4) Based on valence bond theory, what is the hybridization of the central atom(s) in C,F?A) both carbons are sp3B) both carbons are sp2C) one carbon is sp3 and the other carbon is sp25) Which element contains triple covalent bonds?A) nitrogenB) oxygenC) iodine

Answered: Image /qna-images/answer/1948e0d7-b28d-4e4e-a3a6-9924ae044264.jpg

Answered: 4) Based on valence bond theory, what…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter10: Molecular Structure And Bonding Theories

Section: Chapter Questions

Problem 10.67QE

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It is possible to write a simple Lewis structure for the SO42- ion, involving only single bonds, which follows the octet rule. However, Linus Pauling and others have suggested an alternative structure, involving double bonds, in which the sulfur atom is surrounded by six electron pairs. (a) Draw the two Lewis structures. (b) What geometries are predicted for the two structures? (c) What is the hybridization of sulfur in each case? (d) What are the formal charges of the atoms in the two structures?
9) HCCCO₂H, is an organic hydrocarbon. a) Draw a geometrically accurate structure so that the formal charge of each atom is zero identifying the bond angles (Draw it BIG!). b) Identify the hybridization about each atom (not H) forming a bond c) How many o or π bonds are there in this molecule d) The combustion of the hydrocarbon produces carbon dioxide and water in the gaseous state. Use average bond enthalpies to determine enthalpy of reaction
Draw the Lewis structures for the Sulfite (SO32-) and Sulfate (SO42-)anions. a) On your structures, indicate the formal charge at each atom. b) Draw any resonance structures. c) What is the hybridization of the sulfur atom in each structure d) How many sigma and pi bonds are on each structure
Copy the structure below and give the a) Expanded Lewis Structure b) Condensed Lewis Structure c) Bond line Structure d) Give the hybridization carbon atom.
4. Knowing that H has an electronegativity value between those of B and N, what conclusion can be drawn from the fact that BH3 is nonpolar but NH3 is polar? QUestion shown in photo! a) The boron atom in BH3 is sp3 hybridized, while the nitrogen atom in NH3 is sp2 hybridized. b) The nitrogen atom in NH3 has a lone pair of electrons, whereas the boron atom in BH3 does not. c) BH3 forms a ring structure. d) The nitrogen atom in NH3 lacks enough electrons to complete its octet.
4) Based on valence bond theory, what is the hybridization of the central atom(s) in CF4? A) both carbons are sp3 B) both carbons are sp2 C) one carbon is sp3 and the other carbon is sp2
Hybridization around central Molecular Number of Lewis Structure Sketch 3D Molecular Electron shape of electron Formula Valence Geometry Geometry Electrons atom domains around central atom (include all atoms in the sketch) CO2 SbCls NH3
A, B, and C
Consider the following ion: BrO3¯. a) Show the full electron configuration for Br. b) Draw the most correct Lewis structure for BrO3¯ and briefly explain why your Lewis structure is correct. c) If the structure is stabilised by resonance, draw at least one of the possible resonance forms. If it is not stabilised by resonance, briefly explain why. d) What is the electronic geometry of BrO3-? What is its molecular shape? e) Does BrO3 have a dipole moment? Briefly justify your answer. f) On average, would you expect IO3¯ to have longer or shorter bonds than BrO3¯? Briefly explain your answer. g) Which of the following molecules would you expect to have the lowest vapour pressure? Briefly explain your choice. Br HO HO. Br- Compound A Compound B Compound C h) What is the molecular formula for Compound C? What is the empirical formula for Compound C?
I have a question regarding hybrid vs atomic orbitals: 1) What would be the hybridizations of C and O in the molecule H2CO? It asks to draw an electron orbital diagram (with arrows) of all the electrons in C before and after hybridization. 2) Draw a diagram of the H2CO molecule showing the overlap of orbitals between the C and O atoms that make up the sigma (σ) and pi (π) bonds. Which orbitals make up the σ bond? Which ones form the π bond?
2. Consider the following molecules or ions: H2O, SF4, IF4", and COF2. Answer the following questions based on the Lewis structures and VSEPR theory prediction of their molecular shapes. (a) Which one has only bond angles of 109.5°? (b) Which one has only bond angles of 120°? (c) Which one has bond angles of 90 and 180°? (d) Which one has bond angles of 90, 120, and 180°?
4. Valence Bond Theory. Consider formaldehyde, H₂CO. ( a) Draw a Lewis structure of formaldehyde. b) Draw a picture using valence bond theory showing the bonding of formaldehyde using appropriate hybrid orbitals. (Include electrons) c) Describe the bonding of the C-O bond and C-H bond by listing the bond type (σ, π) and the orbitals contributing to the bonding. C-O: C-H:

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4) Based on valence bond theory, what is the hybridization of the central atom(s) in C2F? A) both carbons are sp3 B) both carbons are sp2 C) one carbon is sp3 and the other carbon is sp2 5) Which element contains triple covalent bonds? A) nitrogen B) oxygen C) iodine