Ionic Compounds Notes with added notes from class.notebook November 08, 2016
Ionic Compoundsand
Ionic Bonding
Table of Contents: Ionic Compounds and Ionic BondingClick on the topic to go to that section
• Periodic Table Review
• Valence Electrons and the Octet Rule• Ions• Ionic Bonding
• Predicting an Ionic Compound's Formula
• Naming Ionic Compounds
• Properties of Ionic Compounds
• Formulas and Names of Ionic Compounds with Transition Metals
• Polyatomic ions• Formula and Names of Compounds with Polyatomic ions (Ternary Ionic Compounds)
• Polyatomic Patterns
Ionic Compounds Notes with added notes from class.notebook November 08, 2016
Periodic Table Review
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Periodic Table Review
The periodic table is "periodic" because of certain trends that are seen in the elements.
Some of these trends are atomic size, ionization energy, electronegativity and metallic character.
Elements from the same family/group have similar chemical properties because of their similar electron configuration.
Ionic Compounds Notes with added notes from class.notebook November 08, 2016
The Periodic Table of the Elements
As
BSi
TeGe
Sb?
The periodic table can be divided into three large classifications of elements.
What type of elements are highlighted in blue, in yellow and in pink? What is unique about the elements that are highlighted in pink?
As
BSi
TeGe
Sb?
More metallic Less metallic Nonmetallic
Most metallic
Metallic Character of the ElementsWhen comparing elements in a period (row) , elements on the left generally have a "weaker" pull on their electrons due to the fewer protons in the nucleus.
The weaker the pull on electrons, the more easily the electrons are lost, and the greater the metallic character of the element.
Ionic Compounds Notes with added notes from class.notebook November 08, 2016
As
BSi
TeGe
Sb?
More metallic Less metallic Nonmetallic
Most metallic
Metallic Character of the ElementsAs one moves down a column in the periodic table, atoms become larger due to more filled orbitals. The larger the atom, the farther the outer electrons are from the nucleus, and the easier it is for the atom to lose those electrons.
The easier it is to lose electrons, the more metallic the element.
1 Elements __________ exhibit similar physical and chemical properties.
A with similar chemical symbolsB with similar atomic masses
C in the same period of the periodic table
D on opposite sides of the periodic table
E in the same group of the periodic table
Answer
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2 Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties?
A Li, NaB Cs, BaC Ca, SiD Ga, GeE C, O
Answer
3 Which of the following is a nonmetal?
A WB SrC OsD IrE S
Answer
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4 Potassium is a __________ and chlorine is a __________.
A metal, nonmetalB metal, metalC metal, metalloidD metalloid, nonmetalE nonmetal, metal A
nswer
#. Which element from each pair is more metallic?
Sodium or Sulfur?
Calcium or Francium?
Magnesium or Fluorine?
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Valence Electrons and the Octet Rule
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Octet Rule: Atoms will gain, lose, or share electrons in order to have complete outer shells of electrons (This gives the atom stability).
A full outer shell in most atoms will contain 8 electrons:2 electrons in the s subshell and6 electrons in the p subshell ( s2p6 configuration)
Small atoms, like Li, Be, and B, will lose electrons to have a full s2 configuration. This is called a duet.
Octet Rule
Which elements on the periodic table have a complete outer shell? What is true about these elements relative chemical reactivity?
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Valence Electrons
Valence electrons are the electrons in the highest occupied energy level of an element’s atoms.
The valence electrons determine the chemical properties of an element. Why do you think this would be true?
Atoms in group 3 have 3 valence electrons, atoms in group 17 have 7 valence electrons, etc.
Valenceelectron
To find the number of valence electrons in an atom of a representative element (elements found in the s and p blocks), simply look at its group number.
Valence Electrons
1 2 3 4 5 6 7 8
1 4
There is one exception: helium has only 2 valence electrons.
Number of valence electrons in neutral atoms:
Ionic Compounds Notes with added notes from class.notebook November 08, 2016
Valence Electrons
Lithium 1s22s1 has 1 valence electron in its outermost,
n=2, energy level.
