Chapter #14 Solutions - Physical Science with Modern Applications - Melvin Merken - 5th Edition

 

1. List the noble gas elements. Get solution

2. What is the relation between the octet rule and a noble gas structure? Get solution

3. Explain why the chemical activity of tire noble gases went undiscovered for so long. Get solution

4. Draw the Lewis dot structures for the following atoms(a) N(b) Na(c) Cl(d) Ne(e) Br Get solution

5. The following substances are isoelectronic with one another. Write a Lewis structure for each.(a) CH4(b) NH3(c) H2O(d) HF(e) Ne Get solution

6. Write Lewis structures for the following compounds.(a) sodium fluoride: NaF(b) carbon tetrachloride: CCl4(c) boron trifluoride: BF3(d) molecular nitrogen: N2(e) carbon monoxide: CO Get solution

7. Differentiate between the molecular formula and Lewis formula of water. Get solution

8. Give the total number of outer-shell electrons in each of the following.(a) NH3(b) CaCl2(c) Al2S3(d) ...(e) ... Get solution

9. Write the Lewis structure for O2. What kind of bond has to be formed between the two oxygens to satisfy the octet rule? Get solution

10. Give the number of the periodic group and the number of valence electrons for each of the following atoms.(a) S(b) C(c) Mg(d) Ne(e) B Get solution

11. Does the Ca2+ ion possess a noble gas configuration? Explain. Get solution

12. Is the formula MgF3 likely to represent a stable compound? Explain. Get solution

13. Using Lewis structures, diagram the reaction that occurs between Ca atoms and F atoms. Get solution

14. Account for the fact that the second ionization energy of lithium (75.6 eV) is greater dian the first (5.4 eV). Get solution

15. (a) List four ions that are isoelectronic with the noble gas xenon, and (b) give the charge of each. Get solution

16. Write Lewis symbols to represent the electron transfer between K and S to form ions with noble gas configurations. Get solution

17. Explain why argon does not form ionic bonds. Get solution

18. What are the charges on the ions in Al2S3? Get solution

19. Why would it be misleading to refer to “molecules” of sodium chloride (NaCl) in the crystalline state? Get solution

20. Explain why the halogens (fluorine, chlorine, bromine, and iodine) occur as diatomic molecules. Get solution

21. How do a bromine atom, a bromine molecule, and a bromide ion differ? Write the formula for each. Get solution

22. Why does neon not form covalent bonds? Get solution

23. What is (a) a double bond; (b) a triple bond? Get solution

24. How many covalent bonds are normally formed by(a) F?(b) O?(c) N?(d) C? Get solution

25. Which electron pairs in tire Lewis formula of H2S are bonding and which are lone pairs? Get solution

26. How does a coordinate covalent bond differ from an ordinary covalent bond? Get solution

27. Predict (a) whether the bonds between the following pairs of elements would be ionic or covalent, and (b) if covalent, tire percent ionic character of tire bond.(a) Ba, O(b) Al, S(c) N, Cl(d) C, S(e) Si, C Get solution

28. Although fluorine is the most electronegative element, silicon tetrafluoride (SiF4) does not have-a dipole moment. Explain. Get solution

29. Based on the electronegativities of the atoms, arrange the following bonds in order of increasing ionic character.... Get solution

30. Why is an HCl molecule polar whereas a Cl2 molecule is nonpolar? Get solution

31. Predict whether a bond will form and, if so, whether it will be ionic or covalent, between(a) Br and F.(b) Li and Na.(c) K and S.(d) N and Ne. Get solution

32. Which atom in ClF is more negatively charged? Get solution

33. How do the electronegativities of the elements vary from (a) left to right across a period and (b) from the top to the bottom of a group? Get solution

34. What geometric structure would you predict for each of tire following substances?(a) CF4(b) BeCl2(c) BBr3(d) AsH3(e) SF6 Get solution

35. (a) What bond angle would you predict when all of the valence electrons of an atom are involved in three single bonds? (b) Would the presence of a lone pair of electrons in addition to three bonds change your prediction? If so, how? Get solution

36. On the basis of molecular structure, explain why NH3 has a dipole moment but BF3 does not. Get solution

37. The H2S molecule has a geometry similar to that of water. Is the H2S molecule a dipole? If so, where are the partial charges located? Get solution

38. How many atoms are directly bonded to the central atom in a tetrahedral molecule? Get solution

39. What are some properties of water that are determined by the presence of a dipole moment? Get solution

40. Explain why copper wire is a good conductor of electricity. Get solution

41. (a) List three types of solids based on the nature of the bonding forces, and (b) give an example of each. Get solution

42. Account for the characteristic luster of silver metal. Get solution

43. Why are metals good conductors of heat and electricity? Get solution

44. Account for the relatively high density of metals. Get solution

45. How are the atoms in a metal held together? Get solution

46. Multiple ChoiceA. In the Lews structure for fluorine, the number of dots surrounding the symbol for fluorine is(a) one.(b) four.(c) five.(d) seven.B. The most electronegative element on the Pauling electronegativity scale is(a) oxygen.(b) neon.(c) fluorine.(d) cesium.C. The kind of bonding in sodium chloride is(a) ionic.(b) covalent.(c) coordinate covalent.(d) metallic.D. The compound that has the greatest covalent character is(a) H2O.(b) NaCl.(c) Br2.(d) Fe2O3.E. The bond between two nitrogen atoms in nitrogen gas is(a) single.(b) double.(c) triple.(d) electrovalent.F. The chemical formula for the compound formed when 14Si reacts with 17Cl is(a) SiCl.(b) SiCl2.(c) SiCl3.(d) SiCl4.G. Which of the following molecules could not possibly be polar?(a) H2O(b) HCl(c) I2(d) NH3H. Sodium chloride has(a) ionic bonds.(b) covalent bonds.(c) nonpolar bonds.(d) coordinate covalent bonds.I. When K and O react to form the ionic compound K2O,(a) each potassium atom loses one electron.(b) each potassium atom loses two electrons.(c) each oxygen atom loses one electron.(d) each oxygen atom loses two electrons.J. A covalent bond is formed(a) when electrons are transferred.(b) when electrons are shared.(c) when a cation and anion come together.(d) only when shared electrons come from the same atom. Get solution