Which one of the following sets of quantum numbers is not possible? What is the

Question

Which one of the following sets of quantum numbers is not possible? What is the maximum number of electrons in an atom that can have the following set of quantum numbers? n = 4 l = 3 m_ = -2 m_ = +1/2 A) 0 B) 1 C) 2 D) 6 E) 10 Electrons in an orbital with l = 3 are in a/an A) d orbital. B) f orbital. C) g orbital. D) p orbital. E) s orbital. The number of orbitals in a d subshell is A) 1 B) 2 C)3 D) 5 E) 7 "No two electrons in an atom can have the same four quantum numbers" is a statement of A) the Pauli exclusion principle. B) Bohr's equation. C) Hund's rule. D) de Broglie's relation. E) Dalton's atomic theory. The orbital diagram for a ground-state nitrogen atom is Which ground-state atom has an electron configuration described by the following orbital diagram? A) phosphorus B) nitrogen C) arsenic D) vanadium E) none of these How many unpaired electrons does a ground-state atom of sulfur have? A) 0 B) 1 C) 2 D) 3 E) 4 Which element has the following ground-state electron configuration? [Kr]5s^1 4d^5 A) Mn B) Mo C) Nb D) Re E) Tc The electron configuration of a ground-state copper atom is A) [Ar]4s^2 4d^4 B) [Ar]4s^2 4p^6 3d^3 C) [Ar] 4s^2 3d^9 D) [Ar] 3d^9 E) [Ar]4s^1 3d^10

Explanation / Answer

18.

For option A, n = 4, so l can have values from 0 to (n-1) that is 0,1,2,3 and given value of l is 3 which is correct. As l = 3, ml can have values (-l to +l) -3,-2,-1,0,+1,+2,+3. The given value of ml is -2 which is within the range. ms is +1/2 which is also correct. Hence, this set of quantum numbers is possible.

For option B, n = 3, so l can be 0. But ml can not be 1, hence the given set of quantum numbers is not possible.

For option C, n = 3, so l can have a value of 0. ml is also 0 which is correct. ms has the value of +1/2 which is also correct. Hence, this set of quantum numbers is possible.

For option D, n = 2, so l can have values 0,1. And as l = 1, ml can have values -1,0,+1. Hence, given set of values is possible.

For option E, n = 2, so l can have a value of 0 and hence ml will be 0. Thus, this set of quantum numbers is possible.

Hence, the answer is B.

19.

With n = 4 and l = 3, it is a 4f subshell. Also, ml = -2, it represents an orbital in 4f subshell which can have two electrons. Of the two electrons, only one can have ms=+1/2 .

Hence, the answer is B).

20.

l = 3 refers to the f orbital. Hence, the answer is B).

21.

The d subshell has 5 orbitals. Hence, the answer is D).

22.

Pauli exclusion principle states that, ' No two electrons in an atom can have the same four quantum numbers '.

Hence, the answer is A).

23.

According to Hund's rule, nitrogen (atomic number 7) fills 1s and 2s subshells and has one electron in each of the three 2p orbitals. These three electrons have unpaired spins.

Hence, the answer is A.

24.

[Ne] represents the 1s22s22p6 electron configuration of neon(atomic number 10). There are two paired electrons in 3s and three unpaired electrons in 3p orbitals. That represents the atom with atomic number 15 that is phosphorus.

Hence, the correct option is A).

25.

The third shell of sulfur has 6 electrons, 3s23px23py13pz1. So there are 2 unpaired electrons in 3py and 3pz. Hence, the correct option is C).

26.

Krypton has atomic number 36. The given electron configuration gives atomic number 42. So the element is molybdenum (Mo).

Hence, the correct option is B).

27.

For copper, atomic number is 29.

So, the electronic configuration is: 1s22s22p63s23p64s13d10

Argon has electron configuration : 1s22s22p63s23p6

hence, ground state electron configuration of copper is: [Ar]4s13d10

The correct option is E).

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