Chemistry

Introduction to Chemistry

Dimensional Analysis

Atomic Structure

Electron Configurations

Periodic Trends

Bonding

Naming and Formula Writing

Mole

Chemical Reactions

Stoichiometry

Thermochemistry

States of Matter

Gas Laws

Acids, Bases, Solutions

1.1

Matter, Properties

1.2

Measurements

2.1

Dimensional Analysis - 1 and 2 Step Conversions

3.1

History of Atomic Structure

3.2

Atomic Structure

3.3

Ions

3.4

Atomic Mass

4.1

Intro to Electron Configurations

4.2

Electron Configurations and Orbital Notations

4.3

Noble Gas Abbreviations and Valence Electrons

4.4

Quantum Numbers

5.1

History of the Periodic Table

5.2

Trend: Atomic Size

5.3

Trend: Ionization Energy

5.4

Trend: Ionic Size and Electronegativity

6.1

Bonding Basics

6.2

Ionic Bonding

6.3

Covalent Bonding

6.4

Molecular Geometry

6.5

Polarity

7.1

Basic - Properties of Ionic and Covalent Compounds

7.2

Name to Formula (ionic)

7.3

Formula to Name (ionic)

7.4

Naming Acids

7.5

Naming and Formula Writing for Molecular Compounds

8.1

History and Particle Conversions

8.2

Molar Mass - 1 Step Conversions

8.3

Molar Mass - 2 Step Conversions

8.4

Volume Conversions

8.5

Percent Composition

8.6

Empirical Formulas

8.7

Molecular Formulas

9.1

Introduction to Word Equations and Formula Equations

9.2

Balancing Chemical Equations

9.3

Putting It All Together

9.4

Predicting Products - Synthesis and Decomposition

9.5

Predicting Products - Single Replacement

9.6

Predicting Products - Double Replacement

10.1

Mole-Mole Calculations

10.2

Mass-Mass Calculations

10.3

Volume and Particle Calculations

10.4

Limiting Reactants

10.5

Excess Reactants

10.6

Percent Yield

11.1

Introduction to Thermochemistry

11.2

Calorimetry

11.3

Thermochemical Equations

11.4

Limiting Reactants with Thermal Equations

11.5

Heating Curves

11.6

Hess' Law

12.1

KMT - Gases

12.2

KMT - Liquids

12.3

KMT - Solids

12.4

Phase Diagrams

13.1

Introduction to Gas Laws

13.2

Boyle's and Charles's Gas Laws

13.3

Gay-Lussac's and Combined Gas Laws

13.4

Ideal Gas Law

13.5

Dalton vs. Graham's Gas Laws and Real vs. Ideal Gas Laws

14.1

Introductions to Solutions

14.2

Molarity

14.3

Acids and Bases Properties

14.4

Acid-Base Calculations

14.5

Titrations

1.1.a

I can define the states of matter and compare and contrast their properties.

1.1.b

I can classify materials as elements, compounds, or mixtures, stating the evidence for classification.

1.1.c

I can describe several techniques for the separation of mixtures.

1.1.d

I can distinguish between physical and chemical properties / changes.

1.1.e

I can define melting point, boiling point, and solubility.

1.2.a

I can identify and define fundamental and derived SI Units.

1.2.b

I can convert any number from decimal to scientific notation, and vice versa.

1.2.c

I can use metric prefixes to define different sized metric units.

1.2.d

I can convert units in the SI and English systems.

1.2.e

I can define accuracy and precision.

1.2.f

I can determine the number of significant figures in a measurement and calculation.

1.2.g

I can define and calculate density.

2.1.a

I can use the appropriate conversion factors to modify base units.

2.1.b

I can identify the units used in the SI system for length, mass, and volume.

3.1.a

I can explain the contributions of various scientists to atomic theory.

3.1.b

I can explain the observations and interpret results from the Gold Foil and Cathode Ray Tube experiments.

3.2.a

I can find the atomic mass, atomic number, and symbols of elements off the Periodic Table.

3.2.b

I can calculate the number of neutrons in a particular atom.

3.2.c

I can differentiate the properties for isotopes of a particular element.

3.3.a

I can describe how anions and cations are formed.

3.3.b

I can give the resulting charge for an ion from the number of protons and electrons.

3.3.c

I can show the appropriate abbreviations for ions with mass number, atomic number, and charge.

3.4.a

I can calculate the atomic mass when provided with percent abundances and atomic masses of isotopes.

3.4.b

I can compare the relative abundance of isotopes for a particular element.

4.1.a

I can explain the organization of electrons within an atom.

4.1.b

I can describe what an energy level, sublevel, and atomic orbital is.

4.1.c

I can draw the shape of each sublevel.

4.1.d

I can predict how many electrons can be held in each level, sublevel, or orbital.

4.2.a

I can write electron configurations in the proper long-form notation.

4.2.b

I can write orbital notations for elements in the proper notation.

4.2.c

I can identify elements from their electron configuration or orbital notation.

4.3.a

I can write electron configurations for elements and monatomic ions.

4.3.b

I can write noble gas abbreviations using previous electron configuration objectives.

4.3.c

I can classify elements based on their outermost electron configuration.

4.3.d

I can obtain the amount of valence electrons from an electron configuration.

4.4.a

I can identify the four quantum numbers by names and symbols.

4.4.b

I can write quantum numbers in order to describe an electron’s position in an atom.

4.4.c

I can determine which electron is being identified by a set of quantum numbers.

5.1.a

I can describe how the modern Periodic Table is arranged.

5.1.b

I can explain basic similarities and differences among groups and periods on the Periodic Table.

5.1.c

I can locate and label common groups on the periodic table.

5.1.d

I can locate and list properties of metals and nonmetals.

5.1.e

I can describe what a metalloid is.

5.2.a

I can explain how atomic radius is found.

5.2.b

I can explain the trend for atomic radius across periods and down groups.

5.2.c

I can explain what shielding is, and describe the role it plays in atomic radius.

5.3.a

I can explain what ionization energy is.

5.3.b

I can describe the ionization energy trend from the periodic table.

5.3.c

I can explain why it requires more energy to remove each subsequent electron after the first.

5.4.a

I can explain the periodic trend for ionic size and electronegativity.

5.4.b

I can compare the size of cations to the size of anions.

5.4.c

I can provide explanations for each of these trends.

6.1.a

I can explain how ionic and covalent bonding occurs.

6.1.b

I can write Lewis dot diagrams for the representative elements.

6.1.c

I can determine the number of valence electrons for a particular element.

6.2.a

I can write formulas for ionic compounds.

6.2.b

I can explain what an empirical formula is.

6.2.c

I can describe the properties of ionic compounds.

6.2.d

I can model the formation of an ionic compound using Lewis dot diagrams.

6.3.a

I can write structural formulas and dot formulas for covalently bonded molecules.

6.3.b

I can identify shared and unshared electrons.

6.3.c

I can explain the difference between single, double, and triple bonds - and write them using structural formulas / dot formulas.

6.4.a

I can explain Valence Shell Electron Pair Repulsion Theory (VSPERT).

6.4.b

I can use structural formulas to describe the molecular geometry of molecules.

6.4.c

I can identify the correct geometric name for the shape of the molecule.

6.4.d

I can identify approximate bond angles for molecules.

6.5.a

I can define the term polarity.

6.5.b

I can explain why certain atoms have more attraction for electrons.

6.5.c

I can identify molecules as either polar or nonpolar based on their symmetry.

6.5.d

I can identify which geometries will generally be polar molecules.

7.1.a

I can list differences between ionic and covalently bonded compounds.

7.1.b

I can identify polyatomic and monatomic ions and name them correctly.

7.2.a

I can write chemical formulas for ionic compounds.

7.2.b

I can explain the meaning of the Roman Numeral when in a chemical name.

7.3.a

I can write the chemical names for ionic compounds.

7.3.b

I can write the chemical name when given the chemical formula.

7.3.c

I can determine the Roman Numeral on a transition metal.

7.4.a

I can write the chemical names of acids given their chemical formula.

7.4.b

I can write the chemical formulas for acids given their chemical name.

7.5.a

I can write chemical names and formulas for molecules.

8.1.a

I can identify key scientists in the development of the mole.

8.1.b

I can use dimensional analysis to calculate how many atoms, molecules or formula units in one mole of that substance.

8.1.c

I can use correct significant figures and units in these calculations.

8.2.a

I can calculate the molar mass of a substance.

8.2.b

I can use molar mass to calculate the mass of a substance given, then the number of moles and vice versa.

8.3.a

I can perform two-step conversions using molar mass and representative particles (atoms, molecules, and formula units).

8.4.a

I can calculate the volume of a gas at STP.

8.4.b

I can perform two step volume conversions.

8.5.a

I can calculate percent composition for various compounds.

8.6.a

I can calculate the empirical formulas for various compounds given their percent composition.

8.7.a

I can calculate molecular formulas for various compounds, given their empirical formula.

9.1.a

I can identify and write formulas for the diatomic elements.

9.1.b

I can write a formula equation given the word equation for a chemical reaction.

9.2.a

I can explain the Law of Conservation of Atoms.

9.2.b

I can balance equations using the “tally method.”

9.3.a

I can write balanced formula equations from word equations.

9.4.a

I can identify synthesis and decomposition reactions.

9.4.b

I can use patterns to predict the products of synthesis and decomposition reactions.

9.5.a

I can identify single replacement reactions.

9.5.b

I can predict whether or not a single replacement reaction will occur.

9.6.a

I can identify double replacement and combustion reactions.

