Warning

1
Warning!

• This program was designed to help you review your
  first semester of GHS Chemistry while learning
  about reactions
• It only gives brief information. Use your book
  for a more in depth review of the information you
  miss.
• Periodically there are sounds that are meant to
  be amusing but might be hurtful
• If you are sensitive please turn off the sound
  before you continue
• If you would like a specific topic to work on you
  can click in the upper left hand corner of any
  page and it will take you to an index page.
• Explore this program. There is a lot of
  information here. It can help you

I accept the responsibility of the above
information and I will not hold Galena High
School or any of its employees liable for any
damage that this program might do to me.
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I do not accept
Note This review has been done by a single
teacher. There are errors. Please email me at
ngreenhalgh_at_washoe.k12.nv.us if you find any
errors. I would greatly appreciate it.
2
Good Bye!
EXIT
3
Chemical Reaction Detour
On each page you will be given new information
that you are responsible for knowing. All words
in red must be in defined in the vocabulary
section of your notebook. Then you will be asked
a question on a topic previously covered in
class. A correct answer will allow you to
continue on your travels through reactions. If
you give a wrong answer you will be detoured.
Too many detours will probably hinder your
ability to completely grasp the new material. It
is recommended that you replay until you very few
detours.
What is the atomic mass of Oxygen?
15
15.9994
16
8
4
When a chemical reaction happens the substances
that go into the reaction are called reactants
and the substances that come out of the reaction
are called the products. The characteristics of
the products are completely different than the
characteristics of the reactants. For example,
chlorine gas (Cl2) is a yellow toxic gas that can
kill almost anything. Sodium (Na) is a shiny
silver metal that explodes violently in water.
Together they make salt, a white crystalline
structure, that is necessary for all living
organisms.
How many neutrons are there in an atom of
Sodium-24?
11
13
12
11.9898
5
A chemical equation is a symbolic representation
of a chemical reaction

• Coefficients-the small whole number preceding
  each formula telling how many of the units are
  needed to balance the equation. If there is no
  coefficient then only one of the units is needed
  to balance the equation.
• Formula-written according to the rules that you
  have learned
• Symbols-(g) gas, (s) solid, (l) liquid, (aq)
  dissolved in water, ? yields or reaction has
  happened, (?) product is a gas, used to
  separate the reactants or to separate the
  products.

Below is a balanced chemical equation for the
reaction of a piece of metallic zinc with
hydrochloric acid (remember that acids are always
aqueous). When mixed they will form the zinc
chloride and hydrogen gas.
Zn (s) 2 HCl (aq) ? ZnCl2 (aq) H2 (g)
Which formula above would have a formula unit as
its representative particle?
Zn
HCl
ZnCl2
H2
6
Types of Chemical Reactions

• There are five basic types of chemical reactions
• Combination- joining together
• Decomposition- breaking apart
• Single Replacement-a metal replacing a cation or
  a nonmetal replacing an anion
• Double Replacement-exchanging partners
• Combustion-burning a fuel

Which of the following is the correct Lewis Dot
Structure for Carbon Dioxide?
7
Combination Reactions

• A combination reaction is when two or more
  reactants are added together to form a single
  larger product. All combination reactions follow
  this basic format
• A B ? AB
• An example of this would be the formation of
  sodium chloride from sodium metal and chlorine
  gas
• 2Na(s) Cl2(g) ? 2NaCl(s)

What is the electron configuration for phosphorus?
1s22s42p43s23p3
1s22s22p63s23p64s23d104p1
1s22s22p63s23p3
1s22s22p83s23p1
8
Decomposition Reactions

• A decomposition reaction is when one larger
  substance is broken down into two or more smaller
  substances. One reactant means that it is a
  decomposition reaction. A decomposition reaction
  will always follow the format AB
  ? A B
• An example of this would be calcium carbonate
  breaking down into calcium oxide and carbon
  dioxide
• CaCO3(s) ? CaO(s) CO2(g)
• Or Nitrogen dioxide breaking to nitrogen gas and
  oxygen gas.
• 2NO2 (g) ? N2 (?) 2 O2 (g)

