orbitals

• The principal quantum number (n) determines the energy level of an orbital, while the azimuthal quantum number (l) determines the shape or angular momentum of the orbital.
• The radiation's energy increases from the radio wave end of the spectrum to the gamma ray end.
• Visible light is a very small part of the entire spectrum.
• The speed of light, c, is constant.
• The energy of a photon, E, is related to the frequency, v, and the wavelength, X, of the radiation as E = hv.
• Kinetic energy, KE, is stored in the motion of an object.
• Potential energy, PE, is the energy of an object based on its interaction with others, such as gravity or electrostatic interaction.
• Gravity is a type of potential energy.
• Electrostatic interaction is a type of potential energy.
• The unit of energy is the Joule (J).
• Different forms of energy can be converted into each other, for example, a calorie (cal) can be converted into 1 Kcal.
• An electronvolt (eV) is equal to 1.6 x10-19J.
• Total energy is always constant and is conserved in a closed system.
• Some observations are inconsistent with the wave picture of light.
• Blackbody radiation is the glow emitted by hot, macroscopic objects.
• The observed spectrum of blackbody radiation is continuous with a peak who's position depends on temperature (higher temperature = lower wavelength)
• The peak position of the observed spectrum depends on temperature, with a higher temperature resulting in a lower wavelength.
• Classical theory, which assumes that light is a wave, predicts that there is an infinite amount of low-frequency light shining on metals, also known as "blacklight".
• The photoelectic effect, which assumes that light is a particle, predicts that electrons will be emitted when shining light on metals.
• Max Planck assumed that energy is quantized: the amount of energy at some higher frequency is always an integer multiple of the fundamental packet size.
• Photons, which have energy v = frequency, are emitted when light is a stream of particles, n = planck's constant (6.62x10-3 Js).
• Hydrogen gas emits light at specific wavelengths/frequencies/energy.
• White light is transmitted through cold hydrogen gas.
• Atoms emit light only at specific wavelengths/frequencies/energy.
• Atoms absorb light only at the same wavelengths/frequencies/energies.
• An atom in a high-energy state can transition to a lower-energy state, and the energy that the atom lost is carried away by an emitted photon.
• An atom in a low-energy state can absorb a photon of transition to a higher-energy state if the photon energy matches the difference in atom energies exactly.
• A double slit experiment can show a diffraction pattern caused by interference.
• Matter also exhibits wave-particle duality.
• An object of mass m moving with velocity v behaves like a wave with wavelength x = h/(m xv).
• Bohr's Model describes the electron (of the Hydrogen atom and other single-electron atoms) as having charge -1.
• In Bohr's Model, the electron moves in circular orbits around the nucleus.
• These orbits are stable, because electrostatic and nucleus charge are in balance.
• The wavelength of the electron must fit into orbit n times, where n is always an integer or whole number.
• Certain orbits, aka certain values of the energy, are allowed.
• The energy levels of single-electron atoms are represented by the formula n = 1, 2, 3, ...
• Single-electron atoms are referred to as Rydberg atoms.
• All energy levels of Rydberg atoms are negative.
• The largest space between energy levels of Rydberg atoms is between n = 1 and n = 2.
• A transition in Rydberg atoms is a change of state from an initial value ni to a final value ne.