3-1 CHEM 100, Fall 2013 LA TECH Instructor: Dr. Upali Siriwardane e-mail: [email protected]...

3-1CHEM 100, Fall 2013 LA TECH

Instructor: Dr. Upali Siriwardane

e-mail: [email protected]

Office: CTH 311

Phone 257-4941

Office Hours: M,W, 8:00-9:30 & 11:30-12:30 a.m

Tu,Th,F 8:00 - 10:00 a.m. Or by appointment

Test Dates:

Chemistry 100(02) Fall 2013

September 30, 2013 (Test 1): Chapter 1 & 2

October 21, 2013 (Test 2): Chapter 3 & 4

November 13, 2013 (Test 3) Chapter 5 & 6

November 14, 2013 (Make-up test) comprehensive: Chapters 1-6 9:30-10:45:15 AM, CTH 328


REQUIRED :

Textbook: Principles of Chemistry: A Molecular Approach, 2nd Edition-Nivaldo J. Tro - Pearson Prentice

Hall and also purchase the Mastering Chemistry

Group Homework, Slides and Exam review guides and sample exam questions are available online:

http://moodle.latech.edu/ and follow the course information links.

OPTIONAL :

Study Guide: Chemistry: A Molecular Approach, 2nd Edition-Nivaldo J. Tro 2nd Edition

Student Solutions Manual: Chemistry: A Molecular Approach, 2nd Edition-Nivaldo J. Tro 2nd

Text Book & Resources

http://moodle.latech.edu/


3.1 Hydrogen, Oxygen, and Water……………………………. 78

3.2 Chemical Bonds…………………………………………… 80

3.3 Representing Compounds: Chemical Formulas and Molecular Models.. 82

3.4 An Atomic-Level View of Elements and Compounds…………….. 84

3.5 Ionic Compounds: Formulas and Names…………………… 87

3.6 Molecular Compounds: Formulas and Names……………………… 93

3.7 Formula Mass and the Mole Concept for Compounds………… 97

3.8 Composition of Compounds…………………………….. 100

3.9 Determining a Chemical Formula from Experimental Data……… 105

3.10 Writing and Balancing Chemical Equations…………………… 110

3.11 Organic Compounds………………………. 114

Chapter 3. Molecules, Compounds, and Chemical Equations


Chapter 3. KEY CONCEPTS

• Writing Molecular and Empirical

Formulas (3.3)• Classifying Substances as Atomic

Elements, Molecular Elements, Molecular Compounds, or Ionic Compounds (3.4)

• Writing Formulas for Ionic Compounds (3.5)

• Naming Simple Ionic Compounds (3.5)

• Naming Ionic Compounds Containing Polyatomic Ions (3.5)

• Naming Molecular Compounds (3.6)• Naming Molecular Compounds (3.6)• Naming Acids (3.6)• Calculating Formula Mass (3.7)• Using Formula Mass to Count

Molecules by Weighing (3.7)• Calculating Mass Percent

Composition (3.8)

• Using Mass Percent Composition as a Conversion Factor (3.8)

• Using Chemical Formulas as Conversion Factors (3.8)

• Obtaining an Empirical Formula from Experimental Data (3.9)

• Calculating a Molecular Formula from an Empirical Formula and Molar Mass (3.9)

• Obtaining an Empirical Formula from Combustion Analysis (3.9)

• Balancing Chemical Equations (3.10)


Elements and Compounds Groupings• Atomic elements : – elements whose particles are single atoms (He)• Molecular elements:– elements whose particles are multi-atom molecules (O2)• Molecular compounds: – compounds whose particles are molecules made of only

nonmetals (H2O)• Ionic compounds:– compounds whose particles are cations and anions (NaCl)• Metallic elements – elements whose particles are made up of metal atoms

(Cu)• Metallic compounds (alloy)– compounds whose particles are mixture of metal atoms

(Cu-Zn)


The compound propane contains

individual C3H8 molecules.

The sodium chloride molecule, NaCl,

is composed of an array of

Na+

ions and Cl– ions.

Ionic vs. Molecular Compounds

The platinum, Pt, metal

is composed of an array of

Pt atoms.


Ionic: Complete transfer of 1 or more electrons from one atom to another, usually between a metal and a nonmetal element

Covalent: The sharing of valence electrons shared between nonmetal elements

Metallic: The communal sharing of electrons between metals

*Note: Most molecular bonds are actually somewhere in between covalent and ionic types.

