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Inorganic Chemistry > P Block Elements (Grp - 15) > Flashcards

P Block Elements (Grp - 15) Flashcards

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1
Q

MP of Hydrides

A

PH₃ < AsH₃ < SbH₃ < BiH₃ < NH₃

NH₃ forms intramolecular H-Bonding

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2
Q

BP of Hydrides

A

PH₃ < AsH₃ < NH₃ < SbH₃ < BiH₃

NH₃ forms intramolecular H-Bonding

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3
Q

Common oxidation State

A

+3, +5, -3

N : +1,+2,+3,+4,+5,-5
Bi : hardly -3

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4
Q

Covalency

A

5 or 6

N : 4 (tendency to for pπ-pπ bond)

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5
Q

Down the grp

NH₃
PH₃
AsH₃
SbH₃
BiH₃

A

Bond angle ↓ (as only NH₃ is hybridised ~ 107°, others 90°)

E-H bond energy ↓
Reducing power ↑
Acidity ↑ (easy to release H⁺)

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6
Q

ECl₃ + H₂O

A

NCl₃ + H₂O → NH₃ + HCl
PCl₃ + H₂O → H₃PO₃ + HCl
AsCl₃ + H₂O → As₂O₃ + HCl
SbCl₃ + H₂O → SbOCl + HCl
BiCl₃ + H₂O → BiOCl + HCl

EOCl - Element Oxychloride

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7
Q

E³⁻ + M⁺

A

Ca⁺² + N³⁻ → Ca₃N₂
Na⁺ + N³⁻ →Na₃N
Ca²⁺+ + P³⁻ →Ca₃P₂
Zn + Sb³⁻ → Zn₃Sb₂

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8
Q

Fractional Distillation of liquid air

A

Preparation of N₂

NH₄Cl + NaNO₂ Δ→ N₂ + H₂O + Nacl

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9
Q

(NH₄)₂Cr₂O₇

A

Preparation of N₂

(NH₄)₂Cr₂O₇ / Δ→N₂ + H₂O + Cr₂O₃ (Green)

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10
Q

NaN₃ Δ→
Ba(N₃)₂ Δ→

A

Preparation of N₂

NaN₃ Δ→ Na + N₂
Ba(N₃)₂ Δ→ Ba + N₂

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11
Q

Haber’s Process

A

Preparation of Ammonia

N₂ + 3H₂ → 2NH₃

CATALYST
200 atm
450 - 500°C
Mo - Promoter
Fe(FeO.K₂O.Al₃O₂) - Iron Catalyst

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12
Q

N₂ + O₂ / Δ→

A

N₂ + O₂ / Δ→ 2NO

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13
Q

Ammonium salt + Base → NH₃

A

Preparation of Ammonia

NH₄Cl + KOH → NH₃ + KCl + H₂O

(NH₄)₂SO₄ + NaOH → NH₃ + Na₂SO₄ + H₂O

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14
Q

Fe³⁺ + NH₄OH

A

Fe³⁺ + NH₄OH → Fe(OH)₃
[Do not react with further NH₄OH]

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15
Q

Al³⁺ + NH₄OH

A

Al³⁺ + NH₄OH → Al(OH)₃
[Do not react with further NH₄OH]

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16
Q

Cu²⁺ + NH₄OH

A

Cu²⁺ + NH₄OH → Cu(OH)₂ + NH₄OH → [Cu(NH₃)₄]²⁺ - Deep blue

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17
Q

Zn²⁺ + NH₄OH

A

Zn²⁺ + NH₄OH → Zn(OH)₂ + NH₄OH → [Zn(NH₃)₄]²⁺ - Clear soln

18
Q

AgCl + NH₄OH

A

AgCl + NH₄OH → [Ag(NH₃)₂]Cl

19
Q

NH₄⁺ + K[HgI₄] (Nessler’s reagent)

A

NH₂.HgO.HgI - Iodide of millon’s base

Test for NH₄⁺

20
Q

PbO + NH₃
CuO + NH₃

NH₃ - Weak Reducing agent

A

PbO + NH₃ → Pb + N₂ + H₂O
CuO + NH₃ →Cu + N₂ + H₂O

21
Q

N₂ + Cl₂

A

N₂(excess)+ Cl₂ → NH₄Cl + N₂
N₂ + Cl₂(excess) → NCl₃ + HCl

22
Q

NH₃ + O₂ in Pt/Rh

A

NH₃ + O₂ in Pt/Rh → NO + H₂O

23
Q

Oxides of Nitrogen

A

Refer Notes

24
Q

Ostwald’s Process

Pt/Rh

A

NH₃ + O₂ + Pt/Rh→ NO + H₂O
NO + O₂ → NO₂
NO₂ + H₂O → HNO₃ + NO

25
Q

HNO₃ + NaOH

A

HNO₃ + NaOH→ NaNO₂ + H₂O

acidic nature of HNO₃

26
Q

Oxidation of metals and non- metals by HNO₃

A

Refer notes

27
Q

Brown ring test

A

Identify NO₃⁻ (Nitrate ion)

NO₃⁻ + Fe²⁺ → NO + Fe³⁺ + H₂O

NO + Fe²⁺ + H₂O → [Fe(H₂O)₅NO]²⁺ (Brown Ring)

28
Q

white P₄ + O₂

A

P₄ + O₂ → P₄O₁₀ - vapour of P₄ (Poisonous)

29
Q

white P₄ + NaOH

A

white P₄ + NaOH → PH₃ + NaH₂PO₂ + H₂O

disproportionation rxn

30
Q

white P₄ + 573 K

A

white P₄ + 573 K ⇄ Red P₄

Transition Temp. = 573K

31
Q

Preparation of Phosphine

A

Zn₃P₂ + dil.HCl → ZnCl₂ + PH₃

Ca₃P₂ + H₂O→ Ca(OH)₂ + PH₃

32
Q

Purification of PH₃

A

PH₃ + HI → PH₄I + Impurities
PH₄I + KOH → PH₃(pure) + H₂O + KI

33
Q

Holme’s signal

A

CaC₂ + Ca₃P₂

CaC₂ + H₂O →C₂H₂ + Ca₃P₂ → PH₃

This mixture produces impure PH₃ (Phosphine) - gives signal in smokescreen, etc

34
Q

Properties of PH₃

A

PH₃ + CaSO₄ → Ca₃P₂ + H₂O
PH₃ + HgCl₂→ Hg₃P₂ + H₂O

PH₃ + HCl→PH₄Cl

35
Q

Oxides of P

A

Refer notes

36
Q

Halides of P

A

Refer notes

37
Q

Oxoacids of P

A

Refer notes

38
Q

α - Black P

A

Red P + 803 K in sealed tube

39
Q

β- Black P

A

White P + 473 K in sealed tube

40
Q

N
P
As
Sb
Bi

Down the grp

A

Size ↑
Ionisation potential (∆iH) ↓
BP ↑ [Ex. Sb>Bi]
MP ↑ [Till As and decrease]

41
Q

Electron affinity

A

Grp 15 < Grp 16

Bcas grp 15 has half filled config. which is quite stable

42
Q

Fajan’s Rule

A

sai - small anion - ionic

EX₃ > EX₅

EX₅ is more covalent due to big anion (more anion)

or +5 in EX₅ - more polarising

Inorganic Chemistry (3 decks)

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