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1 Name: Date: Class: Win, Lose, or Draw Application Problem: What are the shapes and polarity of some common molecules (covalent compounds)? Materials: Ball and stick model pieces and a Periodic Table Information: As you learned in the last unit nuclear charge, the shielding effect and the energy levels of the electrons determines how the electrons behave in an atom. The valence electrons (the ones on the outside) specifically are responsible for reacting and forming chemical bonds. You have seen that some atoms are willing to gain electrons to form anions; others are willing to lose electrons to form cations. In this activity, you will see that other atoms are willing to share electrons. This is called covalent bonding. The fact that an atom will gain, lose or share electrons so that it has the electron configuration of a noble gas is called the octet rule. If the number of electrons being shared is 2, this is called a single bond. A double bond will share 4 electrons and a triple bond will share 6 electrons. When two atoms share electrons to complete their octet, the amount of time the shared electrons, also known as bonding electrons, spend between the atoms does not have to be equal. Electronegativity was defined as the ability of an atom to attract an electron to itself in a bond. This means that when two atoms are bonded covalently the electrons may be more attracted to one atom than the other based on the atoms electronegativities. When this happens, the bond between the two atoms is called a polar bond and the electronegativity difference between the two atoms is generally A difference below 0.5 is considered to be equal sharing of the electrons and the bond is considered to be nonpolar; above 1.7 and the bond is considered to be ionic, the electrons are not shared at all but completely transferred. Based on how the bonds are arranged in a molecule, a molecule may be considered polar or nonpolar as well. Valence Shell Electron Pair Repulsion (VSEPR) Theory states that the electrons will in a molecule will always be found in pairs and that these pairs of electrons will repel each other as much as possible. Unshared pairs also known as lone pairs or nonbonding pairs of electrons repel other electrons and bonding electrons the most. The distance between the pairs of electrons created by the repulsion results in the shape of the molecule. When this shape is created, if the molecule has any polar bonds, you must look at where the electrons are being attracted (pulled toward). As in a tug of war, if the electrons are being pulled equally, no one bond wins and the molecule is considered to be nonpolar. However, if one bond or several bonds on the same of the molecule attracts electrons more, then the molecule is polar. Prelab Questions: 1) What does the word octet mean? 2) How many valence electrons do most of the noble gases have? 3) Which noble gas is an exception to the octet rule? Why? What other elements would be an exception to the octet rule when they react? 4) Would an electron be attracted to an atom with a high electronegativity or a low one? 5) Why would pairs of electrons repel each other as described in the VSEPR theory? Procedure: Fill out the table of information on the molecules by doing the following: 1. Prepare Lewis dot structures of each of the following molecules. Based on what you know about their Lewis dot diagrams and the octet rule.
2 2. Determine if the bonds are polar or nonpolar by subtracting the electronegativities of the two atoms in each bond.. This must be done for EVERY bond in the molecule. Then list the total number of bonds and the total number of lone pairs of electrons. 3. Build the molecule using the model pieces and then draw a three dimensional representation of each molecule. 4. Name the shape of the three dimensional structure for each molecule using the information on the last page of this packet. 5. In the shape picture, draw an arrow on any polar bond you determined in step 2 in the direction of the atom with the higher electronegativity. Based on the arrows, determine if one side of the molecule wins a tug-of-war. If yes, the entire molecule is polar. Use this to fillin the last column of the table. 6. Then answer the summary questions. Molecules Model Pieces H 2 NH 3 C = black Cl 2 H 2 O H = yellow CF 3 H CO 2 O = red AlH 3 O 2 N = light blue PH 3 N 2 Halogens (F, Cl, Br, I) = green, orange, purple HCl CH 2 F 2 CH 4 Al, P = white (Be very gentle with these.) Formula Lewis dot diagram Bonds polar or nonpolar? # bonds & # lone pairs Name of Shape 3-D picture of shape Molecule polar or nonpolar? H 2 Cl 2 CF 3 H
3 Formula Lewis dot diagram Bonds polar or nonpolar? # bonds & # lone pairs Name of Shape 3-D picture of shape Molecule polar or nonpolar? NH 3 PH 3 AlH 3 HCl CH 4
4 Formula Lewis dot diagram Bonds polar or nonpolar? # bonds & # lone pairs Name of Shape 3-D picture of shape Molecule polar or nonpolar? CO 2 H 2 O O 2 N 2 CH 2 F 2
5 Summing Up: 1. What minimum number of bonds does an atom need to form in order to be a central atom? 2. Can any element be a central atom? Why or Why not? 3. Compare and contrast the Lewis dot structures of AlH 3 and PH 3? 4. Compare the shapes of AlH 3 and PH 3? 5. In H 2 O, the oxygen has two hydrogens attached. In CO 2, the carbon has two oxygens attached. Explain why the geometries of H 2 O and CO 2 are different. 6. Summarize the effect of the presence of unshared electrons on the shape of a molecule. 7. What two factors do you have to use to determine the polarity of a molecule?
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