1. Read the section above about balancing charges and give formulas that represent overall neutral compounds between the following pairs of ions. + a. Cs and Cl- + b. Cs and Se²- c. Fe2+ and Br d. Fe3+ and Br e. Fe2+ and CO3²- 2-
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- eaching and lear X G The element in period 5 that has X ment/takeCovalentActivity.do?locator=assignment-take [Review Topics] [References] We can draw three inequivalent Lewis structures for the sulfite ion, SO32. The concepts of formal charge and electronegativity can help us choose the structure that is the best representation. Formal Charge 1. Assign formal charges to the elements in each of the structures below. Note: Count oxygen atoms starting from the left for each structure. 40 S 01 02 03 Submit Answer :O: 4- --0000 :0: 4+ C Solved The following Lewis diagr x 2. The best Lewis structure for SO3²- is V. fg Yo 144 :0: Retry Entire Group 9 more group attempts remaining fo B 0% " A a 112 :0: C :0: + O ins prt sc Previous A ENG delete home 11:54 A 11/28/20 endDraw the Lewis structure (with formal charges) of the chemical species: 1. CINO2 (N is the central atom) 2. CO3^2- 3. NO2- 4. SO3 5. BrNO2 (N is the central atom) 6. HCO3- (H is bonded to one of the O's) 7. SeO2 8. HC2O4- (each C has two O atoms and H is on one of the O's) 9. HNO3 (H is bonded to one of the O's) 10. CH3NO2 11. HCO2- (H and both O's are bonded to C)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 4th
- 5. Write the chemical formula that results when the following pairs of ions combine to form an ionic bond. a. Sr2* and 02- b. Mn4 and O2- C. Lit and CI- d. Cst+ and Sz-2. Identify the true statement. a. Polar covalent compounds result from a complete transfer of at least one electron. b. Sodium is unlikely to form a bond with lithium. c. Covalent compounds exist in large lattices. d. The smallest unit of an ionic compound is a molecule. 3. A piece of zinc metal is placed in an aqueous solution of magnesium sulfate. The products of this reaction are a. ZnMg(s) + SO4(aq) b. Mg(s) + ZnSO4(aq) c. MgS(s) + ZnO4(aq) d. ZnO(s) + MgSO4(aq) e. There will be no reaction. 4. The shape of the NC13 molecule is a. linear b. trigonal planar c. tetrahedral d. trigonal pyramidal e. V-shaped Imi 5. Which of the following would have the highest boiling point? a. NH3 b. PH3 c. AsH3 d. They would all have approximately the same boiling point. 20 6. Aqueous solutions of silver nitrate and sodium sulfate are mixed. The products of the reaction are a. Ag2SO4(aq) + 2 NaNO3(aq) b. AgSO4(s) + Na2(NO3)2(aq) c. Ag2SO4(s) + 2 NaNO3(aq) d. AgSO4(aq) + Na2(NO3 e. There will be no…1. Chapter 8, Problem 66: Use bond energy values (Table 8.4) to estimate AH for each of the following reactions. H- a. HCN(g) + 2H2(g) → H н (g) b. H. (g) + 2F2(g) → N2(g) + 4HF(g)
- Write Lewis structures that obey the octet rule for each of the following. a. HCN b. PH3 c. CHCl3 d. NH4+ e. H2CO f. SeF2 g. CO2 h. O2 i. HBr Except for HCN and H2CO, the first atom listed is the central atom. For HCN and H2CO , carbon is the central atom.Draw the Lewis structure for a molecule of each of thesecompounds and ions.a. H 2 S c. S O 2b. B F 4 — d. SeC l 214 Cancel RESET 4. Draw Lewis structures for each of the following molecules or polyatomic ions. State whether they obey the octet rule and if any coordinate covalent bonds form. In each case, the first atom listed is the central atom. K/UC (a) POCI, (b) SO2- (c) PO 3- (d) CIO A fty. © Done
- We can draw three inequivalent Lewis structures for the selenite ion, Se032-. The concepts of formal charge and electronegativity can help us choose the structure that is the best representation. 1. Assign formal charges to the elements in each of the structures below. Note: Count oxygen atoms starting from the left for each structure. Formal Charge Se 01 02 03 Se || :0: A 0° 2- Se :0: 2. The best Lewis structure for SeO32- i: ✓ B 2. O Se :0: C 12-What is chemical formula of the neutral compound formed from the ions below: PART A. Cr3+ ions and Cl− ions PART B. Mn4+ ions and O2− ions PART C. Mg2+ ions and CO32- ionsPlease explain where I am going wrong. I can't seem to figure it out.
