-
What is the oxidation state of K in\[K{{O}_{2}}\]?
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The \[{{E}^{o}}\] for
\[C{{l}_{2}}/C{{l}^{-}}\]is + 1.36, for iodine \[{{I}_{2}}/{{I}^{-}}\]is +0.53,
for \[A{{g}^{+}}/Ag\]is \[+0.79\],\[N{{a}^{+}}/Na\] is\[-2.71\]and for\[L{{i}^{+}}/Li\]
is\[-\text{ }3.04\]. Arrange the following species in order of reducing
strength: \[{{I}^{-}},Ag,C{{l}^{-}},Li,Na\]
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Why is \[K{{O}_{2}}\] paramagnetic?
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-
Why does the solubility of alkaline earth metal hydroxides
in water increase down the group?
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Why does the solubility of alkaline earth metal carbonates
and sulphates in water decreases down the group?
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-
What are the common physical and chemical features of alkali
metals?
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-
Discuss the general characteristics and gradation in properties
of alkaline earth metals:
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Why alkali metals do not found free in nature?
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-
Find the oxidation state of sodium in\[N{{a}_{2}}{{O}_{2}}\].
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Explain why is sodium less reactive than potassium?
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-
Compare the alkali metals and alkaline earth metals with
respect to (i) ionisation enthalpy (ii) basicity of oxides (iii) solubility of
hydroxides.
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In what ways lithium shows similarities to magnesium in its
chemical behaviour?
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Explain why can alkali and alkaline earth metals not be obtained
by chemical reduction methods?
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-
Why are potassium and caesium, rather than lithium used in
photoelectric cells?
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-
When an alkali metal dissolves in liquid ammonia, the solution
can acquire different colours. Explain the reasons for this type of colour
change.
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Beryllium and magnesium do not give colour to flame whereas
other alkaline earth metals do so. Why?
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-
Discuss the various reactions that occur in the Solvay ammonia
process.
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Potassium carbonate cannot be prepared by Solvay process.
Why?
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-
Why does \[L{{i}_{2}}C{{O}_{3}}\] decompose at lower
temperature whereas \[N{{a}_{2}}C{{O}_{3}}\]at higher temperature?
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-
Compare the solubility and thermal
stability of the following compounds of the alkali metals with those of
alkaline earth metals:
(a) nitrates
(b) carbonates
(c) sulphates.
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Starting with sodium chloride,
how would you proceed to prepare :
(i) sodium metal (ii) sodium hydroxide (iii) sodium peroxide
(iv) sodium carbonate?
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What happens when :
(i) Magnesium
is burnt in air?
(ii) Quick
lime is heated with silica?
(iii) Chlorine
reacts with slaked lime?
(iv) Calcium nitrate
is heated?
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Describe two important uses of
each of the following:
(i) Caustic soda (ii) sodium carbonate (iii) quick lime.
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Draw the structure of: (i) \[BeC{{l}_{2}}\] (vapour state)
(ii)\[BeC{{l}_{2}}\] (solid).
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-
The hydroxides and carbonates of sodium and potassium are
easily soluble in water while the corresponding salts of magnesium and calcium
are sparingly soluble in water. Explain.
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-
Describe the importance of: (i) limestone (ii) Cement(iii)
Plaster of Paris.
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Why are lithium salts commonly hydrated and those of other
alkali ions are usually anhydrous?
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Why \[LiF\] is almost insoluble in water whereas \[LiCl\]soluble
not only in water but also in acetone?
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-
Explain the significance of sodium, potassium, magnesium and
calcium in biological fluids.
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-
What happens when:
(i) sodium is
dropped in water?
(ii) sodium metal is
heated in free supply of air?
(iii) sodium peroxide is dissolved in water?
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Comment on each of
the following observations:
(a) The
mobilities of alkali metal ions in aqueous solutions are
\[L{{i}^{+}}
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State as to why:
(a) a solution of \[N{{a}_{2}}C{{O}_{3}}\]is
alkaline?
(b) alkali metals
are prepared by electrolysis of their fused chlorides?
(c) sodium is found to be more useful than potassium?
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Write balanced equations for
the reactions between:
(a)\[N{{a}_{2}}{{O}_{2}}\]and
water (b) \[K{{O}_{2}}\]and water
(c)\[{{N}_{2}}O\]and\[C{{O}_{2}}\].
