Consider the following three atomic orbitals. They are drawn to scale and orbital a has n=2.

how many orbitals can have the following set of quantum numbers n = 3    l = 2   ml = -2 1, 2, 5, 7 or 10?

The following are possible energy values for the electron orbiting the nucleus in Bohr’s model for the hydrogen atom.    n = 1:    E1 = -21.79 x 10–19 J;        n = 2:    E2 = - 5.45 x 10–19 J;    n = 3:    E3 = - 2.42 x 10–19 J;    n = 4:    E4 = - 1.36 x 10–19 J; If an electron jumps from the orbit n = 4 to orbit n = 2, and a quantum of energy is emitted in the form of light, what is the wavelength of the emitted light in nm?             (A) 365 nm           (B) 486 nm           (C) 1095 nm           (D) 1460 nm

Give the orbital designations of electrons with the following quantum numbers. (Type your answer using the format 1s for 1s.) n = 4, l = 2, ml = -1

what are the 17 sets of quantum numbers that discribe the 17 electrons of chlorine?

Which quantum numbers are needed to define the subshell?

Use the graphs of the hydrogen 2s and 2p orbitals (probability density) to explain why the energy of the 2s orbital is lower even though it has a higher expectation value for the radius

What is the maximum number of orbitals that can be identified by the following set of quantum numbers?   1) If n=4, l=3, ml= 4 2) if n=2, l=2, ml= 0

How many orbitals have n = 3 and m? = -1?

6s, 5p, 3d, 4p Rank orbitals from smallest to largest energy