Download Review Guide: Atomic Theory and Structure (Including the mole

Review Guide: Atomic Theory and Structure (Including the mole)
1. Identify the three subatomic particles: a.
proton
b. neutron
c.
electron
2. The
proton
and
neutron
are located in the nucleus of the atom.
3. The
electrons
are located on the energy
levels
outside the nucleus.
4. Which subatomic particle(s) make up the majority of the mass of an atom?
Proton and neutrons (nucleus)
5. What is an isotope? Atoms of same element with different numbers of neutrons
6. How is the mass number calculated? Protons + neutrons
7. The number of protons is given by the atomic
number
8. The number of electrons is equal to the number of
protons
9. Fill in the following table:
Nuclear
Name
Mass
Protons
Neutrons
Symbol
Number
16
O
Oxygen-16
16
8
8
.
.
Electrons
8
8
17
8O
Oxygen-17
17
8
9
8
18
8O
Oxygen-18
18
8
10
8
35Br
Bromine80
Potassium40
Iron-55
80
35
45
35
40
19
21
19
55
26
29
26
80
40
55
19K
26Fe
10. Magnesium has 3 isotopes. Magnesium-24 has a % abundance of 78.99%; Magnesium-26 has a % abundance
of 11.01%. What is the percent abundance of Magnesium-25? Calculate the average atomic mass of
Magnesium. (24 x 78.99) + (26x11.01) + (25x10) = 24.03
100
11. Which subatomic particle determines the identity of an atom?
Protons (atomic number)
12. What determines the identity of the isotope? Mass number
13. Fill in the following table
Scientist
Accomplishments/Contributions to our
knowledge of the atom
Democritus
1st atomic theory
Dalton
Modern atomic theory
Thomson
Discovered the electron
Rutherford
Discovered nucleus/atom mostly empty
space
Chadwick
Discovered neutron
Bohr
Planetary model
Experiment
None
None
Cathode ray tube
Gold foil experiment
NA
none
Millikan
Moseley
Discovered charge and mass of an electron
Discovered the atomic number of each
element
Oil drop experiment
x-ray tube experiment
14. Describe or draw a picture of the model of the atom that each of the following scientists developed:
Dalton:
Thomson
Bohr
See previous notes
15. Draw the Bohr diagram for each of the following isotopes:
Carbon-12
Calcium-40
Magnesium-24
Sulfur-32
\\
16. The element selected as the standard for the atomic mass scale was _carbon________.
17. There are _6.02 x 1023_____________________ atoms of cesium in one mole.
18. One atom of cesium has a mass of _137__________ amu.
19. One mole of cesium has a mass of __137 g_________.
20. Two moles of nitrogen have a mass of _28 g__________.
21. Two moles of nitrogen contain ___12.04 x 1023_____________________atoms.
22. Another name for the number of objects in a mole is _Avogardo’s____________ number.
Conversions:
23. 4.59 moles of Krypton is equal to how many grams of Krypton?
386 g
24. 34.4 grams of Aluminum is equal to how many atoms of Aluminum?
7.67 x 1023
25. 8.36x1024 atoms of Boron is equal to how many moles of Boron?
13.9 moles
Boron-11
26. 26.25x1026atoms of Magnesium is equal to how many grams of Magnesium?
104, 651 g
27. 5.6 moles of Sodium is equal to how many atoms of Sodium?
33.71 x 1023 or 3.371 x 1024