Atomic Structure and Isotopes Quiz

Atomic Structure Fundamentals

• Atomic Number: Represents the number of protons in an atom's nucleus, determining the element's identity.
• Bohr Model: Describes the atom as having a dense nucleus surrounded by electrons in defined orbits, helping to explain atomic properties and behaviors.
• Electron: A subatomic particle with a negative charge, orbiting the nucleus at various energy levels; relative mass is 1/1836 of a proton.
• Ion: Refers to an atom or molecule that has gained or lost electrons, resulting in a charged state.

Isotopes and Their Properties

• Isotopes: Variants of a chemical element that have the same number of protons and electrons but differing numbers of neutrons, leading to different atomic masses.
• Mass Number: The sum of protons and neutrons in an atomic nucleus, indicating the total number of these particles.

Instrumentation and Measurement

• Mass Spectrometry: A technique used to derive precise details on isotopic mass and the relative abundance of each isotope within a sample.
• Neutron: A subatomic particle with no charge, located in the nucleus with a relative mass of 1.
• Proton: A positively charged subatomic particle also found in the nucleus, possessing a relative mass of 1.

Mass Measurement Concepts

• Relative Abundance: Metric assessing the quantity of one substance in relation to another, often used in isotopic studies.
• Relative Atomic Mass: The average mass of an atom of an element, calculated relative to 1/12th the mass of a carbon-12 atom.
• Relative Isotopic Mass: Represents the mass of an individual isotope against 1/12th the mass of a carbon-12 atom.
• Relative Formula Mass: The mass of a compound's formula unit, particularly in giant structures, such as the NaCl with a relative formula mass of 58.44 g/mol.
• Relative Molecular Mass (Mr): The mass of a discrete molecule, often used in molecular chemistry.