High School Chemistry

Inquiry, Reflection & Social Implication

Scientific Inquiry
Scientific Reflection and Social Implications

Forms of Energy

Potential Energy: Three forms of potential energy are gravitational, elastic, and chemical.
Chemical Potential energy: It is the result of electrostatic attraction between atoms.
Molecules in Motion
Molecular Entropy: With increase in temperature, the average kinetic energy and the entropy of the molecules in a sample increases.
Breaking Chemical Bonds
Electron Movement
Nuclear Stability: Nuclear stability is related to a decrease in potential energy when the nucleus forms from protons and neutrons.
Half Life

Energy Transfer And Conservation

Conservation of Energy: When energy is transferred from one system to another, the quantity of energy before transfer equals the quantity of energy after transfer.
Hess’s Law: For chemical reactions where the state and amounts of reactants and products are known, the amount of energy transferred will be the same regardless of the chemical pathway. This relationship is called Hess’s law.
Energy Transfer
Enthalpy
Heating Impacts
Bond Energy
Endothermic and Exothermic Reactions: Chemical interactions either release energy to the environment (exothermic) or absorb energy from the environment (endothermic).
Enthalpy and Entropy
Mass Defect: Nuclear reactions involve energy changes many times the magnitude of chemical changes. In chemical reactions matter is conserved, but in nuclear reactions a small loss in mass (mass defect) will account for the tremendous release of energy. The energy released in nuclear reactions can be calculated from the mass defect using E = mc2.

Properties of Matter

Kinetic Molecular Theory
Elements, Compounds, and Mixtures: Elements are a class of substances composed of a single kind of atom. Compounds are composed of two or more different elements chemically combined. Mixtures are composed of two or more different elements
Molecular and Empirical Formulas
Nomenclature
Properties of Substances
Conductivity
Solids: Solids can be classified as metallic, ionic, covalent, or network covalent,different types of solids have different properties that depend on the particles and forces found in the solid.
Molecular Polarity
Ideal Gas Law
Moles: The mole is the standard unit for counting atomic and molecular particles in terms of common mass units.
Solutions
Atomic Structure
Historical evidence for structure of atom
Electron Configuration: Electrons are arranged in main energy levels with sub levels that specify particular shapes and geometry.
Quantum Theory
Periodic Table: In the periodic table, elements are arranged in order of increasing number of protons (called the atomic number).
Electron Energy Levels: The rows in the periodic table represent the main electron energy levels of the atom. Within each main energy level are sub levels that represent an orbital shape and orientation.
Neutral Atoms: A neutral atom of any element will contain the same number of protons and electrons.
Ions:Ions are charged particles with an unequal number of protons and electrons.
Isotopes: Isotopes are atoms of the same element with different numbers of neutrons and essentially the same chemical and physical properties.
Average Atomic Mass: The atomic mass listed on the periodic table is an average mass.

Changes in Matter

Conservation of Matter
When substances undergo changes of state, neither atoms nor molecules themselves are changed in structure. Mass is conserved when substances undergo changes of state.
Rates of Reactions
Chemical Changes: Chemical changes can occur when two substances, elements, or compounds interact and produce one or more different substances whose physical and chemical properties are different from the interacting substances.
Balancing Equations
Types of Chemical equations
Equilibrium: Most chemical reactions reach a state of dynamic equilibrium where the rates of the forward and reverse reactions are equal.
Phase Change/Diagrams:Changes of state require a transfer of energy.
Changes of State
Chemical Bonds — Trends: An atom’s electron configuration, particularly of the outermost electrons, determines how the atom can interact with other atoms.
Chemical Bonds
Reduction/Oxidation Reactions
Acids and Bases
Acids and bases are important classes of chemicals that are recognized by easily observed properties in the laboratory. Acids and bases will neutralize each other.
Brønsted-Lowry
Reactions that involve proton transfer are known as acid/base reactions
Carbon Chemistry
The chemistry of carbon is important. Carbon atoms can bond to one another in chains, rings, and branching networks to form a variety of structures, including synthetic polymers, oils, and the large molecules essential to life.