Name___________KEY______________________________________
Hour_______
Chemistry Unit (Part 3) Study Guide
Goal 1
1. List properties of each in the table below. (Hint: We filled out notes from the textbook and glued it in our
NB.)
Metals




Metalloids
Luster
Malleable
Ductile
Good conductor of heat
and electricity


Nonmetals
Has properties of both
metals and nonmetals
(some are malleable or
ductile or have luster or a
combination)
Semiconductors - good
conductors at high temps.



Dull (no luster)
Not malleable
Not ductile
Many are gases at
room temperature
Good insulators


2. Using the periodic table, determine if each element is a metal, nonmetal, or metalloid. Then give its group
and period.
Element
Metal/Nonmetal/Metalloid
Group
Period
Helium
Nonmetal
18
1
Cobalt
Metal
9
4
Barium
Metal
2
6
Iodine
Nonmetal
17
5
3.
Give the properties of the elements in each of the FAMILIES:
Family
Properties
Alkali Metals
Alkaline Earth
Metals
Transition
Metals
Halogens
Noble Gases
•React quickly with
React quickly
with other
elements, but not
as quickly as the
alkali metals.
Do not occur
naturally. They
combine with
other elements
and form
compounds.
Soft and silvery.
Some exist in
nature as free
elements.
Because of their
high densities,
strength, and
resistance to
corrosion,
transition
elements make
good building
materials.
The term halogen
refers to an
element that can
react
with a metal and
form a salt.
Halogens only
can occur
naturally in
compounds. All
halogens are very
reactive.
Do NOT form
compounds
naturally.
other elements, such
as oxygen.
•React violently with
water.
•In nature, they occur
only in compounds.
•Pure alkali metals
have a silvery
appearance.
•Soft enough to cut
with a knife.
•Lowest densities of all
metals.
Noble gases are
usually
nonreactive.
Goal 2
4. Give an example that proves a single element is different than a compound that contains that element.
Explain why they are different.
Elements are completely different than the compounds that contain them. Hydrogen
(H) and Oxygen (O) are both gases. Hydrogen is highly flammable and oxygen is what we
need to breath. They combine to make water (H20), which is a liquid that is not flammable
and completely different from hydrogen and oxygen.
5. What elements make up the compound Na2Cl3? How many atoms of each element are in a molecule of
that compound?
2 Sodium & 3 Chlorine atoms
6. What elements make up the compound K2SO4? How many atoms of each element are in a molecule of
that compound?
2 Potassium, 1 Sulfur, & 4 Oxygen atoms
Goal 3
Use the following chemical equations to answer the questions:
6H2O
→
Photosynthesis
6CO2 +
Cellular Respiration
C6H12O6 + 6O2 →
C6H12O6
+
6H2O
6CO2
+
6O2
7. What are the reactants in photosynthesis?
6CO2 +
6H2O (carbon dioxide & water)
8. What are the products in cellular respiration?
6H2O
+
6CO2 (water & carbon dioxide)
9. How does the law of conservation of mass/matter apply to a chemical equation?
Mass is conserved (no loss of matter) during a chemical reaction because the number
of atoms going in equals the number of atoms coming out.
The same elements that go into a chemical reaction must go out, they will likely be
rearranged in different compounds though. (Ex: for photosynthesis, the elements that
go into the reaction are Carbon, Oxygen, and Hydrogen, AND only those same
elements come out, they are just rearranged in a different way)
Challenge Only (# 10-13) - balance the following chemical equations.
10. _1___H2SO4 + __2__NaNO2 → _2___HNO2 + __1__Na2SO4
11. _1___FeCl3 + _3___NaOH → _1___Fe(OH)3 + _3___NaCl
12. _1___CH4 + _2___O2 → __1__CO2 + _2___H2O
13. __2__K + __1__MgBr2 → __2__KBr + _1___Mg
Goal 4
14. List the charges of the following particles. (neutral, positive or negative)
a. Protons ______positive______________
b.
Neutrons ________neutral________
c.
Electrons _____negative____________
15. Draw diagrams of the following atoms. Label each part (nucleus, electrons, neutrons, protons, electron
cloud)
Fluorine
Protons _9__ Neutrons _10__ Electrons _9__
Lithium
Protons _3__ Neutrons _4__ Electrons _3_
Goal 5
16. Fill in each of the empty boxes for the ISOTOPES below.
Isotope Name
Atomic
Number
Protons
Neutrons
Electrons
Mass Number
Mercury-203
80
80
123
80
203
Zirconium-90
40
40
50
40
90
105
45
45
60
45
105
24
24
34
24
58
Rh
Chromium-58
17. Draw the following isotopes with the correct number of protons, neutrons, and electrons.
Carbon-13
Protons _6_ Neutrons __7_ Electrons _6_
Helium-3
Protons _2_ Neutrons 1 Electrons _2__
18. What does the number in the isotope name mean?
The atomic mass or mass number
19. How is Carbon-14 different from Carbon-12?
The atomic mass is different because there are a different number of NEUTRONS. Carbon-14 has 8
and Carbon-12 has 6 neutrons.
Goal 6
20. How is the ion He+ different from He - ?
He+ has ONE more protons than electrons so it is positively charged. He- has ONE more electrons than
protons so it is negatively charged.
21. Draw the following IONS with the correct number of protons, electrons, and neutrons.
B2+
Li3-
Protons _5_ Neutrons _6_ Electrons _3_
Protons _3_ Neutrons _4_ Electrons _6_
22. Fill out the table below for the following IONS.
Ion Name (Ex: N+)
Protons
Neutrons
Electrons
Bi3-
83
126
86
Y2-
39
50
41
Cs+
55
78
54
Ge+
32
41
31
Cu+
29
35
28
Te2-
52
76
54
Xe3-
54
77
57
Goal 7 - CHALLENGE ONLY!
23. Draw the following atoms with the correct number of protons, neutrons and the correct number of
electrons in each energy level:
Magnesium
Protons _12__ Neutrons _12__ Electrons _12__
Neon
Protons _10__ Neutrons _10__ Electrons _10__
24. Fill out the number of electrons for each atom in the table below.
Energy Level
Astatine (At)
Strontium (Sr)
Gallium (Ga)
1
2
2
2
2
8
8
8
3
18
18
18
4
32
8
3
5
18
2
---
6
7
----
---