At the Conclusion of This Unit, Students Will Be Able To

UNIT 2 OBJECTIVES

Unit 2 includes chapters 3 and 4 from the text.

At the conclusion of this unit, students will be able to:

Describe the historical progression of the atomic theory (AT).

Explain that science exists in a historical context.

Relate the development of the AT to its historical context.

Describe individuals and their contributions to the AT.

State the four ideas of Dalton’s AT.

Describe, in some technical detail, Thomson’s work with CRT’s.

Describe, in some technical detail, Millikan’s oil drop experiment.

Describe, in some technical detail, Rutherford’s gold foil experiment.

Describe the various models of the atom.

Describe similarities and differences of isotopes.

Determine atomic #, mass #, and particles in assigned isotopes.

Determine names and symbols of isotopes.

Determine average atomic mass of an element.

Explain relative abundances of isotopes.

Calculate average atomic mass.

Calculate formula mass.

Define mole, and state Avogadro’s number.

Solve for moles and/or mass and/or number of particles.

Describe and sketch the electromagnetic spectrum.

Label the spectrum ends with regard to E, ν, λ.

Identify forms of EM radiation in regard to higher/lower E, ν, λ.

State and describe the speed of light.

Solve problems, calculating c, E, ν, λ.

State and discuss specific uses of EM.

Define spectroscopy.

Use spectra to identify substances.

Define and describe quantum numbers.

Name and describe each of the quantum numbers.

State possible values of each quantum number.

Define orbital.

Describe shapes and sizes of various orbitals.

State quantum numbers for particular orbitals/electrons.

State and apply the Aufbau Principle.

State and apply Hund’s Rule.

State and apply the Pauli Exclusion Principle.

Complete an orbital filling diagram.

Write the electron configuration of a given atom.

Identify the valence electrons in an electron configuration.

Draw electron dot diagrams.

Dalton’s Four Ideas:

1. All matter is composed of tiny particles called atoms.

2. Atoms of the same element are the same, atoms of different elements are different.

3. Atoms combine in small whole-number ratios to make compounds.

4. Atoms are re-arranged in chemical reactions.

The Mole Day Song

http://www.youtube.com/watch?v=ReMe348Im2w

Express all answers in scientific notation

1. Solve the following:

(1.5 X 105)(4.0 X 10-9) (12.0 X 10-26)(4.0 X 1010)

7.0 X 106 9.6 X 10-4

3.5 X 10-3 3.2 X 109

12.5 X 10-6 15.0 X 1011

6.25 X 1012 3.0 X 1012

(2.5 X 1016)(3.0 X 10-4) (8.5 X 10-7)(2.0 X 102)

(4.15 X 107)(5.03 X 10-5) (4.5 X 10-15)(6.11 X 107)

(7.52 X 106)(9.30 X 10-5) (4.37 X 10-8)(9.94 X 102)

(9.01 X 103)(8.39 X 109) (3.115 X 10-5)(2.88 X 105)

Solve the following problems, being careful to:

1. Show all work

2. Include all units, etc.

3. Keep all work neat and organized.

1. The world population is estimated at 6.79 X 109. If the average person speaks 3.5 X 103 words per day, how many words are spoken in a year?

2. If 6.022 X 1023 atoms of copper have a mass of 63.546g, determine the mass of 5.00 X 105 L of copper.

3. Determine the number of particles (molecules) exhaled in one breath, given that the volume of a breath is 2.5L. 2.24 X 104 ml of air is known to contain 6.022 X 1023 molecules of air, and the density of air is 1.29 X 10-3 g/ml.

4. What would it cost to buy a single atom of aluminum, if aluminum costs $3.20 per pound, and 6.022 X 1023 atoms of aluminum have a mass of 26.982g?

Extra practice: moles and EM

1. Calculate the frequency of radio waves of a wavelength of 1.50cm.

2. Calculate the wavelength of UV with a frequency of 9.0 X 1015 Hz.

3. Calculate frequency of gamma rays with wavelength of 5.0 X 10-3 nm.

4. Calculate the energy of one photon of UV that has a frequency of 6.77 X 1016 Hz.

5. Calculate the energy of a radio photon of a wavelength of 32cm.

6. Describe the process (steps) by which an atom emits a photon (of visible light).

7. If an atom emits visible light at 450nm, what is the energy of the electronic transition (electron change) causing this emission?

8. What is the frequency of electromagnetic radiation corresponding to an electron transition of 7.39 X 10-14 J? What type of EM is this?

1. 2.00X1010 cm/s 2. 3.3X10-8 m 3. 6.0X1019 1/s 4. 4.49X10-17 J 5. 6.2X10-25 J 6. e- absorbs E, is “excited. e- releases excess E as a photon as it goes to lower E. 7. 4.42X10-19 J 8. 1.12X1020 1/s gamma

1. Calculate the mass of 3.2 mol water.

2. Determine the number of formula units in .25 mol FeCl3.

3. How many atoms are present in .032g sulfur?

4. Determine the mass of 1.2 X 1017 molucules CH4.

5. Calculate the number of molecules in 3.6g glucose (C6H12O6).

6. Calculate the mass of 9.0X 1026 formula units Ca(NO3)2.

1. 58g water 2. 1.5 X 1023 formula units FeCl3. 3. . 6.0 X 1020 atoms S 4. 3.2 X10-6g CH4

5. 1.2 X 1022 molecules C6H12O6 6. 2.5 X 105 g Ca(NO3)2