Atomic Theory Lecture 1

A historical progression of models explaining the structure of atoms.

Ancient Greek philosophers proposed that matter was composed of indivisible particles called atoms.

Dalton proposed four postulates about atoms: indivisible, indestructible, identical within the same element, and combine to create compounds.

Thomson discovered the electron, and proposed a model of the atom with negatively charged electrons embedded in a positively charged sphere.

Rutherford discovered the nucleus, a dense, positively charged center of the atom, surrounded by orbiting electrons.

Bohr proposed that electrons orbit the nucleus in specific energy levels or shells.

A model based on quantum mechanics; it describes electrons probabilistically, as clouds of electron density, rather than definite orbits.

Regions of space around the nucleus where there is a high probability of finding an electron.

The number of waves that pass a given point in a unit of time.

The distance between two corresponding points of a wave.

Energy of radiation is proportional to frequency.

A fundamental constant that relates the energy of a photon to its frequency.

The range of all types of electromagnetic radiation.

A discrete packet of energy, like a step in a stepwise relationship.

The emission of electrons when light shines on a material.

Energy exists in discrete packets or quanta.

Specific, quantized energy levels for electrons in an atom, also called shells.

Regions in space where electrons are likely to be found, solutions to his equation.

It is impossible to know both the exact position and momentum of a particle simultaneously.

Theory describing the behavior of matter and energy at the atomic and subatomic levels.

The number of waves that pass a point per second, measured in Hertz (Hz).

Energy transmitted through space as waves, with electric and magnetic fields.

A shorter wavelength corresponds to a higher frequency, and vice versa, according to the equation : 𝜆 = c.

The smallest unit of an element that retains the chemical properties of that element.

A historical progression of models describing the atom's structure, from ancient Greek ideas to modern quantum mechanics.

Discovered the electron and proposed a model where negatively charged electrons were embedded in a positively charged sphere.

Discovered the nucleus, a densely packed, positively charged center, surrounded by orbiting electrons.

Proposed electrons orbiting the nucleus in specific energy levels or shells, quantifying their energy.

A specialized microscope that allows scientists to image atomic orbitals, giving us a glimpse of the electron distribution around the atom's nucleus.

Electrons in atoms occupy specific energy levels, called orbits or shells, which are quantized (discrete, distinct values).

Schrödinger's equation, a mathematical model, describes the behavior of electrons in atoms, and its solutions define the regions of space where electrons are likely to be found, called atomic orbitals.

Electromagnetic radiation travels as waves with a specific wavelength, which represents the distance between two corresponding points on the wave.

Longer wavelengths correspond to lower frequencies, and shorter wavelengths correspond to higher frequencies. This relationship is described by the equation: wavelength = speed of light / frequency.

Describes the wave-particle duality of matter. The wavelength of a moving particle is inversely proportional to its momentum.

Quantum mechanics describes the behavior of very small particles, while classical mechanics, which is based on Newton's laws, describes the motion of larger objects.

The wavelength of electromagnetic radiation is inversely proportional to its frequency. This means a shorter wavelength corresponds to a higher frequency, and vice versa. The relationship is defined by the equation: 𝜆 = c, where 𝜆 is the wavelength, c is the speed of light, and ν is the frequency.

The frequency (ν) of electromagnetic radiation can be calculated using the formula: ν = c/λ, where c is the speed of light (3.00 x 10^8 m/s) and λ is the wavelength in meters.

The energy (E) of electromagnetic radiation is directly proportional to its frequency (ν). This means that the higher the frequency, the greater the energy. The relationship is described by Planck's equation: E = hν, where h is Planck's constant (6.626 x 10^-34 J·s).

Planck's constant (h) is a fundamental constant in physics that relates the energy of a photon to its frequency. It has a value of 6.626 x 10^-34 J·s.

This equation, known as Planck's equation, describes the relationship between the energy (E) of a photon and its frequency (ν), where h is Planck's constant. It essentially states that the energy of a photon is proportional to its frequency.