Quantum Theory of the Atom

What is the range of integral values for the magnetic quantum number (ml)?

How many orbitals are present in the p subshell?

What is the value of the electron spin quantum number (ms) for an electron spinning in one direction?

How many integral values does the magnetic quantum number (ml) take for l=2?

What distinguishes the three p orbitals from each other?

Which of the following accurately represents the number of orbitals in an f subshell?

What is the total number of orbitals available when l=1?

What defines the energy and shape differences among various types of subshells?

What does the principal quantum number (n) determine about an orbital?

How is the angular momentum quantum number (l) related to the principal quantum number (n)?

What is the maximum value of the angular momentum quantum number (l) for n=4?

Which quantum number specifies the magnetic property of an electron's spin?

What does the energy of an orbital primarily depend on?

What term describes the three-dimensional region where an electron is most likely to be found?

If an electron is in a 5d orbital, what is the value of n and l?

In which scenario does the energy of an orbital increase for a given principal quantum number n?

Quantum Theory of the Atom

Each electron in an atom is described by four quantum numbers.
Three of these quantum numbers (n, l, and ml) describe the electron's wave function, determining the probability of finding the electron in various locations.
The fourth quantum number (ms) describes the electron's spin.

Quantum Numbers

Principal Quantum Number (n):
- Integral values (1, 2, 3...).
- Higher n values indicate higher energy levels.
- Higher n values also correspond to orbitals further from the nucleus.
Angular Momentum Quantum Number (l):
- Integral values from 0 to n-1.
- Related to the shape of atomic orbitals.
- Values of l are often represented by letters: 0=s, 1=p, 2=d, 3=f, 4=g.
Magnetic Quantum Number (ml):
- Integral values between -l and +l, including zero.
- Indicates the orientation of the orbital in space.
- For a given l, there are 2l+1 possible ml values.
Electron Spin Quantum Number (ms):
- Can be +1/2 or -1/2.
- Represents the intrinsic angular momentum (spin) of the electron.

Atomic Orbitals

A wave function for an electron in an atom is called an atomic orbital.
Each subshells contains one or more orbitals - s = 1 orbital, p = 3 orbitals, d = 5 orbitals, f= 7 orbitals
Each orbital type has a different shape and energy.
An orbital can hold 2 electrons.

Examples of quantum numbers

2p has n=2, l=1.
3d has n=3, l=2.
4f has n=4, l=3.

Orbital Shapes

Examples of s, p & d orbitals shapes are presented.
Note that p orbitals have different spatial orientations, while d orbitals have a broader range of shapes.

This quiz covers the quantum theory of the atom, specifically focusing on the four quantum numbers that describe electrons. It explores the principal, angular momentum, magnetic, and spin quantum numbers and their significance in determining an electron's behavior and properties. Test your understanding of these foundational concepts in quantum mechanics.