S Block Elements Class 11

Elements in which valence or outermost electron enters in the S–orbital are called S – block elements. The S – block elements are placed to the left hand side of long form of the periodic table. S – Orbital can accommodate a maximum of two electrons. The S–block contains two groups (vertical columns) in periodic table, namely group–1 and group-2. Elements of group -1 are called alkali metals and those of group -2 are called alkaline earth metals.

OCCURRENCE OF S BLOCK ELEMENTS

S – Block elements do not occur in nature in free state. Among the alkali metals sodium and potassium are abundant and lithium, rubidium and cesium have lower abundance. Among the alkaline earth metals magnesium and calcium are abundant in the earth crust. Radium is rarest of all.

GROUP – 1 ELEMENTS : ALKALI METALS

The general electronic configuration of group – 1 element is ns¹. All alkali metals have one valance electron hence form monovalent M⁺ ions, and are highly reactive. Group – 1 consists of following elements.

Hydrogen (H), Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), Cesium (S) and Francium (Fr).

The electronic configuration of group – 1 elements is as follows –

Elements	Symbol	Atomic Number	Electronic configuration in condensed form
Hydrogen	H	1	1s¹
Lithium	Li	3	[He] 2s¹
Sodium	Na	11	[Ne] 3s¹
Potassium	K	19	[Ar] 4s¹
Rubidium	Rb	37	[Kr] 5s¹
Cesium	Cs	55	[Xe] 6s¹
Francium	Fr	87	[Rn] 7s¹

ANOMALOUS PROPERTIES OF LITHIUM

Amongst alkali metals, lithium has smallest size and highest polarizing power (charge / radius ratio) due to this reason lithium behaves different from other elements of group-1 (alkali metals). It shows following anomalous properties.

· Lithium is hard metal, its melting point and boiling point are highest among the group.

· Lithium is least reactive among all alkali metals and it is the strongest reducing agent.

· Lithium hydride is the stable amongst all the alkali metal hydrides.

· LiOH is weak base while hydroxides of other alkali metals behave as strong bases.

· Lithium nitrate when heated gives lithium monoxide(Li₂O). While other alkali metal nitrates decompose to give corresponding nitrites.

· Lithium combines with ammonia to form lithium amide (Li₂NH) while other alkali metals form amides of the general formula MNH₂ (where M = Na, K, Rb, Cs).

DIAGONAL RELATIONSHIP OF LITHIUM WITH MAGNESIUM

The element lithium of second row shows similar properties with its diagonally opposite member magnesium of third row. This is known as diagonal relationship. The diagonal relationship is due to the similarity in ionic sizes and polarizing power (i.e. charge/radius ratio) of lithium and magnesium. Also electronegativity of Li (1.00) and Mg (1.20) are not much different.

s block elements class 11 chemistry notes

PERIODIC TRENDS OF ALKALI METALS

1. Atomic and ionic radius of S Block Elements

Alkali metals have the largest atomic and ionic radius in their respective periods. On moving down the group, the size goes on increasing due to the presence of extra shells hence the atomic and ionic radius also increases.

2. Ionization enthalpy or energy of S Block Elements

Ionization enthalpies of alkali metals are low and decrease down the group from Li to Cs. This is due to increase in atomic number, size, nuclear charge and increase in screening effect.

3. Electronegativity of S Block Elements

The electronegativity of the alkali metals is very low due to their electropositive character. The electronegativity decreases from Li to Cs as the electropositive character increases.

4. Melting and boiling point of S Block Elements

Alkali metals have very low melting and boiling points due to presence of weak intermetallic bonds. It decreases on moving down the group.

5. Oxidation States of S Block Elements

Due to the presence of only one electron in the valence shell, they exhibit only +1 oxidation state or oxidation number.

S BLOCK ELEMENTS CHEMICAL REACTIVITY

The alkali metals are highly reactive due to their large size and low ionization enthalpy.

1. Reactions of S-block elements with oxygen (air)

Alkali metals burns vigorously in oxygen to form oxides. Lithium forms monoxide (Li₂O) and sodium forms peroxide, (Na₂O₂).

