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general chemistry principles

Questions and Answers of General Chemistry Principles

Write electron configurations consistent with the following data on numbers of unpaired electrons: Ni2+, 2; Cu2+, 1; Cr3+, 3.
(A) Refer to the periodic table on the inside front cover, and arrange the following in the expected order of increasing first ionization energy Cl, K, Mg, S.(B) Refer to the periodic table on the
Which of the following species would you expect to be diamagnetic and which paramagnetic? (a) K+;(b) Cr3+;(c) Zn2+;(d) Cd; (e) Co3+;(f) Sn2+;(g) Br.
Refer to the periodic table on the inside front cover, and arrange the following in the expected order of increasing first ionization energy: As, Sn, Br, Sr. REIHEN 3 A W 1 2 Li=7 4 K 56 94 Gruppe 1
Which of the following species has the greatest number of unpaired electrons (a) Ge; (b) Cl; (c) Cr3+;(d) Br-?
Unpaired electrons are found in only one of the following species. Indicate which one, and explain why: F-, Ca2+, Fe2+, S2-.
(A) Refer only to the periodic table on the inside front cover, and arrange the following species in order of increasing size: Ti2+, V3+, Ca2+, Br-, and Sr2+.(B) Refer only to the periodic table on
Refer only to the periodic table on the inside front cover, and arrange the following species in order of increasing size: K+, Cl-, S2-, and Ca2+. REIHEN 3 A W 1 2 Li=7 4 K 56 94 Gruppe 1 Gruppe 11
(A) Use the periodic table on the inside front cover to predict which is the smallest atom: As, I, or S.(B) Which of the following atoms do you think is closest in size to the Na atom: Br, Ca, K, or
Write the Lewis structure of the acetate ion, CH3COO-.
Describe what is wrong with each of the following Lewis structures. (a) H-H-N-Ö-H (b) Ca-0:
(A) Draw Lewis structures to represent the resonance hybrid for the SO2 molecule.(B) Draw Lewis structures to represent the resonance hybrid for the nitrate ion.
The molecule NH3 has the dipole moment μ = 1.47 D, whereas for the similar molecule NF3, μ = 0.24 D. Why do you suppose there is such a large difference in these two values?
Predict the molecular geometry of the polyatomic anion ICl4-.
Describe what is wrong with each of the following Lewis structures. (a) :0-C-0: (b) [.C=N:]
(A) Predict the molecular geometry of nitrogen trichloride.(B) Predict the molecular geometry of phosphoryl chloride, POCl3, an important chemical in the manufacture of gasoline additives, hydraulic
NO2- and NO2+ are made up of the same atoms. How would you expect the nitrogen-to-oxygen bond lengths in these two ions to compare?
Predict the molecular geometry of formaldehyde, H2CO, used to make a number of polymers, such as melamine resins. The Lewis structure of the H2CO molecule is shown here. Η Η C :Ö:
Only one of the following Lewis structures is correct. Select that one and indicate the errors in the others. (a) cyanate ion (b) carbide ion (c) hypochlorite ion (d) nitrogen (II)
(A) Predict the shape of the COS molecule.(B) Nitrous oxide, N2O, is the familiar laughing gas used as an anesthetic in dentistry. Predict the shape of the N2O molecule.
Methyl isocyanate, CH3NCO, is used in the manufacture of insecticides, such as carbaryl (Sevin). In the CH3NCO molecule, the three H atoms and the O atom are terminal atoms and the two C and one N
Indicate what is wrong with each of the following Lewis structures. Replace each one with a more acceptable structure. (a) Mg:0: (b) [:O-N=0:1 (c) (d) [:S-C=N:] [:a::r [C: Cl :0
(A) Sketch, by using dash and wedge symbols, the methanol molecule, CH3OH. Indicate the bond angles in this molecule.(B) Glycine, an amino acid, has the formula H2NCH2COOH. Sketch, by using dash and
Which of these molecules would you expect to be polar: Cl2, ICl, BF3, NO, SO2?
Under appropriate conditions, both hydrogen and nitrogen can form monatomic anions. What are the Lewis symbols for these ions? What are the Lewis structures of the compounds (a) Lithium hydride;(b)
Provide the best estimate you can of these bond lengths for the (a) The nitrogen-to-hydrogen bonds in NH3;(b) The bromine-to-chlorine bond in BrCl.
(A) Only one of the following molecules is polar. Which is it, and why? SF6, H2O2, C2H4.(B) Only one of the following molecules is nonpolar. Which is it, and why? Cl3CCH3, PCl5, CH2Cl2, NH3.
Write Lewis structures for the following ionic compounds:(a) Calcium chloride; (b) Barium sulfide;(c) Lithium oxide; (d) Sodium fluoride.
What is the formal charge of the indicated atom in each of the following structures?(a) The central O atom in O3(b) Al in AlH4-;(c) Cl in ClO3-;(d) Si in SiF62-;(e) Cl in ClF3.
The concept of formal charge helped us to choose the more plausible of the Lewis structures for NO2+ given in expressions (10.14) and (10.15). Can it similarly help us to choose a single Lewis
Derive the correct formulas for the following ionic compounds by writing Lewis structures. (a) Lithium sulfide; (b) Sodium fluoride; (c) Calcium iodide;(d) Scandium chloride.
(A) Use bond energies to estimate the enthalpy change for the reaction (B) Use bond energies to estimate the enthalpy of formation of NH3(g). 2 H₂(g) + O2(g) 2 H₂O(g)
One of the steps in the formation of monochloromethane (Example 10-15) is the reaction of a gaseous chlorine atom (a chlorine radical) with a molecule of methane. The products are an unstable methyl
(A) Is the following reaction endothermic or exothermic?(B) Predict whether the following reaction should be exothermic or endothermic: CH3COCH3(g) + H₂(g) (CH3)2CH(OH)(g)
Each of the following ionic compounds consists of a combination of monatomic and polyatomic ions. Represent these compounds with Lewis structures.(a) Al(OH)3;(b) Ca(CN)2;(c) NH4F;(d) KClO3;(e)
Assign formal charges to each of the atoms in the following structures. (a) [H-C=C:] (b) :0: C :0: 72- O: (c) [CH3-CH-CH3]+
Assign formal charges to each of the atoms in the following structures. (a) (b) (c) S N
Both oxidation state and formal charge involve conventions for assigning valence electrons to bonded atoms in compounds, but clearly they are not the same. Describe several ways in which these
Although the notion that a Lewis structure in which formal charges are zero or held to a minimum seems to apply in most instances, describe several significant situations in which this appears not to
Assign formal charges to the atoms in the following species, and then select the more likely skeletal structure.(a) H2NOH or H2ONH (b) SCS or CSS (c) NFO or FNO (d) SOCl2 or OSCl2 or OCl2S (e)
Show that the idea of minimizing the formal charges in a structure is at times in conflict with the observation that compact, symmetrical structures are more commonly observed than elongated ones
Write acceptable Lewis structures for the following molecules: (a) H2NNH2; (b) HOClO; (c) (HO)2SO;(d) HOOH; (e) SO42-.
Two molecules that have the same formulas but different structures are said to be isomers. (In isomers, the same atoms are present but linked together in different ways.) Draw acceptable Lewis
The following polyatomic anions involve covalent bonds between O atoms and the central nonmetal atom. Propose an acceptable Lewis structure for each.(a) SO32-; (b) NO2-; (c) CO32-; (d) HO2-.
Represent the following ionic compounds by Lewis structures: (a) Barium hydroxide; (b) Sodium nitrite;(c) Magnesium iodate; (d) Aluminum sulfate.
Write a plausible Lewis structure for crotonaldehyde, CH3CHCHCHO, a substance used in tear gas and insecticides.
(A) Estimate the bond lengths of the carbon-to-hydrogen bonds and the carbon-to-bromine bond in CH3Br.(B) In the thiocyanate ion, SCN-, the length of the carbon-to-nitrogen bond is 115 pm. Write a
The reaction of methane (CH4) and chlorine produces a mixture of products called chloromethanes. One of these is monochloromethane, CH3Cl, used in the preparation of silicones. Calculate ΔrH for the
Write a plausible Lewis structure for C3O2, a substance known as carbon suboxide.
Write Lewis structures for the molecules represented by the following molecular models. (a) (b)
Write Lewis structures for the molecules represented by the following molecular models. (a) (b)
Write Lewis structures for the molecules represented by the following line-angle formulas. (a) C1- (b) HO OH 0 ОН
Write Lewis structures for the molecules represented by the following line-angle formulas. (a) (b) Cl NH₂
Identify the main group that the element X belongs to in each of the following Lewis structures. For the types of molecule shown, give an example that exists. (a) [:X—X; :Ö: 2- (c) |:0
Identify the main group that the element X belongs to in each of the following Lewis structures. For the types of molecule shown, give an example that exists.
Which of the following molecules would you expect to have a resultant dipole moment (μ)? Explain. (a) F2;(b) NO2; (c) BF3;(d) HBr; (e) H2CCl2;(f) SiF4;(g) OCS.
What is the percent ionic character of each of the following bonds? (a) S—H;(b) O—Cl;(c) Al—O;(d) As—O.
Plot the data of Figure 10-6 as a function of atomic number. Does the property of electronegativity conform to the periodic law? Do you think it should?Figure 10-6 4.0- 3.5 Electronegativity 3.0 N
Use a cross-base arrow (⇸) to represent the polarity of the bond in each of the following diatomic molecules. Then use the data below to calculate, in the manner described, the partial charges (δ)
Use a cross-base arrow (⇸) to represent the polarity of the bond in each of the following diatomic molecules. Then use the data below to calculate the partial charges (δ) on the atoms in each
Which electrostatic potential map corresponds to F2 = O, and which to H2 = O?
Match the correct electrostatic potential map corresponding to HOCl, FOCl, and HOF.
Two electrostatic potential maps are shown, one corresponding to a molecule containing only S and F, the other Si and F. Match them. What are the molecular formulas of the compounds?
Two electrostatic potential maps are shown, one corresponding to a molecule containing only Cl and F, the other P and F. Match them. What are the molecular formulas of the compounds?
Through appropriate Lewis structures, show that the phenomenon of resonance is involved in the nitrite ion.
Dinitrogen oxide (nitrous oxide, or “laughing gas”) is sometimes used as an anesthetic. Here are some data about the N2O molecule: N—N bond length = 113 pm; N—O bond length = 119 pm. Use
Which of the following species requires a resonance hybrid for its Lewis structure? Explain. (a) CO2;(b) OCl-;(c) CO32-;(d) OH-.
The Lewis structure of nitric acid, HONO2, is a resonance hybrid. How important do you think the contribution of the following structure is to the resonance hybrid? Explain. H-O=N :0: :O:
Draw Lewis structures for the following species, indicating formal charges and resonance where applicable:(a) HCO2-(b) HCO3-(c) FSO3-(d) N2O32-.
Draw Lewis structures for the following species, indicating formal charges and resonance where applicable:(a) HOSO3-(b) H2NCN (c) FCO2-(d) S2N2.
Write plausible Lewis structures for the following odd-electron species: (a) CH3; (b) ClO2; (c) NO3.
Write plausible Lewis structures for the following free radicals: (a) · C2H5;(b) HO2 · ;(c) ClO ·.
Which of the following species would you expect to be diamagnetic and which paramagnetic? (a) OH-;(b) OH; (c) NO3; (d) SO3; (e) SO32-; (f) HO2.
Write a plausible Lewis structure for NO2, and indicate whether the molecule is diamagnetic or paramagnetic. Two NO2 molecules can join together (dimerize) to form N2O4. Write a plausible Lewis
In which of the following species is it necessary to employ an expanded valence shell to represent the Lewis structure: PO43-, PI3, ICl3, OSCl2, SF4, ClO4-? Explain your choices.
Describe the carbon-to-sulfur bond in H2CSF4. That is, is it most likely a single, double, or triple bond?
Use VSEPR theory to predict the geometric shapes of the following molecules and ions: (a) N2; (b) HCN;(c) NH4+; (d) NO3-; (e) NSF.
Use VSEPR theory to predict the geometric shapes of the following molecules and ions: (a) PCl3;(b) SO42-;(c) SOCl2;(d) SO3;(e) BrF4+.
Each of the following is either linear, angular (bent), planar, tetrahedral, or octahedral. Indicate the correct shape of (a) H2S;(b) N2O4;(c) HCN; (d) SbCl6-;(e) BF4-.
Predict the geometric shapes of (a) CO; (b) SiCl4;(c) PH3; (d) ICl3;(e) SbCl5;(f) SO2;(g) AlF63-.
One of the following ions has a trigonal-planar shape: SO32-; PO43-; PF6-; CO32-. Which ion is it? Explain.
Comment on the similarities and differences in the molecular structure of the following four-atom species: NO3-, CO32-, SO32-, and ClO3-.
Comment on the similarities and differences in the molecular structure of the following triatomic species: CO2, NO2-, O3, and ClO2-.
Draw a plausible Lewis structure for the following series of molecules and ions: (a) ClF2-; (b) ClF3;(c) ClF4-; (d) ClF5.Describe the electron group geometry and molecular structure of these
Draw a plausible Lewis structure for the following series of molecules and ions: (a) SiF62-; (b) PCl3;(c) AsCl5;(d) ClF3; (e) XeF4.Describe the electron group geometry and molecular structure of
Sketch the propyne molecule, CH3C ≡ CH. Indicate the bond angles in this molecule. What is the maximum number of atoms that can be in the same plane?
One reaction involved in the sequence of reactions leading to the destruction of ozone is Calculate ΔrH° for this reaction by using the thermodynamic data in Appendix D. Use your ΔrH° value,
R. S. Mulliken proposed that the electronegativity (EN) of an atom is given bywhere Ei and Eea are the ionization energy and electron affinity of the atom, respectively. Using the electron affinities
(A) How much heat is required to vaporize a 2.35 g sample of diethyl ether at 298 K?(B) Calculate a more accurate answer to Example 12-2 by using ΔvapH = 40.7 kJ mol-1 for water at 100 °C, 85.0 °C
Using ideas from this section, explain why highly exothermic processes tend to be spontaneous. Under what condition(s) will a highly exothermic process be nonspontaneous?
Use data from Appendix D to calculate the standard reaction entropy at 298.15 K for the conversion of nitrogen monoxide to nitrogen dioxide (a step in the manufacture of nitric acid). 2 NO(g) +
Use ideas from this chapter to explain this famous remark attributed to Rudolf Clausius (1865): “Die Energie der Welt ist konstant; die Entropie der Welt strebt einem Maximum zu.” (“The energy
At 298 K, for the reaction 2 H+(aq) + 2 Br-(aq) + 2 NO2(g) → Br2(l) + 2 HNO2(aq), ΔrH° = -61.6 kJ mol-1 and the standard molar entropies are H+(aq), 0 J mol-1 K-1; Br-(aq), 82.4 J mol-1 K-1;
In what important way would Figure 14-23 change if it were based on the phase diagram of water rather than for the general case shown? Would a boiling-point elevation and a freezing-point depression
Suggest reasons why the following do not exist as stable molecules: (a) H3; (b) HHe; (c) He2;(d) H3O.
(A) Write a Lewis structure for nitrosyl chloride based on the skeletal structure N—O—Cl and show that this structure is not as plausible as the one obtained in Example 10-8.(B) Write two Lewis
Methyl isocynate, CH3NCO, can be represented as a hybrid of three Lewis structures. The most satisfactory structure is the one given above in Example 10-12. Draw the other two structures. On the
For the following reversible reactions, write thermodynamic equilibrium constant expressions, making appropriate substitutions for activities. Then relate K to Kc or Kp where this can be done.(a) The
(A) What is the partial pressure of NH3 in the ammonia synthesis reaction if the Gibbs energy of reaction is –82.00 kJ mol–1 and the partial pressures of hydrogen and nitrogen are each 0.500 bar?
Indicate whether entropy increases or decreases in each of the following reactions. If you cannot be certain simply by inspecting the equation, explain why. (a) CCl4(1) CC14(g) . (b) CuSO4 3 H₂O(s)

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