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Which of the following outer electron configurations would you expect to belong to a reactive metal?
a. ns2
b. ns2 np6
c. ns2 np5
d. ns2 np2

Respuesta :

joseaaronlara

Answer:

The answer to your question is: a

Explanation:

Electron configurations are:

ns is for alkali metals and alkali earth metal

nd is for transition metals

nf is for Inner transition metals

np is for nonmetals

np⁶ is for noble gases

a. ns2  This is the electron configuration of an alkali earth metal

b. ns2 np6  This is the electron configuration of a noble gas

c. ns2 np5  This is the electron configuration of nonmetals

d. ns2 np2 This is the electron configuration of nonmetals

pstnonsonjoku

The outer electron configurations expected for a reactive metal is ns2.

The most reactive metals are metals of group 1 and 2 in the periodic table. This is shown by their very negative values of reduction potential.

The general outer electron configuration of group 2 elements is ns2.

ns2 np6 is the outer electronic configuration of the noble gases, ns2 np5 is the outer electronic configuration of the halogens. ns2 np2 is the outer electronic configuration of group 14 elements.

Therefore, the outer electron configurations expected for a reactive metal is ns2.

Learn more: https://brainly.com/question/14283892

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