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Pearson ChemistryMatta, Staley, Waterman, Wilbraham 3,747 solutions Physical Science Concepts in Action2nd EditionFrank, Wysession, Yancopoulos 1,490 solutions Glencoe Physical Science1st EditionMcLaughlin, Thompson, Zike 1,515 solutions Compared to the atomic radius of S, the atomic radius of Al is: A. smaller, due to decreased nuclear charge. Answer D Moving left to right across a period, nuclear charge increases due to increasing atomic number (number of protons). As the positive nuclear charge increases, effective nuclear charge increases and electrons are pulled closer to the nucleus, resulting in a decreased atomic radius. Aluminum is therefore larger than sulfur. This problem can also be treated as a two-by-two if you know the periodic trend for atomic radius, which decreases up and to the right. Based on this trend, it can be determined that Al is larger than S, eliminating the choices using "smaller." The distinction between the final two choices can then be determined based on the effect of nuclear charge. What is the reactivity, as indicated by the tendency to lose an electron, of sodium compared to potassium? A. This cannot be determined from the information given. Answer C Reactivity of metallic elements increases down a column of the periodic table. This increase in reactivity corresponds with increased shielding from inner electron shells, increased atomic radius, and decreased ionization energy. Thus, electrons are easier to remove in potassium versus sodium. Give the electron configuration of a ground state Zn2+ ion. A. [Ar] 4s23d8 Answer B First, eliminate choices that involve the wrong number of electrons. Since an atom of zinc contains 30 electrons, a Zn2+ ion contains 28, eliminating [Ar] 4s23d10. Recall that when electrons are removed from a transition metal such as zinc, the electrons always come from the valence s orbital first. Therefore, the electron configuration, [Ar] 3d10 is the correct one. In organic solution, F- deprotonates dissolved HCl. Which of the following explains this observation? A. F- has a smaller radius than Cl-. Answer: A Since F- has a smaller radius than does Cl-, it is less stable with excess charge, and therefore a better Bronsted base. It outcompetes Cl- for the proton. Which of the following appropriately ranks the atoms from smallest to largest atomic radius? A. Ge < Al < P < C Answer B This is a ranking question, which is best approached by evaluating the extremes. For a given family, atomic radius increases as period increases due to greater shielding, which means that Ge must be larger than C. This eliminates choices Ge < P < Al < C and Ge < Al < P < C. Now, we must evaluate Al vs. P. These two atoms are in the same period. However, atomic radius decreases as you go left to right in the same period due to a greater effective nuclear charge, which means that P is smaller than Al. Thus, the atoms from smallest to largest atomic radius is C < P < Al < Ge Which of the following is true of ionization energy? A. It increases with period, and the second ionization energy is greater than the first. Answer D his is a 2 x 2 question that is best approached by evaluating one of the arguments to eliminate answer choices. As period increases, ionization energy decreases due in part to the greater degree of shielding present. Thus, we can eliminate the two choices that begin with the choice "it increases." Evaluating the other argument, the second ionization energy is always greater than the first because electrons are more tightly bound after one is displaced (a more positively charged atom is less likely to give up an additional electron). Thus, ionization energy decreases with period and the second ionization energy is greater than the first. Which of the following gives the ground-state electron configuration of a calcium atom once it acquires an electric charge of +2? A. [Ar] 4s23d2 Answer C The ground-state electron configuration of a calcium atom once it acquires an electric charge of +2 is [Ar]. A calcium atom normally contains 20 electrons, so if it acquires a charge of +2, it must have lost 2 electrons, leaving just 18. Only [Ar] accounts for 18 electrons. What are the 7 common strong acids? HCl - Hydrochloric Which is the electron configuration for zinc?[Ar] 3d¹⁰ 4s²Zinc / Electron configurationnull
What is Zn 30 electron configuration?Electronic Configuration of First 30 Elements with Atomic Numbers. Which of the following is the correct electron configuration for Zn2+ quizlet?Since an atom of zinc contains 30 electrons, a Zn2+ ion contains 28, eliminating [Ar] 4s23d10. Recall that when electrons are removed from a transition metal such as zinc, the electrons always come from the valence s orbital first. Therefore, the electron configuration, [Ar] 3d10 is the correct one.
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What is the electron configuration for zinc quizlet?
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