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P Block Flashcards

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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
Q

Why can’t fluorine expand its octet?

A

It has no d-orbitals in its valence shell and is highly electronegative, exhibiting mostly –1 oxidation state.

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26
Q

What is the electronic configuration of Group 18 elements?

A

ns2np6

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27
Q

Why are noble gases considered zero valent?

A

They have no tendency to gain or lose electrons.

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28
Q

What unique property allows xenon to exhibit higher oxidation states?

A

It has an expandable d-orbital.

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29
Q

Provide examples of xenon compounds in higher oxidation states.

A
  • XeF2 (+2)
  • XeF4 (+4)
  • XeF6 (+6)
  • XeO3 (+6)
  • XeOF4 (+6)
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30
Q

What type of hydrides do Group 16 elements form with hydrogen?

A

H2E where E = O, S, Se, Te, Po

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31
Q

What is the acidic character of hydrides in Group 16?

A

Weakly acidic

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32
Q

As you move from H2O to H2Te, what happens to the acidic character and thermal stability?

A

Acidic character increases and thermal stability decreases.

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33
Q

Fill in the blank: The bond dissociation enthalpy of H−E bond ______ from H2O to H2Te.

A

decreases

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34
Q

Arrange the following hydrides in order of reducing property: H2S, H2Se, H2Te.

A

H2S < H2Se < H2Te

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35
Q

What is the order of acidic strength of hydrogen halides?

A

HF < HCl < HBr < HI

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36
Q

True or False: The thermal stability of hydrogen halides decreases in the order HF > HCl > HBr > HI.

A

True

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37
Q

What type of oxides do Group 16 elements form?

A

EO2 and EO3 where E = S, Se, Te, Po

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38
Q

What are the properties of SO2 and SeO2?

A
  • SO2 is a gas and acidic in nature.
  • SeO2 is solid and also acidic.
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39
Q

What do EO3 type oxides dissolve in water to form?

A

Acids

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40
Q

What is the chemical equation for the formation of sulphurous acid from SO2?

A

SO2 + H2O → H2SO3

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41
Q

What are the two thermally stable oxides formed by fluorine?

A

OF2 and O2F2

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42
Q

What is the stability trend of halogen oxides?

A

Higher oxides are more stable than lower ones.

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43
Q

What type of compounds do halogens form with themselves?

A

Interhalogen compounds

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44
Q

What is the chemical reaction for the formation of metal halides by halogens?

A

2Na(s) + Cl2(l) → 2NaCl(s)

45
Q

What is the trend of ionic character in metal halides?

A

MF > MCl > MBr > MI

46
Q

What are the two allotropes of oxygen?

A

O2 and O3 (ozone)

47
Q

What are the two important allotropes of sulfur?

A

Rhombic sulfur (α-sulfur) and Monoclinic sulfur (β-sulfur)

48
Q

What is the method of preparation for rhombic sulfur?

A

Evaporation of roll sulfur in CS2

49
Q

What is the acidic strength trend of halogen oxoacids?

A

Increases with increasing oxidation state of halogen.

50
Q

What are the stable oxoacids of halogens?

A
  • Hypofluorous acid (HOF)
  • Perchloric acid (HClO4)
  • Iodic acid (HIO3)
  • Metaperiodic acid (H2IO6)
51
Q

What are the laboratory methods for preparing dioxygen?

A
  • Heating oxygen-containing salts
  • Thermal decomposition of metal oxides
  • Decomposition of hydrogen peroxide
52
Q

What are the physical properties of dioxygen?

A
  • Colourless and odourless gas
  • Sparingly soluble in water
  • Liquefies at 90 K
  • Freezes at 55 K
53
Q

What is the primary use of dioxygen?

A

Respiration to sustain animal and aquatic life

54
Q

What is the reaction for the formation of sulfur trioxide from sulfur dioxide and oxygen?

A

2SO2 + O2 –⎯⎯→ 2SO3

55
Q

What is dioxygen’s role in respiration?

A

It sustains animal and aquatic life.

56
Q

List three uses of oxygen.

A
  • Manufacturing of steel
  • Oxyacetylene flame for welding and cutting
  • Oxygen cylinders in hospitals
57
Q

What is a binary compound of oxygen with another element called?

A

Oxide

58
Q

What type of oxide dissolves in water to give an acid?

A

Acidic oxide

59
Q

Provide an example of an acidic oxide.

A

SO2

60
Q

What characterizes a basic oxide?

A

It dissolves in water to give a base or reacts with an acid to give salt.

61
Q

Give an example of a basic oxide.

A

Na2O

62
Q

What is an amphoteric oxide?

A

An oxide that reacts with both an acid and a base.

63
Q

Provide an example of an amphoteric oxide.

A

Al2O3

64
Q

What are neutral oxides?

A

Oxides that are neither acidic nor basic.

65
Q

Provide an example of a neutral oxide.

A

CO

66
Q

What is ozone (O3)?

A

An allotrope of oxygen

67
Q

How is ozone formed in the upper atmosphere?

A

Oxygen absorbs UV light and changes to atomic oxygen, which combines with molecular oxygen.

68
Q

What is the protective function of the ozone layer?

A

It protects the earth’s surface from harmful UV radiations.

69
Q

What process is used to prepare ozone in the laboratory?

A

Passing silent electric discharge through pure and dry oxygen.

70
Q

What is the physical state of pure ozone?

A
  • Pale-blue gas
  • Dark blue liquid
  • Violet-black solid
71
Q

True or False: Ozone is a powerful oxidizing agent.

A

True

72
Q

What happens when ozone oxidizes lead sulfide?

A

It forms lead sulfate.

73
Q

What is ozone depletion?

A

Thinning of the ozone layer in the upper atmosphere.

74
Q

List two causes of ozone depletion.

A
  • NO from exhaust systems
  • Chloro-fluoro-carbons (freons)
75
Q

What are some uses of ozone?

A
  • Air purification
  • Sterilizing drinking water
  • Bleaching delicate fabrics
76
Q

What is the preparation reaction for sulfur dioxide from sulfur?

A

S(s) + O2(g) → SO2(g)

77
Q

What is the physical property of sulfur dioxide?

A

Colorless gas with a pungent smell.

78
Q

Sulfuric acid is produced by which process?

A

Contact process

79
Q

What is the first step in the manufacture of sulfuric acid?

A

Burning sulfur to produce sulfur dioxide.

80
Q

What is the density of sulfuric acid at 298 K?

A

1.84 g/cm3

81
Q

What characterizes chlorine gas?

A

Greenish-yellow color and pungent odor.

82
Q

What is the Deacon’s process used for?

A

Manufacturing chlorine.

83
Q

What happens when chlorine reacts with metals?

A

It forms chlorides.

84
Q

What is the reaction of chlorine with hydrogen?

A

H2 + Cl2 → 2HCl

85
Q

What is the boiling point of chlorine?

A

293 K

86
Q

What is the chemical reaction for the preparation of chlorine using manganese dioxide?

A

MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O

87
Q

What is the reaction of chlorine with hydrogen?

A

H2 + Cl2 → 2HCl

Chlorine has a great affinity for hydrogen, forming hydrochloric acid.

88
Q

What is the product of the reaction between chlorine and hydrogen sulfide?

A

2HCl + S

The reaction is represented as H2S + Cl2 → 2HCl + S.

89
Q

What happens when chlorine reacts with excess ammonia?

A

Produces ammonium chloride and nitrogen

The reaction is: 8NH3 + 3Cl2 → 6NH4Cl + N2.

90
Q

What is the result of chlorine reacting with hot concentrated alkali?

A

Produces chloride and chlorate

The reaction is: 6NaOH + 3Cl2 → 5NaCl + NaClO3 + 3H2O.

91
Q

What does chlorine produce when reacted with dry slaked lime?

A

Bleaching powder

The reaction is: 2Ca(OH)2 + 2Cl2 → Ca(OCl)2 + CaCl2 + 2H2O.

92
Q

What is the outcome of chlorine reacting with saturated hydrocarbons?

A

Gives substitution products

Example: CH4 + Cl2 → CH3Cl + HCl.

93
Q

True or False: Chlorine can oxidize ferrous salts to ferric salts.

A

True

Chlorine has oxidizing properties, as shown in: 2FeSO4 + H2SO4 + Cl2 → Fe2(SO4)3 + 2HCl.

94
Q

What is the chemical equation for the bleaching action of chlorine in the presence of moisture?

A

Cl2 + H2O → HOCl + HCl

This reaction produces hypochlorous acid, which has bleaching properties.

95
Q

What is the primary use of chlorine in water treatment?

A

Purification (sterilizing) of drinking water

Chlorine is widely used to disinfect water supplies.

96
Q

How was hydrogen chloride first prepared?

A

By heating common salt with concentrated sulfuric acid

This method was discovered by Glauber in 1648.

97
Q

What is the physical state of hydrogen chloride at room temperature?

A

Colorless and pungent smelling gas

It can be liquefied and freezes to a white crystalline solid.

98
Q

How does hydrogen chloride behave in water?

A

Highly soluble and ionizes to form H3O+ and Cl−

Aqueous HCl is a strong acid.

99
Q

What is aqua regia?

A

A mixture of concentrated HCl and concentrated HNO3

Aqua regia is capable of dissolving noble metals like gold and platinum.

100
Q

What are interhalogen compounds?

A

Binary compounds formed by different halogen atoms

They can be ionic or neutral, depending on the halogens involved.

101
Q

Fill in the blank: An interhalogen compound is regarded as the halide of a more _______ halogen.

A

Electropositive

This is due to the varying electronegativities of the halogens.

102
Q

What is the general formula for interhalogen compounds?

A

XX’ n

X is the more electropositive halogen, while X’ is the more electronegative one.

103
Q

What are the four types of interhalogen compounds based on their composition?

A
  • XX’
  • XX’3
  • XX’5
  • XX’7

Each type has different examples and properties based on the halogens involved.

104
Q

What property do all interhalogen compounds share?

A

They are all diamagnetic

This is due to the absence of unpaired electrons in their molecular structure.

105
Q

What noble gas can form compounds due to its lower ionization energy?

A

Xenon

Heavier noble gases like Kr, Xe, and Rn can form compounds.

106
Q

What is the outcome of the hydrolysis of XeF2?

A

Forms HF

The reaction is: 2XeF2 + 2H2O → 4HF + 2Xe + O2.

107
Q

What is a major use of helium?

A

For artificial breathing in asthma patients

Helium is also used in welding and as a coolant in various applications.

108
Q

What is the primary use of neon?

A

In neon discharge lamps and signs

Neon signs are highly visible and used for advertising.

109
Q

What is argon’s role in welding?

A

Produces an inert atmosphere

This helps prevent oxidation during the welding process.

Chemistry (3 decks)

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