Final Review PP

1. Final Review PP

2. Fill in the following: States of Matter – Graphic Organizer

3. States of Matter – Graphic Organizer

4. 1. Why is Potassium (K) placed after Argon (Ar) on the periodic table of the elements even though it has a lower average atomic mass than argon? a. Potassium has one more proton b. Argon was discovered first c. Potassium has fewer electrons d. Argon has a lower density

5. 1. Why is Potassium (K) placed after Argon (Ar) on the periodic table of the elements even though it has a lower average atomic mass than argon? a. Potassium has one more proton b. Argon was discovered first c. Potassium has fewer electrons d. Argon has a lower density • A) Because the periodic table is arranged by increasing atomic # (which is the # of protons)

6. 2. When cations and anions join, they form what kind of chemical bond? a. ionic b. hydrogen c. metallic d. covalent

7. 2. When cations and anions join, they form what kind of chemical bond? a. ionic b. hydrogen c. metallic d. covalent a) Ionic bonds are when electrons are exchanged between two atoms, creating ions (cations & anions) that have a + or – charge. This difference in charge results in a strong bond where the ions are attracted together in a crystal lattice structure.

8. 3. Which of the following elements has the same Lewis dot structure as Silicon? a. germanium (Ge) b. aluminum (Al) c. arsenic (As) d. gallium (Ga)

9. 3. Which of the following elements has the same Lewis dot structure as Silicon? a. germanium (Ge) b. aluminum (Al) c. arsenic (As) d. gallium (Ga) a) Ge because all elements in the same group A family have the same # of valence electrons

10. How do you calculate a molar mass of a molecule? • A. You add up the number of protons • B. You add up the mass of the largest atom and multiply it by the coefficient • C. You multiply the subscripts by the mass from periodic table and add them all up • D. You multiply the coefficient by all the elements mass from periodic table and add them all up

11. Solve: • C—using the mass from periodic table & number of atoms in the element(subscript) not the coefficients(the number of molecules)

12. How many moles is 6 grams of CH4 • CX1 = 12.01 g • HX4 = 4.04 g • CH4 =16.05g

13. Solve • 6g CH4 X 1 mole 16.05g CH4 .37 moles of CH4

14. 6. The most abundant isotope of lead contains 82 protons and 124 neutrons packed closely together in the nucleus. Why do the protons stay together in the nucleus rather than fly apart? a. Electrons in neighboring atoms neutralize repulsive forces between protons. b. Neutrons effectively block the protons and keep them far apart to prevent repulsion. c. Electrostatic forces between neutrons and protons hold the nucleus together. d. Nuclear forces overcome repulsive forces between protons in the nucleus.

15. 6. The most abundant isotope of lead contains 82 protons and 124 neutrons packed closely together in the nucleus. Why do the protons stay together in the nucleus rather than fly apart? a. Electrons in neighboring atoms neutralize repulsive forces between protons. b. Neutrons effectively block the protons and keep them far apart to prevent repulsion. c. Electrostatic forces between neutrons and protons hold the nucleus together. d. Nuclear forces overcome repulsive forces between protons in the nucleus. d) the strong nuclear force is what holds protons and neutrons together in the nucleus.

16. 7. Some of the molecules found in the human body are NH2CH2COOH (glycine), and C6H12O6 (glucose). The bonds they form are a. nuclear. b. ionic. c. metallic. d. covalent.

17. 7. Some of the molecules found in the human body are NH2CH2COOH (glycine), and C6H12O6 (glucose). The bonds they form are a. nuclear. b. ionic. c. metallic. d. covalent. d) covalent. ***Be able to see the difference between covalent molecules & Ionic compounds

18. Molecules have different shapes NaCl is ionic; Crystal Lattice; Repeating Structure

19. 8. Which of the following is a nonpolar molecule? A) HF B) H2O C) CH4 D) NH3

20. 8. Which of the following is a nonpolar molecule? A) HF B) H2O C) CH4 draw it! D) NH3

21. 9. How many electrons are shared in a single covalent bond? A) 1 B) 2 C) 3 D) 8

22. 9. • How many electrons are shared in a single covalent bond? • A) 1 • B) 2 • C) 3 • D) 8 • B) a pairof electrons (2 electrons) is shared in a single covalent bond.

23. 10. What type of force holds ions together in salts such as CaF2? a. electrostatic b. magnetic c. gravitational d. nuclear

24. 10. What type of force holds ions together in salts such as CaF2? a. electrostatic b. magnetic c. gravitational d. nuclear a) Electrostatic force: the attraction between positive & negative (IONIC!) This is the same force between protons (+) & electrons (-)

25. 11. Which of the following is a monatomic gas at STP (standard temperature and pressure)? a. argon b. fluorine c. hydrogen d. nitrogen

26. 11. Which of the following is a monatomic gas at STP (standard temperature and pressure)? a. argon b. flourine c. hydrogen d. nitrogen a) Argon – all others are diatomic molecules at STP.

27. 12. 12.

28. 12. • Carbon has 4 valence electrons that can make covalent bonds with 4 different hydrogen atoms.

29. 13.

30. 13. Diatomic molecules are always covalent bonds. Memorize ammonia and methane!!!

31. 14.

32. 14.

33. 15.

34. 33. Which of the following atoms has the largest atomic radius? A barium (Ba) B chlorine (Cl) C iodine (I) D magnesium (Mg)

35. 33. Which of the following atoms has the largest atomic radius? A barium (Ba) B chlorine (Cl) C iodine (I) D magnesium (Mg)

36. 33.

37. 15. 6g Carbon x 1 mole Carbon = 0.5 mole 12 g Carbon

38. 16. • Nuclear Chemistry (not covered in 2015-16)

39. Nuclear Chemistry • Alpha • Beta • Gamma

40. 17. Which statement best describes the density of an atom’s nucleus? A The nucleus occupies most of the atom’s volume but contains little of its mass. B The nucleus occupies very little of the atom’s volume and contains little of its mass. C The nucleus occupies most of the atom’s volume and contains most of its mass. D The nucleus occupies very little of the atom’s volume but contains most of its mass.

41. 17. Which statement best describes the density of an atom’s nucleus? D The nucleus occupies very little of the atom’s volume but contains most of its mass. Protons and neutrons are very densely packed in the nucleus.

42. 18. Standard temperature and pressure (STP) are defined as A) 0 ºC and 1.0 atm pressure. B) 0 ºC and 273 mm Hg pressure. C) 0 K and 1.0 atm pressure. D) 0 K and 760 mm Hg pressure.

43. 18. Standard temperature and pressure (STP) are defined as A) 0 ºC and 1.0 atm pressure. B) 0 ºC and 273 mm Hg pressure. C) 0 K and 1.0 atm pressure. D) 0 K and 760 mm Hg pressure. Memorize this!

44. 20. What is the equivalent of 423 Kelvin in degrees Celsius? • –223 ºC • –23 ºC • 150 ºC • 696 ºC

45. 20. What is the equivalent of 423 Kelvin in degrees Celsius? • –223 ºC • –23 ºC • 150 ºC • 696 ºC 0 K = -273 ºC +423 K = +423K 423 K = 150 ºC

46. 21. The temperature at which all molecular motion stops is A) −460 ºC. B) −273 K. C) 0 K. D) 0 ºC.

47. 21. The temperature at which all molecular motion stops is A) −460 ºC. B) −273 K. C) 0 K. D) 0 ºC. Memorize this definition for “Absolute Zero”

48. 22. The random molecular motion of a substance is greatest when the substance is A condensed. B a liquid. C frozen. D a gas.

49. 22. The random molecular motion of a substance is greatest when the substance is A condensed. B a liquid. C frozen. D a gas.

50. 23. Theoretically, when an ideal gas in a closed container cools, the pressure will drop steadily until the pressure inside is essentially that of a vacuum. At what temperature should this occur? A 0ºC B −460 ºC C −273 K D 0 K