Unit 6
Chemical Names &
Formulas
Elements & Compounds
Symbols in a formula
KClO3
Subscript - tells
how many atoms
are in the formula
Examples
H2 0
2 Hydrogens
1 Oxygen
Sr(NO2)2
1 Strontium
2 Nitrogens
4 Oxygens
More Examples
Mg3(PO4)2
Ca(NO3)2
3 Magnesiums
1 Calcium
2 Phosphorus
2 Nitrogens
8 Oxygens
6 Oxygens
Elements & Compounds
Symbols in an Ion
+1
K
Superscript- oxidation
number (charge)
Types of Compounds
1. Metallic = Metals only
2. Ionic = Metal with nonmetal
3. Covalent/ molecular =
Nonmetals only
Multivalent Elements
Elements with more than
one possible charge.
To find their charge, look
at the Periodic Table we
color coded!
Example – Charge of Cu?
Polyatomic Ions
A charged group of
covalently bonded
atoms
To name them look on
the back of the PT
STOP!
Complete
Worksheet #1 as a
review
Today…
 Turn in:
Goal Sheet
 Add your test and calculate your totals.
 Get out WS#1 to check
 Take Home Your Personal PT
 Our Plan:
 Round Table Review
 Puzzle Activity
 Notes
 Worksheet #2
 Wrap Up – Go Fish
 Homework (Write in Planner):
 Complete WS#2

Quick Round Table Review –
p. 3 booklet
1. How many oxygens are in
Fe(OH)3?
2. How many oxygens are in
Ba2(PO4)3?
3. What is the name of the
polyatomic ion NO3-1?
4. What are the charges of copper?
Round Table Review
Can You Name:
5.
6.
NaCl
Ca(OH)2
Puzzle Time
Use a chromebook to complete Part 1
of the activity on p. 5 of the WS
Packet.
Complete the first three columns of
the puzzle activity individually on p. 6
of the WS packet.
When finished, ask Mrs. C how to do
the 4th column.
Daily Challenge – p. 3
booklet
Name the following
compounds:
1. K3PO4
2. Ca(NO3)2
To Write Formulas…
Elements form compounds
because they want to be stable.
The charge tells you how many
electrons they want to gain or lose:
 +2 = want to lose 2 electrons
 -2 = want to gain 2 electrons
To Write Formulas…
In a compound, the sum of the
oxidation numbers (charges) is 0!
That means that elements combine
so that their charges cancel out.
Use subscripts to cancel out the
charges and do the math in your
head.
For Example
+2
Ca
+3
Al
with
with
-1
F
-2
O
= CaF2
= Al2O3
OR……
Use Mrs. C’s “Super
Easy Way” for Writing
Formulas!
Writing Formulas for Ionic
Bonds – the “Super Easy Way”
Positive ion (cation) is always
first
Write charges as a superscript
on each ion:
For multivalent charge, look
at the Roman numeral
Writing Formulas for Ionic
Bonds – the “Super Easy Way”
Criss-Cross charges Down!
If
they don’t cancel out,
write as a subscript
Examples
a. Magnesium oxide
+2
Mg
-2
O
Mg2O2
MgO
Example
b. Potassium Phosphide
K+1
K3P
P-3
Example
c. Copper (II) Chloride
Cu+2
Cl-1
CuCl2
Example
d. Silver Iodide
Ag+1
AgI
-1
I
Example
e. Zinc hydroxide
Zn+2
OH-1
Zn(0H)2
Example
f. Tin (IV) Sulfate
Sn+4
SO4
-2
Sn2(SO4)4
Simplify! Sn(SO4)2
Naming Binary Ionic
Compounds
2 elements = BINARY (NaCl)
Rules:
Name
Metal (cation)
Name Nonmetal (anion) with
“ide” ending
Naming Non-Binary Ionic
Compounds (Ex: NaOH)
Name the cation
Name the anion
 Use
the back of your PT for
the names of the polyatomic
ions
 For multivalent, include the
charge as a roman numeral in
parentheses
Important Point…
There are
never more
than 2 parts
to a name!
Example
a. Na Cl
Sodium Chloride
b. KI
Potassium Iodide
c. CaBr2
Calcium Bromide
More Examples
d. Mg(NO3)2
Magnesium
Nitrate
e. Na3PO4
Sodium Phosphate
f. CuCO3
Copper (II) Carbonate
Challenge!
Predict the charge
of copper in
Cu3(PO4)2.
Naming Acids-- Memorize
HCl
Hydrochloric Acid
HNO3
Nitric Acid
H2SO4
Sulfuric Acid
H3PO4
Phosphoric Acid
HC2H3O2 Acetic Acid
H2CO3
Carbonic Acid
STOP!
Complete WS#2 by
next class.
Have Mrs. C look at
least 10 AND check
the key!
Wrap Up
Let’s play Go Fish!
Today…
 Turn in:
Get out WS#2 to check
 Our Plan:
 Bond with a Classmate Review
 Ban DHMO Reading
 Notes – Covalent Nomenclature
 WS#3
 Spoons (if time)
 Wrap Up – Exit Slip
 Homework (Write in Planner):
 Worksheet #3 – Due next time

