Question

Which statement about electrons is true? (a) Electrons attract one another. (b) Electrons are repelled by protons. (c) Some electrons have a charge of \(1-\) and some have no charge. (d) Electrons are much lighter than neutrons.

Short answer

The true statement about electrons is (d) Electrons are much lighter than neutrons.

Step-by-step solution

Understanding Fundamental Particle Interactions

Particles with like charges repel each other, and particles with unlike charges attract each other. Electrons, which have a negative charge, will be repelled by other negatively charged electrons and attracted to positively charged protons.

Assessing the Validity of each Statement

Evaluate each statement: (a) states the opposite of fundamental charge interactions, so it's false; (b) is incorrect as it contradicts the basic principle of opposite charges attracting; (c) is false because all electrons have a charge of exactly \(1-\), with none having no charge; (d) can be verified by comparing the masses of electrons and neutrons.

Comparing Electron and Neutron Mass

By looking at the known values of electron and neutron mass (electron: approximately 9.109 x 10^-31 kg, neutron: approximately 1.675 x 10^-27 kg), it is clear that electrons are much lighter than neutrons.

Key concepts

Charge Properties of Electrons

Electrons are fundamental particles known for carrying a negative electrical charge, denoted as \(-1e\). With an intrinsic property called ‘electric charge’, electrons play a crucial role in electricity, magnetism, and chemical bonding.

Electrons are perpetually in motion around the nucleus of an atom and their negative charge is essential in balancing the positive charge of protons in the nucleus. It’s this balance of charges that determines the overall charge of an atom or molecule. This balance is also responsible for creating the attractive forces which hold atoms and molecules together in various states of matter.

Mass Comparison Between Electrons and Neutrons

When comparing the mass of an electron to that of a neutron, one can observe a significant difference. An electron has a mass approximately equal to \(9.109 \times 10^{-31}\) kilograms, which is less than one-thousandth the mass of a proton or neutron. In contrast, a neutron has a mass of around \(1.675 \times 10^{-27}\) kilograms.

Despite their tiny mass, electrons play an essential role in determining the chemical properties of elements and their reactions. However, because of their low mass, they contribute far less to the actual weight of an atom compared to protons and neutrons, the latter being nearly 2000 times heavier than electrons.

Basic Principles of Electrical Charge

The basic principles of electrical charge are relatively straightforward: like charges repel each other, and unlike charges attract. There are two types of electrical charges, positive and negative. Protons carry a positive charge, electrons carry a negative charge, and neutrons are neutral—it is the attraction between the negatively charged electrons and the positively charged protons that keeps electrons in orbit around the nucleus.

These principles of electrical charge govern a wide range of phenomena, from the forces that bind atoms together to form molecules, to the operation of electronic devices, and even the attraction or repulsion between objects that have become electrically charged through friction.

Atomic Particle Interactions

Atomic particle interactions refer to the ways in which protons, neutrons, and electrons interact within an atom and with other atoms. Electrons form a cloud around the nucleus, which consists of protons and neutrons. The interactions between these particles are governed by the electromagnetic force, one of the four fundamental forces of nature, as well as by the strong nuclear force that holds the nucleus together.

When atoms come close together, the electrons can be shared or transferred between atoms, leading to chemical bonds such as ionic or covalent bonds. It is these microscopic interactions that dictate the atomic and molecular structures and, consequently, the macroscopic properties of all matter.