How many kilograms are there is 8.6 X 108
centigrams?
8.6 X 109
8.6 X 105
8.6 X 1013
8600
9
Single Replacement Reactions

• In a single replacement reaction, atoms of one
  element replace atoms of another element in a
  compound. A single replacement reaction will
  always follow the format
• A BC ? AC B
• Or
• A BC ? BA C
• An example of this would be the reaction of
  aluminum in an aqueous solution of Copper (II)
  chloride.
• 2Al (s) 3CuCl2 (aq) ? 2AlCl3 (aq) 3Cu (s)

What is the correct name for Mn3(PO4)4?
Manganese phosphate
Manganese(III) phosphate
trimanganese tetraphosphate
Manganese (IV) phosphate
10
Single Replacement
The more aggressive dog will chase out the less
aggressive dog, the more reactive metal will
chase out the less reactive metal. If you analyze
the following reaction carefully you will see
that the copper is a neutral atom in the
beginning and a cation in the end. Therefore it
lost an electron. The silver was a cation in the
beginning and a neutral atom in the end so it
gained an electron. In single replacement
reactions one element loses electrons (oxidation)
and one element gains electrons (reduction).
Cu (s) AgNO3 (aq) ? CuNO3 (aq) Ag (s)
Atoms are to elements as _______ are to ionic
compounds.
atoms
molecules
formula units
Representative particles
11
Activity Series
Activity Series of Metals

• Whether one metal will replace another metal in a
  compound is determined by comparing their
  relative activities (see the activity series).
  If the incoming element is more active (higher)
  than the element already in the compound it will
  replace it! The activity series for Metals is on
  P. 217 in your book.

In a reaction between zinc and calcium chloride,
what will the products be?
No reaction will happen
Zinc chloride and calcium
Zinc calcium and chlorine
Zinc and calcium chloride
12
You need to try a little harder

• Go through it one more time!

One more time!
13
Double Replacement Reactions

• Similar to the single replacement reaction, in
  the double replacement reaction the positive ions
  are exchanged between two compounds. A double
  replacement reaction will always follow the
  format
• AB XY ? AY XB
• Changing dancing partners. The positive of the
  first gets together with the negative of the
  second.

Metal atoms _____electrons to become ____ions and
nonmetal atoms _____ electrons to become ______
ions.
Gain, negative, lose, positive
Gain, positive, lose, negative
Lose, positive, gain, negative
14
Acid Base ? Salt Water

• A special type of double replacement is an acid
  base neutralization.
• Hydrochloric acid plus sodium hydroxide
  (hydroxides are bases) will yield salt water.
• HCl (aq) NaOH (aq) ? NaCl (aq) HOH (l)
• All ionic compounds are called salts in chemistry
• It is easier to balance if you leave the water as
  HOH

Name the following substance. HNO2
Hydronitric Acid
Nitric Acid
Nitrous Acid
Hydronitrous Acid
15
Combustion Reactions

• A combustion reaction involves oxygen reacting
  with another substance to produce energy in the
  form of heat and light. The reactants in
  combustion reaction are hydrocarbons (substances
  made up of hydrogen and carbon) and oxygen. The
  complete combustion of a hydrocarbon produces
  water and carbon dioxide. An example of this
  would be the burning of methane
• CH4(g) 2O2(g) ? CO2(g) 2H2O(g) heat light

What is the density of an object with a volume of
32 cm3 and a mass pf 96 g?
3072 g/cm3
3 g/cm3
.3333 g/cm3
6 g/cm3
16
Significant Figures
The accuracy of any measurement is limited by the
precision of the tool used to measure. For
example if you have a meter stick that is only
divided in to cm units you can estimate that it
is .2 or .5 of a cm but you cannot measure the
length of an object and say that it is 12.18256
cm. Your measuring device will not allow that
degree of accuracy. In measurements and in the
calculations that you make with those
measurements it is critical that you do not imply
more accuracy than you actually knew. Therefore
it is imperative that you follow the Sig Fig
rules when dealing with numbers other than
counted numbers (number of atoms in a mole, or
the number of milliliters in a liter).
I
Next
17
Quick Significant Figure Rules

• Digits from 1-9 are always significant.
• Zeros between two other significant digits are
  always significant
• One or more additional zeros to the right of both
  the decimal place and another significant digit
  are significant.
• Zeros used solely for spacing the decimal point
  (placeholders) are not significant. 

