Chemistry in
Motion: Unit 4
Hobbs
1. Bell Ringer: March 31, 2014
The oxidation number
(charge) of an atom is
show with a _______.
a. Negative number
b. Positive Number
c. Superscript
d. Subscript
2. Bell Ringer: Tuesday, 04.01.14
What three items are
needed for a Lewis
structure?
**If you missed the Unit
3 Test the last day to
make it up is
Thursday!!!! Study!
3. Bell Ringer: Wednesday,
04.02.14
In a chemical formula, like H2O,
the number of each type of
atom in the compound is
shown by numbers called
___________.
a. Superscripts
b. Chemical symbols
c. Oxidation numbers
d. Subscripts
4. Bell Ringer: 04.03.14
What is the correct chemical
formula for magnesium oxide?
a. MgO
b. MgO2
c. Mg2O2
d. Mg2O
***Naming Quiz TODAY!!!!***
TODAY is the last day to make up
your UNIT 3 TEST!!!!
5. Bell Ringer: Friday,
04.04.14
Balance the following equation:
___NH3 + ___ HCl  ___
NH4Cl
11. Bell Ringer: 04.14.14
Balance the following chemical equation:
__CaBr2 + __Na2CO3 __CaCO3
+ __NaBr
12. Bell Ringer: 04.15.14
• What is the difference between the
two mixtures below? Can you
name each?
13. Bell Ringer: Wednesday,
04.16.14
What is the difference
between unsaturated,
saturated, and
supersaturated?
(Think in terms of how much
solute vs. solvent)
14. Bell Ringer: Thursday,
04.17.14
Lenox made sweet tea for her
family’s dinner that evening. She
mixed the sugar in the tea, but not
all of the sugar would dissolve. Has
Lenox made an unsaturated,
saturated, or supersaturated
solution? Explain your answer.
16. Bell Ringer: Monday,
04.21.14
The concentration of a solution that
contains a large amount of solute in
the solvent could be described as
___________.
a. Concentrated
b. Dilute
c. Polar
d. Unsaturated
17. Bell Ringer: Tuesday,
04.22.14
A substance that produces
hydroxide (OH-) ions in water is
a(n)
a.Acid
Thursday is
b.Base
BLACK and WHITE DAY!
c.Hydrocarbon BRING MONEY
THURSDAY for the
d.Salt
th
RELAY RALLY 4
BLOCK!!!
18. Bell Ringer: Wednesday,
04.23.14
• In a ________________ reaction, an
acid and a base produce a salt
and water.
• A. decomposition
• B. dilute
Thursday is
• C. neutralization BLACK and WHITE DAY!
BRING MONEY
• D. concentrated
DO NOT TOUCH ANYTHING, UNTIL I TELL
YOU TO DO SO OTHERWISE, IT IS
BOOKWORK for THE WHOLE BLOCK!
THURSDAY for the
RELAY RALLY 4th
BLOCK!!!
19. Bell Ringer: Thursday,
04.24.14
• Tomato juice has a pH of 4. What
substance would be needed to
neutralize tomato juice?
• A. vinegar (pH 3)
• B. pure water (pH 7)
• C. soap (pH 10)
BRING MONEY
• D. ammonia (pH 12) THURSDAY for the
RELAY RALLY 4th
BLOCK!!!
20. Bell Ringer: Friday,
04.25.14
• Which solutions
are most likely
acids?
• A. 1 and 3
• B. 2 and 5
• C. 3 and 6
• D. 4 and 7
Solution
Effect on
Blue Litmus
Effect on
Red Litmus
1
None
Turns blue
2
None
Turns blue
3
None
None
4
Turns red
None
5
None
Turns blue
6
None
None
7
Turns red
None
Once you finish, turn in BELL RINGERS and STUDY for your TEST,
don’t act like you didn’t know you had a test, it’s been on the
board for weeks and I have also been telling you all week!
Unit 3 Review
Two elements with
the same number
of protons, but
different number
of neutrons?
Unit 3 Review
What is the name
of the elements
along the stair
step line?
Unit 3 Review
Halogens are
located in
which group?
Unit 3 Review
Differences
between alphabeta-gamma?
Unit 3 Review
What are the
general
properties of
metals?
Unit 3 Review
Boron has a mass
number of 11 and
an atomic number
of 5. How many
neutrons are in a
Unit 3 Review
How many
electrons are in
the outer energy
level of Group 17
elements?
Unit 3 Review
How many
protons are in
the nucleus of
Kr-81?
Unit 3 Review
•A(n)
________________ is
a horizontal row in
the periodic table.
