1. HOLD UP YOUR BOARD!
Chapter 7 Review game

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Rules
Use the same periodic table.
Use the mass as written on the periodic table
Round up your calculations to 2 decimal points
Follow significant rule for your final answer
Do the calculation on the board and circle your answer
All your units must be included for full credit!
If you get a questions wrong, you are out until you get the “COME BACK” questions correct.
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Rules
Everyone will need to show their own work on a separate sheet of paper for a 1 HW credit.
The winning team will receive 5pt extra credit on the test.
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4. Find the number of molecules or ions 2.00 mol Fe 3+
Question #1
Find the number of molecules or ions
2.00 mol Fe 3+
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6.02 x 1023 ions
2.00 mol
1 mol
= 1.20 x 1024 ions
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6. Find the number of moles.
Question #2
Find the number of moles.
3.01 x 1023 molecules of H2O
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1 mol
3.01 x molecules
6.02 x 1023 molecules
= mol H2O
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8. Find the number of moles of sodium ions Na+ Na2CO3
Question #3
Find the number of moles of sodium ions Na+
Na2CO3
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2 mol of Na+
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10. Find the number of sodium ions 3.00 mol Na2CO3
Question #4
Find the number of sodium ions
3.00 mol Na2CO3
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3.00 mol Na2CO3
2 mol Na+
6.02 x 1023 ions
1 mol Na+
1 mol Na2CO3
= 3.61 x 1024 atoms
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Question #5
Find the mass in grams
4.30 x atoms of He
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4.30 x atoms
1 mol
4.00 g
6.02 x 1023 molecules
1 mol
= 2.86 x 10-7 g He
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COME BACK!!!!!
Find the mass in grams
4.01 x atoms of Ca
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4.01 x atoms
1 mol
40.08 g
6.02 x 1023 molecules
1 mol
= 26.7 g Ca
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16. What is the percent composition of Na in NaCl?
Question #6
What is the percent composition of Na in NaCl?
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NaCl = g Na
22.99g Na g Cl = g NaCl
22.99 g Na x 100 %
58.44 g NaCl
= 39.34% Na
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18. Determine the empirical formula of a compound that is 63.50% Ag,
Question #7
Determine the empirical formula of a compound that is
63.50% Ag,
8.25% N
28.25% O.
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63.50g Ag = 0.59 mol Ag
8.25 g N = 0.59 mol N
28.25 g O = 1.77 mol O
Divide all the mol by 0.59.
AgNO3
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20. Determine the empirical formula of a compound that is
Question #8
Determine the empirical formula of a compound that is
56.34% P
And the rest is O.
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56.34g P = 1.82 mol P
43.66 g O = 2.73 mol O
Divide all the mol by 1.82.
PO1.5
Multiply by 2 for whole number ratio
P2O3
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Question #9
A compound has an empirical formula of CH. Its molecular mass is 78 g/mol. What is its molecular formula?
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C = g/mol
H = g/mol
13.02 g/mol
78 g/mol
13.02 g/mol = = 6
6 (CH) = C6H6
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Question #10
The empirical formula is P2O5. Its molar mass is 284 g/mol. Determine the MOLECULAR formula.
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P x 2 = g/mol x 2
O x 5 = g/mol x 5
g/mol
284 g/mol
g/mol = 2
2 (P2O5) = P4O10
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