How many significant figures are there in 2100 km?
1
2
3
4
18
More on Sig Figs
RULE 1 - All digits 1 through 9 are significant
If the mass of an object is measured as 12.3 g,
this means that the mass is known to lie between
12.2 and 12.4 g. There are 3 significant figures
in 12.3. If the mass of an object is measured as
12.3456 g, this means that the mass is known to
lie between 12.3455 and 12.3457 g. There are 6
significant figures in 12.3456.
RULE 2 - Zero is significant when it is between
two non-zero digits. The quantities 306, 30.6,
3.06 and .306 all contain 3 significant figures
since the 0 between the 3 and 6 is significant.
RULE 3 - A terminal zero to the right of a
decimal point in a number greater than one is
significant. The quantities 279.0, 27.90 and
2.790 all contain 4 significant figures.
RULE 4 - A terminal zero to the right of a
decimal point in a number less than one is
significant. The quantities .2790 and .27900
have 4 and 5 significant figures respectively.
RULE 5 - A zero used to fix a decimal point in a
number less than one is not significant. The
quantities 0.456, 0.0456, 0.00456 and 456000 all
contain 3 significant figures.
How many sig figs are there in 10400.0?
2
4
5
6
19
Sig Figs with addition subtraction

• SIGNIFICANT FIGURES ADDITION AND SUBTRACTION
• When adding and subtracting numbers with
  consideration for significant figures, line up
  decimals and add or subtract as normal. Then,
  look at the numbers which you added or
  subtracted. Whatever the least number of digits
  that are present in those added or subtracted
  numbers, to the right of the decimal, that must
  be the same number of digits to the right of the
  decimal in your final answer. You round off to
  get those digits. Notice that the only
  consideration is to be those digits which are to
  the right of the decimal in the added or
  subtracted numbers.
• Example 19.3 6.09 .2 207.0 10
• 19.3 6.09 .2 207.0 10
• 242.59 243
• Note that in the above example, in the final
  number being added (10) there are no digits to
  the right of the decimal. (In fact, there is no
  decimal.) Therefore, your final answer should
  have no digits to the right of the "decimal
  position."
• Example 1.987 10.6 10.23 10.921
• 1.987 10.6 10.23 10.921
  33.738 33.7
• Note that in this example, the least number of
  digits in the added numbers is one digit (in the
  10.6.) Therefore, the final answer should have
  only one digit to the right of the decimal
  position.

Quiz Me!
20
Perform the following calculations. Express the
answer to the answer to the correct number of
significant figures.
3021.68048
3021.68
3021.68 4.80 X 10-4
3022.16
3069.68
21
Sig Figs for Multiplication and Division
When multiplying and dividing numbers with
respect to significant figures, you look at the
total number of digits that are present in each
figure being multiplied or divided. Then, you
note the number with the least total significant
digits. When you obtain your final answer, round
so that you have an answer with equal digits as
the lowest number of digits present in any given
number. Example 20.1 x 10.111 203.2311 203
Note that you round the final answer off so that
you have 3 digits in it. 20.1 had three digits
and you have in the final answer, digits equal to
the least number of digits in any given number
being multiplied or divided. Example 100 x
1000.23 100023 In this case, according to the
significant figure rules for zeros, in the 100
there is only 1 significant figure. Therefore,
your final answer must have only one digit in it
Rounding 100023 1, but there is no sensible
way that 100023 equals 1. What, then, do you do?
You place the answer in scientific notation, so
that the correct place value is held and you can
at the same time hold the correct number of
significant figures. 100023 1 x 105 or 100,000
Quiz Me!
22
The distance across the country is 3000 miles.
If you travel at a constant speed of 71.325
miles/hour, how long will it take you to travel
across the country?
42.061 Hours
40.00 Hours
40 Hours
42 Hours
23
That is not Right!

