Place the species in order of increasing bond length and bond energy. (Use the appropriate <, =, or > symbol to separate substances in the list.)

CN^- CN CN^+

Use the figure attached to answer the following questions.
(a) Would the bonding molecular orbital in HF place greater electron density near the H or the F atom?
__H
__F
Both atoms would share electrons equally.
Why?
__The H atom is more electronegative.
__The F atom is more electronegative.
__Both atoms have equal electronegativity.
(b) Would the bonding molecular orbital have greater fluorine 2p character, greater hydrogen 1s character, or an equal contribution from both?
__greater fluorine 2p character
__greater hydrogen 1s character
__equal contribution from both
Why?
__The bonding MO is closer in energy to the 2p atomic orbital.
__The bonding MO is closer in energy to the 1s atomic orbital.
__The energy difference between the bonding MO and the 2p and 1s atomic orbitals is the same.
(c) Would the anti-bonding molecular orbital in HF place greater electron density near the H or the F atom?
__H
__F
__Both atoms would share electrons equally.
Would the anti-bonding molecular orbital have greater fluorine 2p character, greater hydrogen 1s character, or an equal contribution from both?
__greater fluorine 2p character
__greater hydrogen 1s character
__equal contribution from both
Why?
__The anti-bonding MO is closer in energy to the 2p atomic orbital.
__The anti-bonding MO is closer in energy to the 1s atomic orbital.
__The energy difference between the anti-bonding MO and the 2p and 1s atomic orbitals is the same.