General Chemistry: Principles and Modern Applications (11th Edition)
11th Edition
ISBN: 9780132931281
Author: Ralph H. Petrucci, F. Geoffrey Herring, Jeffry D. Madura, Carey Bissonnette
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Textbook Question
Chapter 9, Problem 8E
Concerning the incomplete seventh period of the periodic table, what should be the
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
(a) Identify the number of electrons in the ground-state outer shell of atomic oxygen (atomic number 8).(b) How many electrons are in the ground-state outer shell of fluorine?
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?
Consider the following information about three atoms: (a) How are they similar to one another? (b) How do they differ from one another? (c) What are the members of such a group of atoms called? (d) Using the planetary model, draw the atomic configuration of 126C showing the relative position and numbers of its subatomic particles.
Chapter 9 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
Ch. 9 - Prob. 1ECh. 9 - Suppose that lanthanum (Z = 57) were a newly...Ch. 9 - The following densities, in grams per cubic...Ch. 9 - The blowing melting points are in degrees Celsius....Ch. 9 - Mendeleev's periodic table did not preclude the...Ch. 9 - Prob. 6ECh. 9 - Prob. 7ECh. 9 - Concerning the incomplete seventh period of the...Ch. 9 - For each of the following pairs, indicate the atom...Ch. 9 - Indicate the smallest and the largest species...
Ch. 9 - Explain why the radii of atoms do not simply...Ch. 9 - The masses of individual atoms can be determined...Ch. 9 - Which is (a) the smallest atom in group 13; (b)...Ch. 9 - How would you expect the sizes of the hydrogen...Ch. 9 - Prob. 15ECh. 9 - Explain why the generalizations presented in...Ch. 9 - Among the following ions, several pairs are...Ch. 9 - Prob. 18ECh. 9 - All the isoelectronic species illustrated in the...Ch. 9 - Prob. 20ECh. 9 - Use principles established in this chapter to...Ch. 9 - Are there any atoms for which the second...Ch. 9 - Some electron affinities are negative quantities,...Ch. 9 - How much energy, in pules, must be absorbed to...Ch. 9 - How much energy, in kilojoules, is required to...Ch. 9 - Prob. 26ECh. 9 - The production of gaseous bromide ions from...Ch. 9 - Use ionization energies and electron affinities...Ch. 9 - The Naa ion and the Ne atom are isoelectronic. The...Ch. 9 - Prob. 30ECh. 9 - Compare the elements Al, Si, S, and Cl. a. Place...Ch. 9 - Compare the elements Na, Mg, O, and P. a. Place...Ch. 9 - Unpaired electrons are found in only one of the...Ch. 9 - Which of the following species has the greatest...Ch. 9 - Which of the following species would you expect to...Ch. 9 - Write electron configurations consistent with the...Ch. 9 - Must all atoms with an odd atomic number be...Ch. 9 - Neither Co24 nor Co24 has 4s electrons in its...Ch. 9 - Use ideas presented in this chapter to indicate...Ch. 9 - Arrange the following atoms in order of increasing...Ch. 9 - Arrange the following species in order of...Ch. 9 - For the following groups of elements, select the...Ch. 9 - Prob. 43ECh. 9 - Of the species Naa, Na, F, and F-, which has the...Ch. 9 - Match each of the lettered items on the left with...Ch. 9 - Prob. 46ECh. 9 - Which of the following ions are unlikely to be...Ch. 9 - Which of the following ions are likely to be found...Ch. 9 - Four atoms and/or ions are sketched below in...Ch. 9 - Prob. 50IAECh. 9 - In Mendeleev's time, indium oxide, which is 82.5%...Ch. 9 - Instead of accepting the atomic mass of indium...Ch. 9 - Refer to Figure 9-11 and explain why the...Ch. 9 - Explain why the third ionization energy of Li(g)...Ch. 9 - Prob. 55IAECh. 9 - Prob. 56IAECh. 9 - Studies done in 1880 showed that a chloride of...Ch. 9 - Assume that atoms are herd spheres, and use the...Ch. 9 - When sodium chloride is strongly heated in a...Ch. 9 - Use information from Chapters 8 and 9 to calculate...Ch. 9 - Refer only to the periodic table on the inside...Ch. 9 - Refer to the footnote on page 393. Then use values...Ch. 9 - Prob. 63IAECh. 9 - Prob. 64IAECh. 9 - The work functions for a number of metals are...Ch. 9 - The following are a few elements and their...Ch. 9 - Gaseous sodium atoms absorb quanta with the...Ch. 9 - A method for estimating electron affinities is to...Ch. 9 - We have seen that the wave functions of...Ch. 9 - In your own words, define the following terms (a)...Ch. 9 - Briefly describe each of the following ideas or...Ch. 9 - Explain the important distinctions between each...Ch. 9 - Prob. 73SAECh. 9 - Prob. 74SAECh. 9 - Prob. 75SAECh. 9 - Prob. 76SAECh. 9 - Prob. 77SAECh. 9 - An ion that is isoelectronic with Se2- is (a) S2-...Ch. 9 - Write electron configurations to show the first...Ch. 9 - Explain why the first ionization energy of Mg is...Ch. 9 - Prob. 81SAECh. 9 - Prob. 82SAECh. 9 - Find three pairs of elements that are out of order...Ch. 9 - Prob. 84SAECh. 9 - Prob. 85SAECh. 9 - Prob. 86SAECh. 9 - Prob. 87SAECh. 9 - Prob. 88SAECh. 9 - In multielectron atoms many of the periodic trends...Ch. 9 - Consider a nitrogen atom in the ground state and...Ch. 9 - Prob. 91SAECh. 9 - Describe how the ionization energies of the ions...Ch. 9 - Prob. 93SAECh. 9 - Prob. 94SAECh. 9 - When compared to a nonmetal of the same period, a...Ch. 9 - Prob. 96SAECh. 9 - Which of the following has a smaller radius than a...Ch. 9 - Prob. 98SAECh. 9 - The electrons lost when Fe ionizes to Fe2- are (a)...Ch. 9 - Prob. 100SAE
