1: Determine the number of electrons. 2: Apply the Aufbau principle. 3: Follow the order of increasing sublevel energies (1s, 2s, 2p, 3s, 3p, etc.). 4: Use the periodic table as a guide.

1: Determine the electron configuration. 2: Represent each orbital as a box. 3: Follow the Aufbau principle, Pauli exclusion principle, and Hund's rule to fill the orbitals with arrows representing electrons.

1: Write the electron configuration. 2: Identify the outermost shell (highest principal quantum number). 3: Count the electrons in the s and p orbitals of the outermost shell.

A subatomic particle located in the nucleus with a charge of +1 and a mass of approximately 1 amu.

A subatomic particle located in the nucleus with a charge of 0 and a mass of approximately 1 amu.

A subatomic particle orbiting the nucleus with a charge of -1 and negligible mass.

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

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

Electrons located in the outermost s and p orbitals of an atom; they determine chemical properties.

The arrangement of electrons within an atom, specifying the energy levels and sublevels occupied.

Core Electrons: Located in inner shells, do not participate in bonding. | Valence Electrons: Located in the outermost shell, determine chemical properties and bonding behavior.

Bohr Model: Electrons orbit the nucleus in fixed, circular paths with specific energy levels. | Quantum Mechanical Model: Electrons exist in orbitals (regions of probability) with different shapes and energy levels, described by quantum numbers.