• The number 3000 has only one significant figure.
• That is the lowest number of significant figures
  of all factors
• The lowest number of significant figures
  determines the number of significant figures that
  can be expressed in the answer

I will learn the rules.
24
Way to many Sig Figs!

• Your answer has 6 significant figures
• 3000 only has one
• It is wrong to express your answer as a number
  that is more accurate than one of the numbers
  used to calculate that number
• An answer is only as strong as the weakest link

I will learn the rules.
25
You better learn Sig Figs!

• Your answer contains 2 significant figures
• 3000 miles only has one significant figure
• Your answer can be no more significant than your
  weakest number
• Try again

Let me review!
26
Scientific Notation
Scientific notation is simply a method for
expressing, and working with, very large or very
small numbers.  It is a short hand method for
writing numbers, and an easy method for
calculations.  Numbers in scientific notation are
made up of three parts the coefficient, the base
and the exponent.  Observe the example below  
5.67 x 105 This is the scientific notation for
the standard number, 567 000.  Now look at the
number again, with the three parts
labeled.             5.67 x 105
                                         
coefficient          base  exponent    In order
for a number to be in correct scientific
notation, the following conditions must be true
1. The coefficient must be greater than or equal
to 1 and less than 10. 2. The base must be 10.
3. The exponent must show the number of decimal
places that the decimal needs to be moved to
change the number to standard notation.  A
negative exponent means that the decimal is moved
to the left when changing to standard notation. 
Tell me more!
27
More about scientific notation

• A negative exponent means that the actual number
  is a decimal (fraction)
• A positive exponent means that the actual number
  is a large number
• When putting a number that is in scientific
  notation in your calculator put in the
  coefficient, then find the EXP or EE button,
  press it. Put in the exponent. If negative put
  the /- or the (-) button (not the subtraction
  button).
• Never Never Never put times 10. The calculator
  will do that for you.
• It is a number not an operation. Do not expect
  the calculator to do anything with that number
  until you tell it to.

Quiz Me!
28
What is the actual number?
.0000000078
7.8 X 10-9
7800000000
.000000009
.00000000078
29
Use your calculator the following
4.0 X1014
400

• 4.8 X 108 1.2 X 10-6

4.0 X10-14
.0040
30
Moles

• All calculations involving atoms so far have
  dealt with terms that are defined in relation to
  infinitesimally small particles atomic number
  relates to the number of protons mass number
  relates to the number of protons and neutrons an
  amu is a mass unit that chemists came up with so
  that they would have a unit that would work
  conveniently on the minute masses that they deal
  with. Rather than always dealing on ant atomic
  scale, chemists often find it useful to work with
  a unit that represents a large collection of
  atoms. Such a unit serves as a bridge between
  the invisible world of atoms and the macroscopic
  world of the materials and objects that we deal
  with every day. A mole is a collection of
  6.022137 X 1023 (602213700000000000000000)
  pieces. This large number was named in honor of
  Amadeo Avogadro and is commonly called Avogadros
  number. In theory you could have a mole of
  anything but most things are too large and it
  would be very impractical if not impossible to
  have a mole of. But atoms, molecules and formula
  units are ideal size to obtain a mole of them.
  Determine the weight of a mole, the weight has no
  bearing on whether something is a mole or not.
  Every mole in existence has 6.02 X 1023 chemical
  units. Just like every dozen has exactly 12
  units in it. The chemical units contained in a
  mole are 1) atoms if we are dealing with an
  element 2) molecules if we are dealing with a
  compound with covalent bonds, where the chemical
  formula describes an exact molecule and 3)
  formula units, if the substance is ionically
  bonded. In ionic substances, it is impossible to
  describe an exact molecule, since the positive
  and negative ions can cling together in any
  numbers. A formula unit is the smallest whole
  number ratio that they can be attracted to make a
  neutrally charged compound.

