4.a) For the following descriptions of molecules, draw the Lewis structure of the molecule and show allbond angles (assuming ideal VSEPR angles).An organic compound with the molecular formula HĄCN20. Both N atoms are sp3 hybridized, while Cand O are sp? hybridized.i.An organic compound with the molecular formula CNS-. C is sp hybridized, while N and S are sp?hybridized.ii.:=

We would use the given hybridization to determine the shape around that atom and central atom.

4. a) For the following descriptions of molecules, draw the Lewis structure of the molecule and show all bond angles (assuming ideal VSEPR angles). An organic compound with the molecular formula H,CN2O. Both N atoms are sp³ hybridized, while C and O are sp? hybridized. i. An organic compound with the molecular formula CNS-. C is sp hybridized, while N and S are sp? hybridized. ii.

4. a) For the following descriptions of molecules, draw the Lewis structure of the molecule and show all bond angles (assuming ideal VSEPR angles). An organic compound with the molecular formula H,CN2O. Both N atoms are sp³ hybridized, while C and O are sp? hybridized. i. An organic compound with the molecular formula CNS-. C is sp hybridized, while N and S are sp? hybridized. ii.

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...

See similar textbooks

Similar questions

b. PCIS dal How many and what type(s) of bonds (single, double, triple) are on the carbon? single How many lone pair electrons are in the structure? What is the electron orientation? trigonal by pyramital What is the shape of the molecule? What is the hybridization on the central atom? What is the hybridization of each chlorine?
Determine a hybridization and bonding scheme for COIH. Draw its Lewis structure. Determine the hybridization, electron and molecular geometry for the central atom and the number of o and T bonds. Sketch the molecule including overlapping orbitals, label all bonds. (Make sure overlapping orbitals are the appropriate shape orbital that is ½ filled and can share an electron.). Is this molecule polar or non-polar?
In each of the groups below, all molecules except one share the same orbital hybridization of the central atom. Identify which molecule is different, and name the hybridization for that molecule and the rest of the group. a) NO3", CO32", SO;2", BCI3 b) H2S, SIF4, SeO2, PB13 c) HCN, N2O, NO2", CS2 (Hint: N is the central atom in N2O) d) ClO3", NC13, AlCl3, H3O*
Acetic acid can be made by the oxidation of acetaldehyde (CH;CHO). Molecules of acetaldehyde have a -CH; group, an oxygen atom, and a hydrogen atom attached to a carbon atom. Draw the Lewis diagram for this molecule, give the hybridization of each carbon atom, and describe the T orbitals and the number of electrons that occupy each one. Draw the three-dimensional structure of the molecule, showing all angles.
Resour The molecule 2-butene is able to undergo a process called cis-trans isomerization, where the molecule switches from being a cis- alkene to a trans-alkene. This transformation can be induced by light. स - x H. H3C H. light H3C CH3 CH3 What is the hybridization of the two central carbon atoms in 2-butene? sp O sp O sp The isomerization requires breaking the n bond. Use the table of bond energies to determine the approximate amount of energy (in joules) required to break the C-Ca bond in 2-butene, both per mole and per molecule. E = 2.61 x105 J/mol 4.33 x1019 E = J/molecule Incorrect What is the wavelength of light that would be required to perform the cis-trans isomerization of one molecule of 2-butene?
Fill the information in the following table by relying on the concepts studied in localized bonding models. (Lewis Structures, VSEPR and VBT) Compounds Effective Electron Pairs Hybridization IR Active (yes or no) CIFS XeF. H2S
B. Answer the next two questions about the Lewis structure of XYZ shown below. メー三 -YEz: I. What is the hybridization of the central atom? II. For all covalent bonds, specify the type of bond (o vs. T) and the atomic orbitals that overlap to form the bond. For example, in a molecule of H2, the only bond is o: H(s)-H(s).
Draw orbital diagrams (boxes with arrows in them) to represent the electron configurations—without hybridization—for all the atoms in SF2. Circle the electrons involved in bonding. Draw a three-dimensional sketch of the molecule and show orbital overlap. What bond angle do you expect from the unhybridized orbitals? How well does valence bond theory agree with theexperimentally measured bond angle of 98.2°?
6. Consider the molecule sulfur dioxide. Draw the Lewis structure such that it follows the octet rule. Include any formal charges. What is the electron geometry? What is the molecular shape? What are the expected bond angles? What kind of intermolecular forces does it have? How many sigma bonds are there? How many pi bonds? What is the hybridization of the sulfur atom? In the space below, sketch the hybridized orbitals.
Determine the hybridization of the marked N atom in tofacitinib, a drug used to treat rheumatoid arthritis. In what type of orbital does the lone pair on this N atom reside? (Lone pairs have been omitted in this structure.) N. ok N. nt tofacitinib N. nces sp hybridized; p orbital sp° hybridized; p orbital 3 sp° hybridized; sp orbital sp hybridized; sp orbital O sp hybridized; sp orbital NN 1. O O O
3. Carefully consider the relevant factors and then estimate the bond angles in the molecule NO:Cl. Draw the Lewis structures and show that the atom geometry is trigonal planar but the actual bond angles deviate from the ideal 120°. Two of the are 115°, and the other is 130°. Identify which two bond angles are 115°, and which bond angle is 130°.