Inorganic > 16th Group > Flashcards

16th Group Flashcards

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1
Q

Common electronic configuration

A

ns2 np4

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2
Q

Valences

A

2 & 4 (but O differs)

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3
Q

What are the metallic characters of 16th group elements

A

O and S are non-metals

Se, Te, Po show both metal and non-metal characters

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4
Q

What is the only element in 16th group which exists in gaseous state?

A

O

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5
Q

Oxidation states

A

Except O, other elements in the group can form even numbered oxidation states from -2 upto +6

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6
Q

What are the 16th group hydrides?

A

H2O
H2S
H2Se
H2Te

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7
Q

2 allotropic forms of oxygen

A

O2 and O3

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8
Q

Describe O3

A

Ozone is a light blue colored (colorless) gas with a pungent odor

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9
Q

What special properties does O3 have due to its ability to produce atomic oxygen?

A
  1. Oxidizing agent
  2. Reducing agent
  3. Disinfecting agent
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10
Q

Describe O2

A

O2 is colorless, and odorless

Slightly water soluble

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11
Q

How is O2 prepared in the laboratory?

A

Catalytic decomposition of KClO3

KClO3 ———-> KCl + O2

(heating with MnO2 or Pt)

Catalytic decomposition of H2O2

H2O2 ——-> H2O + O2

(heating with MnO2)

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12
Q

How is O2 produced industrially?

A

By fractional distillation of liquid air

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13
Q

What is the most widely used solvent?

A

water

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14
Q

Show the ionization of H2O

A

2H2O —> OH- + H30+

revers.

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15
Q

Show water’s reactions with acids and bases

A

NH3 + H2O —> NH4+ + OH-

HCl + H20 —–> Cl- + H3O+

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16
Q

water’s reaction w bases

A

NH3 + H2O —> NH4+ + OH-

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17
Q

water’s reaction w acids

A

HCl + H20 —–> Cl- + H3O+

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18
Q

Why is water considered amphiprotic?

A

It can either donate or accept a proton

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19
Q

Decomposition of H2O2 in sunlight

A

H2O2 —>H2O + O2

So, H2O2 is usually stored in brown or black colored bottles

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20
Q

Describe H2O2

A
  • viscous, colorless liquid
  • compared to water, MP, BP and density higher. This is due to presence of OH groups
  • Due to excess mass, comparatively stronger London forces are also possible.
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21
Q

How does H2O2 release atomic oxygen

A

H2O2 —-> H2O + O

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22
Q

uses of H2O2

A

Oxidizing agent
Disinfecting agent
Bleaching agent
Reducing agent
Used as a rocket fuel

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23
Q

Properties of H2O2

A
  1. Oxidizing agent
  2. Reducing agent
  3. Antiseptic agent
  4. Bleaching agent
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24
Q

How does H2O2 react as an oxidizing agent?

