(a)
Interpretation:
The shapes of the resulting bonding and anti-bonding
Concept introduction:
The linear combination of atomic orbital (LCAO) states that two atomic orbitals combine together to form a new orbital which is known as bonding molecular orbital.
The molecular orbital theory also states that two atoms combines together to form a molecule. During the formation of a molecule, the electrons are shared between two atoms to form a
(b)
Interpretation:
The total number of nodes in the given molecular orbitals is to be stated.
Concept introduction:
The linear combination of atomic orbital (LCAO) states that two atomic orbitals combine together to form a new orbital which is known as bonding molecular orbital.
The molecular orbital theory also states that two atoms combines together to form a molecule. During the formation of a molecule, the electrons are shared between two atoms to form a chemical bond.
(c)
Interpretation:
The orbital interaction diagram for side-to-side molecular orbital formation is to be shown.
Concept introduction:
The linear combination of atomic orbital (LCAO) states that two atomic orbitals combine together to form a new orbital which is known as bonding molecular orbital.
The molecular orbital theory also states that two atoms combines together to form a molecule. During the formation of a molecule, the electrons are shared between two atoms to form a chemical bond.
(d)
Interpretation:
The validation corresponding to the fact that whether the resulting bond is
Concept introduction:
The linear combination of atomic orbital (LCAO) states that two atomic orbitals combine together to form a new orbital which is known as bonding molecular orbital.
The molecular orbital theory also states that two atoms combines together to form a molecule. During the formation of a molecule, the electrons are shared between two atoms to form a chemical bond.
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EBK ORGANIC CHEMISTRY STUDY GUIDE AND S
- Use valence bond theory to explain the bonding in F2, HF, and ClBr. (a) F2 This molecule is symmetrical. The single bond present in this molecule is derived from the overlap of two (1s, 2s, 2p, 3s, 3d, 3p, 4s, 4d, 4p) orbitals contributed by each of the F atoms. (b) HF This molecule is asymmetrical. The single bond present in this molecule is derived from the overlap of one (1s, 2s, 2p, 3s, 3d, 3p, 4s, 4d, 4p) orbital contributed by the H atom and one (1s, 2s, 2p, 3s, 3d, 3p, 4s, 4d, 4p) orbital contributed by the F atom. (c) ClBr This molecule is also asymmetrical. The single bond present in this molecule is derived from the overlap of one (1s, 2s, 2p, 3s, 3d, 3p, 4s, 4d, 4p) orbital contributed by the Cl atom and one (1s, 2s, 2p, 3s, 3d, 3p, 4s, 4d, 4p) orbital contributed by the Br atom. Sketch the overlap of the atomic orbitals involved in the bonds.arrow_forward2. Consider the following molecules or ions: CIOF5, NOBr, NH2F, and XeO2F3+. 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°?arrow_forwardConsider the reaction BF3 + NH3 -> F3B-NH3 (a) Describe the changes in hybridization of the B and N atoms as a result of this reaction. (b) Describe the shapes of all the reactant molecules with their bond angles. (c) Draw the overall shape of the product molecule and identify the bond angles around B and N atoms. (d) What is the name of the bond between B and N. (e)Describe the bonding orbitals that make the B and F, B and N & N and H bonds in the product molecule.arrow_forward
- Butadiene, C4H6, is a planar molecule that has the followingcarbon–carbon bond lengths: (a) Predict the bond angles around each of the carbon atoms and sketch the molecule. (b) From left to right, what is the hybridization of each carbon atom in butadiene? (c) The middle C—C bond length in butadiene (1.48 Å) is a little shorter than the average C—C single bond length (1.54 Å). Does this imply that the middle C—C bond in butadiene is weaker or stronger than the average C—C single bond? (d) Based on your answer for part (c), discuss what additional aspects of bonding in butadiene might support the shorter middle C—C bond.arrow_forwardIn following decomposition reaction:2C3H8(g)⟶ C2H4(g)+ C3H6(g) + CH4(g) + H2(g)For each of the four carbon compounds, do the following: (a) Draw Lewis structure.(b) Predict the geometry about the carbon atom.(c) Determine the hybridization of each type of carbon atom.arrow_forwardThe molecular orbitals depicted below are derived from 2p atomic orbitals in F₂⁺. (a) Give the orbital designations. (b) Which is occupied by at least one electron in F₂⁺? (c) Which is occupied by only one electron in F₂⁺?arrow_forward
- For each statement, indicate whether it is true or false. (a) The greater the orbital overlap in a bond, the weaker the bond. [b] The greater the orbital overlap in a bond, the shorter the bond. [c] To create a hybrid orbital, you could use the s orbital on one atom with a p orbital on another atom. [d] Nonbonding electron pairs cannot occupy a hybrid orbital.arrow_forwardAzo dyes are organic dyes that are used for many applications,such as the coloring of fabrics. Many azo dyes arederivatives of the organic substance azobenzene, C12H10N2.A closely related substance is hydrazobenzene, C12H12N2.The Lewis structures of these two substances are given (Recall the shorthand notation used for benzene.)(a) What is the hybridization at the N atom in each of thesubstances? (b) How many unhybridized atomic orbitalsare there on the N and the C atoms in each of the substances?(c) Predict the N—N—C angles in each of thesubstances. (d) Azobenzene is said to have greater delocalizationof its π electrons than hydrazobenzene. Discussthis statement in light of your answers to (a) and (b). (e) Allthe atoms of azobenzene lie in one plane, whereas thoseof hydrazobenzene do not. Is this observation consistentwith the statement in part (d)? (f) Azobenzene is an intensered-orange color, whereas hydrazobenzene is nearly colorless.Which molecule would be a better one to use in…arrow_forward(a) How does a polar molecule differ from a nonpolar one? (b) Atoms X and Y have different electronegativities. Will the diatomic molecule X—Y necessarily be polar? Explain. (c) What factors affect the size of the dipole moment of a diatomic molecule?arrow_forward
- In hydrogen isocyanide molecules (HCN), both carbon (C: 1s2 2s2 2p2 ) and nitrogen (N: 1s2 2s2 2p3 ) atoms undergo sp hybridization. (a) Use Orbital Hybridization theory to determine the molecular shape of HCN molecules. (b) Explain how the C atom binds to the N atom in HCN molecules.arrow_forwardWhich molecule in each pair has the greater dipole mo-ment? Give the reason for your choice.(a) ClO₂ or SO₂(b) HBr or HCl(c) BeCl₂ or SCl₂(d) AsF₃ or AsF₅arrow_forward(a) An AB6 molecule has no lone pairs of electrons on the Aatom. What is its molecular geometry? (b) An AB4 moleculehas two lone pairs of electrons on the A atom (in additionto the four B atoms). What is the electron-domain geometryaround the A atom? (c) For the AB4 molecule in part (b), predictthe molecular geometry.arrow_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning