Question

An ion with one less electron than it has protons has a charge.

Short answer

The given ion has one less electron than it has protons, which means it has lost one electron. This results in a net positive charge of \(+1\), making it a cation.

Step-by-step solution

Understanding atomic structure

An atom consists of three main particles: protons, neutrons, and electrons. Protons and neutrons are located in the nucleus at the center of the atom, and electrons are found in orbitals surrounding the nucleus. Protons have a positive charge (+1), electrons have a negative charge (-1), and neutrons have no charge (0).

Understanding ions

Ions are formed when atoms lose or gain electrons. When an atom loses an electron, it has more protons than electrons, resulting in a net positive charge and the formation of a positive ion (also known as a cation). When an atom gains an electron, it will have more electrons than protons, resulting in a net negative charge and the formation of a negative ion (also known as an anion).

Identifying the given ion's electron loss

The given ion has one less electron than it has protons. In other words, it has lost one electron. This means that the ion has one more proton than electron, giving it a net positive charge.

Calculating the charge of the ion

To calculate the charge of the ion, we need to find the difference between the number of protons and the number of electrons. Since there is one more proton than electron, the charge will be +1. Because the ion has a net positive charge, it is a cation. So, the charge of the ion is \(+1\).

Key concepts

Atomic Structure

Every atom is like a mini universe containing three primary particles: protons, neutrons, and electrons. It’s important to understand where these particles are located and what kind of charge they hold. Picture the atom's protons and neutrons as a cluster in the center, forming the nucleus. This is the dense core of the atom. The protons in the nucleus carry a positive charge, each contributing a charge of +1. Neutrons are neutral, meaning they have no charge. Electrons are the free spirits of the atomic world. They move around the nucleus in regions called orbitals and carry a negative charge of -1 each. This balance of charges is crucial because it determines the atom's overall charge. Understanding how these components interact is the first step to comprehending ionic changes.

Cations

A cation is a positive ion, created when an atom loses electrons. Similarly, you can think of cations as atoms that have 'donated' one or more electrons. When this loss happens, the atom’s balance of protons and electrons is disturbed. For instance, losing one electron means the atom will have one extra proton compared to electrons, resulting in a net charge of +1. This imbalance causes the atom to become a positive ion or cation. The process of losing electrons is vital because it allows atoms to form ionic bonds with other atoms or ions, which helps to stabilize their electronic structure. The tendency to form cations is common in metals, which can easily loose electrons in chemical reactions.

Electrical Charge

Electrical charge is a fundamental property of particles, determining how they interact with each other. In atoms, protons and electrons are responsible for this property. The charge is usually neutral when an atom has equal numbers of protons and electrons, cancelling each other out. However, when there’s a mismatch, the atom becomes an ion.

• Positive Charge (+): Occurs in cations, where protons outnumber electrons, giving the ion a net positive charge.
• Negative Charge (-): Occurs in anions, where electrons outnumber protons, creating a net negative charge.

The charge of an ion can be calculated by subtracting the number of electrons from the number of protons. This concept is crucial in chemistry as it explains why elements behave the way they do in different chemical reactions and why they form compounds. The play of electrical charges is what keeps atoms together in molecules and creates the diverse matter around us.