Bond with a Classmate
 Choose an ion to wear around your neck
 Move around the classroom to find a
classmate to “bond” with
 Fill out one row of the table to describe
your “bond”
 After 3 bonds, get a new card and repeat
the steps until your paper is full!
Ban DHMO!
Complete the Anticipation Guide
by filling in the first column before
you read.
Fill in the second column during
reading.
Answer the questions that follow
after reading.
Questions After Reading
The author of this article is
trying to persuade you to do
and believe something.
There are several techniques
that authors use to persuade
their readers into action:
Bandwagon Approach
“Everyone is doing
it”
You’ve probably
tried this with your
parents 
Glittering Generalities
Refers to vague goals
and common interests
that everyone would
seem to share.
patriotism, peace
Testimonials
Use testimony of well-known
personalities even if they have
no relevance to the topic
Movie stars supporting a
presidential candidate
Citing Authority
Stating the opinion of
an expert in the field.
9 out of 10 doctors
recommend Gold Bond.
Statistics
Use statistical figures to
persuade the reader.
90% of men who tried
the product liked it
Fear Appeal
Author focuses on the worst-
case scenario to scare the reader
into believing his or her case.
The Ogallala Aquifer, our state’s
major source of water will be dry
in the next 20 years unless we
start conserving water now!
Video
 http://www.youtube.com/watch?v=yi3erd
gVVTw
 http://www.dhmo.org/
Molecular Compounds
What are they?
Covalently
bonded
NONMETALS
Covalent= SHARING
ELECTRONS
Nomenclature Rules
1. Use prefixes to indicate how
many of each element there are
in the compound

Exception- omit mono on the
first element
Nomenclature Rules
2. Give the last
element an “ide”
ending.

The vowel at the end of a prefix is
sometimes dropped when the name
of the element begins with a vowel.
Prefixes
Number
1
2
3
4
5
6
7
8
9
10
Prefix
MonoDiTriTetraPentaHexaHeptaOctaNonaDeca-
Examples
a. P4O10
Tetraphosphorus
Decaoxide
b. N2O3
Dinitrogen
c. ICl3
Trioxide
Iodine Trichloride
Try It Out!
d. PBr5
Phosphorus Pentabromide
e. SO2
Sulfur Dioxide
f. AsF6
Arsenic Hexafluoride
Examples
g. Carbon Tetrafluoride
C F4
h. Hexacarbon Octaoxide
C6 O8
i. Pentaphosphorus Nonafluoride
P5 F 9
STOP!
Complete Worksheet
#3 by next class period!
Wrap Up – exit slip
In your group, number off 1 – 4.
You will each get a different
compound. Tell your group if it
is ionic or covalent and then
name it. As a group, decide if
each person is correct or not!
Wrap Up
Person 1 – C4O9
Person 2 – Cu2CO3
Person 3 – Sr3(PO4)2
Person 4 – N5C2Cl7
Today…
 Turn in:
 Get
WS #3 out to check
 Our Plan:
 Naming
Race
 Clicker Review
 Nomenclature Quiz
 Homework (Write in Planner):
 Nothing
Today…
 Turn in:
Figure out the names/formulas on your card(s) and write
them on the back of your note booklet
 Our Plan:

I have, who has…
 Notes
 Worksheet #4
 High Five

 Homework (Write in Planner):

