Unit Objectives
Unit 1 –Measurement and Matter
-Convert numbers from standard form to scientific notation and vice versa
-Identify the number of significant figures in a number using significant figure rules
-Round answers to addition/subtraction and multiplication/division problems correctly using significant figure rules
- Convert measurements using the commonly used prefixes of the metric system
-Calculate density using the equation d=m/v
-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.
Unit 2: Elements, Atoms, Ions, and Nuclear
-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
-Classify an element as either metal, non-metal, or metalloid based on location on the periodic table
-Locate the following on the periodic table: alkali metals, alkaline earth metals, transition metals, lanthanides, actinides, halogens, noble gases.
-Define an isotope, be able to write isotopes of elements using both hyphen notation and nuclear symbol
-Calculate the average atomic mass of an unknown element using the mass and mass percent of the isotopes and identify the unknown element. (Honors only)
-Count and calculate the number of atoms in a compound when given a chemical symbol
-Define ions (cations and anions) and identify periodic trends of common elemental ions
-Create stable compounds of anions and cations by balancing charges
-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
Unit 3: EMR, Orbitals, and Periodic Trends
-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
- Describe the Bohr model of an atom, how it was correct, how it was incorrect
- Define an orbital (a highly probable location about a nucleus where an electron may be found), define quantized (only certain values are allowed), define electromagnetic radiation (energy that exhibits wavelike behavior as it travels through space)
-Distinguish between orbitals(s,p,d,f) and orbital levels(1,2,3,4…). Discuss the shape of each orbital and how many electrons it takes to fill each orbital. Rank the orbitals in terms of energy
-State the symbol for each quantum number, define each quantum number, and determine location of an element on the periodic table based on the quantum number
-Define valence electrons; count the number of valence electrons based on position in the periodic table
-Identify periodic trends concerning the following: atomic radius, ionization energy
-Define the Pauli exclusion principle (an orbital can hold a maximum of two electrons and those two electrons must have opposite spins), Hund’s rule(orbitals of equal energy are occupied by one electron before any is occupied by a second electron), and Aufbau principle(Electrons occupies the lowest energy orbital that can receive it)
-Express elements in electron configuration and noble gas configuration. Identify elements based on their electron configurations
- Show the orbital filling notation for elements
-Using the following two equations: E=hv and c=vλ calculate the energy(E), frequency(v) , or wavelength(λ) when given sufficient information
Unit 4: Bonding, LDS, and VSEPR
- Define a bond and bond energy. Differentiate between ionic bonding, covalent bonding, and polar covalent bonding.
- Explain the relationship between electronegativity and bond polarity. Determine the type of bond by calculating the difference in polarity.
- Define a dipole moment and how it relates to bonding and the structure of a molecule.
-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 molecules with multiple bonds (double, triple).
-Compare the energy and length of a single, double, and triple bond.
-Define resonance and be able to draw resonance structures for the appropriate molecules.
-Define the VSEPR model and utilize it to predict the structure and geometry of a molecule and determine the polarity.
Unit 5: Types of 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. Include state of matter abbreviations in the chemical equation.
Unit 6 - Nomenclature, Molar Mass, Empirical & Molecular
-Balance charges in an ionic compound to make a neutral compound.
-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.
-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 with correct amount of significant figures.
-Convert grams to moles using the calculated molar mass of a compound with correct amount of significant figures.
- 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.
Unit 7 - Stoichiometry
-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.
- 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.
-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 8 - 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.
-Calulate the change in energy of a system as well as the specific heat capacity of different chemical compounds.
-Use Hess’s Law to calculate the change in enthalpy.
-Define entropy and use it to apply the second law of thermodynamics to real world situations.
Unit 9 - Reaction Rates
- 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.
- Calculate the equilibrium constant (Keq) for a chemical equation using the concentrations of reactants and products.
- Determine whether reactants or products are favored in a chemical equation by examining the value of the equilibrium constant.
Unit 10 - 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 11 - Gases
-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.
Unit 1 –Measurement and Matter
-Convert numbers from standard form to scientific notation and vice versa
-Identify the number of significant figures in a number using significant figure rules
-Round answers to addition/subtraction and multiplication/division problems correctly using significant figure rules
- Convert measurements using the commonly used prefixes of the metric system
-Calculate density using the equation d=m/v
-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.
Unit 2: Elements, Atoms, Ions, and Nuclear
-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
-Classify an element as either metal, non-metal, or metalloid based on location on the periodic table
-Locate the following on the periodic table: alkali metals, alkaline earth metals, transition metals, lanthanides, actinides, halogens, noble gases.
-Define an isotope, be able to write isotopes of elements using both hyphen notation and nuclear symbol
-Calculate the average atomic mass of an unknown element using the mass and mass percent of the isotopes and identify the unknown element. (Honors only)
-Count and calculate the number of atoms in a compound when given a chemical symbol
-Define ions (cations and anions) and identify periodic trends of common elemental ions
-Create stable compounds of anions and cations by balancing charges
-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
Unit 3: EMR, Orbitals, and Periodic Trends
-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
- Describe the Bohr model of an atom, how it was correct, how it was incorrect
- Define an orbital (a highly probable location about a nucleus where an electron may be found), define quantized (only certain values are allowed), define electromagnetic radiation (energy that exhibits wavelike behavior as it travels through space)
-Distinguish between orbitals(s,p,d,f) and orbital levels(1,2,3,4…). Discuss the shape of each orbital and how many electrons it takes to fill each orbital. Rank the orbitals in terms of energy
-State the symbol for each quantum number, define each quantum number, and determine location of an element on the periodic table based on the quantum number
-Define valence electrons; count the number of valence electrons based on position in the periodic table
-Identify periodic trends concerning the following: atomic radius, ionization energy
-Define the Pauli exclusion principle (an orbital can hold a maximum of two electrons and those two electrons must have opposite spins), Hund’s rule(orbitals of equal energy are occupied by one electron before any is occupied by a second electron), and Aufbau principle(Electrons occupies the lowest energy orbital that can receive it)
-Express elements in electron configuration and noble gas configuration. Identify elements based on their electron configurations
- Show the orbital filling notation for elements
-Using the following two equations: E=hv and c=vλ calculate the energy(E), frequency(v) , or wavelength(λ) when given sufficient information
Unit 4: Bonding, LDS, and VSEPR
- Define a bond and bond energy. Differentiate between ionic bonding, covalent bonding, and polar covalent bonding.
- Explain the relationship between electronegativity and bond polarity. Determine the type of bond by calculating the difference in polarity.
- Define a dipole moment and how it relates to bonding and the structure of a molecule.
-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 molecules with multiple bonds (double, triple).
-Compare the energy and length of a single, double, and triple bond.
-Define resonance and be able to draw resonance structures for the appropriate molecules.
-Define the VSEPR model and utilize it to predict the structure and geometry of a molecule and determine the polarity.
Unit 5: Types of 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. Include state of matter abbreviations in the chemical equation.
Unit 6 - Nomenclature, Molar Mass, Empirical & Molecular
-Balance charges in an ionic compound to make a neutral compound.
-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.
-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 with correct amount of significant figures.
-Convert grams to moles using the calculated molar mass of a compound with correct amount of significant figures.
- 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.
Unit 7 - Stoichiometry
-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.
- 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.
-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 8 - 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.
-Calulate the change in energy of a system as well as the specific heat capacity of different chemical compounds.
-Use Hess’s Law to calculate the change in enthalpy.
-Define entropy and use it to apply the second law of thermodynamics to real world situations.
Unit 9 - Reaction Rates
- 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.
- Calculate the equilibrium constant (Keq) for a chemical equation using the concentrations of reactants and products.
- Determine whether reactants or products are favored in a chemical equation by examining the value of the equilibrium constant.
Unit 10 - 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 11 - Gases
-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.