Download FINAL REVIEW 1st SEMESTER 2014-2015

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1. Write the name of the following compounds.
a. HC2H3O2 ______________________________________
b. Co2(CO3)2 ______________________________________
c. NH3 ____________________________________________
d. H3PO4 __________________________________________
2. Write the formula for each of the following compounds.
a. dinitrogen tetraoxide
b. manganese(IV) sulfide _____________________________
c. sodium hypochlorite ______________________________
d. nitric acid _______________________________________
3. How many significant digits are in the following numbers?
a. .0012 __________
b. 4002 _________
4. Calculate the formula mass for:
a. CuSO4· 5H2O ____________________________________
b. NH4C2H3O2 _____________________________________
5. Calculate the mass in grams for:
a. 2.80 moles Al(OH)3
b. 3.00 x 1024 molecules O2
Find the percent of hydrogen in CaCl2· 6H2O.
7. Balance the following equation.
Cu + HNO3 → Cu(NO3)2 + NO2 + H2O
Balance the following equation.
aluminum acetate + sodium hydroxide → aluminum hydroxide + sodium acetate
9. Find the empirical formula for the compound that contains 1.24 g Cr and .76 g O.
10. Find % of Fe and % of Cl in FeCl2
11. Find the formula of the hydrate. A hydrated compound has an analysis of 18.2% Ca, 32.37% Cl,
and 49.3% H2O
CH 3, 4, 5 RED BOOK
electron configurations (to include orbitals, quantum numbers, order of filling, relation to position of
element in periodic table to its configuration)
relate atomic number and atomic mass to position in the periodic table, isotopes, numbers of
subatomic particles (protons, neutrons, electrons)
compare the three subatomic particles (protons, neutrons, and electrons)
distinguish between a solute, solvent, solution, and precipitate and give examples of each
difference between a physical and a chemical property, an element and a compound, homogenous
mixture and a heterogeneous mixture,