Answer:
The correct option is A) 3, 2, -2, -1/2.
Explanation:
Quantum numbers represent different properties regarding the level, sublevel and orbital in which an electron is. There are 4 quantum numbers:
- Principal quantum number (<em>n</em>): indicates the level of energy and gives information about the size of an orbital. It can only take positive and integer values, e. g., 1, 2, 3...
- Angular quantum number (<em>l</em>): indicates the sublevel of energy and provides information about the shape of the orbital. Some common shapes are spherical (<em>l</em>=0) and polar(<em>l</em>=1). Shapes for bigger l are more complicated. <em>l</em> values depend on <em>n</em> values. <em>l</em> values can be integers up to (<em>n</em>-1). For example. if <em>n</em> = 2, <em>l</em> can take the values 0 and 1.
- Magnetic quantum number (<em>m</em>): it gives information about the orientation in space of an orbital. It may take any integer value between -l and +l. For example, if <em>l</em> = 1, <em>m</em> can take values -1, 0 and 1, each one referring to an orbital p along a different axis in the space (x, y and z axes).
- Spin quantum number (<em>ms</em>): it refers to the spin angular momentum of an electron and it can take 2 values: -1/2 or +1/2.
A) 3, 2, -2, -1/2 is correct because it follows every rule.
B) 3, 3,-4, 1/2 is wrong because if <em>n</em>=3, <em>l</em> can only be up to 2, and l from -3 to +3.
C) 3,2,0,0 is wrong because <em>ms</em> cannot take the value 0.
D) 3,3,3, -1/2 is wrong because if <em>n</em>=3, <em>l</em> can only be up to 2.
E) 3, 4, 6, -1/2 is wrong because if <em>n</em>=3, <em>l</em> can only be up to 2, and <em>l</em> from -3 to +3.
