AP Chemistry Summer Assignment
The summer assignment for AP Chemistry is quite simple (but not easy). You need to master the formulas,
charges, and names of the common ions. On the first day of the school year, you will be given a quiz on these
ions. You will be asked to:
 write the names of these ions when given the formula and charge
 write the formula and charge when given the names
I have included several resources in this packet. First, there is a list of the ions that you must know on the first
day. This list also has, on the back, some suggestions for making the process of memorization easier. For
instance, many of you will remember that most of the monatomic ions have charges that are directly related
to their placement on the periodic table. There are naming patterns that greatly simplify the learning of the
polyatomic ions as well.
Also included is a copy of the periodic table used in AP Chemistry. Notice that this is not the table used in first
year chemistry. The AP table is the same that the College Board allows you to use on the AP Chemistry test.
Notice that it has the symbols of the elements but not the written names. You need to take that fact into
consideration when studying for the afore‐mentioned quiz!
I have included a sheet of flashcards for the polyatomic ions that you must learn. I strongly suggest that you
cut them out and begin memorizing them immediately. Use the hints on the common ions sheet to help you
reduce the amount of memorizing that you must do.
Do not let the fact that there are no flashcards for monatomic ions suggest to you that the monatomic ions are
not important. They are every bit as important as the polyatomic ions. If you have trouble identifying the
charge of monatomic ions (or the naming system) then I suggest that you make yourself some flashcards for
those as well.
.
Common Ions and Their Charges
A mastery of the common ions, their formulas and their charges, is essential to success in
AP Chemistry. You are expected to know all of these ions. You will always be allowed a periodic table,
which makes indentifying the ions on the left “automatic.” For tips on learning these ions, see the opposite
side of this page.
From the table:
Cations
H++
Li
Na+
K+ +
Rb
Cs+
Be2+
Mg2+
Ca2+
Ba2+
Sr2+
Al3+
Anions
-
H
F- Cl
BrIO2S2Se2N3P3As3Type II Cations
Fe3+
Fe2+
Cu2+
Cu+
Co3+
Co2+
Sn4+
Sn2+
Pb4+
Pb2+
Hg2+
Name
Hydrogen
Lithium
Sodium
Potassium
Rubidium
Cesium
Beryllium
Magnesium
Calcium
Barium
Strontium
Aluminum
Name
Hydride
Fluoride
Chloride
Bromide
Iodide
Oxide
Sulfide
Selenide
Nitride
Phosphide
Arsenide
Name
Iron(III)
Iron(II)
Copper(II)
Copper(I)
Cobalt(III)
Cobalt(II)
Tin(IV)
Tin(II)
Lead(IV)
Lead(II)
Mercury(II)
Ions to Memorize
Cations
Name
+
Ag
Silver
2+
Zinc
Zn 2+
Mercury(I)
Hg2
NH4+
Ammonium
Anions
NO2NO3SO32SO42HSO4OHCNPO43HPO42H2PO4NCSCO32- HCO3
ClO- ClO2
ClO3ClO4BrO- BrO2
BrO3BrO4IOIO2IO3IO4C2H3O2MnO4Cr2O72CrO42O22C2O-42NH2
BO33S2O32-
Name
Nitrite
Nitrate
Sulfite
Sulfate
Hydrogen sulfate (bisulfate)
Hydroxide
Cyanide
Phosphate
Hydrogen phosphate
Dihydrogen phosphate
Thiocyanate
Carbonate
Hydrogen carbonate (bicarbonate)
Hypochlorite
Chlorite
Chlorate
Perchlorate
Hypobromite
Bromite
Bromate
Perbromate
Hypoiodite
iodite
iodate
Periodate
Acetate
Permanganate
Dichromate
Chromate
Peroxide
Oxalate
Amide
Borate
Thiosulfate
Tips for Learning the Ions
“From the Table”
These are ions can be organized into two groups.
1. Their place on the table suggests the charge on the ion, since the neutral atom gains or loses a
predictable number of electrons in order to obtain a noble gas configuration. This was a focus in first
year chemistry, so if you are unsure what this means, get help BEFORE the start of the year.
a. All Group 1 Elements (alkali metals) lose one electron to form an ion with a 1+ charge
b. All Group 2 Elements (alkaline earth metals) lose two electrons to form an ion with a 2+
charge
c. Group 13 metals like aluminum lose three electrons to form an ion with a 3+ charge
d. All Group 17 Elements (halogens) gain one electron to form an ion with a 1- charge
e. All Group 16 nonmetals gain two electrons to form an ion with a 2- charge
f. All Group 15 nonmetals gain three electrons to form an ion with a 3- charge
Notice that cations keep their name (sodium ion, calcium ion) while anions get an “-ide” ending
(chloride ion, oxide ion).
2. Metals that can form more than one ion will have their positive charge denoted by a roman numeral
in parenthesis immediately next to the name of the
Polyatomic Anions
Most of the work on memorization occurs with these ions, but there are a number of patterns that can
greatly reduce the amount of memorizing that one must do.
