Chemistry Chapters 7-11 Study Guide

Comprehensive vocabulary flashcards covering chemical bonding, molecular geometry, reaction types, nomenclature, and stoichiometry from Chapters 7 through 11.

Octet rule

The principle that atoms bond because they want a full outer shell of $8$ valence electrons.

Ionic bond

A bond formed by the transfer of electrons between a metal and a non-metal, resulting in a 1:1 ratio of 1 cation and 1 anion with a hard solid structure and high melting point.

Covalent bond

A bond formed by the pairing or sharing of electrons between two non-metals, generally characterized by weak forces, low melting points, and being poor conductors.

Metallic bond

Communal sharing of electrons (sea model) between two metals where electrons are delocalized and not focused on one atom.

Valence Bond Theory (VBT)

The theory that bonds are thought to form through the overlapping of orbitals, creating either sigma or pi bonds.

Sigma ($\sigma$) bond

A stronger bond located between the plane of the atoms.

Pi ($\pi$) bond

A bond located above or below the bond plane that is more stretched out; found in double and triple bonds.

Double bond

A bond consisting of one sigma ($\sigma$) bond and one pi ($\pi$) bond.

Triple bond

A bond consisting of one sigma ($\sigma$) bond and two pi ($\pi$) bonds.

VSEPR

Valence Shell Electron Pair Repulsion; a theory where electrons in the outer shell repel each other to give a molecule its 3D shape.

Molecular Orbital Theory (MOT)

A theory where new orbitals are made, classified as bonding or antibonding, to predict if a bond will form and its magnetic attraction.

Paramagnetism

A property predicted by Molecular Orbital Theory caused by lone electrons in new orbitals, resulting in magnetic attraction of molecules.

Sea model

The model for metallic bonding where electrons are delocalized, making metals malleable, ductile, and great conductors.

Alloys

A mixture of metals, such as stainless steel, bronze, or silver.

Cation

An atom that becomes positively charged by giving electrons away.

Anion

An atom that becomes negatively charged by adding an electron.

Formula units

Simplified ratios of the ions in an ionic compound.

Polar bonds

Bonds formed by the unequal sharing of electrons due to a difference in electronegativity between atoms, leading to partial charges ($\delta$).

Deca-

The numerical prefix used in naming binary covalent compounds representing the number $10$.

Ternary Acid naming (ate)

The rule where the polyatomic ion suffix '-ate' is changed to '-ic' for the acid name.

Ternary Acid naming (ite)

The rule where the polyatomic ion suffix '-ite' is changed to '-ous' for the acid name.

Catalyst

A substance, symbolized by $Pt$ or a triangle ($\Delta$) for heat, that speeds up a reaction without being consumed.

Synthesis

A reaction type where two or more reactants combine to form one product ($A + B \rightarrow AB$).

Combustion

A reaction where a hydrocarbon reacts with $O_2$ to produce $CO_2$ and $H_2O$.

Decomposition

A reaction type where a single reactant breaks down into two or more products ($AB \rightarrow A + B$).

Single replacement

A reaction where one element replaces another in a compound ($A + BC \rightarrow AC + B$); A must be more reactive than B.

Spectator ions

Ions that do not participate in the chemical reaction and are eliminated when writing a net ionic equation.

Mole

An SI unit used to measure the amount of something, equal to $6.072 \times 10^{25}$ (Avogadro).

Molar mass

The mass of one mole of a substance, calculated by adding up each element's mass in $g/mol$.

Empirical formula

The simplified ratio of the elements in a compound.

Molecular formula

The true ratio of elements in a compound, which is always a multiple of the empirical formula.

Limiting reactant

The reactant that is completely consumed in a reaction and determines the maximum amount of product that can be formed.

Excess reactant

The reactant that remains after a chemical reaction has stopped because the limiting reactant is used up.