Chemistry: Structure and Properties Custom Edition for Rutgers University General Chemistry
15th Edition
ISBN: 9781269935678
Author: Nivaldo J. Tro
Publisher: Pearson Education
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Question
Chapter 4, Problem 99E
Interpretation Introduction
To determine: The substitute for K+.
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Suppose you were trying to find a substitute for K+ in nerve signal transmission. Where would you begin your search? What ions would be most like K+ ? For each ion you propose, explain the ways in which it would be similar to K+ and the ways it would be different. Refer to periodic trends in your discussion.
Suppose you were trying to find a substitute for K+ for some application. Where would you begin your search? Which ions are most like K+? For each ion you propose, explain the ways in which it is similar to K+ and the ways it is different. Refer to periodic trends in your discussion.
Suppose you were trying to find a substitute for Na+ for some application. Where would you begin your search? What ions are most like Na+? For each ion you propose, explain the ways in which it is similar to Na+ and the ways it is different. Use periodic trends in your discussion.
Chapter 4 Solutions
Chemistry: Structure and Properties Custom Edition for Rutgers University General Chemistry
Ch. 4 - 1. According to Coulomb's law, if the separation...Ch. 4 - Prob. 2SAQCh. 4 - Choose the correct electron configuration for Se....Ch. 4 - Prob. 4SAQCh. 4 - Which set of four quantum numbers corresponds to...Ch. 4 - Prob. 6SAQCh. 4 - Which statement is true about electron shielding...Ch. 4 - Prob. 8SAQCh. 4 - What is the electron configuration for Fe2+?...Ch. 4 - Which species is diamagnetic? Zn Cr 2+ C Mn
Ch. 4 - Prob. 11SAQCh. 4 - Prob. 12SAQCh. 4 - Prob. 13SAQCh. 4 - Prob. 14SAQCh. 4 - Prob. 15SAQCh. 4 - Prob. 16SAQCh. 4 - What are periodic properties?Ch. 4 - Use aluminum as an example to explain how density...Ch. 4 - Explain the contributions of Dobereiner and...Ch. 4 - Who is credited with arranging the periodic table?...Ch. 4 - Prob. 5ECh. 4 - Prob. 6ECh. 4 - What is an electron configuration? Provide an...Ch. 4 - Prob. 8ECh. 4 - Prob. 9ECh. 4 - What is penetration? How does the penetration of...Ch. 4 - Why are the sublevels within a principal level...Ch. 4 - Prob. 12ECh. 4 - Prob. 13ECh. 4 - What are degenerate orbitals? According to Hund’s...Ch. 4 - List all orbitals from 1s through 5s according to...Ch. 4 - Prob. 16ECh. 4 - Copy this blank periodic table onto a sheet of...Ch. 4 - Explain why the s block in the periodic table has...Ch. 4 - Explain why the rows in the periodic table become...Ch. 4 - Explain the relationship between a main-group...Ch. 4 - Explain the relationship between an element's row...Ch. 4 - Which of the transition elements in the first...Ch. 4 - Explain how to write the electron configuration...Ch. 4 - Explain the relationship between the properties of...Ch. 4 - Prob. 25ECh. 4 - Prob. 26ECh. 4 - What is effective nuclear charge? What is...Ch. 4 - When an alkali metal forms an ion, what is the...Ch. 4 - When a halogen forms an ion, what is the charge of...Ch. 4 - Use the concepts of effective nuclear charge,...Ch. 4 - For transition elements, describe the trends in...Ch. 4 - Prob. 32ECh. 4 - Explain how to write an electron configuration for...Ch. 4 - Prob. 34ECh. 4 - Prob. 35ECh. 4 - Prob. 36ECh. 4 - What are the exceptions to the periodic trends in...Ch. 4 - Prob. 38ECh. 4 - Prob. 39ECh. 4 - What is metallic character? What are the observed...Ch. 4 - Prob. 41ECh. 4 - Prob. 42ECh. 4 - Determine whether each element is a main-group...Ch. 4 - Determine whether each element is a transition...Ch. 4 - Write the full electron configuration for each...Ch. 4 - Prob. 46ECh. 4 - Write the full orbital diagram for each element. N...Ch. 4 - Prob. 48ECh. 4 - Use the periodic table to write the electron...Ch. 4 - Use the periodic table to determine the element...Ch. 4 - Use the periodic table to determine each quantity....Ch. 4 - Use the periodic table to determine each quantity....Ch. 4 - Prob. 53ECh. 4 - Prob. 54ECh. 4 - Determine the number of valence electrons in each...Ch. 4 - Prob. 56ECh. 4 - Which outer electron configuration would you...Ch. 4 - Prob. 58ECh. 4 - Prob. 59ECh. 4 - List the number of valence electrons in each...Ch. 4 - Which pair of elements do you expect to be most...Ch. 4 - Prob. 62ECh. 4 - Predict the charge of the ion formed by each...Ch. 4 - Predict the charge of the ion formed by each...Ch. 4 - According to Coulomb’s law, which pair of charged...Ch. 4 - Prob. 66ECh. 4 - Prob. 67ECh. 4 - Arrange the atoms according to decreasing...Ch. 4 - If core electrons completely shielded valence...Ch. 4 - In Section 3.6/, we estimated the effective...Ch. 4 - Prob. 71ECh. 4 - Choose the larger atom in each pair. Sn or Si Br...Ch. 4 - Arrange these elements in order of increasing...Ch. 4 - Arrange these elements in order of decreasing...Ch. 4 - Write the electron configuration for each ion. O2...Ch. 4 - Write the electron configuration for each ion. Cl...Ch. 4 - Write orbital diagrams for each ion and determine...Ch. 4 - Write orbital diagrams for each ion and determine...Ch. 4 - Which is the larger species in each pair? LiorLi+...Ch. 4 - Which is the larger species in each pair? SrorSr2+...Ch. 4 - Arrange this isoelectronic series in order of...Ch. 4 - Arrange this isoelectronic series in order of...Ch. 4 - Choose the element with the higher first...Ch. 4 - Prob. 84ECh. 4 - Arrange these elements in order of increasing...Ch. 4 - Prob. 86ECh. 4 - For each element, predict where the “jump” occurs...Ch. 4 - Prob. 88ECh. 4 - Choose the element with the more negative (more...Ch. 4 - Prob. 90ECh. 4 - Choose the more metallic element in each pair....Ch. 4 - Prob. 92ECh. 4 - Prob. 93ECh. 4 - Prob. 94ECh. 4 - Prob. 95ECh. 4 - Prob. 96ECh. 4 - Both vanadium and its 3+ ion are paramagnetic. Use...Ch. 4 - Use electron configurations to explain why copper...Ch. 4 - Prob. 99ECh. 4 - Suppose you were trying to find a substitute for...Ch. 4 - Prob. 101ECh. 4 - Which pair of elements would you expect to have...Ch. 4 - Consider these elements: N, Mg, O, F, Al. Write...Ch. 4 - Consider these elements: P, Ca, Si, S, Ga. Write...Ch. 4 - Prob. 105ECh. 4 - Explain why vanadium (radius = 134 pm) and copper...Ch. 4 - The lightest noble gases, such as helium and neon,...Ch. 4 - The lightest halogen is also the most chemically...Ch. 4 - Prob. 109ECh. 4 - Prob. 110ECh. 4 - Prob. 111ECh. 4 - Write the electronic configurations of the six...Ch. 4 - You have cracked a secret code that uses elemental...Ch. 4 - The electron affinity of sodium is lower than that...Ch. 4 - Use Coulomb’s law to calculate the ionization...Ch. 4 - Prob. 116ECh. 4 - Consider the densities and atomic radii of the...Ch. 4 - Prob. 118ECh. 4 - Consider the metals in the first transition...Ch. 4 - Imagine a universe in which the value of ms can be...Ch. 4 - A carbon atom can absorb radiation of various...Ch. 4 - Only trace amounts of the synthetic element...Ch. 4 - What is the atomic number of the as yet...Ch. 4 - The trend in second ionization energy for the...Ch. 4 - Unlike the elements in groups 1A and 2A, those in...Ch. 4 - Using the data in Figures 3.19 and 3.20/,...Ch. 4 - Prob. 127ECh. 4 - Prob. 128ECh. 4 - The heaviest known alkaline earth metal is radium,...Ch. 4 - Predict the electronic configurations of the first...Ch. 4 - Prob. 131ECh. 4 - The outermost valence electron in atom A...Ch. 4 - Prob. 133ECh. 4 - Give a combination of four quantum numbers that...Ch. 4 - Prob. 135E
