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chemistry a molecular approach
Chemistry A Molecular Approach 5th Edition Nivaldo Tro - Solutions
Write a hybridization and bonding scheme for bromine trifluoride, BrF3.
What is the molecular geometry about nitrogen in CH3NH2?(a) Trigonal planar (b) Tetrahedral (c) Trigonal pyramidal (d) Bent
Determine the hybridization about carbon in H2CO.a) sp b) sp2 c) sp3d) sp3d
How do you determine whether a molecule is polar? Why is polarity important?
Write a hybridization and bonding scheme for acetaldehyde, O H3C-C-H
A molecule contains three identical polar bonds in a trigonal planar molecular geometry. Is the molecule polar?(a) Yes (b) No (c) Unable to determine whether the molecule is polar without more information
According to valence bond theory, which kind of orbitals overlap to form the P—Cl bonds in PCl5? a) P(sp³) -Cl(p) b) P(sp³d) - Cl(s) c) P(sp³) -Cl(s) d) P(sp³d) - Cl(p)
What is a chemical bond according to valence bond theory?
Use valence bond theory to write a hybridization and bonding scheme for ethene, H2C = CH2.
The answer to the question “What is a chemical bond?” depends on the bonding model. What is a chemical bond according to valence bond theory?(a) Lone electron pair (b) The overlap between half-filled atomic orbitals on two atoms (c) The overlap between filled atomic orbitals on two atoms (d)
Apply MO theory to determine the bond order in C2.a) 0 b) 1 c) 2 d) 3
In valence bond theory, what determines the geometry of a molecule?
Use MO theory to predict the bond order in H2–. Is the H2– bond a stronger or weaker bond than the H2 bond?
How many sp3 hybrid orbitals result from the hybridization of one s and three p orbitals?(a) 1 (b) 2 (c) 3 (d) 4
Apply MO theory to predict which species has the strongest bond.a) N2 b) N2– c) N2+d) All bonds are equivalent according to MO theory.
In valence bond theory, the interaction energy between the electrons and nucleus of one atom with the electrons and nucleus of another atom is usually negative (stabilizing) when ____________ .
Draw an MO energy diagram and determine the bond order for the N2– ion. Do you expect the bond in the N2– ion to be stronger or weaker than the bond in the N2 molecule? Is N2–diamagnetic or paramagnetic?
We learned that double bonds are stronger and shorter than single bonds. For example, a C—C single bond has an average bond energy of 347 kJ/mole, whereas a C = C double bond has an average bond energy of 611 kJ/mole. According to valence bond theory, why is a double bond not simply twice as
Apply MO theory to determine which molecule is diamagnetic.a) CO b) B2 c) O2d) None of the above (all are paramagnetic)
What is hybridization? Why is hybridization necessary in valence bond theory?
Use MO theory to determine the bond order of the CN– ion. Is the ion paramagnetic or diamagnetic?
What is the hybridization of C in CO2?(a) sp(b) sp2(c) sp3
Which hybridization scheme occurs about nitrogen when nitrogen forms a double bond?a) sp b) sp2 c) sp3d) sp3d
How does hybridization of the atomic orbitals in the central atom of a molecule help lower the overall energy of the molecule?
What is the bond order for a second-period diatomic molecule containing three electrons in antibonding molecular orbitals and six electrons in bonding molecular orbitals?(a) 1 (b) 1.5 (c) 2 (d) 2.5
Which molecular geometry results when a central atom has five total electron groups, with three of those being bonding groups and two being lone pairs?a) Trigonal bipyramidalb) Seesawc) T-shapedd) Bent
How is the number of hybrid orbitals related to the number of standard atomic orbitals that are hybridized?
