Chapter 5
Honors Chemistry 1
Wilmington High School
Section 5.1: Simple Ions and Ionization
Write the electron configuration for each of the following atoms or ions:
1) Oxygen
2) O2-
3) Magnesium
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2+
4) Mg
5) Ne
6) Chlorine
7) Cl-
8) Potassium
9) K+
10) Argon
Cations and Anions:
In general, metals tend to _____________ electrons and nonmetals tend to _______________ electons.
A cation is an ion that has_____________ electrons. An anion is an ion that has _____________ electrons
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Predict the electric charges for the most stable ions of the following atoms:
1) Barium ______
2) Aluminum ______
3) Fluorine ______
4) Carbon ______
5) Potassium ______
Valence Electrons:
What is a valence electron?
Draw a diagram of the following atoms and indicate the valence electrons by either circling them, highlighting
them, or coloring them in a different color:
1) Magnesium
2) Silicon
3) Phosphorus
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4) Bromine
The five questions that follow refer to the image provided below.
1) How many valence electrons do all members of group 16 of the periodic table have?
2) What is the ionic charge for all of the alkali metals?
3) Which group shown above have no ionic charge associated with them?
4) Atoms of group 14 have what ionic charge when they ionize?
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Chapter 5
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5) Predict the ionic charge for each of the ions below:
a. Be ______
b. Li ______
c. B ______
d. N ______
e. H ______
f. S ______
Ions with Noble Gas Configurations
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Chapter 5
Honors Chemistry 1
Wilmington High School
IMPORTANT!!! Ions have the electron configuration of noble gases, but please understand that they still
have a different number of protons in their nucleus (which doesn’t change during ionization), meaning that they
are NOT ACTUALLY NOBLE GASES!!! Having a noble gas electron configuration does NOT mean the atom is
now a noble gas!!!
Fill in the information below for the ions indicated
Ion
Protons
Electrons
2+
Sr
26
24
15
18
16
18
47
45
28
26
IAs3-
K+
Sn4+
S2-
Ion Symbol
Protons
Neutrons
Electrons
80
124
78
26
32
23
48
66
46
108
+
47Ag
211
4+
82Pb
67
2+
30Zn
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Chapter 5
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Transition Metals and Ionization:
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Type 1 cations primarily include the alkali metals, alkaline earth metals, and the aluminum family
o They only form one type of ion…for instance, a calcium atom only ionizes to form a Ca2+ ion
Many transition metals, along with some other heavy metals (e.g., lead), are typically referred to as
“Type 2 Cations”
o These atoms are capable of ionizing into more than one different ion!! For instance, Indium can
ionize into In+, In2+, and even In3+, depending on what it’s forming a compound with!
Type 2 Cations do NOT assume noble gas electron configurations when they ionize
o All of the type 1 cations take on a noble gas electron configuration when they ionize!!!
All transition metals form __________________ (positively charged ions)
Many transition metals are capable of assuming more than one ionic charge (see below)
The table above shows the common transition metals and ionized forms of many atoms. Please note that this
list is NOT the entire collection of all possible ions…these are simply the most common ions for the atoms
shown. For most of the metals shown above, chemists typically use Roman Numerals to indicate the ionic
charge for an ion. Below is a table of some other common type II cations that you will encounter in this class
Ion
Sn4+
Pb4+
Systematic Name
Tin (IV) ion
Lead (IV) ion
***Important note regarding the transition metal ions
Most of the metals that can take on variable charges are transition metals, those which occur from block 3B to
2B. We indicate these charges by using Roman Numerals. However, we typically do NOT use Roman
Numerals for transition metal ions such as Zn2+ or Cd+. If there is any doubt in your mind about whether to
include a Roman Numeral for a transition ion charge, just include the Roman Numeral. It is NEVER WRONG
to do so, even though it might be technically unnecessary in the case of Zn2+, for instance.
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Chapter 5
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Examples: Fill in the table below involving type II cations:
Transition metal Ion
Fe2+
Name of ion (with Roman Numerals)
Fe3+
Copper (I) ion
Copper (II) ion
Platinum (II) ion
Platinum (IV) ion
Au3+
Au+
Cobalt (II)
Cobalt (III)
Re5+
Ag+
Pb2+
Note that in nature, Ag2+ is quite rare, so most chemists do not use a Roman Numeral for the silver ion. Once
again, however, it isn’t technically incorrect to include the charge for silver.
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Chapter 5
Honors Chemistry 1
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Section 5.2: Salts and Ionic Compounds
Ionic Bonding and Ionic Compounds:


Ionic bonds form between ions that have _______________________________
Example: sodium and bromine ions form a salt as shown below:

