Answer: Which of the following statements are true? Select all that apply.
Select all that apply.
i. Electrons cannot occupy an antibonding orbital.
ii. Antibonding orbitals are higher in energy than bonding orbitals (if all orbitals are created from the same atomic orbitals).
iii.The probability is 100% for finding an electron at the nucleus in a π∗ orbital.
iv. s orbitals can make only σ or σ∗ molecular orbitals.
Answer :
I. True , Ii. True , iii. False iv. True
Explanation:
Here are few paragraphs explaining each claims above.
The Pauli exclusion principle dictates that no two electrons in an interacting system may have the same quantum state. If the bonding orbitals are filled, then any additional electrons will occupy antibonding orbitals.
Antibonding molecular orbitals are normally higher in energy than bonding molecular orbitals. Bonding and antibonding orbitals form when atoms combine into molecules. If two hydrogen atoms are initially far apart, they have identical atomic orbitals.
In general, an electron belonging to an atom somewhere in different where you are has a nonzero probability of being found right here where I am sitting — and likewise there is a nonzero probability of being found at the other end of the Andromeda galaxy. (Note that while they are nonzero, they average out to zero at quite a large number of significant digits.)
100 % cannot be used since that would put everything into an orbital and therefore the concept of an orbital would lose its usefulness.
In the s orbital there are two types of sigma orbitals formed, antibonding sigma orbitals (abbreviated σ∗), and bonding sigma orbitals (abbreviated σ). Notice that the σ∗ orbital is empty and has a higher energy than the σ orbital.
