Bonding in Carbon - The Covalent Bond

Why are most carbon compounds poor conductors of electricity?

Which one of the following structures correctly depicts the compound ${\mathrm{CaCl}}_2$?

List two differences between the properties exhibited by covalent compounds and ionic compounds.

Draw the electron dot structure for ethyne.

Consider the following organic compounds:

$\left(\mathrm{i}\right) \mathrm{H}—\underset{\stackrel{|}{\mathrm{H}}}{\overset{\underset{|}{\mathrm{H}}}{\mathrm{C}}}—\underset{\stackrel{|}{\mathrm{H}}}{\overset{\underset{|}{\mathrm{H}}}{\mathrm{C}}}—\stackrel{\underset{|}{\mathrm{H}}}{\mathrm{C}}=\mathrm{O} \left(\mathrm{ii}\right) \mathrm{H}—\underset{\stackrel{|}{\mathrm{H}}}{\overset{\underset{|}{\mathrm{H}}}{\mathrm{C}}}—\stackrel{\underset{|}{\mathrm{H}}}{\mathrm{C}}=\mathrm{O}$

State the relationship between these compounds and draw the structure of any other compound having similar functional group.

Consider the following organic compounds:

$\left(\mathrm{i}\right) \mathrm{H}—\underset{\stackrel{|}{\mathrm{H}}}{\overset{\underset{|}{\mathrm{H}}}{\mathrm{C}}}—\underset{\stackrel{|}{\mathrm{H}}}{\overset{\underset{|}{\mathrm{H}}}{\mathrm{C}}}—\stackrel{\underset{|}{\mathrm{H}}}{\mathrm{C}}=\mathrm{O} \left(\mathrm{ii}\right) \mathrm{H}—\underset{\stackrel{|}{\mathrm{H}}}{\overset{\underset{|}{\mathrm{H}}}{\mathrm{C}}}—\stackrel{\underset{|}{\mathrm{H}}}{\mathrm{C}}=\mathrm{O}$

Write the general formula for the compounds of this functional group.

Consider the following organic compounds:

$\left(\mathrm{i}\right) \mathrm{H}—\underset{\stackrel{|}{\mathrm{H}}}{\overset{\underset{|}{\mathrm{H}}}{\mathrm{C}}}—\underset{\stackrel{|}{\mathrm{H}}}{\overset{\underset{|}{\mathrm{H}}}{\mathrm{C}}}—\stackrel{\underset{|}{\mathrm{H}}}{\mathrm{C}}=\mathrm{O} \left(\mathrm{ii}\right) \mathrm{H}—\underset{\stackrel{|}{\mathrm{H}}}{\overset{\underset{|}{\mathrm{H}}}{\mathrm{C}}}—\stackrel{\underset{|}{\mathrm{H}}}{\mathrm{C}}=\mathrm{O}$

Name the functional group present in their compounds.

Write the number of single bonds present in the saturated compound with four carbon atoms.

Write the name and draw the structure of a saturated hydrocarbon with four carbon atoms.

Carbon can neither form ${\mathrm{C}}^{4-}$ nor ${\mathrm{C}}^{4+}$ ions. Why?

It is observed that covalent compounds are bad conductors of electricity. Give reason.

State the reasons, why carbon cannot gain four electrons to form ${\mathrm{C}}^{4-}$ anion. How does carbon overcome this problem to form compounds?

State the reasons, why carbon cannot lose four electrons to from ${\mathrm{C}}^{4+}$ cation.

"Two different forms of carbon-diamond and graphite have different structures and very different physical properties even though their chemical properties are same." Explain why.

 "Carbon prefers to share its valence electrons with other atoms of carbon or with atoms of other elements rather than gaining or losing the valence electrons in order to attain noble gas configuration." Give reasons to justify this​ statement.

Consider the carbon compounds having following molecular formula: $\left(\mathrm{i}\right){\mathrm{C}}_3{\mathrm{H}}_6, \left(\mathrm{ii}\right) {\mathrm{C}}_3{\mathrm{H}}_8, \left(\mathrm{iii}\right) {\mathrm{C}}_4{\mathrm{H}}_6, \left(\mathrm{iv}\right) {\mathrm{C}}_6{\mathrm{H}}_6, \left(\mathrm{v}\right) {\mathrm{C}}_6{\mathrm{H}}_{12}$.

State the number of double covalent bonds present in ${\mathrm{C}}_3{\mathrm{H}}_6$.

Show the covalent bond formation in nitrogen molecule.

Differentiate between saturated and unsaturated carbon compounds on the basis of their general formula.