CHEMISTRY SEMESTER 1 UNIT OBJECTIVES 2016-2017
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For the semester exam you may use a 3x5 index card, both sides, hand written. It will be turned in with the test
Unit 1 Chemistry Chapter Objectives – Measurement and Calculations (pp 29 - 59)
Section 2.2: Units of Measurement
 What is “SI” and what are the standard units of measure for length, mass, time, and temperature?
 Explain why density, area, volume and velocity are called “derived” units.
 Memorize the SI prefixes, values, and abbreviations as follows:
milli (m) = .001 = 1/1000 = 1x10-3
centi (c) = .01 = 1/ 100 = 1x10-2
deci (d) = .1 = 1/10= 1x10-1
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Know how to use all conversion factors in dimensional analysis problems including:
micro () = .000001 = 1/1 x 106 = 1 x 10-6
nano (n) = .000000001 = 1/1x109 = 1 x 10-9
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deca (da) = 10x=1x101
hecto (h) = 100x=1x102
kilo (k) = 1000x=1x103
mega (M) = 1 000 000 x=1x106
giga (G) = 1 000 000 000 x1x109
Know how to use Dimensional Analysis (unit cancellation) to solve problems.
Memorize the density equation: D = m/v. Define each variable.
Solve density problems, including changing density units into appropriate units (mass = grams, volume = cm3 or
mL, density = grams/cm3 or g/mL).
Memorize and be able to use the conversion factor: 1 L = 1000 mL = 1000 cm3 = 1 dm3
Section 2.3: Using Scientific Measurements
 Define and distinguish between accuracy and precision
 Describe how significant figures are determined from scientific measurements.
 Determine the number of significant figures for any measurement.
 Round off numbers according to the simplified rules for rounding presented in class.
 Perform mathematical operations in appropriate sig figs and scientific notation.
Chemistry Unit 2 Objectives: MATTER & CHANGE
Section 1.1 - Chemistry Is a Physical Science
 Define chemistry
 List examples of branches of chemistry and know what each one studies
 Compare & contrast basic research, applied research, and technological development
Section 1.2 - Matter and Its Properties
 Differentiate between mass & weight
 Distinguish between the physical properties (intensive/extensive) and chemical properties of matter
 Know reactants and products of a chemical reaction
 Classify changes of matter as physical or chemical
 Explain the states of matter in terms of particle spacing and movement
 Know the classification structure of matter and be able to define each and list examples of each
 Distinguish between a mixture and a pure substance
Section 1.3 Elements
 Know the common elements that we use and be able to give both name & symbol (The first 36 elements along
w/ Sr-Ag-Sn-Sb-I-Cs-Ba-Au-Hg-Pb-Bi-Ra-U)
 Describe the arrangement of the periodic table along with group names
 List the characteristics that distinguish metals, nonmetals, and metalloids and know where they are found on
the periodic table
Section 2.1 – Scientific Method
 Describe the purpose of the scientific method
 List & describe the steps involved in the scientific method (observing- formulating-hypotheses-testingtheorizing-results)
 Distinguish between quantitative & qualitative
 Know difference between a law & theory
OBJECTIVES FOR UNIT 3 - ATOMS: THE BUILDING BLOCKS OF MATTER
Section 3.1: The Atom: From Philosophical Idea to Scientific Theory
 Know the five essential points of Dalton’s atomic theory
 Know and understand the law of conservation of mass, definite composition, & multiple proportions
Section 3.2: The Structure of the Atom
 Summarize the observed properties of cathode rays that led to the discovery of the electron
 Summarize the experiment conducted by Rutherford that led to the discovery of the nucleus.
 Describe the properties of protons, neutrons, and electrons
 Define atom & isotopes
 Describe the structure of an atom
Section 3.3: Counting Atoms
 Define atomic number and mass number and describe how they apply to isotopes and nuclides
 Determine the number of protons, neutrons, and electrons in a nuclide, given the identity of the nuclide
 Know difference between relative & average atomic mass
 Calculate the average atomic mass of an element given the relative abundance of each isotopes of the element
 Define a mole in terms of Avogadro’s number
 Define molar mass and be able to solve molar mass problems
 Solve all sorts of mole problems (using dimensional analysis)
Section 4.1: Development of a New Atomic Model
 Know how the ground state of an electron differs from the excited state.
 Be able to describe and know the limitations of the Bohr Model
Section 4.2: Quantum Model of the Atom
 Describe de Broglie’s role in the development of the model of the atom
 Compare and contrast the Bohr model and the quantum model of the atom
OBJECTIVES FOR UNIT 4 - THE NUCLEUS
Section 21.1: The Nucleus
 Describe how strong force attracts nucleons
 Predict the stability of a nucleus by considering factors such as nuclear size, binding energy, and the ratio of
neutrons to protons in the nucleus
 Explain why nuclear reactions occur.
Section 21.2: Radioactive Decay
 Describe the different types of radioactive decay and their effects on the nucleus.
 Know the particles of decay and their symbols (beta 0-1e, alpha 42He,
 positron 0+1e, proton 11H, neutron 10n, )
 Predict the particles given off in nuclear decay and be able to balance nuclear decay reactions
Section 21.4: Nuclear Fission & Nuclear Fusion
 Explain the difference between fission and fusion
OBJECTIVES FOR UNIT 5 – Electron Configuration & the Periodic Table
Section 4.1: Development of a New Atomic Model
 Know how the ground state of an electron differs from the excited state.
 Be able to describe and know the limitations of the Bohr Model
Section 4.2: Quantum Model of the Atom
 Describe de Broglie’s role in the development of the model of the atom
 Compare and contrast the Bohr model and the quantum model of the atom
Section 4.3: Electron Configurations
 Know the Aufbau principle and Hund’s rule.
 Memorize and be able to reproduce the “diagonal rule.”
 Describe the orientation of electrons in an atom using the following: orbital notation, electron configuration,
and shorthand notation.
 Define an octet of electrons and describe its importance to electron notations.
 Describe the noble-gas configuration and write it for any noble gas.
 Be able to use the periodic table to do a noble gas electron configuration.
Section 5.1 - History of the Periodic Table
 Explain why Mendeleev left “spaces” in his original periodic table.
 Describe how Mendeleev predicted the properties of elements that were unknown and undiscovered in his
time.
 Know the groups of elements added to the table after Mendeleev’s time.
 Define the periodic law.
Section 5.2 - Electron Configuration and the Periodic Table
 Identify the following from The Periodic Table:
alkali metals
alkaline-earth metals
actinide series
noble gases
lanthanide series
actinide series
transition elements
metalloids
halogens
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Give characteristics and examples of each of the above.
Define the term main-group elements.
Section 5.3 - Electron Configuration and Periodic Properties
 Define the terms group trend and periodic trend
 Describe the following terms:
atomic radius
ionization energy
electron affinity
ionic radius
electronegativity
 Identify the group and periodic trends relating to the above terms.
 Explain the terms cation and anion.
 Define the term valence electron. Describe the relationship between group numbers and the number of valence
electrons in the main-group elements.