(a)
Interpretation:
Whether the given species have permanent dipole moment or not is to be predicted.
Concept introduction:
Dipole moment is defined as the product of the distance and the amount of charge. Dipole moment arises due to the difference in the electronegativity of the atom or ions in a molecule. The dipole moment is from lower electronegative atom to higher electronegative atom.
(b)
Interpretation:
Whether the given species have permanent dipole moment or not is to be predicted.
Concept introduction:
Dipole moment is defined as the product of the distance and the amount of charge. Dipole moment arises due to the difference in the electronegativity of the atom or ions in a molecule. The dipole moment is from lower electronegative atom to higher electronegative atom.
(c)
Interpretation:
Whether the given species have permanent dipole moment or not is to be predicted.
Concept introduction:
Dipole moment is defined as the product of the distance and the amount of charge. Dipole moment arises due to the difference in the electronegativity of the atom or ions in a molecule. The dipole moment is from lower electronegative atom to higher electronegative atom.
(d)
Interpretation:
Whether the given species have permanent dipole moment or not is to be predicted.
Concept introduction:
Dipole moment is defined as the product of the distance and the amount of charge. Dipole moment arises due to the difference in the electronegativity of the atom or ions in a molecule. The dipole moment is from lower electronegative atom to higher electronegative atom.
(e)
Interpretation:
Whether the given species have permanent dipole moment or not is to be predicted.
Concept introduction:
Dipole moment is defined as the product of the distance and the amount of charge. Dipole moment arises due to the difference in the electronegativity of the atom or ions in a molecule. The dipole moment is from lower electronegative atom to higher electronegative atom.
(e)
Interpretation:
Whether the given species have permanent dipole moment or not is to be predicted.
Concept introduction:
Dipole moment is defined as the product of the distance and the amount of charge. Dipole moment arises due to the difference in the electronegativity of the atom or ions in a molecule. The dipole moment is from lower electronegative atom to higher electronegative atom.
Want to see the full answer?
Check out a sample textbook solutionChapter 13 Solutions
Physical Chemistry
- Show, if overlap is ignored, (a) that if a molecular orbital is expressed as a linear combination of two atomic orbitals in the form ψ = ψA cos θ + ψB sin θ, where θ is a parameter that varies between 0 and π, with ψA and ψB are orthogonal and normalized to 1, then ψ is also normalized to 1. (b) To what values of θ do the bonding and antibonding orbitals in a homonuclear diatomic molecule correspond?arrow_forwardIdentify the likely structure dipole moment of the theoretical molecule C(OH)3Cl. Provide a hand-drawn illustration showing the molecule's 3D structure and dipole moment if applicable.arrow_forwardIf an electron is removed from a fluorine molecule, an F+2molecular ion forms.(a) Give the molecular electron configurations for F2 and F+2 (for the MOs constructed from valence AOs).(b) Give the bond order of each species.(c) Predict which species should be paramagnetic.(d) Predict which species has the greater bond dissociation energy.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_forwardAcetylene (C2H2) has a tendency to lose two protons (H+) and form the carbide ion (C22−), which is present in a number of ionic compounds, such as CaC2 and MgC2. (a) What is the bond order of the carbide dianion C22−? (b) For comparison, what is the bond order of C2?arrow_forwardThe strength of a covalent bond depends upon the size of the atoms and the bond order. In general short bonds are strong bonds. For each pair of covalently bonded atoms, choose the one expected to have the higher bond energy.(A) N≡N(B) N-N ...... (A,B) fill in the blank 1(C) C=O(D) C≡O ...... (C,D) fill in the blank 2arrow_forward
- Organic compounds (a) A simple molecule with alternating single and double bonds is buta-1,3-diene. (i) Draw its skeletal structure. (ii) Write its molecular formula and empirical formula. (iii) How many carbon atoms have sp2 hybridization in buta-1,3-diene?arrow_forwardA benzene molecule can be modeled as six carbon atoms arrangedin a regular hexagon in a plane. At each carbon atom, one of threeradicals NH2, COOH, or OH can be attached. How many suchcompoundsare possible?arrow_forwardThe molecule shown here is difluoromethane 1CH2F22, which isused as a refrigerant called R-32. (a) Based on the structure, howmany electron domains surround the C atom in this molecule?(b) Would the molecule have a nonzero dipole moment? (c) Ifthe molecule is polar, which of the following describes the directionof the overall dipole moment vector in the molecule:(i) from the carbon atom toward a fluorine atom, (ii) from thecarbon atom to a point midway between the fluorine atoms,(iii) from the carbon atom to a point midway between the hydrogenatoms, or (iv) from the carbon atom toward a hydrogenatom? [Sections 9.2 and 9.3]9.5arrow_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_forwardThe substance chlorine monoxide, ClO(g), is important inatmospheric processes that lead to depletion of the ozonelayer. The ClO molecule has an experimental dipole momentof 1.24 D, and the Cl¬O bond length is 1.60 Å. (a)Determine the magnitude of the charges on the Cl and Oatoms in units of the electronic charge, e. (b) Based on theelectronegativities of the elements, which atom would youexpect to have a partial negative charge in the ClO molecule?(c) Using formal charges as a guide, propose the dominantLewis structure for the molecule. (d) The anion ClOexists.What is the formal charge on the Cl for the best Lewisstructure for ClO-?arrow_forwardUsing hybridization, predict how the bond length of the C − C σ bond in HC ≡ C − C ≡ CH should compare with the C − C σ bonds in CH3CH3 and CH2 = CH − CH = CH2.arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY