Untitled Quiz

Study Notes

Hertz: SI unit of frequency; measures the number of waves passing a given point per unit time.
Atomic Orbital: Region around an atomic nucleus where an electron is likely to be found.
Spectrum: Range of colors produced when light passes through a prism, revealing various wavelengths.
Emission Spectrum: Specific lines of colored light emitted by an element when light is passed through a prism.
Quantum of Energy: The minimum amount of energy needed to move an electron from one energy level to a higher one.
Amplitude: Maximum distance from the wave's axis to the crest; indicates the strength of the wave.
Wavelength: Distance between successive crests of a wave; measured in nanometers.
Energy Level: The fixed distance from the nucleus where electrons exist; electrons occupy the lowest energy levels first (Aufbau Principle).
Frequency: Number of occurrences of a repeating event; in waves, it's how many waves pass a point in a second.
Aufbau Principle: Electrons fill orbitals starting from the lowest energy level upwards.
Pauli Exclusion Principle: No two electrons in an atom can have the same set of quantum numbers; each orbital can hold two electrons at most.
Hund’s Rule: Electrons will occupy degenerate orbitals singly before pairing up in orbitals of equal energy.
Ground State: The lowest energy state of an atom, with electrons in the most stable configuration.
Photons: Particles of light that carry quantized energy.

Maximum number of electrons in an energy level: (2n^2)
Maximum number of orbitals in an energy level: (n^2)
As frequency increases, wavelength decreases; these two are inversely proportional.
As wavelength increases, energy decreases; these two are also inversely proportional.
As energy increases, frequency increases; energy and frequency are directly proportional.

Full Electron Configurations: Describe how electrons are distributed among the atomic orbitals for elements and ions, such as Sodium (Na), Chlorine (Cl), and Nickel (Ni).
Condensed Electron Configurations: Use the noble gas shorthand for simplicity in representing electron arrangements of elements and ions.

When an atom absorbs energy, electrons transition to higher energy states (excited state).
An atom releases the same quantum of energy absorbed when returning to a lower energy state, often observed as emitted light.
Energy absorption vs. emission occurs during transitions between defined energy levels.

All types of electromagnetic waves vary in wavelength and frequency; the spectrum includes gamma rays, X-rays, ultraviolet, visible light, infrared, microwaves, and radio waves.
Each type of wave can be defined by its relative energy, wavelengths, and frequencies, arranged from longest to shortest.

Ensure familiarity with various atomic orbitals (s, p, d, f) and their characteristics in terms of shape and energy.
Practice calculating wavelength, frequency, and energy using the appropriate formulas.
Understand and apply the principles governing electron configurations and transitions between energy levels.
Review the characteristics of the electromagnetic spectrum and its implications in different scientific applications.