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Covalent Bond

The most stab...

Question

The most stable form of carbon at high temperature is $X$ . The $C - C$ bond length in diamond is $Y$ while $C - C$ bond length in graphite is $Z$ .
What are $X, Y$ and $Z$ respectively?

Graphite,

1.42 ˚ A, 1.54 ˚ A

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Coke,

1.54 ˚ A, 1.84 ˚ A

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Diamond,

1.54 ˚ A, 1.42 ˚ A

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Fullerene,

1.54 ˚ A, 1.54 ˚ A

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Solution

The correct option is C Diamond, $1.54 ˚ A, 1.42 ˚ A$
The standard enthalpy of formation of the diamond ( Hof = 2.425 kJ/mol) is slightly larger than the enthalpy of formation of graphite, which is the most stable form of carbon at $25^{0} C$ and 1 atm pressure. Thus, at a very high temperature and pressure, diamond becomes more stable than graphite.
Thus X is diamond.

The C-C bond length in diamond is $1.54 ˚ A$ while the graphite has a simple planar structure. The nearest neighbour carbon atoms are separated by $1.42 ˚ A$ .

Answer:- (C) Diamond, $1.54 ˚ A, 1.42 ˚ A$

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Similar questions

(1.49 A^{\circ})

(1.54 A^{\circ})

\circ A

1.54 \circ A

The c-c bond length in propene is little shorter $(1.49 \circ A)$ then the c-c bond length $(1.54 \circ A)$ is ethane. This is due to

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˚ A

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C - C

1.54 ˚ A

109.5

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On catalytic hydrogenation ethylene gives ethane. During this reaction

hybridization of carbon atoms changes from SP² to SP³

bond angle decreases from 120 to 109.5

C-C Bond length increases from 1.34 A° to 1.54 A°

all of these

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