HS Chem

1

Chemistry Final Exam Topics

-The majority of the exam will cover second semester topics (Ch. 10, 11, 12), but understanding of the following first semester topics will be necessary (Ch. 8, 9). Ionic Compounds (Ch. 8)

Define a chemical bond Explain how and why chemical bonds are formed Describe the formation of anions and cations Describe the formation of ionic bonds Account for the physical properties of ionic compounds (ex: lattice structure, melting

point, boiling point, electrical conductivity, brittleness, etc.) Write the chemical formulae for ionic compounds given the IUPAC name Write the IUPAC name for chemicals given the chemical formulae Describe metallic bonds Explain the physical properties of metals in terms of metallic bonds (ex: structure,

melting point, boiling point, electrical conductivity, brittleness, etc.)

Covalent Compounds (Ch. 9 )

Covalent Bonds Identifying molecules containing covalent bonds

Chemical Reactions (Ch. 10) Vocabulary: Here is a list of some of the vocabulary words covered this unit. o Chemical reaction o Reactant o Product o Word equation o Skeleton equation o Chemical equation o Coefficient o Subscript o Balancing o Synthesis reaction o Combustion reaction o Decomposition reaction o Single replacement reaction

o Double replacement reaction

o Precipitate

o Neutralization o Solute o Solvent o Aqueous solution o Complete ionic equation o Net ionic equation o Spectator ion o Soluble o Insoluble o Dissolve o Dissociate o Hydrocarbon o Irreversible

HS Chem

2

Concepts:

Reactions and Equations Recognize evidence of chemical change Represent chemical reactions with equations

Word Skeleton Balanced/Chemical Complete ionic Net ionic Overall (with double displacement reactions that produce gas)

Outline the characteristics of each type of equation Predict the products of chemical reactions given the reactants Identify the state of matter for each species in a reaction Write chemical formulas from IUPAC names and vice versa

Classifying Chemical Reactions Classify chemical reactions

Synthesis Decomposition Single Replacement (use activity series) Double Replacement (use solubility table)

Precipitate reaction (solid is produced from two aqueous solutions) Neutralization reaction (acid + base water + salt) Gas-forming reaction (common gases: HCN, H2S, and CO2 [look for an

acid reacting with a carbonate which will give two reactions a double displacement followed by a decomposition])

Combustion (O2 is a reactant and energy is a product) Identify the characteristics of different classes of chemical reactions

Reactions in Aqueous Solutions Describe aqueous solutions

Use terms like dissolve and dissociate Write complete ionic and net ionic equations for chemical reactions in aqueous solutions

Predict whether a reaction in aqueous solutions will produce a precipitate, water, or a gas

Extra Practice: Nomenclature (names to formulas and formulas to names) Chemical Equations and Reaction Types

HS Chem

3

The Mole (Ch. 11)

Vocabulary: Here is a list of some of the vocabulary words covered this unit. o Mole o Avogadros number o Particles / Representative

particles o Atoms o Ions o Molecules o Formula units o Conversion factor o Molar mass o Gram atomic mass o Gram formula mass o Gram molecular mass

o Percent Composition o Empirical Formula o Molecular Formula

Concepts:

Measuring Matter Describe how a mole is used in chemistry Relate a mole to common counting units (ex: pair, dozen) Convert moles to number of representative particles and number of representative

particles to moles Recall: representative particles = atoms/ions/molecules/formula units

HS Chem

4

Mass and the Mole Relate the mass of an atom to the mass of a mole of atoms Calculate the number of moles in a given mass of an element and the mass of a given

number of moles of an element Calculate the number of moles of an element when given the number of atoms of the element

Calculate the number of atoms of an element when given the number of moles of the element

Moles of Compounds

Recognize the mole relationships shown by a chemical formula Calculate the molar mass of a compound

Recall: molar mass = gram atomic mass/gram molecular mass/gram formula mass

Particles

atoms

ions

molecules

formula units

HS Chem

5

Calculate the number of moles of a compound from a given mass of the compound, and the mass of a compound from a given number of moles of the compound

Determine the number of atoms or ions in a mass of a compound

Empirical and Molecular Formulas Explain what is meant by the precent composition of a compound Determine the empirical and molecular formulas for a compound from mass percent

and actual mass data

Stoichiometry (Ch. 12)

Vocabulary: Here is a list of some of the vocabulary words covered this unit. o Stoichiometry o Mole Ratio o Limiting Reactant o Excess Reactant o Theoretical Yield o Actual or Experimental Yield o Percent Yield

Molar Mass

Gram atomic mass

Gram molecular mass

Gram formula mass

HS Chem

6

Concepts: Stoichiometry

Identify the quantitative relationships in a balanced chemical equation. Determine the mole ratios from a balanced chemical equation.

Stoichiometric Calculations

Explain the sequence of steps used in solving stoichiometric problems. Use the steps to solve stoichiometric problems

Limiting Reactants

Identify the limiting reactant in a chemical equation. Identify the excess reactant and calculate the amount remaining after the reaction is complete.

Calculate the mass of a product when the amounts of more than one reactant are given.

Percent Yield

Calculate the theoretical yield of a chemical reaction from given data. Determine the percent yield for a chemical reaction.