Unit 3 Review
A vertical
column of
elements is
also referred
Unit 3 Review
When an atom is
chemically stable,
how many electrons
are in its outer energy
level?
a. 0 b. 7 c. 4 d. 8
Make sure group numbers,
oxidation numbers and valence
electrons are CORRECT!!!!
Electron Dot Diagram/Lewis
Structure
Electron dot diagram – a diagram or drawing where you
use the element’s chemical symbol and valence
electrons to show how atoms bond.
Electron Dot Diagram/Lewis
Structure
1)
2)
3)
•
•
Find your element on the periodic table.
Determine the number of valence electrons.
This is how many electrons you will draw.
Find out which group (column) your element is in.
This will tell you the number of valence electrons
your element has.
• You will only draw the valence electrons.
Lewis Structures
1) Write the
element symbol.
2) Carbon is in the
4th group, so it
has 4 valence
electrons.
3) Starting at the
right, draw 4
electrons, or
dots, counterclockwise
Lewis Structures
On your worksheet,
try these elements on
your own:
a)
b)
c)
d)
e)
P
Ca
Ar
Cl
Al
Useful Vocabulary
• Subscript - is number next to the symbol of an
element. It represents how many atoms of a
particular element is present in the chemical
formula.
• Superscript – is the number above the symbol of an
element. It represents the oxidation number
(charge) of an atom/molecule.
• Binary compound – a compound composed of two
elements.
Chemistry
• Chemical bond – attraction
between atoms that allows the
formation of chemical
substances with two or more
atoms.
Bonding
Metallic Bonds
Ionic Bonds
Covalent Bonds
• Metal and
metal bonded
• Metal and
nonmetal
bonded to
form a
compound
• Metal is giving
its valence
electron to the
nonmetal
• Example: NaCl
• Nonmetal and
nonmetal
bonded to
form a
compound
• The valence
electrons will
be shared
• Example: N2O2
Compounds
• A compound is a substance composed of two or
more elements combined in a specific ratio and
held together by chemical bonds.
• Familiar examples of compounds are water and salt
(sodium chloride).
Ionic Compounds
The resulting electrically neutral
compound, sodium chloride, is
represented with the chemical
formula NaCl.
The chemical formula, or simply
formula, of an ionic compound
denotes the constituent
elements and the ratio in which
they combine.
Naming Ions and Ionic
Compounds
Balancing Equations
•Law of Conservation of
Mass - in a chemical
reaction, the mass of the
products equals the mass
of the reactants.
Balancing Equations: Parts of
an Equation
• 1. Reactants – come after
the yield sign
• 2. Products – come before
the yield sign
• 3. Coefficients – are used to
multiply and occur in front of
chemical formula
Balancing Equations
Types of Chemical
Reactions
• Synthesis: A synthesis reaction is when two or more
simple compounds combine to form a more
complicated one. These reactions come in the
general form of:
• A + B ---> AB
• One example of a synthesis reaction is the
combination of iron and sulfur to form iron (II) sulfide:
• 8 Fe + S8 ---> 8 FeS
Types of Chemical
Reactions
• Decomposition: A decomposition reaction is the
opposite of a synthesis reaction - a complex
molecule breaks down to make simpler ones. These
reactions come in the general form:
• AB ---> A + B
• One example of a decomposition reaction is the
electrolysis of water to make oxygen and hydrogen
gas:
• 2 H2O ---> 2 H2 + O2
Types of Chemical
Reactions
• Single replacement: This is when one element trades
places with another element in a compound. These
reactions come in the general form of:
• A + BC ---> AC + B
• One example of a single displacement reaction is
when magnesium replaces hydrogen in water to
make magnesium hydroxide and hydrogen gas:
• Mg + 2 H2O ---> Mg(OH)2 + H2
Types of Chemical
Reactions
• Double replacement: This is when the anions and
cations of two different molecules switch places,
forming two entirely different compounds. These
reactions are in the general form:
• AB + CD ---> AD + CB
• One example of a double displacement reaction is
the reaction of lead (II) nitrate with potassium iodide
to form lead (II) iodide and potassium nitrate:
• Pb(NO3)2 + 2 KI ---> PbI2 + 2 KNO3
How do we classify matter?
Molecules
Atoms
Matter
Substances
Elements
Compounds
Mixtures
Homogene
ous
Solute
Heterogeneous
Solvent
Matter
• Matter is
anything
made of
atoms and
molecules.
• It is anything
that has mass
and takes up
space.
How do we classify
matter?
