Practical Atomic Model offers practical explanations for atoms and their behaviors.In 1913, Niels Bohr's atomic model defined circular orbits for an atom's electrons.In 1916, Gilbert Lewis defined a dot structure for a simple method of managing each element's circular ring of valence electrons. Its use continues though with known limitations.By the 1920s, quantum mechanics brought uncertainty claiming electrons behaved like a wave having its position defined by probabilities.In 1952, Charles Coulson marked the start of modern valence bond theory. Since the 1980s, its difficult problems were solved. Each element has a specific pattern for its electrons around its nucleus. These configurations are predictable. In chemistry, there is no uncertainty about electrons. Bonding between atoms is certain given their known valence behavior. Chemical reactions require time because the atomic collision rate has many factors.If the uncertainty principle truly applied to electrons, then chemistry could not predict these reactions.All of the evidence supports an atom's electrons are found in a defined sequence of circular rings with each having a defined capacity of electrons.There are 20 elements having an anomaly where an electron has moved to an adjacent circular ring in the configuration. This transfer is awkward for the quantum orbitals which are driven by probabilities and have different patterns of lobes in the set of distinct s/p/d/f shells. Circular rings having a similar radius enable such a transfer.Chemists have used these verified electron configurations for decades.This predictability should have diminished with the introduction of quantum mechanics and its uncertainty principle. QM claimed electrons behave like waves and their position cannot be defined except as a probability, often called a wave function. Chemical reactions and their molecular bonds require consistency in an element's electron configuration.There is much less uncertainty in an atom than is currently claimed in the current atomic model. Electrons are real particles, having a measured size and mass. The effective size of each element's electron cloud has been measured. The size and the sequence of the respective rings are well established.For quantum mechanics to persist in an atomic model, it requires evidence for its crucial claim that an electron's location is uncertain and can be found only by probabilities.The book describes an atom's use of protons and electrons, the 2 fundamental particles. Combinations of their odd and even counts affect the stability and radioactive decay of the atom's nucleus. The 118 elements and their isotopes have an atomic weight ranging from 1 to 295. These 295 are analyzed to reveal the behavior for nucleus stability driven by or even counts of its nucleons.A practical atomic model provides a better explanation of certain atomic behaviors, such as a) suggesting a new naming convention for the concentric rings of electrons to suit the actual configuration in their order from the nucleus; this new order directly helps identify the valence electrons from the outer rings, b) building a nucleus using protons and electrons as affected by the odd/even counts affecting its topology, c) describing the steps of radioactive decay, and d) describing an atom's interactions with light. Light carries a continuum of energy which can span many wave lengths. Atoms react to wave lengths in the continuum, not to particles; photons do not exist.This book follows Practical Particle Physics which explained: a) the atomic mass defect behavior; b) there are only 2 fundamental particles, electron and proton; c) Quarks are non-functional debris from a collision of particles; and d) Quasi-particles like a photon and graviton do not exist. There are no quarks and quasi-particles in a practical atomic model.