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How would you
explain?
(i) \[BeO\]
is insoluble but \[BeS{{O}_{4}}\] is soluble in water.
(ii) \[BaO\]
is soluble but\[BaS{{O}_{4}}\] is insoluble in water.
(iii) \[LiI\] is
more soluble than \[KI\] in ethanol.
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Which of the alkali metals is
having least melting point?
(a) Na (b) K (c) \[Rb\] (d) Cs
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Which of the following alkali
metals gives hydrated salts?
(a) Li (b) Na (c) K (d) Cs
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Which one of the
alkaline earth metal carbonates is thermally the most stable?
(a)\[MgC{{O}_{3}}\] (b)
\[CaC{{O}_{3}}\]
(c) \[SrC{{O}_{3}}\] (d)
\[BaC{{O}_{3}}\]
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question_answer38)
The alkali metals are low melting. Which
of the following alkali metal is expected to melt if the room temperature rises
to\[30{}^\circ C\]?
(a)\[Na\] (b)
\[K\] (c) \[Rb\] (d)
\[Cs\]
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question_answer39)
Alkali metals react with water
vigorously to form hydroxides and dihydrogen. Which of the following alkali
metals reacts with water least vigorously?
(a) Li (b) Na (c)
K (d) Cs
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question_answer40)
The reducing power of a metal
depends on various factors. Suggest the factor which makes lithium, the
strongest reducing agent in aqueous solution :
(a) sublimation enthalpy (b)
ionisation enthalpy
(c) hydration enthalpy (d)
electron gain enthalpy
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question_answer41)
Metal carbonates decompose on
heating to give metal oxide and carbon dioxide. Which of the metal carbonates
is most stable thermally?
(a) \[MgC{{O}_{3}}\] (b)
\[CaC{{O}_{3}}\] (c) \[SrC{{O}_{3}}\] (d)
\[BeC{{O}_{3}}\]
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question_answer42)
Which of the carbonates given
below is unstable in air and is kept in \[C{{O}_{2}}\] atmosphere to avoid
decomposition?
(a)\[BeC{{O}_{3}}\] (b)
\[MgC{{O}_{3}}\] (c) \[CaC{{O}_{3}}\] (d)
\[BaC{{O}_{3}}\]
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question_answer43)
Metals form basic hydroxides.
Which of the following metal hydroxides is the least basic?
(a) \[Mg{{(OH)}_{2}}\] (b)\[Ca{{(OH)}_{2}}\] (c)
\[Sr{{(OH)}_{2}}\] (d) \[Ba{{(OH)}_{2}}\]
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question_answer44)
Some of the group 2 metal
halides are covalent and soluble in organic solvents. Among the following metal
halides the one which is soluble in ethanol is :
(a)\[BeC{{l}_{2}}\] (b)
\[MgC{{l}_{2}}\] (c) \[CaC{{l}_{2}}\] (d)
\[SrC{{l}_{2}}\]
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question_answer45)
The order of decreasing
ionisation enthalpy in alkali metals is :
(a)\[~Na\text{ }>\text{
}Li\text{ }>\text{ }K\text{ }>\text{ }Rb\] (b)
\[Rb\text{ }<\text{ }Na\text{ }<\text{ }K\text{ }<\text{ }Li\]
(c)\[Li>Na>K>Rb~~~~\] (d)
\[K<\text{ }Li\text{ }<\text{ }Na\text{ }<\text{ }Rb\]
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question_answer46)
The solubility of metal halides
depends on their nature, lattice enthalpy and hydration enthalpy of the
individual ions. Amongst fluorides of alkali metals the lowest solubility of\[~LiF\]
in water is due to :
(a) ionic nature of lithium
fluoride (b) high lattice enthalpy
(c) high hydration enthalpy for
Li-ion (d) low ionisation enthalpy of Li-atom
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question_answer47)
Amphoteric hydroxides react with
both alkalies and acids.
Which of the following group 2
metal hydroxides is soluble in sodium hydroxide?
