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General Chemistry Principles And Modern Applications 11th Edition Ralph Petrucci, Jeffry Madura, F. Herring, Carey Bissonnette - Solutions

Gaseous sodium atoms absorb quanta with the energies shown in the table below.(a) The ionization energy of the ground state is 496 kJ mol-1. Calculate the ionization energies for each of the states given in the table.(b) Calculate Zeff for each state.(c) Calculate r̅nℓ for each state.(d)
A method for estimating electron affinities is to extrapolate Zeff values for atoms and ions that contain the same number of electrons as the negative ion of interest. Use the data in the table to answer the questions that follow.(a) Estimate the electron affinity of F, and compare it with the
We have seen that the wave functions of hydrogen-like atoms contain the nuclear charge Z for hydrogen-like atoms and ions, but modified through equation (9.3) to account for the phenomenon of shielding or screening. In 1930, John C. Slater devised the following set of empirical rules to calculate a
In your own words, define the following terms:(a) Isoelectronic; (b) Valence-shell electrons; (c) Metal;(d) Nonmetal; (e) Metalloid.
Briefly describe each of the following ideas or phenomena:(a) The periodic law; (b) Ionization energy;(c) Electron affinity; (d) Paramagnetism.
Explain the important distinctions between each pair of terms: (a) Actinide and lanthanide element;(b) Covalent and metallic radius; (c) Atomic number and effective nuclear charge; (d) Ionization energy and electron affinity; (e) Paramagnetic and diamagnetic.
The element whose atoms have the electron configuration [Kr]4d105s25p3(a) Is in group 13 of the periodic table; (b) Bears a similarity to the element Bi; (c) Is similar to the element Te; (d) Is a transition element.
The fourth-period element with the largest atom is (a) K; (b) Br; (c) Pb; (d) Kr.
Which of the following has the largest radius (a) An Ar atom; (b) A K+ ion; (c) A Ca2+ ion; (d) A Cl- ion?
The highest first ionization energy of the following is that of (a) Cs; (b) Cl; (c) I; (d) Li.
The most negative electron affinity of the following elements is that of (a) Br; (b) Sn; (c) Ba; (d) Li.
Which of the following orbital diagrams is incorrect? Explain. Which of the correct diagrams corresponds to an excited state and which to the ground state of the neutral atom?
When the ionization energies of a series of isoelectronic atoms and ions are compared, an interesting relationship is observed for some of them. In particular, if the square root of the ionization energy (in kJ mol-1) for the series Li, Be+, B2+, C3+, N4+, O5+, and F6+ is plotted against the atomic
Use data from Figure 9-1 and equation (9.1) to estimate the density of the recently discovered element 114.Figure 9-1Eq. 9.1 Atomic (molar) volume, 103 cm³/mol 80 70 60 50 40 30 20 10 T Na 10 K 20 30 Rb Cs 40 50 Atomic number 60 70 80 90 100
Refer only to the periodic table on the inside front cover, and determine which is the largest atom: Sc, Ba, or Se.
Estimate Zeff for a 3p electron in Si by assuming the inner (core) electrons screen outer (valence) electrons perfectly and the outer electrons do not screen each other.
On the blank periodic table in the margin, locate the following:(a) The smallest group 13 atom (b) The smallest period 3 atom (c) The largest anion of a nonmetal in period 3 (d) The largest group 13 cation. 1 1 234 55 3 4 5 6 7 2 13 14 15 16 17
The graph in the margin represents the variation of Zeff and atomic radius with atomic number. Which axis and correspondingly colored line corresponds to Zeff and which to atomic radius?
Suppose that lanthanum (Z = 57) were a newly discovered element having a density of 6.145 g/cm3. Estimate its molar mass.
The following densities, in grams per cubic centimeter, are for the listed elements in their standard states at 298 K. Show that density is a periodic property of these elements: Al, 2.699; Ar, 0.0018; As, 5.778; Br, 3.100; Ca, 1.550; Cl, 0.0032; Ga, 5.904; Ge, 5.323; Kr, 0.0037; Mg, 1.738; P,
Which of the following would you expect to be diamagnetic and which paramagnetic?(a) Na atom (b) Mg atom (c) Cl- ion (d) Ag atom.
On the blank periodic table in the margin, locate the following:(a) The group 14 element with the highest first ionization energy (b) The element with the greatest first ionization energy in period 4 (c) A p-block element in period 4 that has a lower first ionization energy than the element
(A) Which of the following are paramagnetic and which are diamagnetic: Zn, Cl, K+, O2-, and Al?(B) Which has the greater number of unpaired electrons, Cr2+ or Cr3+? Explain.
(A) Francium (Z = 87) is an extremely rare radioactive element formed when actinium (Z = 89) undergoes alpha-particle emission. Francium occurs in natural uranium minerals, but estimates are that little more than 15 g of francium exists in the top 1 km of Earth’s crust. Few of francium’s
On the blank periodic table in the margin locate the group expected to have (a) The most negative electron affinities in each period (b) The least negative electron affinities in each period (c) All positive electron affinities in each period. 1 234567 2 4 6 1 2 11 13 14 15 16 17 18
The following melting points are in degrees Celsius. Show that melting point is a periodic property of these elements: Al, 660; Ar, -189; Be, 1278; B, 2300; C, 3350; Cl, -101; F, -220; Li, 179; Mg, 651; Ne, -249; N, -210; O, -218; P, 590; Si, 1410; Na, 98; S, 119.
On the blank periodic table in the margin locate the following:(a) The period 4 transition element having a cation in the +3 oxidation state that is diamagnetic (b) The period 5 element existing in the -2 oxidation state as an anion that is diamagnetic (c) The period 4 transition element having a
Mendeleev’s periodic table did not preclude the possibility of a new group of elements that would fit within the existing table, as was the case with the noble gases. Moseley’s work did preclude this possibility. Explain this difference.
Explain why the several periods in the periodic table do not all have the same number of members.
The Al atom and Al3+ ion have essentially the same mass but very different polarizabilities. Which has the greater polarizability, Al or Al3+?
Assuming that the seventh period is 32 members long, what should be the atomic number of the noble gas following radon (Rn)? Of the alkali metal following francium (Fr)? What would you expect their approximate atomic masses to be?
Concerning the incomplete seventh period of the periodic table, what should be the atomic number of the element (a) For which the filling of the 6d subshell is completed; (b) That should most closely resemble bismuth;(c) That should be a noble gas?
For each of the following pairs, indicate the atom that has the larger size: (a) Te or Br; (b) K or Ca; (c) Ca or Cs; (d) N or O; (e) O or P; (f) Al or Au.
Indicate the smallest and the largest species (atom or ion) in the following group: Al atom, F atom, As atom, Cs+ ion, I- ion, N atom.
Explain why the radii of atoms do not simply increase uniformly with increasing atomic number.
The masses of individual atoms can be determined with great precision, yet there is considerable uncertainty about the exact size of an atom. Explain why this is the case.
Which is (a) The smallest atom in group 13; (b) The smallest of the following atoms: Te, In, Sr, Po, Sb? Why?
How would you expect the sizes of the hydrogen ion, H+, and the hydride ion, H-, to compare with that of the H atom and the He atom? Explain.
Explain why the generalizations presented in Figure 9-19 cannot be used to answer the question, Which is larger, an Al atom or an I atom?Figure 9-19 Atomic radius and polarizability का Ionization energy Nonmetallic character Metallic character Atomic radius and polarizability Ionization energy
Arrange the following in expected order of increasing radius: Br, Li+, Se, I-. Explain your answer.
Among the following ions, several pairs are isoelectronic. Identify these pairs. Fe2+, Sc3+, Ca2+, F-, Co2+, Co3+, Sr2+, Cu+, Zn2+, Al3+.
The following species are isoelectronic with the noble gas krypton. Arrange them in order of increasing radius and comment on the principles involved in doing so: Rb+, Y3+, Br-, Sr2+, Se2-.
All the isoelectronic species illustrated in the text had the electron configurations of noble gases. Can two ions be isoelectronic without having noble-gas electron configurations? Explain.
Is it possible for two different atoms to be isoelectronic? two different cations? two different anions? a cation and an anion? Explain.
Use principles established in this chapter to arrange the following atoms in order of increasing value of the first ionization energy: Sr, Cs, S, F, As.
Are there any atoms for which the second ionization energy is smaller than the first? Explain.
Some electron affinities are negative quantities, and some are zero or positive. Why is this not also the case with ionization energies?
How much energy, in joules, must be absorbed to convert to Na+ all the atoms present in 1.00 mg of gaseous Na? The first ionization energy of Na is 495.8 kJ/mol.
How much energy, in kilojoules, is required to remove all the third-shell electrons in a mole of gaseous silicon atoms?
The production of gaseous bromide ions from bromine molecules can be considered a two-step process in which the first step isIs the formation of Br-(g) from Br2(g) an endothermic or exothermic process? Br2(g) 2 Br(g) ΔΗ = +193 kJ mol -1
What is the maximum number of Cs+ ions that can be produced per joule of energy absorbed by a sample of gaseous Cs atoms?
Use ionization energies and electron affinities listed in the text to determine whether the following reaction is endothermic or exothermic. Mg(g) + 2F(g) Mg²(g) + 2F (g)
From the data in Figure 9-12, the formation of a gaseous anion Li- appears energetically favorable. That is, energy is given off when gaseous Li atoms accept electrons. Comment on the likelihood of forming a stable compound containing the Li- ion, such as Li+ Li- or Na+ Li-.Figure 9-12 First
The Na+ ion and the Ne atom are isoelectronic. The ease of loss of an electron by a gaseous Ne atom, first ionization energy, has a value of 2081 kJ/mol. The ease of loss of an electron from a gaseous Na+ ion, second ionization energy, has a value of 4562 kJ/mol. Why are these values not the same?
Compare the elements Al, Si, S, and Cl.(a) Place the elements in order of increasing ionization energy.(b) Place the elements in order of increasing electron affinity.(c) Place the elements in order of increasing polarizability.
Compare the elements Na, Mg, O, and P.(a) Place the elements in order of increasing ionization energy.(b) Place the elements in order of increasing electron affinity.(c) Place the elements in order of increasing polarizability.
Microwave ovens are not just being put to use in the kitchen—they are also useful in the chemical laboratory, particularly in drying samples for chemical analysis. Atypical microwave oven uses microwave radiation with a wavelength of 12.2 cm. Are there any electronic transitions between
A hypothetical electromagnetic wave is pictured here. What is the wavelength of this radiation? 1.17 nm
Red laser light is passed through a device called a frequency doubler. What is the approximate color of the light that exits the frequency doubler? How are the wavelengths of the original light and the frequency-doubled light related?
(A) The protective action of ozone in the atmosphere comes through ozone’s absorption of UV radiation in the 230 to 290 nm wavelength range. What is the energy, in kilojoules per mole, associated with radiation in this wavelength range?(B) Chlorophyll absorbs light at energies of 3.056 x 10-19
The wavelength of light needed to eject electrons from hydrogen atoms is 91.2 nm. When light of 80.0 nm is shone on a sample of hydrogen atoms, electrons are emitted from the hydrogen gas. If, in a different experiment, the wavelength of the light is changed to 70.0 nm, what is the effect compared
For the electromagnetic wave described in Exercise 1, what are (a) The frequency, in hertz, and (b) The energy, in joules per photon?Exercise 1A hypothetical electromagnetic wave is pictured here. What is the wavelength of this radiation? 1.17 nm
(A) Is there an energy level for the hydrogen atom, En = –2.69 x 10-20 J?(B) The energy of an electron in a hydrogen atom is -4.45 x 10-20 J. What level does it occupy?
When comet Shoemaker–Levy 9 crashed into Jupiter’s surface, scientists viewed the event with spectrographs. What did they hope to discover?
(A) Determine the wavelength of light absorbed in an electron transition from n = 2 to n = 4 in a hydrogen atom.(B) Refer to Figure 8-13 and determine which transition produces the longest wavelength line in the Lyman series of the hydrogen spectrum. What is the wavelength of this line in
The magnesium spectrum has a line at 266.8 nm. Which of these statements about this radiation is (are) correct? Explain.(a) It has a higher frequency than radiation with wavelength 402 nm.(b) It is visible to the eye.(c) It has a greater speed in a vacuum than does red light of wavelength 652
Which of the following electronic transitions in a hydrogen atom will lead to the emission of a photon with the shortest wavelength, n = 1 to n = 4, n = 4 to n = 2, n = 3 to n = 2?
The most intense line in the cerium spectrum is at 418.7 nm.(a) Determine the frequency of the radiation producing this line.(b) In what part of the electromagnetic spectrum does this line occur?(c) Is it visible to the eye? If so, what color is it? If not, is this line at higher or lower energy
(A) Determine the wavelength of light emitted in an electron transition from n = 5 to n = 3 in a Be3+ ion.(B) The frequency of the n = 3 to n = 2 transition for an unknown hydrogen-like ion occurs at a frequency 16 times that of the hydrogen atom. What is the identity of the ion?
An electron has a mass approximately 1/2000th of the mass of a proton. Assuming that a proton and an electron have similar wavelengths, how would their speeds compare?
(A) Assuming Superman has a mass of 91 kg, what is the wavelength associated with him if he is traveling at one-fifth the speed of light?(B) To what velocity (speed) must a beam of protons be accelerated to display a de Broglie wavelength of 10.0 pm? Obtain the proton mass from Table 2.1.Table 2.1
Without doing detailed calculations, determine which of the following wavelengths represents light of the highest frequency: (a) 6.7 x 10-4 cm; (b) 1.23 mm;(c) 80 nm; (d) 6.72 μm.
For a particle in a one-dimensional box, in which state (value of n) is the greatest probability of finding the particle at one-quarter the length of the box from either end?
Without doing detailed calculations, arrange the following electromagnetic radiation sources in order of increasing frequency: (a) A red traffic light;(b) A 91.9 MHz radio transmitter;(c) Light with a frequency of 3.0 x 1014 s-1;(d) Light with a wavelength of 49 nm.
(A) Superman has a mass of 91 kg and is traveling at one-fifth the speed of light. If the speed at which Superman travels is known with a precision of 1.5%, what is the uncertainty in his position?(B) What is the uncertainty in the speed of a beam of protons whose position is known with the
What type of orbital has three angular nodes and one radial node?
How long does it take light from the sun, 93 million miles away, to reach Earth?
The following orbital diagram represents an excited state of an atom. Identify the atom and give the orbital diagram corresponding to its ground state orbital diagram. [Ar] NNNNN 3d 4s 4p
(A) What is the fraction, as a percentage of the total probability of finding, between points at 50 pm and 75 pm, an electron in the n = 6 level of a one-dimensional box 150 pm long?(B) A particle is confined to a one-dimensional box 300 pm long. For the state having n = 3, at what points (not
In astronomy, distances are measured in light-years, the distance that light travels in one year. What is the distance of one light-year expressed in kilometers?
(A) Calculate the wavelength of the photon emitted when an electron in a box 5.0 x 101 pm long falls from the n = 5 level to the n = 3 level.(B) A photon of wavelength 24.9 nm excites an electron in a one-dimensional box from the ground state to the first excited state. Estimate the length of the
Determine (a) The energy, in joules per photon, of radiation of frequency 7.39 x 1015 s-1;(b) The energy, in kilojoules per mole, of radiation of frequency 1.97 x 1014 s-1.
(A) Can an orbital have the quantum numbers n = 3, ℓ = 0, and mℓ = 0?(B) For an orbital with n = 3 and mℓ = 1, what is (are) the possible value(s) of ℓ?
Determine (a) The frequency, in hertz, of radiation having an energy of 8.62 x 10-21 J/photon;(b) The wavelength, in nanometers, of radiation with 360 kJ/mol of energy.
(A) Write an orbital designation corresponding to the quantum numbers n = 3, ℓ = 1, and mℓ = 1.(B) Write all the combinations of quantum numbers that define hydrogen-atom orbitals with the same energy as the 3s orbital.
(A) Determine which set of the following quantum numbers (n, ℓ, mℓ, ms) is wrong and indicate why:(B) Identify the error in each set of quantum numbers below: (3,2,-21) (3,1,-2) (3,0,0) (230) (1.0.0-) (2-1,-1) (1,0,0,- 2
A certain radiation has a wavelength of 574 nm. What is the energy, in joules, of (a) One photon; (b) A mole of photons of this radiation?
(A) Which two of the following orbital diagrams are equivalent?(B) Does the following orbital diagram for a neutral species correspond to the ground state or an excited state? (c) 1s 2s A↓ 1s 2s 2p 2p (b) N 14 1s 2s (d) 1s 2s 2p 2p
What is the wavelength, in nanometers, of light with an energy content of 2112 kJ/mol? In what portion of the electromagnetic spectrum is this light?
Without doing detailed calculations, indicate which of the following electromagnetic radiations has the greatest energy per photon and which has the least: (a) 662 nm;(b) 2.1 x 10-5 cm; (c) 3.58 μm;(d) 4.1 x 10-6 m.
(A) Identify the element having the electron configuration 1s22s22p63s23p63d24s2.(B) Use spdƒ notation to show the electron configuration of iodine. How many electrons does the I atom have in its 3d subshell? How many unpaired electrons are there in an I atom?
Without doing detailed calculations, arrange the following forms of electromagnetic radiation in increasing order of energy per mole of photons: (a) Radiation with n = 3.0 x 1015 s-1; (b) An infrared heat lamp;(c) Radiation having λ = 7000 Å; (d) Dental X-rays.
(A) Represent the electron configuration of iron with an orbital diagram.(B) Represent the electron configuration of bismuth with an orbital diagram.
In what region of the electromagnetic spectrum would you expect to find radiation having an energy per photon 100 times that associated with 988 nm radiation?
(A) For an atom of Sn, indicate the number of (a) Electronic shells that are either filled or partially filled; (b) 3p electrons; (c) 5d electrons; and (d) Unpaired electrons.(B) Indicate the number of (a) Electrons in Y atoms; (b) Electrons in Ge atoms; and (c) Unpaired electrons in Au
High-pressure sodium vapor lamps are used in street lighting. The two brightest lines in the sodium spectrum are at 589.00 and 589.59 nm. What is the difference in energy per photon of the radiations corresponding to these two lines?
(A) Calculate the de Broglie wavelength of a helium atom at 25 °C and moving at the root-mean-square velocity. At what temperature would the average helium atom be moving fast enough to have a de Broglie wavelength comparable to that of the size of a typical atom, about 300 pm?(B) By using a
The lowest-frequency light that will produce the photoelectric effect is called the threshold frequency.(a) The threshold frequency for indium is 9.96 x 1014 s-1. What is the energy, in joules, of a photon of this radiation?(b) Will indium display the photoelectric effect with UV light? With
The minimum energy required to cause the photoelectric effect in potassium metal is 3.69 x 10-19 J. Will photoelectrons be produced when visible light shines on the surface of potassium? If 520 nm radiation is shone on potassium, what is the velocity of the ejected electrons?
Use the Balmer equation (8.4) to determine (a) The frequency, in s-1, of the radiation corresponding to n = 5;(b) The wavelength, in nanometers, of the line in the Balmer series corresponding to n = 7;(c) The value of n corresponding to the Balmer series line at 380 nm.Eq. 8.4

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