9.6.b

I can use patterns to predict the products of double replacement and combustion reactions.

9.6.c

I can predict the products in words for double replacement reactions.

9.6.d

I can predict the products and balance combustion reactions.

10.1.a

I can calculate the number of moles of a substance that can be produced or consumed using the mole ratio.

10.1.b

I can describe the ways in which balanced equations can be interpreted.

10.1.c

I can review the basics of how to balance equations.

10.2.a

I can calculate the mass of a substance used or produced during a chemical reaction.

10.3.a

I can calculate the volume or number of particles used or produced during a chemical reaction.

10.4.a

I can identify the limiting and excess reactants.

10.4.b

I can use stoichiometric calculations as evidence to support the identification of limiting and excess reactants.

10.5.a

I can calculate how much of the excess reactant reacts once the limiting reactant is completely used up.

10.5.b

I can calculate how much excess reactant remains after the reaction is complete.

10.6.a

I can calculate the percent yield of a reaction.

11.1.a

I can explain what thermochemistry is.

11.1.b

I can list different types of energy.

11.1.c

I can explain what happens to particle motion when heat energy is added.

11.1.d

I can convert between units of calories (cal), joules (J), and kilojoules (kJ).

11.2.a

I can describe what a calorimeter is and its function.

11.2.b

I can explain what temperature change is dependent on.

11.2.c

11.3.a

I can define what a thermochemical equation is and use its information to calculate the energy used or produced in a chemical reaction.

11.3.b

I can explain what the deltaH of a reaction is and how it can be found.

11.4.a

I can use thermochemical equations to calculate limiting reactant.

11.5.a

I can explain what occurs on each point of a heating curve.

11.5.b

I can calculate the total energy required for water to go through phase changes.

11.6.a

I can add, multiply, divide, or reverse chemical equations.

11.6.b

I can calculate enthalpy changes for an overall reaction using Hess’ Law.

12.1.a

I can describe basic principles of the kinetic theory of gases.

12.1.b

I can explain where pressure comes from and what affects it.

12.1.c

I can convert in between units of pressure.

12.1.d

I can explain what will happen mathematically to the average kinetic energy if temperature changes.

12.2.a

I can explain the properties of liquids according to the kinetic theory.

12.2.b

I can relate a kinetic energy diagram to the process of evaporation.

12.2.c

I can describe the equilibrium process.

12.2.d

I can describe vapor pressure and how it is affected by temperature and nature of the liquid.

12.2.e

I can explain the relationship between boiling point and vapor pressure.

12.2.f

I can predict a way to boil a liquid without changing the temperature of the liquid.

12.3.a

I can describe the properties of solids according to the Kinetic Theory.

12.3.b

I can explain the differences and similarities between ionic and molecular solids.

12.4.a

I can draw a phase diagram and label each state of matter, changes of state, and triple point.

12.4.b

I can identify at what temperature or pressure a substance will change state.

12.4.c

I can infer which phase of a substance is the most dense.

13.1.a

I can explain the factors that affect gas pressure.

13.1.b

I can describe real-world experiences and how they relate to gas pressure, temperature, and volume.

13.1.c

I can predict the behavior of a gas by changing one of its variables.

13.2.a

I can explain the effect on gas properties using Boyles’ and Charles’ laws.

13.2.b

I can calculate an unknown pressure, temperature, or volume by solving algebraically.

13.3.a

I can explain the effect on gas properties using Gay-Lussac’s Law and the Combined Gas Law.

13.3.b

I can calculate an unknown pressure, temperature, or volume by solving algebraically.

13.4.a

I can explain what an ideal gas is.

13.4.b

I can calculate an unknown pressure, temperature, volume, or amount of gas using the ideal gas law equation.

13.5.a

I can describe Dalton’s law of partial pressures and calculate Ptotal or a partial pressure.

13.5.b

I can explain Graham’s law of effusion and calculate the rate at which gases effuse.

13.5.c

I can explain what is meant by the term “real” vs. “ideal” gases.

14.1.a

I can explain the differences between the three different types of solutions.

14.1.b

I can describe how to make a supersaturated solution.

14.1.c

I can describe how to increase the rate of dissolving.

14.2.a

I can define molarity in terms of its mathematical formula.

14.2.b

I can calculate moles, liters, or molarity of a given solution.

14.2.c

I can explain how to make a solution.

14.3.a

I can define an acid and base according to the Arrhenius definition.

14.3.b

I can review the correct way to write the names and formulas for acids and bases.

14.3.c

I can describe and list properties that pertain to acids and bases.

14.4.a

I can explain the correlation to the strength of acids and bases to pH and pOH scale.

14.4.b

I can calculate pH, pOH, [H+], and [OH-].

14.5.a

I can explain what a neutralization reaction is.

14.5.b

I can write the corresponding formulas in neutralization reactions.

14.5.c