0 1 2 4 Question 2 Imagine a molecule formed from two Helium atoms that has lost

Question

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Question 2

Imagine a molecule formed from two Helium atoms that has lost 2 e-. Its formula will be He22+. Which of the following is most likely to be correct? (Use the diagram in Model 1 and Table 2 to help you determine an answer)  

He22+will have a bond energy similar to that of He2

He22+ will have a bond length similar to that of Li2

He22+ will have a bond energy similar to that of H2

He22+ is unlikely to form

Question 3

The activity works through the molecular orbital description of bonding for both F2 and O2. How many electrons would O2 need to lose to have the same bond order as F2?

none, they are already the same

1 electron

2 electrons

4 electrons

Question 5

According to Molecular Orbital Theory, a molecule will form if all the electrons in the molecule are at lower energy than they are in the individual atoms.

True

False

Question 6

According to Molecular Orbital Theory, e- are relatively less stable in antibonding orbitals than in bonding orbitals because e- can't occupy the space between the two nuclei in an antibonding orbitals

True

False

Question 7

According to Molecular Orbital Theory, a molecule will be more stable (meaning, its bond will be stronger) if there are more electrons in bonding orbitals and relatively few electrons in antibonding orbitals.

True

False

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Explanation / Answer

Multiple choice

Q1. Electrons in valence shell orbital in a H2 molecule

2

1 e- each from H combines to form H2 and thus have 2e-'s

Q2. When He2^2+ is formed.

The correct statement about this would be,

He2^2+ will have a bond energy similar to H2

Both have 2 e-'s to fill which goes in bonding M.O.

Q3. The number of electrons to loose from O2 to have same bond order as F2 would be,

4 electrons

F2 has bond order of 1. loosing 4 electrons from O2 M.O. would give a bond order of 1 as well.

Q5. According to molecular orbital Theory, a moleculae would be formed If all the electrons in it occupy lower energy than that in individual atoms,

True

Q6. According to Molecular Orbital Theory, e- are relatively less stable in antibonding orbitals than in bonding orbitals because e- can't occupy the space between the two nuclei in an antibonding orbitals

True

Q7. According to Molecular Orbital Theory, a molecule will be more stable (meaning, its bond will be stronger) if there are more electrons in bonding orbitals and relatively few electrons in antibonding orbitals.

True

This raises bond order and so bonds between two atoms forming the molecule.

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