4Li + O₂ → 2Li₂O (Oxide)

2Na + O₂ → Na₂O₂ (Peroxide)

The other elements form super-oxides.

M + O₂ → MO₂ (Superoxide)

(where, M = K, Rb, Cs)

2. Reaction of S-block elements with water

The alkali metals react with water to form corresponding hydroxides and evolve hydrogen gas (Dihydrogen). (M = Li, Na, K, Rb, Cs)

2M + 2H₂O → 2MOH + H₂ ↑

3. Reaction of S-block elements with hydrogen (Dihydrogen)

The alkali metals react with dry hydrogen at high temperature (673K) to form corresponding hydrides.

2M + H₂ → 2MH

4. S-block elements Reaction with halogens

All the alkali metals react vigorously with halogen to form their respective ionic crystalline halides with general formula M⁺X^- where M = Na, K, Rb, Cs and X = Cl, Br, I and F.

2M + X₂ ^Δ→ 2M⁺X^-

SOME IMPORTANT COMPOUNDS OF SODIUM

1] Sodium carbonate (washing soda, Na₂CO₃)

Sodium carbonate is usually prepared by a process known as the ammonia–soda process or Solvay process. Raw materials are NaCl, NH₃ and limestone (for CO₂).

The process involves the following steps

Step – I

CO₂ gas bubbled through a solution of NH₃ to form NH₄HCO₃ i.e. ammonium hydrogen carbonate.

NH₃ + H₂O + CO₂ → NH₄HCO₃

Step – II

Sodium hydrogen carbonate (NaHCO₃) precipitates out because of the common ion effect caused due to the presence of excess NaCl.

NH₄HCO₃ + NaCl → NaHCO₃ + NH₄Cl

Step III

The precipitate NaHCO₃ is then filtered of and ignited to get sodium carbonate (Na₂CO₃)

2NaHCO₃ ^Δ→ Na₂CO₃ + CO₂ + H₂O

Properties of Na₂CO₃

Sodium carbonate crystallizes from water as a decahydrate (sodium carbonate decahydrate, Na₂CO₃.10H₂O, also known as washing soda).Above 373K, the monohydrate from becomes completely anhydrous and change to a white powder called soda ash.

Na₂CO₃.H₂O ^{above 373K}→ Na₂CO₃ + H₂O

(Anhydrous)

Uses of Na₂CO₃

i. It is used in the manufacture of glass soap, borax and caustic soda.

ii. It is used in water softening in laundry and cleaning.

iii. It is used in paper, paints and textile industries.

2] Sodium hydroxide (caustic soda, NaOH)

Commercially sodium hydroxide is prepared by the electrolysis of sodium chloride in Costner – Kellner cell. It is also prepared by adding calcium hydroxide to the solution of sodium carbonate.

Na₂CO₃ + Ca(OH)₂ → 2NaOH + CaCO₃ ↑

Properties of NaOH

Sodium hydroxide is a deliquescent, white crystalline solid. It is readily soluble in water and forms a strong alkaline solution.

The solution of sodium hydroxide at the surface reacts with CO₂ in the atmosphere to form Na₂CO₃.

2NaOH + CO₂ ↔ Na₂CO₃ + H₂O

Uses of NaOH

i. It is useful in purification of bauxite and to manufacture of soap, paper, artificial silk and a number of chemicals.

ii. It is useful in petroleum refining and textile industries.

iii. It is important as laboratory reagent and in preparation of pure fats and oils.

3] Sodium Chloride (NaCl)

It is also known as common salt or table salt. It is mainly obtained by the evaporation of sea water. Crude sodium chloride thus obtained contains CaSO₄, CaCl₂, MgCl₂ as impurities and is deliquescent. Pure NaCl is obtained by passing HCl gas through saturated solution of crude NaCl. Due to common ion effect NaCl gets precipitated.

Properties of Sodium Chloride (NaCl)

It is white crystalline solid. It has melting point 1081K and boiling point 1713K. It has solubility of 36gram per 100gram of water at 273K. NaCl when heated with concentrated H₂SO₄ and MnO₂ it liberates chlorine gas.

