calculate how much energy in kilojoules is released or absorbed during the reaction of 1 mole of C2H4 Show the numbers added and subtracted?

Enthalpy change ....

During the reaction of C2H4 with what? The reaction to make ethylene from carbon and hydrogen? Your question seems to imply that the enthalpy change should be computed from bond energies. If that is the case, everything must be in the gaseous state, including carbon. Therefore, you will also need the enthalpy of atomization of carbon, that is, the energy needed to take carbon from a solid to a gas. That is +716 kJ/mol.

2C(g) + 2H2(g) --> C2H4(g)

ΔH = ΣBE ..... BE for breaking a bond is positive, and negative for bond making

ΔH = 2(C(s)->C(g)) + 2(H-H) + C=C + 4(C-H)

ΔH = 2(+716 kJ) + 2(+436 kJ) + (-614 kJ) + 4(-414 kJ)

ΔH = +34 kJ

The reaction is endothermic since ΔH is positive.