Tell me more!
31
Fill in the following blanks and then write a
paragraph describing why the number 6.022137
X1023 is the number that has been
internationally accepted by chemists for over 140
years.
I understand!
If you have the same number of atoms of hydrogen
and carbon the ratio of their masses will be
112. Since the ratio of 1 gram of hydrogen and
12 grams of carbon is still the the same 112
mass ratio isnt it logical that there must be
the same number of atoms in those masses? What
is that number? Fill in the following
dimensional analysis problem and solve to answer
that question.
6.02 X 1023
6.02 X 1023
32
Moles

• How many is a "couple? (2)
• How many in "one dozen"? (12)
• How many is a "few"? (3)
• How many sodas in one case? (24)
• How many are in one "gross"? (144)
• How many atoms are in a mole? (6.02 X1023)
• How many molecules are in a mole? (6.02 X1023)
• How many formula units are in a mole? (6.02
  X1023)
• Atoms-Molecules-Formula Units are called
  Representative Particles

Tell me more!
33
Molar Mass

• For an element-the molar mass is the atomic mass
  in grams
• For a molecule or a formula unit, the molar mass
  is the sum the atomic mass of all the atoms in
  the formula.
• For Example Water is H2O One mole of water will
  weigh
• 2 H _at_ 1.00797 2.01594 grams
• 2 O _at_ 15.9994 15.9994 grams
• Molar Mass H2O 18.0153 grams

Tell me more!
34
3 Molar Equalities

• To be used in Dimensional Analysis
• 6.02 X 1023 representative particles 1 mole
• Molar Mass (grams) 1Mole
• 22.4 Liters of a gas at STP 1 mole

Tell me more
35
Next
36
Examples

• How many grams are there in 8.4 X1018 molecules
  of Carbon Dioxide?

.000614 grams
Let me try!
37
Remember a mole of any gas at STP will occupy a
volume of 22.4 Liters

• 43 grams of Argon at STP (standard temperature
  and pressure) will occupy what volume in liters?
• Convert to moles first.

22.4 Liters
7.14 X 10-23 Liters
24.08 Liters
1.075 Liters
38
The Periodic Table of Elements

• The PTOE is named because the characteristics of
  the elements repeat periodically.
• When the elements that have similar
  characteristics are grouped together the PTOE is
  created.
• The Roman Numerals at the top of each column tell
  the number of valence electrons
• 1-7 next to family 1 tell the number of energy
  levels.
• The s, p, d, and f blocks tell the orbital that
  the electrons will likely be found.
• Families are the columns
• Periods are the rows

I know this information
39
Periodic Trends-Atomic Radius

• Atomic radius is simply the radius of the atom,
  an indication of the atom's volume.
• Period - atomic radius decreases as you go from
  left to right across a period.
• Why? Stronger attractive forces from the nucleus
  as you go from left to right. The positive charge
  of the protons in the nucleus pulling on the
  electrons cause the atom to be 'sucked' together
  a little tighter. Additional electrons are added
  in the same or lower energy levels.
• Family - atomic radius increases as you go down a
  group.
• Why? There is a significant jump in the size of
  the nucleus (protons neutrons) each time you
  move from period to period down a family.
  Additionally, new energy levels of elections
  clouds are added to the atom as you move from
  period to period down a family, making each atom
  significantly larger, both in mass and volume.