Intramolecular Chemical Bonding Types


Types of CompoundsA) Molecular or Covalent Compounds:

non-metal + non-metal nonmetal oxide or halides: SO2

Organic compounds: C3H8

B) Ionic compounds: Metal + non-metal:a) Type I ionic compound (fixed charge) NaClb) Type II ionic compound

FeCl2 and FeCl3, SnCl2 and SnCl4


Formula of a CompoundFormula are used to represent

elements and compound.

For molecular compounds, formula tell how many of each kind of atom are in a molecule.

For ionic compounds, formula tell the simples ratio of actions and anions.

Formula are used to represent elements and compound.

For molecular compounds, formula tell how many of each kind of atom are in a molecule.

For ionic compounds, formula tell the simples ratio of actions and anions.

Molecular Weight ?

Molecular compounds

Formula Weight?

Ionic compounds


• Ionic compounds

• Molecular compounds(Inorganic & organic)

• Acids and bases

• Hydrated compounds

Nomenclatuere: Naming Compounds


Formation of Ionic Compound, NaCl


Ionic Compounds

Characteristics of compounds with ionic bonding:

Compound of metal and non-metal

Composed of ions: cation and anion

non-volatile, thus high melting points

solids do not conduct electricity, but melts (liquid state) do

many, but not all, are water soluble


Electrical Conductivity ofIonic Solution

Electrolytes

Aqueous solutions conducts electricity

strong-electrolytes

weak-electrolytes

Non-electrolytes

Aqueous solutions do not conducts electricity


Ionic Compounds

Type II ionic compound

FeCl2 and FeCl3,

SnCl2 and SnCl4

Type I ionic compound

(fixed charge) NaCl


Type I Type II


Charges on Some Common Monatomic Cations and Anions


Charge on Metal IonsMonatomic Ions (Type I)Group IA +1 Group A #Group IIA +2 Group A #Non-metalsGroup IIB -1 (8 - Group B #)

Monatomic Ions (Type II)Transition metal ionic compounds:

have ions with different chargesE.g. Iron :Fe2+ and Fe3+


Name Formulaacetate C2H3O2

–

carbonate CO32–

hydrogen carbonate(aka bicarbonate) HCO3

–

hydroxide OH–

nitrate NO3–

nitrite NO2–

chromate CrO42–

dichromate Cr2O72–

ammonium NH4+

Name Formulahypochlorite ClO–

chlorite ClO2–

chlorate ClO3–

perchlorate ClO4–

sulfate SO42–

sulfite SO32–

hydrogen sulfate(aka bisulfate)

HSO4–

hydrogen sulfite(aka bisulfite)

HSO3–

Some Common Polyatomic Ions

with Their Charge


1) Identify the types of ions in the following list: F-,Fe2+, Fe3+,Ca2+,H3O+,Ba2+,Cl-,Cu+, Cu2+, Sr2+,Ra2+,Ni2+, Ni4+,

Br-,CrO42-, Cr2O7

2-, MnO4-, C2O4

2-, NH4+,

a) Cations: Type I :

b) Cations: Type II :

c) Monoatomic anions:

d) Polyatomic anions:

e) Polyatomic cations:


Polyatomic Ions

More than one atom joined together

have negative charge except for NH4+

and its relatives

negative charges range from

-1 to -4

Table in the Book


a) Cl-

b) SO42-

c) SO3

2-

d) Fe3+

e) Sr2+

f) CO3-2 g) NO3

- h) PO43- i) Hg2+ j) Hg2

2+

k) Cr2O72-

l) MnO4

-

m) C2O4

2-

n) NH4

+,

o) U4+

p) HCO3-

q) C2H3O2

- or CH3COO-

r) HSO3-

s) HPO4

-

t) H2PO4

-

2) Give the names of the following ions:


Ion Ion name Acid formula

Acid name

Ion Ion name

a) ClO- i) IO-

b) ClO2- j) IO2

-

c) ClO3- k) IO3

-

e) ClO4- l) IO4

-

f) SO4-2 m) SeO4

-2

g) C2H3O2- n)BrO3

-

3) Give the name of ion and the name and formula of acid it came from


• Alkali and Alkaline Earth Metals– Metal name first, followed by

nonmetal– Nonmetal ending is exchanged

with “IDE”Examples:– MgCl2: magnesium chloride– KNO3: potassium nitrate

• Alkali (+1) and alkaline earth (+2) metals’ oxidation states are known.

