valence bond theory

21 Questions

What is the term used to describe the distance at which two hydrogen atoms achieve the lowest overall energy of the system?

Optimum distance

What is the energy difference between the two separated hydrogen atoms and the H2 molecule at the bond distance of 74 pm?

7.24 × 10^-19 J

What term is used to describe the amount of energy released when a bond is formed?

Bond energy

What does it take to break one H-H bond?

7.24 × 10^-19 J

What is the bond length observed for the H2 molecule?

74 pm

What is the first C-H bond energy in CH4?

439.3 kJ/mol

Which element combination has a bond length of 141.2 pm and an energy of 159 kJ/mol?

F-F

What quantity of energy is required to break one mole of H-H bonds?

$4.36 \times 10^5 J$

Which bond requires the highest energy to break per mole according to Table 8.1?

C≡N

What is the bond length for an H-Cl bond?

141.4 pm

How much energy is required to break the first C-H bond in a common paint thinner molecule?

$375.5 kJ/mol$

At what distance do the two hydrogen atoms achieve the lowest overall energy of the system?

$74 pm$

Which bond has a length of 150.6 pm and an energy of 347 kJ/mol?

C-C

What is the energy difference between the energy minimum and the energy of two separated atoms at the bond distance of 74 pm for the H2 molecule?

$7.24 \times 10^{-19} J$

Which bond has a length of 160.9 pm?

H-I

What is the energy required to break the first C=O bond?

$745 kJ/mol$

What is the energy required to break one mole of H-H bonds?

4.36 \times 10^5 J

What is the bond energy difference between breaking the first C-H bond in CH4 and in H-CH2C6H5?

63.8 kJ/mol

What is the bond length of the C≡C bond?

120.8 pm

How much energy is required to break the Cl-Cl bond per mole?

243 kJ/mol

What is the energy difference between the energy minimum and the energy of two separated hydrogen atoms at the bond distance of 74 pm for the H2 molecule?

7.24 \times 10^{-19} J

Learn about the formation of π bonds through side-by-side overlap of p orbitals. Explore the regions of orbital overlap and nodes in a π bond.

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