1. For the following group of elements: Nitrogen (N), Hydrogen (H), Sulfur (S). Nitrogen has an atomic number of 7, and electronegativity of 3.04. Hydrogen has an atomic number of 1, and an electronegativity of 2.20. Sulfur has an atomic number of 16 and an electronegativity of 2.58. a. Draw the electron configuration diagrams for each element shown. b. Draw a molecule that could be made using these elements. Do not worry about whether the molecule is actually stable in nature, just try to fill the electron shells. You have to use all of the elements in your molecule, but you can use any element more than once. c. Label each bond as non-polar, polar, or ionic. Show the partial or full charges.

1. For the following group of elements: Nitrogen (N), Hydrogen (H), Sulfur (S). Nitrogen has an atomic number of 7, and electronegativity of 3.04. Hydrogen has an atomic number of 1, and an electronegativity of 2.20. Sulfur has an atomic number of 16 and an electronegativity of 2.58. a. Draw the electron configuration diagrams for each element shown. b. Draw a molecule that could be made using these elements. Do not worry about whether the molecule is actually stable in nature, just try to fill the electron shells. You have to use all of the elements in your molecule, but you can use any element more than once. c. Label each bond as non-polar, polar, or ionic. Show the partial or full charges.

Chemistry In Focus

7th Edition

ISBN:9781337399692

Author:Tro, Nivaldo J.

Publisher:Tro, Nivaldo J.

Chapter5: Chemical Bonding

Section: Chapter Questions

Problem 46E: CH3COCH3 (acetone) is a common laboratory solvent that is often used in nail polish remover. Its...

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In a covalent bond between two atoms, the more electronegative atom will attract more electron density toward itself, causing a polar bond. The more electronegative element is the negative pole, whereas the less electronegative element is the positive pole. The direction of the dipole is always toward the more electronegative element. This is often inflicated by an arrow, as shown in the figure. (Figure 1) The magnitude of the bond polarity is the difference in electronegativity values of the atoms. For example, in the molecule Cl2, the CICI bond is nonpolar because there is no difference in electronegativity between two atoms of the same element. In the CIBr molecule, However, the C1 Br bond is polar because Cl and Br have different electroneaativitv values. A CI I bond would be more polar than a C1 Br bond because there is a greater electronegativity difference between Cland I than between CI and Br.
Draw the Lewis Dot structure for N2 (on paper, not on Canvas) then answer the questions. a. How many total valence electrons are in N2? Express your answer as a whole number. b. How many single bonds are in N2? Express your answer as a whole number. c. How many double bonds are in N2? Express your answer as a whole number. d. How many triple bonds are in N2? Express your answer as a whole number.
Atom A has 4 valence electrons. Atom Z has 6 valence electrons. For the AZ3-2 ion, answer the following questions about its Lewis dot structure (drawn according to Chm 130 guidelines). a. How many valence electrons are in the structure? b. How many single bonds are in the structure? c. How many double bonds are in the structure? d. How many triple bonds are in the structure? e. How many lone pairs are on the central atom in the structure? f. What is the shape of the structure? g. What are the bond angles of this ion?
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CH3COCH3 (acetone) is a common laboratory solvent that is often used in nail polish remover. Its Lewis structure and space-filling molecular image are shown here: Acetone is a polar molecule; the oxygen end has a slightly negative charge (oxygen is more electronegative), whereas the carbon and hydrogen end has a slightly positive charge. In liquid acetone, the molecules are attracted to each other via these polar ends-the positive end of one molecule is attracted to the negative end of its neighbor-and therefore align as shown here: Draw a Lewis structure and space-filling molecular image for CH2Cl2 (dichloromethane), another common laboratory solvent. Is the molecule polar? Which end of the molecule has a slightly negative charge? Which end has a slightly positive charge? Draw several space-filling molecular images of CH2Cl2 showing how they align in liquid dichloromethane.