Question

Compared to the atoms of nonmetals in period 3, the atoms of metals in period 3 have
1. fewer valence electrons
2. more valence electrons
3. fewer electron shells
4. more electron shells

Answer 1

Answer : Option A) Fewer valence electrons

Explanation : Compared to the atoms of non metals in period 3, atoms of metals in period 3 have fewer valence electrons.

There are 8 elemental members in third period which are eight: sodium, magnesium, aluminium, silicon, phosphorus, sulfur, chlorine, and argon.

The first 2 elements belong to s-block whereas the other elements belong to p-block. The atomic radius is found to decrease across the period.

The electrons in the valence shell increases as we go from left to right in the period, which means when we move from metal to non-metal side the number of valence electrons also increases. This clearly shows that metals have fewer valence electrons as compared to the non-metals.

Answer 2

Compared to the atoms of nonmetals in period 3, the atoms of metals in period 3 have fewer valence electrons.

Option 1 is correct.

In the periodic table, the period runs from left to right on the table while the group runs from top to bottom on the table.

In period 3, the period starts with Sodium Na(alkali metal), Magnesium Mg(alkaline earth metals), Aluminium Al(other non metals), Silicon Si (non metals), Phosphorus (non-metals), Sulfur (non-metals). etc.

From left to right across period 3, the valence electrons in the outermost increase.

Hence, the metals will have fewer valence electrons since the metals start period 3.

Therefore, we can conclude that compared to the atoms of nonmetals in period 3, the atoms of metals in period 3 have fewer valence electrons.

Learn more about the periodic table here:

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