Question

Which of the following explain how an ion is formed? Explain your answer. a. adding or subtracting protons to/from an atom. b. adding or subtracting neutrons to/from an atom. c. adding or subtracting electrons to/from an atom.

Short answer

The correct answer is option c, which states that an ion is formed by adding or subtracting electrons to/from an atom. Adding or subtracting electrons changes the overall charge of the atom, forming either a positively charged ion (cation) or a negatively charged ion (anion).

Step-by-step solution

Understanding atomic structure

To find the correct answer, we should first understand the basic structure of an atom. An atom is made up of three types of particles: protons, neutrons, and electrons. Protons and neutrons are present in the nucleus of the atom, while electrons move around the nucleus in specific energy levels.

Analyzing option a

Option a states that an ion is formed by adding or subtracting protons to/from an atom. Adding or subtracting protons to/from an atom would change its atomic number, which determines the identity of the element. This process is not related to ion formation and is incorrect.

Analyzing option b

Option b states that an ion is formed by adding or subtracting neutrons to/from an atom. Changing the number of neutrons in an atom results in the formation of isotopes, but it doesn't affect the overall charge of the atom, so this option is also incorrect for ion formation.

Analyzing option c

Option c states that an ion is formed by adding or subtracting electrons to/from an atom. This is the correct answer, as adding or subtracting electrons from an atom changes the overall charge of the atom and forms ions. An atom becomes a positively charged ion (cation) if it loses electrons, and it becomes a negatively charged ion (anion) if it gains electrons. In conclusion, the correct answer is option c, which states that an ion is formed by adding or subtracting electrons to/from an atom.

Key concepts

Atomic Structure

The concept of atomic structure is fundamental to understanding chemistry and physics. Every atom consists of three main particles: protons, neutrons, and electrons. Protons and neutrons reside in the atom's nucleus, which serves as the dense, central core.
Electrons, on the other hand, orbit the nucleus in specific regions called energy levels or shells. This arrangement of particles forms the foundation of all matter in the universe. The roles of these particles are crucial to the atom's nature:

• Protons: These are positively charged particles and their number, known as the atomic number, determines an element's identity.
• Neutrons: Neutral particles that contribute to the atom's mass but do not affect its charge.
• Electrons: Negatively charged particles that are much lighter than protons and neutrons.

The interplay of these particles defines the characteristics and reactions of different elements, making atomic structure a cornerstone concept in science.

Protons and Electrons

Protons and electrons are vital to the identity and behavior of atoms. The balances and imbalances between them lead to fascinating chemical phenomena. Protons, with their positive charge, find balance with the negatively charged electrons, maintaining a neutral charge in a complete atom.
However, when atoms gain or lose electrons, they transform into ions, which play pivotal roles in electrical conductivity and chemical reactions. Understanding protons and electrons involves recognizing:

• The charge of protons is +1, making them central in identifying the atomic number of an element.
• Electrons have a -1 charge and live in defined energy levels, dictating interaction and bonding behavior.
• When electrons are either added or removed, the atom becomes an ion, which can either be a cation (positive) or an anion (negative).

This balance and interaction are central to understanding how matter around us behaves and reacts.

Isotopes and Ions

Isotopes and ions are distinct yet crucial concepts in atomic chemistry. Isotopes relate to the changes in the neutron count within the nucleus, while ions come from changes in the electron count.
Although these may sound similar at first, they influence properties in very different ways. Let's break down the ideas:

• Isotopes: Atoms with the same number of protons but different numbers of neutrons. They have virtually identical chemical properties, but can have different physical properties, such as stability and mass.
• Ions: Atoms that have gained or lost electrons. This change in electron count results in a net electric charge - either positive or negative, affecting how the atom interacts electrically with its surroundings.

These concepts are pivotal in fields ranging from nuclear chemistry to electrochemistry, highlighting their importance in fundamental scientific theories as well as practical applications.