When ionic bonds are formed between metals and nonmetals, metallic atoms generally tend to do what with their outer shell electrons?

Introduction / Context:
Ionic bonding is one of the basic types of chemical bonding taught in school level chemistry. It typically occurs between metals and nonmetals. Metals tend to form positively charged ions, while nonmetals tend to form negatively charged ions. Understanding what happens to the valence electrons of a metallic atom during ionic bond formation is essential for predicting formulas of ionic compounds, such as NaCl or MgO, and for understanding electrical conductivity in molten salts.

Given Data / Assumptions:

• We are considering ionic bonds, not covalent or metallic bonds.
• The bonding is between metallic atoms and nonmetal atoms.
• Valence electrons are the outer shell electrons involved in bonding.
• Metals usually have low ionisation energies compared with nonmetals.

Concept / Approach:
Metals have relatively few electrons in their outermost shell and low ionisation energies, so they can easily lose these electrons to achieve a stable noble gas configuration. Nonmetals, on the other hand, have higher electronegativities and tend to gain electrons. In ionic bonding, electrons are transferred from metal atoms to nonmetal atoms. The metal becomes a positively charged cation, and the nonmetal becomes a negatively charged anion. The electrostatic attraction between these oppositely charged ions forms the ionic bond. The correct description of metallic atom behaviour is therefore that they lose electrons and form cations.

Step-by-Step Solution:
Step 1: Recall that metals, especially those in groups 1 and 2, have one or two electrons in their outermost shell and seek stability by losing these electrons. Step 2: When a metal atom loses one or more valence electrons, it becomes a positively charged ion, called a cation, because it now has more protons than electrons. Step 3: Nonmetals, which have higher electronegativities, accept these electrons and become negatively charged anions. Step 4: The electrostatic attraction between the positively charged metal cations and negatively charged nonmetal anions forms an ionic bond. Step 5: Therefore, the correct statement is that metallic atoms lose electrons to become positively charged cations when ionic bonds are formed.

Verification / Alternative check:
Examples support this description. Sodium, a group 1 metal, loses one electron to form Na⁺ in sodium chloride. Magnesium, a group 2 metal, loses two electrons to form Mg²⁺ in magnesium oxide. In each case, the metal cation pairs with a nonmetal anion such as Cl⁻ or O²⁻ to form an ionic crystal. This pattern is repeated in many ionic compounds like KBr, CaCl2 and Al2O3. In all these examples, metals clearly lose electrons and form positive ions, confirming the general rule.

Why Other Options Are Wrong:
Option A describes sharing electrons equally, which is characteristic of nonpolar covalent bonding, not ionic bonding. Option B suggests that metals gain electrons and become anions, which is opposite to their normal behaviour; nonmetals are the ones that gain electrons. Option D claims that metals neither gain nor lose electrons, which contradicts the fundamental definition of ionic bonding as involving electron transfer. Option E suggests that metallic atoms break apart into neutral atoms with no charge, which does not describe bonding at all. Only option C correctly states that metals lose electrons to become positively charged cations when ionic bonds form.

Common Pitfalls:
Students sometimes confuse ionic bonds with covalent bonds and mistakenly think that metals share electrons in the same way nonmetals do. Another pitfall is to mix up cations and anions, forgetting which is positive and which is negative. To remember, note that cation starts with the same letter as cat, which might be thought of as a positive pet, and anion contains the letter n as in negative. Also remember that metallic behaviour is characterised by electron loss, which explains why metals conduct electricity and form positive ions in electrolysis.

Final Answer:
When ionic bonds are formed, metallic atoms generally Lose electrons to become positively charged cations, which then attract nonmetal anions to form ionic compounds.