Atomic Structure Quiz

Subatomic Structure Overview

• Three primary subatomic particles: protons, neutrons, and electrons.

Nucleus Composition

• The nucleus is composed of protons and neutrons, forming the dense core of an atom.

Nucleus Size Relationship

• A larger nucleus diameter corresponds to a larger overall atom diameter and increased mass.

Protons

• Protons are located in the nucleus, carry a positive charge, and define the atomic number of an element.

Neutrons

• Neutrons also reside in the nucleus, possess no charge (neutral), and contribute to atomic mass alongside protons.

Electrons

• Electrons are negatively charged particles found in energy levels surrounding the nucleus, organized in an electron cloud.

Electron Mass Comparison

• The mass of an electron is significantly smaller than that of protons and neutrons, about 1/1830, contributing negligibly to atomic mass.

Atomic Neutrality

• An atom is neutral when the number of protons equals the number of electrons, balancing positive and negative charges.

Ions

• Ions are charged atoms, formed by the exchange of electrons.
• Positive ions have more protons than electrons, while negative ions have more electrons than protons.

Simplest Atom

• The simplest atom, hydrogen, contains one proton and one electron.

Atomic Number

• The atomic number indicates the number of protons in an element, which defines the element's identity.

Specific Atomic Numbers

• Carbon has an atomic number of 6, while iron has an atomic number of 26.

Isotopes and Mass Number

• The mass number combines the total count of protons and neutrons, while electrons are excluded due to their minimal mass.

Sodium Example

• Sodium has an atomic number of 11 (11 protons); with an atomic mass of 23, it has 12 neutrons (23 - 11 = 12).