Structure of the Atom

Atomic structure: This includes subatomic particles such as protons, neutrons, and electrons that make up an atom.

Rutherford's model of the atom: This model proposed that the atom has a positively charged nucleus containing protons and neutrons, surrounded by negatively charged electrons in orbitals.

Electron configuration: This refers to the arrangement of electrons in an atom's orbitals and can help predict reactivity and chemical bonding behaviour.

Bohr's model of the atom: This model proposed that electrons exist in specific energy levels or shells around the nucleus and can only move from one energy level to another by absorbing or emitting energy.

Quantum mechanics: This field explains the behaviour of particles at the atomic and subatomic levels and uses mathematical models to predict phenomena such as electron behaviour and chemical bonding.

Quantum numbers: These are a set of four numbers that describe the properties of electrons in orbitals such as energy level, orbital shape, orientation, and spin.

Electron orbitals and energy levels: These describe the spatial distribution of electrons around the atom's nucleus at specific energy levels.

Periodic trends: These are predictable patterns in the properties of elements when arranged in order of increasing atomic number on the periodic table, including size, ionization energy, and electronegativity.

Electron configuration of ions: This refers to the arrangement of electrons in a positively or negatively charged ion and can differ from the configuration in a neutral atom.

Nuclear reactions: These involve changes to the nucleus of an atom, including radioactive decay, fusion, and fission.

Isotopes: These are different forms of an element that have the same number of protons but different numbers of neutrons.

Mass spectrometry: This technique analyzes the mass-to-charge ratio of particles to identify isotopes and determine the composition of a sample.

X-ray diffraction: This is a technique used to study the arrangement of atoms in crystals and to determine the chemical bond distances between atoms.

Atomic spectroscopy: This is a technique used to study the interaction of atoms with electromagnetic radiation and can be used to identify the composition of substances.

Photoelectric effect: This refers to the emission of electrons from a metal surface when exposed to light and was a key experiment that supported the wave-particle duality of particles.

The Bohr Model: This model proposes that electrons orbit the nucleus in specific layers or shells.

The Quantum Mechanical Model: This model describes the electrons in terms of their probability clouds, rather than as discrete particles orbiting the nucleus.

The Wave Model: This model treats electrons as waves rather than particles, and it uses mathematical equations to describe their behavior.

The Rutherford Model: This model proposes that atoms consist of a small, dense, positively charged nucleus surrounded by negatively charged electrons.

The Electron Cloud Model: This model depicts electrons as existing within a three-dimensional space around the nucleus, rather than in specific orbits.

The Plum Pudding Model: This model, developed by J.J. Thomson, proposes that atoms consist of a diffuse, positively charged substance with negatively charged electrons embedded throughout.

The Shell Model: This model uses a series of energy levels to describe the distribution of electrons in an atom. Each level can hold a specific number of electrons.

The Nuclear Shell Model: This model describes the distribution of protons and neutrons in the nucleus of an atom.

The Resonance Model: This model proposes that electrons can exist in multiple, equivalent energy states simultaneously, and that they shift between these states in a process called resonance.

The Pauli Exclusion Principle: This principle states that no two electrons in an atom can have the same set of quantum numbers, which are properties that describe their energy levels and other characteristics.