"A particle that consists of a nucleus of protons and neutrons surrounded by an electromagnetically-bound cloud of electrons."
The study of the structure of atoms, including their electrons, protons, and neutrons.
The history of atomic theory: The developmental stages of atomic theory, from ancient Greece to the present day.
Matter and energy: The relations between matter and energy including their properties and behaviour.
Atomic structure: The composition of atoms, including the subatomic particles such as protons, neutrons, and electrons.
Elements and isotopes: The atomic structure of elements and isotopes, and how they differ in their physical and chemical properties.
Electromagnetic radiation and spectroscopy: The relationship between electromagnetic radiation and atomic structure, and how these are related to spectroscopy.
Quantum Mechanics: The principles of quantum mechanics, including wave-particle duality and the Heisenberg Uncertainty Principle.
Electron configuration: The arrangement of electrons in atoms, including the importance of valence electrons.
Periodic properties of the elements: The periodic table of elements and its relationship to the atomic structure of elements.
Chemical bonding: The types of chemical bonds, including covalent, ionic, and metallic bonds, and how these are formed.
Molecular structure: The molecular structure of compounds, including their geometry, polarity, and bonding.
Kinetic theory of gases: The behaviour of gases, including their pressure, temperature, and energy.
Thermodynamics: The principles of thermodynamics, including the laws of thermodynamics and their applications in atomic structure.
Chemical reactions and stoichiometry: The principles of chemical reactions, including balancing equations and calculating stoichiometry.
Nuclear structure and radioactivity: The structure of atomic nuclei, including the principles of radioactivity and nuclear decay.
Photochemistry: The relationship between light and chemical reactions, including photochemical reactions and the photoelectric effect.
Quantum electrodynamics: The study of the interaction between light and matter in their quantum mechanical forms.
Nanotechnology and materials science: The application of atomic theory in nanotechnology and materials science, including the development of new materials and technologies.
Bohr's Model: It is a model of the hydrogen atom proposed by Niels Bohr. According to this model, electrons move in fixed orbits around the nucleus and can only exist in certain allowed energy levels.
Quantum mechanics: This theory describes the behavior of particles at the atomic level, where particles are represented as waves of probability. This theory is essential to understanding modern atomic and molecular physics.
Schrodinger's equation: A mathematical equation that determines the energy and behavior of particles on the atomic level.
Electron orbitals: These describe the probability of finding an electron at a specific location around the nucleus of an atom.
Pauli Exclusion Principle: This principle states that no two electrons in an atom can have the same quantum numbers.
Hund's Rule: This rule states that the electrons in a subshell with multiple orbitals will occupy each orbital singly before pairing up.
Born-Oppenheimer Approximation: This approximation allows to separate the motion of electrons and nuclei in molecular physics.
Bonding and anti-bonding orbitals: A bonding orbital is a region of space in which electrons are more likely to be found between two atoms in a bond. An anti-bonding orbital is a region of space where electrons are less likely to be found between two atoms in a bond.
Valence electrons: These are the electrons in the outermost shell of an atom and are involved in chemical bonding.
Molecular orbitals: These are energy states of a molecule that result from the mixing of atomic orbitals on the constituent atoms.
Electron spin and magnetic moment: The electron has a spin with a magnetic moment which affects its behavior in magnetic fields.
Ionization energy: The amount of energy required to remove an electron from an atom or ion.
Electron affinity: The energy released when an electron is added to an atom or ion.
Electronegativity: The ability of an atom to attract electrons towards itself when forming a chemical bond.
Isotopes: Atoms with the same number of protons but different numbers of neutrons.
"The chemical elements are distinguished from each other by the number of protons that are in their atoms."
"The number of protons that are in their atoms."
"Any atom that contains 11 protons is sodium, and any atom that contains 29 protons is copper."
"The number of neutrons."
"Atoms are so small that accurately predicting their behavior using classical physics is not possible due to quantum effects."
"Typically around 100 picometers across."
"More than 99.94%."
"If the numbers of protons and electrons are equal, as they normally are, then the atom is electrically neutral."
"If it has more protons than electrons, it has a positive charge, and is called a positive ion (or cation)."
"If an atom has more electrons than protons, then it has an overall negative charge, and is called a negative ion (or anion)."
"The electrons of an atom are attracted to the protons in an atomic nucleus by the electromagnetic force." "The protons and neutrons in the nucleus are attracted to each other by the nuclear force."
"The nuclear force is usually stronger than the electromagnetic force."
"When the repelling electromagnetic force becomes stronger than the nuclear force."
"The nucleus splits and leaves behind different elements."
"Chemical bonds to form chemical compounds such as molecules or crystals."
"The ability of atoms to attach and detach from each other."
"Chemistry is the discipline that studies these changes."
"A nucleus of protons and neutrons."
"If any are present, have no electric charge."