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Illustrate the Lewis structures for:
Water (H2O)
Carbon dioxide (CO2)
Phosphorous trichloride (PCl3)
Molecules &
Molecular
Compounds
Ions & Ionic
Compounds
Chemical
Nomenclature
Some Simple
Organic
Compounds
E.Q.: How do I represent molecules and molecular
compounds through chemical and empirical
formulas?

Covalently bound groups of the same atom!
 Hydrogen (H2), Oxygen (O2), and Sulfur (S8 ).



Behaves as a single object!
Most will only contain nonmetals!
Molecular compounds are slightly different!


Molecule: Same atom...
Molecular compound: Different atoms...
 Water (H2O) and Hydrogen peroxide (H2O2)
 Carbon monoxide (CO) and Carbon dioxide (CO2)

Methane (CH4)

Ammonia (NH3)
Nitrous
Oxide (N2O)


All compounds have a chemical formula.
 Name and subscript used to classify a compound.
 Hydrogen, H2
Sulfur, S8
 Oxygen, O2
 Nitrogen, N2

Properties of a compound can change
greatly by changing the number of atoms
(i.e. O3)

Chemical formula for hydrogen peroxide:H2O2
 Indicates the actual numbers and types of atoms in
a molecule.

Empirical formula for hydrogen peroxide: HO
 Indicates the relative number of atoms of each
type molecule. Simply divide by a common factor.
 Not all molecules have an empirical formula.
▪ i.e. H2O. No common factor to divide by.

Write the empirical formulas for the
following molecules whose chemical
formulas are given:
Ethylene, C2H6

Dodecane (Jet fuel), C12H26

Glucose, C6H12O6


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Molecules...
Molecular Compounds...
Chemical Formulas...
Empirical Formulas...
Study Your Notes!

Provide an example of a monoatomic and a
polyatomic ion.

Explain the relationship between ionic
bonding and octet rule.
Molecules &
Molecular
Compounds
Ions & Ionic
Compounds
Chemical
Nomenclature
Chemical
Nomenclature
II
E.Q.: How I identify ionic bonding within ionic compounds?

Ion – Atom that has lost/gained e-.
 Found in the human heart (K+, Na+, and Ca2+)
 Found in batteries (Li+, H-, and Fe2+)
 Oxides (O2-), Peroxides (O22-), and Superoxides
(O2+)
 Can be positive (cation) or negative (anion).
 Can be polyatomic – Ion with multiple atoms
(i.e. NH4+, OH-, or HCO3-).



Poly – “Many”
Atoms joined together as in a molecule..but
they have a charge!
Have parentheses around them when
writing compounds.


Cation - Loss of e- (Metals)
Anion - Gain of e- (Nonmetals)

Atoms gain/lose e- to end up with the same
number of e- of the noble gas closest to
them in the periodic table. (Why?)

Ions form ionic compounds

Formed between metal (cation) and
nonmetal (anion).

Complete the following chemical equations:




Ions...
Formation of Ions...
Polyatomic Ions
Ionic Compounds...
Study Your Notes!

Name the following compounds:
 NaCl
 KCl
 MgI2
 HCl
 HBr
Molecules &
Molecular
Compounds
Ions & Ionic
Compounds
Chemical
Nomenclature
Chemical
Nomenclature
II
E.Q.: Can I use IUPAC system to name chemical
compounds?

IUPAC nomenclature - Set of rules that leads
to a name for each chemical substance.

Cations:
 Monoatomic: No name change
 Polyatomic: Change ending to –ium.

