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engineering
chemical engineering

Questions and Answers of Chemical Engineering

The ionic substance strontium oxide, SrO, forms from the reaction of strontium metal with molecular oxygen. The arrangement of the ions in solid SrO is analogous to that in solid NaCl (Figure
Explain the variation in ionization energies of carbon, as displayed in this graph:
Group 4A elements have much more negative electron affinities than their neighbors in groups 3A and 5A (see Figure 7.11). Suggest an explanation.
(a) Use orbital diagrams to illustrate what happens when an oxygen atom gains two electrons. (b) Why does O3- not exist?
Use electron configurations to explain the following observations: (a) The first ionization energy of phosphorus is greater than that of sulfur. (b) The electron affinity of nitrogen is lower (less
The electron affinities, in kJ / mol, for the group 1B and group 2B metals are(a) Why are the electron affinities of the group 2B elements greater than zero? (b) Why do the electron affinities of
Hydrogen is an unusual element because it behaves in some ways like the alkali metal elements and in other ways like nonmetals. Its properties can be explained in part by its electron configuration
The first ionization energy of the oxygen molecule is the energy required for the following process: O2 (g) → O2+ (g) + e- The energy needed for this process is 1175kJ/mol, very similar to the
A certain AB4 molecule has a "seesaw" shape:From which of the fundamental geometries shown in Figure 9.3 could you remove one or more atoms to create a molecule having this seesaw shape?
The diagram that follows shows the highest-energy occupied MOs of a neutral molecule CX, where element X is in the same row of the periodic table as C.(a) Based on the number of electrons, can you
The azide ion, N3-, is linear with two N-N bonds of equal length, 1.16 Ã….(a) Draw a Lewis structure for the azide ion.(b) With reference to Table 8.5, is the observed bond length
In ozone, O3, the two oxygen atoms on the ends of the molecule are equivalent to one another. (a) What is the best choice of hybridization scheme for the atoms of ozone? (b) For one of the
Butadiene, C4H6, is a planar molecule that has the following carbon-carbon bond lengths:(a) Predict the bond angles around each of the carbon atoms and sketch the molecule. (b) Compare the bond
The following sketches show the atomic orbital wave functions (with phases) used to construct some of the MOs of a homo-nuclear diatomic molecule. For each sketch, determine the type of MO that will
Write the electron configuration for the first excited state for N2 - that is, the state with the highest-energy electron moved to the next available energy level. (a) Is the nitrogen in its first
Azo dyes are organic dyes that are used for many applications, such as the coloring of fabrics. Many azo dyes are derivatives of the organic substance azo-benzene, C12H10N2. A closely related
(a) Using only the valence atomic orbitals of a hydrogen atom and a fluorine atom, and following the model of Figure 9.46, how many MOs would you expect for the HF molecule?(b) How many of the MOs
Carbon monoxide, CO, is iso-electronic to N2.(a) Draw a Lewis structure for CO that satisfies the octet rule.(b) Assume that the diagram in Figure 9.46 can be used to describe the MOs of CO. What is
The energy-level diagram in Figure 9.36 shows that the sideways overlap of a pair of p orbitals produces two molecular orbitals, one bonding and one anti-bonding. In ethylene there is a pair of
A compound composed of 2.1% H, 29.8% N, and 68.1% O has a molar mass of approximately 50 g/mol. (a) What is the molecular formula of the compound? (b) What is its Lewis structure if H is bonded to
An AB2 molecule is described as linear, and the A-B bond length is known. (a) Does this information completely describe the geometry of the molecule? (b) Can you tell how many nonbonding pairs of
Sulfur tetra-fluoride (SF4) reacts slowly with O2 to form sulfur tetra-fluoride monoxide (OSF4) according to the following unbalanced reaction:SF4 (g) + O2 (g) †’ OSF4 (g)The O atom and the
The phosphorus tri-halides (PX3) show the following variations in the bond angle X-P-X: PF3, 100.3o, PCl3, PBr3, 101.0o PI3, 102.0o. The trend is generally attributed to the change in the
