Questions 1-15: Orbital Basics and Quantum Numbers

An orbital is best defined as:

• The circular path of an electron around the nucleus

• A region of space where there is a high probability of finding an electron

• The exact location of an electron

• The energy level of an electron

How many quantum numbers are needed to completely describe an electron in an atom?

• 2

• 3

• 4

• 5

The principal quantum number (n) describes:

• The shape of the orbital

• The orientation of the orbital in space

• The main energy level and size of the orbital

• The spin of the electron

What are the possible values for the principal quantum number (n)?

• 0, 1, 2, 3...

• 1, 2, 3, 4...

• -1, 0, +1

• Any integer

The angular momentum quantum number (l) describes:

• The energy level

• The shape of the orbital

• The spin of the electron

• The size of the orbital

For a given value of n, the possible values of l range from:

• 0 to n

• 1 to n

• 0 to (n-1)

• -n to +n

If n = 3, what are the possible values of l?

• 0, 1, 2

• 1, 2, 3

• 0, 1, 2, 3

• -3 to +3

The magnetic quantum number (m_l) describes:

• The energy of the orbital

• The shape of the orbital

• The orientation of the orbital in space

• The spin of the electron

For a given value of l, the possible values of m_l range from:

• 0 to l

• 1 to l

• -l to +l

• 0 to (l-1)

The spin quantum number (m_s) can have values of:

• 0 or 1

• -1 or +1

• -1/2 or +1/2

• Any integer