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1
Q

What are p-block elements?

A

Elements where the differentiating electron enters the p-orbital of the outermost shell

P-block elements include groups 13 to 18 in the periodic table.

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2
Q

How many groups are in the p-block?

A

6 groups (13 to 18)

Each group corresponds to the number of electrons that can occupy the p-subshell.

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3
Q

What elements constitute Group 16?

A
  • Oxygen (8O)
  • Sulphur (16S)
  • Selenium (34Se)
  • Tellurium (52Te)
  • Polonium (84Po)

Group 16 is also known as the oxygen family or chalcogens.

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4
Q

What is the significance of the term ‘chalcogens’?

A

It means ‘ore forming’

Many metal ores are oxides or sulphides.

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5
Q

What percentage of air volume is composed of oxygen?

A

20.95%

Oxygen is the most abundant element on Earth.

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6
Q

What is the occurrence of sulphur in the Earth’s crust?

A

0.034% by mass

Mainly found in combined forms as sulphates and sulphides.

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7
Q

What elements constitute Group 17?

A
  • Fluorine (9F)
  • Chlorine (17Cl)
  • Bromine (35Br)
  • Iodine (53I)
  • Astatine (85At)

Group 17 is known as halogens.

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8
Q

Why are halogens highly reactive?

A

Due to high electronegativities

They are not found in a free state.

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9
Q

What is the main source of chlorine in seawater?

A

Sodium chloride (NaCl)

Seawater contains chlorides, bromides, and iodides.

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10
Q

What are the main noble gases in Group 18?

A
  • Helium (2He)
  • Neon (10Ne)
  • Argon (18Ar)
  • Krypton (36Kr)
  • Xenon (54Xe)
  • Radon (86Rn)

All noble gases except radon occur in the atmosphere.

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11
Q

What is the general electronic configuration for Group 16 elements?

A

ns2np4

This configuration is crucial for understanding their chemistry.

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12
Q

What happens to atomic and ionic radii down the groups?

A

They increase due to an increase in the number of shells

Across periods, they decrease due to increased effective nuclear charge.

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13
Q

What is the trend of ionization enthalpy in groups 16, 17, and 18?

A

High ionization enthalpy that decreases down the group

Increases across periods with increasing atomic number.

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14
Q

What are the common oxidation states of Group 16 elements?

A
  • -2
  • +2
  • +4
  • +6

Oxygen typically shows -2, +2 in OF2, and -1 in peroxides.

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15
Q

What is the most electronegative element in the periodic table?

A

Fluorine

Halogens have very high electronegativity.

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16
Q

What is the anomalous behavior of oxygen attributed to?

A
  • Small atomic size
  • High electronegativity
  • Absence of d-orbitals

These factors lead to unique properties compared to other group 16 elements.

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17
Q

What is the state of oxygen at room temperature?

A

Gas

Other group 16 elements are solids at room temperature.

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18
Q

What is the typical covalency of oxygen?

A

2

Other group 16 elements can exceed a covalency of four.

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19
Q

What defines the physical state of halogens at room temperature?

A
  • Fluorine and chlorine are gases
  • Bromine is a liquid
  • Iodine is a solid

This reflects their molecular weights and interactions.

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20
Q

What is the bond dissociation enthalpy order for halogen molecules?

A

Cl—Cl > Br—Br > F—F > I—I

This indicates the strength of the bonds among halogens.

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21
Q

What is the electron gain enthalpy trend in groups 16 and 17?

A

Becomes less negative down the group

Smaller atomic size results in less negative values for oxygen and fluorine compared to their heavier counterparts.

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22
Q

What is the significance of the inert pair effect?

A

Stability of higher oxidation states decreases down the group

This effect explains the behavior of elements in groups 13 to 16.

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23
Q

What characterizes the chemical behavior of noble gases?

A

They are zero valent and exist as monoatomic

This is due to their stable electronic configuration and lack of tendency to gain or lose electrons.

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24
Q

What oxidation states occur in oxides and oxoacids of Cl and Br?

A

+4 and +6

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25
Why can't fluorine expand its octet?
It has no d-orbitals in its valence shell and is highly electronegative, exhibiting mostly –1 oxidation state.
26
What is the electronic configuration of Group 18 elements?
ns2np6
27
Why are noble gases considered zero valent?
They have no tendency to gain or lose electrons.
28
What unique property allows xenon to exhibit higher oxidation states?
It has an expandable d-orbital.
29
Provide examples of xenon compounds in higher oxidation states.
* XeF2 (+2) * XeF4 (+4) * XeF6 (+6) * XeO3 (+6) * XeOF4 (+6)
30
What type of hydrides do Group 16 elements form with hydrogen?
H2E where E = O, S, Se, Te, Po
31
What is the acidic character of hydrides in Group 16?
Weakly acidic
32
As you move from H2O to H2Te, what happens to the acidic character and thermal stability?
Acidic character increases and thermal stability decreases.
33
Fill in the blank: The bond dissociation enthalpy of H−E bond ______ from H2O to H2Te.
decreases
34
Arrange the following hydrides in order of reducing property: H2S, H2Se, H2Te.
H2S < H2Se < H2Te
35
What is the order of acidic strength of hydrogen halides?
HF < HCl < HBr < HI
36
True or False: The thermal stability of hydrogen halides decreases in the order HF > HCl > HBr > HI.
True
37
What type of oxides do Group 16 elements form?
EO2 and EO3 where E = S, Se, Te, Po
38
What are the properties of SO2 and SeO2?
* SO2 is a gas and acidic in nature. * SeO2 is solid and also acidic.
39
What do EO3 type oxides dissolve in water to form?
Acids
40
What is the chemical equation for the formation of sulphurous acid from SO2?
SO2 + H2O → H2SO3
41
What are the two thermally stable oxides formed by fluorine?
OF2 and O2F2
42
What is the stability trend of halogen oxides?
Higher oxides are more stable than lower ones.
43
What type of compounds do halogens form with themselves?
Interhalogen compounds
44
What is the chemical reaction for the formation of metal halides by halogens?
2Na(s) + Cl2(l) → 2NaCl(s)
45
What is the trend of ionic character in metal halides?
MF > MCl > MBr > MI
46
What are the two allotropes of oxygen?
O2 and O3 (ozone)
47
What are the two important allotropes of sulfur?
Rhombic sulfur (α-sulfur) and Monoclinic sulfur (β-sulfur)
48
What is the method of preparation for rhombic sulfur?
Evaporation of roll sulfur in CS2
49
What is the acidic strength trend of halogen oxoacids?
Increases with increasing oxidation state of halogen.
50
What are the stable oxoacids of halogens?
* Hypofluorous acid (HOF) * Perchloric acid (HClO4) * Iodic acid (HIO3) * Metaperiodic acid (H2IO6)
51
What are the laboratory methods for preparing dioxygen?
* Heating oxygen-containing salts * Thermal decomposition of metal oxides * Decomposition of hydrogen peroxide
52
What are the physical properties of dioxygen?
* Colourless and odourless gas * Sparingly soluble in water * Liquefies at 90 K * Freezes at 55 K
53
What is the primary use of dioxygen?
Respiration to sustain animal and aquatic life
54
What is the reaction for the formation of sulfur trioxide from sulfur dioxide and oxygen?
2SO2 + O2 –⎯⎯→ 2SO3
55
What is dioxygen's role in respiration?
It sustains animal and aquatic life.
56
List three uses of oxygen.
* Manufacturing of steel * Oxyacetylene flame for welding and cutting * Oxygen cylinders in hospitals
57
What is a binary compound of oxygen with another element called?
Oxide
58
What type of oxide dissolves in water to give an acid?
Acidic oxide
59
Provide an example of an acidic oxide.
SO2
60
What characterizes a basic oxide?
It dissolves in water to give a base or reacts with an acid to give salt.
61
Give an example of a basic oxide.
Na2O
62
What is an amphoteric oxide?
An oxide that reacts with both an acid and a base.
63
Provide an example of an amphoteric oxide.
Al2O3
64
What are neutral oxides?
Oxides that are neither acidic nor basic.
65
Provide an example of a neutral oxide.
CO
66
What is ozone (O3)?
An allotrope of oxygen
67
How is ozone formed in the upper atmosphere?
Oxygen absorbs UV light and changes to atomic oxygen, which combines with molecular oxygen.
68
What is the protective function of the ozone layer?
It protects the earth's surface from harmful UV radiations.
69
What process is used to prepare ozone in the laboratory?
Passing silent electric discharge through pure and dry oxygen.
70
What is the physical state of pure ozone?
* Pale-blue gas * Dark blue liquid * Violet-black solid
71
True or False: Ozone is a powerful oxidizing agent.
True
72
What happens when ozone oxidizes lead sulfide?
It forms lead sulfate.
73
What is ozone depletion?
Thinning of the ozone layer in the upper atmosphere.
74
List two causes of ozone depletion.
* NO from exhaust systems * Chloro-fluoro-carbons (freons)
75
What are some uses of ozone?
* Air purification * Sterilizing drinking water * Bleaching delicate fabrics
76
What is the preparation reaction for sulfur dioxide from sulfur?
S(s) + O2(g) → SO2(g)
77
What is the physical property of sulfur dioxide?
Colorless gas with a pungent smell.
78
Sulfuric acid is produced by which process?
Contact process
79
What is the first step in the manufacture of sulfuric acid?
Burning sulfur to produce sulfur dioxide.
80
What is the density of sulfuric acid at 298 K?
1.84 g/cm3
81
What characterizes chlorine gas?
Greenish-yellow color and pungent odor.
82
What is the Deacon's process used for?
Manufacturing chlorine.
83
What happens when chlorine reacts with metals?
It forms chlorides.
84
What is the reaction of chlorine with hydrogen?
H2 + Cl2 → 2HCl
85
What is the boiling point of chlorine?
293 K
86
What is the chemical reaction for the preparation of chlorine using manganese dioxide?
MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O
87
What is the reaction of chlorine with hydrogen?
H2 + Cl2 → 2HCl ## Footnote Chlorine has a great affinity for hydrogen, forming hydrochloric acid.
88
What is the product of the reaction between chlorine and hydrogen sulfide?
2HCl + S ## Footnote The reaction is represented as H2S + Cl2 → 2HCl + S.
89
What happens when chlorine reacts with excess ammonia?
Produces ammonium chloride and nitrogen ## Footnote The reaction is: 8NH3 + 3Cl2 → 6NH4Cl + N2.
90
What is the result of chlorine reacting with hot concentrated alkali?
Produces chloride and chlorate ## Footnote The reaction is: 6NaOH + 3Cl2 → 5NaCl + NaClO3 + 3H2O.
91
What does chlorine produce when reacted with dry slaked lime?
Bleaching powder ## Footnote The reaction is: 2Ca(OH)2 + 2Cl2 → Ca(OCl)2 + CaCl2 + 2H2O.
92
What is the outcome of chlorine reacting with saturated hydrocarbons?
Gives substitution products ## Footnote Example: CH4 + Cl2 → CH3Cl + HCl.
93
True or False: Chlorine can oxidize ferrous salts to ferric salts.
True ## Footnote Chlorine has oxidizing properties, as shown in: 2FeSO4 + H2SO4 + Cl2 → Fe2(SO4)3 + 2HCl.
94
What is the chemical equation for the bleaching action of chlorine in the presence of moisture?
Cl2 + H2O → HOCl + HCl ## Footnote This reaction produces hypochlorous acid, which has bleaching properties.
95
What is the primary use of chlorine in water treatment?
Purification (sterilizing) of drinking water ## Footnote Chlorine is widely used to disinfect water supplies.
96
How was hydrogen chloride first prepared?
By heating common salt with concentrated sulfuric acid ## Footnote This method was discovered by Glauber in 1648.
97
What is the physical state of hydrogen chloride at room temperature?
Colorless and pungent smelling gas ## Footnote It can be liquefied and freezes to a white crystalline solid.
98
How does hydrogen chloride behave in water?
Highly soluble and ionizes to form H3O+ and Cl− ## Footnote Aqueous HCl is a strong acid.
99
What is aqua regia?
A mixture of concentrated HCl and concentrated HNO3 ## Footnote Aqua regia is capable of dissolving noble metals like gold and platinum.
100
What are interhalogen compounds?
Binary compounds formed by different halogen atoms ## Footnote They can be ionic or neutral, depending on the halogens involved.
101
Fill in the blank: An interhalogen compound is regarded as the halide of a more _______ halogen.
Electropositive ## Footnote This is due to the varying electronegativities of the halogens.
102
What is the general formula for interhalogen compounds?
XX' n ## Footnote X is the more electropositive halogen, while X' is the more electronegative one.
103
What are the four types of interhalogen compounds based on their composition?
* XX' * XX'3 * XX'5 * XX'7 ## Footnote Each type has different examples and properties based on the halogens involved.
104
What property do all interhalogen compounds share?
They are all diamagnetic ## Footnote This is due to the absence of unpaired electrons in their molecular structure.
105
What noble gas can form compounds due to its lower ionization energy?
Xenon ## Footnote Heavier noble gases like Kr, Xe, and Rn can form compounds.
106
What is the outcome of the hydrolysis of XeF2?
Forms HF ## Footnote The reaction is: 2XeF2 + 2H2O → 4HF + 2Xe + O2.
107
What is a major use of helium?
For artificial breathing in asthma patients ## Footnote Helium is also used in welding and as a coolant in various applications.
108
What is the primary use of neon?
In neon discharge lamps and signs ## Footnote Neon signs are highly visible and used for advertising.
109
What is argon's role in welding?
Produces an inert atmosphere ## Footnote This helps prevent oxidation during the welding process.
110
What are p-block elements?
Elements where the differentiating electron enters the p-orbital of the outermost shell ## Footnote P-block elements include groups 13 to 18 in the periodic table.
111
How many groups are in the p-block?
6 groups (13 to 18) ## Footnote Each group corresponds to the number of electrons that can occupy the p-subshell.
112
What elements constitute Group 16?
* Oxygen (8O) * Sulphur (16S) * Selenium (34Se) * Tellurium (52Te) * Polonium (84Po) ## Footnote Group 16 is also known as the oxygen family or chalcogens.
113
What is the significance of the term 'chalcogens'?
It means 'ore forming' ## Footnote Many metal ores are oxides or sulphides.
114
What percentage of air volume is composed of oxygen?
20.95% ## Footnote Oxygen is the most abundant element on Earth.
115
What is the occurrence of sulphur in the Earth's crust?
0.034% by mass ## Footnote Mainly found in combined forms as sulphates and sulphides.
116
What elements constitute Group 17?
* Fluorine (9F) * Chlorine (17Cl) * Bromine (35Br) * Iodine (53I) * Astatine (85At) ## Footnote Group 17 is known as halogens.
117
Why are halogens highly reactive?
Due to high electronegativities ## Footnote They are not found in a free state.
118
What is the main source of chlorine in seawater?
Sodium chloride (NaCl) ## Footnote Seawater contains chlorides, bromides, and iodides.
119
What are the main noble gases in Group 18?
* Helium (2He) * Neon (10Ne) * Argon (18Ar) * Krypton (36Kr) * Xenon (54Xe) * Radon (86Rn) ## Footnote All noble gases except radon occur in the atmosphere.
120
What is the general electronic configuration for Group 16 elements?
ns2np4 ## Footnote This configuration is crucial for understanding their chemistry.
121
What happens to atomic and ionic radii down the groups?
They increase due to an increase in the number of shells ## Footnote Across periods, they decrease due to increased effective nuclear charge.
122
What is the trend of ionization enthalpy in groups 16, 17, and 18?
High ionization enthalpy that decreases down the group ## Footnote Increases across periods with increasing atomic number.
123
What are the common oxidation states of Group 16 elements?
* -2 * +2 * +4 * +6 ## Footnote Oxygen typically shows -2, +2 in OF2, and -1 in peroxides.
124
What is the most electronegative element in the periodic table?
Fluorine ## Footnote Halogens have very high electronegativity.
125
What is the anomalous behavior of oxygen attributed to?
* Small atomic size * High electronegativity * Absence of d-orbitals ## Footnote These factors lead to unique properties compared to other group 16 elements.
126
What is the state of oxygen at room temperature?
Gas ## Footnote Other group 16 elements are solids at room temperature.
127
What is the typical covalency of oxygen?
2 ## Footnote Other group 16 elements can exceed a covalency of four.
128
What defines the physical state of halogens at room temperature?
* Fluorine and chlorine are gases * Bromine is a liquid * Iodine is a solid ## Footnote This reflects their molecular weights and interactions.
129
What is the bond dissociation enthalpy order for halogen molecules?
Cl—Cl > Br—Br > F—F > I—I ## Footnote This indicates the strength of the bonds among halogens.
130
What is the electron gain enthalpy trend in groups 16 and 17?
Becomes less negative down the group ## Footnote Smaller atomic size results in less negative values for oxygen and fluorine compared to their heavier counterparts.
131
What is the significance of the inert pair effect?
Stability of higher oxidation states decreases down the group ## Footnote This effect explains the behavior of elements in groups 13 to 16.
132
What characterizes the chemical behavior of noble gases?
They are zero valent and exist as monoatomic ## Footnote This is due to their stable electronic configuration and lack of tendency to gain or lose electrons.
133
What oxidation states occur in oxides and oxoacids of Cl and Br?
+4 and +6
134
Why can't fluorine expand its octet?
It has no d-orbitals in its valence shell and is highly electronegative, exhibiting mostly –1 oxidation state.
135
What is the electronic configuration of Group 18 elements?
ns2np6
136
Why are noble gases considered zero valent?
They have no tendency to gain or lose electrons.
137
What unique property allows xenon to exhibit higher oxidation states?
It has an expandable d-orbital.
138
Provide examples of xenon compounds in higher oxidation states.
* XeF2 (+2) * XeF4 (+4) * XeF6 (+6) * XeO3 (+6) * XeOF4 (+6)
139
What type of hydrides do Group 16 elements form with hydrogen?
H2E where E = O, S, Se, Te, Po
140
What is the acidic character of hydrides in Group 16?
Weakly acidic
141
As you move from H2O to H2Te, what happens to the acidic character and thermal stability?
Acidic character increases and thermal stability decreases.
142
Fill in the blank: The bond dissociation enthalpy of H−E bond ______ from H2O to H2Te.
decreases
143
Arrange the following hydrides in order of reducing property: H2S, H2Se, H2Te.
H2S < H2Se < H2Te
144
What is the order of acidic strength of hydrogen halides?
HF < HCl < HBr < HI
145
True or False: The thermal stability of hydrogen halides decreases in the order HF > HCl > HBr > HI.
True
146
What type of oxides do Group 16 elements form?
EO2 and EO3 where E = S, Se, Te, Po
147
What are the properties of SO2 and SeO2?
* SO2 is a gas and acidic in nature. * SeO2 is solid and also acidic.
148
What do EO3 type oxides dissolve in water to form?
Acids
149
What is the chemical equation for the formation of sulphurous acid from SO2?
SO2 + H2O → H2SO3
150
What are the two thermally stable oxides formed by fluorine?
OF2 and O2F2
151
What is the stability trend of halogen oxides?
Higher oxides are more stable than lower ones.
152
What type of compounds do halogens form with themselves?
Interhalogen compounds
153
What is the chemical reaction for the formation of metal halides by halogens?
2Na(s) + Cl2(l) → 2NaCl(s)
154
What is the trend of ionic character in metal halides?
MF > MCl > MBr > MI
155
What are the two allotropes of oxygen?
O2 and O3 (ozone)
156
What are the two important allotropes of sulfur?
Rhombic sulfur (α-sulfur) and Monoclinic sulfur (β-sulfur)
157
What is the method of preparation for rhombic sulfur?
Evaporation of roll sulfur in CS2
158
What is the acidic strength trend of halogen oxoacids?
Increases with increasing oxidation state of halogen.
159
What are the stable oxoacids of halogens?
* Hypofluorous acid (HOF) * Perchloric acid (HClO4) * Iodic acid (HIO3) * Metaperiodic acid (H2IO6)
160
What are the laboratory methods for preparing dioxygen?
* Heating oxygen-containing salts * Thermal decomposition of metal oxides * Decomposition of hydrogen peroxide
161
What are the physical properties of dioxygen?
* Colourless and odourless gas * Sparingly soluble in water * Liquefies at 90 K * Freezes at 55 K
162
What is the primary use of dioxygen?
Respiration to sustain animal and aquatic life
163
What is the reaction for the formation of sulfur trioxide from sulfur dioxide and oxygen?
2SO2 + O2 –⎯⎯→ 2SO3
164
What is dioxygen's role in respiration?
It sustains animal and aquatic life.
165
List three uses of oxygen.
* Manufacturing of steel * Oxyacetylene flame for welding and cutting * Oxygen cylinders in hospitals
166
What is a binary compound of oxygen with another element called?
Oxide
167
What type of oxide dissolves in water to give an acid?
Acidic oxide
168
Provide an example of an acidic oxide.
SO2
169
What characterizes a basic oxide?
It dissolves in water to give a base or reacts with an acid to give salt.
170
Give an example of a basic oxide.
Na2O
171
What is an amphoteric oxide?
An oxide that reacts with both an acid and a base.
172
Provide an example of an amphoteric oxide.
Al2O3
173
What are neutral oxides?
Oxides that are neither acidic nor basic.
174
Provide an example of a neutral oxide.
CO
175
What is ozone (O3)?
An allotrope of oxygen
176
How is ozone formed in the upper atmosphere?
Oxygen absorbs UV light and changes to atomic oxygen, which combines with molecular oxygen.
177
What is the protective function of the ozone layer?
It protects the earth's surface from harmful UV radiations.
178
What process is used to prepare ozone in the laboratory?
Passing silent electric discharge through pure and dry oxygen.
179
What is the physical state of pure ozone?
* Pale-blue gas * Dark blue liquid * Violet-black solid
180
True or False: Ozone is a powerful oxidizing agent.
True
181
What happens when ozone oxidizes lead sulfide?
It forms lead sulfate.
182
What is ozone depletion?
Thinning of the ozone layer in the upper atmosphere.
183
List two causes of ozone depletion.
* NO from exhaust systems * Chloro-fluoro-carbons (freons)
184
What are some uses of ozone?
* Air purification * Sterilizing drinking water * Bleaching delicate fabrics
185
What is the preparation reaction for sulfur dioxide from sulfur?
S(s) + O2(g) → SO2(g)
186
What is the physical property of sulfur dioxide?
Colorless gas with a pungent smell.
187
Sulfuric acid is produced by which process?
Contact process
188
What is the first step in the manufacture of sulfuric acid?
Burning sulfur to produce sulfur dioxide.
189
What is the density of sulfuric acid at 298 K?
1.84 g/cm3
190
What characterizes chlorine gas?
Greenish-yellow color and pungent odor.
191
What is the Deacon's process used for?
Manufacturing chlorine.
192
What happens when chlorine reacts with metals?
It forms chlorides.
193
What is the reaction of chlorine with hydrogen?
H2 + Cl2 → 2HCl
194
What is the boiling point of chlorine?
293 K
195
What is the chemical reaction for the preparation of chlorine using manganese dioxide?
MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O
196
What is the reaction of chlorine with hydrogen?
H2 + Cl2 → 2HCl ## Footnote Chlorine has a great affinity for hydrogen, forming hydrochloric acid.
197
What is the product of the reaction between chlorine and hydrogen sulfide?
2HCl + S ## Footnote The reaction is represented as H2S + Cl2 → 2HCl + S.
198
What happens when chlorine reacts with excess ammonia?
Produces ammonium chloride and nitrogen ## Footnote The reaction is: 8NH3 + 3Cl2 → 6NH4Cl + N2.
199
What is the result of chlorine reacting with hot concentrated alkali?
Produces chloride and chlorate ## Footnote The reaction is: 6NaOH + 3Cl2 → 5NaCl + NaClO3 + 3H2O.
200
What does chlorine produce when reacted with dry slaked lime?
Bleaching powder ## Footnote The reaction is: 2Ca(OH)2 + 2Cl2 → Ca(OCl)2 + CaCl2 + 2H2O.
201
What is the outcome of chlorine reacting with saturated hydrocarbons?
Gives substitution products ## Footnote Example: CH4 + Cl2 → CH3Cl + HCl.
202
True or False: Chlorine can oxidize ferrous salts to ferric salts.
True ## Footnote Chlorine has oxidizing properties, as shown in: 2FeSO4 + H2SO4 + Cl2 → Fe2(SO4)3 + 2HCl.
203
What is the chemical equation for the bleaching action of chlorine in the presence of moisture?
Cl2 + H2O → HOCl + HCl ## Footnote This reaction produces hypochlorous acid, which has bleaching properties.
204
What is the primary use of chlorine in water treatment?
Purification (sterilizing) of drinking water ## Footnote Chlorine is widely used to disinfect water supplies.
205
How was hydrogen chloride first prepared?
By heating common salt with concentrated sulfuric acid ## Footnote This method was discovered by Glauber in 1648.
206
What is the physical state of hydrogen chloride at room temperature?
Colorless and pungent smelling gas ## Footnote It can be liquefied and freezes to a white crystalline solid.
207
How does hydrogen chloride behave in water?
Highly soluble and ionizes to form H3O+ and Cl− ## Footnote Aqueous HCl is a strong acid.
208
What is aqua regia?
A mixture of concentrated HCl and concentrated HNO3 ## Footnote Aqua regia is capable of dissolving noble metals like gold and platinum.
209
What are interhalogen compounds?
Binary compounds formed by different halogen atoms ## Footnote They can be ionic or neutral, depending on the halogens involved.
210
Fill in the blank: An interhalogen compound is regarded as the halide of a more _______ halogen.
Electropositive ## Footnote This is due to the varying electronegativities of the halogens.
211
What is the general formula for interhalogen compounds?
XX' n ## Footnote X is the more electropositive halogen, while X' is the more electronegative one.
212
What are the four types of interhalogen compounds based on their composition?
* XX' * XX'3 * XX'5 * XX'7 ## Footnote Each type has different examples and properties based on the halogens involved.
213
What property do all interhalogen compounds share?
They are all diamagnetic ## Footnote This is due to the absence of unpaired electrons in their molecular structure.
214
What noble gas can form compounds due to its lower ionization energy?
Xenon ## Footnote Heavier noble gases like Kr, Xe, and Rn can form compounds.
215
What is the outcome of the hydrolysis of XeF2?
Forms HF ## Footnote The reaction is: 2XeF2 + 2H2O → 4HF + 2Xe + O2.
216
What is a major use of helium?
For artificial breathing in asthma patients ## Footnote Helium is also used in welding and as a coolant in various applications.
217
What is the primary use of neon?
In neon discharge lamps and signs ## Footnote Neon signs are highly visible and used for advertising.
218
What is argon's role in welding?
Produces an inert atmosphere ## Footnote This helps prevent oxidation during the welding process.

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