Question

Discussing this chapter, a classmate says, "An element that commonly forms a cation is a metal." Do you agree or disagree? Explain your answer.

Short answer

I agree with the statement "An element that commonly forms a cation is a metal." This is because metals have a tendency to lose their valence electrons due to their electron configuration, which results in the formation of positive ions or cations. For example, sodium (Na) loses one electron to form a sodium cation (Na+), and magnesium (Mg) loses two electrons to form a magnesium cation (Mg2+). Therefore, it is true that metals commonly form cations.

Step-by-step solution

Understanding cations

A cation is a positively charged ion that has lost one or more electrons. This process is called ionization. Elements can form cations by losing electrons, which increases their overall positive charge.

Understanding metals

Metals are elements that have some characteristic properties such as being shiny, malleable, ductile, and good conductors of heat and electricity. In general, metals have one to three electrons in their outermost energy levels (valence electrons). These electrons have a relatively weak attachment to their nucleus, which makes it easier for metals to lose electrons and form cations.

Determining if metals commonly form cations

Metals, due to their properties and electron configuration, have a tendency to lose their valence electrons, which results in the formation of positive ions or cations. For example, sodium (Na) loses one electron to form a sodium cation (Na+), and magnesium (Mg) loses two electrons to form a magnesium cation (Mg2+). Therefore, it is true that an element that commonly forms a cation is a metal.

Conclusion

We agree with the statement "An element that commonly forms a cation is a metal," as metals tend to lose their valence electrons due to their electron configuration, forming cations in the process.

Key concepts

Metals

Metals are fascinating elements with distinct properties that make them unique. They are known for their shiny appearance and are typically malleable and ductile, which means they can be shaped or stretched into wires without breaking.
Metals are excellent conductors of heat and electricity, which is why they are commonly used in many electrical applications.
Additionally, metals are generally found on the left side and towards the center of the periodic table.
Due to their structure, metals have a tendency to lose electrons easily, primarily to achieve a stable electron configuration. This property makes them more likely to form cations, which are positively charged ions usually created when a metal atom loses one or more electrons.

Electron Configuration

Electron configuration is a way to describe how electrons are distributed around an atom's nucleus. Each atom has distinct energy levels that can hold a certain number of electrons.
The electrons closest to the nucleus occupy the lowest energy levels, while those further away reside in higher energy levels.
For metals, the electrons in their outermost energy level, or shell, are called valence electrons.
These valence electrons are key players in chemical reactions because they are the most loosely bound to the nucleus.
When metals lose their valence electrons, they achieve a more stable electron configuration, often resembling the nearest noble gas, which has a full outer shell.
This stability is a driving factor behind the formation of cations.

Ionization

Ionization is a process where an atom loses or gains electrons, resulting in the formation of ions.
For metals, ionization involves losing electrons to form cations. In a typical ionization process, especially for metals, energy called ionization energy is needed to remove electrons from the atom.
The tendency of metals to lose electrons during ionization is largely because their valence electrons are held less tightly due to the larger atomic radius and the shielding effect from inner electrons.
Therefore, metals have relatively low ionization energies, making it easier for them to lose valence electrons, leading to cation formation.

Valence Electrons

Valence electrons are the outermost electrons of an atom and play a critical role in chemical bonding and reactions.
In metals, these valence electrons are usually one to three in number and are less tightly bound to the nucleus.

• This weak hold allows the electrons to be easily removed during reactions.
• The loss of valence electrons helps the atom achieve a stable electron configuration.

This vulnerability is what enables metals to readily form cations.
When a metal atom loses valence electrons, it often achieves the electron configuration of the nearest noble gas, stabilizing the ion through energy minimization.