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

2. 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.

3. Noble gases have a full outermost energy level.

4. 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.

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

6. 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.

7. gaining an electron to form a negative ion

8. 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.

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

10. 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.

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

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

13. subscript

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

15. coefficient

16. 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

17. 8

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

19. ionic

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

21. 9

22. 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

23. 7 ammonium acetate NH 4 C 2 H 3 O 2

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

25. ion

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

27. positive

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

29. negative

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

31. polar

32. 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

33. the number of protons in the nucleus

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

35. valence electrons

36. 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

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

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

39. shared equally

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

41. Mg(NO 3 ) 2

42. 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.

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

44. 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

45. 1Fe 3+ ion and 1Cl - ion

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

47. Aluminum

48. 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

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

50. 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

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

52. Last Laugh…

54. Last Laugh…Really!