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Standard XII

Chemistry

Atomic Size and Electronegativity

Calculate the...

Question

Calculate the electronegativity of carbon from the following data:
Bond energy of H-H bond $E_{H - H} = 104.2 k c a l m o l^{- 1}$
Bond energy of C-C bond $E_{C - C} = 83.1 k c a l m o l^{- 1}$
Bond energy of C-H bond $E_{C - H} = 98.8 k c a l m o l^{- l}$
Electronegativity of Hydrogen $X_{H} = 2.1.$

3.75

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-3.75

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2.59

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-2.59

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Solution

The correct option is C 2.59
Let the electronegativity of carbon be $X_{C}$ . Applying Pauling equation, we get:
$X_{C} - X_{H} = 0.208 [E_{C - H} - (E_{C - C} \times E_{H - H})^{0.5}]^{0.5}$
In this equation, bond energies are taken in $k c a l m o l^{- 1}$
$X_{C} - 2.1 = 0.208 [98.8 - (83.1 \times 104.2)^{0.5}]^{0.5}$
$X_{C}$ = 2.59

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Similar questions

Q. Calculate the electronegativity of fluorine from the following data:
Bond energy of H-H bond

E_{H - H} = 104.2 k c a l m o l^{- 1}

Bond energy of F-F bond

E_{F - F} = 36.6 k c a l m o l^{- 1}

Bond energy of H-F bond

E_{H - F} = 134.6 k c a l m o l^{- l}

Electronegativity of Hydrogen

X_{H} = 2.1.

Q. Calculate the electronegativity of fluorine from the following data:
Bond energy of H-H bond

E_{H - H} = 104.2 k c a l m o l^{- 1}

Bond energy of F-F bond

E_{F - F} = 36.6 k c a l m o l^{- 1}

Bond energy of H-F bond

E_{H - F} = 134.6 k c a l m o l^{- l}

Electronegativity of Hydrogen

X_{H} = 2.1.

Q. From the following data:

E_{H - H} = 104.2 k c a l m o l^{- 1}

;

E_{C - C} = 83.1 k c a l m o l^{- 1}

;

E_{C - H} = 98.8 k c a l m o l^{- 1}

.
The electronegativity of carbon is

128.5 x \times 10^{- 2}

. Then, the value of

x

is: (up to nearest integer)

H | C | H = H | C | H + H - H \to H - H | C | H - H | C | H - H

From the following bond energies:

H - H

bond energy :

431.37 k J m o l^{- 1}

C = C

bond energy :

606.10 k J m o l^{- 1}

C - C

bond energy :

336.49 k J m o l^{- 1}

C - H

bond energy :

410.50 k J m o l^{- 1}

Enthalpy for the reactions, will be?

Q. Find the enthalpy of formation of Hydrogen flouride on the basis of following data :
Bond energy of

H - H = 434 k J m o l^{- 1}

Bond energy of

F - F = 158 k J m o l^{- 1}

Bond energy of

H - F = 565 k J m o l^{- 1}

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Atomic Size and Electronegativity

Standard XII Chemistry

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Calculate the electronegativity of carbon from the following data: Bond energy of H-H bond EH−H=104.2 kcal mol−1 Bond energy of C-C bond EC−C=83.1 kcal mol−1 Bond energy of C-H bond EC−H=98.8 kcal mol−l Electronegativity of Hydrogen XH=2.1.

The correct option is C 2.59Let the electronegativity of carbon be XC. Applying Pauling equation, we get: XC−XH=0.208[EC−H −(EC−C ×EH−H)0.5]0.5 In this equation, bond energies are taken in kcal mol−1 XC−2.1=0.208[98.8 −(83.1 ×104.2)0.5]0.5 XC = 2.59