• Atoms – is the
simplest form of
matter
• Molecules - a
group of atoms
bonded together,
representing the
smallest
fundamental unit
of a chemical
compound
Substance
• A pure substance
is a sample of
matter with both
definite and
constant
composition with
distinct chemical
properties (ex:
fluorine)
How do we classify
matter?
• Elements –
substance that
cannot be broken
into two or more
simpler substances
(ex: mercury)
• Compounds - is a
substance formed
when two or more
chemical elements
are chemically
bonded together.
(ex: NO2)
Mixture
• a mixture is when
two or more
substances are
mixed together
but not
combined
chemically.
How do we classify
matter?
• Mixtures
• Homogeneous - is
simply any mixture that
is uniform in
composition
throughout, therefore
the different parts
cannot be seen.
(examples: koolaid,
lemonade, sweet tea)
• Heterogeneous - is
made of different
substances that remain
physically separate, so
the different parts are
seen.
(ex: trail mix, salads,
cereal)
Mixtures
• Solute – is the
smaller portion of
the mixture and
the part that is
being dissolved.
• Solvent – the
bigger portion of
the mixture and
the part doing the
dissolving.
Mixtures
• Mixtures
• Homogeneous - is
simply any mixture that
is uniform in
composition
throughout, therefore
the different parts
cannot be seen.
(examples: koolaid,
lemonade, sweet tea)
• Heterogeneous - is
made of different
substances that remain
physically separate, so
the different parts are
seen.
(ex: trail mix, salads,
cereal)
Mixtures
• Solute – is the
smaller portion of
the mixture and
the part that is
being dissolved.
• Solvent – the
bigger portion of
the mixture and
the part doing the
dissolving.
Solutions
• Reading Essentials Book
• Page 378-382
• On your own paper
• Respond to questions in the
margins, except DO NOT DO THE
FOLDABLE!
Solutions
• A solution is a
mixture of two
or more
substances,
aka
homogeneous
mixture.
Solubility
• Saturated: describes a
solution that has
dissolved the
maximum amount of
solute
• Unsaturated: describes
a solution that has less
than the maximum
amount of solute
dissolved
• Supersaturated:
describes a solution
that has dissolved
more than the
maximum amount of
solute
Solutions
• Dilute - make (a
liquid) thinner or
weaker by
adding water or
another solvent to
it.
• Precipitate – a
substance is
deposited in solid
form from a
solution.
Solutions
• Scientist use the axiom
“LIKE DISSOLVES LIKE”
• Nonpolar solute dissolves
in a nonpolar solvent
• Polar solute dissolves in a
polar solute
• Electronegativity affects
solubility of solutions. If
you have nonpolar and
polar, your solute will not
dissolve.
• As you go from left to
right across the periodic
table electronegativity
increases.
Can a solution conduct
electricity?
• Electrolytes are
substances that
conduct electricity
when dissolved in
water.
• Nonelectrolytes
are substances
that don’t conduct
electricity when in
these states.
• Examples: NaCl
and Sucrose
What affects solubility rate of
solute?
• A. Temperature –
heat vs. room
temperature or
cold
• B. Surface Area –
compare small
area to large
area
• C. Agitation –
stirring, shaking
Solubility Curve
Solubility Curve
• What
temperature
would a solution
need to be to
dissolve 110kg of
solute?
Solubility Curve
• If a solution had
100kg of solute
dissolved in 80°C,
is it a saturated
solution?
Solubility Curve
• Which solute
is most
soluble at
10°C?
• How much
NaCl can be
dissolved in
90°C solvent?
Solubility Curve: Gases
• Affected by:
• Temperature
• Pressure
• Inverse
relationship
• Ex: O2 and lake
Create a foldable: Acids
and Bases
• Need 2 pieces of paper
• Fold one into the other,
create four flaps, then
staple the top two corners
Once you finish,
start on page 470
1-20
• 1. How Litmus paper/pH
paper works
• 2. List of household
Acids and Bases and
pH
• 3. pH scale with
numbers and labels
(weak acid, weak
Acids
base, neutral, strong
and
acid, strong base)
Bases
• 4. Acids and Bases
starts on
Facts
page 694
Litmus paper
• Changes colors in the
presence of acids and bases
• Litmus paper can be either
blue or red
• ABR – acids turn BLUE litmus
paper RED
• BRB – bases turn RED litmus
paper BLUE
pH paper
• pH paper is blotting paper that has been treated
with a mixture of different indicators. Each indicator
changes color over a different pH range.
pH scale
• pH is a measure of how
acidic or basic a solution is.
•The pH scale ranges from 0
to 14.
• Acidic solutions have pH
values below 7
• A solution with a pH of 0 is
very acidic.
