Atomic Nomenclature

A

Atomic Mass Number (Z + N = A) (whole number)

Z

Atomic Number (# of protons)

N

Number of Neutrons (A - Z = N)

Atomic Mass Number

Whole number representing the total number of nucleons (protons + neutrons)

Isotopes

Atoms with the same number of protons but different atomic mass numbers

Isobars

Atomic nuclei with the same atomic mass number but different atomic numbers

Isotones

Atoms with the same number of neutrons but different numbers of protons

Isomers

Atoms with the same atomic number and atomic mass number but exist at different energy states due to nucleon arrangement

Covalent Bonds

Formed by the sharing of electrons between atoms

Covalent Bonds Example

H₂O (Water)

Covalent Bonding in Water

Oxygen (6 valence electrons) shares 2 electrons with 2 hydrogen atoms

Ionic Bonds

Formed by the transfer of electrons between atoms

Ionic Bonds Example

NaCl (Salt)

Ionic Bonding in NaCl

Sodium (Na) loses 1 electron to Chlorine (Cl), forming Na⁺ and Cl⁻ ions

Radioactivity

Emission of particles and energy to achieve stability

Radioactive Decay

Unstable nuclei spontaneously emit particles and energy, transforming into another atom