General Chemistry
Course Features
Course Details
Course Overview
Acellus General Chemistry provides students with a basic introduction to chemistry. Students are introduced to various forms of matter. They learn about the basic components of the atom and electron orbitals. They will become familiar with the Periodic Table and learn how to use it to predict properties of specific elements. They will learn about chemical bonding, practice stoichiometry, and learn basic reactions. A brief introduction of organic chemistry is also included.
Acellus General Chemistry is taught by Dr. James Chapman.
Acellus General Chemistry is A-G Approved through the University of California.
Course Objectives & Student Learning Outcomes
Upon completion of Acellus General Chemistry, students will be able to: explain reasons for studying chemistry, characterize matter, and apply the scientific method; solve chemical equations that include SI units and prefixes; conversions between SI units for temperature; derived units for volume and density; scientific notation for addition, subtraction, multiplication, and division; unit conversion in dimensional analysis; data analysis; significant figures and rounding; and calculations using significant figures in addition, subtraction, multiplication, and division; apply the principles for states and properties of matter, physical versus chemical changes, elements versus compounds, and types of mixtures; and make connections between the organization of the atom, what makes atoms different, quantum theory as it relates to the atom, and electronic configuration. Students will also be able to apply principles of the modern periodic table, electronic configuration and periodicity, and periodic trends; relate valence electrons, ionic bonds and compounds, properties and formulas of ionic compounds, and names of ions and ionic compounds; and covalent bonds, single and multiple covalent bonds, the strength of covalent bonds, names of binary molecular compounds, naming acids, and Lewis Structures for covalent compounds and polyatomic ions; identify, compare, and contrast valence shell electron pair repulsion (VSEPR), electronegativity, and polarity; and apply principles of chemical reactions, balancing chemical equations, types of chemical reactions, and reactions in water. Students will be able to solve problems involving what a mole is, how to convert moles to particles and to mass, the mole ratios of compounds, percent composition calculations, and empirical and molecular formula calculations; solve problems involving chemical reactions in terms of stoichiometric calculations, including mole to mole, mole to mass, mass to mole, mass to mass, and percent yield; apply principles of gases in terms of behavior, units, and the kinetic-molecular theory, and in terms of Dalton's Law of Partial Pressures. Also covered are liquids, solids, and the intermolecular forces that determine the state of matter; and apply the laws that pertain to gases, including Boyle's, Charles's, and Gay-Lussac's laws, as well as the Combined Gas Law and the Ideal Gas Law. Finally, students will be able to solve problems that pertain to heterogeneous and homogeneous mixtures, as well as concentration as percent by mass, percent by volume, molarity, dilution of molar solutions, molality, and mole fractions; as well as solvation in ionic and molecular compounds, solubility, and colligative properties; apply the Arrhenius, Bronsted-Lowry, and Lewis Models, the strength of acids, weak acid ionization constants, the strength of bases, weak base ionization constant, hydrogen ions, ion product constant, pH and pOH, pH and H+ calculations, pOH and OH- calculations, pH and pOH calculations, and pH and pOH strong acids and bases; as well as neutralization reactions for acids and bases; and solve problems that pertain to hydrocarbons, including alkanes, drawing structures, straight-chain alkanes, and branched-chain alkanes.Scope and Sequence
Unit 1 – Introduction to Chemistry This unit discusses why we study chemistry, the characteristics of matter, the scientific method, and scientific notation. Also discussed are scientific notation in multiplication, division, addition, and subtraction, SI units and prefixes, and conversions between SI units for temperature. Additionally, this unit addresses derived units for volume and density, data analysis, significant figures and rounding, calculations using significant figures in addition, subtraction, multiplication, and division, and unit conversion in dimensional analysis. Unit 2 – Matter and The Periodic Table This unit discusses states and properties of matter, physical versus chemical changes, elements versus compounds, and types of mixtures. Separation methods for mixtures, the organization of the atom, what makes atoms different, radioactive decay, quantum theory as it relates to the atom, and electronic configuration are also addressed. This unit also delves into the modern periodic table, electronic configuration and periodicity, and periodic trends. Unit 3 – Chemical Bonding This unit discusses valence electrons, ionic bonds and compounds, properties and formulas of ionic compounds, and names of ions and ionic compounds. This unit also discusses covalent bonds, single and multiple covalent bonds, and the strength of covalent bonds. Unit 4 – Naming Compounds & Lewis Structures This unit covers the names of binary molecular compounds, naming acids, and Lewis Structures for covalent compounds and polyatomic ions. Unit 5 – Molecular Shapes & Chemical Equations This unit discusses valence shell electron pair repulsion (VSEPR), electronegativity, and polarity. This unit also covers chemical reactions, balancing chemical equations, types of chemical reactions, and reactions in water. Unit 6 – The Mole This unit discusses what a mole is, how to convert moles to particles and to mass, the mole ratios of compounds, calculations for molar mass of compounds, percent composition calculations, and empirical and molecular formula calculations. Following this unit students are presented with the Mid-term Review and Exam. Unit 7 – Stoichiometry This unit discusses chemical reactions in terms of stoichiometric calculations. The discussion includies mole to mole, mole to mass, mass to mole, mass to mass, and percent yield. Unit 8 – Solids, Liquids, and Gases This unit discusses gases in terms of behavior, units, and the kinetic-molecular theory, and in terms of Dalton's Law of Partial Pressures. Also covered are liquids, solids, and the intermolecular forces that determine the state of matter. Unit 9 – Gas Laws This unit covers the laws that pertain to gases, including Boyle's, Charles's, and Gay-Lussac's laws. Also covered are the Combined Gas Law and the Ideal Gas Law, including the Ideal Gas Law as it relates to m0lar mass and density. Unit 10 – Mixtures and Solutions This unit discusses heterogeneous and homogenous mixtures, as well as concentration as percent by mass, percent by volume, molarity, dilution of molar solutions, molality, and mole fractions. Also covered are solvation in ionic and molecular compounds, solubility, and colligative properties. Unit 11 – Acids and Bases This unit discusses the Arrhenius, Bronsted-Lowry, and Lewis Models, the strength of acids, weak acid ionization constants, the strength of bases, weak base ionization constant, hydrogen ions, ion product constant, pH and pOH, pH and H+ calculations, pOH and OH- calculations, pH and pOH calculations, and pH and pOH strong acids and bases. Further discussion covers neutralization reactions for acids and bases, as well as basic, acidic, and neutral salt solutions, and buffer solutions. Unit 12 – Organic Chemistry This unit discusses hydrocarbons, including alkanes, drawing structures, naming straight-chain alkanes, branched-chain alkanes, cyclic alkanes, structures from names, alkenes, alkynes, aromatics, and isomers. Also covered are substituted hydrocarbons in functional groups, halocarbons, alcohols, ethers, amines, aldehydes, ketones, carboxylic acid, and carboxylic acid-ester. Following this unit students are presented with the Final Review and Exam.
This course was developed by the International Academy of Science.
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Full Year 
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