What is a chemical bond according to MO theory?(a) According to MO theory, a chemical bond is the overlap between half-filled atomic orbitals.(b) According to MO theory, a chemical bond is a shared electron pair.(c) According to MO theory, atoms join together (or bond) when the electrons in the
Determine the correct molecular geometry (from left to right) about each interior atom in CH3CH2OH.a) 1st C tetrahedral; 2nd C trigonal planar; O linearb) 1st C trigonal planar; 2nd C bent; O linearc) 1st C trigonal planar; 2nd C trigonal pyramidal; O bentd) 1st C tetrahedral; 2nd C tetrahedral; O
Sketch each set of hybrid orbitals.a. sp b. sp2 c. sp3 d. sp3d e. sp3d2
The central atom in a molecule has a bent molecular geometry. Determine the hybridization of the orbitals in the atom.a) sp b) sp2 c) sp3d) Hybridization cannot be determined from the information given.
In the Lewis model, the two bonds in a double bond look identical.However, valence bond theory shows that they are not.Describe a double bond according to valence bond theory.Explain why rotation is restricted about a double bond but not about a single bond.
Explain the difference between hybrid atomic orbitals in valence bond theory and LCAO molecular orbitals in MO theory.
What is a chemical bond according to MO theory?
Name the hybridization scheme that corresponds to each electron geometry.a. Linearb. Trigonal planarc. Tetrahedrald. Trigonal bipyramidale. Octahedral
What is a bonding molecular orbital?
What is an antibonding molecular orbital?
What is the role of wave interference in determining whether a molecular orbital is bonding or antibonding?
In MO theory, what is bond order? Why is it important?
How is the number of molecular orbitals approximated by a linear combination of atomic orbitals related to the number of atomic orbitals used in the approximation?
Sketch each molecular orbital.a. σ2sb. σ*2σ c. σ2pd. σ*2p e. π2pf. π*2p
Draw an energy diagram for the molecular orbitals of period 2 diatomic molecules. Show the difference in ordering for B2, C2, and N2 compared to O2, F2, and Ne2.
Why does the energy ordering of the molecular orbitals of the period 2 diatomic molecules change in going from N2 to O2?
Explain the difference between a paramagnetic species and a diamagnetic one.
When applying MO theory to heteronuclear diatomic molecules, the atomic orbitals used may be of different energies. If two atomic orbitals of different energies make two molecular orbitals, how are the energies of the molecular orbitals related to the energies of the atomic orbitals? How is the
In MO theory, what is a nonbonding orbital?
Write a short paragraph describing chemical bonding according to the Lewis model, valence bond theory, and MO theory.Indicate how the theories differ in their description of a chemical bond and describe the strengths and weaknesses of each theory. Which theory is correct?
A molecule with the formula AB3 has a trigonal pyramidal geometry.How many electron groups are on the central atom (A)?
A molecule with the formula AB3 has a trigonal planar geometry.How many electron groups are on the central atom?
For each molecular geometry, list the number of total electron groups, the number of bonding groups, and the number of lone pairs on the central atom. (a) (b) (c)
For each molecular geometry, list the number of total electron groups, the number of bonding groups, and the number of lone pairs on the central atom. နာ (a) (b) (c)
Determine the electron geometry, molecular geometry, and idealized bond angles for each molecule. In which cases do you expect deviations from the idealized bond angle?a. PF3 b. SBr2 c. CHCl3 d. CS2
Determine the electron geometry, molecular geometry, and idealized bond angles for each molecule. In which cases do you expect deviations from the idealized bond angle?a. CF4 b. NF3 c. OF2 d. H2S
Which species has the smaller bond angle, H3O+ or H2O? Explain.
Which species has the smaller bond angle, ClO4– or ClO3–? Explain.
