Concept explainers
(a)
Interpretation: The electronic configuration and the bond order for the given diatomic species, using the molecular orbital model is to be determined. The paramagnetic species are to be identified.
Concept introduction: The electronic configuration for multi-electron diatomic is written using the molecular orbitals, derived from the
The bond order is calculated by difference between the anti-bonding electrons and the bonding electrons by two. This can be stated as,
As the bond order increases, the stability also increases.
The species have an unpaired electron in their valence shell are known as paramagnetic species.
To determine: The electronic configuration, bond order and the paramagnetic nature of
(b)
Interpretation: The electronic configuration and the bond order for the given diatomic species, using the molecular orbital model is to be determined. The paramagnetic species are to be identified.
Concept introduction: The electronic configuration for multi-electron diatomic is written using the molecular orbitals, derived from the
The bond order is calculated by difference between the anti-bonding electrons and the bonding electrons by two. This can be stated as,
As the bond order increases, the stability also increases.
The species have an unpaired electron in their valence shell are known as paramagnetic species.
To determine: The electronic configuration, bond order and the paramagnetic nature of
(c)
Interpretation: The electronic configuration and the bond order for the given diatomic species, using the molecular orbital model is to be determined. The paramagnetic species are to be identified.
Concept introduction: The electronic configuration for multi-electron diatomic is written using the molecular orbitals, derived from the
The bond order is calculated by difference between the anti-bonding electrons and the bonding electrons by two. This can be stated as,
As the bond order increases, the stability also increases.
The species have an unpaired electron in their valence shell are known as paramagnetic species.
To determine: The electronic configuration, bond order and the paramagnetic nature of
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Chemistry: An Atoms First Approach
- • explain how hybridization reconciles observed molecular shapes with the orbital overlap model.arrow_forwardPredict the valence electron molecular orbital configurations for the following, and state whether they will be stable or unstable ions. (a) Na,2+ (b) Mg,2 (c) AI,2 (d) Si,2 (e) p2+ (f) s,2 (g) F,2 (h) Ar,2 40. Predict the valence electron molecular orbital configurations for the following, and state whether they will be stable or unstable ions. (a) Na22+ (b) Mg22+ (c) Al22+ (d) Si22+ (e) P22+ (f) S22+ (g) F22+ (h) Ar22+arrow_forward7.59 What type of hybrid orbital is generated by combining the valence s orbital and all three valence p orbitals of an atom? How many hybrid orbitals result?arrow_forward
- Methylcyanoacrylate is the active ingredient in super glues. Its Lewis structure is (a) How many sigma bonds are in the molecule? (b) How many pi bonds are in the molecule? (c) What is the hybridization of the carbon atom bonded to nitrogen? (d) What is the hybridization of the carbon atom bonded to oxygen? (e) What is the hybridization of the double-bonded oxygen?arrow_forwardIdentify the molecules with a dipole moment: (a) SF4 (b) CF4 (c) Cl2CCBr2 (d) CH3Cl (e) H2COarrow_forwardWhen two amino acids react with each other, they form a linkage called an amide group, or a peptide link. (If more linkage. are added, a protein or polypeptide is formed.) (a) What are the hybridizations of the C and N atoms in the peptide linkage? (b) Is the structure illustrated the only resonance structure possible for the peptide linkage? If another resonance structure is possible. compare it with the o ne shown. Decide which is the more important structure. (c) The computer-generated structure shown here, which contains a peptide linkage, shows that this linkage is flat. This is an important feature of proteins. Speculate on reasons that the CONH linkage is planar. What are the sites of positive and negative charge in this dipeptide?arrow_forward
- a Mercury(II) chloride dissolves in water to give poorly conducting solutions, indicating that the compound is largely nonionized in solutionit dissolves as HgCl2 molecules. Describe the bonding of the HgCl2 molecule, using valence bond theory. b Phosphorus trichloride, PCl3, is a colorless liquid with a highly irritating vapor. Describe the bonding in the PCl3 molecule, using valence bond theory. Use hybrid orbitals.arrow_forwardFClO2 and F3ClO can both gain a fluoride ion to form stable anions. F3ClO and F3ClO2 will both lose a fluoride ion to form stable cations. Draw the Lewis structures and describe the hybrid orbitals used by chlorine in these ions.arrow_forward3. What hybridization and molecular geometry would you expect for the underlined atom in each of the following (Hint: Drawing Lewis structures is a very good place to start.)? Are these polar or non-polar molecules? If a molecule is polar, indicate the direction of the polarity using the crossed arrow notation. a. CH₂O b. BH4 C. SO3 d. CBr3H e. SCI5I f. AsF5arrow_forward
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