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Review Sheet : Atoms – The Building Blocks of Matter
1. Draw a picture of what the model looks like in each of the following models.
a. Thomson Model:
b. Rutherford Model
c. Bohr Model
d. Quantum Mechanical Model:
2. Highlight the parts of Dalton's atomic theory that were proved to be false in later theories:
• All elements are made up of tiny indivisible particles called atoms.
• Atoms of the same element are identical. The atoms of one element are different from the atoms of another
element.
• Atoms of different elements chemically combine to form chemical compounds.
• During chemical reactions, atoms are rearranged, separated or combined.
3. How does the existence of isotopes contradict part of Dalton’s theory above? Which part?
4. How did Thomson’s cathode ray tube experiment contradict part of Dalton’s theory above?
5. Explain Rutherford’s experiment in your own words. What did this prove about the atom in 1911?
6. Match the scientists below to their contributions to the atomic theory. You may use one more than once.
Democritus
__________
__________
__________
__________
__________
__________
__________
Dalton
Thomson
Rutherford
Bohr
Schrodinger
electrons orbit the nucleus like planets around the sun
first mental model of the atom; “atomos”
electrons exist in electron cloud where there is a 90% probability of finding the electron
electrons are housed in energy levels filling the lowest energy level first
proved the existence of atoms as small, indivisible particles; atoms combine in ratios
nucleus is a small, dense central part of the atom containing all of the atom’s mass
found that the atom is NOT the smallest particle in the atom, charged particles exist within the atom
7. Complete the following table using notes over parts of an atom.
Location in atom
Symbol
Proton
Charge
Mass (amu)
Neutron
Electron
(not zero) What
is it really?
8. If you had a balance and weighed a proton, how many electrons would you need to equal the mass of one
proton?
9. List at least two ways isotopes of the same element are alike and at least two ways they are different
Review - Continued
10. How is atomic number determined?
11. How is mass number calculated?
12. If lithium has an average atomic mass of 6.941 amu, would Li-6 or Li-7 be more abundant? Explain.
13. Complete the following table.
Atom Identity
Atomic
Number
Mass
Number
Number of
protons
39
19
Number of
neutrons
Number of
electrons
𝟏𝟏𝟏𝟏𝟏𝟏
𝟕𝟕𝟕𝟕 𝐀𝐀𝐀𝐀
𝟐𝟐𝟐𝟐
𝟏𝟏𝟏𝟏 𝐌𝐌𝐌𝐌
10
50
10
120
hydrogen-1
hydrogen-2
-
+
+
-
+
+
+
+
-
14. Neon has three natural isotopes: neon - 20 (88.52%, 19.99244 u), neon - 21 (2.27%, 20.99395 u)
neon - 22 (9.22%, 21.99138 u). Calculate the average atomic mass of neon. SHOW YOUR WORK.
1 mole = ___________________ particles/atoms/molecules
1 mole = ___________________ grams
1 mole = ___________________ liters
15. What is the mass in grams of 3.45 x 1020 atoms of carbon?
16. What is the mass in grams of 2.95 moles of Al?
17. How many moles of neon are contained in 7.00 L of neon?
18. How many g of lead are equivalent to 1.50 x 1018 atoms?