Oxygen 1s22s22p4 has 6 valence electrons
5 How many valence electrons does potassium have?
A 3
B 1
C
D 4
19
Answer
E 8
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6 How many valence electrons does Aluminum have?
A 5
B 7
C 3D 27
E 13
Answer
7 How many valence electrons does Barium have?
A 1
B 2
C 52
D 3
Answer
E 6
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8 Arsenic (As) has 6 valence electrons.
True
False
Answer
Ions
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Cations are positive and are formed by elements on the left side of the periodic chart (metals).
Ions
Anions are negative and are formed by elements on the right side of the periodic
chart (nonmetals).
Ions are atoms or groups of atoms that have become charged by either gaining or losing electrons.
The Formation of CationsMetals usually give up/lose valence electrons to become
more stable.
This results in a noble gas electron configuration (usually 8 electrons, but 2 in the case of He) in their now outermost shell.
How many electrons does the Na+ ion have?
Na : 1s2 2s2 2p6 3s1 Na +1 : 1s2 2s2 2p6
Loss of valence electrons
Ne atom
1s
2s
2p
3s
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The Formation of Cations
Na atom Na+ ion
loses e
11p11e
11p10e
The Na+ ion is smaller than the Na atom. Do you remember what factors cause this reduction in size?
Cations of Group 1A elements always lose 1 electron and have a charge of 1+.
Cations of Group 2A elements always lose 2 electrons and have a charge of 2+.
The Formation of Cations
Mg Mg2+ 2e+
Mg atom(electricallyneutral,
charge = 0)
Mg ion(+2 indicates 2 units of positive
charge)
(2 in front of e indicates 2 units
of negative charge)
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Nonmetals usually gain valence electrons. This results in a noble gas configuration of 8 electrons in their outer shell
The Formation of Anions
How many electrons does the Cl have?
Cl 1s22s22p63s23p5 Cl 1s22s22p63s23p6 Ar atom
2s
2p
3s
3p
The Formation of Anions
Cl atom Cl ion
Gains an e17P17e
17p18e
Single anions are named with a shortened element name and an "ide" ending. Cl is named chloride.
Ionic Compounds Notes with added notes from class.notebook November 08, 2016
The Formation of Anions
Anions of Group 15 elements always gain 3 electrons and have a charge of 3
Anions of Group 16 elements always gain 2 electrons and have a charge of 2
Anions of Group 17 elements always gain 1 electron and have a charge of 1
Consider Group 14 elements, what common charge(s) would you predict for these elements?
Formation of Ions and Metallic Character
The more metallic an element, the easier it loses electrons, resulting in the formation of cations.
The less metallic an element, the greater the hold on electrons, and the less likely they are to form cations.
Ionic Compounds Notes with added notes from class.notebook November 08, 2016
Ion Symbols
To write the symbol for an ion, write the symbol of the element and show the ion charge as a superscript, with the number value first followed by the + or sign.
Ex: Ca2+
When an ion has a charge of 1+ or 1, it is not necessary to put the 1 in the ion symbol, just the + or sign.
Ex: F1 may simply be written F.
9 Metals tend to __________ electrons and nonmetals tend to __________ electrons. A gain, gainB lose, loseC gain, loseD lose, gainE neither, they keep their electrons
Answer
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10 Anions tend to be __________ and cations tend to be __________.
A metals, metalsB nonmetals, nonmetals
C metals, nonmetals
D nonmetals, metalsE metalloids, metalloids
Answer
11 Metals lose electrons to form cations
True
False
Answer
True
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12 Anions are formed from nonmetals
True
False
Answer
13 Nonmetals tend to lose electrons forming ions
True
False Answer
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14 This is the ion formed from a calcium atom
A Ca+
B Ca2+
C Ca
D Ca2
Answer
15 Phosphorous forms an ion with a charge of __________. A 1+B 2
C 3+
D 3
E 2+
Answer
D
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16 Aluminum forms an ion with a charge of __________.
A 2+
B 1
C 3+
D 2
E 0 Answer
17 Of the following, __________ contains the greatest number of electrons.
A P3+
B PC P2
D P3
E P2+
Answer
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18 Oxygen forms an ion with a charge of __________. A 2
B 2+
C 3
D 3+
E 6+
Answer
19 Iodine forms an ion with a charge of __________. A 7
B 1+
C 2
D 2+
E 1
Answer
Ionic Compounds Notes with added notes from class.notebook November 08, 2016
20 This is the ion formed from nitrogen
A N
B N2
C N3+
D N3
Answer
21 Predict the charge of the most stable ion of S? A 3+B 1C 6+D 2+E 2
Answer
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22 What would be the expected charge on the gallium (Ga) ion?A +1B +2C +3D +13E 5
Answer
Ionic Compounds Notes with added notes from class.notebook November 08, 2016
Ionic Bonding
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Ionic Compounds Notes with added notes from class.notebook November 08, 2016
Introduction to Chemical Bonds
Ionic The electrostatic ( positive to negative) attraction between ions
Covalent The sharing of electrons between atoms
Metallic Each metal atom bonds to other metals atoms within a "sea" of electrons (covered in a later unit)
There are three basic types of bonds:
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ElectronegativityElectronegativity is how strongly an atom attracts electrons from a neighboring atom.
Electronegativity
Electronegativity increases left to right across the periodic table, and decreases as you move down a column. Flourine is the most electronegative element.
Francium is the least electronegative element.
Ionic Compounds Notes with added notes from class.notebook November 08, 2016
Atoms with a high electronegativity will be able to attract electrons away from atoms with a much lower electronegativity.
This removal of electrons can occur when the difference in electronegativity between the two atoms is approximately 1.7 or higher.
Once a positive and negative ion are formed, they will be attracted to each other via the electrostatic force.
Ionic Bonding
Ionic Bonding
Neutral atom
7 valence electrons
High Electronegativity
+ Cation Anion
Neutral atom
1 valence electron
Low Electronegativity
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Ionic Bonding
The atom with high electronegativy attracts valence electrons from the atom with lower electronegativity.
Generally when a metal reacts with a nonmetal, the metal loses electrons to form a cation and the nonmetal gains electrons to form an anion.
When the atoms become oppositely charged ions the electrostatic force of attraction brings them together.
Electrostatic force of attraction = bond
+ Cation Anion
Compounds composed of cations and anions are called ionic compounds.
Although they are composed of ions, ionic compounds are electrically neutral since the electrons being lost by the metal are the same electrons being gained by the nonmetal.
The electrostatic forces that hold ions together in ionic compounds are called ionic bonds.
Ionic Bonding
Ionic Compounds Notes with added notes from class.notebook November 08, 2016
Na Cl
Ionic BondsThe electron transfer process in creating an ionic bond:
The dots represents the valence electrons in an atom.
click here for an animation of this reaction
An electronegativity difference of approximately 1.7 can only occur between a metal and a nonmetal.
Ionic Bonding
Ionic Compounds Notes with added notes from class.notebook November 08, 2016
23 Which pair of atoms will form an ionic bond?
A Li and NeB K and BrC K and CsD S and Cl
Answer
24 Which pair of atoms will form an ionic bond?
A Li and BeB Na and MgC K and CaD Na and Cl
Answer
Ionic Compounds Notes with added notes from class.notebook November 08, 2016
25 An ionic bond would form between Sc and F?
True
False
Answer
True
26 Which of the following compounds would you expect to be ionic?
A H2OB CO2
C SrCl2D SO2
E H2S
Answer
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Properties of Ionic Compounds
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Properties of Ionic Compounds
1. They are crystalline solids at room temperature The cations and anions are arranged in a repeating
geometric pattern.
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2. They have high melting points due to the strength of the ionic bonds.