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Similar questions
- What neutral atoms are isoelectronic with the following ions? (a) Pb4+ (b) Br (c) S2 (d) Ni3+arrow_forwardUsing your knowledge of the trends in element sizes on going across the periodic table, explain briefly why the density of the elements increases from K through V.arrow_forwardName and give the symbol of the element that has the characteristic given below. (a) Its electron configuration in the excited state can be 1s22s22p63s1 3p3. (b) It is the least electronegative element in period 3. (c) Its +3 ion has the configuration [36Kr]. (d) It is the halogen with the largest atomic radius. (e) It has the largest ionization energy in Group 16.arrow_forward
- Write electron configurations for the following elements. a. The Group III A element in the same period as 4Be b. The Period 3 element in the same group as 5B c. The lowest-atomic-numbered metal in Group IIA d. The two Period 3 elements that have no unpaired electronsarrow_forwardSuppose you were trying to find a substitute for Na* in nerve signal transmission. Where would you begin your search? What ions would be most like Na*? For each ion you propose, explain the ways in which it would be similar to Nat and the ways it would be different. Use periodic trends in your discussion.arrow_forwardSuppose you were trying to find a substitute for K* in nerve signal transmission. Where would you begin your search? What ions would be most like K+? For each ion you propose, explain the ways in which it would be similar to K* and the ways it would be different. Refer to periodic trends in your dis- cussion.arrow_forward
- III. For each of the following questions, consider your knowledge of periodic trends and the table of data given below then answer each question TRUE (A) or FALSE (B). Provide a rationale (reason) for your answer. ale Element Rb Sr Y Zr Nb Мо Tc Ru Rh Pd Ag Cd Atomic 2.65 2.19 2.12 2.06 1.98 1.90 1.83 1.78 1.73 1.69 1.65 1.61 radius (À) IE: (eV) 4.18 5.69 6.22 6.63 6.76 7.09 7.12 7.36 7.46 8.34 7.58 8.99 18. TRUE (A) or FALSE (B)? The ionization energies of the elements above decreases as their atomic radii increase. 19. TRUE (A) or FALSE (B)? Silver (Ag), as an element, is more electronegative than palladium (Pd). 20. TRUE (A) or FALSE (B)? The ionization energy of indium (In), the next element in this series, is >8.99 eV. 21. TRUE (A) or FALSE (B)? The ionic radius of the most likely cations formed from ionization of Zirconium (Zr) is less than 2.06 Å.arrow_forwardConsider Si, S, and P.1) Based purely on ideas of electron screening and effective nuclear charge, which of these elements do you expect to have the highest first ionization energy?2) Based on experimental data, P has the highest first ionization energy. Explain this observation in terms of electron configuration arguments.arrow_forwardChoose the element with the higher ionization energy from each of the following pairs. 1. Between As and Bi, the element with the higher ionization energy is 2. Between As and Br, the element with the higher ionization energy is 3. Between S and I, the element with the higher ionization energy is 4. Between S and Sb, the element with the higher ionization energy isarrow_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_forwardCan you answer part Barrow_forwardWhich element would you expect to have the highest second ionization energy (IE2)? Na, Mg, Alarrow_forward
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