16th Group Flashcards
Common electronic configuration
ns2 np4
Valences
2 & 4 (but O differs)
What are the metallic characters of 16th group elements
O and S are non-metals
Se, Te, Po show both metal and non-metal characters
What is the only element in 16th group which exists in gaseous state?
O
Oxidation states
Except O, other elements in the group can form even numbered oxidation states from -2 upto +6
What are the 16th group hydrides?
H2O
H2S
H2Se
H2Te
2 allotropic forms of oxygen
O2 and O3
Describe O3
Ozone is a light blue colored (colorless) gas with a pungent odor
What special properties does O3 have due to its ability to produce atomic oxygen?
- Oxidizing agent
- Reducing agent
- Disinfecting agent
Describe O2
O2 is colorless, and odorless
Slightly water soluble
How is O2 prepared in the laboratory?
Catalytic decomposition of KClO3
KClO3 ———-> KCl + O2
(heating with MnO2 or Pt)
Catalytic decomposition of H2O2
H2O2 ——-> H2O + O2
(heating with MnO2)
How is O2 produced industrially?
By fractional distillation of liquid air
What is the most widely used solvent?
water
Show the ionization of H2O
2H2O —> OH- + H30+
revers.
Show water’s reactions with acids and bases
NH3 + H2O —> NH4+ + OH-
HCl + H20 —–> Cl- + H3O+
water’s reaction w bases
NH3 + H2O —> NH4+ + OH-
water’s reaction w acids
HCl + H20 —–> Cl- + H3O+
Why is water considered amphiprotic?
It can either donate or accept a proton
Decomposition of H2O2 in sunlight
H2O2 —>H2O + O2
So, H2O2 is usually stored in brown or black colored bottles
Describe H2O2
- 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.
How does H2O2 release atomic oxygen
H2O2 —-> H2O + O
uses of H2O2
Oxidizing agent
Disinfecting agent
Bleaching agent
Reducing agent
Used as a rocket fuel
Properties of H2O2
- Oxidizing agent
- Reducing agent
- Antiseptic agent
- Bleaching agent
How does H2O2 react as an oxidizing agent?
- with acidified iodide ions
H2O2 —> H2O
I- —> I2
- Reaction with Fe2+ ions
H2O2 —> H2O
Fe2+ —> Fe3+
How does H2O2 react with acidified iodide
ions
- with acidified potassium ions
H2O2 —> H2O
I- —> I2
How does H2O2 react with Fe2+ ions
- Reaction with Fe2+ ions
H2O2 —> H2O
Fe2+ —> Fe3+
How does H2O2 act as a reducing agent?
- Reaction w/ acidified KMnO4
MnO4- —–> Mn2+
violet colorless
H2O2 —> O2
- Reaction w/ acidified K2Cr2O7
Cr2O72- —-> Cr3+
orange green
H2O2 —–> O2
- Reaction w/ MnO2
MnO2 –> Mn2+
brown colorless
H2O2 —> O2
Reaction of H2O2 w/ MnO2
MnO2 –> Mn2+
brown colorless
H2O2 —> O2
Reaction of H2O2 w/ acidified K2Cr2O7
Cr2O72- —-> Cr3+
orange green
H2O2 —–> O2
Reaction of H2O2 w/ acidified KMno4
MnO4- —–> Mn2+
violet colorless
H2O2 —> O2
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
2 types of S
crystalline sulphur
non-crystalline sulphur
2 types of crystalline sulphur
rhombic s. (alpha s.) and monoclinic s. (beta s.)
2 types of non-crystalline sulphur
plastic s. and colloidal s
How are crystalline sulphur formed?
s8 rings
What’s the most stable form of crystalline sulphur?
Rhombic sulphur (stable below 95C)
When is monoclinic sulphur stable?
Above 95C
How can monoclinic s. be prepared?
by cooling molten sulphur slowly
another name for colloidal sulphur
milk of sulphur
Oxidation no.s of sulphur
-2 to +6
show reducing reactions of s
S + O2 —> SO2
S + hot conc. H2SO4 —-> SO2 + H2O
S+ hot conc. HNO3 —–? H2SO4 + NO2 + H2O
disproportioning of S
S + NaOH ——> Na2S + Na2S2O3 + H2O
uses of sulphur
- good fungicide
- manufacturing medicinal drugs for skin diseases
- used in sulphuric manufacturing process
- used in rubber vulcanization
Oxoacids of S
H2SO4
H2S
H2S2O3
Describe H2SO4
Strong, diprotic acid
How is H2SO4 produced?
SO3 + H20 ——> H2SO4
ionization of H2SO4
H2SO4 + H2O ——> HSO4- + H3O+
HSO4- + H20 ——-> SO42- + H3O+
Properties of H2SO4
Dil. H2SO4 —-> STRONG ACID
CONC. H2SO4 ——> STRONG OXIDIZING AGENT
STRONG DEHYDRATING AGENT
Show H2SO4 reactions as a strong acid
H2SO4 + 2H2O —-> SO42- + H3O+
dil. H2SO4 acts as a strong acid and gives 2 protons as above
H2SO4 reactions as a strong oxidizing agent
- reactions w/ metals
Mg + conc. H2SO4 ———> MgSO4 + SO2 + H2O
Cu + conc. H2SO4 ——–> CuSO4 + SO2+ H2O
- reactions w/ non-metals
S + Conc. H2SO4 ——–> SO2 + H2O
C + conc. H2SO4 ———> CO2 + SO2 + H2O
Reactions of H2SO4 with metals
Mg + conc. H2SO4 ———> MgSO4 + SO2 + H2O
Cu + conc. H2SO4 ——–> CuSO4 + SO2+ H2O
Reactions of H2SO4 with non-metals
S + Conc. H2SO4 ——–> SO2 + H2O
C + conc. H2SO4 ———> CO2 + SO2 + H2O
Why does H2SO4 have a dehydrating property?
