At the end of this unit, you should be able to :
1. define matter. 2. define inertia. 3. define energy.
4. differentiate between potential and kinetic energy. 5. state and describe the law of conservation of mass. 6. state and describe the law of conservation of energy 7. state and describe the law of conservation of mass-energy.
8. identify the SI fundamental quantities and their units of measurement. 9. identify the major metric prefixes and their powers of 10.
10. differentiate between SI fundamental quantities and derived quantities. 11. differentiate between mass and weight.
12. differentiate between accuracy and precision.
13. identify the correct number of significant digits in a measurement.
14. correctly use the correct number of significant digits in solving problems.
15. measure length, mass, volume and temperature to the greatest number of significant. digits. 16. use the density equation to solve problems involving mass, volume and density.
17. become familiar with safety procedures in the chemistry laboratory. 18. convert units within the metric system.
Chemistry: Chapter 3 Objectives
1. Differentiate between heterogeneous and homogeneous materials and give examples of each kind of material.
2. Define phase and identify phases in different materials. 3. Define a solution in terms of a solute and solvent
4. When given an example of a solution, identify the solvent and solutes. 5. Define a substance as either a compound or an element.
6. Differentiate between inorganic and organic substances 7. Define “physical change” and “chemical change.”
8. When given an example of a change, identify the change as physical or chemical. 9. Define “physical property” and “chemical property.”
10. When given an example of a property, identify the property as physical or chemical. 11. Define “extensive property” and “intensive property.”
12. When given an example of a property, identify the property as intensive or extensive. 13. Tell the difference among thermal energy, heat, and temperature.
14. Describe the potential and kinetic energy in a chemical reaction. 15. Define “ endothermic” and “exothermic” reactions.
16. When given an example of a reaction, identify the reaction as endothermic or exothermic. 17. Diagram endothermic and exothermic reactions.
18. Define specific heat.
19. Define calorie, kilocalorie, Calorie, and Joule. 20. Convert between units of heat energy.
21. Calculate energy changes in terms of quantity of heat, mass, specific heat, and temperature change. Examples
Describe the contributions of Democritus and Aristotle to early models of matter.
1. Describe the atomic models (include experimental evidence) proposed by each of the following scientists
Dalton
Thomson Cathode Ray Tube
Rutherford Scattering Experiment
Bohr Hydrogen spectrum
1. When given the ratios of masses of elements of two samples, determine if the compounds are the same (definite proportions) or different (multiple proportions)
2. Calculate the number of protons, neutrons, and electrons in a given element from data given on the periodic table.
3. Compare and contrast protons, neutrons, and electrons in terms of mass, charge, and location. 4. Identify the Z and A numbers of atoms of a given element.
5. Calculate the number of protons, neutrons, and electrons in a given element from the nuclear symbol, e.g. 92
238
U
.6. Identify a given element by its atomic number.
7. Describe the continuous visible electromagnetic spectrum.
8. Given a picture of a wave, identify the wavelength and amplitude and describe the frequency.
9. Arrange the colors of the visible electromagnetic spectrum in order of increasing frequency, wavelength, and energy.
10. Describe how a given element may be identified by its atomic emission spectrum (either gas discharge tubes or flame tests.)
11. Explain the difference between atomic emission and atomic absorption spectra. 12. Explain why atomic spectra are considered the “fingerprints of atoms”.
13. Describe the lines on the atomic emission spectrum of an element in terms of the movement of electrons from one energy level to another.
14. Describe the difference between excited electrons and electrons in the ground state.
15. Calculate the atomic mass of an isotope as the sum of the protons and neutrons in the nucleus.
16. Calculate the atomic weight (average atomic mass) of an atom, given the atomic masses and the percent abundance of its isotopes.
MAAA+MBAB+.. . . 100
Chemistry Chapter 5 Objectives
At the end of this chapter, the student should be able to
1. relate the principal quantum number to the energy level of an electron. 2. calculate the maximum number of electrons possible in each principal energy
level.
