Construct an energy level diagram showing all orbitals for the hydrogen atom up to n = 5, labeling each orbital with its appropriate quantum numbers. How many different orbitals are in each shell?

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Bryllant BaluyutLv10

28 Dec 2020

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Which of the following statements is true for energy level differences seen when comparing the s, p, d, and f orbitals in the hydrogen atom for a given value of n?

	a.There are different values of quantum number m l for each orbital which cause differences in energy.
	b.There are no differences in energy between the s,p,d, and f orbitals.
	c.There are different values of quantum number l for each orbital which cause differences in energy.
	d.There are different values of quantum number m s for each orbital which cause differences in energy.

(a) Using only the valence atomic orbitals of a hydrogen atom and a fluorine atom, and following the model of Figure 9.46, how many MOs would you expect for the HF molecule? (b) How many of the MOs from part (a) would be occupied by electrons? (c) It turns out that the difference in energies between the valence atomic orbitals of H and F are sufficiently different that we can neglect the interaction of the 1s orbital of hydrogen with the 2s orbital of fluorine. The 1s orbital of hydrogen will mix only with one 2p orbital of fluorine. Draw pictures showing the proper orientation of all three 2p orbitals on F interacting with a 1s orbital on H. Which of the 2p orbitals can actually make a bond with a 1s orbital, assuming that the atoms lie on the z-axis? (d) In the most accepted picture of HF, all the other atomic orbitals on fluorine move over at the same energy into the molecular orbital energy-level diagram for HF. These are called “nonbonding orbitals.” Sketch the energy-level diagram for HF using this information and calculate the bond order. (Nonbonding electrons do not contribute to bond order.) (e) Look at the Lewis structure for HF. Where are the nonbonding electrons?