3. They conduct electricity when melted (molten) or dissolved in water (aqueous) due to the ability of the ions to move around.
Properties of Ionic Compounds
A chemical formula shows the kinds and numbers of atoms in the smallest representative unit of a substance.
A formula unit is the lowest wholenumber ratio of ions in an ionic compound. This is also called the empirical formula.
Formula Units
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Chemical formulas
Chemical formulas are written using the chemical symbol followed by a subscript indicating the number of that atom or ion.
NaCl indicates a ratio of 1 Na+ : 1 Cl
H2O indicates a ratio of 2 H : 1 O
Predicting an Ionic Compound's Formula
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Ionic Compounds Notes with added notes from class.notebook November 08, 2016
Predicting an Ionic Compound FormulaPotassium (K) with an electronegativity of 0.8 and oxygen (O) with an electronegativity of 3.5 will form an ionic compound.
What is the formula for an ionic compound of potassium and oxygen?
KO
K
How many additional valence electrons does oxygen need? 2
How many valence electrons does potassium have? 1
How many potassium atoms will it take to give oxygen the electrons it needs? 2
The formula unit is K2O
The metal is always first in the formula, followed by the nonmetal.
Predicting an Ionic Compound Formula
What is the formula for an ionic compound of Mg and N?
How many additional valence electrons does N need? 3
How many valence electrons does Mg have to offer? 2
How many Mg atoms will it take to give how many N the electrons it needs? (Find the lowest common multiplier first.)
MgN
NMg
Mg
3 Mg : 2 N
The formula unit is Mg3N2
Ionic Compounds Notes with added notes from class.notebook November 08, 2016
MgN
NMg
Mg
Ionic compounds are neutral
As you can see in the diagram, all electrons lost by a Mg must be taken by a N.
This causes the total positive charge (electrons lost) to be equal to the total negative charge (electrons gained).
Example: Write the formula for calcium sulfide.
Step 1: Identify the cation & write its common ion
Calcium is in group 2: Ca2+
Step 2: Identify the anion & write its formula
Sulfur is in group 6: S2
Step 3: Only one cation and one anion are needed to make a neutral compound.
Step 4: The formula is written CaS
Predicting an Ionic Compound Formula
Ionic Compounds Notes with added notes from class.notebook November 08, 2016
27 The formula for barium sulfide is Ba2S2 .
True
False
Answer
28 The formula for the ionic compound between Mg and S is:
A Mg2S2
B MgS
C MgS2
D SMg
E I don't know how to do this.
Answer
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29 The formula for the ionic compound between Cs and O is:
A CsO2
B OCs2C Cs2O
D OCs2
E I don't know how to do this. Answer
30 The ionic compound formed between Ca and N is:
A CaN
B Ca2N2
C Ca3N2
D Ca2N3
E I don't know how to do this.
Answer
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31 The ionic compound formed between Al and O
A Al3O2
B Al2O3
C AlO
D Al2O2
E I don't know how to do this. Answer
32 What is the ionic compound formed between Ca and Al?
A CaAl
B Ca3Al2C Al2Ca3
D No compound is formed.
Answer
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33 What is the ionic compound formed between P and Br?
A P3Br
B BrP
C This compound is not considered ionic
D (BrP)2E I don't know how to do this.
Answer
34 What is the formula for sodium phosphide?
A SP3
B NaP
C Na3P
D NaP3
E I don't know how to do this. Answer
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35 What is the formula for strontium bromide?
A SrBr
B SrBr2
C Sr2Br
D BrSr2
Answer
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Naming Ionic Compounds
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Naming Binary Ionic Compounds Cations
Charge Formula Name
+1
+2
+3
H+ Li+ K+ Cs+ Ag+
Mg2+ Ca2+ Ba2+ Cd2+
Al3+
Hydrogen ionLithium ionPotassium ionCesium ionSilver ion
Magnesium ion Calcium ion Barium ion Cadmium ion
Aluminum ion
Many cations have the same name as the original, neutral atom.
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All monoatomic anions end in "ide".
Nitride N3
Phosphide P3
Oxide O2
Sulfide S2
Fluoride F
Chloride Cl
Bromide Br
Iodide I
Group 15 Group 16 Group 17
Naming Binary Ionic Compounds Anions
Binary (twoelement) compounds are named by writing the name of the cation followed by the name of the anion.
The name of the cation is the same as the metal name.
The name of the anion is the name of the nonmetal with the suffix changed to ide.
Naming Binary Ionic Compounds
Examples:
NaCl = sodium chlorideKI = potassium iodideLi2S = lithium sulfide
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36 The correct name for Na2S is
A Sodium sulfateB Sodium sulfideC Disodium sulfideD Sulfur nitride
Answer
37 The correct name for SrO is __________.
A strontium oxide B strontium hydroxide C strontium peroxide D strontium monoxide E strontium dioxide
Answer
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38 The correct name for Al2O3 is __________.
A aluminum trioxide B dialuminum oxide C dialuminum trioxide D aluminum oxide E aluminum hydroxide
Answer
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Names and Formulas of Ionic Compounds with Transition Metals
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Recall that sblock metals and some p block elements like aluminum have only one possible ionic charge, based on the Octet Rule.
However, most transition metals (d block elements) can form more than one type of cation with different charge.
Sn, Pb from the pblock are called posttransition metals and will form more than one type of ion and behave like transition metals.
Cations formed by Transition Elements
Cations formed by Transition Elements
The 2+ charge is very common among the transition metals since they lose their two "s" electrons first, before losing others from their "d" orbital.
http://philschatz.com/chemistrybook/contents/m51186.html
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Cations Formed by Transition ElementsOnly common transition metals are shown.
Silver, cadmium and zinc only form one cation, Ag+ , Cd2+ and Zn2+
Note the two mercury cations, one is a single atom, the other is made up of two atoms together this is called a polyatomic ion.
Silver, Zinc, and Cadmium IonsWhy do these ions only have one possible charge?
Let's look at their electron configurations.
The "d" orbital of both zinc and cadmium are full and therefore very stable so the only electrons it will lose are the two "s" electrons...
Zn: [Ar]4s23d10 Zn2+: [Ar]3d10
The "d" orbital is also full with silver as it has largely taken an electron from it's own "s" orbital to make stabilize the "d" orbital. Therefore, it only has 1 electron left to lose.
Ag: [Kr]5s14d10 Ag+ : [Kr]4d10
Ionic Compounds Notes with added notes from class.notebook November 08, 2016
Cations formed by Transition ElementsWe will use the Stock naming system. The name of the transition metal MUST be followed by Roman Numerals indicating its charge.
Formula Name
Cu+1 Copper (I) ion
Co+2 Cobalt (II) ionFe+2 Iron (II) ionMn+2 Manganese (II) ionPb+2 lead (II) ion
Cr+3 Chromium (III) ionFe+3 Iron (III) ion
What would be the names of Cu 2+ and Mn 7+?
Writing Formulas with Transition Metals
The charge on the cation is indicated by the Roman numeral, as shown in this example.
Fe2O3
Reduce if necessary.
Write ion formulas.
Determine ratio of cations to anions.
Fe3+ O2
Iron (III) oxide
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Writing Formulas with Transition Metals
The charge on the cation is indicated by the Roman numeral, as shown in this example.
Tin (IV) oxide
Write ion formulas.
Determine ratio of cations to anions.
Reduce if necessary.SnO2
Sn2O4
Sn4+ O2
39 Which metal is capable of forming more than one cation?
A KB CsC BaD AlE Sn
Answer
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40 Which metal is not capable of forming more than one cation?
A Cu
B Au
C Fe
D Sn
E Al
Answer
Naming a Compound with a Transition Metal
In order to correctly name a formula containing a transition metal, it is necessary to first determine the charge on the cation.
Since all compounds are neutral, the total positive cation charge must equal the total negative anion charge AND since anion charges don't vary, we can use this formula to find the charge on the transition metal.
