Download ChLM Final Review Name: Period: Base Knowledge 1. Classify the

ChLM Final Review
Name:
Period:
9. For generic element “X”, define what goes in each location in the
symbol (hint: remember these are all whole numbers).
Base Knowledge
1. Classify the following as observations or inferences
a) The liquid is green because food coloring was added.
b) The beaker has green liquid in it.
c) The beaker can hold up to 250 mL.
d) The beaker will be the best tool for this lab.
2. Measure the following, circle your estimated digit and include units
X
10. Complete the following table.
Element Symbol Atomic Mass
mass
number
Atomic # of
number p+
# of
n0
# of
e-
Neon
a)
b)
Atoms
3. What part of an atom determines which element it is?
__________________
4. Which particle determines the chemical reactivity of an atom?
____________________
5. What does the word “neutral” mean? When is an atom neutral?
Nickel
Ions
11. What happened to the electrons to make a cation? ___________
12. What happened to the electrons to make an anion? ___________
13. What is the difference between a magnesium atom and a
magnesium ion (+2)?
14. What is different between a fluorine atom and a fluoride ion (-1)?
6. Define the following words, use equations when helpful:
a) Atomic Number
b) Mass Number
c) Atomic Mass
7. How do you get from Atomic Mass to Mass Number?
_________________________________
8. How do you find the number of neutrons in an atom?
15. Complete the following table.
Element Symbol
Mass
Number
Silver
108
+
47
Iodine
127
53
Oxygen 16
8
Ag
I
O
Protons
Neutrons
Electrons
10
Periodic Table
16. On the Periodic Table, which type of elements make cations? Which
type make anions?
17. List three metals.
18. List three nonmetals.
19. List two halogens. How many valence electrons do the halogens
have?
20. List two alkaline earth metals. How many valence electrons do the
alkaline earth metals have?
21. Why don’t the noble gases react with anything?
22. Draw arrows showing where periods and groups are on the periodic
table.
23. Use the periodic table to identify the element in period 3, group 17.
What do you know about this element? (What is the name of its
group? How many valence electrons does it have?
24. As you move left to right in a period, what happens to the mass of
the elements?
Rutherford
25. What kind of particles did Rutherford shoot at the thin gold foil?
_________________
26. What did we learn about atomic structure because of Rutherford’s
experiment?
Isotopes
27. How many protons, neutrons and electrons are in one neutral atom
of each of the following isotopes?
a) Beryllium-9 p =
b) Silicon-28
p=
c) Silicon-29
p=
n=
n=
n=
e=
e=
e=
28. Write the complete symbols for neutral atoms of Potassium-39 and
Potassium-40.
29. Which of the above isotopes is the most common? How did you
decide this?
30. The less common isotope in #10 is radioactive. What does it mean if
something is radioactive? Use the words “stable,” “nucleus,” and
“decay” in your answer.
Radioactive Decay
31. What are the three types of radioactive decay you learned about?
Write the symbol for each (include all relevant numbers).
32. Which part of the atom changes during radioactive decay?
Half-Life
33. Use the following graph to determine the half-life of Uranium-238.
Ionic/Covalent
38. What kinds of elements are in ionic bonds? _____________ &
________________
39. What kinds of elements are in covalent bonds? ________________ &
______________
40.
Ionic Formulas & Naming – give the appropriate name or formula
for the following ionic compounds.
Chemical Name
Chemical Formula (make
sure your ratio is correct)
Potassium iodide
34. If you started with 100 g of Uranium-238, how many grams would
be left after 9000 million years? How many half-lives is 9000 million
years?
Calcium nitride
Rb2O
Al2S3
Electromagnetic Spectrum
35. What is the highest energy color of visible light? Which is the
lowest?
Bohr Model
36. How many electrons can fit on the first energy level of the Bohr
model? _____ How many on the second? _____
41. Covalent Formulas & Naming – give the appropriate name or formula
for the following covalent compounds. (remember prefixes in your notes)
Chemical Name
Chemical Formula
Sulfur hexafluoride
Dihydrogen monoxide
CH4
37. Draw the complete Bohr model for Beryllium and Magnesium
(remember to show protons & neutrons). What do the electrons have
in common between these two elements?
P2Cl5
Which of the following compounds would you expect to have a
lower melting point? How did you decide?
a) LiBr or
NO2
b) PCl3 or
MgCl2
43.
Which of the following compounds would you expect to conduct
electricity when dissolved in water? How did you decide?
a) LiBr or
NO2
b) PCl3 or
MgCl2
42.
44.
What do we call one unit of a covalent compound?
45.
How are covalent compounds held together?
Balancing
46.
Which side of a chemical equation are the reactants on? The products?
47.
___(NH4)2S (aq) + ___ZnCl2 (aq)  ___ ZnS (s) + ___NH4Cl (aq)
Reaction type: _________________
48.
___Na2CO3 (s)  ___ Na2O (s) + ___CO2 (g)
Reaction type: _________________
49.
___H2 (g) + ___I2 (s)  ___ HI (g)
Reaction type: _________________
50.
___Rb (s) + ___HCl (aq)  ___ RbCl (aq) + ___H2 (g)
Reaction type: _________________
51.
___C9H20 (l) + ___O2 (g)  ___ H2O (l) + ___CO2 (g)
Reaction type: _________________