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.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter12: Chemical Bonding

Section: Chapter Questions

Problem 100AP

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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.

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