Understanding Atomic Structure and Isotopes

These flashcards cover key vocabulary terms related to atomic structure and isotopes, including definitions and important concepts discussed in the lecture notes.

Atomic Number (Z)

The number of protons in the nucleus of an atom, which determines the identity of the atom.

Mass Number (A)

The total number of protons and neutrons in an atom's nucleus.

Neutron

A neutral subatomic particle found in the nucleus of an atom, with a mass of approximately 1.0087 amu.

Charge of an Electron

The charge of an electron is -1.602 x 10^-19 coulombs.

Cation

A positively charged atom that has lost one or more electrons.

Anion

A negatively charged atom that has gained one or more electrons.

Unified Atomic Mass Unit (u)

A unit of mass equal to 1/12 of the mass of a carbon-12 atom, approximately 1.6605 x 10^-24 g.

Mass Defect

The difference between the expected mass of an atom's subatomic particles and its actual mass.

Isotope

Atoms of the same element that have the same number of protons but different numbers of neutrons.

Average Atomic Mass

The weighted average mass of an element's isotopes based on their relative abundances.

Mass Spectrometry (MS)

An analytical technique used to measure the mass-to-charge ratio of ions to identify and quantify substances.

Chemical Symbol

An abbreviation that designates a chemical element, typically consisting of one or two letters.

Fundamental Unit of Charge (e)

The charge of a single electron, approximately 1.602 x 10^-19 coulombs.

Proton

A positively charged subatomic particle found in the nucleus, with a mass of approximately 1.0073 amu.

Subatomic Particle

Particles that make up atoms, including protons, neutrons, and electrons.