EBK GENERAL CHEMISTRY
11th Edition
ISBN: 8220103631259
Author: Bissonnette
Publisher: YUZU
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Textbook Question
Chapter 9, Problem 83SAE
Find three pairs of elements that are out of order in the periodic table in terms of their
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The periodic table is the most important organizing principle in chemistry. There is a regular progression in the periodic table that reflects a similar regularity in the structures and properties of the different elements. If you know the properties of any one element in a group, you can make a good guess at the properties
of every other element in the same group and even the elements in neighboring groups. Familiarizing yourself with the structure and arrangement of the periodic table early on will help you later on in chemistry.
Part A
Classify the following elements as main group elements, transition metals, or inner transition metals.
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Ca Sn Fm Pd Zn S
Transition metals
Inner transition metals
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Explain why the rows in the periodic table become progressively longer as we move down the table. For example, the first row contains two elements, the second and third rows each contain eight elements, and the fourth and fifth rows each contain 18 elements.
What would be your reaction to a claim that a new element had been discovered, and it fit between tin (Sn) and antimony (Sb) in the periodic table?
Chapter 9 Solutions
EBK GENERAL CHEMISTRY
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
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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
- In many Periodic Tables, a zig–zag line slanting down and to the right is shown in the p–block of the Table. Discuss the periodic trends in atomic properties of the elements that explain the shape, position and meaning of this line.arrow_forward8.Pick four elements in the main group (representative element) of the fourth period. a.Write its abbreviated electron configuration. b.Write the correct formula for its oxide. If it forms more than one oxide, you may list them all, but it is not necessary. If it does not form an oxide, state that. c.Is the most common ion the element forms larger or smaller than its neutral atom? Explain your answer in terms of electronic shells/subshells.arrow_forwardDescribe the basic features of the periodic tablearrow_forward
- Based on results of his study of atomic x-ray spectra, Moseley discovered a relationship that replaced atomic mass as the crite-rion for ordering the elements. By what criterion are the elements now ordered in the periodic table? Give an example of a sequence of element order that was confirmed by Moseley’s findings.arrow_forwardWhat statement best describes how the periodic table is organized? All elements in a period have the same number of electrons as there are elements in the period. The elements are arranged so that elements in a group all have the same valence subshell and thus have similar properties. All elements in a period can have up to the number of electrons as there are elements in a period. The period number represents the number of the valence shell.arrow_forwardThe lanthanides are a series of elements in the periodic table, from Z = 57 to Z = 70, that appear in a row set below the main table. Explain why there are exactly 14 elements in this row.arrow_forward
- Arrange the given elements from largest atomic radius to smallest atomic radius. Explain your reasoning in the given space here in this question. Only use qualitative information (meaning you have to use the trends you learned in the class, you cannot use atomic radius numbers to answer this question). Your explanation should clearly indicate why you are expecting that arrangement. K, Ne, Ar, Na, Parrow_forwardThe maximum number of valence electrons that any element in the periodic table may have is eight. True or False?arrow_forwardWhy is the group A elements (s-block and the p-block) are called the representative elements?arrow_forward
- 11. How do the core charges for H, Li, and Na compare to each other? Based on this answer and their respective ionization energies, which species has the valence shell with the largest radius? Which has the valence shell with the smallest radius? 12. Can you deduce a trend in ionization energy as you move from left to right across a period (row)? Can you deduce a trend in core charge as you move from left to right across a period (row)? Explain.arrow_forward15. (a) b) Identify the element that is described by the following information. Refer to a periodic table if necessary. It is a group 14 (III A) metalloid in the 3rd period. It is a group 15 (VA) metalloid in the 5th period. It is the other metalloid in group 15 (VA). d) It is a halogen that exists in the liquid state at room temperature. 16. What is the relationship between electron arrangement and the organization of elements in the periodic table?arrow_forwardA ceramic plate has a shiny rim. The ceramic plate is mostly composed of silicon and oxygen atoms. The shiny rim is mostly silver. When the plate is heated in a microwave oven, sparks are observed. Compare the ionization energy values of silver to those of the silicon and oxygen atoms. Explain what is happening in the oven. Why are microwaveable containers usually non-metallic? Why are most pots and pans metallic?arrow_forward
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