Total cation charge + Total anion charge = 0
(charge of cation) (# of cations) + (charge of anion) (# of anions) = 0
Ionic Compounds Notes with added notes from class.notebook November 08, 2016
Example Formula with Transition Metals
In the case of FeCl3 , we know there is 1 Fe and 3 Cl, and the charge on Chloride is always 1.
Fill in these values and solve for the charge on Fe.
(charge of cation) (# of cations) +(charge of anion) (# of anions) = 0
(x) (1) + (1) (3) = 0
So x = 3 and the cation is Fe3+ .The compound is Iron (III) Cloride
Formulas with Transition Metals
Cr1 O1
Cr2+ O2
CrO: Determine the charge of O.
Since O has charge of 2, Cr must have a charge of 2+
Cr2O2
Chromium (II) Oxide
Here's another practice problem.
Ionic Compounds Notes with added notes from class.notebook November 08, 2016
41 The correct name of the compound V2O3
is vanadium(II)oxide.
True
False
Answer
42 The correct name for Cu3N is:
A copper nitrideB copper (I) nitrideC copper (II) nitrideD copper(III)nitrideE copper(III) nitrogen
Answer
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43 The name of FeCl3 is
A iron chlorideB iron (II) chlorideC iron (III) chlorideD iron(I)chloride
Answer
44 The correct formula for tin (IV) oxide is:
A SnO2B SnOC Sn4O4D Sn4O2
Answer
A
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45 The formula for copper (II) sulfide is
A CuS2
B CuS C Cu2 S2
D (CuS)2
Answer
E Cu2S
46 Which one of the following compounds is copper(I) chloride?
A CuCl
B CuCl2C Cu2ClD Cu2Cl2E Cu3Cl2 A
nswer
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47 The charge on the cation in the salt Fe2O3 is __________.
A 1+B 2+
C 3+
D 5
E 6 Answer
48 What is the charge on zirconium ion in ZrO2 ?
A 2+
B 4+
C 1+D 2
[*]
E 3+
Answer
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Polyatomic Ions
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A polyatomic ion is a group of atoms bonded together that have a charge and acts like a single unit or ion. They are commonly part of an ionic compound, as either the cation or the anion.
Sulfate = (SO4)2
Nitrate = (NO3)
Carbonate = (CO3)2
When writing formulas for compounds containing polyatomic ions, use ( ) to keep the atoms together.
Do not change the subscripts inside the "( )"
Polyatomic Ions
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Most of the polyatomic ions contain oxygen atoms.
Many anions names end with “ite” or “ate”
In “ite/ate” pairs, the ion with fewer oxygen atoms will have the “ite” ending
Examples: sulfite /sulfate nitrite /nitrate
Note that the suffix does not indicate the actual number of O atoms.
Polyatomic Ions
Ionic Compounds Notes with added notes from class.notebook November 08, 2016
Polyatomic Ions
Familiarize yourself with the polyatomic ions on your reference sheetBe careful of ide, ite, and ate!
H+ = proton or hydrogen ion
or bicarbonate
]
.
Formulas and Names of Ionic Compounds with
Polyatomic Ions (Ternary Ionic Compounds)
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Writing Formulas for Ternary Ionic Compounds
Ternary ionic compounds, compounds that contain 3 or more elements, are neutral, just like binary ionic compounds. Therefore, the goal is to find the lowest ratio of cations to anions that will yield a neutral compound.
This ratio is represented in a formula unit.
Examples of formula units
CaCO3 Zn(C2H3O2 )2
AgNO3 Na2SO3
Writing Formulas for Ternary Ionic Compounds
To write a formula
Example: Write the formula for lithium phosphate.
Step 1: Identify the cation & write its formula
Lithium is in group 1 > Li+
Step 2: Identify the anion & write its formula
Phosphate is a polyatomic ion > PO43
Step 3: Find the ratio of cation to polyatomic anion
Li3(PO4)1 or simply Li3(PO4)
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Writing Formulas for Ternary Ionic Compounds
Example 1: Write the formula for
lithium chlorate.
