1. Quiz Review Ionic Bonding Periodic Trends Formula Writing and Naming

2. During a lab experiment you mixed together two different solutions and observed whether or not a precipitate formed. A precipitate is defined as a. any liquid mixture b. The liquid part of a chemical reaction c. A clear solution d. A solid that forms and separates from a liquid mixture.

3. A solid that forms and separates from a liquid mixture.

4. All atoms on the periodic table desire to become like the noble gases. Why? a.Noble gases have a full outermost energy level. b.Noble gases bond easily with other elements. c.Noble gases make really neat explosions. d.Noble gases have 7 valence electrons.

5. Noble gases have a full outermost energy level.

6. Which statement about the alkali metals is correct? a.They are located in the left-most column on the periodic table. b.They are extremely nonreactive. c.They are usually gases. d.They form negative ions with a -1 charge.

7. They are located in the left-most column on the periodic table

8. Most halogens form compounds by a.gaining an electron to form a negative ion. b.losing an electron to form a positive ion. c.losing protons. d.losing neutrons.

9. gaining an electron to form a negative ion

10. Which element is more reactive, potassium or sodium? a.Potassium - It gains electrons easily because of its atomic radius. b.Potassium - It loses electrons easily because of its atomic radius. c.Sodium - It gains electrons easily because of its atomic radius. d.Sodium - It loses electrons easily because of its atomic radius.

11. Potassium - It loses electrons easily because of its atomic radius

12. Which element is more reactive, fluorine or iodine? a.Fluorine - It loses electrons easily because of its mass. b.Fluorine - It gains electrons easily because of its mass. c.Iodine - It loses electrons easily because of its mass. d.Iodine - It gains electrons easily because of its mass.

13. Fluorine - It gains electrons easily because of its atomic mass

14. In a chemical formula, the number of atoms in the compound is shown by the a.oxidation number b.coefficient c.superscript d.subscript

15. subscript

16. In a chemical formula, the number of molecules in the compound is shown by the a.oxidation number b.coefficient c.superscript d.subscript

17. coefficient

18. How many electrons are needed in the outer energy levels of most atoms for the atom to be chemically stable? a.2 b.6 c.4 d.8

19. 8

20. What kind of chemical bond is formed when electrons are transferred from one atom to another? a.ionic b.metallic c.covalent d.hydrogen

21. ionic

22. What is the total number of atoms in the compound Ca(ClO 3 ) 2 ? a.2 b.6 c.3 d.9

23. 9

24. How many total hydrogen atoms are present in one molecule of ammonium acetate NH 4 C 2 H 3 O 2 ? a.3 b.7 c.4 d.11

25. 7 ammonium acetate NH 4 C 2 H 3 O 2

26. An atom that has an electrical charge is called a/an a.element b.isotope c.ion d.molecule

27. ion

28. When an atom loses electrons, the atom gains a ________charge. a.positive b.negative

29. positive

30. When an atom gains an electron, the atom gains a _________ charge. a.positive b.negative

31. negative

32. A molecule that shares electrons unevenly between the atoms is called a.nonpolar b.ionic c.polar d.neutral

33. polar

34. The order of atoms on the periodic table is based on a.the number of protons in the nucleus b.the number of neutrons in the nucleus c.the electric charge of the nucleus d.atomic mass

35. the number of protons in the nucleus

36. Atoms of elements in the same group have the same number of a.protons b.valence electrons c.neutrons d.protons and neutrons

37. valence electrons

38. Alkali metals are extremely reactive because they a.have very small atomic masses b.are not solids at room temperature c.have one valence electron that is easily lost to form a positive ion. d.have two valence electrons that form compounds with calcium and magnesium

39. have one valence electron that is easily lost to form a positive ion.

40. The electrons in a nonpolar covalent bond are a. gained b. shared equally c. lost d. shared unequally

41. shared equally

42. The formula for magnesium nitrate is a. MgNO 3 b. Mg(NO 3 ) 2 c. Mg 2 NO 3 d. Mg 2 (NO3) 3

43. Mg(NO 3 ) 2

44. How many electrons are gained/lost by magnesium and what is the charge of the ion that it forms? a. Loses 2 electrons to form a magnesium ion with a -2 charge. b. Gains 2 electrons to from a magnesium ion with a -2 charge. c. Loses 2 electrons to form a magnesium ion with a +2 charge. d. Gains 2 electrons to form a magnesium ion with a +2 charge.

45. Loses 2 electrons to form a magnesium ion with a +2 charge

46. What ions make up the compound FeCl 3 ? a.1Fe 3+ ion and 1Cl - ion b.1Fe 3+ ion and 3 Cl - ions c.1Fe 2+ ionic and 3Cl - ions d.3Fe 3+ ions and 1Cl - ion

47. 1Fe 3+ ion and 3 Cl - ions

48. Which element has the largest atomic radius? a.Aluminum b.Sulfur c.Silicon d.Chlorine e.Phosphorus

49. Aluminum

50. Water is considered a polar molecule because a. the molecule has a net positive charge b. the molecule has a net negative charge c. the molecule has a net zero charge d. the ends of the molecule have partial negative and positive charges

51. The ends of the molecule have partial negative and positive charges

52. Metalloids have characteristics similar to a. Metals b. Nonmetals c. Metals and nonmetals d. Noble gases

53. Metals and nonmetals

54. Ni 2 O 3 is named nickel (III) oxide because it contains a. Three oxygen atoms b. Ni 3+ ions. c. Three nickel atoms d. O 3+ ions

55. Ni 3+ ions

56. Write the formula for the following ionic bonding pairs and name them! Ca + Br K + I Na + O B + S Al + F Al + SO 4 NH 4 + Cl Fe (III) + NO 3

57. Identify the # of atoms of each element and # of molecules C 6 H 12 O 6 2 SrCl 2 NH 4 (SO 4 ) 2 2Pb(CH 3 CoO) 2 MgSO 4

58. How would you draw a carbon water molecule? Label the atoms Hydrogen Oxygen

59. How would you draw a carbon dioxide molecule? Label the atoms. oxygen carbon oxygen

60. Last Laugh…

62. Last Laugh…Really!