3. describe each sublevel in terms of a. shape (s, p, and d only)
b. total number of electrons per sublevel c. number of possible orbitals
d. number of electrons per orbital.
4. use orbital notation to fill electrons into orbitals, sublevels, and principal energy levels.
5. identify elements which do not follow the diagonal rule for filling electrons, and write the electron configurations of those elements.
6. use the orbital notation of an atom to write the quantum number states of the atom:
a. principal quantum number, n, is equal to the principal energy level of the electron. b. the second quantum number, l, is the energy sublevel and may have values 0 to
n-1.
l=0 is an s-sublevel l=1is a p-sublevel l=2 is a d-sublevel l=3 is a f-sublevel
c. the third quantum number, m, is the orbital quantum number and may have values of –l through +l:
s m=0 m=-1
p m=0
m=+1
m=-2 m=-1 d m=0 m=+1 m=+2
m=-3 m=-2 m=-1
f m=0
m=+1 m=+2 m=+3
d. the fourth quantum number is the spin quantum number and may have the vaues +1/2 (clockwise) or -1/2 (counterclockwise.)
7. When given the four quantum numbers, identify the electron. 8. When given the electron, identify the four quantum numbers.
9. Use the periodic table or orbital notation to write electron configurations and abbreviated electron configurations for the elements.
10. Identify the s, p, d and f blocks on the periodic table
Ch 6. Periodic Table Objectives
1. Describe the contributions of Doberiener, Newlands, and Mendeleev to the development of the periodic table.
2. State the periodic law
3. Describe the contribution of Moseley to the development of the periodic law.
4. Relate the outer electron configuration of the elements to their position on the periodic table. 5. Identify the s,p,d, and f blocks of the periodic table.
6. Identify the metals, metalloids, and nonmetals based on their location on the periodic table. 7. Identify the properties of metals, metalloids, and nonmetals.
8. Locate the following families of elements on the periodic table:
Alkali metals Alkaline earth metals Chalcogens Halogens Noble gases Transition metals Inner transition elements
Lanthanoids Actinoids
Ch. 10: Periodic properties/trends objectives
1. Describe what is meant by a periodic property.
2. Define and describe the trends (horizontal and vertical) of the following properties of elements on the periodic table:
Atomic Radius Ionization energy Electronegativity Shielding effect Oxidation number Ionic Radius
Chemistry
Ch 6. Periodic Table Objectives
9. Describe the contributions of Doberiener, Newlands, and Mendeleev to the development of the periodic table.
10. State the periodic law
11. Describe the contribution of Moseley to the development of the periodic law.
12. Relate the outer electron configuration of the elements to their position on the periodic table. 13. Identify the s,p,d, and f blocks of the periodic table.
14. Identify the metals, metalloids, and nonmetals based on their location on the periodic table. 15. Identify the properties of metals, metalloids, and nonmetals.
16. Locate the following families of elements on the periodic table:
Alkali metals Alkaline earth metals Chalcogens Halogens Noble gases Transition metals Inner transition elements
Lanthanoids Actinoids
Ch. 10: Periodic properties/trends objectives
4. Describe what is meant by a periodic property.
5. Define and describe the trends (horizontal and vertical) of the following properties of elements on the periodic table:
Atomic Radius Ionization energy Electronegativity Shielding effect Oxidation number Ionic Radius
At the end of this chapter the student should be able to:
1. calculate the molar mass of a substance
a. gram atomic mass (elemental substances.) b. molecular mass ( compounds.)
c. gram formula mass (ionic compounds.) 2. define a mole as
a. a number of particles (6.02 X 1023particles.) b. a mass (molar mass.)
c. a volume of gases at STP (22.4L.)
3. convert among moles, particles, mass, and volumes. 4. determine the percent composition from
a. chemical formula. b. experimental data.
5. determine empirical formula from a. percent composition. b. experimental data.
