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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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If we were to compare the SINGLE bond in Fluorine to two people, what would the best comparison be ?
A. Two people who work for the same boss but have different working hours?
B Two kids in their first relationship,always arguing over the smallest things?
C. Two people who happen to have the same father but different mothers?
D. Two people in business who are trying to cheat each other out of money?
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- Some plant fetilizers contain potassium oxide [K2O] calcium phosphate [Ca3(PO4)2], phosphorus oxide [P2O5], and ammoinum sulfate [(NH4)2SO4], and potassium chloride [KCl]. Which of these contain only ionic bonds? A. potassium chloride and potassium oxide B. potassium oxide and phosphorus oxide C. ammonium sulfate and potassium oxide D. calcium phosphate and potassium chloridearrow_forwardDraw the Lewis structure (with formal charges) of the indicated chemical species. If there is resonance, show all possible resonance structures. 13. CH2O (Both H atoms are bonded to C) 14. SCl2arrow_forwardNot a covalentarrow_forward
- Which of the following compounds is likely to have the strongest H-X bond? a.HBr (141 pm) b.HI (161 pm) c.HF (92 pm) d.H2S (134 pm) e.HCl (127 pm)arrow_forwardConsider the molecules — BrF5. A. Draw the best Lewis structure for this molecule. Label any atoms with nonzero formal charge. B. Label each bond angle. As part of your answer be sure to include if it is more or less than the ideal bond angle. C. What is the electron geometry around the bromine atom? D. Are the bonds in the molecule polar? E. Is the overall molecule polar? — CH2 F2 . A. Draw the best Lewis structure for this molecule. B. Label each bond angle. Answers for A-D here: C. Redraw the shape of the molecule. Draw all dipoles. D. Is the overall molecule polar? — Consider the molecule CH2 CF2 . A. Draw the best Lewis structure for this molecule. B. Label each bond angle. C. Redraw the shape of the molecule (according to the exacting specifications of your instructor). Draw all dipoles. D. Is the overall molecule polar?arrow_forwardUse average bond energies to estimate the enthalpy changes of the following reaction? 2HF-->H2 + F2 a. -466kJ b. +38.6kJ c, -413kJ d. -93kJarrow_forward
- c) Explain which would have the lowest second ionization energy. Explain which species in each of the following pairs would have the greater electronegativity. a. lithium or nitrogen b. sulfur or selenium Consider the following table of ionization energies in kJ/mole. Element 1st 2nd 3rd 4th 5th 6th Na 496 4562 6912 9544 13353 16610 738 1451 7733 Mg Al 10540 13630 17995 18378 578 1817 2745 11577 14831 Si 786 1577 3232 4356 16091 19785 P 1012 1903 2912 4957 6274 21269 a. Explain why the first ionization energy generally increases as one goes down the group of elements listed above. b. Explain why for a particular element , the second ionization energy is greater than the first jonization energy, the third is greater than the second etc. c. Explain why Mg has a higher first ionization energy than does Na, but a lower second ionization energy than does Na. d. Explain why for aluminum there is a large increase in ionization from 3rd to 4tharrow_forwardWhich of the following compounds would have the smallest enthalpy of formation? The bond energies are given in parentheses. a. HF (H-F = 567 kJ/mol) O b. H₂ (H-H = 436 kJ/mol) O C. HCI (H-CI = 431 kJ/mol) Od. HBr (H-Br = 366 kJ/mol) Oe. HI (H-I = 299 kJ/mol)arrow_forwardHelparrow_forward
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