionic acid (group 16)

A

H2SnO6

n varies from 2 to 5

63
Q 
H2S2O3
H2S2O4
H2S2O5
H2S2O6
H2S2O7
H2S2O8
 (group 16)
A 
H2S2O3 - thiosulphuric acid
H2S2O4 - dithionus acid
H2S2O5 - disulphurous acid
H2S2O6 - dithionic acid
H2S2O7 - pyrosulphuric acid ( fuming sulphuric acid )
H2S2O8 - peroxodisulphuric acid
64
Q

H2SO4
H2SO3
H2SnO6
(group 16)

A

H2SO4 - sulphuric acid
H2SO3 - sulphurous acid
H2SnO6 - polythionic acid

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