Name_________________________Per___________Date__________
Name_________________________Per___________Date__________
Atomic Structure Practice Review
Complete the following questions. Be sure to show all your work to receive credit.
1. Calculate the following for Bromine-80
|Protons |Electrons |Neutrons |
|35 |35 |45 |
2. Iridium has two isotopes 191Ir and 193Ir. Which isotope is more abundant? What is that percent abundance? Show all your work.
192.2 = (191 x X) + (193 x (1-X)
192.2 = 191X + 193 – 193X
-0.8 = -2X
Ir-191 = 40%
Ir-193 = 60 % - Most abundant
3. Silicon has three naturally occurring isotopes. Silicon- 28, Silicon-29, and Silicon-30. Using the information below calculate the average atomic mass of Silicon. (Show your work)
|Isotope |Exact Mass |% Abundance |
|Silicon- 28 |27.976927 |92.23 |
|Silicon-29 |28.976495 |? 4.67 |
|Silicon-30 |29.973770 |3.10 |
Avg atomic mass = (27.976927 x 0.9223) + (28.976495 x 0.0467) + (29.973770 x .0310)
Avg atomic mass = 28.0855 ( 28.1 amu
4. Give the nuclear symbol for the isotope Arsenic-76: 76As
33
Identify the following:
|Atomic Number |Mass Number |Protons |Neutrons |Electrons |
|33 |76 |33 |43 |33 |
5. What are isotopes?
• Atoms with the same number of protons and a different number of neutrons.
6. What are ions?
• An electrically charged atom due to the gain or loss of electrons.
7. How does an ion acquire a positive and negative charge?
• By gaining or losing electrons.
Identify each of the following elements using the format AX Z
|Description |Isotope |
|8. 77 protons and 75 electrons |192Ir |
| |77 |
|9. 25 electrons (neutral atom) |55Mn |
| |25 |
|10. mass number 208 and 126 neutrons |208Pb |
| |82 |
|11. 62 neutrons and 46 protons |108Pd |
| |46 |
12. Calculate the following for Mg+2.
|Protons |Electrons |Neutrons |
|12 |10 |12 |
13. Carbon has two naturally occurring isotopes Carbon -12 and Carbon-13.
The masses of the two isotopes are 12.00 amu and 13.003 amu respectively (in order). Calculate the relative abundance for the two isotopes of carbon.
12.01 = (12.00 x X) + (13.003 x (1-X)
12.01 = 12.00X + 13.003 – 13.003X
-0.993 = -1.003X
X = 0.99
C-12 = 99.00%
C-13 = 1.000%
14. Complete the table:
|Particle |Location |Mass |Charge |Discoverer |Experiment that led to |
| | | | | |discovery |
|n |Nucleus |1 |0 |Chadwick | |
|e- |Space surrounding |1/1837 |-1 |Thomson |Cathode Ray Tube |
| |nucleus | | | | |
15. What 3 ideas about the atom were determined by Rutherford’s gold foil
experiment?
a) Atoms formed a small dense center (mostly filled with empty space).
b) Nucleus was orbited by electrons.
c) Protons existed in nucleus.
16. What were the 5 principles of Dalton’s Atomic Theory?
a) All matter is composed of extremely small particles called atoms.
b) Atoms of an element are identical in size, mass, and other properties; atoms of different elements differ in size, mass, and other properties.
c) Atoms cannot be subdivided, created, or destroyed.
d) Atoms of different elements combine in simple whole-number ratios to form chemical compounds.
e) In chemical reactions, atoms are combined, separated, or rearranged.
Answer the following challenges.
17. A vacuum tube containing a filament and a fluorescent screen:
• Cathode Ray Tube
18. 9.1 x 10-31 kg:
• Mass of an electron
19. Has a relative mass of 1/1837:
• Electron
20. What discovery did the deflection of electrons in a cathode ray tube
lead to?
• All elements have electrons.
21. Has no charge and a mass of 1.6 x 10-27 kg:
• Neutron
22. Electrons embedded in a positively-charged sphere:
• Plum Pudding
23. Distinguishes a proton from a neutron:
• Charge
24. The two things involved in the oil drop experiment:
• Mass and Charge
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