1. “ate” anions have one more oxygen then the “ite” ion, but the same charge. If you memorize the
“ate” ions, then you should be able to derive the formula for the “ite” ion and vice-versa.
a. sulfate is SO4-2- , so sulfite has the same charge but one less oxygen (SO-32-)
b. nitrate is NO3 , so nitrite has the same charge but one less oxygen (NO2 )
2. If you know that a sufate ion is SO 42- then to get the formula for hydrogen sulfate ion, you add a
hydrogen ion to the front of the formula. Since a hydrogen ion has a 1+ charge, the net charge on
the new ion is less negative by one.
a. Example:
HPO 42H2PO 4PO43phosphate
hydrogen phosphate
dihydrogen phosphate
3. Learn the hypochlorite chlorite chlorate perchlorate series, and you also know the series
containing iodite/iodate as well as bromite/bromate.
a. The relationship between the “ite” and “ate” ion is predictable, as always. Learn one and you
know the other.
b. The prefix “hypo” means “under” or “too little” (think “hypodermic”, “hypothermic” or
“hypoglycemia”)
i. Hypochlorite is “under” chlorite, meaning it has one less oxygen
c. The prefix “hyper” means “above” or “too much” (think “hyperkinetic”)
i. the prefix “per” is derived from “hyper” so perchlorate (hyperchlorate) has one more
oxygen than chlorate.
d. Notice how this sequence increases in oxygen while retaining the same charge:
ClOhypochlorite
ClO2chlorite
ClO 3chlorate
ClO4perchlorate
I
no NOT OF.TA C:H FROM ROOK.
PERIODIC TABLE OF THE ELEMENTS
I
2
H
He
1.008
3
4
6
7
8
9
4.00
10
Li
5
Be
B
c
N
0
F
Ne
6.94
11
9.01
12
10.81
13
12.01
14
14.01
15
16.00
16
Al
Si
p
Na i\·lg
r(,
'
Cl
0
0
z
-<
0
-<
22.99
24.30
19
20
-<
-:
Cl
m
29
30
Cr i\·ln Fe
Co
Ni
Cu
Zn
Ga
52.00
42
54.94
43
58.?3
58.69
63.55
65.3')
If).72
45
46
47
48
49
Nb Mo
Tc
Ru
Rh
Pd
Ag
Cd
In
92.91
IOI.I
102.91
106.42
76
71
78
Os
Ir
Pt
22
23
24
K
Ca
Sc
Ti
v
39.10
37
4-0.08
38
44.96
47.90
40
50.94
41
Rb
Sr
y
Zr
85.47
87.62
8$,.91
9 1.22
55
56
l7
Cs
Ba *La Hf
39
72
138.91 178.49
89
104
25
73
74
(981
75
Ta
\V
Re
95.94
180.95 183.85 186.21
105
106
107
26
55.85
44
107.87 1 12.4 1 1 14.32
79
81
80
Au
Hg
137.33
87
88
Fr
Ra tAc
Rf
Db
Sg
Bh
Ds
Rg
C2l.3)
226.02 221.03
(261)
(262)
(266)
(264)
(277)
(2()8)
(271)
(272)
58
59
60
61
62
63
64
65
66
Ce
Pr
Nd
Eu
Gd
Tb
Dy
•Lanth ,11ide Series
140.12 140.9 1
91
90
tActinide Series
Th
232.04
Pa
144.24
92
u
23 1.04 238.03
190
.2
108
109
Hs Mt
Pm Sm
( 145)
93
191.2
150.4
94
Tl
195.08 196.97 200.59 204.38
110
111
132.9 1
m
z
x
28
I
: J:
m
2'
26.98
31
151 97 157.25 158.93 162.50
98
97
96
9S
28.09
32
30.97
33
Ge
As
72.59
74.9?
50
51
Sn
Sb
1 18.71 12 1.75
s
32.06
19.00
17
Cl
Ar
35.45
39.95
34
35
36
Se
Br
Kr
78.96
52
79.90
53
83.80
54
Te
127.60
I Xe
126.91
131.29
86
82
83
84
85
Pb
Bi
Po
At
Rn
(2IO)
(2?2)
207.2
208.S1! /209)
67
68
69
Ho
Er Tm
70
71
Yb
Lu
164.93 167.26 168.93 173.04 174.97
100
10 1
102
103
99
Np
Pu Am Cm
Bk
er
Es
Fm
Md
No
Lr
(237)
(244)
(247)
(251)
(252)
(257)
(258)
(259)
(262)
(2(])
(247)
20.18
18
Sulfite
Sulfate
Hydrogen
sulfate
Phosphate
Dihydrogen
Phosphate
Hydrogen
Phosphate
Nitrite
Nitrate
Ammonium
Thiocyanate
Carbonate
Hydrogen
carbonate
Borate
Chromate
Dichromate
Permanganate
Oxalate
Amide
Hydroxide
Cyanide
Acetate
Peroxide
Hypochlorite
Chlorite
Chlorate
Perchlorate
Thiosulfate
HSO4-
SO42-
SO32-
HPO42-
H2PO4-
PO43-
NH4+
NO3-
NO2-
HCO3-
CO32-
NCSSCN-
Cr2O72-
CrO42-
BO33-
NH2-
C2O42-
MnO4-
C2H3O2CH3COO-
CN-
OH-
ClO2-
ClO-
O22-
S2O32-
ClO4-
ClO3-