A
  1. with acidified iodide ions

H2O2 —> H2O
I- —> I2

  1. Reaction with Fe2+ ions

H2O2 —> H2O
Fe2+ —> Fe3+

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25
How does H2O2 react with acidified iodide ions
1. with acidified potassium ions H2O2 ---> H2O I- ---> I2
26
How does H2O2 react with Fe2+ ions
2. Reaction with Fe2+ ions H2O2 ---> H2O Fe2+ ---> Fe3+
27
How does H2O2 act as a reducing agent?
1. Reaction w/ acidified KMnO4 MnO4- -----> Mn2+ violet colorless H2O2 ---> O2 2. Reaction w/ acidified K2Cr2O7 Cr2O72- ----> Cr3+ orange green H2O2 -----> O2 3. Reaction w/ MnO2 MnO2 --> Mn2+ brown colorless H2O2 ---> O2
28
Reaction of H2O2 w/ MnO2
MnO2 --> Mn2+ brown colorless H2O2 ---> O2
29
Reaction of H2O2 w/ acidified K2Cr2O7
Cr2O72- ----> Cr3+ orange green H2O2 -----> O2
30
Reaction of H2O2 w/ acidified KMno4
MnO4- -----> Mn2+ violet colorless H2O2 ---> O2
31
Describe Sulphur
- has a high ability to produce chain structures/cyclic structures by joining sulphur atoms together by single bonds - so, it can form a higher no. of allotropic forms - they can be classified into 2 main types: crystalline sulphur and non-crystalline sulphur - crystalline sulphur: rhombic s. (alpha s.) and monoclinic s. (beta s.) - amorphous sulphur: plastic s. and colloidal s
32
2 types of S
crystalline sulphur non-crystalline sulphur
33
2 types of crystalline sulphur
rhombic s. (alpha s.) and monoclinic s. (beta s.)
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2 types of non-crystalline sulphur
plastic s. and colloidal s
35
How are crystalline sulphur formed?
s8 rings
36
What's the most stable form of crystalline sulphur?
Rhombic sulphur (stable below 95C)
37
When is monoclinic sulphur stable?
Above 95C
38
How can monoclinic s. be prepared?
by cooling molten sulphur slowly
39
another name for colloidal sulphur
milk of sulphur
40
Oxidation no.s of sulphur
-2 to +6
41
show reducing reactions of s
S + O2 ---> SO2 S + hot conc. H2SO4 ----> SO2 + H2O S+ hot conc. HNO3 -----? H2SO4 + NO2 + H2O
42
disproportioning of S
S + NaOH ------> Na2S + Na2S2O3 + H2O
43
uses of sulphur
- good fungicide - manufacturing medicinal drugs for skin diseases - used in sulphuric manufacturing process - used in rubber vulcanization
44
Oxoacids of S
H2SO4 H2S H2S2O3
45
Describe H2SO4
Strong, diprotic acid
46
How is H2SO4 produced?
SO3 + H20 ------> H2SO4
47
ionization of H2SO4
H2SO4 + H2O ------> HSO4- + H3O+ HSO4- + H20 -------> SO42- + H3O+
48
Properties of H2SO4
Dil. H2SO4 ----> STRONG ACID CONC. H2SO4 ------> STRONG OXIDIZING AGENT STRONG DEHYDRATING AGENT
49
Show H2SO4 reactions as a strong acid
H2SO4 + 2H2O ----> SO42- + H3O+ dil. H2SO4 acts as a strong acid and gives 2 protons as above
50
H2SO4 reactions as a strong oxidizing agent
1. reactions w/ metals Mg + conc. H2SO4 ---------> MgSO4 + SO2 + H2O Cu + conc. H2SO4 --------> CuSO4 + SO2+ H2O 2. reactions w/ non-metals S + Conc. H2SO4 --------> SO2 + H2O C + conc. H2SO4 ---------> CO2 + SO2 + H2O
51
Reactions of H2SO4 with metals
Mg + conc. H2SO4 ---------> MgSO4 + SO2 + H2O Cu + conc. H2SO4 --------> CuSO4 + SO2+ H2O
52
Reactions of H2SO4 with non-metals
S + Conc. H2SO4 --------> SO2 + H2O C + conc. H2SO4 ---------> CO2 + SO2 + H2O
53
Why does H2SO4 have a dehydrating property?
It has the ability to remove H and O in a 2:1 ration from a compound
54
reactions of H2SO4 as a dehydrating agent
C6H12O6 ----------> 6C + 6H2O C2H5OH -------> C2H4 + H2O in presence of conc. H2SO4
55
Describe H2SO3
- weak, diprotic acid - Reactions of SO2 w/ water makes H2SO3 - unstable - can dissociate into SO2 + H2O
56
Describe H2S2O3
- acid unstable, but salts of H2S2O3 are stable - It can decompose as below H2S2O3 + H2O ----> S + SO2 + H2O Na2S2O3 + HCl --------> NaCl + S + SO2 + H2O
57
How does H2S2O3 help iodometric titrations
S2O32- ion can act as a reducing agent. I2 + S2O32- -------> I- + S4O62-
58
Describe H2S
- Colorless, toxic gas with odor of rotten eggs - Weakly acidic - H2S burns in air with a blue flame to give H2O and SO2
59
Preparation of H2S
Reaction of a metal sulphide with a strong acid FeS + HCl ------> H2S + FeCl2
60
Identification of H2S
When H2S is allowed to pass through a filter paper moistened with Pb(CH3COOH) it turns black due to formation of PbS Pb(CH3COOH) + H2S ---> PbS + CH3COOH We can also use Pb(NO3)2, AgNO3 and CuSO4 for this Pb(NO3)2 + H2S ------> PbS + HNO3 AgNO3 + H2S -------> Ag2S + HNO3 CuSO4 + H2S ------> CuS + H2SO4
61
Reactions of H2S identification
Pb(CH3COOH) + H2S ---> PbS + CH3COOH Pb(NO3)2 + H2S ------> PbS + HNO3 AgNO3 + H2S -------> Ag2S + HNO3 CuSO4 + H2S ------> CuS + H2SO4
62
