Chapter 3: – Chemical Bonding
B.sc 1st year Book (Page 3)
Lattice energy
There are two forces that are operating on ionic crystals.
(a) The electrostatic force of attraction between cations and anions. and
(b) Interatomic repulsive forces acting between nuclei of these two ions. The variation of potential energy (P.E.) of oppositely charged ions varies with their internuclear distance of separation (r0) as shown in figure 3.01.
(a) The electrostatic force of attraction between cations and anions. and
(b) Interatomic repulsive forces acting between nuclei of these two ions. The variation of potential energy (P.E.) of oppositely charged ions varies with their internuclear distance of separation (r0) as shown in figure 3.01.
where r0 is the equilibrium distance between two ions when P.E. has a minimum value. If we assume that an infinite distance separates the ions then the value of P.E. is zero and this value is equal to the lattice energy (U) of an ionic crystal. Thus, the lattice energy of an ionic crystal M+X−is defined as “the energy released when a certain number of cations and anions are brought together from an infinite distance to form one gram mole of the ionic crystal or solid.”.
M^{+}_{(g)} +X^{}_{(g)} → M^{+}X^{}_{(s)} + U(lattice energy)
It is also defined as “the energy required to remove ions of one gram mole of a solid ionic crystal from their equilibrium position in a crystal to an infinite distance”.
M^{+}X^{}_{(s)} + (Energy supplied) → M^{+}_{(g)} +X^{}_{(g)}
Here the value of U is the same but has the opposite sign.
Related Topic  Chemical Bonding 
Theoretical calculation of lattice energy :
The lattice energy can be calculated theoretically on the basis of the Coulombic force of attraction between the ions forming an ionic crystal i.e. attractive forces acting between the ions of opposite charges and repulsive forces acting between them resulting from inter
penetration of the outermost electron cloud. When both the opposite ions approach together, the attractive force acting between them is directly proportional to the product of the charges carried by the ions and inversely proportional to the distance ‘r‘ of their separation. Thus, attractive potential energy may be expressed as:
where b= Repulsion coefficient or proportionality constant or Born coefficient.
n= Born exponent, Z+ and Z−are the number of charges on Mn+ and Xn− ions respectively. e= charge on an electron (4.8×10−10 e.s.u. )
The value of ‘ n ‘ for a given ion depends on its configuration for ions as shown below:
n= Born exponent, Z+ and Z−are the number of charges on Mn+ and Xn− ions respectively. e= charge on an electron (4.8×10−10 e.s.u. )
The value of ‘ n ‘ for a given ion depends on its configuration for ions as shown below:
Table 3.1: Born exponent for different isoelectronic ions :

Ion

Electron

Electronic configuration

'n' value

Li^{+}, Be^{2+}

2

1s^{2} (Hetype)

5

Na^{+}, Mg^{2+}, O^{2+}, O^{2}, F^{}

10

1s^{2}2s^{2}2p^{6} (Netype)

7

K^{+}, Ca^{2+}, S^{2}, Cl^{}

18

1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}

9

Rb^{+}, Sr^{2+}, Br^{}

36

[Ar]3s^{2}3p^{6}3d^{10}4s^{2}4p^{6} (Krtype)

10

Cs^{+}, Ba^{2+}, I^{}

54

[Kr]4s^{2}4p^{6}4d^{10}5s^{2}5p^{6 } (Xetype)

