1. Write formulas for the following compounds:
a)
b)
c)
d)
e)
f)
sodium carbonate
hydrochloric acid
carbon tetrachloride
diphosphorus pentoxide
ammonium sulfate
barium chloride
g) lithium sulfide
h) potassium phosphide
i) cobalt (II) bromide
j) iron(III) oxide
2. Write names for the following formulas:
a)
b)
c)
d)
e)
f)
BeCl2
Na2S
CuCl
Ca(OH)2
Mg(NO3)2
Na3PO4
g) FeS
h) NiSO4
i) AgBr
j) SiCl4
k) SF6
3. What is the charge (sign & magnitude) on the calcium ion in CaO? What is the charge on the oxide ion in CaO?
4. Give 2 examples of chemical changes and 2 examples of physical changes.
5. Find the mass of 2.36 moles of sulfur trioxide. How many sulfur trioxide molecules are in this sample?
6. Express 100C in Kelvin. Express 303 K in degrees Celsius.
7. Write and balance the equation for the reaction between iron and phosphoric acid to form iron(III) phosphate and hydrogen gas.
What reaction type is this?
8. How many protons, neutrons, and electrons make up an atom of potassium-39?
9. Give the symbols for 3 elements that most commonly form 2+ ions.
10. Give the symbols for 3 elements in the same family.
11. Describe the experiments that led to the discovery of the nucleus and the electron in the atom. Which scientists are credited with
these experiments/discoveries?
12. State the Law of Conservation of Matter. Explain what this means in your own words.
13. State the Law of Multiple Proportions. Explain what this means in your own words.
14. When an atom gains one or more electrons, it forms a __________ ion. When an atom loses one or more electrons, it forms a
__________ ion. How many protons, neutrons, and electrons are in a chloride ion (Cl -)?
15. Explain the meaning of the following notation:
40
20Ca.
16. What does the mass number of an element represent? Describe the location of protons, neutrons, and electrons in the atom, and
state their relative masses.
17. What is an isotope? How does one isotope of an element differ from another? What is one way to separate isotopes of the same
element from each other?
18. Where are metal elements located in the periodic table? Where are the nonmetals? Where are the metalloids?
19. What is an orbital? Describe the shape of s, p, and d orbitals. How many electrons can occupy each type of sublevel (s,p,d)?
How many electrons can occupy one orbital?
20. Write the electron configurations for an atom of sulfur and an atom of potassium. How will the configurations be different for a
sulfide ion, S2-, and a potassium ion, K+ ?
21. What produces the brightly colored lights of “neon” signs?
22. Write the balanced equation for the reaction of sulfuric acid and potassium hydroxide to form potassium hydrogen sulfate and
water. What reaction type is this?
23. If one mole of sulfuric acid reacts as in the reaction described in the problem above, how many moles of water form?
24. Find the number of moles of chlorine required to react with aluminum to form 75.0 g of aluminum chloride. What volume at STP
would this amount of chlorine gas occupy? What type of reaction is this?
25. Ethylene glycol, the substance used in automobile antifreeze, is composed of 38.7% C, 9.7% H, 51.6% O by mass. Its molar mass
is 62.1 g/mol. What is the empirical formula of ethylene glycol? What is its molecular formula?
26. Write and balance the equation for the complete combustion of butane, C4H10. How many moles of oxygen would be required to
burn 58.0 g of butane?
27. Determine the percent by mass of carbon in butane.
28. How many grams of water can be formed from 5.00 grams of hydrogen reacting with excess oxygen?
29. How many atoms of each element are in a formula unit of aluminum chromate, Al2(CrO4)3? What is the total number of atoms in
one formula unit of aluminum chromate?
30. Write and balance the equation for the reaction of magnesium and nitrogen to form magnesium nitride. How many moles of
magnesium are required to react with 8.00 moles of nitrogen?