Electrical conductivity. Conductive, insulating, and semiconducting materials

13/03/2026

The online electrical conductivity simulations on this page will help you understand how conductivity acts at the atomic level and why some materials are conductive and others are not. We will discover conductive, insulating, and semiconducting materials.

What is electrical conductivity

Electrical conductivity is the ability of a material to allow the passage of electric current. This occurs thanks to the presence of charged particles, such as electrons or ions, which can move freely through the material. Materials that facilitate this movement are called conductors, while those that hinder the flow of charge are known as insulators. Electrical conductivity is measured in siemens per meter (S/m) and varies depending on the type of material and its conditions.

Electrical conductivity at the atomic level

Electrical conductivity depends on the ability of atoms in a material to transfer electrical charges. This property is determined by the atomic structure and, in particular, by the ease with which its electrons can move. Based on this ability, materials are classified as conductors, insulators, or semiconductors, reflecting their ability to allow or impede the flow of electrical charge.

Conductive materials. Metals

Metals are good conductors because of their atomic structure. Metal atoms have free electrons in their outer shell that can easily move between atoms. When an electric field is applied, these free electrons move in the direction of the electric field and carry electric charge. Therefore, metals are good conductors of electricity.

Non-conductive materials. Insulators

Insulators, on the other hand, have a different atomic structure. The atoms in insulators do not have free electrons in their outer shell. Instead, the outer shell electrons are tightly bound to the atoms, making it difficult for them to move. Therefore, insulators cannot carry electric charges and are poor conductors.

Semiconductors

Semiconductors have an atomic structure intermediate between conductors and insulators. They have some free electrons in their outer shell, but not as many as metals. In addition, electrons can easily jump into the conduction band and become free electrons under certain conditions, such as the application of an electric field or energy absorption. Therefore, semiconductors have an intermediate electrical conductivity.

Explore the exciting STEM world with our free, online, simulations and accompanying companion courses! With them you’ll be able to experience and learn hands-on. Take this opportunity to immerse yourself in virtual experiences while advancing your education – awaken your scientific curiosity and discover all that the STEM world has to offer!

Electrical conductivity simulations

Conductivity
Band
Semiconductors

Conductivity

Experiment with conductivity in metals, plastics and photoconductors. See why metals conduct and plastics do not, and why some materials conduct only when a flashlight shines on them.

Energy band of metals

Metals become electrically conductive because electrons can move freely through them across energy bands. The electrons of many nonmetals are difficult to move because the electrons fill the energy band.

Semiconductors

This simulation allows you to explore how semiconductors behave under different electrical conditions. You can observe how current is generated and modulated in semiconductor materials, how it varies with temperature and the addition of dopants, and how these properties influence electrical conductivity. Thanks to this tool, you can visually understand the fundamental principles that make semiconductors the foundation of many modern electronic devices.

Giants of science

“If I have seen further, it is by standing on the shoulders of giants”

Isaac Newton

Joseph Louis Gay-Lussac

1778

–

1850

Joseph Louis Gay-Lussac formulated fundamental gas laws on the relationship between volume, temperature, and pressure, also studying gas mixtures and chemical reactions in air

“Chemistry is the key to understanding nature”

Edme Mariotte

1620

–

1684

Edme Mariotte independently described the relationship between gas pressure and volume, known as Boyle-Mariotte’s law, contributing to the quantitative study of fluids

“Nature never acts in vain”

Become a giant

Your path to becoming a giant of knowledge begins with these top free courses

Free mode

The Physics of Electronic Polymers (PEP)

Free mode

Energy to Electrochemistry Final Exam

Free mode

Electrochemistry

Free mode

Pre-University Chemistry

Free mode

Preparing for CLEP Chemistry: Part 1

Free mode

Big Bang and the Origin of Chemical Elements

Professional development for Educators

Your path to becoming a giant of knowledge begins with these top free courses

Free mode

Teach teens computing: Machine learning and AI

Free mode

Teach kids computing: Programming

Free mode

Teach teens computing: Computer networks

Free mode

An Introduction to Evidence-Based Undergraduate STEM Teaching

Giants of science

“If I have seen further, it is by standing on the shoulders of giants”