Determine the molecular geometry and sketch each molecule or ion using the bond conventions shown in “Representing Molecular Geometries on Paper” in Section 11.4.a. SF4 b. ClF3 c. IF2– d. IBr4–
Determine the molecular geometry about each interior atom and sketch each molecule.a. C2H2 (skeletal structure HCCH)b. C2H4 (skeletal structure H2CCH2)c. C2H6 (skeletal structure H3CCH3)
Determine the molecular geometry about each interior atom and sketch each molecule.a. N2b. N2H2 (skeletal structure HNNH)c. N2H4 (skeletal structure H2NNH2)
Each ball-and-stick model shows the electron and molecular geometry of a generic molecule. Explain what is wrong with each molecular geometry and provide the correct molecular geometry, given the number of lone pairs and bonding groups on the central atom. (a) (b) (c)
Determine the geometry about each interior atom in each molecule and sketch the molecule. (Skeletal structure is indicated in parentheses.)a. CH3OH(H3COH) b. CH3OCH3(H3COCH3)c. H2O2(HOOH)
Each ball-and-stick model shows the electron and molecular geometry of a generic molecule. Explain what is wrong with each molecular geometry and provide the correct molecular geometry, given the number of lone pairs and bonding groups on the central atom. (a) (b) (c)
Determine the geometry about each interior atom in each molecule and sketch the molecule. (Skeletal structure is indicated in parentheses.)a. CH3NH2(H3CNH2)b. CH3CO2CH3 (H3CCOOCH3 one O atom attached to 2nd C atom; the other O atom is bonded to the 2nd and 3rd C atom)c. NH2CO2H (H2NCOOH both O
Explain why CO2 and CCl4 are both nonpolar, even though they contain polar bonds.
CH3F is a polar molecule, even though the tetrahedral geometry often leads to nonpolar molecules. Explain.
Determine whether each molecule in Exercise 35 is polar or nonpolar.Exercise 35Determine the electron geometry, molecular geometry, and idealized bond angles for each molecule. In which cases do you expect deviations from the idealized bond angle?a. PF3 b. SBr2 c. CHCl3 d. CS2
Determine whether each molecule in Exercise 36 is polar or nonpolar.Exercise 36Determine the electron geometry, molecular geometry, and idealized bond angles for each molecule. In which cases do you expect deviations from the idealized bond angle?a. PF3 b. SBr2 c. CHCl3 d. CS2
Determine whether each molecule is polar or nonpolar.a. SCl2 b. SCl4 c. BrCl5
Determine whether each molecule is polar or nonpolar.a. SiCl4 b. CF2Cl2c. SeF6 d. IF5
The valence electron configurations of several atoms are shown here. How many bonds can each atom make without hybridization?a. Be 2s2 b. P 3s23p3 c. F 2s22p5
Give the correct electron and molecular geometries that correspond to each set of electron groups around the central atom of a molecule.a. Four electron groups overall; three bonding groups and one lone pair.b. Four electron groups overall; two bonding groups and two lone pairs.c. Five electron
The valence electron configurations of several atoms are shown here. How many bonds can each atom make without hybridization?a. B 2s22p1 b. N 2s22p3 c. O 2s22p4
Write orbital diagrams (boxes with arrows in them) to represent the electron configurations—without hybridization—for all the atoms in PH3. 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
Write 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
Write orbital diagrams (boxes with arrows in them) to represent the electron configuration of carbon before and after sp3 hybridization.
Write orbital diagrams (boxes with arrows in them) to represent the electron configurations of carbon before and after sp hybridization.
Which hybridization scheme allows the formation of at least one π bond? sp³, sp², sp³d²
For each compound, draw the Lewis structure, determine the geometry using VSEPR theory, determine whether the molecule is polar, identify the hybridization of all interior atoms, and make a sketch of the molecule, according to valence bond theory, showing orbital overlap.a. IF5 b. CH2CHCH3 c.
Most vitamins can be classified as either fat soluble, which results in their tendency to accumulate in the body (so that taking too much can be harmful), or water soluble, which results in their tendency to be quickly eliminated from the body in urine. Examine the structural formulas and
Water does not easily remove grease from dishes or hands because grease is nonpolar and water is polar. The addition of soap to water, however, allows the grease to dissolve. Study the structure of sodium stearate (a soap) and describe how it works. CH3(CH₂) 16C-ONa+
Draw a molecular orbital energy diagram for ClF. (Assume that the σp orbitals are lower in energy than the p orbitals.) What is the bond order in ClF?
