Name:____________________________
Date:______________________________
Unit 2 Atomic Structure – Ions Guided Notes
Pd:________
Atoms can lose or gain electrons to become Ions!
Key Vocabulary
_______________: atom with a plus or a minus charge. Atom with a different number of protons and electrons.
_______________: an atom with a positive charge. Atom with more protons (+) than electrons (-)
•
Cats have paws….Cations are pawsitive…
______________: an atom with a negative charge. Atom with more electrons (-) than protons (+)
•
A negative ion, looks like onion (make you cry… is negative)
Charge on this Atom?______________ or ____________
Charge on this Atom?______________
Charge on this Atom?______________
Na+
Positive one charge means it has one __________electron (negative particle) than proton.
Mg2+ Two ____________electrons than protons.
F1-
One ___________ electron than protons.
N3-
Three __________ electron than protons.
Atoms lose or gain ELECTRONS!
PROTON NUMBER ___________ CHANGES!
Justification?
Practice
In Summary
# of
Protons
Look at the Atomic Number
1. Round the Average Atomic Mass
to a Whole Number
# of
Neutrons
To
determine
2. Subtract the Atomic Number
FROM the rounded Atomic
Mass
3. # of Neutrons = Atomic Mass-Atomic Number
1. In a Neutral Atom,
Look at the Atomic Number
# of
Electrons
a. If Positive Charge
[ Atomic Number- Charge]
2. In an Ion
b. If Negatively Charged
Charge on Atom
# protons #electrons =
Charge
[ Atomic Number + Charge]
Name:____________________________
Date:______________________________
Isotope and Ion Classwork
Pd:________
1. State the number of p+, n, and e- that are present in the following atoms.
p+
en
7
a.
Li
3
b.
199
Hg
80
c.
112
Cd
48
59
Co
27
2. State the number of p+, n, and e- that are present in the following atoms.
p+
n
a.
Sodium - 23
d.
b.
e-
Barium - 137
c. Manganese - 55
d.
Chlorine - 37
3. Write the nuclear symbol ( 𝐴𝑍𝑋) for each of the following isotopes. Use the periodic table to determine the
correct symbol to use instead of “X”.
a. Chromium with an atomic mass of 54: _____________
b. Silver with a total of 157 subatomic particles: _____________
c. Calcium with 42 nucleons (particles in the nucleus): _____________
d. Sulfur with 18 neutrons: _____________
4. Circle the required symbol(s) that answer each question. (“X” is just a general symbol.)
16
15
15
14
a. have the same atomic mass
8
8
7
7
X
X
X
X
b. have the same atomic
number
32
16
X
30
16
X
32
15
X
35
17
X
c. isotopes of the same
element
18
9
X
18
8
X
18
7
X
20
9
X
d. same number of neutrons
15
7
X
16
8
X
18
10
X
14
6
X
5. For each of the following ions, indicate the total number of protons and electrons in the ion.
Ion
Number of Protons
Number of Electrons
Co+2
Co+3
Cl-1
K+1
S-2
Sr+2
Al+3
P-3
6. Fill in the following chart
Element/Ion
1
1
1
1
Number of
Protons
Number of
Neutrons
Number of
Electrons
Mass
Number
28
66
H
H+
12
6
7
3
C
Li
Cl-
35
17
39
19
24
12
Atomic
Number
K
Mg 2+
75
33
108
47
As
Ag +
32
16
S2-
30
76
114
7. How can you tell if an atom has a negative charge?
8. How can you tell if an atom has a positive charge?
9. Define an isotope.
10. What would happen if the number of protons were to change in an atom?