• A solution with a pH of 7 is
neutral.
•Pure water has a pH of 7.
•Basic solutions have pH
values above 7.
pH scale
•A change of 1 pH unit represents a tenfold
change in the acidity of the solution.
•For example, if one solution has a pH of 1 and a
second solution has a pH of 2, the first solution is
not twice as acidic as the second—it is ten times
more acidic.
Household Acids
• Acids
0 - Hydrochloric Acid (HCl)
1.0 - Battery Acid (H2SO4 sulfuric
acid)
2.0 - Lemon Juice
2.2 - Vinegar
3.0 - Apples
4.5 - Tomatoes
6.6 - Milk
Household Bases
• Bases
7.4 - Human Blood
8.3 - Baking Soda (Sodium
Bicarbonate)
10.5 - Milk of Magnesia
11.0 - Ammonia
12.4 - Lime (Calcium Hydroxide)
13.0 - Lye
14.0 - Sodium Hydroxide (NaOH)
Acid & Base Facts: What is
an acid?
• An acid is a solution that has an excess
of H+ ions. It comes from the Latin word
acidus that means "sharp" or "sour".
• The more H + ions, the more acidic the
solution.
Acid & Base Facts:
Properties of an acid…
• Tastes Sour
• Conduct Electricity
• Corrosive, which
means they break
down certain
substances. Many
acids can corrode
fabric, skin, and
paper
• Some acids react
strongly with metals
• Turns blue litmus
paper red
Acid & Base Facts: Uses of
Acids
• Acetic Acid =
Vinegar
• Citric Acid = lemons,
limes, & oranges. It is
in many sour candies
such as lemonhead
& sour patch.
• Ascorbic acid =
Vitamin C which
your body needs to
function.
• Sulfuric acid is used
in the production of
fertilizers, steel,
paints, and plastics.
• Car batteries
Acid & Base Facts: What is
a base?
• A base is a solution that has an excess of OHions.
• Another word for base is alkali.
• Bases are substances that can accept
hydrogen ions
Acid & Base Facts:
Properties of a base
Feel Slippery
Taste Bitter
Corrosive
Can conduct
electricity. (Think
alkaline batteries.)
• Do not react with
metals.
• Turns red litmus
paper blue.
•
•
•
•
Acid & Base Facts: Uses of
Bases
• Bases give soaps,
ammonia, and many
other cleaning
products some of their
useful properties.
• The OH- ions interact
strongly with certain
substances, such as
dirt and grease.
• Chalk and oven
cleaner are examples
of familiar products
that contain bases.
• Your blood is a basic
solution.
Acid & Base Facts: AcidBase Reactions
• A reaction
between an
acid and a base
is called
neutralization.
An acid-base
mixture is not as
acidic or basic
as the individual
starting solutions.
• Acid + Base 
salt + water
Acid & Base Facts: AcidBase Reactions
• Each salt listed in
this table can be
formed by the
reaction between
an acid and a
base.
Acids vs. Bases Lab
• You will be in groups of 2-3 people
• Each group will have ONE answer sheet
• Each group will have one set of unknowns (one well
plate)
• Each group will have one set of test papers (red
litmus paper, blue litmus paper, and pH paper)
• Each UNKNOWN is to be tested with EACH PAPER!!!!
(so test it once with the red litmus paper, once with
the blue litmus paper, and once with pH paper and
RECORD your FINDINGS AFTER EACH on your answer
sheet)
• Each group will need a paper towel, number the
paper towel so you can place each unknown’s test
strips in their respective place.
AFTER the LAB
• CLEAN UP YOUR MESS, I AM NOT
YOUR MAID!
• Complete page 470 1-20, will be graded
for accuracy and completion
• Complete page 690 1-18, will be graded
for accuracy and completion
Unknowns
•
•
•
•
•
•
•
•
•
•
1. lemon juice
2. coffee creamer
3. coke
4. green tea
5. dish soap
6. coconut milk
7. ammonia
8. windex
9. lysol cleaner
10. coffee
TODAY: 04.24.14
• Complete page 470 1-20, will
be graded for accuracy and
completion
• Complete page 690 1-18, will
be graded for accuracy and
completion
•REVIEW for TEST
04.25.14: TEST DAY
• Once finishing YOUR TEST, turn in
your test to the lab table (stack for
scantrons (A/B), stack for tests
(A/B))
• Turn in your textbook to Chapter 7
(page 192-199), read the section
and answer questions 1-5, bonus
points if you answer question 6
• NO TALKING UNTIL ALL TESTS and
WORK IS TURNED IN!