Atomic Structure Review Guide

Practice flashcards covering subatomic particles, the Bohr and Schrodinger models, quantum numbers, and electron orbital characteristics based on the provided lecture review guide.

Proton

A subatomic particle with a mass of $1\,amu$ and a positive electric charge.

Neutron

A subatomic particle with a mass of $1\,amu$ and a neutral electric charge.

Electron

A subatomic particle with a mass of approximately $0\,amu$ and a negative electric charge.

Principal quantum number (n)

Represents the orbital number, energy level of the electron, or the distance from the nucleus.

Emission

The process where electrons fall to lower energy levels and release photons of energy.

Absorption

The process where electrons absorb photons and move to higher energy levels.

Ground state

The state or shell of an atom that is closest to the nucleus.

Excited state

Any state or shell other than the ground state, which contains more energy.

Photon

A packet of energy released or emitted when an electron drops to a lower energy level.

Double slit experiment

An experiment proving wave-particle duality, showing that electrons behave as both particles and waves.

Schrodinger equation

An equation that predicts where a particle should be or the likelihood of its position around the nucleus.

Ground state energy ($E_1$)

The energy level for hydrogen at $n=1$, which is $-13.60\,eV$.

Spin quantum number

A quantum number indicating the direction of spin, having $2$ possible values: $+\frac{1}{2}$ and $-\frac{1}{2}$.

S orbital

A sphere-shaped orbital with $1$ orbital per subshell that holds a total of $2$ electrons.

P orbital

A figure-eight shaped orbital with $3$ orbitals per subshell that hold a total of $6$ electrons.

D orbital

Descriptions include a four leaf clover-ish shape, listed as $D=5$ with $4$ orbitals per subshell and a total of $8$ electrons.

F orbital

A complex-shaped orbital with $7$ orbitals per subshell that hold a total of $14$ electrons.

Angular quantum number (I)

The quantum number that determines the shape of an orbital.

Magnetic quantum number ($M_\ell$)

The quantum number that determines the orientation of an orbital in space.

Nuclear Model Problems

Fails to explain atomic instability (electrons spiraling into the nucleus) and the constant emission of energy (line spectra).

Speed of light (C)

A constant value defined in the notes as $3 \times 10^8$.

Planck's Constant (H)

A constant value listed in the review guide as $4.14 \times 10^{15}$.

Meter to Nanometer conversion

A conversion factor listed in the notes as $1\,\text{meter} = 10^{-9}\,\text{nanometers (nm)}$.