Ive got it!
Ive got it!
40
Periodic Trends-Ionic Radius

• Cations are positive ions. The are made when
  metal atoms lose their valence electrons, to
  attain the electron configuration of the previous
  Noble Gas. All of the Noble Gases have 8 valence
  electrons. Metal atoms lose their entire valence
  energy level in order to have 8 valence
  electrons. Since the outer most energy level is
  gone the ion is smaller than its parent atom.
• Anions are negative ions. They are made when
  non-metals gain electrons to attain the magic
  number of 8 valence electrons. Since they are
  gaining negatively charged particles, the ion
  will have a negative charge. Since there are
  more electrons than there are protons the pull of
  the protons is not as strong and therefore the
  anion is larger than its parent atom.

Tell Me More!
41
Periodic Trends-Nuclear Charge

• The Effective Nuclear Charge is the pull that the
  positively charged protons in the nucleus have on
  the negatively charged electrons. The greater
  the number of protons the greater the ability to
  pull in on the electrons.
• Period The nuclear charge increases as you
  proceed from left to right in any given period.
• Why? The energy level of the outer orbitals
  remains constant while the number of protons
  increases. This increase in nuclear charge is
  what causes the radius of the atom to decrease as
  you proceed from left to right across a period.
• Family As you move down a family the number of
  energy levels in the atoms increased.
• Why? The increase in the number of energy levels
  has a greater impact on the volume of the atom
  than the greater pull caused by additional
  protons in the nucleus.

Tell Me More
42
Periodic Trends-Ionization Energy

• Ionization Energy is the energy required to
  remove the outermost electron from an atom. It is
  an atom that is all by itself, not hooked up to
  others in a solid or a liquid. When enough energy
  is added to an atom the outermost electron can
  use that energy to pull away from the nucleus
  completely, leaving behind a positively charged
  ion. That is why it's called ionization because
  one of the things formed in the process is an
  ion. The ionization energy is the exact quantity
  of energy that it takes to remove the outermost
  electron from the atom.
• Period - ionization energy increases as you go
  from left to right across a period.
• Why? Elements on the right of the chart want to
  take others atom's electron (not given them up)
  because they are close to achieving the octet.
  The means it will require more energy to remove
  the outer most electron. Elements on the left of
  the chart would prefer to give up their electrons
  so it is easy to remove them, requiring less
  energy (low ionization energy).
• Family - ionization energy decreases as you go
  down a group.
• Why? More energy levels in an atom, the further
  the distance from the protons in the nucleus.
  This makes it easier to remove the outer most
  electrons from those atoms that have many
  electrons (those near the bottom of the chart).

Electronegativity Is Next!
43
Periodic Trends-Electronegativity

• Electronegativity is a measure of the attraction
  of an atom for electrons within a bond.
• Fluorine, the most reactive non-metal, is
  assigned the highest value since it has the
  greatest attraction for the electron being shared
  by the other element. Oxygen is also highly
  electronegative and has a strong attraction for
  electrons. Metals have low electronegativities
  since they have weak attraction for any shared
  electrons.
• When two unlike atoms are covalently bonded, the
  shared electrons will be more strongly attracted
  to the atom of greater electronegativity. Such a
  bond is said to be polar. A polar bond results in
  the unequal sharing of the electrons in the bond.
  Electronegativity increases as you move from left
  to right within a period and decreases as you
  move down a family. Ionic bonds occur when the
  difference in the electronegitivity is so great
  that the electron is completely transferred.
• Why? Moving across a period increases the number
  of protons while the electrons are not getting
  any farther from the nucleus.
• Electronegativity decreases as you go down a
  family because the valence electrons are further
  away from the pull of the nucleus.
•  

Next
44
Periodic Trends
I know Periodic Trends
45
Lets review reactions!
Now it is up to you to identify the type of
reaction shown in each of the following chemical
equations. Just click on the button next to your
answer. If you get it right you will get to move
on to the next problem. If you choose
incorrectly you shall be publicly humiliated and
sent back to the proper section to review. Each
time you are sent back you must start the
problems over from the beginning!
Bring it on!
46
Chemical Reactions

• Identify the type of reaction shown below
• C2H6 O2 ? CO2 H2O heat light
• Combination
• Decomposition
• Single Replacement
• Double Replacement
• Combustion