Worksheet #4
The Mole
The amount of a substance
that contains 6.022 X 1023
representative particles of that
substance
6.022 X 1023 is called
Avogadro’s number
The Mole
A mole is kind of
like a dozen!
The Mole!
Get ready to dance,
because…
Here comes
the Mole song!
 http://www.youtube.com/watch
?v=1R7NiIum2TI&feature=relat
ed
How big is a mole?
 http://www.youtube.com/watch?v=TEl4je
ETVmg
How about some mole jokes?
Q: What did Avogadro
teach his students in
math class?
A: Moletiplication
How about some mole jokes?
Q: What kind of fruit
did Avogadro eat in the
summer?
A: Watermolens
How about some mole jokes?
Q: What do you get when
you have a bunch of moles
acting like idiots?
A: A bunch of Moleasses
How about some mole jokes?
What cell phone
provider does a mole
have?
A: T-Molebile
 Philip Steele, 2011
How about some mole jokes?
Q: How do moles defend
themselves?
A: TiKwanMole
 Caleb Colucci, 2012
How about some mole jokes?
Q: What do moles do for
fun?
A: Moller Skate
 Devan Castle, 2010
How about some mole jokes?
Q: What kind of test do
chemistry students like best?
A: Mole-tiple Choice
 Nicole Crites/Callie Price, 2010
How about some mole jokes?
Q: What do you call a mole
that goes bad?
A: Moledy
 Jeff Franco, 2011
How about some mole jokes?
Q: What kind of theater
production does a mole go
to?
A: A MOLEsical
 Becky Lyne, 2011
How about some mole jokes?
Q: What is a mole’s favorite
candy?
A: Hot Tamoles
 Ani Mitchell, 2012
How about some mole jokes?
Q: Why was the chem lab
closed for a month?
A: They were reMOLEdeling
 Emily Crites, 2012
How about some mole jokes?
Q: What does Avogadro use
in church on Sundays?
A: Moley Water
 Katey Roberts, 2010
How about some mole jokes?
Q: Why were the moles in a
Japanese village running
away in terror?
A: Molezilla was taking over
the world!
 Haydee Mendez, 2011
How about some mole jokes?
Q: What is a mole’s favorite
hairdo?
A: A mollet
 Addison Dougherty & Mickey
McConnell, 2013
The Best One…
 A mama mole, a papa mole, and a baby mole
all live in a little mole hole.
One day the papa mole sticks his head out of
the hole, sniffs the air and says,"Yum! I smell
maple syrup!"
The mama mole sticks her head out of the hole,
sniffs the air and says "Yum! I smell honey!"
The baby mole tries to stick his head out of the
hole to sniff the air, but can't because the bigger
moles are in the way so he says, "Geez, all I
can smell is MOLASSES!"
There’s even MOLE DAY!
It’s on October 23
from 6:02 am to
6:02 pm!
Molar Mass
The mass of one mole
of a substance
Written as g/mole
Found on the PT
Calculating Molar Mass
H2O
Calculating Molar Mass
C6H12O6
Try It Out
H3PO4
Mg(NO3)2
Conversions
#grams
1 mole
Mass in
Grams
Molar
Mass
1 mole
6.022 X 1023 molecules
Moles
6.022 X 1023
PT
22.4 L
Volume
(L)
Molecules
Or
Atoms
Example 1
Convert 7.6 moles NaOH
into molecules.
Example 2
Find the mass of 1.65 moles
of NH3.
Example 3
Mass in grams of 2.50
moles of oxygen gas.
Example 4
Moles of Ca(OH)2 in 4.5 grams
Example 5
Molecules of HCl in 56.21 grams.
9.27 X 1023 molecules
Example 6
Liters of O2 in 4.23 grams.
Try It Out!
Find the mass, in
grams, of 1.7 moles of
potassium chloride. (130
g)
Try It Out!
How many
molecules of NaOH
are in 3.45 grams?
5.36 X
22
10
molecules
STOP!
Begin Worksheet #4
Due
next class
Wrap Up – p. 11
High Five – As a group,
come up with 5 things
that you learned today!
Today…
 Turn in:
Get Worksheet #4 out to be Checked
 Our Plan:
 Conversions Team Review
 Conversions Quiz
 Begin Penny Lab
 What’s in a Name Lab
 Wrap Up – Nomenclature Memory
 Homework (Write in Planner):
 What’s in a Name Lab

Worksheet 4 Questions?
Another Video
Conversions
#grams
1 mole
Mass in
Grams
Molar
Mass
1 mole
6.022 X 1023 molecules
Moles
6.022 X 1023
PT
22.4 L
Volume
(L)
Molecules
Or
Atoms
Review Activity
Complete the
team review with
your group of 4!
The Answers
1.1173.060
2.3.4 x
24
10
3.2,155
+ 3010
Wrap Up
Nomenclature Memory
Today…
 Turn in:
Pull out penny lab handout, Periodic Table, and
calculator THEN put on goggles & an apron, THEN
get pennies from the back table
 Our Plan:
 Finish Penny Lab and Answer all questions – turn in
 Nomenclature Memory/Go Fish/Spoons/Old Maid
 Homework (Write in Planner):
 Lab

Lab Time!
 Show all work! Check Sig Figs!
 Only do the calculations for YOUR
penny
 Clean up and place everything on the
side counter
 Helpful Formulas:
D = M/V
 %E = |A-E|/A x 100

Today…
 Turn in:
Nothing
 Our Plan:
 Find Someone Who…
 Percent Water in Popcorn
 Percent Composition POGIL
 Worksheet #5
 Wrap Up – REVIEW FORMULAS
 Homework (Write in Planner):
 Worksheet #5 – Due Next Class

