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Bellwork 11-13-2014 Honors Have homework out – case studies Take out your note-taker from yesterday on the three types of bonds  Use as much information.

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Presentation on theme: "Bellwork 11-13-2014 Honors Have homework out – case studies Take out your note-taker from yesterday on the three types of bonds  Use as much information."— Presentation transcript:

1 Bellwork Honors Have homework out – case studies Take out your note-taker from yesterday on the three types of bonds  Use as much information as you can from the evidence you gathered yesterday to describe the difference between ionic and covalent bonds.

2 Bellwork Have out your lab notebook to be collected Have out packet on ionic and covalent bonding (Per. 5 and 6) 1. Fill in the T-chart to describe the difference between ionic and covalent bonds. IonicCovalent

3 Announcements Turn in lab report – honors Lab make up Friday Nov. 14

4 Intervention Coming into class unprepared will no longer be tolerated I expect you come in quietly and get started on the bellwork Anyone being loud or not starting on the bellwork will cause the whole class to go out and try again Warnings You will get two yellow cards, a third equals a red and a summative quiz

5 Warnings Talking after I call for your attention (normal signal – clap once, clap twice) 5 sec and then warning Talking while I am talking or a classmate is talking/giving an answer iPad out when not necessary – ask me first if you need to use it for something in class Excessive loudness during group work Distracting behavior – out of seat, messing around with materials when not instructed to, excessive laughing or loud annoying noises

6 You will be accumulating evidence for each type of bond: Non-polar covalent Polar covalent Ionic You will work on one type of bond at a time for 10 minutes and share your results Use the evidence with your group to come up with information to fill out your note-taker Ionic vs. Covalent wrap up

7 Example C-C bond Use information you know or information on your desk to fill out all of the information on non-polar covalent bonds Non-polar covalent

8 Example H-N bond Use information you know or information on your desk to fill out all of the information on polar covalent bonds Polar Covalent

9 Example K-Cl bond Use information you know or information on your desk to fill out all of the information on ionic bonds Ionic

10 Case Studies #1  Polar covalent  C-O, C is slightly positive and O is slightly negative  Electronegativity difference is medium.  Would not conduct electricity because electrons are shared and they do not break up in solution to full positive and full negative charges.  Lower melting point than ionic because the bonds are weaker than ionic bonds

11 Case Studies #2 1. Ionic because there are full positive and negative charges on the atoms in the network 2. Ba+, O- 3. Metals and nonmetals 4. Yes because the atoms would dissociate into positive and negative ions when dissolved. 5. The electronegativity difference is high causing it to have a high melting point because the bond is very strong between positive and negative ions.

12 Videos https://www.youtube.com/watch?v=pj0F-zv79rM https://www.youtube.com/watch?v=QqjcCvzWwww

13 Summative Writing Take out a blank sheet of paper Put everything else away EXCEPT your note- taker This is an independent assignment, plagiarism is cheating and will receive a zero. Answer #1 in 5-7 sentences and underline keywords (use all in each question)!

14 Scoring 4 – All keywords are used and underlined, meets minimum length requirements, all ideas are described in detail and accurate. 3 – A few keywords missing or not underlined, 1 or 2 sentences short, all ideas are described accurately. 2 – Half of the the keywords are missing, 3 or 4 sentences short, ideas are somewhat accurate. 1 – Only a couple keywords are used, only 1 or 2 sentences in length, ideas are inaccurate. 0 – Assignment missing

15 Summative Writing Assignment 1. Describe the similarities and differences between a IONIC bond and a POLAR COVALENT bond. 2. Draw an example of each type of bond with any charge that is associated with each atom. Keywords: electronegativity difference, electrons, metal/nonmetal, dissociation (separation), shared/unshared, charge (+, -, δ +, δ - ), electrical conductivity.

16 Bellwork  In the ionic compound LiF, which element is the metal and which is the non-metal?  Which element gets the positive charge, metal or non-metal?  Which element gets the negative charge, metal or non-metal?

17 Bellwork Honors  Is lithium a metal or non-metal? What is its charge (how many electrons does it give away)?  Is oxygen a metal or non-metal? What is its charge (how many electrons does it want)?  How many lithium ions would it take to complete Oxygen’s octet?

18 Ionic Bonding Lab Notes Metals lose electrons and become positive ions or cations. Non-metals gain electrons and become negative ions or anions.

19 Depiction + Cation - Anion

20 Chemical Formulas: you try Oxygen is in group 6 and needs 2 more electrons to fill its shell. Once it gains 2 electrons, it will have a -2 charge. Magnesium is in group 2 and wants to give away 2 electrons to arrive at a full shell. Once it gives up these 2 electrons, it will have a +2 charge

21 Atom vs. Ion Size Cations get smaller as they lose electrons, anions get larger as they gain electrons

22 Chemical formula writing The subscripts show the ratio of each atom in the compound. For an ionic bond, the subscripts, or number of each atom in the compound, need to balance the charges on the ions. The subscript of each ion changes to make the compound neutral. The chemical formula shows how many of each ion are needed to balance the charges between both ions and make the compound neutral.

23 Naming Cation name stays the same Anion name changes the ending to –ide Example: Cation + anion = Magnesium Chloride

24 Lab Time! 1. Get out your lab notebook and write down the title for the lab ONE LAB NOTEBOOK PER PAIR 2. Write the title and a question for the lab 3. Copy the data table into your notebook: you will be creating 12 compounds 4. You will be working with one partner (next to you) today, otherwise your lab will not be graded

25 Cut out pieces Cut out the pieces on the purple sheet I handed out IGNORE THE WILDCARDS – YOU WILL NOT NEED THESE Your goal is to complete 12 neutral compounds and fill out the chart you created in your lab notebook.

26 Make a Poster With your partner: On a separate sheet of paper, paste or tape down 5 compounds that you made. Label them with their chemical formula and their ionic compound name.

27 Discussion Questions You have 15 minutes now to answer discussion questions in class Come show me when you AND your partner are finished, I will only check you off if you are both done! If you do not finish, this is homework

28 Kahoot Review Log on to Kahoot.it!

29 Monoatomic Ionic Compounds So far we have only been looking at monoatomic ionic compounds  compounds with only one element of each ion Ex. Na 2 O Na +1 and O -2

30 Polyatomic Ionic Compounds These are ionic compounds containing ions with multiple elements Poly = many Ex. NaNO 3 Na +1 NO 3 -1

31

32 Naming Polyatomic Ionic Compounds Criss-Cross Method: Write out the two ions you are using in the compound (cation first) Write the charges they would receive above each one Cross the cation charge to to the anion subscript and the anion charge to cation subscript

33 Example 1 – Monoatomic Calcium Bromide Ca Br Ca 1 Br 2 CaBr 2 +2

34 Example 2 – Polyatomic Magnesium Phosphate Mg PO 4 Mg 3 PO 4 2 Mg 3 (PO 4 )

35 Try These! 1. sodium bicarbonate 8. aluminum (III) sulfate 2. sodium fluoride 9. silver (II) nitrite 3. iron (III) chloride10. calcium sulfate 4. sodium carbonate 5. copper (II) sulfate 6. magnesium hydroxide 7. barium nitrate

36 Name These! Mg 2 SO 4 Ca(NO 3 ) 2 Li 3 PO 4 NaClO 2 (NH 4 ) 2 CO 3 Fe(OH) 2

37 Homework Finish lab questions if you did not finish in class Homework on writing and naming ionic compounds


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