Honor Chemistry

Categories: Chemistry
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About Course

This course is a more accelerated version of the standard-level course, and topics are covered in greater depth. After an introduction to measurement and matter, students learn about the development of atomic theory, how matter is organized on the Periodic Table, ionic and covalent bonding, liquids and solids, and chemical reactions. Then, the course draws on mathematics to study stoichiometry, gases, thermochemistry, kinetics, equilibrium, rate of reaction, and acids and bases.

Course Content

Unit 1. introduction to Chemistry
in this unit the student will be able to: • Know the difference between a theory and a law and be able to give examples. • Understand the difference between random and systematic errors. • Be able to convert between Celsius and Kelvin. • Know and understand the nature of absolute zero. • Know the difference between and be able to identify physical and chemical changes. • Know the difference between and be able to identify pure substances (elements and • compounds) and mixtures (heterogeneous and homogeneous). • Be able to count significant figures. • Understand the difference between accuracy and precision. • Know how to take measurements to the appropriate number of significant figures. • Be able to add, subtract, multiply, and divide using significant figures. • Know how to calculate density. • Be able to convert numbers to scientific notation. • Be able to perform unit conversions between units with the following prefixes: mega, kilo, deci, centi, milli, micro, nano. • Know the basic characteristics of solids, liquids, and gases and how we can convert from • one phase to another. Know the terms that describe these phase changes. • Understand how to separate mixtures using distillation and filtration. • Know that electrolysis is one means available for separating compounds into their constituent elements

  • The Scientific Method, Law, and Theory.
  • Temperature Conversions
  • Physical and Chemical Changes and Properties
  • Matter Pure Substance and Mixtures
  • Significant Figures
  • Density Calculations
  • Dimensional Analysis
  • State of Matter
  • Separations Techniques

Unit 2. Atomic Theory
In this unit, the student will learn and be able to: • History of the atom: Democritus, John Dalton, J.J. Thompson, and Ernest Rutherford • Be able to calculate protons, neutrons, and electrons. • Know what ions are and how they differ from atoms. • Know the definition of an isotope and be able to identify isotopes. • Know the definition of isoelectronic and be able to identify species that are isoelectronic. • Know the terms mass number, atomic number, and atomic mass. • Be able to calculate atomic mass given the abundances of isotopes. • Know the electromagnetic spectrum. • Know the relationship between energy, frequency, and wavelength. • Be able to explain how we get line spectra. • Know which transitions release which frequency of light in the hydrogen atom. • Understand the Bohr model. Electrons are quantized, move in fixed orbits around nucleus, can be excited by absorbing energy, release energy as they relax. • Know that matter has wavelike properties, Louis de Broglie. • Heisenberg’s Uncertainty Principle. • Know the features of the quantum mechanical model of the electron: electrons quantized, Heisenberg, electrons are waves, orbitals, energy levels (with sublevels) but no orbits. • Know shapes of s and p orbitals. • Know number and type of each orbital, how many electrons they hold. • Be able to write full and abbreviated electron configurations. • Be able to draw orbital diagrams. • Understand and be able to apply Aufbau, Pauli Exclusion Principle, and Hund’s Rule. • Be able to calculate the number of unpaired electrons. • Be able to determine the number of core and valence electrons. • Be able to write electron configurations for simple ions. • Be able to recognize and compare isoelectronic species. • Know where the s, p, d, and f blocks are on the Periodic Table. • Understand why certain transition metals exhibit color and be able to predict • whether a particular transition metal ion will be colored. • Understand how excited state electron configurations differ from ground state • electron configurations.

Unit 3. The Periodic Table
In this unit the student will learn and be able to: • Understand the contributions that Mendeleev made to the development of the periodic table. • Know definitions and significance of groups and periods and be able to name the special groups (e.g. noble gases). • Be able to calculate number of valence electrons. • Know definitions and trends of ionization energy, atomic radius, and electronegativity. • Understand the concept of electron affinity. • Know how ionization energy and atomic radius are affected when an atom ionizes. • Know the diatomic elements. • Given a group of atoms or ions, be able to compare ionization energy, atomic radius, and electronegativity, including for isoelectronic species. • Know trends in reactivity for alkali metals, alkaline earth metals, and halogens. • Know the common ions that form. Understand that transition metals and Sn and Pb can form more than one ion. • Given a chart of ionization energies, be able to determine key facts about unknown elements, including number of valence electrons and group. • Know the octet rule and understand its importance in chemistry. • Be able to explain the trends using your knowledge of what is happening at the atomic level. • Know properties of metals and nonmetals and where to find each on the Periodic Table. • Know that metals lose electrons to form positive ions while nonmetals do the opposite. • Know the definitions of an anion and a cation. • Know the definitions of endothermic and exothermic.

Unit 4. Chemical Compounds and Nomenclature
in this unit, the student will learn and be able to: ● Differentiate between the forces between different substances versus the forces within a substance. ● Explain what is meant by the statement, “Bonding is a spectrum.” ● Write a sentence to summarize the connections between chemical bonds, chemical reactions, and compounds. ● Explain why most atoms form chemical bonds and why some atoms don’t. ● Explain the difference between what a chemical formula tells you about an ionic versus a covalent compound. ● Create a chart to distinguish covalent bonds from ionic bonds. ● Create a chart to distinguish the properties of covalent compounds from the properties of ionic compounds. ● Be able to explain what a chemical formula tells you about a compound and predict properties of the compound based on the bonds that hold it together. ● Be able to identify a bond or a compound as ionic or covalent based on a picture, description, difference in electronegativity, for example. ● Be able to use an element’s location on the periodic table to predict its oxidation number and bonding tendencies. ● List the number of atoms of each element in a compound. ● Explain the connection between electronegativity and the formation of an ionic bond. ● Use an example of an ionic compound to explain the “rule of zero charge”. ● Differentiate between binary ionic compounds, compounds with polyatomic ions, and binary molecular compounds. ● Explain why it is necessary to include a Roman numeral when naming an ionic compound with a transition metal. ● Give an example of a common compound and how the properties of the elements that make it up are different from that of the compound itself. ● Be able to illustrate the formation of ionic bonds using Lewis structures. ● Be able to apply nomenclature rules to determine the chemical formula and the name of an ionic ● compound, including those with polyatomic ions and/or transition metals. ● Draw Lewis structures to represent ionic and covalent compounds. ● Name and write the chemical formulas for ionic compounds, including those with polyatomic ions and transition metals.

Unit 5. Bonding
in this lesson the student will be able to: • Be able to draw Lewis structures. • Be able to calculate regions of electron density for covalent compounds. • Be able to determine geometries of molecules that have up to four regions of electron density. • Know the approximate bond angle for molecules with up to four regions of electron density. • Predict the effect of lone pairs on the bond angle. • Be able to calculate the total number of valence electrons in a molecule. • Be able to determine the polarity of a molecule and direction of the dipole. • Understand the concept of electronegativity. • Understand the tenets of Valence Shell Electron Pair Repulsion Theory (VSEPR). • Understand the concept of resonance and be able to draw resonance structures. • Understand the difference between intramolecular and intermolecular bonding. • Know the three types of intermolecular forces for molecular covalent substances: • hydrogen bonding, dipole-dipole attractions, and dispersion forces. Be able to identify which • forces apply for a given molecule. • Know what factor affects the strength of dispersion forces. • Be able to compare the strength of different types of intermolecular forces. • Understand the relationship between intermolecular forces and boiling point. • Understand the meaning of the terms endothermic and exothermic. • Be able to use the Maxwell-Boltzmann kinetic energy distribution curve to explain evaporation. • Know how a change in temperature affects the shape of the Maxwell-Boltzmann curve as well as the rate of evaporation. • Be able to use your knowledge of IMFs to compare relative escape energies for a • series of substances at a given temperature.