Chapter 6 Memorize CHM 1100 Review

A set of practice flashcards covering formulas, constants, and atomic structure rules from Chapter 6.

$$c = \lambda \nu$$

The formula representing the speed of light as the product of wavelength and frequency.

$$E = h \nu$$

The formula used to calculate the energy of a photon using frequency.

$$E = \frac{hc}{\lambda}$$

The formula used to calculate the energy of a photon using wavelength.

$$E_n = \frac{-2.18 \times 10^{-18}}{n^2}$$

The formula for the energy of an electron at a specific level (n) in a hydrogen atom.

$$\Delta E = E_f - E_i$$

The formula for the change in energy, calculated as final energy minus initial energy.

$$c$$

The speed of light constant, which is $3.00 \times 10^8\,\text{m/s}$.

$$h$$

Planck's constant, which is $6.63 \times 10^{-34}\,\text{J}\cdot\text{s}$.

Up transition

Electron movement that results in absorption and a positive energy change ($+\Delta E$).

Down transition

Electron movement that results in emission and a negative energy change ($-\Delta E$).

Wavelength for emitted light

Calculated using the formula $\lambda = \frac{hc}{\Delta E}$.

ROYGBIV

The order of colors in the visible spectrum: Red → Orange → Yellow → Green → Blue → Indigo → Violet

Wavelength and frequency relationship

These properties are opposites, described as $\alpha \uparrow \Rightarrow v \downarrow \downarrow$.

Frequency and energy relationship

These properties move together, described as $v \uparrow \Rightarrow E \uparrow$.

Red light characteristics

LONG wavelength, LOW frequency, and LOW energy.

Violet light characteristics

SHORT wavelength, HIGH frequency, and HIGH energy.

Electromagnetic spectrum order

Radio $\\rightarrow$ Microwave $\\rightarrow$ Infrared $\\rightarrow$ Visible $\\rightarrow$ UV $\\rightarrow$ X-ray $\\rightarrow$ Gamma.

RMIVUXG

A mnemonic used for the electromagnetic spectrum: Radio, Microwave, Infrared, Visible, UV, X-ray, Gamma.

Gamma radiation trend

Moving toward gamma results in energy increasing ($\uparrow$), frequency increasing ($\uparrow$), and wavelength decreasing ($\downarrow$).

$$l = 0$$

The angular momentum quantum number assigned to the s subshell.

$$l = 1$$

The angular momentum quantum number assigned to the p subshell.

$$l = 2$$

The angular momentum quantum number assigned to the d subshell.

$$l = 3$$

The angular momentum quantum number assigned to the f subshell.

$$m_l$$

The magnetic quantum number, consisting of integers from $-1$ through $+1$ (as noted for p subshells).

$$m_s$$

The spin quantum number, which is either $+$ or $-$.

$$27 + 1$$

The formula given to calculate the number of orbitals in a subshell.

Subshell orbitals (s)

The s subshell contains 1 orbital.

Subshell orbitals (p)

The p subshell contains 3 orbitals.

Subshell orbitals (d)

The d subshell contains 5 orbitals.

Subshell orbitals (f)

The f subshell contains 7 orbitals.

Electron capacity (s)

The s subshell has a capacity of 2 electrons.

Electron capacity (p)

The p subshell has a capacity of 6 electrons.

Electron capacity (d)

The d subshell has a capacity of 10 electrons.

Electron capacity (f)

The f subshell has a capacity of 14 electrons.

Filling order

The sequence for electron filling: $1s\ 2s\ 2p\ 3s\ 3p\ 4s\ 3d\ 4p$.

Hund's rule

The requirement to fill orbitals singly before pairing electrons.

Valence electrons

The electrons located in the highest $n$ for main-group atoms.

Cation

A positive ($+$) ion created by the loss of electrons.

Anion

A negative ($-$) ion created by the gain of electrons.

Noble gas shorthand

A condensed electron configuration using the previous noble gas in brackets.

Chromium exception

The specialized electron configuration represented as $[Ar]\ 3d^5 4s^1$.