(a) \[Be{{(OH)}_{2}}\] (b)
\[Mg{{(OH)}_{2}}\] (c) \[Ca{{(OH)}_{2}}\] (d)
\[Ba{{(OH)}_{2}}\]
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question_answer48)
In the synthesis of sodium
carbonate, the recovery of ammonia is done by treating \[N{{H}_{4}}Cl\] with\[Ca{{(OH)}_{2}}\].
The by product obtained in this process is :
(a) \[CaC{{l}_{2}}\] (b)
\[NaCl\] (c) \[NaOH\] (d) \[NaHC{{O}_{3}}\]
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question_answer49)
When sodium is dissolved in
liquid ammonia, a solution of deep blue colour is obtained. The colour of the
solution is due to :
(a) ammoniated electron (b)
sodium ion
(c) sodium amide (d)
ammoniated sodium ion
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question_answer50)
By adding gypsum to
cement:
(a) setting time of cement
becomes less (b) setting time of cement increases
(c) colour of cement becomes
light (d) shining surface is obtained
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question_answer51)
Dead burnt plaster is :
(a) \[CaS{{O}_{4}}\] (b)
\[CaS{{O}_{4}}\cdot \frac{1}{2}{{H}_{2}}O\] (c) \[CaS{{O}_{4}}\cdot
{{H}_{2}}O\] (d) \[CaS{{O}_{4}}\cdot 2{{H}_{2}}O\]
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question_answer52)
Suspension of slaked lime in
water is known as:
(a) lime water (b)
quick lime (c) milk of lime (d) aqueous
solution of slaked lime
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question_answer53)
Which of the following elements
does not form hydride by direct heating with dihydrogen?
(a)\[Be\] (b)\[Mg\] (c)\[Sr\] (d)
\[Ba\]
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question_answer54)
The formula of soda ash is:
(a) \[N{{a}_{2}}C{{O}_{3}}.10{{H}_{2}}O\] (b)
\[N{{a}_{2}}C{{O}_{3}}\cdot 2{{H}_{2}}O\] (c)\[N{{a}_{2}}C{{O}_{3}}\cdot
{{H}_{2}}O\] (d) \[N{{a}_{2}}C{{O}_{3}}\]
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question_answer55)
A substance which gives brick
red flame and breaks down on heating to give oxygen and a brown gas is:
(a) magnesium nitrate (b)
calcium nitrate (c) barium nitrate (d) strontium nitrate
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question_answer56)
Which of the following
statements is true about\[Ca{{(OH)}_{2}}\]?
(a) It is used in the
preparation of bleaching powder
(b) It is a light blue solid
(c) It does not possess
disinfectant property
(d) It is used in the
manufacture of cement
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question_answer57)
A chemical ?A? is used for the
preparation of washing soda to recover ammonia. When \[C{{O}_{2}}\] is bubbled
through an aqueous solution turns milky. It is used in white washing due to
disinfectant nature. What is the chemical formula of ?A??
(a) \[Ca{{(HC{{O}_{3}})}_{2}}\] (b)
\[CaO\] (c) \[Ca{{(OH)}_{2}}\] (d) \[CaC{{O}_{3}}\]
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question_answer58)
Dehydration of hydration of
halides of calcium, barium and strontium i.e.,\[CaC{{l}_{2}}\cdot
6{{H}_{2}}O,BaC{{l}_{2}},2{{H}_{2}}O,SrC{{l}_{2}}\cdot 2{{H}_{2}}O\]can be
achieved by heating. These become wet on keeping in air. Which of the following
statements is correct about these halides?
(a) Act as dehydrating agent
(b) Can absorb moisture from air
(c) Tendency to form hydrate
decreases from calcium to barium
(d) All of the above
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question_answer59)
Metallic elements are described by
their standard electrode potential, fusion enthalpy, atomic size, etc. The
alkali metals are characterised by which of the following properties?
(a) High boiling point (b)
High negative standard electrode potential
(c) High density (d)
Large atomic size
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question_answer60)
Several sodium compounds find
use in industries. Which of the following compounds are used in textile
industry?
(a) \[N{{a}_{2}}C{{O}_{3}}\] (b)
\[NaHC{{O}_{3}}\] (c)\[NaOH\] (d)\[~NaCI\]
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question_answer61)
Which of the following compounds
are readily soluble in water?
