Atomic Orbitals and Electron Spin

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Questions and Answers

Which quantum number defines the subshell of an electron?

Azimuthal (l) (correct)

Principal (n)

Magnetic (ml)

Spin-magnetic (ms)

In the context of quantum numbers, which value is NOT possible for the azimuthal quantum number (l)?

-1 (correct)

How is the spin state of an electron represented according to its spin-magnetic quantum number (ms)?

+1 for ↑; -1 for ↓

0 for both ↑ and ↓

1 for ↑; -1 for ↓

+½ for ↑; -½ for ↓ (correct)

As the principal quantum number (n) increases, what happens to the average distance of the electron from the nucleus?

It increases. Signup and view all the answers

Which of the following wavefunctions corresponds to the s-orbital?

l = 0 Signup and view all the answers

What does the magnetic quantum number (ml) indicate?

Orbital orientation within a subshell Signup and view all the answers

What is the highest possible value of the azimuthal quantum number (l) if n = 4?

3 Signup and view all the answers

In which of the following situations would two electrons have the same set of quantum numbers?

If they are in the same orbital Signup and view all the answers

Which statement is true regarding electron characteristics as defined by the Heisenberg uncertainty principle?

The position and momentum of an electron cannot be determined simultaneously. Signup and view all the answers

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

Natural numbers excluding 0 Signup and view all the answers

What is the maximum number of electrons that can occupy the d-orbitals in a sublevel?

10 Signup and view all the answers

Which statement accurately describes the magnetic quantum number (ml) for d-orbitals?

ml can take values from -2 to +2. Signup and view all the answers

Which orbital type is closest to the nucleus for a given energy level?

s-orbitals Signup and view all the answers

What are the possible values of the spin quantum number (ms) for a single electron?

+½ and -½ Signup and view all the answers

In which situation does an electron experience the highest electrostatic repulsion?

Between two electrons in the same orbital. Signup and view all the answers

Which quantum number indicates the shape of an atomic orbital?

Angular momentum quantum number (l) Signup and view all the answers

What is the shape of all s-orbitals?

Spherical Signup and view all the answers

How many rational numbers can the spin quantum number (ms) take?

Two values Signup and view all the answers

Why is the effective nuclear charge less than the actual nuclear charge?

Electrons shield each other from the nucleus. Signup and view all the answers

No two electrons in an atom can have the same set of four quantum numbers. What principle does this statement represent?

Pauli exclusion principle Signup and view all the answers

Study Notes

Orbitals and Bonding

Electrons exhibit wavelike properties, making their location uncertain.
Atomic orbitals represent the probability of finding an electron in a specific region of space.
Each atomic orbital is defined by three quantum numbers:
- Principal quantum number (n): identifies the shell, increasing with distance from the nucleus
- Azimuthal quantum number (l): identifies the subshell (s, p, d, f).
- Magnetic quantum number (ml): identifies specific orbitals within a subshell.

Electronic Spin

Electrons have two spin states, represented by ↑ (up) and ↓ (down).
Spin-magnetic quantum number (ms) distinguishes spin states:
- +½ for ↑ electrons
- –½ for ↓ electrons

Electronic Configurations and Quantum Numbers

Each electron in an atom is assigned a unique set of four quantum numbers (n, l, ml, ms).
n: corresponds to the shell number, generally matching the row of the periodic table.
l: determines the subshell type (s, p, d, f):
- 0 = s-orbital (1 orbital)
- 1 = p-orbitals (3 orbitals)
- 2 = d-orbitals (5 orbitals)
- 3 = f-orbitals (7 orbitals)
- Each orbital can hold up to two electrons with opposite spins (↑↓).

Orbital Energies

Electron repulsion influences orbital energy levels, causing d-orbitals to be higher in energy than s-orbitals of the next higher shell.
s-orbitals penetrate closer to the nucleus, experiencing a higher effective nuclear charge.
The effective nuclear charge is reduced by shielding from other electrons.

s-Orbitals

s-orbitals are spherical and exist in only one orientation per shell.
The boundary surface represents the 90% probability zone of finding the electron.
s-orbitals increase in size as the principle quantum number (n) increases: 1s < 2s < 3s.

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Description

Explore the fascinating world of atomic orbitals and electron spin in this quiz. Understand the significance of quantum numbers in defining electron configurations and their wavelike behaviors. Test your knowledge on the principles that govern atomic structure and bonding.