Inorganic Chemistry Flashcards
(141 cards)
1
Q
What’s the observation for reaction between phosphurus and oxygen?
A
White flame
White solid
Clouds of White smoke
3WS
2
Q
What’s the colour of sulfur in solid state?
A
Yellow
3
Q
Which metals give a white flame when reacted with oxygen?
A
Magnesium
ALuminium
Phosphorus
4
Q
Which metal gives a blue flame when reacted with oxygen?
TO become sulfur dioxide,
A
Sulfur
Futher: SO3, vanadium catalyst, Reversible
5
Q
What colour flame does sodium gives when reacted with oxygen?
A
Bright yellow.
6
Q
What’s an observation for sulfur’s reaction with oxygen other than flame?
BLue flame colour
A
Yellow solid melts
7
Q
What are the two oxides of phosphorus?
A
P4 O6
P4 O10
8
Q
Which oxides are insoluble in water?
A
Silicon
Aluminium
Mg
AIright SiAl
9
Q
Observation for reaction of Na with water
A
- Vigourous reaction
- Floats/ moves on the surface of water
- Sodium diaappears
- Effervescene ( H2 produced)
- Sodium melts/ forms a sphere
Not observation but: colourless solution that turns litmus paper blue
10
Q
Observation for reaction of Mg with water
A
Reacts slowly
( reactivity less, left to right)
atomic size lesser isliye, can take days
pH 11 as Mg(OH) doesn’t completely dissolve so less OH ions
11
Q
Reaction of Mg with steam + why MgO
products: MgO plus H2
A
- Fast
- High temp,
Mg(OH) decomposes to MgO and H2O(g)
12
Q
Colours of Halogens
A
- Cl2(g): green
- Br(l): brown
- Iodine(s): dark grey
13
Q
Flame colour for reaction of sodium with chlorine:
A
- bright orange flame
Others: white solid is formed,greenish gas colour dissappears
14
Q
Flame colour for reaction of Magnesium
A
Bright white flame
others: white solid, greenish gas dissappears
15
Q
Reaction of chlorine with aluminium:
we pass gas over heated Al
A
Aluminium glows
white solid (AlCl3) plus green gas disappears
16
Q
Physical state of SiCL4
needs heating to be made
A
LIQUID
colourlessliquid formed
17
Q
What are two chlorides of Phosphorus?
A
PCl3
PCl5
PCL3 is liquid
18
Q
What are the products in all element + chlorine reactions?
A
Only element-chloride
same for oxides
19
Q
For aluminium plus chlorine which of the compounds is produced: AlCl3 or Al2Cl6?
A
both
Remember Aluminium glows
20
Q
AlCl3’s structure?
(SiCL4 and PCl5 are covalent and simple)
A
Giant
why? as its ionic with covalent character.
21
Q
Why no chloride for Argon?
A
- outer shell os full/complete
- Activation energy/ Ionisation energy too high
22
Q
Which oxides are basic?
A
Na2O and MgO
Na2O is also called alkaline oxide
23
Q
Which oxide is Amphoteric?
A
Al2O3
24
Q
Observation for reaction of Na2O plus water( cold)
A
- highly exothermic
- Alkaline solution of 13-14 pH formed depending upon conc
NaOH water soluble
Product: NaOH aqueous only
25
Why metallic oxides are alkaline/ basic?
Contains oxide ion (O2-)
accepts proton, very strong base
O2- + H20 ==>2OH-
26
Which oxides are acidic?
SiO2, P4O10 and SO2/SO3
27
Al2Cl6 type of compund
| ( high temps par hota hai, 180-190)
Covalent and coordinate
28
reaction of **Na2O** and **2HCl**
**2NaCl** plus **H2O**
29
NaOH plus HCL
H2O + NaCl
30
MgO plus water
Mg(OH)2
| weak alkaline solution is formed (pH is around 9),
## Footnote
slighltly soluble less OH-
31
Mg(OH)2 ions reactions
Mg(OH)2⇌ Mg+2 + 2OH-
32
MgO(s) + 2HCl(aq)
MgCl2(aq) + H2O(l)
33
Why Na2O is ionic?
* Very large difference in electronegativity
* between sodium and oxygen
34
Al2O3 plus 6HCl
2AlCl3 + 3H20
35
Al2O3 plus 3H2SO4
Al2(SO4)3 + 3H20
36
Al2O3 + 2NaOH + 3H2O
2NaAl(OH)4
| sodium tetra hydroxy aluminate
37
Al2O3 + NaOH
2NaAlO2 + H2O
38
Why is SiO2 insoluble in water?
