Use the bond energies to answer the question.

Question

H–H = 432
H–O = 467
O–O = 146
O=O = 495
H2 (H–H) combines with O2 (O=O) to become hydrogen peroxide (H2O2) bonded as such: H–O–O–H. Which option shows the difference in total bond energy between the reactants and the products?
1,0801
−153
153
−927

Water (H2O) has two O–H bonds. The electronegativity of oxygen is 3.5, whereas hydrogen is 2.1. Which statement best describes the type of bond this molecule has and how the electrons behave?(1 point)
O–H bonds are nonpolar covalent, and oxygen pulls the shared electrons toward it.
O–H bonds are polar covalent, and hydrogen pulls the shared electrons toward it.
O–H bonds are nonpolar covalent, and hydrogen pulls the shared electrons toward it.
O–H bonds are polar covalent, and oxygen pulls the shared electrons toward it.

Answer 1

H2 + O2 ==> H2O2
H-H bond broken = 432
O=O bond broken = 495
Total bonds broken = ?
O-H formed x 2 = 467 x 2 = ?
O-O formed = 146
Total bonds formed = ?
dH = Bond Energy bonds broken - Bond Energy bonds formed = ?
If dH is - it is exothermic; if + it is endothermic

#2 question.
If electronegativity (EN) for O is 3.5 vs H EN is 2.1, that means O has a stroger pull for electrons than H. The difference in EN is 3.5-2.1 = 1.4 which makes it a polar covalent bond. So O-H is a polar covalent bond with the electrons drawn closer to O than H. Looks like d to me.
Post your work if you get stuck.