Anions:
 Monoatomic: Change ending to –ide.
 Polyatomic: Change ending to either –ite or –ate.
Charge
Formula
Name
1+
H+
Li+
Na+
K+
Hydrogen ion
Lithium ion
Sodium ion
Potassium ion
2+
Mg2+
Ca2+
Sr2+
Ba2+
Magnesium ion
Calcium ion
Strontium ion
Barium ion
3+
Al3+
Aluminum ion


Hydronium Ion: H3O+
Ammonium Ion: NH4 +


Nonmetals - negative ions (Cl forms Cl-)
Replace the ending of the name with -ide
Formula
Name
H-
Hydride (Explosive!)
Cl-
Chloride
O2-
Oxide
N3-
Nitride

Polyatomic ions containing oxygen
Formula
Name
CO32-
Carbonate
NO2-
Nitrite
NO3-
Nitrate
SO32-
Sulfite
SO42-
Sulfate
4A
2
3
CO32Carbonate
5A
6A
NO2Nitrite
NO3Nitrate
C2O42Oxalate
PO33Phosphite
PO43Phosphate
SO32Sulfite
SO42Sulfate
7A (Only
Chlorine)
ClOHypochlorite
ClO2Chlorite
ClO3Chlorate
ClO4Perchlorate
Chemical Formula Name
NaCl
Sodium chloride
Ca(CO3)
Calcium carbonate
Al(NO3) 3
Aluminum nitrate
K3PO4
Potassium phosphate
MgSO4
Magnesium sulfate
________ide
(Chloride, Cl-)
Hydro_______ic acid
(Hydrochloric
Acid, HCl)
_______ate
(Sulfate, SO4)
________ic acid
(Sulfuric Acid,
(H2SO4)

Use chemical nomenclature to name the
following:
 KCl
 Na2SO4

Chemical nomenclature...
 Monoatomic ions...
 Polyatomic ions...
Study Your Notes!

Name the following:
 RbBr
 Na2SO4
 Ag3PO4
 K2NO3
 Na2HCO3
 Na2ClO
Molecules &
Molecular
Compounds
Ions & Ionic
Compounds
Chemical
Nomenclature
Chemical
Nomenclature
II
E.Q.: Can I use IUPAC system to name chemical
compounds?

What is chemical nomenclature?

We’ve looked at the nomenclature for ionic
compounds; now, let’s look at the
nomenclature for binary molecular
compounds!

Binary - Molecular compounds with only
two atoms! (Ex. CO2)




Cl2O
NF3
N2O4
PCl5
dichlorine monoxide
nitrogen ______________?
__________________ tetraoxide
________________________________?

Name the following compounds:
 CO
 CO2
 SO2
 N2O3
 NO3




I’m expecting you to already know prefixes
that represent each number!
Mono1
Di2
Tri3…

Indicate the chemical formula for the
following:
 Silicon tetrabromide
 Carbon disulfide
 Phosphorous trichloride

Chemical Nomenclature II…
 Binary molecular compounds
Study Your Notes!

Based on what you know about the octet
rule and electron configuration, indicate
how many bonds does carbon need to be
stable. Explain.

Skunk Spray Chemistry!
Molecules &
Molecular
Compounds
Ions & Ionic
Compounds
Chemical
Nomenclature
Chemical
Nomenclature
II
E.Q.: Can I use IUPAC system to name chemical compounds?

Welcome to my world!

Study of compounds containing carbon.

Hydrocarbon – Compound containing
hydrogen and carbon (i.e. gasoline).

Carbon needs ________ bonds to have be
stable.


The most basic class of hydrocarbons.
Carbon is bonded to four other atoms.
 Mostly H and other C atoms.



The three simplest alkanes:
Methane, ethane, and propane.
Don’t have normal naming system; instead,
they end in –ane.

Methane:
Propane:
Ethane:

Get longer as you add more carbon atoms!

Butane:
Pentane:
Hexane:


Derivative – Something based on something
else.
Other class of hydrocarbons are obtained
when H atoms are replaced with functional
groups.

Alcohol – Replace H atom with an –OH
group.

Octane is a hydrocarbon with a chemical
formula C8H18. Octanes are found in
gasoline. Based on what you’ve learned,
attempt to draw the Lewis structure for
octane.




Organic Chemistry...
Hydrocarbons...
Alkanes...
Alcohols...
Study Your Notes!