2NaCl + MnO₂ + 2H₂SO₄ → MnSO₄ + Na₂SO₄ + 2H₂O + Cl₂ ↑

Uses of Sodium Chloride (NaCl)

i. It is used as a common salt or table salt for domestic purpose and preservative for meat, fish etc.

ii. It is used for the preparation of Na₂O₂, NaOH, Na₂CO₃ etc.

4] Sodium hydrogen carbonate (NaHCO₃)

It is also known as sodium bicarbonate and baking soda. It is made by saturating a solution of sodium carbonate with CO₂.

Na₂CO₃ + H₂O + CO₂ → 2NaHCO₃

Properties Sodium hydrogen carbonate (NaHCO₃)

It is white crystalline solid, sparingly soluble in water. On heating, it gives Na₂CO₃ and CO₂.

2NaHCO₃ ^373K→ Na₂CO₃ + CO₂ + H₂O

It’s aqueous solution is alkaline due to hydrolysis.

NaHCO₃ + H₂O → NaOH + H₂CO₃

Uses Sodium hydrogen carbonate (NaHCO₃)

i. It is used in fire extinguisher and for baking of cakes breads etc.

ii. It is also used as medicine to minimize the acidity of stomach i.e. antacid.

BIOLOGICAL IMPORTANCE OF SODIUM AND POTASSIUM

Sodium and potassium are very important and play a vital role in biological system. Our bodies obtain them from fruits and vegetable. Common salt is the most important source of sodium in the diet. Their ions maintain the sensitivity of nerves and control muscles.

Deficiency of sodium shows reduction in fat deposit, atrophy, lung infection retarted bone growth, reduces blood pressure etc. Deficiency of potassium reduces heart beats. Hypertrophy of kidneys and paralysis of muscle.

GROUP – 2 ELEMENTS : ALKALINE EARTH METALS

The general electronic configuration of group–2 elements is ns². All alkaline earth metals have two valance electrons, hence form divalent M²⁺ ions, and are highly reactive like alkaline metals. Group – 2 consists of following elements.

Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), Barium (Ba), Radium (Ra).

The electronic configuration of group – 2 elements is an follows –

Elements	Symbol	Atomic Number	Electronic Configuration
Beryllium	Be	4	[He] 2s²
Magnesium	Mg	12	[Ne] 3s²
Calcium	Ca	20	[Ar] 4s²
Strontium	Sr	38	[Kr] 5s²
Barium	Ba	56	[Xe] 6s²
Radium	Ra	88	[Rn] 7s²

ANOMALOUS PROPERTIES OF BERYLLIUM

Beryllium, the first member of the group – 2 metals, shows anomalous properties as compared to magnesium and rest of the members of group-2. It is due to its small size and highest polarizing power. It shows following anomalous properties.

· Beryllium is hard metal while other alkaline earth metals are soft.

· The melting, boiling points and ionization enthalpy of Be are highest of all the alkaline earth metals.

· Be forms covalent compounds while other members form ionic compound.

· Be does not liberate H₂ from acids while other metals liberate H₂.

DIAGONAL RELATIONSHIP BETWEEN BERYLLIUM AND ALUMINIUM

The element beryllium is the first member of group – 2 which shows similar properties with its diagonals opposite element aluminum of group – 13. This diagonal relationship is due to similarity in ionic sizes and polarizing power.

PERIODIC TRENDS OF ALKALINE EARTH METALS

1. Atomic and ionic radius

The atomic and ionic radii of the alkaline earth elements are smaller than those of the corresponding alkaline metals of the same periods. The atomic and ionic radius increases down the group with increase in atomic number.

2. Ionization enthalpy or energy

Ionization enthalpies of alkaline earth metals are higher than those of alkali metals. Ionization enthalpy decreases down the group.

3. Electronegativity

The electronegativity of group–2 elements decreases down the group. Their electronegativity values are higher than those of alkali metals.

4. Melting and boiling point

The melting and boiling points are not regular in the group, mainly due to different crystal structure of the metals. However, these are higher than those of alkali metals.

5. Oxidation states

Due to the presence of only two electrons in the valence shell, they exhibit only +2 oxidation state.

CHEMICAL REACTIVITY

Due to low ionization enthalpy, alkaline earth metals are fairly reactive. However, their chemical reactivity is lower than those of alkali metals.

