Atomic Structure and Properties

Electrons

Photons

Neutrons

Protons

Jump from one principal energy level to another

Introduction of a doubly occupied subshell

Variations in inner shell shielding effect

Formation of a half-filled subshell

Transfer

Gain

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Two inner-shell electrons exhibit greater repulsion among each other than those in outer shells, leading to pronounced distinctive spectral features rather than diffuse ones outer shells exhibit

Inner-shell electrons show less shielding and experience stronger nuclear charge attraction, forcing them into more distinct energy levels resulting in narrower peaks

Inner-shell electrons always have lower energy than outer-shell electrons, thus tightly packed, producing clear-cut sharp signals atop the spectrum

Outer-shell electrons are easier to eject because they're further from the nuclear core, creating broader and less intense peaks due to increased average distances between orbitals

Phosphorus

Aluminum

Silicon

Neon

Silver chloride (AgCl)

Nitric acid (HNO3)

Silver sodium chloride (AgNaCl2)

Sodium nitrate (NaNO3)

Number of protons in the nucleus.

The exact mass of an electron.

Bond angles between atoms in a molecule.

Energy levels of electrons.

The color it exhibits when in a flame test

The precise atomic mass of the isotope examined

The temperature at which it undergoes phase change

The energy levels of its electrons

By detecting heavy metal pollutants in water sources

Monitoring atmospheric nitrogen levels due to industrial emissions

Determining oxygen concentrations dissolved in ocean water layers

Measuring carbon dioxide uptake by plant photosynthesis processes

Reactant side has more compounds than product side.

Atoms are conserved; same number on both sides for all elements involved.

Products have lower potential energy than reactants.

Total kinetic energy is equal on both sides of the equation.