Unit Objectives
Unit 1: Matter and Atomic Theory
Unit 2: Periodic Table and EMR
Unit 3: Bonding and Nomenclature
Unit 4: Chemical Reactions
Unit 5: Moles, Molar Mass, Percent Composition
Unit 6 Stoichiometry
Unit 7 Energy
Unit 8 Rates of Reactions and Equilibrium
Unit 9 Solutions, Acids, & Bases
Unit 10 Nuclear Chemistry and Gases
Unit 1: Matter and Atomic Theory
- Define matter and know the two requirements of matter
- Describe the three states of matter in terms of shape and volume
- Define chemical and physical properties and give examples of both
- Describe a change as physical or chemical
- Differentiate between an element/compound/molecule, pure substance/mixture, and homogeneous mixture/heterogeneous mixture.
- Be able to identify an element by symbol or name using the periodic table
- Describe the subatomic particles that makeup the atom (charge, mass, function)
- Define mass number and atomic number and how they relate to the subatomic particles.
- Calculate the number of subatomic particles, atomic number, and mass number of an element when given the elements name and either the number of neutrons or the mass number
- Define an isotope and an ion, be able to write isotopes of elements using both hyphen notation and nuclear symbol
Unit 2: Periodic Table and EMR
- Define ions (cations and anions) and identify periodic trends of common elemental ions
- Locate the following on the periodic table: alkali metals, alkaline earth metals, transition metals, lanthanides, actinides, halogens, noble gases.
- Classify an element as either metal, non-metal, or metalloid based on location on the periodic table
- Define photons and describe the wave-particle nature of light
- Describe emission spectrums and flame tests in terms of subatomic particles and energy being emitted/absorbed
- Identify periodic trends concerning the following: atomic radius, ionization energy
- Using the following two equations: E=hv and c=vλ calculate the energy(E), frequency(v) , or wavelength(λ) when given sufficient information
Unit 3: Bonding and Nomenclature
- Create stable compounds of anions and cations by balancing charges
- Define valence electrons; count the number of valence electrons based on position in the periodic table
- Define a bond and bond energy. Differentiate between ionic bonding and covalent bonding.
- Explain why elements act in a way to achieve noble gas configuration.
- Draw Lewis Dot Structures for elements and compounds using the octet rule. Differentiate between a bonding pair of electrons and lone pair electrons both in words and in Lewis Dot Structures. Draw Lewis Structures for ionic and covalent compounds
- Define and compare a single, double, and triple bond.
- Use prefixes when naming covalent compounds to communicate how many of each atom there are.
- When given the chemical name write the accurate formula that corresponds to that name for ionic compounds and covalent compounds.
- When given the formula write the correct chemical name that corresponds to that formula for ionic and covalent compounds.
Unit 4: Chemical Reactions
- Define the following types of reactions: Synthesis, Decomposition, Single Replacement, Double Replacement, and Combustion. Be able to identify each of these types of reactions
- Balance a skeleton equation by using coefficients to uphold the law of conservation of mass.
- Predict the products of a chemical reaction when given the reactants. After creating neutral compounds and checking for diatomic elements balance the equation.
- Write a chemical equation using chemical symbols, plus signs, and an arrow.
- Convert a word equation problem into a chemical reaction. After creating neutral compounds and checking for diatomic elements balance the equation.
Unit 5: Moles, Molar Mass, Percent Composition
- Calculate the molar mass of a compound using the average atomic masses from the periodic table for each atom that makes up the compound.
- Convert moles to grams using the calculated molar mass of a compound.
- Convert grams to moles using the calculated molar mass of a compound .
- Determine the empirical and molecular formula of a compound when given percent composition and molar mass.
- Calculate percent composition of each element in a compound when given the molecular formula.
- Define a mole as a counting unit in chemistry used to convert large numbers of particles into easier numbers to work with.
- Convert back and forth between moles and particles.
- Perform two step conversions to go from grams to particles and vice versa.
Unit 6 Stoichiometry
- Define a mole ratio. Balance an equation to find the mole ratio.
- Use the mole ratio, and molar masses to convert a mass of one reactant to a theoretical yield of a product.
- Convert from moles of one reactant/product to another reactant/product.
- Convert moles of one reactant/ product to grams of another reactant/product.
- Convert grams of one reactant/product to grams of another reactant/product.
- Determine the limiting reagent in a chemical reaction by comparing the amount in moles of each reactant.
- Calculate the percent yield of a chemical reaction using the theoretical yield and actual yield.
Unit 7 Energy
- Define Energy in chemistry. Compare kinetic and potential energy.
- Describe the law of conservation of energy and apply it to real-world situations.
- Differentiate between temperature and heat as each pertain to energy.
- Describe the flow of energy in terms of a system and the surrounding. Properly identify a reaction as exothermic or endothermic based on this flow of energy.
- Calculate the change in energy of a system as well as the specific heat capacity of different chemical compounds.
- Complete temperature and energy conversions.
- Use a phase change diagram to determine what the state of matter is and how to calculate the change in energy.
- Define the different phase changes and identify them as endothermic or exothermic
Unit 8 Rates of Reactions and Equilibrium
- Explain why not all collisions of molecules result in chemical reactions with reference to the 2 requirements of the collision theory(enough speed and correct orientation).
- Explain how the following four factors affect reaction rate in terms of the collision theory: temperature, concentration, particle size/surface area, addition of a catalyst.
- Use LeChatelier’s principle to predict how a system in equilibrium would respond to the following stresses: addition/removal of reactant/product, increase/decrease in temperature, increase/decrease in pressure.
Unit 9 Solutions, Acids, & Bases
- Define molarity and solutions.
- Calculate the molarity of a solution by dividing the moles of the solute by the liters of the solvent.
- Perform dilution calculations using the formula M1V1=M2V2.
- Calculate, pH, pOH, [H=], and [OH-] when given pH, pOH, [H=], or [OH-].
- Determine whether a solution is acidic, basic, or neutral based on the pH scale.
- Determine the conjugate acid and conjugate base when looking at a chemical equation.
- Perform a neutralization/titration reaction to determine the concentration of an acid or base.
Unit 10 Nuclear Chemistry and Gases
- Compare and contrast the three different types of radiation: Alpha, Beta, and Gamma.
- Predict the products of nuclear decay reactions and identify the type of nuclear decay.
- Calculate the half life, how much of a product remains, and how many half-lives have gone by when given sufficient information.
- Determine the relationship between volume and pressure of a gas. Calculate the new pressure or volume of a gas if the other changes.
- Determine the relationship between pressure and temperature of a gas. Calculate the new pressure or temperature of a gas if the other changes.
- Determine the relationship between pressure and moles of a gas. Calculate the new pressure or moles of a gas if the other changes.
- Use PV=nRT to calculate pressure, volume, temperature, or amount in moles of an ideal gas.