Chemistry Atoms First2e
2nd Edition
ISBN: 9781947172647
Author: OpenStax
Publisher: OpenStax College
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Chapter 5, Problem 3E
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Chemistry Atoms First2e
Ch. 5 - Explain how σ and bonds are similar and how they...Ch. 5 - Use valence bond theory to explain the bonding in...Ch. 5 - Use valence bond theory to explain the bonding in...Ch. 5 - How many and bonds are present in the molecule...Ch. 5 - A friend tell you N2 has three bonds due to...Ch. 5 - Draw the Lewis Structures for CO2andCO , and...Ch. 5 - Why is the concept of hybridization required in...Ch. 5 - Give the shape that describes each hybrid orbital...Ch. 5 - Explain why a carbon atom cannot from five bonds...Ch. 5 - What is the hybridization of the central atom in...
Ch. 5 - A molecule with the formula AB3 could have one of...Ch. 5 - Methionine, CH3SCH2CH2CH(NH2)CO2H, is an amino...Ch. 5 - Sulfuric acid is manufactured by a series of...Ch. 5 - Two important industrial chemicals,...Ch. 5 - Analysis of a compound indicates that it contains...Ch. 5 - Consider nitrous acid, HNO2(HONO). (a) Write a...Ch. 5 - Strike-anywhere matches contain a layer of KC1O3...Ch. 5 - Identify the hybridization of each carbon atom in...Ch. 5 - Write Lewis structures for NF3andPF5 . On the...Ch. 5 - In addition to NF3, two other fluoro derivatives...Ch. 5 - The bond energy of a C-C single bond averages...Ch. 5 - For the carbonate ion, CO32 -, draw all of the...Ch. 5 - A useful solvent that will dissolve salts as well...Ch. 5 - For the molecule allene, H2C=C=CH2, give the...Ch. 5 - Identify the hybridization of the central atom in...Ch. 5 - Describe the molecular geometry and hybridization...Ch. 5 - For each of the following molecules, indicate the...Ch. 5 - For each of the following structures, determine...Ch. 5 - Draw the orbital diagram for carbon in CO2 showing...Ch. 5 - Sketch the distribution of electron density in the...Ch. 5 - How are the following similar, and how do they...Ch. 5 - If molecular orbitals are created by combining...Ch. 5 - Can a molecule with an odd number of electrons...Ch. 5 - Can a molecule with an even number of electrons...Ch. 5 - Why are bonding molecular orbital lower in energy...Ch. 5 - Calculate the bond order for an ion with this...Ch. 5 - Explain why an electron in the bonding molecular...Ch. 5 - Predict the valence electron molecular orbital...Ch. 5 - Determine the bond order of each member of the...Ch. 5 - For the first ionizations energy for an N2...Ch. 5 - Compare the atomic and molecular orbitaI diagrams...Ch. 5 - Which of the period 2 homonuclear diatomic...Ch. 5 - A friend tells you that the 2s orbital for...Ch. 5 - True or false: Boron contains 2s22p1 valence...Ch. 5 - What charge would be needed on F2 to generate an...Ch. 5 - Predict whether the MO diagram for S2 would show...Ch. 5 - Explain why N22+ is diamagnetic, while O24+, which...Ch. 5 - Using the MO diagrams, predict the bond order for...
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- Describe the hybridization around the central atom and the bonding in SCl2 and OCS.arrow_forwardUse valence bond theory to describe the bonding in methylamine. CH3NH2.arrow_forwardIdentify the hybrid orbitals used by boron in BCl3 and in BCl4, the ion formed from the reaction of BCl3 and Cl. Explain your choices.arrow_forward
- Consider the polyatomic ion IO65-. How many pairs of electrons are around the central iodine atom? What is its hybridization? Describe the geometry of the ion.arrow_forwarda Nitrogen trifluoride, NF3, is a relatively unreactive, colorless gas. How would you describe the bonding in the NF3 molecule in terms of valence bond theory? Use hybrid orbitals. b Silicon tetrafluoride, SiF4, is a colorless gas formed when hydrofluoric acid attacks silica (SiO2) or glass. Describe the bonding in the SiF4 molecule, using valence bond theory.arrow_forwardIn the molecular orbital mode l, compare and contrast bonds with bonds. What orbitals form the bonds and what orbitals form the bonds? Assume the z-axis is the internuclear axis.arrow_forward
- In addition to NF3, two other fluoro derivatives of nitrogen are known: N2F4 and N2F2. What shapes do you predict for these two molecules? What is the hybridization for the nitrogen in each molecule?arrow_forwardDraw the Lewis structure for 1, 1-dimethylhydrazine [(CH3)2NNH2, a compound used as a rocket fuel]. What: is the hybridization for the two nitrogen atoms in this molecule? What orbitals overlap to form the bond between the nitrogen atoms?arrow_forwardThe sulfamate ion, H2NSO3, can be thought of as having been formed from the amide ion, NH2, and sulphur trioxide, SO3. (a) What are the electron-pair and molecular geometries or the amide ion and or SO3? What are the hybridizations of the N and S atoms, respectively? (b) Sketch a structure for the sulfamate ion, and estimate the bond angles. (c) What changes in hybridization do you expect for N and S in the course of the reaction NH2 + SO3 H2NSO3? (d) Is SO3 the donor of an electron pair or the acceptor of an electron pair in the reaction with amide ion? Does the electrostatic potential map shown below confirm your prediction?arrow_forward
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Linear Combination of Atomic Orbitals LCAO; Author: Edmerls;https://www.youtube.com/watch?v=nq1zwrAIr4c;License: Standard YouTube License, CC-BY
Quantum Molecular Orbital Theory (PChem Lecture: LCAO and gerade ungerade orbitals); Author: Prof Melko;https://www.youtube.com/watch?v=l59CGEstSGU;License: Standard YouTube License, CC-BY