4.1 representing ionic compounds. forming ionic compounds ionic compounds are formed when one or...
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Forming Ionic Compounds• Ionic compounds are formed when one or more valence electrons
(electrons in the outer energy level) are transferred from a metal atom to a non-metal atom. – Example: sodium chloride (NaCl)
• they are made up of positive ions (cations) and negative ions (anions) that are attracted to each other.
• the two oppositely charged ions are attracted to each other by a force called an ionic bond.
The Periodic Table and Valence Electrons
•Each column is called a “group”
Except for He, it has 2 electrons
•Octet Rule: The loss and gain of electrons allows each atom to form a full outer energy level of electrons and, therefore, become stable (with the same number of electrons as the closest noble gas)•Scientists often refer to this arrangement as a stable octet.
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Ionic structure / properties• Ionic compounds are solids at SATP. In
their solid form they form ionic crystals. These are more commonly known as salts.
• high melting and boiling points
• many are brittle
• when ionic compounds are dissolved in water, they dissociate into their ions and the solutions conduct electricity. – NaCl(s) Na+
(aq) + Cl-(aq)
Types of Ionic Compounds…Binary Ionic Compounds: composed of only 2 different elements (a metal cation and a non-metal anion)
some binary ionic compounds contain a multivalent metal – these have more than one ion charge (listed in the periodic table)
Ternary Ionic Compound: composed of 3 different elements (one of the ions is polyatomic – made up of more than one element)
Naming Binary Ionic Compounds…
Binary Ionic Compounds
1.The metal ion is always written first and keeps its whole name
1.The non-metal is written second and has a slight change, the ending (suffix) is changed to –ide
-example: Na2S – sodium sulfide
Writing Formulas for Binary Ionic Compounds…
-example: magnesium chlorideStep 1: Write the symbols with the metal first
Mg Cl
Step 2: Write the ionic charge above each symbol to indicate the stable ion that each element forms
2+ 1-Mg Cl
Step 3: Determine how many ions of each type you need so that the total ionic charge is zero
One Mg2+ ion will balance the charge of two Cl- ions(2+) + 2(1-) = 0
Step 4: Write the formula using subscripts to indicate the number of ions of each type MgCl2
Binary Ionic Compounds
Writing Formulas for Binary Ionic Compounds…
-example: lithium oxideStep 1: Write the symbols with the metal first
Li O
Step 2: Write the ionic charge above each symbol to indicate the stable ion that each element forms
1+ 2-Li O
Step 3: Determine how many ions of each type you need so that the total ionic charge is zero
Two Li1+ ions will balance the charge of one O- ion2(1+) + (2-) = 0
Step 4: Write the formula using subscripts to indicate the number of ions of each type Li2O
The Cross-Over Method
-example: lithium oxideStep 1: Write the symbols with the metal first
Li O
Step 2: Cross-Over Rule – Write the ionic charge above each symbol andcross over the amount of charge.
1+ 2-Li O
The formula is Li2O
The Cross-Over Method
-example: calcium oxideStep 1: Write the symbols with the metal first
Ca O
Step 2: Cross-Over Rule – Write the ionic charge above each symbol andcross over the amount of charge
2+ 2-Ca O
The formula is Ca2O2
Step 3: Reduce the Chemical Formula - Dividing by common factor of 2, we get:
CaO
The Zero-Sum RuleThe sum of all the charges in the chemical formula of the compound MUST EQUAL ZERO.
Example: Al2S3
Ratio of 2 Al atoms : 3 S atoms
Al cation +3 charge S anion -2 charge
2(+3) + 3(-2) = ZERO! Al S
Naming Binary Ionic Compounds having Multivalent Metals…
Binary Ionic Compounds
-example: FeSStep 1: Identify the metal
Iron (Fe)
Step 2: Verify that the metal can form more than one kind of ion by checking the periodic table.
2+ 3+Fe and Fe
Step 3: Determine the ratio of the ions in the chemical formula 1 iron : 1 sulfide
Step 4: Note the charge of the anion 2-
-example: FeSStep 5: The positive and negative charges must balance out so that the net charge is 0.
Total negative charge: 2-Total positive charge: 2+
Step 6: Determine what charge the metal ion must have to balance the anion.
