1 chapter 4 some types of chemical reactions. 2 chapter four goals 1. the periodic table: metals,...
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CHAPTER 4
Some Types of Chemical Reactions
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Chapter Four Goals1. The Periodic Table: Metals, Nonmetals, and Metalloids2. Aqueous Solutions: An Introduction3. Reactions in Aqueous Solutions4. Oxidation Numbers
Naming Some Inorganic Compounds5. Naming Binary Compounds6. Naming Ternary Acids and Their Salts
Classifying Chemical Reactions7. Oxidation-Reduction Reactions: An Introduction8. Combination Reactions9. Decomposition Reactions10. Displacement Reactions11. Metathesis Reactions 12. Summary of Reaction Types13. Synthesis Question
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The Periodic Table: Metals, Nonmetals, and Metalloids
1869 - Mendeleev & Meyer Discovered the periodic law
• The properties of the elements are periodic functions of their atomic numbers.
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The Periodic Table: Metals, Nonmetals, and Metalloids
Groups or families Vertical group of elements on periodic table Similar chemical and physical properties
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The Periodic Table: Metals, Nonmetals, and Metalloids Period
Horizontal group of elements on periodic table Transition from metals to nonmetals
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The Periodic Table: Metals, Nonmetals, and Metalloids
Some chemical properties of metals1. Outer shells contain few electrons2. Form cations by losing electrons3. Form ionic compounds with nonmetals4. Solid state characterized by metallic
bonding
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The Periodic Table: Metals, Nonmetals, and Metalloids
Group IA metals Li, Na, K, Rb, Cs, Fr
One example of a periodic trend The reactions with water of Li
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The Periodic Table: Metals, Nonmetals, and Metalloids
Group IA metals Li, Na, K, Rb, Cs, Fr
One example of a periodic trend The reactions with water of Li, Na
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The Periodic Table: Metals, Nonmetals, and Metalloids
Group IA metals Li, Na, K, Rb, Cs, Fr
One example of a periodic trend The reactions with water of Li, Na, & K
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The Periodic Table: Metals, Nonmetals, and Metalloids
Group IIA metals alkaline earth metals
Be, Mg, Ca, Sr, Ba, Ra
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The Periodic Table: Metals, Nonmetals, and Metalloids
Some chemical properties of nonmetals1. Outer shells contain four or more electrons2. Form anions by gaining electrons3. Form ionic compounds with metals and covalent
compounds with other nonmetals4. Form covalently bonded molecules; noble gases
are monatomic
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The Periodic Table: Metals, Nonmetals, and Metalloids
Group VIIA nonmetals halogens F, Cl, Br, I, At
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The Periodic Table: Metals, Nonmetals, and Metalloids
Group VIA nonmetals O, S, Se, Te
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The Periodic Table: Metals, Nonmetals, and Metalloids
Group 0 nonmetals noble, inert or rare gases He, Ne, Ar, Kr, Xe, Rn
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The Periodic Table: Metals, Nonmetals, and Metalloids
Stair step function on periodic table separates metals from nonmetals.
Metals are to the left of stair step. Approximately 80% of
the elements Best metals are on the
far left of the table.
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The Periodic Table: Metals, Nonmetals, and Metalloids
Stair step function on periodic table separates metals from nonmetals.
Nonmetals are to the right of stair step. Approximately 20% of
the elements Best nonmetals are on
the far right of the table.
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The Periodic Table: Metals, Nonmetals, and Metalloids
Stair step function on periodic table separates metals from nonmetals.
Metalloids have one side of the box on the stair step.
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The Periodic Table: Metals, Nonmetals, and Metalloids
Periodic trends in metallic character
PeriodicChart
More MetallicMoreMetallic
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Aqueous Solutions: An Introduction
1. Electrolytes and Extent of Ionization Aqueous solutions consist of a solute
dissolved in water. Classification of solutes:
Nonelectrolytes – solutes that do not conduct electricity in water
Examples: C2H5OH - ethanol
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Aqueous Solutions: An Introduction
C6H12O6 - glucose (blood sugar)
C
OC
C
C C
C
H
H
OH
H OH
OH
H
OH
OH H
H
H
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Aqueous Solutions: An Introduction
C12H22O11 - sucrose (table sugar)
C
OC
C
C C
CH2
H
H
OH
H
OH
OH
HO
H
OH
C C
C
O
C
CH2
H
OH
H
H
OH
CH2
OH
OH
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Aqueous Solutions: An Introduction The reason nonelectrolytes do not
conduct electricity is because they do not form ions in solution.
• ions conduct electricity in solution
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Aqueous Solutions: An Introduction Classification of solutes
strong electrolytes - conduct electricity extremely well in dilute aqueous solutions
Examples of strong electrolytes1. HCl, HNO3, etc.
• strong soluble acids
2. NaOH, KOH, etc.• strong soluble bases
3. NaCl, KBr, etc.• soluble ionic salts• ionize in water essentially 100%
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Aqueous Solutions: An Introduction Classification of solutes
weak electrolytes - conduct electricity poorly in dilute aqueous solutions
1. CH3COOH, (COOH)2 • weak acids
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Aqueous Solutions: An Introduction
2. NH3, Fe(OH)3 • weak bases
3. some soluble covalent salts• ionize in water much less than 100%
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Aqueous Solutions: An Introduction
2. Strong and Weak Acids Acids are substances that generate
H+ in aqueous solutions. Strong acids ionize 100% in water.
-aqaq
%100g Cl H HCl
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Aqueous Solutions: An Introduction
2. Strong and Weak Acids Acids are substances that generate
H+ in aqueous solutions. Strong acids ionize 100% in water.
-
aq3aqOH
3
-aq3aq3
100%2 3
NO + H HNO
or
NO + OH OH HNO
2
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Aqueous Solutions: An Introduction
Some Strong Acids and Their Anions Formula Name1. HCl hydrochloric acid2. HBr hydrobromic acid3. HI hydroiodic acid4. HNO3 nitric acid
5. H2SO4 sulfuric acid
6. HClO3 chloric acid
7. HClO4 perchloric acid
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Aqueous Solutions: An Introduction
Some Strong Acids and Their Anions Acid Anion Name1. HCl Cl- chloride ion2. HBr Br- bromide ion3. HI I- iodide ion4. HNO3 NO3
- nitrate ion
5. H2SO4 SO42- sulfate ion
6. HClO3 ClO3- chlorate ion
7. HClO4 ClO4- perchlorate ion
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Aqueous Solutions: An Introduction Weak acids ionize significantly less
than 100% in water. Typically ionize 10% or less!
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Aqueous Solutions: An Introduction
Some Common Weak Acids and Their Anions Formula Name1. HF hydrofluoric acid2. CH3COOH acetic acid (vinegar)3. HCN hydrocyanic acid4. HNO2 nitrous acid
5. H2CO3 carbonic acid (soda water)
6. H2SO3 sulfurous acid
7. H3PO4 phosphoric acid
8. (COOH)2 oxalic acid
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Aqueous Solutions: An Introduction
Some Common Weak Acids and Their Anions Acid Anion Name1. HF F- fluoride ion2. CH3COOH CH3COO- acetate ion3. HCN CN- cyanide ion4. HNO2 NO2
- nitrite ion
5. H2CO3 CO32- carbonate ion
6. H2SO3 SO32- sulfite ion
7. H3PO4 PO43- phosphate ion
8. (COOH)2 (COO)22- oxalate ion
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Aqueous Solutions: An Introduction
3. Reversible Reactions CH3COOH acetic acid
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Aqueous Solutions: An Introduction All weak inorganic acids ionize
reversibly or in equilibrium reactions. This is why they ionize less than 100%.
CH3COOH – structure of acetic acid
COH
O
CH3
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Aqueous Solutions: An Introduction Correct chemical symbolism for
equilibrium reactions
aq-aq3
7%
3 H + COOCH COOHCH
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Aqueous Solutions: An Introduction
4. Strong Bases, Insoluble Bases, and Weak Bases
Characteristic of common inorganic bases is that they produce OH- ions in solution.
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Aqueous Solutions: An Introduction
Common Strong Bases Formula Name1. LiOH lithium hydroxide2. NaOH sodium hydroxide3. KOH potassium hydroxide4. RbOH rubidium hydroxide5. CsOH cesium hydroxide6. Ca(OH)2 calcium hydroxide
7. Sr(OH)2 strontium hydroxide
8. Ba(OH)2 barium hydroxide Notice that they are all hydroxides of IA and IIA metals
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Aqueous Solutions: An Introduction Similarly to strong acids, strong
bases ionize 100% in water.
(aq)OH 2 + (aq)Ba Ba(OH)
(aq)OH + (aq)K KOH-+2
2
-+
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Aqueous Solutions: An Introduction Insoluble or sparingly soluble bases
Ionic compounds that are insoluble in water, consequently, not very basic.
Formula Name1. Cu(OH)2 copper (II) hydroxide
2. Fe(OH)2 iron (II) hydroxide
3. Fe(OH)3 iron (III) hydroxide
4. Zn(OH)2 zinc (II) hydroxide
5. Mg(OH)2 magnesium hydroxide
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Aqueous Solutions: An Introduction Weak bases are covalent compounds that
ionize slightly in water. Ammonia is most common weak base
NH3
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Aqueous Solutions: An Introduction Weak bases are covalent
compounds that ionize slightly in water.
Ammonia is most common weak base NH3
-(aq)aq42g3 OH + NH OH + NH
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Aqueous Solutions: An Introduction
5. Solubility Guidelines for Compounds in Aqueous Solutions
It is very important that you know these It is very important that you know these guidelines and how to apply them in reactions.guidelines and how to apply them in reactions.
1) Common inorganic acids and low-molecular-weight organic acids are water soluble.
