General Chemistry: Quantum Numbers, Periodic Trends, Chemical Bonding, and VSEPR Theory

Comprehensive vocabulary flashcards covering quantum numbers, periodic table trends, chemical bonding types, formal charge, and VSEPR molecular shapes.

Principal Quantum Number ($n$)

The quantum number representing the main energy level within an atom, taking positive integer values ($n = 1, 2, 3, 4, \dots$).

Angular Momentum Quantum Number ($l$)

The quantum number that designates the shape of the sublevel, where $l$ is an integer satisfying $l \le n - 1$ (taking values from $0$ up to $n - 1$).

Sublevels ($s, p, d, f$)

The four sublevel shapes designated by values of the angular momentum quantum number: $s$ ($l = 0$), $p$ ($l = 1$), $d$ ($l = 2$), and $f$ ($l = 3$).

Magnetic Quantum Number ($m_l$)

The quantum number specifying the particular orbital within a sublevel, taking integer values ranging from $-l$ to $+l$.

Electron Spin Quantum Number ($m_s$)

The quantum number indicating the spin state of an electron, taking values of $+\frac{1}{2}$ or $-\frac{1}{2}$.

Electronegativity Trend

The periodic trend describing how strongly an atom pulls on electrons; Fluorine ($F$) has the highest electronegativity, and elements possess higher electronegativity the closer they are to Fluorine.

Atomic Radius Trend

The periodic trend where Helium ($He$) is the smallest atom and Francium ($Fr$) is the biggest atom; elements have smaller radii the closer they are to Helium.

Ionization Energy Trend

The periodic trend that increases as you move up and to the right on the periodic table; Helium ($He$) has the largest ionization energy and Francium ($Fr$) has the least.

Electron Affinity Trend

The periodic trend measuring electron attraction, where Fluorine ($F$) has the highest electron affinity.

Metals (Periodic Table Location)

Elements located on the left and middle sections of the periodic table.

Nonmetals (Periodic Table Location)

Elements located on the upper right section of the periodic table, plus Hydrogen.

Ionic Bond

A bond between a metal and a nonmetal in which the highly electronegative nonmetal rips the electron completely away from the metal, transferring electrons to create charged ions ($+$ and $-$).

Polar Covalent Bond

A bond between two different nonmetals where electrons are shared unequally (an uneven tug-of-war) because one nonmetal is more electronegative and pulls the shared electrons closer to itself.

Nonpolar Covalent Bond

A bond between two identical nonmetals (or Carbon + Hydrogen) where electrons are shared equally (a tied tug-of-war) because the atoms have identical electronegativity and pull with equal strength.

Bond Polarity Rule

The rule stating that bond polarity is determined by the difference in electronegativity between two atoms: the further apart two nonmetals are on the periodic table, the more polar the bond.

Formal Charge Formula

The formula defined as $\text{Formal Charge} = \text{Valence electrons} - (\text{Dots} + \text{Lines})$, where dots represent unshared electrons and lines represent covalent bonds.

Linear Geometry (VSEPR)

A molecular shape characterized by a bond angle of $180^\circ$, exemplified by $BeCl_2$, $CO_2$ ($O=C=O$), and $I_3^-$.

Trigonal Planar Geometry (VSEPR)

A molecular shape characterized by a bond angle of $120^\circ$, exemplified by molecules such as $BH_3$ and $COCl_2$.

Tetrahedral Geometry (VSEPR)

A molecular shape involving four electron groups ("Tetra = 4") with a bond angle of $109.5^\circ$, exemplified by methane ($CH_4$).

Trigonal Pyramidal Geometry (VSEPR)

A molecular shape characterized by a bond angle of $107^\circ$, exemplified by ammonia ($NH_3$).

Bent Geometry (VSEPR)

A molecular shape characterized by a bond angle of $< 120^\circ$, exemplified by molecules such as $SO_2$ and $H_2O$.