Chemistry Exam 2 Study Guide - Electronic Structure & Periodic Trends

Vocabulary flashcards covering electronic structure, quantum numbers, periodic trends, chemical bonding, orbital filling rules, and polyatomic ions.

Orbital

A region where electrons are most likely to be found; each orbital can hold up to $2$ electrons.

Electronic Spin

The magnetic field produced by an electron.

Principal Quantum Number ($n$)

Quantum number that determines the energy level and size of an orbital ($n = 1, 2, 3, 4, \dots$) and can never equal $0$.

Angular Momentum Quantum Number ($l$)

Quantum number that determines orbital shape ($l = 0 \rightarrow s$ sphere, $l = 1 \rightarrow p$ dumbbell, $l = 2 \rightarrow d$ cloverleaf, $l = 3 \rightarrow f$ complex), equal to $n - 1$.

Magnetic Quantum Number ($m_l$)

Quantum number that determines orbital orientation in space, depending on $l$ with integer values from $-l$ to $+l$.

Spin Quantum Number ($m_s$)

Quantum number representing the direction of electron spin, with values of $+\frac{1}{2}$ or $-\frac{1}{2}$.

Sublevel $s$

A subshell containing $1$ orbital that holds a maximum of $2$ electrons.

Sublevel $p$

A subshell containing $3$ orbitals that holds a maximum of $6$ electrons.

Sublevel $d$

A subshell containing $5$ orbitals that holds a maximum of $10$ electrons.

Sublevel $f$

A subshell containing $7$ orbitals that holds a maximum of $14$ electrons.

Ionic Bond

A chemical bond formed between a metal and a non-metal, typically using Roman numerals to indicate variable charges and no Greek prefixes.

Covalent Bond

A chemical bond formed between two non-metals, using Greek prefixes to denote the number of atoms present.

Atomic Radius

The size of an atom, which gets bigger going down and to the left on the periodic table.

Ionization Energy

The energy required to remove an electron from an atom; increases going up and to the right on the periodic table.

Effective Nuclear Charge ($Z_{\text{eff}}$)

How strongly an electron actually feels the pull of the nucleus, increasing as the number of protons increases.

Shielding

The process where core electrons shield valence electrons from the nucleus, essentially blocking nuclear attraction.

Isoelectronic Ions

Ions that have the exact same number of electrons; among them, species with more protons are smaller due to stronger nuclear pull.

Aufbau Principle

Rule stating that electrons fill lower energy orbitals first before occupying higher energy ones.

Pauli Exclusion Principle

Rule stating that an orbital can hold a maximum of $2$ electrons, and they must have opposite spins.

Hund's Rule

Rule stating that when multiple orbitals of equal energy are available, electrons spread out singly with parallel spins before pairing up.

Ammonium

A positively charged polyatomic cation with the chemical formula $\text{NH}_4^+$.

Acetate

A singly charged anion with the chemical formula $\text{CH}_3\text{CO}_2^-$.

Cyanide

A singly charged anion with the chemical formula $\text{CN}^-$.

Hydroxide

A singly charged anion with the chemical formula $\text{OH}^-$.

Permanganate

A singly charged anion with the chemical formula $\text{MnO}_4^-$.

Nitrate

A singly charged anion with the chemical formula $\text{NO}_3^-$.

Nitrite

A singly charged anion with the chemical formula $\text{NO}_2^-$.

Carbonate

A doubly charged anion with the chemical formula $\text{CO}_3^{2-}$.

Sulfate

A doubly charged anion with the chemical formula $\text{SO}_4^{2-}$.

Sulfite

A doubly charged anion with the chemical formula $\text{SO}_3^{2-}$.

Phosphate

A triply charged anion with the chemical formula $\text{PO}_4^{3-}$.

Chromate

A doubly charged anion with the chemical formula $\text{CrO}_4^{2-}$.

Dichromate

A doubly charged anion with the chemical formula $\text{Cr}_2\text{O}_7^{2-}$.

Hydrogen Carbonate

A singly charged anion, also known as bicarbonate, with the chemical formula $\text{HCO}_3^-$.

Hydrogen Sulfate

A singly charged anion, also known as bisulfate, with the chemical formula $\text{HSO}_4^-$.

Hypochlorite

A singly charged anion with the chemical formula $\text{ClO}^-$.

Chlorite

A singly charged anion with the chemical formula $\text{ClO}_2^-$.

Chlorate

A singly charged anion with the chemical formula $\text{ClO}_3^-$.

Perchlorate

A singly charged anion with the chemical formula $\text{ClO}_4^-$.

Thiosulfate

A doubly charged anion with the chemical formula $\text{S}_2\text{O}_3^{2-}$.