Name: ________________________
Per: ____________
STUDY GUIDE FINAL EXAM
1) Why is the boiling point of water a physical change if water changes from a liquid to a gas?
2) How are elements in the same family on the periodic table similar?
3) Amy is trying to find the density of an unknown metal in the lab. She followed the procedure
below but she spilled soda on her composition notebook so she can’t see some parts of the
procedure. Fill in the missing information for the steps.
I. Find the mass of the unknown metal using ______________
II. Find the ___________ of the unknown metal by measuring water displacement (or by using
a formula and measuring the length of the metal)
III. Divide ________ by ____________ and use the units __________
4)
5) Fill in the following chart:
Atom
Protons
Chlorine-37
14
C
Lithium-7 with a charge
of +1
Boron-10
56
Fe with a charge of +3
Neutrons
Electrons
6)
Timothy wants to show his chemistry teacher that he can produce a chemical change and a
physical change in a lab. But he is a little confused. Write a procedure for him to follow to show
a chemical change and a physical change in the lab. Hint: think about lab safety!
7) Define and explain the differences between an element and a compound? State an example of
each. Draw a particle diagram of an element and of a compound.
8) Explain how to determine:
a. The atomic number
b. The atomic mass
c. The identity of an element
9) Draw a particle for sodium chloride, table salt, hydrogen gas, and magnesium metal. Describe
why these diagrams are different.
10) Group 8A elements are called ________________________
11) Elements located to the left of the stair-step are __________________________
12) Group 1 elements are called _____________________
13) Alkaline Earth Metals are located in group ________
14) Elements touching the stair-step are ___________________________. Their properties are
_______________________________
15) Group 7A elements are called ___________________________
16) An atom with a positive or negative charge is called an ____________________. It becomes
charged when it loses or gains ____________________________.
17) Name the following compounds:
a. CuI2
b. Ca(NO2)2
c. AlCl3
18) Write the chemical formula for the ionic compound formed by each pair of ions.
a. Na+ and Br−
b. Ca2+ and Br− c. K+ and Cl− d. Mg+2 and O−2
19) Write the chemical formula for the ionic compound formed by each pair of ions.
a. Fe+3 and Br− b. Fe+2 and PO4−3
c. Al3+ and OH− d. NH4+ and NO3−
20) For each pair of elements, determine the charge for their ions and write the proper formula for
the resulting ionic compound between them.
a. Ba and O
b. Li and I
21) How can you tell if a compound is ionic?
22) What are the properties of ionic and molecular compounds?
23) State two compounds which would conduct electricity when placed in water, and two
compounds which would not conduct electricity. Discuss why these compounds have different
properties.
24) Name the following compounds:
a. SO2
b. N2S
c. CCl4
d. P4S9
25) State two reasons that cations are smaller than neutral atoms.
26) State two reasons that electronegativity increases as you go to the right.
27) Explain why ionization energy is high as you move across a period using key terms such as
protons, electron shells, and atomic radius.
28) How many moles are in the following?
a) 3.45g Ca ________
b) 2.34x1023 atoms Cu _______
c) 3.34g Ca(NO3)2________
29) How many oxygen atoms are in Ba(NO3)2? Barium atoms? Nitrogen atoms?
30) What is the percent by mass of carbon in C6H12O6?___________
31) Which of the following has the highest percent by mass of Calcium? ___________
a) Ca(NO3)2
b) CaCl2
c) CaO
d) CaBr2
32) What is the total number of molecules of CO2 in 3.34moles CO2? ___________
33) What is the molar mass of (NH4)3PO4? _______
34) How many grams are in the following samples?
a) 4.3 moles C ______
b) 3.45 x 1024 atoms Fe ________
c) 4.96 moles MgBr2 ____
Use the following equation for questions 35-38
Zn+ 2HCl  ZnCl2 + H2
35) State the reactants and products of the reaction ___________________________
36) What is the number of moles of H2 that could be produced from 4 moles of HCl? ________
37) Calculate the number of grams of ZnCl2 that could be made from 34.56 g Zn. ________
38) In a laboratory experiment you mix 32.65 g HCl with 42.33 g Zn, which is the limiting reactant?
________ AND how many grams of ZnCl2 could be produced? ________
Use the following equation for questions 39-44
Fe + O2  Fe2O3
39) Balance the equation
40) How many grams of Fe would be required to produce 3.56g Fe2O3? ________
41) In a laboratory experiment you mix 83.5 g Fe with 65.3 g O2, how many grams of Fe2O3 could be
made? ________
42) In the previous experiment you actually made 110 g Fe2O3, what was your percent yield?
______
43) A compound contains 79.852% Cu and 20.15% S, what is the empirical formula for this
compound?
44) A compound contains 42.88% C and 57.12%O, what is the empirical formula for this compound?
Read the following scenario and answer the questions below
Ani is conducting an experiment to produce NaCl (table salt) by starting with baking soda and adding
hydrochloric acid. The equation for this experiment is show below.
NaHCO3(s) + HCl(aq)  NaCl(s) + CO2(g) + H2O(l)
When the reaction occurs, Ani observed bubbles forming and saw that a liquid formed. She then heated
this liquid until it boiled off and then a white solid was left.
45) What evidence is there that a chemical reaction took place?
46) What was the liquid that boiled off?
47) State at least 4 pieces of lab equipment that Ani would need to conduct this experiment. She
MUST use a hot plate to boil off the liquid.
48) Ani is using this lab to determine the limiting reactant. She began with 10.4 g NaHCO3 and
7.29 g HCl. What would be a valid conclusion from this lab?
49) What is the theoretical yield of H2O?
50) Ani realizes that she is running out of time so she decides that even though she can still see
some liquid, she will stop and find the mass of the solid. What is the problem with this logic?