47
Chemical Reactions

• Identify the type of reaction shown below
• C(s) O2(g) ? CO2(g)
• Combination
• Decomposition
• Single Replacement
• Double Replacement
• Combustion

48
Chemical Reactions

• Identify the type of reaction shown below
• Fe (s) Sn(NO3)2 (aq) ?Fe(NO3)2 (aq) Sn (s)
• Combination
• Decomposition
• Single Replacement
• Double Replacement
• Combustion

49
Chemical Reactions

• Identify the type of reaction shown below
• H2CO3(aq) ? CO2(g) H2O(l)
• Combination
• Decomposition
• Single Replacement
• Double Replacement
• Combustion

50
Chemical Reactions

• Identify the type of reaction shown below
• Pb(NO3)2(aq) 2KI(aq) ? PbI2(s) 2KNO3(aq)
• Combination
• Decomposition
• Single Replacement
• Double Replacement
• Combustion

51
Great Job!
Click Here
52
Choose Topic to Review
Representative Particles
Combination Reactions
Number of Neutrons
Moles
Electron Configuration
Lewis Dot Structures
Decomposition Reactions
Interactive Compound Naming Chart
Dimensional Analysis
Metric System
Single Replacement
Significant Figures
Naming Compounds
Density
Double Replacement
Scientific Notation
Atomic Mass
Acids Bases
Combustion Reactions
Periodic Table
Exit
Click in the upper left hand corner of most pages
to return to this page.
53
Youve been detoured. You need to review Atomic
Mass.
Click here
54
Atomic Mass -the average mass of all the isotopes
of an element, weighted by how commonly they
occur in nature

• Atomic mass is a weighted average
• If one isotope is more common in a sample then
  its weight will be counted more often
• The same way that tests scores are weighted more
  heavily than other scores in your grade
• An atomic mass will have several numbers after
  the decimal point
• Look at your Vegium Lab or P. 118-122 in your
  book for a more in depth review

An element contains 3 isotopes, Goofium-26 is 4
of all goofium, Goofium-27 is 2 of all Goofium
and Goofium-28 is 94 of all Goofium. The atomic
mass would have numbers behind the decimal point.
Which whole number would the atomic mass of
Goofium most likely round to?
26
27
28
27.9
55
Wrong! Lets go back and review
Click Here!
56
Determining the Number of Neutrons
The mass number of an atom is the equal to the
number of protons plus the number of neutrons.
Since it is a counted number it will always be a
whole number. When determining the number of
neutrons in an atom you must first determine the
mass number of the atom. The example that you
just missed, you were given a specific isotope,
that is the mass number of the atom followed the
name of the atom. You then subtract the number of
protons (the atomic number) from the mass number
to get the number of neutrons. If you are not
given the mass number behind the name then you
will us the most common isotope which is
determined by rounding the atomic mass to the
nearest whole number and then subtract the number
of protons in the atom.
How many neutrons are there in the most common
isotope of Iron?
30
26
29.847
56
57
Wrong! Lets go back and review representative
particles.
Click Here!
58
Representative Particles - smallest unit into
which a pure substance can be broken into without
a change in its composition.

• Formula Unit-if it is the smallest unit of an
  ionic compound (metal-nonmetal combination)
• Molecule-if it is the smallest unit of a covalent
  compound (two nonmetals bonded together
• Atom-if it is the smallest unit of an element

What is the representative particle for Silicon?
Atom
Molecule
Formula Unit
Unit
59
Wrong! Lets go back and review...
Click Here!
60
Lewis Dot Structures

• Determine the number of valence electrons in each
  atom in the formula
• Add them up to determine the total number of
  valence electrons in the molecule
• Write the chemical symbol for the central atom
  (the atom that there is only one of or the middle
  if there are 3 elements
• Write the symbol for each of the other atoms
  equally surrounding the central atom
• Draw a dash, representing a single covalent bond
  between the central atom and each of the
  surrounding atoms
• Show dots to complete the octet of each of the
  atoms bonded to the central atom
• Count each dash as two and each dot as one and
  determine the total remaining electrons to place.
• Place all remaining electrons around the central
  atom
• If there are not enough electrons to make an
  octet around the central atom form double bonds
  until all atoms have an octet around them
• Sometimes the central atom will have more or less
  than an octet

