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general chemistry principles

Questions and Answers of General Chemistry Principles

Amino acids contain both an acidic carboxylic acid group (—COOH) and a basic amino group (—NH2). The amino group can be protonated (that is, it has an extra proton attached) in a strongly acidic
In some cases, the titration curve for a mixture of two acids has the same appearance as that for a single acid; in other cases it does not.(a) Sketch the titration curve (pH versus volume of
In your own words, define or explain the following terms or symbols: (a) mmol; (b) HIn; (c) Equivalence point of a titration; (d) Titration curve.
Briefly describe each of the following ideas, phenomena, or methods: (a) The common-ion effect; (b) The use of a buffer solution to maintain a constant pH;(c) The determination of pKa of a weak
Sketch the titration curves that you would expect to obtain in the following titrations. Select a suitable indicator for each titration from Figure 17-7.(a) NaOH(aq) titrated with HNO3(aq)(b) NH3(aq)
Explain the important distinctions between each pair of terms: (a) Buffer capacity and buffer range;(b) Hydrolysis and neutralization; (c) First and second equivalence points in the titration of a
Write equations to show how each of the following buffer solutions reacts with a small added amount of a strong acid or a strong base: (a) HCOOH–KHCOO;(b) C6H5NH2–C6H5NH3+Cl-;(c) KH2PO4–
A 25.00-mL sample of 0.0100 M C6H5COOH (Ka = 6.3 x 10-5) is titrated with 0.0100 M Ba(OH)2. Calculate the pH (a) Of the initial acid solution;(b) After the addition of 6.25 mL of 0.0100 M
To suppress the ionization of formic acid, HCOOH(aq), which of the following should be added to the solution?(a) NaCl; (b) NaOH; (c) NaHCOO; (d) NaNO3.
To increase the ionization of formic acid, HCOOH(aq), which of the following should be added to the solution?(a) NaCl; (b) NaHCOO; (c) H2SO4; (d) NaHCO3.
To convert NH4+(aq) to NH3(aq), (a) Add H3O+;(b) Raise the pH; (c) Add KNO3(aq); (d) Add NaCl.
During the titration of equal concentrations of a weak base and a strong acid, at what point would the pH = pKa? (a) The initial pH; (b) Halfway to the equivalence point; (c) At the equivalence
Calculate the pH of the buffer formed by mixing equal volumes [C2H5NH2] = 1.49 M with [HClO4] = 1.001 M . Kb = 4.3 x 10-4.
Calculate the pH of a 0.5 M solution of Ca(HSe)2, given that H2Se has Ka1 = 1.3 x 10-4 and Ka2 = 1 x 10-11.
The effect of adding 0.001 mol KOH to 1.00 L of a solution that is 0.10 M NH3–0.10 M NH4Cl is to (a) Raise the pH very slightly; (b) Lower the pH very slightly;(c) Raise the pH by several
The most acidic of the following 0.10 M salt solutions is (a) Na2S; (b) NaHSO4;(c) NaHCO3;(d) Na2HPO4.
If an indicator is to be used in an acid–base titration having an equivalence point in the pH range 8 to 10, the indicator must (a) Be a weak base; (b) Have Ka = 1 x 10-9; (c) Ionize in two
Indicate whether you would expect the equivalence point of each of the following titrations to be below, above, or at pH 7. Explain your reasoning.(a) NaHCO3(aq) is titrated with NaOH(aq);(b) HCl(aq)
The ions ICl2- and ICl2+ differ by only two electrons. Would you expect them to have the same geometric shape? Explain.
Write the most plausible Lewis structure of nitrosyl chloride, NOCl, one of the oxidizing agents present in aqua regia, a mixture of concentrated nitric and hydrochloric acids capable of dissolving
Use ΔrH for the reaction in Example 10-15 and other data from Appendix D to estimate ΔfH° [CH3Cl(g)].Example 10-15The reaction of methane (CH4) and chlorine produces a mixture of products called
The synthesis of ammonia by the Haber process occurs by the reaction N2(g) + 3 H2(g) ⇌ 2 NH3(g) at 400 °C. Using data from Appendix D and assuming that ΔrH° and ΔrS° are essentially unchanged
Consider the two-dimensional lattice shown here.(a) Identify a unit cell.(b) How many of each of the following elements are in the unit cell: (c) Indicate some simpler units than the unit cell, and
(A) Write plausible Lewis structures for the following ions: (a) NO+; (b) N2H5+;(c) O2-.(B) Write plausible Lewis structures for the following ions: (a) BF4-; (b) NH3OH+; (c) NCO-.
Give several examples for which the following statement proves to be incorrect. “All atoms in a Lewis structure have an octet of electrons in their valence shells.”
Write the Lewis structure for the nitronium ion, NO2+.
We reasoned that because of resonance, oxygen–oxygen bonds in O3 were halfway between single and double bonds, that is, 1.5 bonds. Do you expect the sulfur–oxygen bonds in SO2 to be single,
(A) Write plausible Lewis structures for (a) CS2, (b) HCN, and(c) COCl2.(B) Write plausible Lewis structures for (a) Formic acid, HCOOH, and (b) Acetaldehyde, CH3CHO.
Which of the following have Lewis structures that do not obey the octet rule: NF3, B(OH)3, SiF62-, SO3, PH4+, PO43-, ClO2, C2H4, SO(CH3).
Write a plausible Lewis structure for cyanogen, C2N2, a poisonous gas used as a fumigant and rocket propellant.
Is resonance possible in the acetic acid (CH3CO2H) molecule? Explain.
(A) Which of the following electrostatic potential maps corresponds to IF, and which to IBr?(B) Which of the following electrostatic potential maps corresponds to CH3OH, and which to CH3SH?
By means of Lewis structures, represent bonding between the following pairs of elements: (a) Cs and Br; (b) H and Sb; (c) B and Cl; (d) Cs and Cl; (e) Li and O; (f) Cl and I. Your structures
Two electrostatic potential maps are shown below. One corresponds to NaF and the other to NaH. Which map corresponds to which molecule?
For molecules, the most satisfactory Lewis structure may have no formal charges (FC = 0) in some cases and formal charges in others. For polyatomic ions, minimally the most satisfactory Lewis
(A) Which of the following bonds are the most polar, that is, have the greatest ionic character: H—Br, N—H, N—O, P—Cl?(B) Which is the most polar bond: C—S, C—P, P—O, or O—F?
Each of the following molecules contains at least one multiple (double or triple) covalent bond. Give a plausible Lewis structure for (a) HCN; (b) SC(NH2)2;(c) F2CO; (d) Cl2SO;(e) C2H2; (f) SO2.
(a) Which bond is more polar, H—Cl or H—O?(b) What is the percent ionic character of each of these bonds?
With the aid of only a periodic table, decide which is the most electronegative atom of each of the following sets of elements: (a) As, Se, Br, I; (b) Li, Be, Rb, Sr;(c) Ge, As, P, Sn.
Explain why the first ionization energy of Mg is greater that of Na, whereas the second ionization of Na is greater than that of Mg.
Refer only to the periodic table on the inside front cover and indicate which of the atoms, Bi, S, Ba, As, and Ca, (a) Is most metallic; (b) Is most nonmetallic;(c) Has the intermediate value when
Refer to the periodic table on the inside front cover and indicate (a) The most nonmetallic element; (b) The transition metal with lowest atomic number; (c) A metalloid whose atomic number is
(A) Write Lewis structures for Br2, CH4, and HOCl.(B) Write Lewis structures for NI3, N2H4, and C2H6.
Write plausible Lewis structures for the following molecules that contain only single covalent bonds.(a) FCl; (b) I2;(c) SF2;(d) NF3;(e) H2Te.
Write a Lewis structure for the ammonia molecule, NH3.
In which groups of the periodic table are the elements most likely to use multiple bonds?
Arrange the following elements in order of decreasing metallic character: Sc, Fe, Rb, Br, O, Ca, F, Te.
For the atom 11950Sn, indicate the number of (a) Protons in the nucleus; (b) Neutrons in the nucleus; (c) 4d electrons;(d) 3s electrons; (e) 5p electrons; (f) Electrons in the valence shell.
Give the symbol of the element (a) In group 14 that has the smallest atoms; (b) In period 5 that has the largest atoms; (c) In group 17 that has the lowest first ionization energy.
Find three pairs of elements that are out of order in the periodic table in terms of their atomic masses. Why is it necessary to invert their order in the table?
(A) Write plausible Lewis structures for (a) Na2S and (b) Mg3N2.(B) Write plausible Lewis structures for (a) Calcium iodide; (b) Barium sulfide;(c) Lithium oxide.
Write Lewis symbols for the following ions. (a) H-;(b) Sn2+;(c) K+;(d) Br-;(e) Se2-;(f) Sc3+.
Write Lewis structures for the following compounds: (a) BaO; (b) MgCl2; (c) Aluminum oxide.
What types of bonds can be used to describe the chemical bonds in BF4-?
How many valence electrons do the Lewis symbols for the elements in group 16 have? Which of the following are correct Lewis symbols for sulfur? :$: :S: •S:
Nitryl fluoride is a reactive gas useful in rocket propellants. Its mass percent composition is 21.55% N, 49.23% O, and 29.23% F. Its density is 2.7 g/L at 20 °C and 1.00 atm pressure. Describe the
(A) Write Lewis symbols for Mg, Ge, K, and Ne.(B) Write the Lewis symbols expected for Sn, Br-, Tl+, and S2-.
Write Lewis symbols for the following atoms. (a) Kr;(b) Ge; (c) N; (d) Ga; (e) As; (f) Rb.
Write Lewis symbols for the following elements: (a) N, P, As, Sb, Bi; (b) Al, I, Se, Ar.
The electrons lost when Fe ionizes to Fe2+ are (a) 4ƒ;(b) 3d; (c) 4s; (d) 3p; (e) None of these.
Which electron is lost when an atom ionizes? (a) The electron with the highest principal quantum number;(b) The electron with lowest principal quantum number;(c) An outer-shell electron with the
Which of the following has a smaller radius than a neon atom? (a) Mg2+; (b) F-; (c) O2–; (d) K+; (e) None of these.
Which of the following is an example of a metalloid?(a) S; (b) Zn; (c) Ge; (d) Re; (e) None of these.
When compared to a nonmetal of the same period, a metal will have a larger (a) Atomic radius; (b) Ionization energy; (c) Electron affinity; (d) Atomic number;(e) None of these.
Why, in general, is the addition of an electron to an atom an exothermic process?
Which element Na or Mg is likely to have ΔeaH greater than zero?
The first ionization energies of Si, P, S, and Cl are given in Table 9.4. Briefly provide an explanation for this trend.Table 9.4 TABLE 9.4 lonization Energies of the Third-Period Elements (in kJ
Describe how the ionization energies of the ions Be+, B+, C+, N+, O+, F+, Ne+, and Na+ vary with atomic number.
Describe how the ionization energies of the ions He-, Li-, Be-, B-, C-, N-, O-, and F- vary with atomic number.
Consider a nitrogen atom in the ground state and comment on whether the following statements are true or false.(a) Zeff for an electron in a 2s orbital is greater than that for the 1s orbital.(b) The
In multielectron atoms many of the periodic trends can be explained in terms of Zeff. Consider the following statements and discuss whether or not the statement is true or false.(a) Electrons in a p
Answer each of the following questions:(a) Which of the elements P, As, and S has the largest atomic radius?(b) Which of the following has the smallest radius: Xe, O2-, N3-, or F-?(c) Which should
Write electron configurations to show the first two ionizations for Cs. Explain why the second ionization energy is much greater than the first.
An ion that is isoelectronic with Se2- is (a) S2-; (b) I-;(c) Xe; (d) Sr2+.
Refer only to the periodic table on the inside front cover, and arrange the following ionization energies in order of increasing value: the first ionization energy of F; the second ionization energy
Use values of basic physical constants and other data from the appendices to show that 1 eV/atom = 96.49 kJ mol-1.
When sodium chloride is strongly heated in a flame, the flame takes on the yellow color associated with the emission spectrum of sodium atoms. The reaction that occurs in the gaseous state
Calculate the second ionization energy for the He atom. Compare your result with the tabulated value of 5251 kJ mol-1.
Assume that atoms are hard spheres, and use the metallic radius of 186 pm for Na to estimate the volumes of one Na atom and of one mole of Na atoms. How does your result compare with the atomic
Two elements, A and B, have the electron configurations shown.(a) Which element is a metal?(b) Which element has the greater ionization energy?(c) Which element has the larger atomic radius?(d) Which
Studies done in 1880 showed that a chloride of uranium had 37.34% Cl by mass and an approximate formula mass of 382 u. Other data indicated the specific heat of uranium to be 0.0276 cal g-1 °C-1.
Two elements, A and B, have the electron configurations shown.(a) Which element is a metal?(b) Which element has the greater ionization energy?(c) Which element has the larger atomic radius?(d) Which
Refer to Figure 9-11 and explain why the difference between the ionic radii of the -1 and -2 anions does not remain constant from top to bottom of the periodic table.Figure 9-11 Li 155 Li+
Explain why the third ionization energy of Li(g) is an easier quantity to calculate than either the first or second ionization energies. Calculate the third ionization energy for Li, and express the
Instead of accepting the atomic mass of indium implied by the data in Exercise 51, Mendeleev proposed that the formula of indium oxide is In2O3. Show that this assumption places indium in the proper
In Mendeleev’s time, indium oxide, which is 82.5% In by mass, was thought to be InO. If this were the case, in which group of Mendeleev’s table should indium be placed?
Sketch a periodic table that would include all the elements in the main body of the table. How many “numbers” wide would the table be?
Four atoms and/or ions are sketched below in accordance with their relative atomic and/or ionic radii.Which of the following sets of species are compatible with the sketch? Explain. (a) C, Ca2+,
Which of the following ions are likely to be found in chemical compounds: Na2+, Li+, Al4+, F2-, or Te2-? Explain briefly.
Which of the following ions are unlikely to be found in chemical compounds: K+, Ga4+, Fe6+, S2-, Ge5+, or Br-? Explain briefly.
Match each of the lettered items in the column on the left with the most appropriate numbered item(s) in the column on the right. Some of the numbered items may be used more than once and some not at
Match each of the lettered items on the left with an appropriate numbered item on the right. All the numbered items should be used, and some more than once. (a) Z = 32 (b) Z = 8 (c) Z = 53 (d) Z
Of the species Na+, Na, F, and F–, which has the highest polarizability? Which has lowest polarizability?
Of the species Cl, Cl+, and Cl–, which has the highest polarizability? Which has lowest polarizability?
For the following groups of elements, select the one that has the property noted:(a) The largest atom: Mg, Mn, Mo, Ba, Bi, Br (b) The lowest first ionization energy: B, Sr, Al, Br, Mg, Pb (c) The
Arrange the following species in order of increasing polarizability: N, S, Be, K, O.
Arrange the following atoms in order of increasing polarizability: F, Na, P, As, Br.
Use ideas presented in this chapter to indicate (a) Three metals that you would expect to exhibit the photoelectric effect with visible light and three that you would not; (b) The noble gas element
Neither Co2+ nor Co3+ has 4s electrons in its electron configuration. How many unpaired electrons would you expect to find in each of these ions? Explain.
Must all atoms with an odd atomic number be paramagnetic? Must all atoms with an even atomic number be diamagnetic? Explain.

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