Draw Lewis structures and MO diagrams for CN+, CN, and CN–.According to the Lewis model, which species is most stable?According to MO theory, which species is most stable? Do the two theories agree?
Bromine can form compounds or ions with any number of fluorine atoms from one to five. Write the formulas of all five of these species, assign a hybridization, and describe their electron and molecular geometry.
Sketch the bonding and antibonding molecular orbitals that result from linear combinations of the 2px atomic orbitals in a homonuclear diatomic molecule. (The 2px orbitals are those whose lobes are oriented along the bonding axis.)
Draw an MO energy diagram and predict the bond order of Li2 + and Li2–. Do you expect these molecules to exist in the gas phase?
Draw an MO energy diagram and predict the bond order of Be2+ and Be2–. Do you expect these molecules to exist in the gas phase?
Sketch the bonding and antibonding molecular orbitals that result from linear combinations of the 2pz atomic orbitals in a homonuclear diatomic molecule. (The 2pz orbitals are those whose lobes are oriented perpendicular to the bonding axis.)How do these molecular orbitals differ from those
Using the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the π2p orbitals lie at lower energy than the σ2p draw MO energy diagrams and predict the bond order in a molecule or ion with each number of total valence electrons. Will the molecule or ion be
Use MO theory to predict if each molecule or ion exists in a relatively stable form. 2- a. H₂²- b. Ne₂ 2+ c. He₂²+ 2- d. F₂²-
Using the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the π2p orbitals lie at higher energy than the σ2p, draw MO energy diagrams and predict the bond order in a molecule or ion with each number of total valence electrons. Will the molecule or ion be
Use MO theory to predict if each molecule or ion exists in a relatively stable form. a. C₂²+ b. Liz C. Be₂2+ d. Li₂² 2-
According to MO theory, which molecule or ion has the highest bond order? Highest bond energy? Shortest bond length? C₂, C₂, C₂
According to MO theory, which molecule or ion has the highest bond order? Highest bond energy? Shortest bond length? 2- 02, 0₂, 0₂²
Draw an MO energy diagram for CO. (Use the energy ordering of O2.) Predict the bond order and make a sketch of the lowest energy bonding molecular orbital.
Draw an energy diagram for HCl. Predict the bond order and make a sketch of the lowest energy bonding molecular orbital.
For each compound, draw the Lewis structure, determine the geometry using VSEPR theory, determine whether the molecule is polar, identify the hybridization of all interior atoms, and make a sketch of the molecule, according to valence bond theory, showing orbital overlap.a. COF2 (carbon is the
Sketch the antibonding molecular orbital that results from the linear combination of two 1s orbitals. Indicate the region where interference occurs and state the kind of interference (constructive or destructive).
Amino acids are biological compounds that link together to form proteins, the workhorse molecules in living organisms.The skeletal structures of several simple amino acids are shown here. For each skeletal structure, complete the Lewis structure, determine the geometry and hybridization about each
The genetic code is based on four different bases with the structures shown here. Assign a geometry and hybridization to each interior atom in these four bases.a. Cytosine b. Adenine c. Thymine d. Guanine H₂C HC6 HC. HC 6 5 INI N. C N H ZHL NH₂ (a) +0100 20 =0 N WN 2C=0 NH H₂N NH₂ HC
The structure of caffeine, present in coffee and many soft drinks, is shown here. How many pi bonds are present in caffeine?How many sigma bonds? Insert the lone pairs in the molecule.What kinds of orbitals do the lone pairs occupy? H3C 0 N 0 'C CH3 -N N CH3 CH
The structure of acetylsalicylic acid (aspirin) is shown here. How many pi bonds are present in acetylsalicylic acid? How many sigma bonds? What parts of the molecule are free to rotate?What parts are rigid? HC HC C. CH OH CH CH3
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