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Chamras Chemistry 110 Lecture Exam 2 Materials

Chapter 5

A Brief Detour on the Development of the Periodic Table of Elements

In Ancient Chinese Philosophy: In Greek Philosophy: Dmitri Mendeleev’s Original Periodic Table: (Based on Average Atomic Mass)

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Chemical Nomenclature A brief review on the Periodic Table:

• The Periodic Table: Lists all the elements that are so far known to us. • Most of the elements are naturally occurring but some are human-made. • Metals and non-metals are separated by the zigzag line starting at B(boron), and ending

At(astatine). • With the exception of aluminum (Al), all the elements touching the metal-non-metal

separation line are called metalloids or semi-metals. • Metals lose electrons (become cations) and non-metals gain electrons (become anions)

when ionized. • Metals of Groups 1, 2, and 13 assume charges of +1, +2, and +3 respectively, when

ionized. • Non-metals of groups 15, 16, and 17, assume charges of –3, –2, and –1 respectively,

when ionized. • When formulating an ionic compound, the Principle of Neutrality applies.

Compound: Definition: Chemical Bonding: Ionic Bonding: Covalent Bonding: Types of Compounds: Ionic Compounds:

Molecular Compounds:

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Review Exercise: Determine the formulas for ionic compounds made with the following ions:

a) Al3+ and O2–: _________ b) Ca2+ and P3–: _________

c) Li+ and Cl–: _________

d) Fe2+ and N3–: _________

Charges of Ions:

Simple Cations with Fixed Charges

H

Li

Na

K

Rb

Cs

Fr

Be

Mg

Ca

Sr

Ba

Ra

Zn

Ag

Al

Cd

Simple Cations with Variable Charges

Cr Mn Fe Co Ni Cu

Au Hg Pb

Sn

Bi

Sb

As

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Chemical Nomenclature: IUPAC: Types of Naming:

a) Ionic Compounds b) Binary Molecular Compounds c) Acids d) Bases

How to tell these types apart by just looking at the formula? Formula Indicator Example Ionic------------ Molecular------ Acid------------ Base------------

Simple AnionsH

N O F

P S Cl

Br

I

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Naming Ions: 1. Cations with fixed charge: {Name of Neutral Element + “ion”} Example: 2. Cations with variable charge: Two methods: a) {Name of Neutral Element + Charge + “ion”} Example: b) {Latin Rootname of Neutral Element + “ous” for lower charge, and “ic” for higher charge + “ion”} Simple Anions: {Rootname of element + “ide”} Example: Naming Ionic Compounds:

Element Name Lower Charge Ion

Name Higher Charge Ion

Name

Cr chromium Cr2+ chromous Cr3+ chromic Mn manganese Mn2+ manganous Mn3+ manganic Fe ferrum Fe2+ ferrous Fe3+ ferric Co cobalt Co2+ cobaltous Co3+ cobaltic Ni nickel Ni2+ nickelous Ni3+ nickelic Cu cuprum Cu+ cuprous Cu2+ cupric Au aurum Au+ aurous Au3+ auric Hg mercury

(hydrargyrum) Hg22+ [Hg+] mercurous Hg2+ mercuric

Sn Stannum Sn2+ stannous Sn4+ stannic Pb Plumbum Pb2+ plumbous Pb4+ plumbic As arsenicum As3+ arsenous As5+ arsenic Sb antimonium

(stibium) Sb3+ antimonious Sb5+ antimonic

Bi bisemutum Bi3+ bisemutous Bi5+ bisemutic

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1. Naming ionic compounds made of simple (monatomic) cations and anions: {…Remember: Formula for ionic compounds cation-anion sequence} The name follows the same sequence as the formula does: a) If the cation is fixed-charge: {Name of the cation + Name of the anion} Example: b) If the cation is a variable-charge, there are two methods:

1) { Name of element + (Charge of cation indicated in Roman numeral form) + Name of the anion}

Example:

2) { Latin name of cation + “ous” or “ic”+ Name of the anion} Example:

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Practice problems for writing names and formulas: Complete the following Table: Chemical Formula IUPAC Name Chem. Formula IUPAC Name Na3P potassium chloride

CaO aurous nitride

FeN (two ways) barium fluoride

manganic oxide

Fe3N2 (two ways) chromium (III) phosphide

iron(II) iodide

HgCl2 cuprous nitride

Al2S3 silver oxide

MgBr2 aluminum bromide

SnO2 copper(I) phosphide

2. Naming ionic compounds made of simple cations and polyatomic anions: Polyatomic Ions: Ions made of more than one atom.

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List of Polyatomic Ions

The Only Polyatomic Cation: NH4

+ ammonium ion Hg22+ mercury(I) or mercurous ion Polyatomic anions:

Charge –1 Charge –2 Charge –3 H2PO4– dihydrogen phosphate HPO42– monohydrogen phosphate PO43– phosphate H2PO3– dihydrogen phosphite HPO32– monohydrogen phosphite PO33– phosphite HCO3– bicarbonate CO32– carbonate (hydrogen carbonate) HSO4– bisulfate SO42– sulfate (hydrogen sulfate) HSO3– bisulfite SO32– sulfite (hydrogen sulfite) NO3– nitrate O22– peroxide NO2– nitrite CrO42– chromate C2H3O2– acetate Cr2O72– dichromate BrO4 – perbromate C2O42– oxalate BrO3– bromate BrO2– bromite BrO – hypobromite CN– cyanide OCN– cyanate SCN– thiocyanate MnO4– permanganate OH– hydroxide

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Practice problems for writing names and formulas: Complete the following table: Chemical Formula IUPAC Name Chem. Formula IUPAC Name Na3PO4 potassium chlorate

CaO2 aurous nitrite

Fe(NO2)2 (two ways) barium perbromate

manganic peroxide

Fe(NO3)3 (two ways) mercury (I) phosphite

iron(II) hypoiodite

Hg2Cl2 cuprous sulfate

Al2(SO4)3 silver oxalate

Mg(BrO2)2 aluminum acetate

Sn(CO3)2 copper(II) permanganate

Naming Binary Molecular Compounds: …Remember: Molecular compounds are made of non-metals. Rules:

1. Naming takes the form: {(# prefix + name of the first element) + (# prefix + name of the second ion)}

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2. The number of each type of element must be specified using Latin prefixes (see table below).

3. The only exception is the first element. If there is only one of the first written element in the formula, then the number should not be specified.

Latin Number Prefixes:

Practice problems for naming binary molecular compounds: Complete the following table:

IUPAC Name Chemical Formula dichloro pentaphosphide CO2 N2O4 dinitrogen monoxide NO Naming Acids: Definition of Acids:

Prefix Meaning Prefix Meaning mono- one hexa- six di- two hepta- seven tri- three octa- eight tetra- four nona- nine penta- five deca- ten

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There are two methods of naming the acids:

a) Binary Acids:

{ “hydro” + rootname of the second element + “ic acid”} Example: HBr(aq)

b) Oxy-Acids: { rootname of the non-oxygen, non-hydrogen element + “ic acid” (with higher

# of oxygens OR “ous acid” with lower # of oxygens} Examples: HBrO3(aq) HBrO2(aq) ***If the formula of the acid is displayed without the (aq) solution indicator, then name it as an ionic compound (name the hydrogen as a cation) uniformly, regardless of the type being binary or oxy-acid. Examples: HBr HBrO3 HBrO2 Practice problems for naming acids: Complete the following table:

IUPAC Name Chemical Formula hydrobromic acid HClO4(aq) HClO3 hydrogen nitrite HNO2(aq) hypoiodous acid hydrogen sulfide H3PO4

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Naming Bases: Definition for bases: Bases should be named as ionic compounds. Examples: NaOH KOH LiOH Ca(OH)2 Ba(OH)2 NH4OH Nomenclature Exercise: Complete the following naming tables:

Name Formula Name Formula barium nitrate H2SO4(aq)

dichloro pentoxide AlI3 mercurous peroxide Hg3(PO4)2

bromic acid AuOH ammonium sulfite Ag2O2

hydrogen perchlorate HBrO2 sulfur trioxide Mn(NO2)3

ferric bicarbonate K2O hydroiodic acid NO

periodic acid HCl Naming Hydrates: Hydrate (Definition): Naming:

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Nomenclature Chart:

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Chapter 6

Chemical Reactions What Is A Chemical Reaction? Evidences for Chemical Reactions:

1. Formation of solid 2. Formation of Gas

3. Evolution or Absorption of Heat (Thermal Energy)

4. Color Change Chemical Equations: A Short Hand Method to Describe Chemical Reactions Example: Solid sodium metal reacts with water and forms aqueous sodium hydroxide and hydrogen gas. Writing Chemical Equations:

• Reactant Side

• Product Side

• Reaction Arrow

• States

• Relative Amounts: Law of Conservation of Mass

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Balancing Chemical Equations

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Chapter 7

Types of Chemical Reactions • Solution:

• Components of Solution:

• Examples of Solutions: SOLVENT SOLUTE Example

• Solubility:

• Rule of Thumb on Solubility:

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• Dissolution Process in Water: a) For SOLUBLE Ionic Compounds:

b) For POLAR Molecular Compounds:

c) For Strong Acids & Bases:

d) For Weak Acids & Bases:

***Dissociation:

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Types of Chemical Reactions

1. Precipitation Reactions: Example: CaCl2(aq) + AgNO3(aq) What happens at the Molecular Level? When is there a NO REACTION case if any? How to Predict the Solubility Behavior of a Product? Use SOLUBILITY RULES ***Solubility Rules for Ionic Compounds:

Behavior Compounds Containing the Ions of… Exception(s) Soluble Group 1 metals & NH4+ None Soluble NO3

- None Soluble Cl-, Br-, I- Ag+, Hg22+, Pb2+ Soluble SO42- Ba2+, Pb2+, Ca2+

Insoluble S2-, CO32-, PO43- Group 1 metals & NH4+ Insoluble OH- Group 1 metals & NH4+, Ca+, Ba2+, Sr2+

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Example: Label the following ionic compounds as S (soluble) or I (insoluble). Na3PO4: AgBr: HgI2: PbCl4: Hg2Cl2: Li2S: BaCO3: Ca(OH)2: Fe(OH)3: 3 Ways to Write Chemical Equations:

1. Complete Molecular Equation:

2. Complete Ionic Equation:

3. Net Ionic Equation: Example:

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2. Neutralization Reactions: (AKA: Acid- Base reactions) MUST KNOW: ACID + BASE

• Acid: Example:

• Base: Example: Strength of Acids & Bases: List of Strong Acids: HCl(aq) HBr(aq) HI(aq) H2SO4(aq) HNO3(aq) HClO4(aq) List of Strong Bases: LiOH NaOH KOH RbOH CsOH Ca(OH)2 Sr(OH)2 Ba(OH)2 Weak Acids: Weak Base:

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How about a hydroxide that is not water-soluble? Exercise:

a) Write the complete balanced molecular equation for the reaction of a solution of sulfuric acid and a solution of potassium hydroxide:

b) Generate the complete ionic equation from part a above:

c) Generate the net ionic equation from part b above:

MUST KNOW: The net ionic equation for the reaction of a strong acid with a strong base:

3. a) Reactions of Metals with Non-metals: (AKA: Oxidation-Reduction) Example:

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Oxidation: Reduction: Oxidation Number: Example: b) Reactions of Oxygen with Non-metals: Example: c) Combustion Reactions: Combustion: Organic Compounds: Example:

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Exercise: Complete and balance the equation for the combustion reaction of pentane (Molecular Formula: C5H12). Other Ways to See and Classify Chemical Reactions:

Combination: Decomposition: Double Displacement: Single Replacement: Combustion: