How would the bond lengths vary in dicarbon species `C_2`, `C_2^-`, `C_2^(2-)`?

The correct order of increasing bond lengths of the following bonds is C-H , C-O , C-C , C=C

Which of the following species has the shortest bond length? N_2^(+) , N_2 , N_2^(-) , N_2^(2-)

How does bond energy vary from N_2^+ and N_2^- . Why?

The molecule in which the distance between the neighbouring carbon atoms is least is:C_6 H_6 C_2 H_2 C_2 H_4 C_2 H_6

In 1, 3-butadiene the single bond length between C_2 and C_3 is

Draw diagrams showing the formation of a double bond and a triple bond between carbon atoms in (a) 'C_2 H_4' (b). 'C_2 H_2' molecules.

The electronegativities of carbon and chlorine are 2.5 and 3.00 respectively. Calculate the C-Cl bond length if C-C and Cl-Cl bond distances are 1.54 A^(@) and 1.0 A^(@)

Indicate the sigma and pi bonds in the following molecules C_6H_6 , C_6H_12 , CH_2Cl_2 , CH_2 = C = CH_2

The number and type of bonds in C_2^(2-) ion in CaC_2 are: