Inorganic Chemistry
5th Edition
ISBN: 9781292134147
Author: Housecroft, Catherine E.
Publisher: Pearson,
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Textbook Question
Chapter 1, Problem 5P
(a) By using the data in appendix 5, account for the isotopic distribution shown in Fig 1.1b. (b) The mass spectrum of
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The sum of IE1through IE₄ for Group 4A(14) elements shows a decrease from C to Si, a slight increase from Si to Ge, adecrease from Ge to Sn, and an increase from Sn to Pb. (a) What is the expected trend for IEs down a group? (b) Suggest a reason for the deviations in Group 4A(14).(c) Which group might show even greater deviations?
Boron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively.
(a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B?
(b) Draw the orbital diagram for an atom of 11B. Which electrons are the valence electrons?
(c) Indicate three ways in which the 1s electrons in boron differ from its 2s electrons.
(d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation for the reaction of solid boron with fluorine gas.
(e) ΔHf° for BF3(g) is -1135.6 kj/mol. Calculate the standard enthalpy change in the reaction of boron with fluorine.
(f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?
(a) Briefly describe how the atomic radii and ionization energies of group 1A(1) elements compared with those of
group 8A(18). Also, explain why the values of these properties are so different between these two groups.
2.
Chapter 1 Solutions
Inorganic Chemistry
Ch. 1 - Chromium has four isotopes C2450r, C2452r, C2453r...Ch. 1 - Prob. 2PCh. 1 - Using the list of naturally occurring isotopes in...Ch. 1 - Hydrogen possesses three isotopes, but tritium ,...Ch. 1 - (a) By using the data in appendix 5, account for...Ch. 1 - Calculate the corresponding wavelength of...Ch. 1 - State which of the following n'n transitions in...Ch. 1 - Calculate the energy (in kJ per mole of photons)...Ch. 1 - 1.9 Four of the lines in Balmer series are at...Ch. 1 - 1.10 Using the Bohr model, determine the values of...
Ch. 1 - 1.11 How is the (a) energy and (b) size of an ns...Ch. 1 - 1.12 Write down a set of quantum numbers that...Ch. 1 - Do the three 4p atomic orbitals possess the same...Ch. 1 - How many radial nodes does each of the following...Ch. 1 - 1.15 Comment on the differences between plots of...Ch. 1 - 1.16 Write down the sets of quantum numbers that...Ch. 1 - Write down the three sets of quantum numbers that...Ch. 1 - How many atomic orbitals make up the set with n=4...Ch. 1 - Prob. 19PCh. 1 - (a) Will a plot of R(r) for the 1s atomic orbital...Ch. 1 - Prob. 21PCh. 1 - Prob. 22PCh. 1 - Write down the six sets of quantum numbers that...Ch. 1 - For a neutral atom, X, the following atomic...Ch. 1 - Using the concepts of shielding and penetration,...Ch. 1 - For each of the following atoms, write down a...Ch. 1 - 1.27 Draw energy level diagrams (see Fig. 1.15) to...Ch. 1 - 1.28 Write down the ground state electronic...Ch. 1 - Write down (with reasoning) the ground state...Ch. 1 - Draw energy level diagrams to show the ground...Ch. 1 - The ground state electronic configuration of a...Ch. 1 - (a) Write down an equation that defines the...Ch. 1 - 1.33 The first four ionization energies of an atom...Ch. 1 - 1.34 In Fig. 1.16, identify the trend in the first...Ch. 1 - 1.35 Figure 1.17 shows the values of for the...Ch. 1 - Using the data in Table 1.5, determine a value for...Ch. 1 - Prob. 37PCh. 1 - What is the evidence that the aufbau principle is...Ch. 1 - The first list in the table on the left contains...Ch. 1 - Prob. 40PCh. 1 - Using data from appendix 8, construct a graph to...Ch. 1 - The sign convention for electron affinity can...Ch. 1 - Prob. 43PCh. 1 - 1.45 Figure 1.18 shows the emission spectrum of...
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- Until the early 1960s the group 8A elements were called the inert gases; before that they were called the rare gases. The term rare gases was dropped after it was discovered that argon accounts for roughly 1% of Earth’s atmosphere. (a) Why was the term inert gases dropped? (b) What discovery triggered this change in name? (c)What name is applied to the group now?arrow_forwardBoron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively.(a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B? (b) Drawthe orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons inboron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation forthe reaction of solid boron with fluorine gas. (e) ΔHf° for BF31g2 is -1135.6 kJ>mol. Calculate the standard enthalpy change in thereaction of boron with fluorine. (f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?arrow_forwardUranium-238 (U238) has three more neutrons than uranium-235 (U235). Compared to the speed of sound in a bar of U235, is the speed of sound in a bar of U238 higher, lower, or the same? There are several factors that play a role. (a) Chemically, the atoms of these two isotopes behave in essentially identical ways, since the number of protons (92) is identical and the clouds of 92 electrons are nearly identical. The interatomic distance, and the effective "stiffness" of the interatomic bond, both depend on the chemical properties of the atoms. Therefore, which of the following statements are true? O The effective stiffness of the interatomic "spring" is greater for U238 because the mass is greater. O The effective stiffness of the interatomic "spring" is the same in the two isotopes, since this "spring" is a model for the interactions of the outer electrons, which are the same for different isotopes of the same atom. O An atom with more mass in the nucleus is bigger, so the distance…arrow_forward
- What is the molar mass of ginkgolide B (C 20H 24O 10), a complex compound isolated from the ginkgo tree? Extracts of the roots, bark, and seeds of the ginkgo tree comprise the most widely taken herbal supplements used today.arrow_forward(a)List the three halogens studied in decreasing order of reactivity, starting with the most reactive and ending with the least reactive. (b) Suggest a cause for the order of reactivities that you listed for the halogens in question (a) based on the electron affinity simulation on the table Combination Initial Top Layer Color Final Top Layer Color Initial Halogen Final Halogen Reaction? (Yes or No) Cl2 + NaBr Clear yellowish orange Cl2 NaBr yes Cl2 + NaI Clear purple Cl2 NaI yes Br2 + NaCI Yellowish Orange yellowish orange Br2 Br2 no Br2 + NaI yellowish orange purple Br2 NaI yes I2 + NaCl purple purple I2 I2 no I2 + NaI purple purple I2 I2 noarrow_forward(a) The third row element with the largest first ionization energy. (b) The Group 3A element with the largest first ionization energy. (c) The Group 3A element with the largest atomic radius.arrow_forward
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