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15th Group Flashcards

1
Q

Common electronic configuration

A

ns2 np3

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2
Q

Main valences

A

3 & 5

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3
Q

How do metallic properties vary down group 15?

A

increases

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4
Q

Metallic character of N & P

A

Non-metals

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5
Q

Metallic character of As, Sb, Bi

A

Poor metals

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6
Q

How do group 15 elements exist?

A

N exists as a gas

All the other elements exist in solid state

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7
Q

Why is electronegativity of N high?

A

Due to smaller atomic radius

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8
Q

What are the two types of oxides produced by group 15 elements

A

Y2O3 oxides

Y2O5 oxides

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9
Q

What’s the acidic character of Y2O3 oxides

A

N2O3 - acidic

P2O3 - weakly acidic

As2O3 - amphoteric

Sb2O3 - amphoteric

Bi2O3 - basic

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10
Q

Acidic character of N2O3

A

acidic

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11
Q

Acidic character of P2O3

A

weakly acidic

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12
Q

Acidic character of As2O3

A

amphoteric

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13
Q

Acidic character of Sb2O3

A

amphoteric

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14
Q

Acidic character of Bi2O3

A

basic

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15
Q

Which oxides exist as dimers?

A

As2O3 and Sb2O3

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16
Q

Write the acidic character of Y2O3 oxides

A

All are acidic

No basic oxides

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17
Q

What oxide isn’t theoretically possible?

A

Bi2O5

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18
Q

What are the oxides produced by N?

A

N2O3, N2O5, NO, N2O, NO2

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19
Q

How do acidic oxides of N and P react with water?

A

Acids are produced

N2O3 + H2O –> HNO2

NO2 + H2O –> HNO2 + HNO3

N2O5 + H2O –> HNO3

P2O3 + H2O –> H3PO4

P2O5 + H2O –> H3PO4

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20
Q

N2O3 reaction w water

A

N2O3 + H2O –> HNO2

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21
Q

NO2 reaction w water

A

NO2 + H20 –> HNO3 + HNO2

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22
Q

N2O5 reaction w water

A

N2O5 + H20 –> HNO3

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23
Q

P2O3 reaction w water

A

P2O3 + H2O –> H3PO4

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24
Q

Write the acidic nature of all N oxides

A

N2O - neutral
NO - neutral
N2O3 - acidic
NO2 - acidic (more)
N2O5 - acidic (highly)

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25
Q

Acidity of N2O

A

Neutral

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26
Q

Acidity of NO

A

Neutral

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27
Q

Acidity of N2O3

A

Acidic

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28
Q

Acidity of NO2

29
Q

Acidity of N2O5

30
Q

Characteristics of N

A
  • N exists with triple bonds as N2 and it is very hard to break. So, N2 is inert
  • Due to inert property, high % of N2 is possible in atmosphere (70.98%)
  • Weakly soluble in water, but more soluble under high pressure
  • N2 doesn’t show allotropic forms even though all other 15th group elements do
31
Q

experimental confirmation of N in atmosphere

A

Burn a piece of Mg tape in air & collect the powder produced by burning

Secondly, add this powder to water and close a filter paper moistened with Nessler’s reagent

Then the filter paper will turn into brown. Evolving NH3 turns Nessler’s reagent brown

Mg + O2 –> MgO

Mg + N2 –> Mg3N2

Mg3N2 + H20 —> Mg(OH)2 + NH3

32
Q

reactions of N in atmosphere

A

Mg + O2 –> MgO

Mg + N2 –> Mg3N2

Mg3N2 + H20 —> Mg(OH)2 + NH3

33
Q

N compound w oxidation no. (-3)

A

Ammonia (NH3)

34
Q

N compound w oxidation no. (-2)

A

Hydrazine (N2H4)

35
Q

N compound w oxidation no. (-1)

A

Hydroxyl amine (NH2OH)

36
Q

N compound w oxidation no. 0

A

Dinitrogen (N2)

37
Q

N compound w oxidation no. (+1)

A

Dinitrogen Monoxide (N2O)

38
Q

N compound w oxidation no. (+2)

A

Nitrogen Monoxide (NO)

39
Q

N compound w oxidation no. (+3)

A

Dinitrogen trioxide (N2O3)

40
Q

N compound w oxidation no. (+4)

A

Nitrogen dioxide (NO2)

Dinitrogen Tetroxide (N2O4)

41
Q

N compound w oxidation no. (+5)

A

Dinitrogen Pentoxide (N2O5)

Nitric Acid (HNO3)

42
Q

What are the nitrogen oxoacids

43
Q

Describe HNO2

A
  • a weak monoprotic acid
  • at room conditions, HNO2 is unstable
44
Q

How can a solution of HNO2 acid be prepared?

A

Adding a dilute acid to a cold dilute solution of a nitrite

NaNO2 + HCl —> NaCl + HNO2

45
Q

How does HNO2 disproportionate?

A

HNO2 –> HNO3 + NO + H2O

NO + O2 —> NO2 (reddish brown)

This fact is used to identify NO2- ions

46
Q

Describe HNO3

A
  • HNO3 is a strong acid
  • An oily, hazardous liquid
  • Pure HNO3 is colorless but usually we can observe HNO3 acid with a yellow color, due to the light induced decomposition of HNO3
47
Q

Decomposition of HNO3 under sunlight

A

HNO3 —> NO2 + O2 + H2O

48
Q

Properties of HNO3

A

HNO3 shows oxidizing, reducing, acid and base properties

  1. Dilute HNO3 as an acid
  2. Conc. HNO3 as an oxidizing agent
  3. HNO3 with H2SO4 as a base (nitration mixture)

NO REDUCING PROPERTIES

49
Q

Reactions of HNO3 as an acid with metals

A

Mg + HNO3 –> Mg(NO3)2 + H2

Zn + HNO3 –> Zn(NO3)2 + H2

50
Q

Reactions of HNO3 as an oxidizing agent

A

Mg + HNO3 –> Mg(NO3)2 + NO2 + H20

Cu + HNO3 –> Cu(NO3)2 + NO2 + H2O

51
Q

How does Cu react with dilute HNO3

A

Cu can’t displace H from dilute acids, but Cu involves in reaction with dil. HNO3 by showing oxidizing properties

Cu + HNO3 —> Cu(NO3)2 + NO + H2O

52
Q

Reactions of conc. HNO3 with non-metals

A

C + HNO3 –> CO2 + NO2 + H2O

S + HNO3 –> H2SO4 + NO2 + H20

53
Q

Describe NH3

A

A colorless gas with a strong, characteristic smell

It’s a basic gas which is soluble in water

NH3 + H2O –> NH3OH

54
Q

Describe NH3 reactions with water

A

NH3 + H2O –> NH3OH

55
Q

How does NH3OH (aq. NH3) act as a base and dissociate?

A

NH4OH –> NH4+ + OH-

56
Q

Properties of NH3

A
  1. base
  2. acid
  3. oxidizing agent
  4. reducing agent
57
Q

How does NH3 act as a base?

A

NH3 + HCL —> NH4Cl (white dense fume)

58
Q

How does NH3 act as an acid?

A

Na + NH3 —> NaNH2 + H2

Mg + NH3 —> Mg3N2 + H2

59
Q

How does NH3 act as an oxidizing agent

A

Na + NH3 —> NaNH2 + H2

Mg + NH3 —> Mg3N2 + H2

60
Q

Reactions of NH3 as a reducing agent

A

NH3 + Cl2 –> N2 + HCl

EXCESS NH3 + HCl –> NH4Cl

NH3 + EXCESS Cl2 –> HCl + NCl3

NCl can react w water as follows

NCl3 + H2O –> NH3 + HOCl

61
Q

Why is NH3 used as a water disinfecting agent

A

Due to formation of HOCl

62
Q

Reaction of NH3 with CuO

A

CuO + NH3 –> Cu + N2 + H20

63
Q

Steps of NH3 identification

A
  1. Nessler’s Reagent

Filter paper moistened with Nessler’s reagent when allowed to contact NH3 gas turns brown color from yellow

  1. Using HCl Vapor

When conc. HCl is allowed to contact with NH3 gas, a white dense fume formation is observed

NH3 + HCl –> NH4Cl (white dense fume)

64
Q

NH3 reaction with HCl vapor

A

NH3 + HCl –> NH4Cl (white dense fume)

65
Q

How do ammonium salts decompose?

A

They decompose easily by heat to give NH3 as a product

(NH4)2CO3 —-> NH3 + CO2 + H2O

NH4Cl –> NH3 + HCl

(NH4)2SO4 —> NH3 + H2SO4

66
Q

How do some NH4 salts with anions oxidize ?

A

They oxidize to give some other products instead of NH3

NH4NO2 —> N2 + H20

NH4NO3 –> N20 + H20

(NH4)2Cr2O7 –> N2 + Cr2O3 + H20

67
Q

How does (NH4)2Cr2O7 oxidize

A

(NH4)2Cr2O7 –> N2 + Cr2O3 + H20

68
Q

Identification of NH4 salts

A

When NH4 salts heat with a strong base (NaOH), all NH4 salts evolve NH3

Evolving NH3 can be identified using HCl vapor or Nessler’s reagent

NH4+ + OH- —> NH3 + H20

NH3 + HCl —-> NH4Cl (white flame)

NH3 —–> brown

69
Q

Reaction of salt with weak component of weak acid/ base

A

It’s possible to displace using a strong component

(NH4)2CO3 + HCl —> NH4Cl + CO2 + h20

(NH4)2CO3 + NaOH —> NH3 + Na2CO3 + H20

Inorganic (9 decks)

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