3. Select CO2 from the drop-down menu on the right of the simulation. Examine the model and real structures for CO2. a. Does each atom have the expected number of bonds? Explain your answer. b. Why is there agreement between the bond angle predicted by VSEPR theory and the actual bond angle?

3. Select CO2 from the drop-down menu on the right of the simulation. Examine the model and real structures for CO2. a. Does each atom have the expected number of bonds? Explain your answer. b. Why is there agreement between the bond angle predicted by VSEPR theory and the actual bond angle?

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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Which statement A-D about VSEPR theory is not correct? Select one: a. The steric number has five values from 2 to 6. b. Statements A-D are all correct. c. In VSEPR theory, the shape or geometry of a molecule is determined by electron-electron repulsion. d. The steric number of a central atom is the sum of the number of bonds and lone pairs around the atom. e. The molecular shape or geometry can differ from the electron-pair geometry.
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1. Consider the diatomic molecules ( molecules with 2 atoms ) in this exercise : O2, N2, Cl2, and HCl . Do you think a diatomic molecule can be any shape other than linear ? Explain . because They are only two alems 2. Look at the Lewis structure you drew for SCl2 and CS2 Both of these molecules are made up of three atoms but have different molecular geometries . a . How is the arrangement of electrons around the central atoms different ? Give the number of lone pairs and bonding groups around each central atom Based on your previous answer , explain why SCl2 can't be linear . c . Explain why one molecule is polar and the other is nonpolar
1.1 Define electronegativity and explain why electronegativity increases with atomic number within a period of the Periodic Table. 1.2 Describe the type of bonding that exists in F2 (g) molecule. How does this type of bonding differ from that found in the HF (g) molecule? 1.3 Define hydrogen bonding using examples. 1.4 PH3 and NH3 moleculea are the same shape but the molecules are non-polar and polar respectively. Explain why this is so. 1.5 Give an example of molecule that has a coordinate covalent bond. 1.6 Draw a Lewis structure for each of the following molecules of ions: a) HF3 b) CIO3-
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