1. Reaction with oxygen

With pure oxygen, Be, Mg and Ca form oxides whereas Ba, Sr and Ra form peroxides.

2M + O₂ ^Δ→ 2MO (M = Be, Mg or Ca)

Metal oxide

M + O₂ ^Δ→ MO₂ (M = Ba, Sr or Ra)

Metal peroxide

The affinity of metals towards oxygen increases down the group.

2. Reaction with water

Alkaline earth metals react with water to form metal hydroxides and evolve hydrogen gas. The chemical reactivity with water increases from Mg to Ba.

M + 2H₂O → M(OH)₂ + H₂ ↑ (M = Mg, Ca, Sr or Ba)

3. Reaction with hydrogen

Except Be all the alkaline earth metals react with hydrogen on heating to form metal hydride of the general formula, MH₂.

M + H₂ ^Δ→ MH₂ (M = Mg, Ca, Sr or Ba)

4. Reaction with halogens

All the alkaline earth metals react with halogens at high temperature to form their halides.

M + X₂ → MX₂ (X = F, Cl, Br, I)

IMPORTANT COMPOUNDS OF CALCIUM

1] Calcium oxide or quick lime (CaO)

It is prepared commercially by heating limestone (CaCO₃) in a reverberatory kiln at 1070 to 1270K.

CaCO₃ ^Δ CaO + CO₂ ↑

Properties Calcium oxide or quick lime (CaO)

Calcium oxide is a white amorphous solid. It has a melting point of 2870K. When it is exposed to atmosphere, it absorbs moisture and carbon dioxide.

CaO + H₂O → Ca(OH)₂

CaO + CO₂ → CaCO₃

Uses Calcium oxide or quick lime (CaO)

i. It is used in the manufacture of sodium carbonate from caustic soda.

ii. It is an important primary material for large scale production of cement.

2] Calcium carbonate (CaCO₃)

Calcium carbonate occurs in nature in several forms like chalk, lime stone, marble state, calcite etc. It is prepared by passing carbon dioxide through slaked lime.

Ca(OH)₂ + CO₂ → CaCO₃ + H₂O

It can also be prepared by adding sodium carbonate to calcium chloride.

CaCl₂ + Na₂CO₃ → CaCO₃ + 2NaCl

Properties Calcium carbonate (CaCO₃)

It is white fluffy powder. It is almost insoluble in water. When CaCO₃ is heated to 1200K, it decomposes to evolve CO₂.

CaCO₃ ^1200K CaO + CO₂ ↑

It reacts with dilute acid to liberate carbon dioxide.

CaCO₃ + H₂SO₄ → CaSO₄ + H₂O + CO₂ ↑

Uses Calcium carbonate (CaCO₃)

i. It is used in the manufacture of quick lime and in building material in the form of marble.

ii. It is used as antacid, mild abrasive of tooth paste, constituent of chewing gum.

3] Calcium hydroxide or slaked lime (Ca(OH)₂)

It is prepared by adding water to quick lime.

CaO + 2H₂O → Ca(OH)₂ + H₂ ↑

It is also prepared by treating calcium chloride with caustic soda.

CaCl₂ + 2NaOH → Ca(OH)₂ + 2NaCl

Properties Calcium carbonate (CaCO₃)

It is white amorphous powder, sparingly soluble in water and the aqueous solution is called lime water. When CO₂ is passed through lime water, it turns milky

Ca(OH)₂ + CO₂ → CaCO₃ + H₂O

Milky

The milkiness disappears on passing CO₂ gas in excess.

CaCO₃ + CO₂ + H₂O → Ca(HCO₃)₂

Soluble milkiness disappears

Uses Calcium carbonate (CaCO₃)

i. It is used to prepare mortar which is an important building material.

ii. It is used glass and tanning industry also to prepare bleaching powder and for purification of sugar.

Hope you enjoy learning s block elements in periodic table. You can also learn with other chemistry notes chapter on other elements in periodic table from given below topics-

P – Block Elements (Chapter 1)

p Block Elements (Chapter 2)

d and f Block Elements

Elements of First Transition Series

S Block Elements Class 11