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Quantum theory
Study of matter at subatomic levels.
Electromagnetic radiation
Wave of oscillating electric and magnetic fields.
Photoelectric effect
Emission of electrons when light hits a material.
Line spectra
Discrete wavelengths emitted by atoms.
Bohr model
Early atomic model focusing on electron orbits.
Quantum Mechanical model
Explains electron behavior in atoms.
Quantum numbers
Set of values describing electron properties.
Atomic orbitals
Regions where electrons are likely found.
Wavelength (λ)
Distance between corresponding points on waves.
Frequency (ν)
Number of waves passing a point per time.
Speed of light (c)
Constant at 3.00 x 10^8 m/s.
Constructive interference
Waves combine to form a larger wave.
Destructive interference
Waves cancel each other out.
Diffraction
Bending of waves around obstacles.
Subatomic particles
Electrons, protons, and neutrons in matter.
Reactive elements
Elements that readily undergo chemical reactions.
Inert elements
Elements that do not readily react.
Helium-Neon laser
Emits red light at 632.8 nm wavelength.
Cell phone frequency
Uses 835.6 MHz for communication.
Periodic table trends
Patterns in element properties based on electron behavior.
Chemical bonding
Attraction between atoms forming compounds.
Photoelectric effect
Electrons emitted when light strikes metal surface.
Threshold frequency
Minimum frequency for electron emission regardless of intensity.
Work function (Φ)
Energy needed to dislodge an electron from metal.
Kinetic energy of electrons
KEelectron = hν - Φ, where h is Planck's constant.
Photon
Quantum of electromagnetic radiation with energy hν.
Emission spectrum
Unique light pattern emitted by excited atoms.
Line spectra
Non-continuous spectra identifying specific elements.
Continuous spectrum
Unbroken range of wavelengths, like white light.
Atomic spectroscopy
Technique to identify elements using emission spectra.
Flame tests
Method to identify elements via color in flames.
Bohr model
Atomic model with quantized electron orbits.
Stationary states
Fixed electron orbits around the nucleus.
Energy quantization
Energy levels in an atom are discrete.
De Broglie wavelength
Wavelength associated with a particle's mass and velocity.
Matter waves
Wavelike behavior of particles proposed by De Broglie.
Electromagnetic radiation
Energy waves including visible light and others.
Energy of a photon
E = hν, where E is energy, h is Planck's constant.
Energy of 1 mole of photons
Multiply energy of one photon by Avogadro's number.
Laser pulse energy
Total energy contained in a laser pulse.
Frequency (ν)
Number of cycles per second of a wave.
Wavelength (λ)
Distance between consecutive peaks of a wave.
Ionization energy
Energy required to remove an electron from an atom.
DeBroglie Wavelength
Wavelength associated with a moving particle.
Electron Diffraction Pattern
Interference pattern showing electron wave nature.
Wave Duality
Electrons exhibit both wave and particle characteristics.
Interference Pattern
Pattern formed by overlapping waves.
Heisenberg's Uncertainty Principle
Position and velocity uncertainties are inversely proportional.
Complementary Properties
More knowledge of one property reduces knowledge of another.
Electron Energy
Kinetic energy related to electron position.
Kinetic Energy Formula
KE = ½mv², where m is mass.
Schrödinger Equation
Equation incorporating wave-particle duality of electrons.
Wavefunction (Ψ)
Describes all information about an electron.
Orbital
Region of high probability for finding an electron.
Quantum Numbers
Set of numbers defining electron's state.
Principal Quantum Number (n)
Indicates energy level and size of orbital.
Energy Level Formula
En = -2.18 × 10⁻¹⁸ J (1/n²).
Angular Momentum Quantum Number (l)
Determines shape of the orbital.
s-Orbital
Spherical shape, l = 0.
p-Orbital
Dumbbell shape, l = 1.
d-Orbital
Four-leaf clover shape, l = 2.
f-Orbital
Eight balloons shape, l = 3.
Multi-Electron Systems
Require approximations to solve Schrödinger's equation.
High Probability Region
Area where electron is likely to be found.
Wave Function Squared (Ψ²)
Defines the probability density of finding an electron.
Magnetic Quantum Number (ml)
Describes orbital orientation; values from -l to +l.
Spin Quantum Number (ms)
Indicates electron spin; +½ or −½ values.
Principal Energy Level (n)
Indicates the energy level of an electron.
Sublevel (l)
Defines shape of orbitals; values from 0 to n-1.
Orbital
Region where an electron is likely found.
Subshell
Group of orbitals with same n and l values.
Energy Level Count
Number of sublevels equals n; orbitals = n².
Orbital Count in Sublevel
Number of orbitals = 2l + 1.
Hydrogen Emission Spectrum
Photon energy equals difference between electron states.
Probability Density (ψ²)
Probability of finding an electron at a point.
Radial Distribution Function
Total probability of finding an electron at distance r.
Node
Point where probability density drops to zero.
s Orbital (l=0)
Spherical shape; one orbital per principal energy state.
p Orbitals (l=1)
Dumbbell shape; three orbitals oriented along axes.
d Orbitals (l=2)
Five orbitals; complex shapes, some aligned with axes.
f Orbitals (l=3)
Seven orbitals; complex shapes, often eight-lobed.
Phase of an Orbital
Sign of wave function; affects orbital interaction.
Emission Spectrum Line
Represents energy transition between electron states.
Electron Relaxation
Electron emits light when transitioning to lower energy.
Quantum Number Set
n, l, ml define unique orbital characteristics.
Energy Transition Requirement
Electron must gain specific energy to move states.
Principal Shell
Another term for principal energy level.
Subshell Type
Also known as subshell; defined by n and l.
