CH 301 Unit 1 Exam 1 Review Flashcards

Vocabulary flashcards covering electromagnetic radiation, photoelectric effect, wave-particle duality, and orbital electron configuration rules for CH 301 Unit 1 Exam 1.

Electromagnetic Radiation Spectrum Ranking

The classification of electromagnetic waves in order of increasing Energy ($E$) and Frequency ($v$): Radio Waves < Microwaves < Infrared < Visible < Ultraviolet < X-Rays < Gamma Rays.

Planck's Constant ($h$)

A fundamental physical constant equal to $6.6 \times 10^{-34}\,J \cdot s$ used to convert photon frequency to energy.

Speed of Light ($c$)

A physical constant representing the speed of electromagnetic waves in a vacuum, given as $3 \times 10^8\,m/s$.

Photon Energy Equations

Equations used to calculate photon energy given frequency ($v$) or wavelength ($\lambda$): $E = h \cdot v$ and $E = \frac{h \cdot c}{\lambda}$.

Visible Light Wavelength Range

The general wavelength range for visible light, spanning from $300\,nm$ to $500\,nm$.

Infrared Wavelength Range

The general wavelength range for infrared radiation, spanning from $800\,nm$ to $1\,\mu m$.

Ultraviolet Wavelength Range

The general wavelength range for ultraviolet radiation, spanning from $300\,nm$ to $10\,nm$.

X-Rays Wavelength Range

The general wavelength range for X-rays, spanning from $0.01\,nm$ to $10\,nm$.

Photoelectric Effect

The ejection of electrons from a surface when struck by light, occurring only if each photon has energy above a minimum threshold frequency.

Work Function ($\text{E}_{\text{threshold}}$)

The minimum threshold energy a photon must possess to successfully eject an electron from an active metal surface.

Photoelectric Energy Conservation Equation

The equation $E = h \cdot v = \text{E}_{\text{threshold}} + K.E.$, stating that total photon energy equals threshold energy plus kinetic energy given to the ejected electron.

Wave-Particle Duality

The concept that both light and matter exhibit properties of waves (such as diffraction) and particles (such as quantized photons and momentum).

Davisson and Germer Experiment

An experiment demonstrating an electron diffraction pattern, proving that electrons (matter) exhibit wave-like properties.

De Broglie Theory

The postulate stating that matter, in addition to acting as a particle, exhibits wave properties.

Aufbau's Rule

The electron configuration rule stating that electrons fill orbitals from the lowest energy orbital to the highest energy orbital.

Hund's Rule

The electron configuration rule stating that in degenerate orbitals (such as $p$ and $d$ orbitals), electrons spread out by placing $1$ electron in each orbital before pairing up.

Pauli Exclusion Principle

The principle stating that no two electrons in an atom can have the same set of quantum numbers, restricting each orbital to a maximum of $2$ electrons with opposite spins.