Salts are electrically neutral ionic compounds
o Examples
 NaCl



LiF
Important!
o Anions aren’t attracted to just _________________________. They form CRYSTALS, and a
single cation is surrounded by anions in a geometrical arrangement. There is a large network of
electrical interactions that makes ionic compounds stable.
Properties of ionic compounds
o Ionic compounds are NOT MOLECULES!!!
 Molecules form when two nonmetals “covalently bond”
o Ionic bonds are extremely strong (due to the electrical interactions between the ions)
o Liquid and dissolved salts conduct electricity (ionic solids do NOT conduct electricity)
o Salts are both _____________ and _______________
A sodium chloride crystal lattice
A more complex ionic crystal lattice
***The crystal lattice (crystal shape) is determined by the size of the ions and the ratio of cations to anions
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Chapter 5
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Please refer to the chart below to answer all questions on this page
1) What evidence in this data table suggests that ionic bonds are extremely strong bonds?
2) Water has a melting point of 0°C and a boiling point of 100°C. Would you classify water as an
“IONIC” or “COVALENT” compound? Why?
3) Which ionic compound listed has the lowest melting point?
4) How many of the ionic compounds listed have negative boiling points?
5) How many of the covalent compounds listed have negative melting points?
6) What factors most likely explain the difference in melting point between MgF2 and CaI2 (both of which
contain 1 cation and 2 anions)
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Chapter 5
Honors Chemistry 1
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Writing ionization equations:



Ionic bonding cannot occur without ions!!! Atoms must ionize!!
Recall that “Ionization energy” is the energy needed to make an atom GIVE UP its electrons! This
usually occurs with atoms in their gaseous form
o Generally, the alkali metals have very low ionization energy…this means that you don’t have to
provide an alkali metal atom with much energy to make it lose its valence electron.
 Alkali metals want to lose an electron because this gives them a stable noble gas electron
configuration!!
Also remember that electron affinity is an atoms tendency to want to GAIN electrons.
o Generally, halogens have very high electron affinity…they want to gain an electron to achieve a
noble gas electron configuration
Write the ionic equation for each of the metals given below:
1) Na
2) K
3) Li
4) Cs
5) Which of the four alkali metals above has the lowest ionization energy? How do you know?
6) How might Mg ionize (hint…it has to give up TWO electrons to reach stability)
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Chapter 5
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Salt formation mechanism:
1) Energy is needed to make solid sodium a gas.
2) Energy is also required to remove an electron from a gaseous sodium atom.
3) Chlorine naturally exists as a “diatomic” molecule containing two chlorine atoms. Energy must be
supplied to separate the chlorine atoms so that they can react with sodium.
4) An electron is added to a chlorine atom to form an anion. This step releases energy.
5) When a cation and anion form an ionic bond, energy is released.
Questions:
1) Steps 1-3 shown above are all ______
a. Exothermic
b. Endothermic
2) Steps 4-5 shown above are extremely ______
a. Exothermic
b. Endothermic
3) Considering the entire mechanism (steps 1-5) for salt formation, this is an ________ process
a. Exothermic
b. Endothermic
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Chapter 5
Honors Chemistry 1
Wilmington High School
The diagram below shows the entire mechanism for the formation of salts. Although this specific example
shows sodium and chlorine forming a salt, it is generalizable for many different ionic substances!
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Chapter 5
Honors Chemistry 1
Wilmington High School
Section 5.3: Polyatomic Ions and Ionic Compounds
Naming common ionic compounds:
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
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

IMPORTANT: Remember that all ionic compounds are compounds that contain positively charged ions
(cations) and negatively charged ions (anions)
Generally, ionic compounds are combinations of metals and nonmetals
You always write the metal first and the nonmetal second
For the NONMETAL ONLY, you drop the ending and add “-ide”
o You do not do this for “polyatomic ions,” which we’ll consider later in this section…you only
follow this rule when a cation forms an ionic compound with a monatomic anion (e.g., F-, N3-,
O2-)
All ionic compounds
must have an overall charge of exactly zero!
Starting simple: Write the empirical formula (simplest formula) of the compounds formed by the ions
given below:
1) H+ and F- ions
2) Na+ and S2- ions
3) Al3+ and Cl- ions
4) Al3+ and O2- ions
5) Ba2+ and N3- ions
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Chapter 5
Honors Chemistry 1
Wilmington High School
Name the following Ionic Compounds:
1) KCl
2) Na2O
3) MgBr2
4) Al2O3
5) AgF
6) CuCl2
7) Fe2O3
8) TiBr3
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Chapter 5
Honors Chemistry 1
Wilmington High School
Write the chemical formula for the following ionic compounds
1) Sodium Iodide
2) Calcium Oxide
3) Barium Chloride
4) Potassium Sulfide
5) Lithium Nitride
6) Magnesium Phosphide
7) Aluminum Sulfide
8) Beryllium Chloride
9) Strontium Nitride
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10) Barium Bromide
11) Calcium Nitride
12) Copper (II) Oxide
13) Iron (III) Fluoride
14) Copper (I) Nitride
15) Manganese (II) Bromide
16) Platinum (IV) Nitride
17) Cobalt (III) Oxide
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18) Mercury (II) Oxide
19) Chromium (III) Sulfide
20) Chromium (III) Fluoride
21) Nickel (II) Phosphide
22) Lead (II) Iodide
23) Tin (II) Nitride
24) Tin (II) Chloride
25) Copper (I) Sulfide
26) Chromium (III) Nitride
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Chapter 5
Honors Chemistry 1
Wilmington High School
Common Polyatomic Ions (Polyatomic = CONTAINS MANY ATOMS)

