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NAME _______________________________
DATE _______________________________
DIRECTIONS: Answer the following questions to help you prepare for your test. Circle
the questions you can’t answer so that you can focus on those to help you study.
Answer the questions on a separate sheet of paper.
1.
What is the simplest form of matter?
The simplest FORM of matter is an ELEMENT.
2.
What is the simplest particle of matter?
The simplest PARTICLE of matter is an ATOM.
3.
Atoms of the same element are the SAME.
4.
Atoms of different elements are DIFFERENT.
5.
What are atoms made up of?
Atoms are made up of subatomic particles; specifically, protons, neutrons,
and electrons.
6.
Describe the location of the particles that make up the atom.
Protons and neutrons are clumped together to make up the nucleus, and
electrons are moving in the electron cloud.
7.
Describe the charges of the particles that make up the atom.
Protons have a + 1 charge, neutrons have no charge (0), and electrons have
a – 1 charge.
8.
Draw the current model of the atom.
9.
How do you determine the charge of an atom?
Since protons have a + 1 charge and electrons have a – 1 charge. The
charge of the atom is (protons – electrons).
10.
What is the atomic number of an atom?
The atomic number of an atom is always the same as the number of protons.
11.
What does the atomic number of an atom tell you about that atom?
The atomic number can tell you what element the atom is.
12.
How do you determine the mass number of an atom?
Protons have a mass of 1 amu, neutrons have a mass of 1 amu, and
electrons have no mass. So the mass number of an atom is equal to the
(protons + neutrons) amu.
13.
What does the mass number of an atom tell you about that atom?
The mass number is the mass of that one individual atom.
14.
What is an isotope?
An isotope is an atom of the same element but has a different mass number
because it has a different number of neutrons.
15.
What is the average of all isotopes of an atom?
When all the mass numbers of an isotope are averaged, you get the ATOMIC
MASS.
16.
What is a symbol?
A symbol is the abbreviation for an element name.
17.
How do you write a complete symbol for an atom?
A complete symbol contains not only the element symbol, but also the mass
number, atomic number, and the charge.
18.
Explain as best you can what the difference is between an element and an
atom.
An element is the name or title given to identify different atoms which are the
physical particle that exists.
19.
Fill in the following table.
SUBATOMIC
PARTICLE
LOCATION
MASS
CHARGE
Proton
Nucleus
1amu
+1
Neutron
Nucleus
1amu
0
Electron
Electron cloud
0 amu
–1
20.
Fill in the following table.
Atomic
Mass
Number Number
Charge
Element
Atomic
Mass
Symbol
65 amu
+2
Zinc
65.38 amu
65
+2
30Zn
80
201 amu
+1
Mercury
200.59 amu
201
+1
80 Hg
53
53
127 amu
0
Iodine
126.90 amu
127
53 I
15
18
15
30 amu
-3
88
138
86
88
226 amu
+2
Radium
226.03 amu
226
+2
88 Ra
12
12
10
12
24 amu
+2
Magnesium
24.31 amu
24
+2
12Mg
35
45
36
35
80 amu
-1
Bromine
79.90 amu
80
–1
35Br
40
51
40
40
91 amu
0
Zirconium
91.22 amu
91
40Zr
p+
n
e-
30
35
28
30
80
121
79
53
74
15
21.
Phosphorus 30.97 amu
30
–3
15P
Draw the complete symbols for three possible isotopes of the following
elements.
A) Iridium
192
77 Ir
B) Manganese
193
77 Ir
194
77 Ir
15
7N
16
7N
C) Nitrogen
14
7N
25
12Mn
26
12Mn
D) Potassium
E) Tin
118
50 Sn
24
12Mn
39
19K
40
19K
41
19K
64
29Cu
65
29Cu
F) Copper
119
50 Sn
120
50 Sn
63
29Cu