Chemistry: Principles and Practice
3rd Edition
ISBN: 9780534420123
Author: Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher: Cengage Learning
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Textbook Question
Chapter 8, Problem 8.71QE
What is the electron configuration of the Ba3+ ion? Suggest a reason why this ion is not normally found in nature.
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Write electron configurations for the following ions of main group elements: (a) N3−, (b) Ba2+, and (c) Be2+.
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whose electron configuration is [ Kr] 5s², 4d10, 5p6.
Species that have the same number of electrons are described as isoelectronic. What +2 ion is isoelectronic with Na+? What −2 ion?
Chapter 8 Solutions
Chemistry: Principles and Practice
Ch. 8 - Define an isoelectronic series. Give the symbols...Ch. 8 - Prob. 8.2QECh. 8 - Graph the atomic radii versus atomic number of the...Ch. 8 - Prob. 8.4QECh. 8 - Prob. 8.5QECh. 8 - Prob. 8.6QECh. 8 - Prob. 8.7QECh. 8 - Prob. 8.8QECh. 8 - Prob. 8.9QECh. 8 - Prob. 8.10QE
Ch. 8 - Prob. 8.11QECh. 8 - Prob. 8.12QECh. 8 - Prob. 8.13QECh. 8 - Prob. 8.14QECh. 8 - Prob. 8.15QECh. 8 - Prob. 8.16QECh. 8 - Prob. 8.17QECh. 8 - Prob. 8.18QECh. 8 - Explain why the electron affinity of lithium is...Ch. 8 - Prob. 8.20QECh. 8 - Prob. 8.21QECh. 8 - Prob. 8.22QECh. 8 - Prob. 8.23QECh. 8 - Prob. 8.24QECh. 8 - Prob. 8.25QECh. 8 - Prob. 8.26QECh. 8 - Prob. 8.27QECh. 8 - Prob. 8.28QECh. 8 - Prob. 8.29QECh. 8 - Prob. 8.30QECh. 8 - Prob. 8.31QECh. 8 - Prob. 8.32QECh. 8 - Prob. 8.33QECh. 8 - Prob. 8.34QECh. 8 - Prob. 8.35QECh. 8 - Prob. 8.36QECh. 8 - Prob. 8.37QECh. 8 - Prob. 8.38QECh. 8 - Write the symbols for a cation and an anion that...Ch. 8 - Prob. 8.40QECh. 8 - Prob. 8.41QECh. 8 - What neutral atoms are isoelectronic with the...Ch. 8 - Prob. 8.43QECh. 8 - Prob. 8.44QECh. 8 - Prob. 8.45QECh. 8 - Prob. 8.46QECh. 8 - Prob. 8.47QECh. 8 - Prob. 8.48QECh. 8 - Prob. 8.49QECh. 8 - Prob. 8.50QECh. 8 - Prob. 8.51QECh. 8 - Prob. 8.52QECh. 8 - Prob. 8.53QECh. 8 - Prob. 8.54QECh. 8 - Prob. 8.55QECh. 8 - Of the atoms with the electron configurations...Ch. 8 - Prob. 8.57QECh. 8 - Prob. 8.58QECh. 8 - Prob. 8.59QECh. 8 - Prob. 8.60QECh. 8 - Prob. 8.61QECh. 8 - Prob. 8.62QECh. 8 - Prob. 8.63QECh. 8 - Prob. 8.64QECh. 8 - Prob. 8.65QECh. 8 - Prob. 8.66QECh. 8 - Prob. 8.67QECh. 8 - Prob. 8.68QECh. 8 - Prob. 8.69QECh. 8 - Prob. 8.70QECh. 8 - What is the electron configuration of the Ba3+...Ch. 8 - Prob. 8.72QECh. 8 - Prob. 8.73QECh. 8 - Prob. 8.74QECh. 8 - Prob. 8.75QECh. 8 - Prob. 8.76QECh. 8 - Prob. 8.77QECh. 8 - Prob. 8.78QECh. 8 - Prob. 8.79QECh. 8 - Prob. 8.80QECh. 8 - Prob. 8.81QECh. 8 - Prob. 8.82QECh. 8 - Prob. 8.83QECh. 8 - Prob. 8.84QECh. 8 - Prob. 8.85QECh. 8 - Prob. 8.86QECh. 8 - Prob. 8.87QECh. 8 - Prob. 8.88QECh. 8 - Prob. 8.89QECh. 8 - Prob. 8.90QECh. 8 - Palladium, with an electron configuration of [Kr]...Ch. 8 - Prob. 8.92QECh. 8 - Prob. 8.93QECh. 8 - Prob. 8.94QECh. 8 - Prob. 8.95QECh. 8 - Prob. 8.96QECh. 8 - Prob. 8.97QECh. 8 - Prob. 8.98QECh. 8 - Arrange the elements lithium, carbon, and oxygen...Ch. 8 - Prob. 8.100QECh. 8 - Prob. 8.101QECh. 8 - Prob. 8.102QECh. 8 - Prob. 8.103QECh. 8 - Prob. 8.104QECh. 8 - Prob. 8.105QECh. 8 - Prob. 8.106QECh. 8 - Prob. 8.107QE
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- If potassium chlorate has the formula KClO3, what formula would you expect for lithium bromate?arrow_forwardAn ion M2+ has the configuration [Ar]3d2, and an atom has the configuration [Ar]4s2. Identify the ion and the atom.arrow_forwardWrite the electron configuration for each of the following ions: (a) As3 (b) I (c) Be2+ (d) Cd2+ (e) O2 (f) Ga3+ (g) Li+ (h) N3 (j) Sn2+ (j) Co2+ (k) Fe2+ (1) As3+arrow_forward
- Give the ground-state electron configurations of the following elements: (a) P (b) Tc (c) Hoarrow_forwardSolid phosphorus pentabromide, PBr5, has been shown to have the ionic structure [PBr4] [Br]. Write the electron-dot formula of the PBr4+ cation.arrow_forwardThe ionic radii of the ions S2–, Cl–, and K+ are 184, 181, 138 pm respectively. Explain why these ions have different sizes even though they contain the same number of electrons.arrow_forward
- what is be2+ valence electron configuration?arrow_forwardPlease solve all questions, including the subparts. What trend in first ionization energy occurs as you go up a group on the periodic table? Explain why this occurs. What trend in atomic radius occurs as you go up a group on the periodic table? Explain why this occurs. Arrange the following in order of increasing electronegativity: Br, F, I, Cl Write four quantum numbers to describe the highest energy electron in the magnesium atom. Be sure to include the four symbols and four correct numbers. Arrange the following in order of increasing first ionization energy: Br, F, I, Clarrow_forwardTo which group of the periodic table does the general valence electron configuration ns2np4 correspond?arrow_forward
- Write the electron configuration for P2. How many electrons are in the 3p orbital? How many total valence electrons are in P2? Name a neutral element that is isoelectronic with P2.arrow_forwardAtoms of which group in the periodic table have the valence shell electron configuration of ns2nd1?arrow_forwardWhich of the following statements about the formation of ions is true? Group 2 (or 2A) elements form +1 charge cations. When an atoms loses electrons to become an ion, its radius decreases. Metals gain electrons to form negative ions. Atoms with a high ionization energy tend to lose electrons easily. Some non-metals can form ions with variable charges.arrow_forward
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