2) All common compounds of the Group IA metal ions and the ammonium ion are water soluble.
LiLi++, Na Na++, K K++, Rb Rb++, Cs Cs++, and NHNH44++
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Aqueous Solutions: An Introduction3) Common nitrates, acetates, chlorates, and perchlorates are water soluble.
NONO33--, CH CH33COOCOO--, ClO ClO33
--, and ClOClO44--
4) Common chlorides are water soluble. Exceptions – AgClAgCl, Hg Hg22ClCl22, & PbClPbCl22
Common bromides and iodides behave similarly to chlorides. Common fluorides are water soluble.
• Exceptions – MgFMgF22, CaF CaF22, SrF SrF22, BaF BaF22, and PbF PbF22
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Aqueous Solutions: An Introduction5) Common sulfates are water soluble.
Exceptions – PbSO PbSO44, BaSO BaSO44, & HgSO HgSO44
Moderately soluble – CaSO CaSO44, SrSO SrSO44, & Ag Ag22SOSO44
6) Common metal hydroxides are water insolubleinsoluble. Exceptions – LiOH, NaOH, KOH, RbOH LiOH, NaOH, KOH, RbOH & CsOH CsOH Common bromides and iodides behave similarly to chlorides. Common fluorides are water soluble.
• Exceptions – MgFMgF22, CaF, CaF22, SrF, SrF22, BaF, BaF22, and , and PbF PbF22
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Aqueous Solutions: An Introduction7) Common carbonates, phosphates, and arsenates are water insolubleinsoluble.
COCO332-2-, PO PO44
3-3-, & AsO AsO443-3-
Exceptions- IA metals IA metals and NH NH44++ plus
Ca to BaCa to Ba Moderately soluble – MgCO MgCO33
8) Common sulfides are water insolubleinsoluble. Exceptions – IA metals IA metals and NH NH44
++ plus IIA metalsIIA metals
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Reactions in Aqueous Solutions
Symbolic representation of what is happening at the laboratory and molecular levels in aqueous solutions. Copper reacting with silver nitrate.
Laboratory level
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Reactions in Aqueous Solutions
Symbolic representation of what is happening at the laboratory and molecular levels in aqueous solutions. Copper reacting with silver nitrate.
Symbolic representation
s2(aq)3aq3s Ag 2)Cu(NOAgNO 2Cu
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Reactions in Aqueous Solutions
Another example of aqueous reactions. Sodium chloride reacting with silver
nitrate. Laboratory level
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Reactions in Aqueous Solutions
Another example of aqueous reactions. Sodium chloride reacting with silver
nitrate. Symbolic representation
aq3saqaq3 NaNOAgClNaCl AgNO
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Reactions in Aqueous Solutions
There are three ways to write reactions in aqueous solutions.
1. Molecular equation Show all reactants & products in molecular or
ionic form
2. Total ionic equation Show the ions and molecules as they exist in solution
(s)(aq)4(aq)4(s) Cu + ZnSO CuSO + Zn
(s)-2aq4
2aq
-2aq4
2aq(s) Cu +SO+ ZnSO+ Cu+Zn
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Reactions in Aqueous Solutions
3. Net ionic equation Shows ions that participate in reaction
and removes spectator ions. Spectator ions do not participate in
the reaction.
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Reactions in Aqueous Solutions Look in total ionic equation for species that
do not change from reactant to product. Spectator ions in < >’s.
Net ionic equation
(s)-2aq4
2aq
-2aq4
2aq(s) Cu +SO+ ZnSO+ Cu+Zn
(s)2aq
2aq(s) Cu + ZnCu + Zn
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Reactions in Aqueous Solutions
In the total and net ionic equations the only common substances that should be written as ions are:
a. Strong acidsb. Strong basesc. Soluble ionic salts
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Oxidation Numbers Guidelines for assigning oxidation
numbers.1. The oxidation number of any free, uncombined
element is zero.2. The oxidation number of an element in a simple
(monatomic) ion is the charge on the ion.3. In the formula for any compound, the sum of the
oxidation numbers of all elements in the compound is zero.
4. In a polyatomic ion, the sum of the oxidation numbers of the constituent elements is equal to the charge on the ion.
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Oxidation Numbers5. Fluorine has an oxidation number of –1 in its
compounds.6. Hydrogen, H, has an oxidation number of +1
unless it is combined with metals, where it has the oxidation number -1.
Examples – LiH, BaH2
7. Oxygen usually has the oxidation number -2. Exceptions: In peroxides O has oxidation number of –1.
• Examples - H2O2, CaO2, Na2O2
In OF2 O has oxidation number of +2.
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Oxidation Numbers8. Use the periodic table to help with
assigning oxidation numbers of other elements.
a. IA metals have oxidation numbers of +1.b. IIA metals have oxidation numbers of +2.c. IIIA metals have oxidation numbers of +3.
• There are a few rare exceptions.d. VA elements have oxidation numbers of –3 in binary
compounds with H, metals or NH4+.
e. VIA elements below O have oxidation numbers of –2 in binary compounds with H, metals or NH4
+. Summary in Table 4-10.
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Oxidation Numbers Example 4-1: Assign oxidation numbers to
each element in the following compounds: NaNO3 Na = +1 (Rule 8) O = -2 (Rule 7) N = +5
Calculate using rule 3. +1 + 3(-2) + x = 0 x = +5
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Oxidation Numbers K2Sn(OH)6
K = +1 (Rule 8) O = -2 (Rule 7) H = +1 (Rule 6) Sn = +5
Calculate using rule 3. 2(+1) + 6(-2) + 6(+1) + x = 0 x = +5
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Oxidation Numbers
H3PO4
You do it!You do it! H = +1 O = -2 P = +5
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Oxidation Numbers
SO32-
O = -2 (Rule 7) S = +4
Calculate using rule 4. 3(-2) + x = -2 x = +4
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Oxidation Numbers
HCO3-
O = -2 (Rule 7) H = +1 (Rule 6) C = +4
Calculate using rule 4. +1 + 3(-2) + x = -1 x = +4
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Oxidation Numbers
Cr2O72-
You do it!You do it! O = -2 Cr = +6
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Naming Some Inorganic Compounds Binary compounds are made of two
elements. metal + nonmetal = ionic compound nonmetal + nonmetal = covalent compound
Name the more metallic element first. Use the element’s name.
Name the less metallic element second. Add the suffix “ide” to the element’s stem.
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Naming Some Inorganic Compounds Nonmetal StemsNonmetal Stems Element Stem Boron bor Carbon carb Silicon silic Nitrogen nitr Phosphorus phosph Arsenic arsen Antimony antimon
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Naming Some Inorganic Compounds Oxygen ox Sulfur sulf Selenium selen Tellurium tellur Phosphorus phosph Hydrogen hydr
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Naming Some Inorganic Compounds Fluorine fluor Chlorine chlor Bromine brom Iodine iod
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Naming Some Inorganic Compounds
Binary Ionic Compounds Binary Ionic Compounds are made of a metal cation and a nonmetal anion. Cation named first Anion named second
LiBr lithium bromide MgCl2 magnesium chloride
Li2S lithium sulfide
Al2O3 You do it!You do it!
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Naming Some Inorganic Compounds LiBr lithium bromide MgCl2 magnesium chloride Li2S lithium sulfide Al2O3 aluminum oxide
Na3P You do it!You do it!
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Naming Some Inorganic Compounds LiBr lithium bromide MgCl2 magnesium chloride
Li2S lithium sulfide
Al2O3 aluminum oxide
Na3P sodium phosphide
Mg3N2 You do it!You do it!
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Naming Some Inorganic Compounds LiBr lithium bromide MgCl2 magnesium chloride
Li2S lithium sulfide
Al2O3 aluminum oxide
Na3P sodium phosphide
Mg3N2 magnesium nitride Notice that binary ionic compounds with metals
having one oxidation state (representative metals) do not use prefixes or Roman numerals.
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Naming Some Inorganic Compounds Binary ionic compounds Binary ionic compounds
containing metals that exhibit containing metals that exhibit more than one oxidation statemore than one oxidation state
Metals exhibiting multiple oxidation states are:1. most of the transition metals2. metals in groups IIIA (except Al), IVA,
& VA
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Naming Some Inorganic Compounds There are two methods to name these
compounds.1. Older method
add suffix “ic” to element’s Latin name for higher oxidation state
add suffix “ous” to element’s Latin name for lower oxidation state
2. Modern method use Roman numerals in parentheses to
indicate metal’s oxidation state
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Naming Some Inorganic Compounds
Compound Old System Modern System FeBr2 ferrous bromide iron(II) bromide
FeBr3 ferric bromide iron(III) bromide SnO stannous oxide tin(II) oxide SnO2 stannic oxide tin(IV) oxide
TiCl2 You do it!You do it!
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Naming Some Inorganic Compounds
Compound Old System Modern System FeBr2 ferrous bromide iron(II) bromide
FeBr3 ferric bromide iron(III) bromide SnO stannous oxide tin(II) oxide SnO2 stannic oxide tin(IV) oxide
TiCl2 titanous chloride titanium(II) chloride
TiCl3 You do it!You do it!
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Naming Some Inorganic Compounds
Compound Old System Modern System FeBr2 ferrous bromide iron(II) bromide
FeBr3 ferric bromide iron(III) bromide SnO stannous oxide tin(II) oxide SnO2 stannic oxide tin(IV) oxide
TiCl2 titanous chloride titanium(II) chloride
TiCl3 titanic chloride titanium(III) chloride
TiCl4 You do it!You do it!
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Naming Some Inorganic Compounds
Compound Old System Modern System FeBr2 ferrous bromide iron(II) bromide
FeBr3 ferric bromide iron(III) bromide SnO stannous oxide tin(II) oxide SnO2 stannic oxide tin(IV) oxide
TiCl2 titanous chloride titanium(II) chloride
TiCl3 titanic chloride titanium(III) chloride
TiCl4 does not workdoes not work titanium(IV) chloride
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Naming Some Inorganic Compounds
Pseudobinary ionic compoundsPseudobinary ionic compounds There are three polyatomic ions that commonly form
binary ionic compounds.1. OH- hydroxide2. CN- cyanide3. NH4
+ ammonium Use binary ionic compound naming system. KOH potassium hydroxide Ba(OH)2 barium hydroxide Al(OH)3 aluminum hydroxide Fe(OH)2 You do it!You do it!
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Naming Some Inorganic Compounds KOH potassium hydroxide Ba(OH)2 barium hydroxide
Al(OH)3 aluminum hydroxide
Fe(OH)2 iron (II) hydroxide
Fe(OH)3 You do it!You do it!
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Naming Some Inorganic Compounds KOH potassium hydroxide Ba(OH)2 barium hydroxide
Al(OH)3 aluminum hydroxide
Fe(OH)2 iron (II) hydroxide
Fe(OH)3 iron (III) hydroxide
Ba(CN)2 You do it!You do it!
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Naming Some Inorganic Compounds KOH potassium hydroxide Ba(OH)2 barium hydroxide
Al(OH)3 aluminum hydroxide
Fe(OH)2 iron (II) hydroxide
Fe(OH)3 iron (III) hydroxide
Ba(CN)2 barium cyanide
(NH4)2S You do it!You do it!
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Naming Some Inorganic Compounds KOH potassium hydroxide Ba(OH)2 barium hydroxide Al(OH)3 aluminum hydroxide Fe(OH)2 iron (II) hydroxide Fe(OH)3 iron (III) hydroxide Ba(CN)2 barium cyanide (NH4)2S ammonium sulfide NH4CN You do it!You do it!
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Naming Some Inorganic Compounds KOH potassium hydroxide Ba(OH)2 barium hydroxide Al(OH)3 aluminum hydroxide Fe(OH)2 iron (II) hydroxide Fe(OH)3 iron (III) hydroxide Ba(CN)2 barium cyanide (NH4)2S ammonium sulfide NH4CN ammonium cyanide
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Naming Some Inorganic Compounds Binary Acids Binary Acids are binary compounds
consisting of hydrogen and a nonmetal. Compounds are usually gases at room
temperature and pressure. Nomenclature for the gaseous compounds is
hydrogen (stem)ide. When the compounds are dissolved in
water they form acidic solutions. Nomenclature for the acidic solutions is hydro (stem)ic acid.
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Naming Some Inorganic Compounds
Formula Name Aqueous Solution
HF hydrogen fluoride hydrofluoric acid HCl hydrogen chloride hydrochloric acid HBr hydrogen bromide hydrobromic acid H2S You do it!You do it!
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Naming Some Inorganic Compounds
Formula Name Aqueous solution HF hydrogen fluoride hydrofluoric acid HCl hydrogen chloride hydrochloric acid HBr hydrogen bromide hydrobromic acid H2S hydrogen sulfide hydrosulfuric acid
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Naming Some Inorganic Compounds
Binary covalent molecular Binary covalent molecular compounds composed of two compounds composed of two nonmetals other than hydrogennonmetals other than hydrogen Nomenclature must include prefixes that
specify the number of atoms of each element in the compound.
Use the minimum number of prefixes necessary to specify the compound. Frequently drop the prefix mono-.
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Naming Some Inorganic Compounds Formula Name CO carbon monoxide CO2 carbon dioxide
SO3 sulfur trioxide
OF2 oxygen difluoride
P4O6 You do it!You do it!
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Naming Some Inorganic Compounds Formula Name CO carbon monoxide CO2 carbon dioxide
SO3 sulfur trioxide
OF2 oxygen difluoride
P4O6 tetraphosphorus hexoxide
P4O10 You do it!You do it!
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Naming Some Inorganic Compounds Formula Name CO carbon monoxide CO2 carbon dioxide
SO3 sulfur trioxide
OF2 oxygen difluoride
P4O6 tetraphosphorus hexoxide
P4O10 tetraphosphorus decoxide
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Naming Some Inorganic Compounds
The oxides of nitrogen illustrate why covalent compounds need prefixes and ionic compounds do not.
Formula Old Name Modern Name N2O nitrous oxide dinitrogen monoxide NO nitric oxide nitrogen monoxide N2O3 nitrogen trioxide dinitrogen trioxide
NO2 nitrogen dioxide nitrogen dioxide
N2O4 nitrogen tetroxide dinitrogen tetroxide
N2O5 nitrogen pentoxide dinitrogen pentoxide
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Naming Some Inorganic Compounds
Ternary Acids and Their Salts Ternary Acids and Their Salts are made of three elements. The elements are H, O, & a nonmetal.
Two of the compounds are chosen as the basis for the nomenclature system. Higher oxidation state for nonmetal is named (stem)ic
acid. Lower oxidation state for nonmetal is named
(stem)ous acid Salts are named based on the acids.
Anions of -ic acids make “ate” salts. Anions of -ous acids make “ite” salts.
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Naming Some Inorganic Compounds
Names and Formulas of the Common “ic” acids Naming these compounds will be easier if you have this list
memorized. Group Name Formula IIIA boric acid H3BO3
IVA carbonic acid H2CO3
silicic acid H4SiO4
VA nitric acid HNO3
phosphoric acid H3PO4
arsenic acid H3AsO4
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Naming Some Inorganic Compounds
VIA sulfuric acid H2SO4
selenic acid H2SeO4
telluric acid H6TeO6
VIIA chloric acid HClO3
bromic acid HBrO3
iodic acid HIO3
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Naming Some Inorganic Compounds Salts are formed by the reaction of the
acid with a strong base. Acid Salt HNO2 NaNO2
nitrous acid sodium nitrite HNO3 NaNO3
nitric acid sodium nitrate H2SO3 Na2SO3
sulfurous acid sodium sulfite
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Naming Some Inorganic Compounds Acid Na Salt H2SO4 You do it!You do it!
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Naming Some Inorganic Compounds Acid Na salt H2SO4 Na2SO4
sulfuric acid sodium sulfate
HClO2 You do it!You do it!
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Naming Some Inorganic Compounds Acid Na salt H2SO4 Na2SO4
sulfuric acid sodium sulfate
HClO2 NaClO2
chlorous acid sodium chlorite
HClO3 You do it!You do it!
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Naming Some Inorganic Compounds Acid Na salt H2SO4 Na2SO4
sulfuric acid sodium sulfate
HClO2 NaClO2
chlorous acid sodium chlorite
HClO3 NaClO3
chloric acid sodium chlorate
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Naming Some Inorganic Compounds There are two other possible acid and salt
combinations. Acids that have a higher oxidation state than
the “ic” acid are given the prefix “per”. These acids and salts will have one more O atom
than the “ic” acid. Acids that have a lower oxidation state than
the “ous” acid are given the prefix “hypo”. These acids and salts will have one less O atom
than the “ic” acid.
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Naming Some Inorganic Compounds Illustrate this series of acids and salts with the Cl
ternary acids and salts. Acid Na Salt HClO NaClO
hypochlorous acid sodium hypochlorite HClO2 NaClO2
chlorous acid sodium chlorite HClO3 NaClO3
chloric acid sodium chlorate HClO4 NaClO4
perchloric acid sodium perchlorate
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Naming Some Inorganic Compounds
Acidic SaltsAcidic Salts are made from ternary acids that retain one or more of their acidic hydrogen atoms. Made from acid base reactions where there is
an insufficient amount of base to react with all of the hydrogen atoms.
Old system used the prefix “bi”“bi” to denote the hydrogen atom.
Modern system uses prefixes and the word hydrogen.
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Naming Some Inorganic Compounds
NaHCO3 Old system sodium bicarbonate Modern system sodium hydrogen carbonate
KHSO4 Old system potassium bisulfate Modern system potassium hydrogen sulfate
KH2PO4
Old system potassium bis biphosphate Modern system potassium dihydrogen phosphate
K2HPO4 You do it!You do it!
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Naming Some Inorganic Compounds
K2HPO4 Old system potassium biphosphateModern system potassium hydrogen phosphate
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Naming SomeInorganic Compounds Basic SaltsBasic Salts are analogous to acidic salts.
The salts have one or more basic hydroxides remaining in the compound.
Basic salts are formed by acid-base reactions with insufficient amounts of the acid to react with all of the hydroxide ions.
Use prefixes to indicate the number of hydroxide groups.
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Naming SomeInorganic Compounds Ca(OH)Cl
calcium monohydroxy chloride
Al(OH)Cl2 aluminum monohydroxy chloride
Al(OH)2Cl You do it!You do it! aluminum dihydroxy chloride
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Oxidation-Reduction Reactions: An Introduction Oxidation is an increase in the
oxidation number. Corresponds to the loss of electrons.
Reduction is a decrease in the oxidation number. Good mnemonic – reduction reduces
the oxidation number. Corresponds to the gain of electrons
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Oxidation-Reduction Reactions: An Introduction
Oxidizing agents are chemical species that:1. oxidize some other substance2. contain atoms that are reduced 3. gain electrons
Reducing agents are chemical species that:1. reduce some other substance 2. contain atoms that are oxidized3. lose electrons
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Oxidation-Reduction Reactions: An Introduction
Two examples of oxidation-reduction or redox reactions.
KMnO4 and Fe2+
Fe2+ is oxidized to Fe3+
MnO41- is reduced to Mn2+
Combustion reactions are redox reactions Combustion of Mg
Mg is oxidized to MgO O2 is reduced to O2-
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Oxidation-Reduction Reactions: An Introduction
Example 4-2: Write and balance the formula unit, total ionic, and net ionic equations for the oxidation of sulfurous acid to sulfuric acid by oxygen in acidic aqueous solution.
Formula unit equation
Total ionic equationYou do it!You do it!
aq42g2aq32 SO H2 O SO H2
2
4(aq)(aq)g2aq32 SO 2 H 4 O SOH 2
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Oxidation-Reduction Reactions: An Introduction Net ionic equation
You do it!You do it!
Which species are oxidized and reduced? Identify the oxidizing and reducing agents.
You do it!You do it!
2
4(aq)(aq)g2aq32 SO 2 H 4 O SOH 2
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Oxidation-Reduction Reactions: An Introduction H2SO3 is oxidized.
The oxidation state of S in H2SO3 is +4.
In SO42-, S has an oxidation state of +6.
O2 is reduced. Oxidation state of O in O2 is 0
In SO42-, O has an oxidation state of –2.
H2SO3 is reducing agent.
O2 is oxidizing agent.
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Combination Reactions Combination reactions occur when two
or more substances combine to form a compound.
There are three basic types of combination reactions.
1. Two elements react to form a new compound
2. An element and a compound react to form one new compound
3. Two compounds react to form one compound
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Combination Reactions
1. Element + Element CompoundA. Metal + Nonmetal Binary Ionic Compound
sg2s NaCl 2ClNa 2
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Combination Reactions
1. Element + Element CompoundA. Metal + Nonmetal Binary Ionic Compound
sg2s MgO 2OMg 2
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Combination Reactions
1. Element + Element CompoundA. Metal + Nonmetal Binary Ionic Compound
s32s AlBr 2 Br3Al 2
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Combination Reactions
1. Element + Element CompoundB. Nonmetal + Nonmetal Covalent Binary
Compound
s104g2s4 O PO 5P
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Combination Reactions
1. Element + Element CompoundB. Nonmetal + Nonmetal Covalent Binary
Compound
3g2s4 PCl4 Cl 6P
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Combination Reactions
1. Element + Element CompoundB. Nonmetal + Nonmetal Covalent Binary
Compound• Can control which product is made with the
reaction conditions.
chlorine limitedin
AsCl 2 Cl 3As 2 s3g2s
chlorine excessin
AsCl 2 Cl 5As 2 s5g2s
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Combination Reactions
1. Element + Element CompoundB. Nonmetal + Nonmetal Covalent Binary
Compound• Can control which product is made with
the reaction conditions.
fluorine limitedin
SeF F 2Se s4g2s
fluorine excessin
SeF F 3Se g6g2s
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Combination Reactions
2. Compound + Element Compound
s5g2s3 AsClClAsCl
g6g2s4 SFFSF
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Combination Reactions
The reaction of oxygen with oxides of nonmetals is an example of this type of combination reaction.
g3 &catalyst
g2g2 SO 2OSO 2
g2g2g COOCO
104264 OPO 2OP
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Combination Reactions
3. Compound + Compound Compound gaseous ammonia and hydrogen chloride
lithium oxide and sulfur dioxide
s4gg3 ClNH HClNH
3222 SO LiSOOLi
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Decomposition Reactions Decomposition reactions occur
when one compound decomposes to form:
1. Two elements2. One or more elements and one or
more compounds3. Two or more compounds
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Decomposition Reactions
1. Compound Element + Element decomposition of dinitrogen oxide
decomposition of calcium chloride
g2g2g2 ON 2ON 2
g2yelectricit
2 ClCaCaCl
2sh
s BAg 2AgBr 2 r
decomposition of silver halides
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Decomposition Reactions
2. Compound One Element + Compound(s)
decomposition of hydrogen peroxide
g22or Mn or Feνh
aq22 OO H2O H23
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Decomposition Reactions
3. Compound Compound + Compound decomposition of ammonium hydrogen
carbonate
g2g2g3s34 COO HNHHCONH
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Displacement Reactions Displacement reactionsDisplacement reactions occur
when one element displaces another element from a compound. These are redox reactions in which the
more active metal displaces the less active metal of hydrogen from a compound in aqueous solution.
Activity series is given in Table 4-14.
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Displacement Reactions1. [More Active Metal + Salt of Less Active Metal]
[Less Active Metal + Salt of More Active Metal] molecular equation
(s)aq3(s) aq3 Ag CuNO Cu +AgNO
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Displacement Reactions Total ionic equation
You do it!You do it!
Net ionic equationYou do it!You do it!
(s)-
aq3aqs-
aq3aq Ag NO+CuCu +NO+ Ag
(s)aq(s)aq Ag Cu Cu +Ag
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Displacement Reactions2. [Active Metal + Nonoxidizing Acid] [Hydrogen +
Salt of Acid] Common method for preparing hydrogen in the laboratory. HNO3 is an oxidizing acid.
Molecular equation
g2aq342aq42(s) H 3 + )(SOAl SO3H + Al 2
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Displacement Reactions Total ionic equation
You do it!You do it!
Net ionic equationYou do it!You do it!
g2-2aq4
3aq
-2aq4aq(s) H 3 + SO 3 + Al 2 SO 3+H 6 + Al 2
g23aqaq(s) H 3 +Al 2 H 6 + Al 2
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Displacement Reactions The following metals are active
enough to displace hydrogen K, Ca, Na, Mg, Al, Zn, Fe, Sn, & Pb
Notice how the reaction changes with an oxidizing acid. Reaction of Cu with HNO3.
• H2 is no longer produced.
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Displacement Reactions3. [Active Nonmetal + Salt of Less Active Nonmetal]
[Less Active Nonmetal + Salt of More Active Nonmetal]
Molecular equation
(aq)s2aqg2 NaCl 2 I NaI 2 + Cl Total ionic equation
You do it!You do it!
-aqaqs2
-aqaqg2 Cl 2 +Na 2 I I 2 + Na 2 +Cl
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Displacement Reactions Net ionic equation
You do it!You do it!
-aqs2
-aqg2 Cl 2 I I 2 +Cl
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Metathesis Reactions Metathesis reactionsMetathesis reactions occur when two
ionic aqueous solutions are mixed and the ions switch partners.
AX + BY AY + BX Metathesis reactions remove ions from
solution in two ways:1. form predominantly unionized molecules like
H2O2. form an insoluble solid
Ion removal is the driving force of metathesis reactions.
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Metathesis Reactions
1. Acid-Base (neutralization) Reactions Formation of the nonelectrolyte H2O acid + base salt + water
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Metathesis Reactions Molecular equation
)(2 (aq)(aq)(aq) OH + KBr KOH + HBr Total ionic equation
You do it!You do it!
)(2-aqaq
-aqaq
-aqaq OH + Br+KOH+K+Br+H
Net ionic equation
You do it!You do it!
)(2-aqaq OH OH +H
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Metathesis Reactions Molecular equation
)(2aq)(23(aq)3(aq)2 OH 2 + )Ca(NOHNO 2 + Ca(OH) Total ionic equation
You do it!You do it! )(2
-aq3
2aq
-aq3aq
-aq
2aq OH 2 +NO 2+ CaNO 2+ H 2+OH 2+Ca
Net ionic equation
You do it!You do it!
)(2aq-aq
)(2aq-aq
OH H+OH
betteror
OH 2 H 2+OH 2
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Metathesis Reactions
2.2. Precipitation reactionsPrecipitation reactions are metathesis reactions in which an insoluble compound is formed.
The solid precipitates out of the solution much like rain or snow precipitates out of the air.
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Metathesis Reactions Precipitation Reactions Molecular equation
(s)3)aq(3aq)(32(aq)23 CaCO +KNO 2 COK + )Ca(NO Total ionic reaction
You do it!You do it!
s3-
aq3aq
-2aq3aq
-aq3
2aq
CaCO NO 2K 2
COK 2 NO 2 Ca
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Metathesis Reactions Net ionic reaction
You do it!You do it!
(s)3-2aq3
2aq CaCO CO +Ca
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Metathesis Reactions Molecular equation
2(s)43)aq(aq)(43(aq)2 POCa +NaCl 6 PONa 2 + CaCl 3
Total ionic reactionYou do it!You do it!
s243-1aq
1aq
-3aq4
1aq
-1aq
2aq
POCa +Cl 6 Na 6
PO2 Na 6 + Cl 6 Ca 3
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Metathesis Reactions Net ionic reaction
You do it!You do it!
s243-3aq4
2aq POCa PO2 Ca 3
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Metathesis Reactions Molecular equation
g22)aq(aq)(32(aq) SO O H+NaCl 2 SONa + HCl2
Total ionic reactionYou do it!You do it!
g22-1aq
1aq
-2aq3
1aq
-1aq
1aq
SO OH +Cl 2Na 2
SO Na 2 + Cl 2H 2
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Metathesis Reactions Net ionic reaction
You do it!You do it!
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Synthesis Question Barium sulfate is a commonly used
imaging agent for gastrointestinal X-rays. This compound can be prepared by some of the simple reactions described in this chapter. Write a balanced aqueous reaction for the production of barium sulfate. You can choose any aqueous starting materials that will form barium sulfate!
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Synthesis Question
Find two aqueous soluble compounds that have Ba in one compound and SO4
2- in the second. When they are mixed, the barium sulfate will precipitate out. One possibility is:
)s(4(aq))aq(422(aq) BaSO + NaCl 2 SONa +BaCl
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Group Activity Pretend that you are one of our lab TA’s
and that you have been given the assignment to prepare unknowns for a qualitative analysis experiment. In a single solution you must have the following ions: Bi3+, Cd2+, and Cu2+. You must make this solution using three different anions. What three compounds would you choose to make this solution so that no precipitate forms?
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End of Chapter 4