Li+1 (ClO3)1
= Li(ClO3)
= LiClO3
Note: The ( ) are removed because only 1 chlorate ion is present.
Example 2: Write the formula for manganese(III) carbonate.
Mn3+ (CO3)2
= Mn2(CO3)3
Note: The ( ) are needed here because more than one carbonate ion are present
Move for AnswerMove for Answer
49 The formula for aluminum phosphate is:
A AlPO4
B Al3 (PO4 )
C Al2 (PO4 )3
D Al3 (PO4 )3
Answer
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50 What would be the correct formula for cobalt(III) carbonate?
A Co3CO3B Co2CO3
C Co2(CO3)3D Co3(CO3)2E CoCO3
Answer
51 The formula for sodium hydroxide is
A Na (OH)2 B NaOH
C Na(OH2 ) D Na(HO)
E NaOH2
Answer
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52 The formula for calcium sulfate is
A CaSO4 B Ca2 (SO4 )2C Ca(SO3 ) D Ca2 (SO3 )2
E CaS
Answer
53 How many nitrate ions are present in the formula of aluminum nitrate? (Write the formula first to find out.)
A 1B 2C 3D 4E 5
Answer
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54 How many total ions (cations and anions) are present in the formula of lithium acetate?
A 1B 2C 3D 4E 5
Answer
Writing Formulas for Ionic CompoundsComplete the table by filling in the formula for the ionic compound formed by each pair of cations and anions, as shown for the first pair.
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Write the formula for the following compounds:
1. Magnesium iodide MgI2
2. Calcium sulfite CaSO3
3. Barium hydrogen carbonate Ba(HCO3)2
4. Iron (III) phosphate FePO4
Writing Formulas for Ternary Ionic Compounds
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Ternary ionic compounds contain three or more different elements due to the presence of polyatomic ion(s).
Just as in binary ionic compounds, the name of the cation is given first, followed by the name of the anion.
Names of ternary compounds often end in ite or ate.Examples
CaCO3 calcium carbonate Zn(C2H3O2 )2 zinc acetateAgNO3 silver nitrateNa2SO3 sodium sulfite
Naming Ternary Ionic Compounds
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Ionic Compounds Notes with added notes from class.notebook November 08, 2016
55 The correct name for NaClO is
A sodium chlorate
B sodium chloride
C sodium chlorite
D sodium chloride oxide
E sodium hypochlorite
Answer
56 Mg(HCO3 )2 is
A Magnesium carbonate
B Magnesium hydrogen carbonate
C Magnesium hydroxide
D Magnesium carboxide E Magnesium dibicarbonate A
nswer
Ionic Compounds Notes with added notes from class.notebook November 08, 2016
57 Ammonium carbonate is
A NH4CO3
B (NH4 )2CO3
C NH4 (CO3 )2
D (NH4 )2CO2
Answer
Naming Ternary Ionic CompoundsIf the formula involves a transition or post transition element, you must first deduce the charge so it can be included in the name.
For example: Name Cu2CO3
1. Determine the charge of the polyatmoic anion CO3, which is 2
Cu2 (CO3)2
2. Determine the charge of the cation, Cu carries a +1 charge
This compound is called copper(I) carbonate
Ionic Compounds Notes with added notes from class.notebook November 08, 2016
58 What is the name for Ga2(SO3)3?
A gallium sulfite
B gallium (I) sulfiteC gallium (III) sulfiteD gallium (III) sulfate
Answer
59 Which is the name for AuF3?
A gold (I) flourideB gold(III) flourideC gold flourideD gold flourineE gold triflouride
Answer
Ionic Compounds Notes with added notes from class.notebook November 08, 2016
60 What is the name for Sn(CO3)2?
A tin carbonateB tin(II) carbonateC tin carbideD tin tetracarbonateE tin (IV) carbonate
Answer
E
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