Question

incorrect
your answer is incorrect.

• row 1: your answer is incorrect.

some patterns of electron - configuration are listed below. in each case, g stands for a noble - gas core and n, m, or o stand for integer numbers like 1, 2, 3 and so on. note: assume g is lighter than rn.
think about the chemical elements made of atoms with an electron - configuration that matches each pattern. in what block or blocks of the periodic table would these elements lie? would they be metals, nonmetals, metalloids, some of each? use your answers to these questions to complete the table.
electron configuration of atoms\tlocation of elements (check all that apply)
\tblocks\tmetals or nonmetals?
gns²md¹⁰np²\ts □ p □ d □ f\tmetals □ nonmetals □ metalloids □
gns²\ts □ p □ d □ f\tmetals □ nonmetals □ metalloids □
gns²md¹⁰np⁵\ts □ p □ d □ f\tmetals □ nonmetals □ metalloids □

Explanation:

Step1: Recall periodic - table block rules

Elements with the out - most electrons in the p - orbital belong to the p - block. For the electron configuration \([G]ns^{2}md^{10}np^{2}\), the last electrons are in the p - orbital, so it's in the p - block. Elements like Si and Ge with this general configuration are metalloids.

Step2: Analyze \([G]ns^{2}\)

Elements with the electron configuration \([G]ns^{2}\) (excluding He) are in the s - block. These are mainly metals (e.g., Mg, Ca).

Step3: Analyze \([G]ns^{2}md^{10}np^{5}\)

Elements with the electron configuration \([G]ns^{2}md^{10}np^{5}\) are in the p - block. Halogens have this configuration and are non - metals.

Answer:

electron configuration of atoms	location of elements (check all that apply)
\([G]ns^{2}md^{10}np^{2}\)	p	metalloids
\([G]ns^{2}\)	s	metals
\([G]ns^{2}md^{10}np^{5}\)	p	nonmetals