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Soloha48 [4]
3 years ago
12

An element with the electron configuration: [noble gas] ns2 (n - 1)d10 np3 has how many_____________ valence electrons.

Chemistry
1 answer:
Marina86 [1]3 years ago
5 0

Answer:

The correct option is e. 5

Explanation:

An element with the electron configuration [noble gas] ns² (n - 1)d¹⁰ np³ belongs to the nitrogen group element - group 15 - in a period higher than 2. The element could be As, Sb or Bi. For example, arsenic (As) has the electron configuration [Ne] 4s² 3d¹⁰ 4p³.

The valence electrons are those in the highest energy level, in a s or p sublevel. For the elements with the general electron configuration [noble gas] ns² (n - 1)d¹⁰ np³ has 5 valence electrons: 2 electrons in a s sublevel and 3 electrons in a p sublevel. The electrons in the d orbital are in a lowest energy level (n-1).

Therefore, the correct option is e. 5.

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