Lattice Energy Class 11 CBSE Chemistry Chapter 4 - Future Study Point

Lattice Energy Class 11 CBSE Chemistry Chapter 4

Lattice energy class 11 cheistry chapter 4

Lattice Energy Class 11 CBSE Chemistry Chapter 4

Lattice Energy: The energy required to build a molecule of an ionic compound from a metallic gaseous ion and a non-metallic gaseous ion. The highly energetic ions (or as it were in a gaseous state) of metal and non-metallic gaseous ions release energy in the formation of ionic compounds. The lattice energy is defined as the energy released by the gaseous cation and gaseous anion in the formation of 1 mole of an ionic compound through the process of exothermic, the same energy is added to the ionic compound to release the gaseous cation and gaseous anion, this energy is known as lattice energy.

Lattice energy class 11 cheistry chapter 4

Lattice Energy Class 11 CBSE Chemistry Chapter 4

Note: Lattice means three-dimensional solids like sodium chloride, potassium chloride etc.

Evaluation of lattice energy: The way of computing lactic energy we don’t have a direct method, we can calculate lattice energy by the Born Haber Cycle.

Born Haber Cycle: The formation of ionic compounds involves the release of several types of heat like sublimation energy, ionization energy, bond dissociation energy, and electron affinity energy through which the lattice energy of ionic compounds is calculated known as the Born Haber Cycle.

The heat of Formation: The amount of heat is released when 1 mole of the compound is formed from its constituent elements in a pure and stable state.

As an example, the pure and stable state of sodium is solid Na and pure and stable state of chlorine is  gaseous Cl2

When Na interacts with Cl2, NaCl is formed with the release of heat which is the heat of formation ΔH

Na + (1/2)Cl→ NaCl +ΔH

The amount of heat released in the formation of a 1-mole compound from its elements in a pure and stabilized state is known as the heat of formation. It is noted down that lattice energy is the energy released in building an ionic compound when a gaseous cation combines with a gaseous anion.

The relationship between the heat of formation and lattice energy:

Na + (1/2)Cl→ NaCl +ΔH

For the transformation of Na to gaseous Na we need to give Na sublimation energy,(S.E), now gaseous Na can be ionized to Na, for this we need to add ionization energy(I.E) to gaseous  Na.

Since Cl2 is already in a gaseous state but in Clthere is a bond between two chlorine atoms so we need to give it the bond dissociation energy(D.E) , there is 1/2  of a molecule of chlorine so we are needed to impart 1/2 of  D.E. Now when chlrine is ionized to Clafter receiving an electron, in this process, the energy released is electron affinity(E.A) which is negative energy rest all other types of energy are positives because those are absorbed.

Therefore net energy is sublimation energy(+) +Ionization energy(+) +1/2 of  D.E – E.A(-)  -Latice Eergy=ΔH

Note: The first electronic affinity energy is negative but when the second electron is accepted by the anion then electronic affinity energy will be negative.

The sign of lattice energy is negative because this energy is released during the reaction of  Na(gaseous)and  Cl– (gaseous)

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