Download Unit Description - Honors Chemistry

Honors Chemistry Review Sheet – Semester 1
Honors Chemistry/1617
You should be able to...
Chapters 1 and 3 – Scientific Method and Matter
 Distinguish among hypothesis, theory and scientific law using examples.
 Identify the common steps of scientific methods.
 Distinguish between qualitative and quantitative data.
 Distinguish between independent and dependent variables, controls and constants.
 Distinguish between matter and energy.
 Compare and contrast mass and weight.
 Describe matter using properties, including physical and chemical, intensive and extensive.
 Distinguish among elements, compounds, and mixtures.
 Distinguish between physical and chemical properties.
 Differentiate among the physical states of matter.
 Classify changes in matter as exothermic or endothermic.
 Define physical change and list several common physical changes.
 Define chemical change and list several indications that a chemical change has taken place.
 Apply the law of conservation of mass to chemical reactions.
 Contrast mixtures and substances.
 Classify mixtures as homogeneous or heterogeneous.
 List and describe several techniques used to separate mixtures.
Chapter 2: Data Analysis and Problem-solving
 Read a chemical formula for type of elements and number present
 Calculate density
 Find density, mass, volume, height, width and length, when given all but one of the values
 Distinguish between the accuracy and precision of a measurement
 Use significant figures in measurements and calculations
 Use metric prefixes to convert metric units
 Convert temperatures from Kelvin to Celsius and vice-versa
 Determine the uncertainty of a measurement
 Determine percent error
 Draw and interpret graphs
Chapter 11: Moles
 Define Avogadro’s number
 Perform conversions between moles and # particles
 Find molar masses of elements, using the periodic table
 Determine molar masses of compounds, given the chemical formula and using the periodic table
 Perform conversions between moles and molar mass of elements or compounds
 Perform conversions between molar mass and # particles
 Perform conversions involving the # atoms of an element in a compound
 Solve problems involving any combination of the above-listed conversions
 Determine percent composition of elements in a compound
 Determine empirical formula of a compound from the masses or percent composition of elements in a compound
 Determine molecular formula of a molecule from mass or percent composition and molecular molar mass
 Calculate solution concentrations in terms of mass percent and molarity
Chapters 4 and 5: Atomic Structure and part of Chapter 6: Periodic Table
Honors Chemistry/1617
You should be able to...
 Compare and contrast the evolution of atomic theories, including Democritus, Dalton, Thomson, Rutherford,
Bohr and quantum mechanics (4.1, 4.2, 5.2)
 Define and discuss the structure of an atom including the locations, relative masses, and charges of electrons,
neutrons and protons (4.3)
 Use the atomic number and mass number to find the number of protons, electrons, and neutrons in an atom (4.3)
(Quiz 8)
 Describe how the isotopes of an atom differ (4.3)
 Calculate the average atomic mass of an element from isotope data using weighted averages (4.3) (Bean Bag
Isotope lab quiz)
 Distinguish between nuclear and chemical reactions (notes)
 Describe and distinguish among the five types of nuclear radiation (4.4, notes)
 Write simple nuclear equations representing radioactive decay, fission and fusion (4.4) (Quiz 9)
 Define radioactive decay (4.4), nuclear fission, chain reaction, critical mass, nuclear fusion, nuclear bullets,
superheavy elements (Ch 25, notes)
 Describe the mathematical relationship among speed, wavelength, and frequency of electromagnetic radiation
(5.1)
 Calculate the frequency and wavelength of EMR, and the associated energy of a photon, using frequency and
Planck’s constant (5.1) (Quiz)
 Explain the quantum concept of EMR energy (5.1)
 Explain how an element can be identified by its spectral lines (5.1)
 Explain the origin of the atomic emission spectrum of an element, using Bohr’s hydrogen spectrum (5.1)
 Describe the quantum mechanical model of the atom (5.2)
 Describe Heisenberg’s Uncertainty Principle (5.2)
 Distinguish between an orbit and an orbital (5.2)
 Distinguish among principal energy level, energy sublevel, and atomic orbital; (5.2)
 Use the Aufbau Principle, the Pauli Exclusion Principle and Hund’s Rule to write the electron configurations and
orbital diagrams of the elements (5.3)
 Relate valence electrons to Lewis (electron dot) structures (5.3)
 Describe the ground-state arrangement of electrons in atoms of any element using orbital notation, electron
configuration, and Lewis structures (5.3)
 Identify electron configuration that contain excited electrons
 Use the periodic table to find the number of valence electrons in an atom (6.2)
 Solve problems using appropriate, logical approaches as well as scientific notation and significant figures
Nomenclature: Naming Ionic compounds and Writing formulas
You will be allowed to use the Ion page in order to write the formulas and names (work sheets)
The test is all multiple choice except Naming Ionic compounds and Writing formulas.
The final is 15% of your final grade.