The molecule 2-butene, C4H8, can undergo a geometric change called cis-trans isomerization:As discussed in the "Chemistry and Life" box on the chemistry of vision, such transformations can be induced
(a) Compare the bond enthalpies (Table 8.4) of the carbon-carbon single, double, and triple bonds to deduce an average -bond contribution to the enthalpy. What fraction of a single bond does this
Use average bond enthalpies (Table 8.4) to estimate for the atomization of benzene, C6H6: C6H6 (g) → 6C (g) + 6 H (g) Compare the value to that obtained by using ΔHof data given in Appendix C and
Many compounds of the transition-metal elements contain direct bonds between metal atoms. We will assume that the z-axis is defined as the metal-metal bond axis. (a) Which of the 3d orbitals (Figure
The organic molecules shown here are derivatives of benzene in which six-member rings are "fused" at the edges of the hexagons.(a) Determine the empirical formula of benzene and of these three
Antibonding molecular orbitals can be used to make bonds to other atoms in a molecule. For example, metal atoms can use appropriate d orbitals to overlap with the π*2p orbitals of the carbon
Methyl isocyanate, CH3NCO, was made infamous in 1984 when an accidental leakage of this compound from a storage tank in Bhopal, India, resulted in the deaths of about 3,800 people and severe and
(a) Methane (CH4) and the perchlorate ion are both described as tetrahedral. What does this indicate about their bond angles? (b) The NH3 molecule is trigonal pyramidal, while BF3 is trigonal planar.
How does a trigonal pyramid differ from a tetrahedron so far as molecular geometry is concerned?
Describe the bond angles to be found in each of the following molecular structures: (a) Planar trigonal, (b) Tetrahedral, (c) Octahedral, (d) Linear.
(a) What is meant by the term electron domain?(b) Explain in what way electron domains behave like the balloons in Figure 9.5.Why do they do so?
(a) How does one determine the number of electron domains in a molecule or ion? (b) What is the difference between a bonding electron domain and a nonbonding electron domain?
Would you expect the nonbonding electron-pair domain in NH3 to be greater or less in size than for the corresponding one in PH3? Explain.
In which of these molecules or ions does the presence of nonbonding electron pairs produce an effect on molecular shape, assuming they are all in the gaseous state? (a) SiH4, (b) PF3, (c) HBr, (d)
In which of the following molecules can you confidently predict the bond angles about the central atom, and for which would you be a bit uncertain? Explain in each case. (a) H2S, (b) BCl3, (c)
How many nonbonding electron pairs are there in each of the following molecules: (a) (CH3)2S, (b) HCN, (c) H2C2, (d) CH3F?
Describe the characteristic electron-domain geometry of each of the following numbers of electron domains about a central atom: (a) 3, (b) 4, (c) 5, (d) 6.
What is the difference between the electron-domain geometry and the molecular geometry of a molecule? Use the water molecule as an example in your discussion. Why do we need to make this distinction?
An AB3 molecule is described as having trigonal bipyramidal electron-domain geometry. How many nonbonding domains are on atom A? Explain.
Give the electron-domain and molecular geometries of a molecule that has the following electron domains on its central atom: (a) Four bonding domains and no nonbonding domains, (b) Three bonding
What are the electron-domain and molecular geometries of a molecule that has the following electron domains on its central atom? (a) Three bonding domains and no nonbonding domains, (b) Three
Give the electron-domain and molecular geometries for the following molecules and ions:(a) HCN(b) SO32-(c) SF4(d) PF6-(e) NH3Cl+(f) N3-
Draw the Lewis structure for each of the following molecules or ions, and predict their electron-domain and molecular geometries: (a) AsF3, (b) CH3+, (c) BrF3, (d) ClO3- (e) XeF2, (f) BrO2-.
The figure that follows shows ball-and-stick drawings of three possible shapes of an AF3 molecule.(a) For each shape, give the electron-domain geometry on which the molecular geometry is based.(b)
For each molecule (a)-(f), indicate how many different electron- domain geometries are consistent with the molecular geometry showna.b. c. d. e. f.