Giant covalent structure
water can't break down its giant structure
39
SiO2(s) + 2NaOH(aq)
| NaOH must be hot and concentrated
## Footnote
Acid-base
Na2SiO3(aq) + H2O(l)
| sodium silicate
40
1. simple structure cause
2. Covalent cause
1. low melting point
2. reacts with water/hydrolysis
41
P4O10(s) + 6H2O
4H3PO4(aq)
| 2pH; reacts vigorously with oxygen;form acidic solution (water dissolve)
42
P4O10 + 12NaOH
4Na3PO4 + 6H2O
43
P4O6(s) + 6H2O
4H3PO3(aq)
44
SO2 + H2O
H2SO3
| sulfurous
45
SO3 + H2O
H2SO4
| sulfuric: fog of sulfuric formed
46
SO2 + 2NaOH
Na2SO3 + H2O
47
SO3 + 2NaOH
Na2SO4 + H2O
48
2NH3+SO2+H2O
(NH4)2SO3
49
2NH3+ H2O+ SO3
(NH4)2SO4
50
2NH3+H2SO4
(NH4)2SO4
51
SO3 + NaOH
NaHSO4
52
What's the reaction with water called?
Hydrolysis
53
Does NaCl react with water?
No, NaCl doesn't:
Water only breaks the lattice
54
Observation of NaCl with water
White solid disappears
COlourless solution
pH: 7
55
Reaction of MgCl2 with water
MgCl2 +(aq) ==>Mg+2 + 2Cl-
56
MgCl2 plus water give what **pH**:
6.5
57
Aluminium chloride plus water
AlCl3(s)+ aq⇌ Al3+(aq) +3Cl-(aq)
[Al(H2O)6]3+⇌ [Al(H2O)5(OH-1)]+2 + H+
| Hydrolysis reaction
58
AlCL3 plus water gives what pH:
about 3
59
AS temp increases, what happens to gas solubilty
It decreases.
60
Which chloride is a liquid?
SiCL4
| (PCl3 bhi hai but whatever)
61
SiCl4(l) + H2O(l)
| H2O is cold
4HCl(g)+ SiO2(s)
62
Observation for SiCl4 and water
* white solid
* Steamy fumes
* pH is 2
* highly exothermic-test tube hot
* pale yellow solution forms
63
PCl3 + H2O
3HCl + H3PO3
| 2 pH; white steamy fumes
64
PCl5+ 4H2O
H3PO4 + 5HCl
| pH is 2; white steamy fumes
65
General trend for colour of halogens
they get darker
66
Colour of iodine in all states
AQ= brown
Solid= dark grey
G= purple vapour
67
Trend of m.p and b.p in halogens
* increases
* More electrons in molecules
* so increased strength of **instantaneous dipole-id** forces of attraction , requiring higher energy
| Less **Volatile** down the group
68
What are oxidising agents?
In exams: remove electrons from other species
concept: Gain electrons
69
Trend in oxidising power of halogens
Decreases down the group
70
# Explain
trend in oxidising power of halogens
* positive charge increases
* distance and shielding outweighs this increaes
* so attraction of nucleus for outer electron decreases
* so **less likely /easier** to attract/**gain **an electron
71
What's a reducing agent?
: it donates electrons
; makes other species gain electrons
72
What are good reducing agents?
Halide **IONS**
73
Whixh halide is the best reducing agent?
Iodide ions are the best reducing agents
74
Explain the trend of reducing power in halide ions.
| Increases down the group
* larger distance between nucleus and valence shell
* more shielding electrons
* outweigh the increased nuclear charge
* nuclear attraction on valence electron decreases so more likely to donate/ lose electrons
75
Reactivity of halogens trend
Decreases down the group
76
Explain the trend in reactivity of halogens.
| (decreases down the group)
more oxidising power, more reactive, remove electron from halide ion/gain electrom
| plus the reasons for oxidising power
77
tell Halogen colours in organic solvent.
| cyclohexane
Iodine: Purple;
Chlorine: PAle green
Bromine: ORange
78
What's the state of hydrogen halides at rtp?
ALL ARE **GASES**
79
H2(g) + F2(g)
| Give products plus conditions
2HF(g)
| explosive in cool dark conditions
80
H2(g) + Cl2(g)
| Give products plus conditions
2HCl(g)
| reacts explosively in sunlight
81
H2(g) + Br2(g)
| observation + products
2HBr(g)
| reacts slowly on heating
82
H2(g) + I2(g)
| onservation plus products
⇌ 2HI(g)
| forms an equiblirium mixture on heating
83
# ```
State the trend in reactivities of the halogens with hydrogen.
| Explain in terms of oxidising power
Decreases down the group
| same as reactivity: oxidising power decreases down the group + reasons.
84
# Explain
the trend of reactivity of halogens with hydrogen halides in terms of **bond energies**
* X-X bond strength decreases from Cl-Cl to I-I
* but decreasing strength of H-X down the group more significant
85
Describe and explain the trend in the b.p of the hydrogen halides other than H-F.
* increases
* greater number of electrons in molecules
* greater VdW forces of attraction
| HF>HI>HBr>HCl
86
Why HF has a higher b.p than rest of the fam?
* HF has hydrogen bonds
* sum of hydrogen bonds and induced dipoles in HF are stronger than the sum of induced dipoles and permanent dipoles as hydrogen bonds are stronger than other imfs
87
What's the trend in thermal stabilities of the hydrogen halides?
It decreases down the group
88
Explain the trend in thermal stabilities of hydrogen halide down the group.
| (decreases down the group)
* lower H-Hal bond enthalpy
* due to increased bond length.
89
What reagents do we use to test halide ions?
AgNO3 + aqueous Ammonia
90
Colours with AgNO3
* Cl-: white ppt, dissolves with dilute aq NH3
* Br- : cream ppt, dissolves in conc NH3
* I- : yellow ppt. doesn't dissolve
91
State the equation for Agcl and ammonia
AgCl(s) +2NH3(aq) -----> [Ag(NH3)2]+Cl-
or
[H3N:-->Ag<--:NH3]+Cl-
92
# reaction: halide ion with conc H2SO4
Preparation of HCl
| INCLUDE STATE SYMBOLS
NaCl(s) + H2SO4(l)--->NaHSO4(s) + HCl(g)
or
2NaCl(s) + H2SO4(l)--->Na2SO4(s) + 2HCl(g)
93
What type of reaction is preparation of HCl ?
| ( jab H2SO4 aur nacl)
Acid base
displacement
| chloride is proton acceptor,
## Footnote
NOT NEUTRALISATION: that has water product
94
Which salt will produce highest yield of hydrogen halide?
Chloride salts
95
Why does NaCl give the highest hydrogen halide yield?
* Chloride ions aren't strong enough reducing agents to reduce H2SO4
* Br- and I- strong enough to react with S in H2SO4.
96
What sort of agent is Sulfuric Acid?
It's a very good oxidising agent
| (remember SO2, however, is a reducing agent)
97
What's the oxidation state of sulfur in H2SO4?
+6
| gains 2 e=SO2, gains 6=S, gains 8e= H2S
98
Reaction of NaBr with conc H2SO4
NaBr(s) + H2SO4(l)-->NaHSO4(s)+ HBr(g)
and
2HBr(g) + H2SO4(l) ----->Br2(g)+ SO2(g) + 2H2O(l)
99
# Observations for
Reaction of NaBr with conc H2SO4
* highly exothermic
* Reddish brown gas due to Br2 formation
100
# Reactions
NaI and sulfuric acid
NaI(s) + H2SO4(l)----> NaHSO4(s)+ HI(g)
6HI(g) +H2SO4(l)---->3I2(g) + S(s) + 4H2O(l)
| 2HI(g) + H2SO4---->I2(g) + SO2(g) + 2H2O
## Footnote
8HI(g) + H2SO4---> 4I2(g) + H2S(g) + 4H2O
101
# Observations
NaI and sulfuric acid
* purple vapor I2(g)
* sulfur yellow solid
* rotten egg smell H2S
102
# State and explain
Role of Sulfuric acid in reactions with NaI and NaCL and difference in reactions
Cl- : as an acid
I-: as an oxidising agent
difference: not strong enought to oxidise cl-
/resucing power of I- vs CL-
ya
products hcl vs I2 etc
103
104
Dispropornation Reaction
| (self oxidation- reduction reaction)
The same elemnet is both oxidised and reduced
105
Aqueous chlorine and cold dilute alkali
| (15 degrees): makes bleach
Cl2(aq)+ 2NaOH(aq) ----> NaCl(aq) + NaClO(aq) + H2O(l)
| Sodium Chlorate 1/ hypochlorite ion
106
What's the common name of NaClO?
Bleach: equal mix of NaCl and NaClO
| kills bacteria /disinfectant and bleaching agent
107
What's the oxidation state of chlorine in NaClO / sodium chlorate 1?
+1
| ( oxygen more e.n than chlorine so us par negative charge)
108
What's chlorine used for?
Kill germs
| like in chlorination
109
Write the ionic equation for cold dilute NaOH and Cl2?
2OH-(aq) + Cl2(aq) ----> Cl-(aq) + Cl+(aq) + H2O(l)
110
Half equations for reaction of cold dilute NaOH and Cl(2)
1/2Cl2(aq) + e- --->Cl-1
(dusra chlorine yeh e dega)
2OH- +1/2Cl2(aq)----> e- + ClO(aq)- + H2O(l)
| yeh reactions iodine and bromine bhi dein gy
111
# Reaction of
hot, concentrated NaOH and aq chlorine
| 70 degrees
3Cl2(aq) + NaOH(aq) ----> 5NaCl(aq) + NaClO3(aq) + 3H2O(l)
| Sodium chlorate (V)
112
What's the oxidation state of chlorine in NaClO3?
+5
113
State the ionic equation for hot con NaOH and Cl2(aq)
3Cl2(aq) + 6OH-(aq)---->5Cl-(aq) + ClO3-(aq)+ 3H2O(l)
114
What type of reaction is chlorination of water?
Hydrolysis
115
State equation for chlorination of water.
Cl2(aq) + H2O(l) -----> HCl(aq) + HClO(aq)
| ClO- responsible to kill bacteria.
116
What explains the lack of reactivity of Nitrogen?
N-N triple bond ,
lot of energy required to break this
non polar in nature
117
How are oxides of nitrogen formed?
* lightening (naturally occuring)
* internal combustion of engine( man made)
118
show reaction of nitrogen with oxygen due to lightening
N2 + O2 ----> 2NO
2NO + O2---> 2NO2
1/2O2 + 2NO2 + H2O----> 2HNO3
or 2NO2 + H2O---> HNO3 + HNO2
| lightening on top of arrow , all of this in air
119
What's the colour and formula of nitrogen IV oxide?
Brown
NO2
| Nitrogen II oxide is NO
120
Why is calcium oxide used to dry ammonia?
Calcium oxide is basic so he doesn't react with ammonia
121
Why is ammonia dried ( base plus ammonium reaction)?
so ammonia doesn't dissolve in water, gas hi nahi mily gi.
122
What are uses of ammonium salts?
Fertilizers: phsophate, sulphates and nitrates
| nitrates soluble and wash away into rivers, algal bloom
123
What does PAN stand for?
Peroxy acetyl nitrate
124
How is PAn formed?
When oxides of nitrogen react with unburnt hydrocarbons.
125
What is PAN?
It causes photochemical smog
126
What is smog?
| Idk why I wrote this
* brownish yellow haze
* presence of compound that irritate eyes and respiratory tract
127
Reactions in combustions engines
reaction of o2 and N2
incomplete combustion
128
What's formed in combustion engines?
oxides of nitrogen
carbon monoxide
| SO2 , and nitrogen ke oxides , ya phir Lead ka koi compound as well
129
# Products of
complete combustion of unburnt hydrocarbons
SO2 , and nitrogen ke oxides , ya phir Lead ka koi compound
130
# Reaction in combustion engine
reaction of o2 and n2
N2 + O2---> 2NO
131
how is CO formed in car engines?
incomplete combustion
132
Show the catalytic removal of oxides of nitrogen from exhaust gases of internal combustion engine.
NO(g) + CO(g) --Pt /rhodium (s)-->CO2(g) + 1/2 N2(g)
| Pt is a catalyst
133
What sort of catalysis is the catalytic conversion of oxides of nitrogen to nitrogen gas?
heterogenous catalysis
| ( when reactants and catalysts aur in different states, haber ki trah
## Footnote
N2(g) + 3H2--FE+450+200-400atm--> 2NH3(g)
134
# contact process
What catalyst is used?
V2O5
135
What are temp and pressure requirements fro contact process?
* 450 degrees
* 1-5 atm
136
# List
reactions in contact process
* S+O2--->SO2
* **SO2 + O2--->2SO3**
* SO3 + H2SO4--->H2S2O7 (oleum)
* H2S2O7 + H2O---> 2H2SO4
137
Sources of sulfur dioxide
* burning of sulfur containing compound at power stations
* Volcanic eruptions
138
How SO2 is converted to SO3 in atmosphere?
SO2(g) +NO2(g)--> SO3(g) +NO(g)
NO(g) + 1/2O2(g) ---> NO2(g)
| NO2 is a homogenous catalyst
NO2 is also an oxidising agent
139
Acid rain from SO3
SO3 + H2O---> H2SO4
140
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Consequences of acid rain
* Aquatic life
* Soil pH lowered
* buildings corroded
141