(a)\[BeS{{O}_{4}}\] (b)
\[MgS{{O}_{4}}\] (c)\[BaS{{O}_{4}}\] (d)\[~SrS{{O}_{4}}\]
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question_answer62)
When zeolite which is hydrated
sodium aluminium silicate is treated with hard water, the sodium ions are
exchanged with which of the ion(s)?
(a)\[{{H}^{+}}\]ions (b)
\[M{{g}^{2+}}\] ions (c) \[C{{a}^{2+}}\]ions (d)
\[SO_{4}^{2-}\] ions
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question_answer63)
Identify the correct formula of
halides of alkaline earth metals from the following :
(a) \[BaC{{l}_{2}}\cdot
2{{H}_{2}}O\] (b) \[BaC{{l}_{2}}\cdot 4{{H}_{2}}O\] (c) \[CaC{{l}_{2}}\cdot
6{{H}_{2}}O\] (d) \[SrC{{l}_{2}}\cdot 4{{H}_{2}}O\]
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question_answer64)
Choose the correct statements
from the following :
(a) Beryllium is not readily
attacked by acids because of the presence of an oxide film on the surface of
the metal
(b) Beryllium sulphate is
readily soluble in water as the greater hydration enthalpy of \[B{{e}^{2+}}\]
overcomes the lattice enthalpy factor
(c) Beryllium exhibits
coordination number more than four
(d) Beryllium oxide is purely
acidic in nature
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question_answer65)
Which of the following are
correct reasons for anomalous behaviour of lithium?
(a) Exceptionally small size of
its atom (b) Its high polarising power
(c) It has high degree of
hydration (d) Exceptionally low ionisation enthalpy
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question_answer66)
How do you account for strong
reducing power of lithium in aqueous solution?
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question_answer67)
When heated in air, the alkali
metals form various oxide. Mention the oxides formed by Li, Na and K.
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question_answer68)
Complete the following reactions
:
(i) \[O_{2}^{2-}+{{H}_{2}}O\to
\]
(ii) \[O_{2}^{-}+{{H}_{2}}O\to
\]
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question_answer69)
Lithium resembles magnesium in
some of its properties. Mention properties and give reasons for this
resemblance.
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question_answer70)
Name an element of group 2 which
forms an amphoteric oxide and a water soluble sulphate.
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question_answer71)
Discuss the trend if the
following :
(a) Thermal stability of
carbonates of group 2 elements.
(b) The solubility and nature of
oxides of group 2 elements.
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question_answer72)
Why are \[BeS{{O}_{4}}\] and \[MgS{{O}_{4}}\]
readily soluble in water while\[CaS{{O}_{4}}\] and \[BaS{{O}_{4}}\] are insoluble?
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question_answer73)
All compounds of alkali metals
are easily soluble in water but lithium compounds are more soluble in organic solvents.
Explain.
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question_answer74)
In the Solvay process, can we
obtain sodium carbonate directly by treating the solution containing \[{{(N{{H}_{4}})}_{2}}C{{O}_{3}}\]
with sodium chloride? Explain.
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question_answer75)
Write Lewis structure of \[O_{2}^{-}\]
ion and find out the oxidation state of each oxygen atom. What is the average
oxidation state of oxygen in this ion?
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question_answer76)
Why do beryllium and magnesium
not impart colour to the flame in the flame test?
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question_answer77)
What is the structure of \[BeC{{l}_{2}}\]
molecule in gaseous and solid state?
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question_answer78)
In the following questions
more than one option of column I and column II may be correlated:
Match the elements given in
column I with the properties mentioned in column II.
|
Column I
|
Column II
|
|
(i)
|
\[Li\]
|
(a)
|
Insoluble sulphate
|
|
(ii)
|
\[Na\]
|
(b)
|
Strongest mono acidic base
|
|
(iii)
|
\[Ca\]
|
(c)
|
Most negative \[{{E}^{{}^\circ }}\] value
among alkali metals
|
|
(iv)
|
Ba
|
(d)
|
Insoluble oxalate
|
|
|
|
(e)
|
\[6{{s}^{2}}\]outer electronic
configuration
|
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question_answer79)
Match the compounds given in
column I with their uses mentioned in column II.
