Chemistry Limiting Reactants and Reactions Quiz

Matter, Chemical Trends and Chemical Bonding

• Bond Types: Ionic bonds form between metals and nonmetals, involving electron transfer. Covalent bonds form between nonmetals, involving electron sharing.
• Naming Compounds (Ionic and Covalent): Ionic compounds are named by naming the metal first, then the nonmetal with -ide. Covalent compounds use prefixes to indicate the number of atoms.
• Atomic Radius: Atomic radius increases down a group and decreases across a period. This is due to increasing electron shells and the increasing effective nuclear charge, respectively.
• Bond Polarity: Bond polarity depends on the difference in electronegativity between atoms. A difference of 1.7 or greater indicates an ionic bond; a difference of less than 0.4 indicates a nonpolar covalent bond; and a difference between 0.4 and 1.7 indicates a polar covalent bond.
• Molecule Polarity: Molecules with polar bonds can be polar or nonpolar, depending on their shape. A polar molecule has a net dipole moment.
• Polarity and Properties: Polar substances tend to have higher boiling points due to stronger intermolecular forces. Solubility follows the "like dissolves like" rule.

Chemical Reactions

• Reaction Types: Synthesis reactions combine two or more reactants to form one product. Decomposition reactions break down a compound into two or more products. Single displacement reactions involve one element replacing another in a compound. Double displacement reactions involve the exchange of ions between two compounds. Combustion reactions involve a substance reacting with oxygen to produce heat, light, CO2, and water. Neutralization reactions involve an acid and a base reacting to form a salt and water.
• Predicting Products: Follow the rules of reaction types to predict products.
• Reactivity Series: A list of elements ranked by their ability to displace each other in compounds.

Quantities in Chemical Reactions

• Molar Mass: The mass of one mole of a substance (grams/mole).
• Moles: The amount of a substance containing Avogadro's number of particles.
• Mole Ratios: The ratio of moles of reactants and products in a balanced chemical equation.
• Empirical Formulas: Empirical formula gives the simplest whole number ratio of elements in a compound.
• Molecular Formulas: The actual number of atoms of each element in a molecule; it is a multiple of the empirical formula.
• Limiting Reactant: The reactant that is completely used up in a reaction, determining how much product can form.
• Theoretical Yield: The maximum amount of product that can be formed from a given amount of limiting reactant.
• Percent Yield: The actual yield divided by the theoretical yield, multiplied by 100%.

Solutions and Solubility

• Concentration: The amount of solute in a given amount of solution.
• Dilution of a Solution: The process of adding solvent to a solution to decrease its concentration.
• Acids and Bases: Acids release H+ ions, bases release OH- ions. pH measures acidity/basicity.
• Neutralization Reactions: These reactions occur when acids and bases react to form water and a salt.
• Dissociation and Ions Formed: Ionic compounds separate into their constituent ions when dissolved in water, which strong acids/bases dissociate completely or weakly.

Gases and Atmospheric Chemistry

• Boyle's Law: At constant temperature, the pressure and volume of a gas are inversely proportional (P1V1 = P2V2).
• Charles' Law: At constant pressure, the volume and temperature of a gas are directly proportional (V1/T1 = V2/T2).
• Gay-Lussac's Law: At constant volume, the pressure and temperature of a gas are directly proportional (P1/T1 = P2/T2).
• Avogadro's Law: At constant pressure and temperature, the volume of a gas is directly proportional to the number of moles (V1/n1 = V2/n2).
• Kelvin Temperature: A temperature scale that starts at absolute zero. To convert, use T (K) = T(°C) + 273.15.
• Ideal Gas Law: PV = nRT.

Other Important Concepts

• Intermolecular Forces: Forces between molecules, including London dispersion forces, dipole-dipole forces, and hydrogen bonding. These determine physical properties like boiling point and solubility.
• Lewis Diagrams and Structures: Visual representations of the valence electrons in molecules, helping to predict molecular shapes
• Solubility Curves: Graphs showing the relationship between solubility and temperature for various substances.
• VSEPR Theory: Valence Shell Electron Pair Repulsion Theory, predicts molecular geometry based on electron pair repulsion.