Just as before, these ions have electric charge. When forming ionic compounds, their charge must
balance with whatever they are forming a compound with!
YOU ARE RESPONSIBLE FOR MEMORIZING ALL OF THESE POLYATOMIC IONS!!!
Others you should commit to memory are listed in the table I’ve created below. These don’t appear as often in
chemistry, but they are extremely important ions!
Ion
O22HPO42SCNS2O32-
Name
peroxide
Hydrogen phosphate
thiocyanate
thiosulfate
Ion
C2O42-
Name
oxalate
Polyatomic ions form ionic compounds just like the simpler ions did before.
You will be using these for the rest of this semester (and the rest of your high school &
college chemistry careers), so I recommend making flashcards and doing significant
practice with all of these polyatomic ions.
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Chapter 5
Honors Chemistry 1
Wilmington High School
Example: Write the empirical formula for the ionic compound formed by the following ions:
1) Li+ and CO32-
2) Al3+ and ClO4-
Name the following ionic compounds. Please do so as I’ve shown below:
1) K2SO4
2K+ and SO42- = Potassium Sulfate
2) Ag2S
3) H2O2
4) Li3PO4
5) CaSO3
6) Ba(OH)2
7) FeCl3
8) NaHCO3
9) AlPO4
10) CrCl3
11) LiMnO4
12) K2C2O4
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Chapter 5
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13) BaCrO4
14) Fe(NO3)3
15) Na2SO4
16) Ba3(PO4)2
17) NaC2H3O2
18) NH4NO2
19) Cu(NO3)2
20) Fe(OH)2
21) CoBr2
22) NH4NO3
23) Cu(ClO4)2
24) SnO2
25) Mn(OH)2
26) Al2(SO3)3
27) Ba(ClO4)2
28) Cr(NO3)3
29) Na2CO3
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Chapter 5
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30) Na2SO3
31) NH4MnO4
32) (NH4)2Cr2O7
33) Pb3(PO4)2
34) ZnHPO4
Write the chemical formulas for the following compounds. Please start by writing the ion and the charge.
I’ve shown you how to do the first one below.
1) Potassium sulfide
K+ and S2- = K2S
2) Potassium sulfate
3) Potassium sulfite
4) Calcium cyanide
5) Copper (II) oxalate
6) Calcium carbonate
7) Nickel (II) Fluoride
8) Ammonium chloride
9) Copper (I) oxide
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Chapter 5
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10) Potassium cyanide
11) Nickel (II) perchlorate
12) Aluminum hydroxide
13) Chromium (III) carbonate
14) Magnesium nitrate
15) Lithium nitride
16) Ammonium acetate
17) Aluminum permanganate
18) Copper (I) thiosulfate
19) Copper (II) thiocyanate
20) Sodium phosphate
21) Magnesium hydrogen carbonate
22) Lithium carbonate
23) Tin (II) dichromate
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Chapter 5
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24) Barium hydroxide
25) Barium acetate
26) Sodium oxalate
27) Ammonium phosphate
28) Manganese (IV) sulfide
29) Manganese (IV) sulfate
30) Zinc Nitrate
31) Iron (III) carbonate
32) Aluminum cyanide
33) Aluminum thiocyanate
34) Magnesium nitride
35) Calcium acetate
36) Cesium perchlorate
37) Iron (II) sulfite
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Chapter 5
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38) Ammonium nitrate
39) Zinc Nitrite
40) Sodium hydroxide
41) Zinc phosphate
42) Copper (II) acetate
43) Potassium hypochlorite
44) Sodium dichromate
45) Mercury (I) Nitrate
46) Manganese (III) thiosulfate
47) Aluminum sulfite
48) Mercury (II) permanganate
49) Strontium acetate
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Chapter 5
Honors Chemistry 1
Wilmington High School
Naming Acids:


Acids are a very important class of hydrogen-containing ionic compounds
Simply put, an acid is composed of an ANION connected to enough H+ cations to totally balance the
anion’s charge!
Examples: Complete the table below
Anion
Number of H+
ions that need
to be added to
neutralize the
anion
Name of the acid
ClSO42NO3ClO4PO43C2H3O2-
For your Chapter 5 Test:
1)
2)
3)
4)
5)
Read all of chapter 5 (pay attention to all visuals and diagrams as well)
Know how to do all examples in this packet, and know all of the information that this packet contains
Complete the book problems
Review all of your quizzes and in-class assignments
If you need extra practice with polyatomic ions or writing ionic formulas, please let me know!!! It is a
very important skill to possess, so I strongly recommend you do everything in your power to master
ionic compounds!
6) Because this chapter built strongly on chapter 4, you should also consider reviewing chapter 4 (e.g.,
periodic trends, ionization, etc.)
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