A chemistry pick up line…
Are you a chemist
‘cause you look
Fluorine Iodine Neon!?
Chemistry Humor!
Introduction to Percent
Composition
As a class, we are going to determine the
percentage of water in a bag of microwave
popcorn.
1. What evidence is there that popcorn
contains water?
2. How can you determine the percentage
of water in popcorn?
3. Let’s try it out.
POGIL Jobs
• Leader – In charge of the group, reads the
questions, summarizes what should be
written
• Task Master – Makes sure the group is on
task and keeps track of time
• Quality Control – Makes sure that
everyone has close to the same answers
recorded
• Motivator – encourages the group and
makes sure that everyone is participating
and that all ideas are heard
Example
 Calculate the mass of chlorine in 120 g of
NaCl.
%Cl =
35.5g
X 100
58.5g
= 60.7% Cl
60.7% x 120 g = 72.8 g
Challenge!
Can you think of real life
examples where percent
composition is found?
Clothing, food, grades,
percent body fat
Wrap Up – p. 12 booklet
Write formulas for:
1.
2.
3.
4.
Calcium acetate
Dinitrogen pentaoxide
Iron (III) chloride
Tin (IV) sulfate
Write names for:
5.
6.
7.
PbO
H3F6N8
K2CrO4
Today…
 Get Out:
 WS#5
 Our Plan:
Review - % Composition Problems
 Challenge & Notes
 Worksheet #6
 Clicker Review
 Homework (Write in Planner):
 Worksheet #6 – Due Next Class

Review
What is the percent
composition of phosphorus
in Ca3(PO4)2?
What is the chemical name
for Ca3(PO4)2?
Daily Challenge
What is the difference
between these 2 formulas?
C8H14O6
C4 H7 O 3
Empirical vs. Molecular
Empirical gives the
lowest whole-number
ratio of the atoms in the
compound.
Empirical vs. Molecular
Molecular show the
actual number & kinds
of atoms present in the
compound.
Examples
C2H2
CH
C6H12O6
CH2O
Which is more
important to know?
MOLECULAR!!!
Rules for Empirical
Calculations
1. Find the percent
composition of each
element
Rules for Empirical Calc.
2. Change percent to mass
(assume 100g sample
unless told otherwise).
Rules for Empirical Calc.
3. Find number of moles
of each element
(multiply by 1 mole / PT
mass)
Rules for empirical Calc.
4. Find the ratio of each
element (divide each molar
quantity by the lowest
molar quantity)
Rules for Empirical Calc.
5. Multiply by a whole
number (2, 3, or 4) if
fractions are left
Rules for Empirical Calc.
6. Write the formula (place
the ratios as
SUBSCRIPTS)
Example
Analysis shows a
compound to contain
26.56% K, 35.41% Cr, &
38.03% O. Find the
empirical formula.
Try it Out!
Analysis shows that a
compound contains 32.38%
sodium, 22.65% sulfur, and
44.99% oxygen. Find the
empirical formula of this
compound. (Na2SO4)
Molecular Formulas
Use the Molar Mass
& the Empirical
Formula of the
compound
Molecular Formula Rules
1. Calculate the empirical
formula (follow all steps)
2. Find the molar mass of
the empirical formula
Molecular Formula Rules
3. Divide the molar
mass of the
compound by the
mass of the
formula
Molecular Formula Rules
4. Multiply the subscripts in
the empirical formula by
that # & write new
formula
Example
Calculate the molecular
formula of the compound
whose molar mass is
60g/mole & empirical
formula is CH4N.
Try it Out!
Analysis of a compound indicates
that it contains 1.04 g K, 0.70 g
Cr, and 0.86 g O. The molar
mass of the compound is 388
g/mole. What is the molecular
formula? (K4Cr2O8)
Example
2K = 2(39) = 78
1Cr = 1(52) = 52
4O = 4(16) = 64
388
=2
194
194g/mole
K4Cr2O8
STOP!
Complete Worksheet #6
by the next class period.
Clicker Review
Wrap Up – Exit Slip
A compound has an empirical
formula C2H5O. If it’s molecular
mass is135 g/mole what is the
molecular formula?
Today…
 Turn in:
Worksheet #6
 Our Plan:
 Station Review
 Card Games
 Test Review
 Homework (Write in Planner):
 Test Review – due next class
 TEST NEXT CLASS!

Today…
Turn in:
 Check
Test Review
Our Plan:
 Quiz, Quiz Trade
 Go Over Test Review Questions
 Final
Homework (Write in Planner):
 Enjoy your Break!