– That is why their charge is NOT indicated in the formula name!

Naming Ionic Compounds:

Metal + Nonmetal: Main Group (“p” Block) Metals


• Metal name first, followed by nonmetal

• Metal’s oxidation state is indicated by a Roman numeral.

• Nonmetal ending is exchanged with “IDE.”• Examples:

» MnBr4: manganese (IV) bromide

» Fe2O3: iron (III) oxide

» SnF2: tin (II) fluoride

Naming Ionic Compounds:

Metal + Nonmetal for Transition and Main Group (“p” Block) Metals


Names of Ionic Compounds

1. Name the metal first.

If the metal has more than one oxidation state, the oxidation state is specified by Roman numerals in parentheses.

2. Then name the non-metal,

changing the ending of the non-metal to -ide.


Ionic compounds

Na+

Mg2+

Al3+

Cl-

O2-

N3-

Some simple ions

Formula for some ionic compounds

NaCl MgCl2 AlCl3

Na2O MgO Al2O3

Na3N Mg3N2 AlN

Cations

Anions

Exchange charge as subscripts on the metal and nonmetal

Give the simple ratio


Nomenclature

NaCl

Fe2O3

NH4NO3

KClO4

CaCO3

NaOH

AgNO3

Mg(C2H3O2)2

Co2(SO4)3

KI

Mg3N2

NaCl sodium chloride

Fe2O3 iron(III) oxide

NH4NO3 ammonium nitrate

KClO4 potassium perchlorate

CaCO3 calcium carbonateNaOH sodium hydroxide

AgNO3 silver nitrate

Mg(C2H3O2)2 magnesium acetate

Co2(SO4)3 cobalt(III) sulfateKI potassium iodide

Mg3N2 magnesium nitride


silver carbonate

potassium hydrogen phosphate

aluminum hydroxide

sodium bicarbonate

calcium acetate

potassium permanaganate

calcium perchlorate

magnesium hydrogen sulfite

sodium hypochlorite

iron(II) carbonate Iron(II)chloride nonahydrate

barium oxide

4) Give the formula of following ionic compounds


tin(IV) chlorite mercury(II) phosphate

tin(II) carbonate

mercurous acetate

lead(II) chromate

copper(I) sulfite stannous dichromate

iron(III) nitrate ferric sulfate ferrous hydroxide

potassium perchlorate

lead(IV) hydrogen phosphate

aluminum sulfate

iron(II) bicarbonate

barium iodate tin(II) hydrogen sulfide

magnesium dihydrogen phosphate

plumbous cyanide

silver phosphate

5) Write the correct formula for:


Hydrate

CoCl2∙6H2O

Anhydrous

CoCl2

Hydrated Compounds vs. Anhydrous Compounds


• Hydrates are ionic compounds containing a specific number of waters for each formula unit.

• Water of hydration is often “driven off” by heating.

• In formula, attached waters follow

– CoCl2•6H2O

• In name, attached waters are indicated by

prefix + hydrate after name of ionic compound.

– CoCl2•6H2O = cobalt(II) chloride hexahydrate

– CaSO4•½H2O = calcium sulfate hemihydrate

Prefix No. of Waters

hemi ½

mono 1

di 2

tri 3

tetra 4

penta 5

hexa 6

hepta 7

octa 8

Hydrated Compounds


Problem:

1. What is the formula of magnesium sulfate heptahydrate?

2. What is the name of NiCl2•6H2O?


Answers:

1. What is the formula of magnesium sulfate heptahydrate?

2. What is the name of NiCl2•6H2O?

Mg2+

+ SO42−

MgSO4

MgSO47H2O

Ni2+

+ 2 Cl−

nickel(II) chloride

nickel(II) chloride hexahydrate


UO2

Co3(PO4)2

cobaltic nitrate

magnesium dihydrogen phosphate

CaCl22H2O ammonium ferrous sulfate hexahydrate

6) Give the chemical name or the formulas for the following ionic compounds:

3-1 CHEM 100, Fall 2013 LA TECH Instructor: Dr. Upali Siriwardane e-mail: [email protected]...

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Transcript of 3-1 CHEM 100, Fall 2013 LA TECH Instructor: Dr. Upali Siriwardane e-mail: [email protected]...