|
|
Column I
|
|
Column II
|
|
(i)
|
\[CaC{{O}_{3}}\]
|
(a)
|
Dentistry ornamental work
|
|
(ii)
|
\[Ca{{(OH)}_{2}}\]
|
(b)
|
Manufacture of caustic soda
|
|
(iii)
|
\[CaO\]
|
(c)
|
Used in paints and distempers
|
|
(iv)
|
\[2CaS{{O}_{4}}\cdot {{H}_{2}}O\]
|
(d)
|
Used in white washing
|
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question_answer80)
Match the elements given in
column I with colour they impart to the flame given in column II.
|
|
Column I
|
Column II
|
|
(i)
|
\[Cs\]
|
(a) Apple green
|
|
(ii)
|
\[Na\]
|
(b) Violet
|
|
(iii)
|
\[K\]
|
(c) Brick red
|
|
(iv)
|
\[Ca\]
|
(d) Yellow
|
|
(V)
|
\[Sr\]
|
(e) Crimson red
|
|
(vi)
|
\[Ba\]
|
(f) Blue
|
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question_answer81)
In the following questions a
statement of Assertion (A) followed by a statement of Reason (R) is given.
Choose the correct option out of the choices given below each question.
Assertion (A): The
carbonate of lithium decomposes easily on heating to form lithium oxide and\[C{{O}_{2}}\].
Reason (R): Lithium being
very small in size polarises large carbonate ion leading to the formation of
more stable\[L{{i}_{2}}O\]and \[C{{O}_{2}}\]
(a) Both A and R
are correct and R is the correct explanation of A.
(b) Both A and R
are correct and R is not the correct explanation of A.
(c) Both A and R
are not correct.
(d) A is not correct but R
is correct.
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question_answer82)
Assertion (A): Beryllium carbonate
is kept in the atmosphere of\[C{{O}_{2}}\].
Reason (R): Beryllium
carbonate is unstable and decomposes to give beryllium oxide and carbon
dioxide.
(a) Both A and R
are correct and R is the correct explanation of A.
(b) Both A and R
are correct and R is not the correct explanation of A.
(c) Both A and R
are not correct.
(d) A is not correct but R
is correct.
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question_answer83)
The s-block elements are characterised
by their-large atomic sizes lower ionisation enthalpies, invariable +1 oxidation
state and solubility of their oxosalts. In the light of these features describe
the nature of their oxides, halides and oxosalts.
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question_answer84)
Present a comparative account of
the alkali and alkaline earth metals with respect to following characteristics:
(i) Tendency to form
ionic/covalent compounds.
(ii) Nature of oxides and their
solubility in water.
(iii) Formation of oxosalts.
(iv) Solubility of oxosalts.
(v) Thermal stability of oxosalts.
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question_answer85)
When a metal of group I was dissolved in
liquid ammonia, the following observations were obtained :
(i) Blue solution was obtained
initially.
(ii) On concentrating the
solution, the blue colour changed to bronze colour. How do you account for the
blue colour of the solution? Give the name of the product formed on keeping the
solution for some time.
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question_answer86)
The stability of peroxide and
superoxide of alkali metals increase as we go down the group. Explain giving
reason.
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question_answer87)
When water is added to compound
(A) of calcium, solution of compound (B) is formed. When \[C{{O}_{2}}\] is
passed into the solution, it turns milky due to formation of compound (C). If
excess of \[C{{O}_{2}}\] is passed into the solution, milkiness disappears due
to formation of compound (D). Identify the compounds (A), (B), (C) and (D).
Explain why milkiness disappears in the last step?
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question_answer88)
Lithium hydride can be used to
prepare other useful hydrides. Beryllium hydride is one of them. Suggest a
route for the preparation of beryllium hydride starting from lithium hydride.
Write chemical equations involved in the process.
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question_answer89)
An element of group 2 forms
covalent oxide which is amphoteric in nature and dissolves in water to give an amphoteric
hydroxide. Identify the element and write chemical reactions of the hydroxide
of the element with an alkali and an acid.
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question_answer90)
Ions of an element of group I
participate in the transmission of nerve signals and transport of sugars and amino
acids into cells. This element imparts yellow colour to the flame in flame test
and forms an oxide and a peroxide with oxygen. Identify the element and write chemical
reaction to show the formation of its peroxide. Why does the element impart colour
to the flame?
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