Download Semester 1 Exam Review Part 1

OBJECTIVE
FINAL
REVIEW
PART 1
SUBTITLE
1. Where are the subatomic
particles of an atom?
Proton
Neutrons
Electrons
2. What are the charges of the
subatomic particles ?
Protons
are positively (+)charged
Neutrons are neutral (0)
Electrons are negatively (-)charged
3. Where are the 3 subatomic particles
located?
 Made
up of:
Protons--inside
nucleus
Neutrons--inside nucleus
Electrons--outside
nucleus in
the cloud
4. Which subatomic charge
determines the charge of atom?
 If
there are more protons than electrons-the charge of the atom will be positive
 If
there are more electrons than protons-the charge of the atom will be negative
 If
the protons are equal to the electrons-the atom will have a neutral charge
5. Which subatomic particle determines
the chemical reactivity of the atom?
 The
chemical reactivity is determined
by the valence electrons--the
number of electrons in the outermost
shell
6. What does the atomic number
of an element refer to?
The
atomic number is equal to the
number of protons in the nucleus
A = Atomic Number
These are all
equal to each
P = Proton Number
other
E = Electron Number
7. How can atomic mass be
calculated?
M = Mass Number
A = Atomic Number (Proton #)
N = NeutronNumber
Protons + Neutrons = Mass Number
8. Fill in the chart.
Proton
+
1 amu
Nucleus
Neutron
Neutral
1 amu
Nucleus
Electron
-
.00054 amu Electron Cloud
9. Label picture and sentences.
Atomic Number
Symbol
Name
Atomic Mass
Atomic number equals the number of
Protons
Electrons
____________
or ______________.
Atomic mass equals the number of
Protons
Neutrons
_____________
+ ______________.
Group/Family
_____________________
Properties
_____________________
Period
_____________________
Non-metals
_____________________
10. Vertical column in the Periodic
Table.
11. Elements in the same family
have similar ___.
12. Horizontal row on the Periodic
Table.
13. Elements on the right side of the
Periodic Table.
Valence
Electrons14.
_____________________
Number of electrons in the outer
most shell.
Ductile
_____________________
15. If it can be drawn or pulled into
wires, it is ___.
Energy Levels
____________________________
16. The period tells what row
an element is in or how
(shells)
many ___ are used.
Metals
____________________________
17. Elements on the left side
of the Periodic Table.
Transition Metals
____________________________
18. Elements in Groups 3-12
on Periodic Table.
Noble Gases
______________________
19. Elements in Group 18; they are
unreactive.
Metalloid
______________________
20. Touches the zig-zag line; has
properties similar to both metal
and non-metal.
Malleable
______________________
21. If it can be bent or hammered
into shape it is ___.
Alkali
Metals
______________________
22. Most reactive metals.
Periods
23. Organization of the Periodic Table of Elements
Metals
Metalloids
Non-metals
Noble Gases
Groups
24. Fill in the chart
Symbol
Na
P
Xe
Si
Proton #
Atomic #
Mass #
11
15
54
14
11
15
54
14
23
31
131
28
Electron #
11
15
54
14
Neutron #
12
16
77
14
Metal, Nonmetal
Valence #
Metalloid or Noble Gas
Group # Electron # Period #
Metal
Nonmetal
Noble Gas
Metalloid
1
15
18
14
1
5
8
4
3
3
5
3
25. As you go down the periodic table, the number of
energy levels Increases
26. List the properties of metals
Luster
a. _________________________________________
Malleable
b. _________________________________________
Ductile
c. _________________________________________
Great
Conductors
d._________________________________________
High
Melting
Points
e. _________________________________________
High Density
f. _________________________________________
27. List the properties of nonmetals
Dull
a. ____________________________________________
Brittle
b. _____________________________________________
Poor
Conductors
c. _____________________________________________
Low Melting Points
d. _____________________________________________
Low Density
e. _____________________________________________
28. What do elements in the same group
have in common?
 Have
the same number of valence electrons
 Similar properties
29. How do you determine the number of
atoms in a compound

4K2CO3
3Ba3(PO4)2
 Type of Atom # of Atoms Type of Atom
# of Atoms
 K
______________
______
_______________
______
- Potassium
8
Ba
- Barium
9
- Carbon
P - Phosphorus ______
 C
______________
______
_______________
4
6
- Oxygen
O - Oxygen
24
12
 O
______________
______
_______________
______
39
24

Total ______
Total ______

30. What are the signs of a chemical
reaction?
 Remember:
 Color
City Girls Like Their Phones On
Change
 Gas Produced (bubbles)
 Light emitted
 Temperature change
 Precipitate Formed
 Odor Let off
31. Which diagram
best demonstrates
the law of
conservation of
mass?
4Fe + 3O2  2Fe2O3
32. The numbers after the symbols and
formulas in the chemical reaction above are
called
A. Subscripts
B. Superscripts
C. Fractions
D. Coefficients
4Fe + 3O2  2Fe2O3
33. Each substance to the right of the arrow
in the equation given above is a
A. Catalyst
B. Precipitate
C. Reactant
D. Product
4Fe + 3O2  2Fe2O3
34. Each to the left of the arrow in the
equation given is a
A. Catalyst
B. Precipitate
C. Reactant
D. Product
4Fe + 3O2  2Fe2O3
35. The numbers before formulas in the chemical
reaction that are added to balance the above
are called
A. Subscripts
B. Superscripts
C. Fractions
D. Coefficients
36. How do you know that the
reaction is balanced?
4Fe + 3O2  2Fe2O3
4 Fe 6 O
4 Fe 6 O