When metallic atoms combine with nonmetallic atoms in ionic bonding, how do the metallic atoms generally behave in terms of electrons and ion formation?

Introduction / Context:
Ionic bonding is a central concept in basic chemistry. It usually occurs between metals and nonmetals, where electrons are transferred rather than shared. Metals tend to lose electrons, and nonmetals tend to gain electrons. This electron transfer leads to the formation of oppositely charged ions that attract each other. This question asks what metallic atoms typically do when they combine with nonmetallic atoms in such reactions.

Given Data / Assumptions:
- We are considering reactions between metals and nonmetals, such as sodium with chlorine. - Metallic atoms are located on the left side of the periodic table. - Nonmetallic atoms are located on the right side of the periodic table. - Ionic bonding involves whole electron transfer from metal to nonmetal.

Concept / Approach:
Metals have relatively low ionisation energy and often have only one, two, or three valence electrons. It is easier for them to lose these electrons and achieve a noble gas configuration. When a metal atom loses one or more electrons, it becomes a positively charged ion called a cation. Nonmetals, by contrast, have higher electronegativity and tend to gain electrons to fill their valence shell, becoming negatively charged anions. In ionic compounds such as NaCl or CaCl2, the metal provides cations and the nonmetal provides anions.

Step-by-Step Solution:
Step 1: Recall that metals, such as sodium and magnesium, are typically found on the left side of the periodic table and have just a few valence electrons. Step 2: It is energetically favourable for these metals to lose their valence electrons to reach a stable noble gas configuration. Step 3: When a metal atom loses electrons, it now has more protons than electrons, resulting in a net positive charge and forming a cation. Step 4: Nonmetals like chlorine or oxygen gain the electrons released by metals and form negatively charged anions. Step 5: The electrostatic attraction between positively charged cations and negatively charged anions forms an ionic bond and produces an ionic compound. Step 6: Therefore, the correct description is that metallic atoms lose electrons and form positively charged cations.

Verification / Alternative check:
Consider the example of sodium chloride. Sodium (Na) has one valence electron and loses it to form Na plus, a cation. Chlorine (Cl) gains this electron to form Cl minus, an anion. The resulting Na plus and Cl minus ions combine to form NaCl. Similar patterns are seen in magnesium oxide, aluminium oxide, and many other ionic compounds. These examples consistently show that metallic atoms lose electrons and form cations when reacting with nonmetals.

Why Other Options Are Wrong:
Option B states that metals gain electrons and form anions, which describes nonmetal behaviour rather than metal behaviour. Option C combines losing electrons with forming anions, which is contradictory, because losing electrons leads to a positive charge, not a negative one. Option D suggests that metals gain electrons yet somehow form cations, which again conflicts with the rule that gaining electrons leads to negative charge.

Common Pitfalls:
Students sometimes confuse metals with nonmetals when memorising trends. Another common mistake is to think that gaining electrons always happens because atoms want to fill their shells, without considering that metals can reach stability more easily by losing electrons. To avoid confusion, remember a simple rule: metals lose electrons and become positive, while nonmetals gain electrons and become negative in typical ionic bonding situations.

Final Answer:
The correct answer is: They lose electrons and form positively charged cations.