Properties of H2S
1. Boiling point of H2S is less than H2O 2. H2S EXISTS AS A GAS while water exists as a liquid at room temperature 3. Acidic character 4. Oxidizing character 5. Reducing character 6. Forms salts with bases
63
Why is boiling point of H2S < H2O
H2O has O-H bonds while H2S has S-H bonds. So, H bonds are possible between H2O molecules and dipole-dipole interactions are possible in-between H2S molecules.
64
Describe H2S acidic character
H2S is a weak, diprotic acid Partially dissociates as follows H2S + H2O ---------> HS- + H3O+ HS- + H2O -----------> S2- + H3O+ revers. Following evidences can be given for the acidic nature of H2S Na + H2S (EXCESS) ---------> NaHS + H2 Na (EXCESS) + H2S ----------> Na2S + H2
65
Evidences for acidic nature of H2S
Na + H2S (EXCESS) ---------> NaHS + H2 Na (EXCESS) + H2S ----------> Na2S + H2
66
How does H2S form salts with bases
NaOH + H2S (EXCESS) ---------> NaHS + H2O NaOH (EXCESS) + H2S ----------> Na2S + H2O
67
Examples for reducing property of H2S
H2S ------> S 1. Reaction w/ KMnO4 MnO4- -------> Mn2+ violet colorless S2- --------> S 2. Reaction w/ K2Cr2O7 Cr2O72- -------> Cr3+ orange green S2- ----------> S forms a turbid green solution 3. Reaction w/ Na3AsO4 AsO43- ------> As3+ S2- --------> S 4. Reaction w/ Cl solution Cl2 -------> Cl- S2- --------> S 5. Reaction w Br Br2 ------> Br- (brown) (colorless) S2- ------> S 6. Reaction w/ SO2 S2- -------->S SO2 -------> S
68
Reaction of H2S with KmnO4
MnO4- -------> Mn2+ violet colorless S2- --------> S
69
Reaction of H2S with K2Cr2O7
Cr2O72- -------> Cr3+ orange green S2- ----------> S forms a turbid green solution
70
Reaction of H2S with Na3AsO4
AsO43- ------> As3+ S2- --------> S
71
Reaction of H2S with Cl solution
Cl2 -------> Cl- S2- --------> S
72
Reaction of H2S with Br solution
Br2 ------> Br- (brown) (colorless) S2- ------> S
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Reaction of H2S with SO2 solution
S2- -------->S SO2 -------> S
74
Show oxidizing property of H2S
H2S -----> H2 1. Reaction w/ Na H2S ----> H2 Na ----> Na2S 2. Reaction with Mg H2S -----> H2 Mg ------> MgS
75
Reaction of H2S with Na
H2S ----> H2 Na ----> Na2S
76
Reaction of H2S with Mg
H2S -----> H2 Mg ------> MgS
77
Describe SO2
- a colorless gas with a pungent or choking smell - poisonous
78
preparation of SO2
1. Reaction of solid sulphide with a dilute acid SO32- + H+ ---------> SO2 + H2O 2. Reaction of S with conc. H2SO4 S + H2SO4 -------> SO2 + H2O 3. Reaction of Cu with conc. H2SO4 Cu + H2SO4 ---------> CuSO4 + SO2 + H2O 4. Adding a dilute acid to a thiosulfate Na2S2O3 + HCl ------> NaCl + SO2 + S + H2O
79
Adding a dilute acid to a thiosulfate
Na2S2O3 + HCl ------> NaCl + SO2 + S + H2O
80
Reaction of Cu with conc. H2SO4
Cu + H2SO4 ---------> CuSO4 + SO2 + H2O
81
Reaction of S with conc. H2SO4
S + H2SO4 -------> SO2 + H2O
82
Reaction of solid sulphide with a dilute acid
SO32- + H+ ---------> SO2 + H2O
83
Identification of SO2
SO2 is allowed to pass through a filter paper moistened with K2Cr2O7. Then formation of green coloured dots can be seen. Or, SO2 gas can be passed through acidic K2Cr2O7 and the solution will turn green color
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Properties of SO2
1. Acidity 2. Bleaching property 3. Oxidizing property 4. Reducing property
85
Show Acidity of SO2
SO2 produces sulfurous acid as below SO2 (S) ----------> SO2 (aq.) SO2 + H2O ----------> H2SO3 (reversible) The acidic property of SO2 is evident by following reaction SO2 + NaOH ------> Na2SO3 + H2O EXCESS SO2 + NaOH ------> NaHSO3
86
Show the acidic property of SO2
SO2 + NaOH ------> Na2SO3 + H2O EXCESS SO2 + NaOH ------> NaHSO3
87
Show reducing property of SO2
SO2 ------> SO42- 1. Reaction of acidified KMnO4 SO2 ------> SO42- MnO4- ------> Mn2+ 2. Reaction of acidified K2Cr2O7 SO2 -------> SO42- Cr2O72- ---------> Cr3+ 3. Reaction of FeCl3 Fe3+ --------> Fe2+ SO2 ----------> SO42-
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Reaction of SO2 with KMnO4
SO2 ------> SO42- MnO4- ------> Mn2+
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Reaction of SO2 with FeCl3
Fe3+ --------> Fe2+ SO2 ----------> SO42-
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Reaction of SO2 with K2Cr2O7
SO2 -------> SO42- Cr2O72- ---------> Cr3+
91
Show oxidizing property of SO2
SO2 --------> S 1. Reaction w H2S SO2 ---> S H2S ---> S 2. Reaction w heated metals Mg + SO2 -----> Mgo + MgS Fe + SO2 -------> FeO + FeS
92
Reaction of SO2 with heated metals
Mg + SO2 -----> Mgo + MgS Fe + SO2 -------> FeO + FeS
Inorganic
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