Download Atomic structure packets

Atomic Theory / History of the Atom
Computer Lab
Part 1: Follow the instructions to complete each set of questions using the power point and the websites linked in the
power point. In some instances, you will have to view an animation or picture from a website.
History of the Atom
Timeline of Contributors to the modern atomic theory.
1. List the main contributors to atomic theory in order of the timeline from the power-point. Include the year of
their work and the main contribution to the theory. For each contributor, answer the questions below the chart.
Contributor
Year of their Work
2. Greek philosopher.
a. Who was responsible for the concept of atoms?
b. What does the word “atom” mean?
c. What is the word origin for “atom?”
3. Foundations of Atomic Theory: Dalton’s Components to Atomic Theory
a. List the 4 components to Dalton’s Atomic Theory
Describe briefly their contribution
b. State at least one principle from Dalton’s theory that have been revised as new information has become
available and explain how this is different from Dalton’s original postulates.
c. What is the Law of Conservation of Mass?
d. Based on this law, use the following
According to the law of conservation of mass, how much zinc was present in the zinc carbonate?
Show your work here and explain how you determined the answer.
4. JJ Thomson
a. What subatomic particle is Thomson credited with discovering?
b. What is the name of Thomson’s famous experiment?
5: Robert Millikan and the electron charge. Click on the link.
Click on the Millikan Oil Drop experiment
a.
What is the name of Millikan’s experiment?
b. What was the purpose of the experiment?
c. What is the charge on a single electron?
6: Ernest Rutherford
a. What is the name of Rutherford’s experiment?
b. What were the findings of this experiment?
c. The result of this experiment showed that most of the mass of an atom was located ____________________________
and the overall charge of this region was _________________________.
d.The results of this experiment also showed that most of the size/volume of an atom is composed of
__________________________.
e. Think about it…If alpha particles have a positive charge, what actually caused the alpha particles to deflect?
6. Niels Bohr
a. Draw Bohr’s model for an atom below.
7. Complete the chart below that indicates the parts and locations of those parts of an atom.
Parts of the atom:
Parts
Protons
Charge
Neutrons
Electrons
Part III:
Fill in the missing information:
Symbol
location
Mass (amu)
Part IV: Isotope Practice
1. Three isotopes of argon occur in nature – Argon-36, Argon-38, and Argon-40. Calculate the average atomic mass of argon to two
decimal places, given the following relative atomic masses and abundances of each of the isotopes: argon-36 (35.97 amu; 0.337%),
argon-38 (37.96 amu; 0.063%), and argon-40 (39.96 amu; 99.600%)
2. Naturally occurring boron is 80.20% boron-11 (atomic mass = 11.01 amu) and 19.80% of some other isotopic form of boron. What
must the atomic mass of this second isotope be in order to account for the 10.81 amu average atomic mass of boron? Write the answer
to two decimal places.
Part V: Practice Problems: show all work in Dimensional Analysis Format.
1.
2 mol He= ? g
2.
3.5 mol Cu = ?g
3.
11.9 g Al = ?moles
4.
How many moles of Ca are contained in 5 g of Ca?
5.
How many moles of Au are contained in 3.60 x 10 –10 g of Au?
6.
3.01 x10 23 atoms of Ag is equal to how many moles?
7.
How many moles of Pb are equivalent to 1.5 x 10 12 atoms?
8.
How many moles of Sn are equivalent to 2500 atoms?
9.
How many atoms of Al are contained in 2.75 moles?
10. What is the mass in grams of 1.2 x 10 8 atoms of Cu?
11. What is the mass in grams of 7.5 x 10 15 atoms of Ni?
12. How many atoms of S are contained in 4.00 g?
13. What is the mass of Au that contains the same number of atoms as 9.0 g of Al?