12

Equation (iii) is known as the Bom equation. It will be seen that the repulsive force, increases more rapidly than the attractive force in equation (iii) with a decrease in the distance r.
Equation (iii) is mainly used to calculate the energy released if a cation and anion which are separated by an infinite distance in a gaseous state are brought together in a crystal at a distance ‘ r ‘ from each other.
Application of Bom equation :
Let us consider the application of the Born equation to a NaCl crystal. In NaCl crystal, there is not one Na+ and one Cl but a large number of these ions arranged together according to a certain specific geometry. Therefore, it is necessary to consider (P.E.) attraction and (P.E.)repulsion between all of them. Since, in the crystal lattice of NaCl, each Na+ is surrounded by
(i) 6Cl ions at a distance r
(ii) 12 other Na^{+} ions at a distance √2r
(iii) 8 more Cl^{1} Ions at a distance √3r
(iv) 6 more Na^{+} ions at a distance √4r
(v) 24 more Cl^{–} ions at a distance √5r
(vi) 24 more Na^{+} ions at a distance √6r and so on.
Therefore, the potential energy due to the first term in the Bom equation is obtained by adding up the effect of all the interactions as follows :
For NaCl crystal Z^{+}= Z¯= 1. The quantity in the bracket which is the sum of infinite series is called the Madelung constant. For NaCl structure, its value is 1.747558. If this constant value is represented by ‘A then the equation (iv) is expressed as :
Now the second term of Born equation may be expressed as:
where B = 6b x e^{2} for NaCl type crystal. Thus,
Crystal Structure

Example

Coordination
number of ions

Madelung constant

Sodium Chloride

NaCl

Na+ = 6 : Cl = 6

1.7475

Cesium Chloride

CsCl

Cs+ = 8 : Cl = 8

1.7627

Zinc Blende

ZnS

Zn^{2+ }= 4 : S2 = 4

1.6381

Wurtzite

ZnS

Zn^{2+ }= 4 : S2 = 4

1.6410

Fluorite

CaF2

Ca2+ = 8 : F^{} = 4

5.0388

Rutile

TiO_{2}

Ti^{4+} = 6 : O^{2} =3

4.8160

Cadmium iodide

Cdl2

Cd^{2+} = 6 : I^{}  3

4.8160

When attractive and repulsive forces are equally balanced at a state of stable equilibrium position, the term ‘B’ may be eliminated. At this stage, the potential energy of the Ion is minimum and
This equation is called the BomLande equation.
Since n is always greater than unity henceU0has the value in a negative sign.
Conclusions are drawn from the BornLande equation :
Since n is always greater than unity henceU0has the value in a negative sign.
Conclusions are drawn from the BornLande equation :
From equation (xi) we may derive the following conclusions :
(i) The higher the charge on cation and anion, the greater would be the value of lattice energy (U0). In other words, greater would be the stability of the crystal. Example :
(i) The higher the charge on cation and anion, the greater would be the value of lattice energy (U0). In other words, greater would be the stability of the crystal. Example :
(ii) The lattice energy is inversely proportional to the interionic distance r0 between the oppositely charged ions in an ionic crystal. I.e. smaller the interionic distance r0, the greater would be the magnitude of lattice energy U0 or the greater would be the stability of the crystal. Example :
(iii) The higher the value of Madelung constant ‘ A ‘ the greater would be lattice energy, U0.
(iv) The higher the value of Bomexponent ‘ n ‘ greater would be the value of lattice energy.
(iv) The higher the value of Bomexponent ‘ n ‘ greater would be the value of lattice energy.
Application of Lattice energy :
1 Lattice energy may help to explain the solubility of ionic salts in suitable solvents. When ionic compounds dissolve in the solvent, solvation of their ions takes place, If water is the solvent, the process is called hydration of the Ions. This ionic solvation is an exothermic process releasing a considerable amount of energy, which is utilized to rupture crystal lattice. The liquids which cause more ease of solvation of ions are good solvents for ionic solids and have a high dielectric constant. The less solubility of Li, Be, Mg, Ca, etc with polyvalent anions such as, etc. in water is due to their high values of lattice energy. Thus, we can say, the greater the value of lattice energy of ionic crystals, the less would be their solubility in water. It is because when these compounds are dissolved in water less amount of energy is released which is insufficient to break their crystal lattice.
2 Lattice energy is involved in the calculation of electron affinities, the heat of formation, proton affinities, etc.
3 It helps to explain the stabilities of the compounds like hydrides, oxides, carbonates, etc.
4 It involves the derivation of crystal field stabilization energies of transition metal complexes.
4 It involves the derivation of crystal field stabilization energies of transition metal complexes.