LARN 065 C17D1
Start the following in class:
1.a. Use the PQ5R or SQ5R method to prepare a study guide for section 8.4 of your chemistry text on Polar Bonds and Molecules or go to https://socratic.org/chemistry to research the topics brought up in section 8.4 of your text. Read section 8.4 in your chemistry text, pages 237 through 246, and as you do, create a study guide using the SQ5R or PQ5R method. You may record vocabulary entries in the body of your study guide, or you may check them off on the chapter 8 vocabulary list as you think about the meanings of the terms and add any notations to the vocabulary list for clarifications sake.
1.b. Writing in blue or black ink, place your hand in number in a circle followed by your name in the upper right white space of a piece of three holed composition paper in your learning log that hasn’t been written on. Place the page reference for the problems to be considered to the left of the red marginal line on the first blue line. Centered on the first blue line, write a descriptive title for the learning activity such as Section [chapter #.section#] Responses. Before you write your response to each question or problem listed below, write its designation to the left of the red marginal line as listed below, followed by your response in ink to the right of the marginal line.
- Study Conceptual Problem 8.3 on page 239 and then show your work for practice problems I8-30abcdef (In chapter 8, problems 30a, 30b, 30c, 30d, 30e, and 30f) and I8-31abcd.
- In the Section Assessment 8.4 on page 244, read, analyze, and show your work for practice problems I8-32 (In chapter 8, problem 32), I8-33, I8-34, I8-35, I8-36, I8-37a [Hint for I18-37a: see page 224, Table 8.2 for a dot/dash structure for H2O2], I8-37bcd, and I8-38.
- After you are finished, check page R88 of the text and check each of those problems that you can by writing in either a check mark (√) or a correction in green ink as we do in class.
- Some questions do not have a suggested response given. For each such question, circle the number of the question in the margin of your notebook paper and check your response with that of your classmates when you come to class.
2. In your Journal Notebook write your journal entry on sheets of three holed 8.5 inch by 11 inch ruled paper. In the upper right corner white space of each upward facing page, use a blue or black pen to write your hand in number within a circle followed by your name. To the left of the marginal line, print J65A and circle it. Each journal entry should either be at least a paragraph of exemplary writing and penmanship concerning a single topic, or be a concept map relating chemistry terms. Begin each day’s paragraph with a topic sentence, follow with explained instances, and close with a focused summary statement. The required journal focus question J65A for today is
a. Compare the similarities and differences between atomic orbitals and molecular orbitals.
b. What are the differences in location and shape of sigma bonding molecular orbitals, σ bonds, and pi bonding molecular orbitals, π bonds?
c. Give examples of sigma bonding molecular orbitals and pi bonding molecular orbitals.
d. For each of your examples, describe the differences in the location and shape of the sigma bonding molecular orbitals.
e. For each of your examples, describe the differences in the location and shape of the pi bonding molecular orbitals.
3. In your Journal Notebook write your journal entry on sheets of three holed 8.5 inch by 11 inch ruled paper. In the upper right corner white space of each upward facing page, use a blue or black pen to write your hand in number within a circle followed by your name. To the left of the marginal line, print J65B and circle it. Each journal entry should either be at least a paragraph of exemplary writing and penmanship concerning a single topic, or be a concept map relating chemistry terms. Begin each day’s paragraph with a topic sentence, follow with explained instances, and close with a focused summary statement. The second required journal focus activity J65B for today is
Compare single, double, and triple covalent bonds in a table with the following seven column headings arrayed from left to right:
| Type of Bond | Dot Symbol for the Bond | Dash Symbol for the Bond | Relative Strength of the Bond
[1, 2, or 3 as Strongest] |
Number of Sigma Bonds (σ bonds) | Number of Pi Bonds (π bonds) | Relative Reactivity of the Bond
[1, 2, or 3 as the most reactive] |
|
| 1 | Single Covalent Bond | ||||||
| 2 | Double Covalent Bond | ||||||
| 3 | Triple Covalent Bond |
Recommended for those who have time left in their 45 minute study period, but not required of all:
1. If you have not already done so, finish constructing dot formulas and dot/dash formulas for the models in the packet of papers distributed for laboratory U05-5 entitled Three Dimensional Models of Covalent Molecules. Use the TE, VE, SE, NBE method of constructing dot formulas that was taught in class. The method is also explained in the handout entitled Draw Lewis Structures for covalently bonded atoms.
Write in small print in the column on the left and show there the calculated numbers of total tendency electrons,TE,the calculated total actual number of valence electrons,VE, the calculated number of shared electrons, SE, and the calculated number of non-bonding electrons, NBE for a molecule of each substance. Then use those calculated quantities to construct a small dot formula fora molecule of each substance in the column on the right.
Finally construct the structural dot/dash formula for the molecule in the column titled Structural Dot/Dash Formula.