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Alkali Metals - Practice Questions & MCQ

Edited By admin | Updated on Sep 18, 2023 18:35 AM | #JEE Main

Quick Facts

  • Chemical Properties of Alkali Metals - 1, Chemical Properties of Alkali Metals - 2 is considered one of the most asked concept.

  • 190 Questions around this concept.

Solve by difficulty

In which of the following species is the underlined carbon having sp^{3} hybridisation?

The ionic mobility of alkali metal ions in aqueous solution is maximum for

Which one among the following metals is the weakest reducing agent?

The density of alkali metals is in the order

Which one of the following properties of alkali metals increases in magnitude as the atomic number rises in the group-

Match List I with List II

LIST I Elements LIST II Colour imparted to the flame
A.\mathrm{K} I.Brick Red
B.\mathrm{Ca} II.Violet
C.\mathrm{Sr} III. Apple Green
D.\mathrm{Ba} IV, Crimson Red

Choose the correct answer from the options given below:

Alkali metal from the following with least melting point is:

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The main oxides formed on combustion of Li, Na, and K more than air are, respectively :

Lithium aluminium hydride can be prepared from the reaction of

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The compound which does not exist is

Concepts Covered - 0

s-block(Alkali Metals)

S-Block Elements - The s-block elements of the Periodic Table are those in which the last electron enters the outermost s-orbital. As the s-orbital can accommodate only two electrons, two groups (1 & 2) belong to the s-block of the Periodic Table.

Alkali Metals : Group 1 of the Periodic Table consists of the elements: lithium, sodium, potassium, rubidium, caesium and francium. They are collectively known as the alkali metals. These are so called because they form hydroxides on reaction with water which are strongly alkaline in nature. lithium , sodium , potassium , rubidium, caesium and francium except hydrogen are all alkali metals.

Alkaline Earth Metals : The elements of Group 2 include beryllium, magnesium, calcium, strontium, barium and radium. These elements with the exception of beryllium are commonly known as the alkaline earth metals. These are so called because their oxides and hydroxides are alkaline in nature and these metal oxides are found in the earth’s crust.

Physical Properties of Alkali Metals - 1

Physical Properties of Alkali Metals :

  •  All the alkali metals are silvery white, soft and light metals.
  • Because of the large size, these elements have low density which increases down the group from Li to Cs. However, potassium is lighter than sodium.
  • The melting and boiling points of the alkali metals are low indicating weak metallic bonding due to the presence of only a single valence electron in them.
  • The alkali metals and their salts impart characteristic colour to an oxidizing flame. This is because the heat from the flame excites the outermost orbital electron to a higher energy level. When the excited electron comes back to the ground state, there is emission of radiation in the visible region of the spectrum as given below:
  • The other physical properties of Alkali metals are:
Physical Properties of Alkali Metals - 2

Physical properties of Alkali Metals- 2 :

Melting and Boiling Point

  • The melting and boiling points of these metals are quite low.
  • Melting point and Boiling point decreases down the group.
  • This is because the metallic bonding becomes weak as we move down the group.
  • The weak metallic bonding can be attributed to involvement of a single electron in the bonding.

Oxidation state

  • All the alkali metals show an oxidation state of +1
  • This is because upon loss of one electron, these attain stable noble gas configuration.
  • All the alkali metal ions are diamagnetic in nature with no unpaired electons
  • Alkali metals, however are paramagnetic in nature due to the presence of an unpaired electron.
Chemical Properties of Alkali Metals - 1

Chemical Properties of Alkali Metals : The alkali metals are highly reactive due to their large size and low ionization enthalpy. The reactivity of these metals increases down the group.

  • Reactivity towards air: The alkali metals tarnish in dry air due to the formation of their oxides which in turn react with
    moisture to form hydroxides. They burn vigorously in oxygen forming oxides.
  • Reactivity towards water: The alkali metals react with water to form hydroxide and dihydrogen.
    2M + 2H_{2}O\rightarrow 2M^{+}+2OH^{-}+H_{2}
  • Reactivity towards dihydrogen: The alkali metals react with dihydrogen at about 673K (lithium at 1073K) to form hydrides. All the alkali metal hydrides are ionic solids with high melting points.
  • Reactivity towards halogens : The alkali metals readily react vigorously with halogens to form ionic halides, M+X- .
    However, lithium halides are somewhat covalent.
  • Reducing nature: The alkali metals are strong reducing agents, lithium being the most and sodium the least powerful
Chemical Properties of Alkali Metals - 2

Chemical Properties of Alkali Metals - 2 :

Carbonates and Bicarbonates

  • The carbonates of the alkali metals are stable to heating except \mathrm{Li_2CO_3}
  •  dissociates upon heating to form its oxide and liberates \mathrm{CO_2} gas

\mathrm{Li_2CO_3 \overset{\Delta}{\longrightarrow} Li_2O + CO_2}

  • Thermal stability of the alkali metal carbonates increase down the group. This is because of Lattice energy effects in which larger anions are more stabilised by larger cations and vice versa.
  • The bicarbonates of the alkali metals are also quite stable and exist in the solid state except Lithium bicarbonate
  • The bicarbonates (except Li) however dissociate upon heating to give the respective  carbonate and release 

\mathrm{2MHCO_3 \overset{\Delta}{\longrightarrow} M_2CO_3 + CO_2 + H_2O}

  • Lithium bicarbonate does not exist in the solid state and is unstable.

Solutions of Alkali Metals in Liquid Ammonia

  • The alkali metals dissolve in liquid ammonia giving deep blue solutions which are conducting in nature.
  • These solutions are also reducing in nature
  • The blue colour of the solution is due to the ammoniated electron which absorbs energy in the visible region of light and thus imparts blue colour to the solution.
  • These solutions are paramagnetic
  • Upon increasing the concentration, the electrons start to pair up and the paramagnetism decreases
  • The colour of the solution also changes to Bronze upon increasing the concentration.

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