It has the ability to remove H and O in a 2:1 ration from a compound
reactions of H2SO4 as a dehydrating agent
C6H12O6 ———-> 6C + 6H2O
C2H5OH ——-> C2H4 + H2O
in presence of conc. H2SO4
Describe H2SO3
- weak, diprotic acid
- Reactions of SO2 w/ water makes H2SO3
- unstable
- can dissociate into SO2 + H2O
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
How does H2S2O3 help iodometric titrations
S2O32- ion can act as a reducing agent.
I2 + S2O32- ——-> I- + S4O62-
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
Preparation of H2S
Reaction of a metal sulphide with a strong acid
FeS + HCl ——> H2S + FeCl2
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
Reactions of H2S identification
Pb(CH3COOH) + H2S —> PbS + CH3COOH
Pb(NO3)2 + H2S ——> PbS + HNO3
AgNO3 + H2S ——-> Ag2S + HNO3
CuSO4 + H2S ——> CuS + H2SO4
Properties of H2S
- Boiling point of H2S is less than H2O
- H2S EXISTS AS A GAS while water exists as a liquid at room temperature
- Acidic character
- Oxidizing character
- Reducing character
- Forms salts with bases
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.
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
Evidences for acidic nature of H2S
Na + H2S (EXCESS) ———> NaHS + H2
Na (EXCESS) + H2S ———-> Na2S + H2
How does H2S form salts with bases
NaOH + H2S (EXCESS) ———> NaHS + H2O
NaOH (EXCESS) + H2S ———-> Na2S + H2O
Examples for reducing property of H2S
H2S ——> S
- Reaction w/ KMnO4
MnO4- ——-> Mn2+
violet colorless
S2- ——–> S
- Reaction w/ K2Cr2O7
Cr2O72- ——-> Cr3+
orange green
S2- ———-> S
forms a turbid green solution
- Reaction w/ Na3AsO4
AsO43- ——> As3+
S2- ——–> S
- Reaction w/ Cl solution
Cl2 ——-> Cl-
S2- ——–> S
- Reaction w Br
Br2 ——> Br-
(brown) (colorless)
S2- ——> S
- Reaction w/ SO2
S2- ——–>S
SO2 ——-> S
Reaction of H2S with KmnO4
MnO4- ——-> Mn2+
violet colorless
S2- ——–> S
Reaction of H2S with K2Cr2O7
Cr2O72- ——-> Cr3+
orange green
S2- ———-> S
forms a turbid green solution
Reaction of H2S with Na3AsO4
AsO43- ——> As3+
S2- ——–> S
Reaction of H2S with Cl solution
Cl2 ——-> Cl-
S2- ——–> S
Reaction of H2S with Br solution
Br2 ——> Br-
(brown) (colorless)
S2- ——> S
Reaction of H2S with SO2 solution
S2- ——–>S
SO2 ——-> S
Show oxidizing property of H2S
H2S —–> H2
- Reaction w/ Na
H2S —-> H2
Na —-> Na2S
- Reaction with Mg
H2S —–> H2
Mg ——> MgS
Reaction of H2S with Na
H2S —-> H2
Na —-> Na2S
Reaction of H2S with Mg
H2S —–> H2
Mg ——> MgS
Describe SO2
- a colorless gas with a pungent or choking smell
- poisonous
preparation of SO2
- Reaction of solid sulphide with a dilute acid
SO32- + H+ ———> SO2 + H2O
- Reaction of S with conc. H2SO4
S + H2SO4 ——-> SO2 + H2O
- Reaction of Cu with conc. H2SO4
Cu + H2SO4 ———> CuSO4 + SO2 + H2O
- Adding a dilute acid to a thiosulfate
Na2S2O3 + HCl ——> NaCl + SO2 + S + H2O
Adding a dilute acid to a thiosulfate
Na2S2O3 + HCl ——> NaCl + SO2 + S + H2O
Reaction of Cu with conc. H2SO4
Cu + H2SO4 ———> CuSO4 + SO2 + H2O
Reaction of S with conc. H2SO4
S + H2SO4 ——-> SO2 + H2O
Reaction of solid sulphide with a dilute acid
SO32- + H+ ———> SO2 + H2O
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
Properties of SO2
- Acidity
- Bleaching property
- Oxidizing property
- Reducing property
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
Show the acidic property of SO2
SO2 + NaOH ——> Na2SO3 + H2O
EXCESS SO2 + NaOH ——> NaHSO3
Show reducing property of SO2
SO2 ——> SO42-
- Reaction of acidified KMnO4
SO2 ——> SO42-
MnO4- ——> Mn2+
- Reaction of acidified K2Cr2O7
SO2 ——-> SO42-
Cr2O72- ———> Cr3+
- Reaction of FeCl3
Fe3+ ——–> Fe2+
SO2 ———-> SO42-
Reaction of SO2 with KMnO4
SO2 ——> SO42-
MnO4- ——> Mn2+
Reaction of SO2 with FeCl3
Fe3+ ——–> Fe2+
SO2 ———-> SO42-
Reaction of SO2 with K2Cr2O7
SO2 ——-> SO42-
Cr2O72- ———> Cr3+
Show oxidizing property of SO2
SO2 ——–> S
- Reaction w H2S
SO2 —> S
H2S —> S
- Reaction w heated metals
Mg + SO2 —–> Mgo + MgS
Fe + SO2 ——-> FeO + FeS
Reaction of SO2 with heated metals
Mg + SO2 —–> Mgo + MgS
Fe + SO2 ——-> FeO + FeS