Drawing Molecular Orbitals

Q: What are molecular orbitals?

A: Molecular orbitals describe the regions in an atom where electrons are most likely to be found. They have different shapes depending on their type — S, P, D, or F.

Q: What should you draw first when sketching molecular orbitals?

A: Always start by drawing a grid or axis to show orientation.

Q: What is the shape of an S orbital?

A: S orbitals are spherical (big circle) and are drawn at the center of the axis.
Examples: 1s, 2s, 3s.

Q: What is the shape of a P orbital?

A: P orbitals are shaped like dumbbells.

Q: How many types of P orbitals are there?

A: There are three — Px, Py, and Pz.

Q: What is the shape of a D orbital?

A: D orbitals have four oval shapes combined (a cloverleaf pattern).

Q: How many types of D orbitals are there?

A: There are five types of D orbitals.

Q: What is the shape of an F orbital?

A: F orbitals have six oval shapes (more complex structure).

Q: How many types of F orbitals exist?

A: There are seven types of F orbitals.

Q: What is atomic radius?

A: Atomic radius is half the distance between the nuclei of two adjacent atoms.

Q: What factors affect atomic radius?

A:

1) The atomic radius tends to increase with increasing “n” values, and decrease with decreasing “n”

2)Effective nuclear charge (Zeff) tends to increase as you

move across a period, which decreases the atomic radii. As you add electrons, the nucleus pulls them strongly towards it (since that means the protons also increased) making it smaller.

Q: What is ionization energy?

Ionization energy is the energy required to remove an electron from a ground-state atom.

📈 Trend Summary:

• ⬆ Up a group: Ionization energy increases

• ➡ Across a period (right): Ionization energy increases

Q: What is electron affinity?

A: The likelihood of an atom attracting an electron.

This results in a change in energy, when electrons are added to a neutral state📈 Trend Summary:

• ⬆ Up a group: Electron affinity increases (atoms attract electrons more strongly)

• ➡ Across a period (right): Electron affinity increases