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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
3-2CHEM 100, Fall 2013 LA TECH
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
3-3CHEM 100, Fall 2013 LA TECH
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
3-4CHEM 100, Fall 2013 LA TECH
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)
3-5CHEM 100, Fall 2013 LA TECH
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)
3-6CHEM 100, Fall 2013 LA TECH
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.
3-7CHEM 100, Fall 2013 LA TECH
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
3-8CHEM 100, Fall 2013 LA TECH
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
3-9CHEM 100, Fall 2013 LA TECH
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
3-12CHEM 100, Fall 2013 LA TECH
• Ionic compounds
• Molecular compounds(Inorganic & organic)
• Acids and bases
• Hydrated compounds
Nomenclatuere: Naming Compounds
3-14CHEM 100, Fall 2013 LA TECH
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
3-15CHEM 100, Fall 2013 LA TECH
Electrical Conductivity ofIonic Solution
Electrolytes
Aqueous solutions conducts electricity
strong-electrolytes
weak-electrolytes
Non-electrolytes
Aqueous solutions do not conducts electricity
3-16CHEM 100, Fall 2013 LA TECH
Ionic Compounds
Type II ionic compound
FeCl2 and FeCl3,
SnCl2 and SnCl4
Type I ionic compound
(fixed charge) NaCl
3-19CHEM 100, Fall 2013 LA TECH
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+
3-20CHEM 100, Fall 2013 LA TECH
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
3-21CHEM 100, Fall 2013 LA TECH
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:
3-22CHEM 100, Fall 2013 LA TECH
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
3-23CHEM 100, Fall 2013 LA TECH
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:
3-24CHEM 100, Fall 2013 LA TECH
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
3-25CHEM 100, Fall 2013 LA TECH
• 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
3-26CHEM 100, Fall 2013 LA TECH
• 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
3-27CHEM 100, Fall 2013 LA TECH
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.
3-28CHEM 100, Fall 2013 LA TECH
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
3-29CHEM 100, Fall 2013 LA TECH
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
3-30CHEM 100, Fall 2013 LA TECH
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
3-31CHEM 100, Fall 2013 LA TECH
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:
3-32CHEM 100, Fall 2013 LA TECH
Hydrate
CoCl2∙6H2O
Anhydrous
CoCl2
Hydrated Compounds vs. Anhydrous Compounds
3-33CHEM 100, Fall 2013 LA TECH
• 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
3-34CHEM 100, Fall 2013 LA TECH
Problem:
1. What is the formula of magnesium sulfate heptahydrate?
2. What is the name of NiCl2•6H2O?
3-35CHEM 100, Fall 2013 LA TECH
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