Inorganic Compound Nomenclature

• Inorganic analytical chemistry is the study of the composition, structure, and behavior of inorganic compounds.
• Quantitative analysis determines the amount of specific substances in a sample.

Naming Compounds

• Naming inorganic compounds involves a set of rules to clearly identify each substance.
• Ionic compounds are named by combining the cation (positive ion) name with the anion (negative ion) name.
• For cations with multiple possible charges, a Roman numeral indicates the charge (e.g., iron(II) chloride).
• Anions are named by adding "-ide" to the root of the element name (e.g., chloride for chlorine).
• Polyatomic ions have specific names that must be memorized (e.g., sulfate, nitrate, phosphate).
• Covalent compounds are named using prefixes to indicate the number of atoms of each element (e.g., carbon dioxide).
• Common prefixes include mono-, di-, tri-, tetra-, penta-, hexa-, and so on.
• Acids are named based on their anion.
• If the anion ends in "-ide," the acid is named hydro- + root + -ic acid (e.g., hydrochloric acid).
• If the anion ends in "-ate," the acid is named root + -ic acid (e.g., sulfuric acid).
• If the anion ends in "-ite," the acid is named root + -ous acid (e.g., nitrous acid).

Balancing Chemical Equations

• Balancing chemical equations ensures that the number of atoms for each element is the same on both sides of the equation.
• This is based on the law of conservation of mass, which states that matter cannot be created or destroyed.
• The process involves adjusting the coefficients (the numbers in front of the chemical formulas) to achieve balance.
• Start by balancing elements that appear in only one reactant and one product.
• Then, balance polyatomic ions as a unit if they appear unchanged on both sides.
• If hydrogen and oxygen are present, balance them last.
• Always double-check that the final equation is balanced.

Mixtures

• A mixture is a combination of two or more substances that are physically combined but not chemically bonded.
• Homogeneous mixtures have uniform composition throughout (e.g., saltwater).
• Heterogeneous mixtures have non-uniform composition (e.g., salad).
• Mixtures can be separated by physical means, such as filtration, evaporation, distillation, or chromatography.
• Filtration separates solids from liquids.
• Evaporation separates a soluble solid from a liquid by vaporizing the liquid.
• Distillation separates liquids with different boiling points.
• Chromatography separates substances based on their different affinities for a stationary and a mobile phase.

Properties of Matter

• Matter is anything that has mass and occupies space.
• Physical properties can be observed or measured without changing the substance's composition (e.g., color, density, melting point, boiling point).
• Chemical properties describe how a substance reacts with other substances (e.g., flammability, reactivity with acids).
• Intensive properties do not depend on the amount of substance (e.g., temperature, density).
• Extensive properties depend on the amount of substance (e.g., mass, volume).
• Density is mass per unit volume and is calculated as density = mass/volume.
• Changes of state are physical changes that occur when a substance changes from one form to another (e.g., solid to liquid, liquid to gas).
• These changes are melting, freezing, vaporization, condensation, sublimation, and deposition.

Types of Chemical Reactions

• Chemical reactions involve the rearrangement of atoms and molecules.
• Five common types of chemical reactions are synthesis, decomposition, single displacement, double displacement, and combustion.
• Synthesis reactions involve the combination of two or more substances to form a single product (A + B → AB).
• Decomposition reactions involve the breakdown of a single reactant into two or more products (AB → A + B).
• Single displacement reactions involve the replacement of one element in a compound by another element (A + BC → AC + B).
• Double displacement reactions involve the exchange of ions between two compounds (AB + CD → AD + CB).
• Combustion reactions involve the rapid reaction between a substance and oxygen, producing heat and light (e.g., CxHy + O2 → CO2 + H2O).
• Redox reactions involve the transfer of electrons between species.
• Oxidation is the loss of electrons, and reduction is the gain of electrons.
• The substance that loses electrons is oxidized and acts as the reducing agent.
• The substance that gains electrons is reduced and acts as the oxidizing agent.
• Precipitation reactions occur when two aqueous solutions are mixed, and an insoluble solid (precipitate) forms.
• Acid-base reactions involve the transfer of protons (H+) from an acid to a base.
• Acids are proton donors, and bases are proton acceptors.
• Neutralization is a specific type of acid-base reaction where an acid and a base react to form a salt and water.