The figure that follows contains ball-and-stick drawings of three possible shapes of an AF4 molecule.(a) For each shape, give the electron-domain geometry on which the molecular geometry is based.(b)
Give the approximate values for the indicated bond angles in the following molecules:(a)(b) (c) (d)
In which of the following AFn molecules or ions is there more than one F-A-F bond angle: SiF4, PF5, SF4, AsF3?
The three species NH2-, NH3, and NH4+ have H-N-H bond angles of 105o, 107o, and 109o, respectively. Explain this variation in bond angles.
(a) Explain why BrF4- is square planar, whereas BF4- is tetrahedral. (b) How would you expect the H-X-H bond angle to vary in the series H2O, H2S, H2Se? Explain.
(a) Explain why the following ions have different bond angles: ClO2- and NO2-. Predict the bond angle in each case. (b) Explain why the XeF2 molecule is linear.
What is the distinction between a bond dipole and a molecular dipole moment?
Consider a molecule with formula AX3. Supposing the A-X bond is polar, how would you expect the dipole moment of the AX3 molecule to change as the X-A-X bond angle increases from 100o to 120o?
(a) Does SCl2 have a dipole moment? If so, in which direction does the net dipole point? (b) Does BeCl2 have a dipole moment? If so, in which direction does the net dipole point?
The molecule shown here is difluoromethane (CH2F2), which is used as a refrigerant called R-32.(a) Based on the structure, how many electron domains surround the C atom in this molecule?(b) Would the
(a) The PH3 molecule is polar. Does this offer experimental proof that the molecule cannot be planar? Explain. (b) It turns out that ozone, O3, has a small dipole moment. How is this possible, given
(a) Consider the AF3 molecules in Exercise 9.29.Which of these will have a nonzero dipole moment? Explain.(b) Which of the AF4 molecules in Exercise 9.30 will have a zero dipole moment?In Exercise
(a) What conditions must be met if a molecule with polar bonds is non-polar? (b) What geometries will signify non-polar molecules for AB2, AB3, and AB4 geometries?
Predict whether each of the following molecules is polar or non-polar: (a) IF (b) CS2 (c) SO3 (d) PCl3 (e) SF6 (f) IF5
Predict whether each of the following molecules is polar or non-polar: (a) CCl4 (b) NH3 (c) SF4 (d) XeF4 (e) CH3Br (f) GaH3
Dichloroethylene (C2H2Cl2) has three forms (isomers), each of which is a different substance. (a) Draw Lewis structures of the three isomers, all of which have a carbon-carbon double bond. (b) Which
Dichlorobenzene, C6H4Cl2, exists in three forms (isomers) called ortho, meta, and para:Which of these has a nonzero dipole moment? Explain.
(a) What is meant by the term orbital overlap? (b) Describe what a chemical bond is in terms of electron density between two atoms.
Draw sketches illustrating the overlap between the following orbitals on two atoms: (a) The 2s orbital on each atom, (b) The 2pz orbital on each atom (assume both atoms are on the z-axis), (c) The
Consider the bonding in an MgH2 molecule. (a) Draw a Lewis structure for the molecule, and predict its molecular geometry. (b) What hybridization scheme is used in MgH2? (c) Sketch one of the
The following plot shows the potential energy of two Cl atoms as a function of the distance between them.(a) To what does energy of zero correspond in this diagram?(b) According to the valence-bond
How would you expect the extent of overlap of the bonding atomic orbitals to vary in the series IF, ICl, IBr, and I2? Explain your answer.
Fill in the blank spaces in the following chart. If the molecule column is blank, find an example that fulfills the conditions of the rest of the row.
Why are there no sp4 or sp5 hybrid orbitals?
(a) Starting with the orbital diagram of a boron atom, describe the steps needed to construct hybrid orbitals appropriate to describe the bonding in BF3. (b)What is the name given to the hybrid
(a) Starting with the orbital diagram of a sulfur atom, describe the steps needed to construct hybrid orbitals appropriate to describe the bonding in SF2. (b)What is the name given to the hybrid
Indicate the hybridization of the central atom in (a) BCl3 (b) AlCl4- (c) CS2 (d) GeH4.
What is the hybridization of the central atom in (a) SiCl4 (b) HCN (c) SO3 (d) TeCl2.
Shown here are three pairs of hybrid orbitals, with each set at a characteristic angle. For each pair, determine the type of hybridization, if any that could lead to hybrid orbitals at the specified
(a) Which geometry and central atom hybridization would you expect in the series BH4-, CH4, NH4+? (b) What would you expect for the magnitude and direction of the bond dipoles in this series? (c)
(a) Draw a picture showing how two p orbitals on two different atoms can be combined to make a sigma bond. (b) Sketch a π bond that is constructed from p orbitals. (c) Which is generally stronger,
In the series SiF4, PF3, and SF2, estimate the F-X-F bond angle in each case and explain your rationale.
(a) If the valence atomic orbitals of an atom are sp hybridized, how many unhybridized p orbitals remain in the valence shell? How many π bonds can the atom form? (b) Imagine that you could hold
(a) Draw Lewis structures for ethane (C2H6), ethylene (C2H4), and acetylene (C2H2). (b) What is the hybridization of the carbon atoms in each molecule? (c) Predict which molecules, if any, are
The nitrogen atoms in N2 participate in multiple bonding, whereas those in hydrazine, N2H4, do not. (a) Draw Lewis structures for both molecules. (b) What is the hybridization of the nitrogen atoms
Propylene, C3H6, is a gas that is used to form the important polymer called polypropylene. Its Lewis structure is(a) What is the total number of valence electrons in the propylene molecule? (b) How
Ethyl acetate, C4H8O2, is a fragrant substance used both as a solvent and as an aroma enhancer. Its Lewis structure is(a) What is the hybridization at each of the carbon atoms of the molecule? (b)
Consider the Lewis structure for glycine, the simplest amino acid:(a) What are the approximate bond angles about each of the two carbon atoms, and what are the hybridizations of the orbitals on each
(a) What is the difference between a localized π bond and a delocalized one? (b) How can you determine whether a molecule or ion will exhibit delocalized π bonding? (c) Is the π bond in NO2-
(a) Write a single Lewis structure for SO3, and determine the hybridization at the S atom. (b) Are there other equivalent Lewis structures for the molecule? (c) Would you expect SO3 to exhibit
Predict the molecular geometry of each of the following molecules:(a).(b). (c).
What hybridization do you expect for the atom indicated in red in each of the following species? (a) CH3CO2- (b) PH4+ (c) AlF3 (d) H2C==CH-CH2+
(a) What is the difference between hybrid orbitals and molecular orbitals? (b) How many electrons can be placed into each MO of a molecule? (c) Can anti-bonding molecular orbitals have electrons in
(a) If you combine two atomic orbitals on two different atoms to make a new orbital, is this a hybrid orbital or a molecular orbital? (b) If you combine two atomic orbitals on one atom to make a new
Consider the H2+ ion. (a) Sketch the molecular orbitals of the H2+ ion and draw its energy-level diagram. (b) How many electrons are there in the ion? (c) Draw the electron configuration of the ion
(a) Sketch the molecular orbitals of the H2- ion and draw its energy-level diagram. (b) Write the electron configuration of the ion in terms of its MOs. (c) Calculate the bond order in H2- (d)
Draw a picture that shows all three 2p orbitals on one atom and all three 2p orbitals on another atom. (a) Imagine the atoms coming close together to bond. How many σ bonds can the two sets of 2p
(a) What is the probability of finding an electron on the inter-nuclear axis if the electron occupies a π molecular orbital? (b) For a homo-nuclear diatomic molecule, what similarities and
(a) What are the relationships among bond order, bond length, and bond energy? (b) According to molecular orbital theory, would either Be2 or Be2+ be expected to exist? Explain.
Explain the following: (a) The peroxide ion, O22-, has a longer bond length than the superoxide ion, O2-. (b) The magnetic properties of B2 are consistent with the π2p MOs being lower in energy
In the hydrocarbon(a) What is the hybridization at each carbon atom in the molecule? (b) How many Ïƒ bonds are there in the molecule? (c) How many Ï€ bonds? (d) Identify all the
(a) What does the term paramagnetic mean?(b) How can one determine experimentally whether a substance is paramagnetic?(c) Which of the following ions would you expect to be paramagnetic: O2+, N22-,

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