Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN: 9781938168390
Author: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher: OpenStax
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Textbook Question
Chapter 6, Problem 81E
Compare both the numbers of protons and electrons present in each to rank the following ions in order of increasing radius:
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Compare both the numbers of protons and electrons present in each to rank the following ions in order of increasing radius: As3–, Br–, K+, Mg2+.
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Na+, Te2−, Li+, Br−
Based on their positions in the periodic table, list the following ions in order of increasing radius: K+, Ca2+, Al3+, Si4+.
Chapter 6 Solutions
Chemistry by OpenStax (2015-05-04)
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Similar questions
- What neutral atoms are isoelectronic with the following ions? (a) Pb4+ (b) Br (c) S2 (d) Ni3+arrow_forwardIndicate whether or not each of the following pairs of atoms/ions are isoelectronic. a. K+ and Ar b. Al3+ and Cl c. S and Cl d. Na+ and Mg2+arrow_forwardWhat is the electron configuration of the Ba3+ ion? Suggest a reason why this ion is not normally found in nature.arrow_forward
- 2-47 Which element in each pair is more metallic? (a) Silicon or aluminum (b) Arsenic or phosphorus (c) Gallium or germanium (d) Gallium or aluminumarrow_forwardHow many unpaired electrons are there 111 the following ions? (a) V3+(b) Sn4+(c) I-(d) W4+arrow_forwardplease explain step by steparrow_forward
- List the following ions in order of increasing radius. (Use the appropriate <, =, or > symbol to separate substances in the list.) Te2−, Br−, Na+, Li+arrow_forwardA hydrogen-like ion is an ion containing only one electron. The energies of the electron in a hydrogen-like ion are given by (2.180 × 10-¹5 1) 2² (1) J) E = kJ where n is the principal quantum number, and Z is the atomic number of the element. Calculate the ionization energy, in your answer to 4 significant digits. mol Note: Reference the Fundamental constants table for additional information. ·2+ of the Li²+ ion. Round Iarrow_forwardArrange these atoms and ions in order of increasing radius: Cs+Cs+, Ba2+Ba2+, I−I−.arrow_forward
- List the following ions in order of increasing radius: Li+, Mg2+, Br–, Te2–.arrow_forwardAluminum (Al) and silicon (Si) are in the same row (period) on the periodic table. The atomic radius of aluminum is 125 pm, while the atomic radius of silicon is 110 pm. Why is the aluminum atom larger than the silicon atom? Choose the best explanation. O Aluminum contains more electrons than silicon, so the electron cloud is larger. O The valence electrons in aluminum experience a lower effective nuclear charge than those in silicon, so they aren't pulled as strongly toward the nucleus. Valence electrons in aluminum are attracted to only 13 protons, while those in silicon are attracted to 14 protons, so the valence electrons aren't pulled as strongly toward the nucleus in aluminum. O Atomic radius decreases left-to-right on the periodic table and aluminum is farther to the left.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
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