Chemistry Midterm Review

1. Chemistry Midterm Review

2. Question One • Describe the atomic model for each scientist listed. Be sure to mention information about the experiment and the location of the subatomic particles. • Dalton • Thomson • Rutherford • Bohr • Modern View Answer

3. Answer 1 • Dalton – indivisible, solid sphere (no subatomic particles) • Thomson- “plum pudding model” electrons are evenly distributed throughout a mass of protons. Model based on his cathode ray experiment • Rutherford- discovered mostly empty space surrounding a dense positively charged nucleus using through the gold foil experiment • Bohr- believed in a small positively charged nucleus containing the protons and neutrons surrounded by electrons in ORBITS of specific energy levels • Modern View- Also called the wave- mechanical model and the quantum model similar to Bohr but electrons are in regions of high probability based on energy level, and orbital.

4. Question 2 • Compare the charge, size, and location of a proton, neutron, and electron. Answer 2

5. Answer 2

6. Question 3 • Explain why the following two elements are isotopes. State the number of protons, electrons, and neutrons each isotope possesses.

7. Answer 3 • They are isotopes because each have a different # of neutrons but the same number of protons and electrons. • Sn -121 has 50 p+, 50 e-, 71 n0 • Sn- 119 has 50 p+, 50 e-, 69 n0

8. Question 4 • List the seven metalloids

9. Answer 4 B Si, Ge, As Sb, Te At

10. Question 5 • Why is the formation of a solution a physical change while the ability to react with a chemical considered a chemical change?

11. Answer 5 • “reacting” indicates a change in the physical properties of an element resulting in a new compound. • Formation of a solution is a physical property because a new compound has not been formed. Evaporation of the water would leave the original compound behind. (ex. salt dissolving in water)

12. Question 6 • List Properties of a metal and a nonmetal.

13. Metals Form cations Shiny Malleable Ductile Good conductors Low electronegativites and IE Solids except Hg Nonmetals Brittle Dull Poor conductors High electronegativities and IE Answer 6

14. Question 7 • A solid substance was tested in the laboratory. The test results are listed below. • • dissolves in water • is an electrolyte • melts at a high temperature • A)Na B) NaCl C) Cl D) NH3

15. Answer 7 • A)Na B) NaClC) Cl D) NH3

16. Question 8 • What is the correct formula for Cobalt(III) bromide?

17. Answer 8 CoBr3

18. Question 9 • What form of matter cannot be decomposed?

19. Answer 9 Element

20. Question 10 • What happens to a nonmetal ion when it becomes a negative ion? • Mention difference in # of electrons • Changes in radius

21. Answer 10 • Gains electrons • Radius increases

22. Question 11 • What is the name of the property that indicates an element’s desire to attract electrons and which element has the greatest attraction?

23. Answer 11 • Electronegativity • Fluorine

24. Question 12 • What are the terms used to identify a pure substance? • What are the terms used to identify a mixture?

25. Answer 12 • Element and compound • Heterogeneous and Homogeneous

26. Question 13 • What is the difference between an excited state electron and a ground state electron?

27. Answer 13 • Ground state electrons are in the lowest energy state • Excited state electrons have absorbed energy allowing them to jump to a higher energy level.

28. Question 14 • Which substance can be decomposed by chemical change? • beryllium • boron • methanol • magnesium

29. Answer 14 • Which substance can be decomposed by chemical change? • beryllium • boron • methanol • magnesium

30. Question 15 • What is the name for each type of phase change? • Solid liquid • Liquid  gas • Gas  liquid • Liquid  solid • Solid  gas

31. Answer 15 • Melting • Boiling or vaporization • Condensation • Freezing / solidification • Sublimation

32. Question 16 • What is the volume of a liquid with a density of 1.5 g/ml and a mass of 78g?

33. Answer 16 • V=m/D • 78g/4.5g/mL • =52 mL

34. Question 17 • When a bond is formed, energy is (released/absorbed) • When a bond is broken, energy is (released/absorbed)

35. Answer 17 • When a bond is formed, energy is (released/absorbed) • When a bond is broken, energy is (released/absorbed)

36. Question 18 • What is the mass number of an atom which contains 28 protons, 28 electrons and 34 neutrons? • 28 • 56 • 62 • 90

37. Answer 18 • What is the mass number of an atom which contains 28 protons, 28 electrons and 34 neutrons? • 28 • 56 • 62 • 90

38. Question 19 • What is the % composition by mass of carbon in carbon dioxide [gram-formula mass 44 grams/mole]?

39. Answer 19 27 % C

40. Question 20 • Why does calcium have similar chemical properties to barium?

41. Answer 20 • Both are Group 2 elements • Both have the same number of valence electrons

42. Question 21 • Which of the following terms indicate a chemical property and which indicate a physical property? • Flatten • Conduct • Corrode • Drawn into a wire • React

43. Chemical Corrode react Physical Flatten Drawn Conduct Answer 21

44. Question 22 • What is the charge on a I-127 nucleus?

45. Answer 22 +53

46. Question 23 Name the type of element as it appears in the order below. Ge  K  Ar  Br

47. Answer 23 Ge  K  Ar  Br Metalloid, metal, noble gas, nonmetal

48. Question 24 How many electrons are contained in an Cu2+ ion?

49. Answer 24 27 electrons

50. Question 25 Which electron configuration represents the electrons of atom of sodium in the excited? • 2-8-1 • 2-8-2 • 2-7-3 • 2-7-2