LARN 056 C14D4
ATTENTION: If you have not already done so, locate three (3) shiny United States pennies that were minted after 1982, the shinier the better, to experiment with. Bring these pennies in to transform two of them into souvenir alloys celebrating your taking chemistry this year! The pennies will be treated to form souvenirs of chemistry class. If the pennies you bring in are dull, you will have the clean them. Store them temporarily in your grommeted, three hole zipper pen case until it is time to do the laboratory activity.
Start the following in class:
1. For your journal entry J56 , you are to construct a concept map. Please turn to page 206 in your text and, in your learning journal, construct a concept map relating the seven terms listed at the bottom of the page. Connect related terms with arrows such that the subject of each sentence explaining the relationship is at the tail of the arrow, the verb describing the relationship of the subject to the predicate is written beside the arrow, and the arrow head is touching the oval of the term which is the object or predicate nominative of the verb that you have chosen.The instructions for how to download and install software on your home PC, Mac, or Linux computer are found in the MNSD Google Drive > Student Resources > How to Register with Selected Web Sites and Download/Install Software folder. Or you can use the links provided below.
2. Locate the Ionic and Metallic Bonding informational packet.
a. Take Cornell notes on the three (3) pages that describe how to write the formulas of ionic compounds using the least common multiple of the absolute values of the charges on the positive and negative ions to calculate the number of positive and of negative charges needed to make each formula unit electrically neutral.
b. Locate the “Writing the Formulas of Ionic Compounds Correctly” worksheet, on page 7 of the Ionic and Metallic Bonding packet. Fill in just the first two (2) horizontal rows for each of the first two cations, Na+ and Ca2+, listed along the left side of the worksheet. As you do this, follow the instructions given below.
In the upper rectangular space formed by the intersection of each row and column, in smaller than usual print write the correct formula of the ionic compound formed from the positive ion listed at the left side of each row and the negative ion listed at the top of the column. Use the least common multiple of the absolute values of the charges on the positive and negative ions to calculate the number of positive and of negative charges needed to write each formula as an electrically neutral compound.
After neutral formulas that show the ion charges on each species have been written for each entire row on the worksheet, below each correctly written formula, write the formula of each neutral compound but without showing the charges on the ions and without retaining parentheses around the ionic symbols unless more than one polyatomic ion is being represented in the formula. Note that the hydroxide ion, OH1-, is a polyatomic anion in which the oxygen and hydrogen atoms are covalently bonded to each other within the ion and stay together as the ion moves around as one unit.
Recommended for those who have time left in their 45 minute study period, but not required of all:
1. Locate the Ionic and Metallic Bonding informational packet.
Do problems 1 through 5 on the page of the worksheet labeled ‘Ionic Bonding” in the Ionic and Metallic Bonding packet. That page shows the dot formulas of Na and Cl before and after reacting.
- Study the example that shows how to write the dot formulas of Na and Cl before and after reacting..
- Then, for each of the five problems, carefully represent reacting atoms with dot formulas and show the transfer of electrons from the low electronegativity metal atom(s) to the high electronegativity nonmetal atom(s).
- Next, for each of the five problems, carefully represent produced positive and negative ions.
- The metal atoms lose all their valence electrons as they become positive ions, cations.
- The nonmetal atoms fill up all their partially filled p orbitals to attain a completely filled valence shell of electrons when they become negative ions, anions.
- Sometimes more than one metal or nonmetal atom will be required so that the number of electrons lost from the metal atom(s) equals the number of electrons gained by the nonmetal atom(s).
- When the number of electrons lost equals the number of electrons gained, the resulting ionic compound is electrically neutral (as it is in real life) and the ratio of the number of cations produced to the number of anions produced will represent the empirical formula of the product compound.
- Record the lowest ratio formula (empirical formula) for each ionic compound formed.
- Record a correct standard name for the product compound by writing the name of the positive ion in front of the name of the negative ion, but with the omission of the word ion twice.
2. Download current ActivInspire unit flipchart by logging on to the MNSD Google Drive and selecting it from the Student Resources > ActivInspire folder. Generally the flipchart name will begin with a capital U to designate the chemistry unit of study and end in a relatively high version number following the v at the end of the flipchart’s title. Download the flipchart on ionic and metallic bonding after clicking on the following link: Ionic&MetallicBonding . Click through the chart quickly and take Cornell notes on concepts that you were unaware of. At the end of your study, write a summary statement of what you learned.
[If you had not yet successfully installed ActivInspire software, use https://drive.google.com/open?id=0B9ft9hAr_RjiR0pqTUpHb3QyMm8 to download and install the latest version of ActivInspire free personal edition software on your home PC, Mac, or Linux computer.]
3. Check out the student made Quizlet for chapter 7 at https://quizlet.com/171092936/ch-7-ionic-metallic-bonding-flash-cards/. Do all the definitions reflect a thorough and correct understanding?