Why do large conjugated molecules absorb visible light? Select all that apply.A. Their electronic energy levels are sufficiently far apart.B. Their electronic energy levels are relatively close together.C. There is a sufficiently small energy gap between the highest-energy filled orbital and the lowest-energy vacant orbital.D. UV light is not high enough in energy to promote an electron.

A molecule absorb in visible region if the energy gap between the highest occupied energy level and…

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Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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5. Answer the following questions about the molecules CH2S (C is the centralatom).a. Draw the Lewis structure.b. Write the valence shell electron configuration for C.c. Draw the valence orbital diagram for C.d. Draw the hybridized orbital diagram for C.e. Give a bond description for each bond in the molecule.
Sulfur hexafluoride SF6 is the most potent greenhouse gas to date. It is 22,800 times more effective at trapping heat than carbon dioxide (CO2), and lasts in the atmosphere for thousands of years. Please refer to the molecule diagrams below to answer the following questions: a. Explain why SF6 has more asymmetrical vibrations than CO2 b. Explain why asymmetrical vibrations in SF6 bonds are stronger than asymmetrical vibrations in CO2 bonds c. Explain the relationship between strength and quantity of asymmetrical vibrations and greenhouse gas potency
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Which of the following molecules/molecular ions would theoretically NOT have an underlying tetrahedral (T) electronic structure...? OA. All of these molecules/ions have an underlying tetrahedral geometry. OB. BF OC. SIFA OD.CFA OE PF ) ) 8. 9. J C V control option command command optic V
1. Which of the following statements is true regarding the periodic table? a. elements of the same group have the same oxidation number b. elements are arranged based on decreasing atomic weight c. both are correct d. both are incorrect 2. Please refer to the picture. The molecular geometry of the right-most carbon in the molecule is: a. trigonal bipyramidal b. trigonal planar c. pyramidal d. tetrahedral 3. Given the following statements: I. The less electronegative atom gains a greater fraction of the shared electron thereby acquiring a partial positive charge indicated by delta plus. II. Increasing the differences in electronegativity is indicative of decreasing bond polarity. a. both are correct b. both are incorrect c. statement 1 is correct d. statement 2 is correct e. statement 1 is incorrect f. statement 2 is incorrect
Configurations that is NOT paramagnetic a. 1s2 2s2 2p6 3s2 3p5 b. 1s2 2s2 2p6 3s2 3p6 c. 1s2 2s2 2p6 3s2 3p4 d. 1s2 2s2 2p6 3s7
From an energy perspective, why do chemical bonds form? to maximize the potential energy O to minimize the potential energy O to compensate for the Pauli exclusion energy O to optimize the interatomic distance
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In In solid Xenon the atoms are close enough such that their probability distribution of charge * .could overlap a. Such overlap is partially attractive or repulsive due to Coulomb interaction O b. Such overlap is mainly repulsive and attractive and due to magnetic and Coulomb interactions, respectively c. Such overlap is mainly repulsive and due to Coulomb interaction O d. Such overlap is mainly attractive and due to Coulomb interaction e. None of above )
8. The polarizing power of Group II elements thermal stability of their compounds down the group and the when go down the group. A. increase, decrease B. decrease, increase C. increase, increase D. decrease, decrease
QUESTION 16 Which of these molecular orbitals is the Lowest in Energy? (click on an actual p orbital that is part of the lowest energy molecular orbitai) B. D. Selected Coordinates Clear

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