Electrical Energy and Capacitance s1

MR. SURRETTE VAN NUYS HIGH SCHOOL

CHAPTER 3: ELEMENTS AND ATOMIC STRUCTURE ATOMS AND ELEMENTS WORKSHEET SOLUTIONS

1. This scientist discovered the electron. 1A. JJ Thomson

2. This scientist proposed the plum pudding model. 2A. JJ Thomson

3. This scientist disproved the plum pudding model. 3A. Ernest Rutherford

4. This scientist discovered the nucleus. 4A. Ernest Rutherford

5. This scientist coined the term “atom.” 5A. Democritus

6. This scientist first organized the periodic table. 6A. Mendeleev

7. Most of the atom’s mass and all of its ______charge are contained in the ______. 7A. positive nucleus

8. The atom’s nucleus contains ______and ______. 8A. protons neutrons

9. An atom with 16 protons, 17 neutrons and 18 electrons has a mass of ______and a charge of ______and belongs to the element ______. 9A. 33 amu - 2 sulfur

10. Classify each of the following as a metal, a nonmetal, or a metalloid: 10a. Cl A. non metal

10b. K A. metal

10c. Si A. metalloid

10d. N A. nonmetal

1 | P a g e CHEMISTRY MR. SURRETTE VAN NUYS HIGH SCHOOL

11. Determine the group or family for each of the following.

11a. F A. halogen

11b. Ca A. alkaline earth metals

11c. Li A. alkali metals

11d. N A. nonmetals

12. A positive ion is called a(n) ______, while a negative ion is called a(n) ______. A. cation anion

13. An iron isotope has 29 neutrons.

13a. What is the atomic symbol for iron? A. Fe

13b. What is the Z value? A. 26

13c. What is the A value? A. (1) A = Z + N (2) A = 26 + 29 (3) A = 55

14. Ni-62 has how many protons and how many neutrons? A. 28 protons 34 neutrons

15. Gallium has two naturally occurring isotopes: Ga-69 and Ga-71. Ga-71 is 6.11% abundant. The atomic mass of gallium is 69.72 amu.

15a. Calculate the natural abundance of Ga-69. A. (1) Total mass of gallium must equal 100%. (2) 100 – 6.11 = 93.89 (3) Natural abundance for Ga-69 is 93.89%

15b. Out of 10,000 gallium atoms, how many would be Ga-69 and Ga-71? A. 611 Ga-71 and 9389 Ga-69

16. Which of the following elements is diatomic? (a) C (b) He (c) Au (d) H

CHAPTER 3: ELEMENTS AND ATOMIC STRUCTURE NUCLEUS WORKSHEET SOLUTIONS

1. A radioactive material initially has an activity of 1200 counts/sec. If six hours later it has an activity of 300 counts/sec, what is its half life? 1A. (1) 1200  600  300 (2) 2 half-lives have gone by, since each arrow represents one half-life. (3) Let x = one half-life. (4) Since the total time is 6 hours: 2x = 6 hours (5) x = 3 hours

2. 88Ra-226 decays to 86Rn-222 by emitting what type of particle: (A) beta (B) proton (C) gamma (D) positron (E) alpha

2A. A= number of nucleons Z = number of protons (1) Parent particle: A = 226 Z = 88 (2) Daughter particle: A = 222 Z = 86 (3) A = 4 Z = 2 (4) alpha particle

3. How does the daughter nucleus differ from the parent in the beta emission process: (A) atomic mass increases by one (B) atomic number increases by two (C) atomic number increases by one (D) atomic mass decreases by two (E) atomic charge increases by two

4. What energy results when one hydrogen atom and one neutron are combined to form a deuterium atom? (hydrogen 1.007825 u, neutron 1.009665 u, deuterium 2.014100 u) 4A. Let mB = “mass before reaction” Let mA = “mass after reaction” (1) mB = 1 H + 1 n (2) mB = 1.007825 u + 1.009665 u (3) mB = 2.01749 u 2 (4) mA = H (5) mA = 2.014100 u

(6) m = mB - mA

4A. continued… (7) m = 2.01749 u – 2.014100 u (8) m = 0.00339 u (9) E = mc2 (10) E = (m)c2 (11) E = (0.00339 u)(931.5 MeV / 1u) (12) E = 3.16 MeV

5. If there are 6 neutrons in C-12, how many neutrons are in C-14? 5A. (1) A1 = Z + N1 (2) Z = A1 – N1 (3) Z = 12 – 6 (4) Z = 6 (number of protons in C) (5) A2 = Z + N2 (6) N2 = A2 – Z (7) N2 = 14 – 6 (8) N2 = 8 (number of neutrons in C-14)

6. What particle is emitted when 15P-32 decays to 16S-32? (A) alpha (B) beta (C) neutron (D) gamma (E) proton

9 7. What is the Q-value for the reaction Be +   12 C + n? (m = 4.0026 u, mBe = 9.01218 u, mc = 2 12.0000 u, mn = 1.008665 u, and c = 931 MeV/u) 7A.

(1) mB = mBe +  m

mu4.0026 u (3) mB = 13.01478 u (4) mA = mc + mn (5) mA = 12.0000 u + 1.008665 u (6) mA = 13.008665 u

(7) m = mB – mA (8) m = 0.006115 u (9) E = (m)c2 (10) E = (0.006115 u)(931.5 MeV/ u) (11) E = 5.69 MeV (Q-value)

8. Nuclear fusion involves combining the nuclei of: (A) low atomic numbers (B) metals (C) non-metals (D) noble gases (E) high atomic numbers

CHAPTER 3: ELEMENTS AND ATOMIC STRUCTURE QUIZ SOLUTIONS

1. These elements are somewhat good conductors of heat and electricity. 1A. metalloids

2. Group 1 elements of the periodic table are called the: 2A. alkali metals

3. Group 18 elements of the periodic table are called the: 3A. noble gases

4. This scientist discovered the electron. 4A. JJ Thomson

5. This scientist proposed the nuclear theory of the atom. 5A. Ernest Rutherford

6. This scientist developed the periodic table. 6A. Dmitri Mendeleev

7. Which of the following elements is diatomic? 7A. Iodine

8. An atom with 15 protons, 17 neutrons and 18 electrons has a mass of ______and a charge of ______and belongs to the element ______. 8A. 32 amu - 3 phosphorus

9. A radioactive material initially has an activity of 1200 counts/sec. If six hours later it has an activity of 600 counts/sec, what is its half life? 9A. (1) 1200  600 (2) 1 half-life has gone by in 6 hours. (3)  = 6 hours

10. 88Ra-226 decays to 86Rn-222 by emitting what type of particle: (A) beta (B) proton (C) gamma (D) positron (E) alpha

11. Convert 302 K into oC 11A. (1) Tc = T – 273 (2) Tc = 302 – 273 (3) Tc = 29 1 o (4) Tc = 2.9 x 10 C

12. Convert 302 K into oF 12A. (1) Tc = T – 273 (2) Tc = 302 – 273 o (3) Tc = 29 C (4) TF = (9/5) Tc + 32 o (5) TF = (9/5) (29 C) + 32 o (6) TF = 84.2 F 1 o (7) TF = 8.42 x 10 F 1 o (8) TF = 8.4 x 10 F

13. Convert 10.18 mg/mL into ng/L 13A. 10.18 mg x 1 g x 109 ng x 1000 mL ------1 mL 1000 mg 1 g 1 L

= 1.018 x 1010 ng/L

14. Sc 14A. metal

15. I 15A. nonmetal

16. Kr 16A. nonmetal

17. If there are 6 neutrons in N-13, how many neutrons are in N-14? 17A. (1) A1 = Z + N1 (2) Z = A1 – N1 (3) Z = 13 – 6 (4) Z = 7 (number of protons in N) (5) A2 = Z + N2 (6) N2 = A2 – Z (7) N2 = 14 – 7 (8) N2 = 7 (number of neutrons in N-14)

18. Mg 18A. alkaline metals

19. What particle is emitted when 15P-32 decays to 16S-32? (A) alpha (B) neutron (C) gamma (D) proton (E) beta

20. Xe 20A. noble gases

21. Na 21A. alkali metals

22. Argon (atomic number 18) has three isotopes: Ar-36: 35.97 amu 0.34% relative abundance Ar-38: 37.96 amu 0.07% relative abundance Ar-40: 39.96 amu 99.59% relative abundance Based on these three isotopes, compute the atomic mass of argon. 22A. (1) A (Ar) = (35.97 x 0.0034) + (37.96 x 0.0007) + (39.96 x 0.9959) (2) A (Ar) = 0.122298 + 0.002772 + 39.796164 (3) A (Ar) = 39.921234 amu (4) A (Ar) = 39.92 amu

23. What is the Q-value for the reaction 9Be +   12 C + n? 2 (m = 4.0026 u, mBe = 9.01218 u, mc = 12.0000 u, mn = 1.008665 u, and c = 931.5 MeV/u) 23A.

(1) mB = mBe +  m

mu4.0026 u (3) mB = 13.01478 u (4) mA = mc + mn (5) mA = 12.0000 u + 1.008665 u (6) mA = 13.008665 u

(7) m = mB – mA (8) m = 0.006115 u (9) E = (m)c2 (10) E = (0.006115 u)(931.5MeV /u) (11) E = 5.69 MeV (Q-value)

24. C-12 has a natural abundance of 98.89%. Out of a random sample of 10,000 carbon atoms, how many would not be C-12? 24A. 111

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