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- How does Daltons atomic theory account for the Law of Conservation of Mass?arrow_forwardThe electron configuration of the isotope 16O is 1s22s22p4. What is the electron configuration of the isotope 18O?arrow_forward2-102 An element consists of 90.51% of an isotope with a mass of 19.992 amu, 0.27% of an isotope with a mass of 20.994 amu, and 9.22% of an isotope with a mass of 21.990 amu. Calculate the average atomic mass and identify the element.arrow_forward
- 2-101 Complete the following table: Symbol Atomic number Atomic weight Mass number # of protons # of neutrons # of electrons H 0 Li 4 3 Al 26 58 78 17 20arrow_forward2.42 What is a period in the periodic table? From what does it derive its name?arrow_forward2.84 Early attempts to arrange the elements often focused on atomic weight. Mendeleev considered a number of properties in addition to atomic weight, so he realized that some elements seemed out of place when ordered by atomic weight. Using the modern periodic table, identify elements for which Mendeleev must have had to switch the order in order to get the correct sequence of elements.arrow_forward
- 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) 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_forwardPredict and test the behavior of α particles fired at a “plum pudding” model atom.(a) Predict the paths taken by α particles that are fired at atoms with a Thomson’s plum pudding model structure.Explain why you expect the α particles to take these paths.(b) If α particles of higher energy than those in (a) are fired at plum pudding atoms, predict how their paths will differ from the lower-energy α particle paths. Explain your reasoning.(c) Now test your predictions from (a) and (b). Open the Rutherford Scattering simulation (http://openstaxcollege.org/l/16PhetScatter) and select the “Plum Pudding Atom” tab. Set “Alpha ParticlesEnergy” to “min,” and select “show traces.” Click on the gun to start firing α particles. Does this match your prediction from (a)? If not, explain why the actual path would be that shown in the simulation. Hit the pause button,or “Reset All.” Set “Alpha Particles Energy” to “max,” and start firing α particles. Does this match your prediction from (b)? If not,…arrow_forwardA neutral atom of an element has two electrons with n=1,eight electrons with n=2,eight electrons with n=3 and one electron with n=4 and has mass number of 39.Deducw the following from the above information. (I) the atomic number of the element (ii) the number of neutrons in the nucleus (iii) total number of s electrons (iv) total number of p electrons (v) the group the element belongs toarrow_forward
- In the table below, I1 – I6 represent first 6 ionization energies of a certain element. All units are kJ/mol. I1 I2 I3 I4 I5 I6 738 1450 7730 10500 13600 18000 This element is in the 3rd row of the periodic table, the row starting with Na. Identify the element, and explain your reasoning, based on the data in the above table.arrow_forwardWhich of the following describes the element Ba? Choose all that apply:(a) is very reactive as a metal; (b) consists of diatomic molecules in elemental form; (c) forms an ion with a charge of 2; (d) forms a cation that is isoelectronic with a noble gas; (e) reacts with alkali metals to form salts; (f) is one of the group of the least reactive elements.arrow_forward(c) Silicon (Si) is the most common chemical element in today's semiconductor industry. It has an atomic number of 14 and belongs to the Group IV (4) of the periodic table with its most common isotope being Si-29. (i) (ii) (iii) Explain what an isotope is. How many protons and how many neutrons are in the nucleus of this Silicon isotope? What is the electron configuration of Si?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Introductory Chemistry: An Active Learning Approa...ChemistryISBN:9781305079250Author:Mark S. Cracolice, Ed PetersPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage Learning
Chemistry: Matter and Change
Chemistry
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Glencoe/McGraw-Hill School Pub Co
Introduction to General, Organic and Biochemistry
Chemistry
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Introductory Chemistry: An Active Learning Approa...
Chemistry
ISBN:9781305079250
Author:Mark S. Cracolice, Ed Peters
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry for Today: General, Organic, and Bioche...
Chemistry
ISBN:9781305960060
Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen
Publisher:Cengage Learning
Quantum Numbers, Atomic Orbitals, and Electron Configurations; Author: Professor Dave Explains;https://www.youtube.com/watch?v=Aoi4j8es4gQ;License: Standard YouTube License, CC-BY
QUANTUM MECHANICAL MODEL/Atomic Structure-21E; Author: H to O Chemistry;https://www.youtube.com/watch?v=mYHNUy5hPQE;License: Standard YouTube License, CC-BY