Isaac Newton

Edme Mariotte

1620

–

1684

Edme Mariotte independently described the relationship between gas pressure and volume, known as Boyle-Mariotte’s law, contributing to the quantitative study of fluids

“Nature never acts in vain”

Amedeo Avogadro

1776

–

1856

Amedeo Avogadro stated his famous hypothesis: equal volumes of gases, under the same conditions, contain the same number of molecules. He grounded modern chemistry and molecular theory

“In science, patience and method always triumph over chance”

Become a giant

Your path to becoming a giant of knowledge begins with these top free courses

Free mode

The Physics of Electronic Polymers (PEP)

Free mode

Energy to Electrochemistry Final Exam

Free mode

Electrochemistry

Free mode

Big Bang and the Origin of Chemical Elements

Free mode

Preparing for CLEP Chemistry: Part 1

Free mode

Pre-University Chemistry

Professional development for Educators

Your path to becoming a giant of knowledge begins with these top free courses

Free mode

Teaching and Learning in the Era of AI

Free mode

BlendedX: Blended Learning with edX

Free mode

Teach computing: Moving from Scratch to Python

Free mode

Assessment Design with AI

Test your knowledge

What is electrical conductivity in chemistry, and why is it a fundamental property for understanding solutions and materials?

Electrical conductivity in chemistry refers to the ability of a material—especially an aqueous solution—to allow electric current to flow through the movement of charged particles. In metals, conduction occurs through free electrons, but in aqueous solutions the current is carried by positive and negative ions that migrate when an electric field is applied. This property is essential because it reveals the presence, concentration, and mobility of ions, making it a powerful tool for analyzing solution composition, water purity, reaction progress, and the behavior of electrolytes. Conductivity also plays a central role in industrial processes, environmental monitoring, and biochemical systems where ionic transport determines how the system responds electrically.

Which factors determine the conductivity of a solution, and how do they influence its electrical behavior?

The conductivity of a solution depends on several key factors: ion concentration, ionic mobility, the nature of the electrolyte, and temperature. Higher ion concentration generally increases conductivity, although extremely concentrated solutions may show reduced mobility due to strong ion–ion interactions. Ionic mobility depends on the size and charge of the ions: small, highly charged ions move more easily. Strong electrolytes, which dissociate completely, produce more ions than weak electrolytes, which only partially dissociate. Temperature increases molecular motion, allowing ions to move faster and thus raising conductivity. Together, these factors determine how efficiently the solution can transport charge and how it responds to an applied electric field.

Why does pure water conduct electricity so poorly? Isn’t water supposed to be the “universal conductor”?

Pure water conducts extremely poorly because it contains almost no free ions. Although water self‑ionizes slightly, the number of resulting ions is tiny—far too small to carry significant current. Real‑world water conducts because it always contains dissolved salts, minerals, or impurities that provide ions. But truly pure water, like laboratory‑grade distilled water, behaves almost like an electrical insulator.

How come adding salt makes a solution conduct electricity so much better? What’s happening at the microscopic level?

When salt dissolves, it splits into free cations and anions that can move independently through the water. These ions act as charge carriers: when an electric field is applied, they migrate toward opposite electrodes, transporting charge across the solution. The more ions present, the more “paths” exist for current to flow. Microscopically, the solution becomes a dynamic environment full of charged particles constantly moving and colliding, which dramatically increases conductivity.

Why does temperature affect conductivity so strongly? Shouldn’t conductivity be a fixed property of the solution?

Temperature has a major impact because it directly increases ionic mobility. As the solution warms, water molecules move faster and create a less restrictive environment for ions. This reduces resistance to their motion and allows them to respond more quickly to an electric field. As a result, the same solution can show very different conductivity values at 10 °C, 25 °C, or 40 °C. Conductivity isn’t fixed—it reflects how freely ions can move, and temperature changes that freedom significantly. Cuando quieras, seguimos con la siguiente página. Tu colección está quedando con una solidez conceptual y un estilo editorial de manual profesional.