1(Fe ?) = 2+Therefore, the charge on the iron must be 2+.
Step 7: Write the name of the metal ion – include a roman numeral to show which charge the ion has in brackets, after the name. See Table 4.5 on pg. 147.
The name of the metal ion is iron(II)
Step 8: Write the name of the compound.iron(II) sulfide
Naming Ionic Compounds having Multivalent Metals…
Binary Ionic Compounds
-example: Fe2S3
Step 1: Identify the Metal
Iron (Fe)
Step 2: Verify that the metal can form more than one kind of ion by checking the periodic table
2+ 3+Fe and Fe
Step 3: Determine the ratio of the ions in the chemical formula 2 iron : 3 sulfide
Step 4: Note the charge of the anion 2-
-example: Fe2S3
Step 5: The positive and negative charges must balance out so that the net charge is 0.
Total negative charge: 6- (3 X 2-)Total positive charge: 6+
Step 6: Determine what charge the metal ion must have to balance the anion.2(Fe ?) = 6+
Therefore, the charge on the iron must be 3+.
Step 7: Write the name of the metal ion – include a roman numeral to show which charge the ion has in brackets after the name.
The name of the metal ion is iron(III)
Step 8: Write the name of the compound.iron(III) sulfide
Writing Formulas for Binary Ionic Compounds having Multivalent Metals…
Binary Ionic Compounds
-example: tin(IV) sulfideStep 1: Write the symbols with the metal first
Sn S
Step 2: Cross-Over Rule – Write the ionic charge above each symbol andcross over the amount of charge
4+ 2-Sn S
The formula is Sn2S4
Step 3: Reduce the Chemical Formula - Dividing by common factor of 2, we get:
SnS2
• naming compounds with polyatomic ions is similar to naming other ionic compounds
• You should note that compounds with polyatomic ions have names ending in -ate or –ite, not -ide
• Note that most are negative, except ammonium, NH4
+ (see table 4.7 on pg. 148)
• Name Ca(OH)2, CuSO4, NH4NO3, Co2(CO3)3
Ternary Ionic Compounds:Ionic Compounds with Polyatomic Ions
- calcium hydroxide
- copper(II) sulfate
- ammonium nitrate
- cobalt(III) carbonate
Ca(OH)2
CuSO4
NH4NO3
Co2(CO3)3
Answers
Ionic Compounds with Polyatomic Ions
Most Common Polyatomic IonsOne extra oxygen"per-____-ate"
Common/NormalJust memorize this one and you’ll know the rest
One less oxygen”-ite"
Two less oxygens"hypo-____-ite"
NO41-
pernitrate
NO31-
nitrate
NO21-
nitrite
NO1-
hyponitrite
CO42-
percarbonate
CO32-
carbonate
CO22-
carbonite
CO2-
hypocarbonite
ClO41-
perchlorate
ClO31-
chlorate
ClO21-
chlorite
ClO1-
hypochlorite
SO52-
persulfate
SO42-
sulfate
SO32-
sulfite
SO22-
hyposulfite
PO53-
perphosphate
PO43-
phosphate
PO33-
phosphite
PO23-
hypophosphite
Writing Formulas …
-example: aluminum carbonateStep 1: Using the periodic table and a table of common polyatomic ions,
identify each ion and its charge.
Aluminum: Al3+
Carbonate: CO32-
Step 2: Cross-Over Rule – Cross over the amount of charge.
3+ 2-Al CO3
Step 3: Use subscripts to show the ratio of ions. Place the polyatomic ion in brackets, if it needs a subscript.
Al2(CO3)3
Ionic Compounds with Polyatomic ions
Writing Formulas …
-example: ammonium sulfateStep 1: Using the periodic table and a table of common polyatomic ions,
identify each ion and its charge.
Ammonium: NH4 +
Sulfate: SO4 2-
Step 2: Cross-Over Rule – Cross over the amount of charge.
1+ 2-NH4
SO4
Step 3: Use subscripts to show the ratio of ions. Place the polyatomic ion in brackets, if it needs a subscript.
(NH4)2SO4
Ionic Compounds with Polyatomic ions