Warmup - work with your table partner Do this on a left-hand page. I will be calling on you. An atom has a total of 15 electrons. An ion of that element has 18 electrons. What is the charge and is the ion larger or smaller than the neutral atom? Write the electron configuration of the first element of Group 16 (oxygen) and the noble gas configuration of the second element of Group 16 (sulfur). If an atom has an electron configuration of 1s2 2s2 2p1, what is the atom and what is its dot diagram? Draw the Lewis dot diagram for a nitrogen atom (N) in the ground state.

Housekeeping Remember that today is the final day to turn in all work from the last unit. Today is the last day to turn in Mendeleev Activity, Coulombic Activity POGIL, and Periodic Trends. If you haven’t completed these yet, get them done and turned in after school. I will be here until at least 4:30. Wednesday next week is the final day to do a RETEST over the last unit.

We will learn about double and triple covalent bonds and review ionic bonds. I will illustrate ionic and covalent bonding with diagrams. Success Criteria Know how to use Lewis dot diagrams to illustrate ionic and covalent bonding. Know how to tell when a bond is ionic and when it is covalent. Know how to determine when covalent bonds are single, double, or triple.

An atom has a total of 15 electrons An atom has a total of 15 electrons. An ion of that element has 18 electrons. What is the charge and is the ion larger or smaller than the neutral atom? Write the electron configuration of the first element of Group 16 (oxygen) and the noble gas configuration of the second element of Group 16 (sulfur). If an atom has an electron configuration of 1s2 2s2 2p1, what is the atom and what is its dot diagram? Draw the Lewis dot diagram for a nitrogen atom (N) in the ground state.

We are going to complete the foldable that we started on Monday about covalent bonding. If you did not get the foldable, please raise your hand.

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How does a covalent bond differ from an ionic bond? Discuss with your table partner and the table in front of you or behind you. You have two minutes to discuss. You need to come up with at least two answers. I will be calling on you to give one answer. I think (or my table partner thinks) that a covalent bond is different from an ionic bond because ______________________.

Why are covalent bonds important? Most of the molecules in living systems contain only six different atoms: hydrogen, carbon, nitrogen, phosphorus, oxygen, and sulfur. These are all nonmetals and form covalent bonds with each other.

Show calculation for determining number of bonds between atoms - handout NEEDED AVAILABLE SHARED BONDS full valence # of electrons O2 2(8) = 16 2(6) = 12 C2H4 2(8) + 4(2) = 24 2(4) + 4(1) = 12

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Lab groups Like last time, we are going to split up into lab groups to work on the assignment. Each of you in a group should be working on a different problem. After you think you have it, show it to your group. When the whole lab group agrees that you have all gotten the correct setup (or have bogged down into a disagreement that you can’t resolve), call me over to check.

Instructions Use the cards and chips to build the dot structure for each atom. Nonmetals are yellow and metals are green. Move electrons from the metal to the nonmetal until the nonmetal is full. If there aren’t enough electrons for the nonmetal to be full (8), get another atom of the metal. If the nonmetal is full, but the metal still needs to get rid of more electrons, then get another atom of the nonmetal. There are just enough cards to have all of the bonds you need built at the same time.

instructions Each person in the group should be working on building a different bond. Then you all check over each other’s work to make sure that it looks right. When you think that it is right, call me over to check. DO NOT just start drawing. You need to build the bonds with the cards and the chips and have me check it first. Each person in the group should be working on a different problem.

To write the formulas … For an IONIC bond, you are supposed the write the METAL first and then the NONMETAL. Use subscripts to show how many you have of each atom when there is more than one of that atom. Examples: dfjlkdjasdlfkjaT This is MgCl2

Ionic example Elements Dot structures of the elements Dot structure for ions Chemical formula Lithium + Sulfur

To write the formulas … PCl3 For a COVALENT bond, you are supposed the write the LESS ELECTRONEGATIVE element first. Use subscripts to show how many you have of each atom when there is more than one of that atom. Examples: PCl3

covalent example Elements Dot structures of the elements Dot structure for ions Chemical formula Sulfur + hydrogen

Start with the covalent side this time Do the covalent side first. If there is time, do the ionic side also. If we run out of time, you need to complete the rest at home as homework. This will be due next class.

WHat have we learned? Know how to use Lewis dot diagrams to illustrate ionic and covalent bonding. How confident do you feel about drawing Lewis dot diagrams for single elements? How confident do you feel about drawing the diagrams for bonding? Know how to tell when a bond is ionic and when it is covalent. What kinds of elements form an ionic bond? What kinds form a covalent bond? Know how to determine when covalent bonds are single, double, or triple. How do you know if you need single, double, or triple bonds?

HAVE A NICE DAY