Multiple Choice
What is the maximum number of electrons that can occupy a single p orbital?
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9. Quantum Mechanics
Quantum Numbers: Magnetic Quantum Number
Multiple Choice
Which of the following statements is false?
a) A set of d orbitals contains 5 orbitals.
b) A set of 4s orbitals would have more energy than a set of 3p orbitals.
c) The second shell of an atom possesses d orbitals.
d) A set of f orbitals contains 3 orbitals.
e) The first energy level contains only s orbitals.
A
a, b
B
b, d
C
c, d
D
d, e
E
b, e
Verified step by step guidance1
Step 1: Understand the concept of atomic orbitals and energy levels. Orbitals are regions in an atom where there is a high probability of finding electrons. Each energy level (or shell) can contain different types of orbitals: s, p, d, and f.
Step 2: Review the number of orbitals in each type. The s orbitals have 1 orbital, p orbitals have 3 orbitals, d orbitals have 5 orbitals, and f orbitals have 7 orbitals. This helps in evaluating statements about the number of orbitals.
Step 3: Analyze the energy levels and their corresponding orbitals. The first energy level (n=1) contains only s orbitals. The second energy level (n=2) contains s and p orbitals, but not d orbitals. The third energy level (n=3) can contain s, p, and d orbitals.
Step 4: Compare the energy of orbitals. Generally, within the same principal energy level, s orbitals are lower in energy than p orbitals, which are lower than d orbitals, and so on. However, when comparing different energy levels, a 4s orbital is typically lower in energy than a 3d orbital due to electron shielding and penetration effects.
Step 5: Evaluate each statement based on the above concepts. Statement a is true because d orbitals contain 5 orbitals. Statement b is false because 4s orbitals are lower in energy than 3p orbitals. Statement c is false because the second shell does not possess d orbitals. Statement d is false because f orbitals contain 7 orbitals, not 3. Statement e is true because the first energy level contains only s orbitals.
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