Every atom in a bond is trying to have ______
valence electrons.
16
8
2
4
61
Wrong! Lets go back and review electron
configuration.
Click Here!
62

• Start from element 1, continue until you get to
  the element that you are doing the electron
  configuration for.
• State the Energy Level (the same as the row that
  it is in on the Periodic Table).
• State the letter representing the orbital as
  shown in the chart. For ex. Hydrogen is 1s
• Count all the boxes in that energy level and
  orbital. Place that number as a superscripted
  number after the orbital letter.
• Add up all the superscripted numbers and make
  sure that they are the same as the atomic number
  of the element.

What is the electron configuration for chlorine?
1s22s42p43s23p5
1s22s22p63s23p64s23d104p5
1s22s22p63s23p5
1s22s22p83s23p3
63
Five d orbitals exist at all energy except the
1st and 2nd. Each d has 4 lobes and is oriented
around the 4 planes shown above. The 5th d
orbital has a very unique shape
s, p, d, and f Orbitals
An orbital is a region in space with a high
probability that up to two electrons will be
found there. The shape of these orbitals is
determined by Laws of Physics. The pull of the
nucleus on the electrons, the repulsive forces of
the other nearby electrons, the space available,
and the energy of the electron itself all play a
part in the shape of these orbitals. The s
orbital is simply a sphere. The s orbital at the
first energy level is a smaller sphere than the s
orbital at the second energy level and so on.
Below are diagrams of the p and the d orbitals
which are more complicated than the s orbitals.
Three p orbitals exist at all energy except the
1st. Each p shaped orbital is oriented around the
x, the y, and the z axis in space.
I recognize the orbitals
64
Another way to write the electron configuration
of an atom is to simply start at the top of the
figure to your left. Follow each arrow down and
then start do the same with the arrow below.
Write down exactly what is in each box in the
order that the arrows tell you to go. Add up the
superscripted numbers until they total the atomic
number of the element that you are writing the
configuration for. You will adjust the last
number so that the total number of electrons in
the atom.
What is the electron configuration for magnesium?
1s22s42p43s2
1s22s22p63s23p64s23d4
1s22s22p63s2
1s22s22p83s2
65
This is scary! You should know your metric
conversions by now.
Click here to Review
66
You must Know These!!!
By putting each of the BU from the box on the
right into both sides of the metric prefix
equalities you can make 12 different equalities.
A conversion factor is simply an equality put in
to a fraction form. Since either side of the
equality can be the denominator or the numerator
the 12 equalities can make 24 conversion factors,
with very little memorizing.
Click the button below that shows to equal
conversion factors derived from the above
equalities.
B
A
67
There are 1000 meters in a kilometer not 1000
kilometers in a meter. That is like saying that
there are 5280 miles in a foot instead of saying
there are 5280 feet in a mile.
I will try harder!
68
Dimensional Analysis

• Choose the given from the problem. It is the
  number and unit that you are to change to another
  unit.
• Place that number in the top of the first space
  on your dimensional analysis table
• Choose a conversion factor that has the same unit
  as the given in the denominator of the Conversion
  Factor.
• When then same units are on the top and the
  bottom they can cancel.
• Then find a new conversion factor that will
  cancel with your new number until you arrive at
  the unit the question asks for.
• In Metric Conversions there will never be more
  than a given and 2 conversion factors.
• Multiple everything on the top and divide by
  everything that is on the bottom. (You must hit
  the divide button on your calculator every time
  before you put in number that are on the bottom.

How many decigrams are there in 76 kilograms?
The grams and the kilograms cancel leaving
decigrams as the answer.
7.6 X 10-3 dg
7.6 X 103 dg
7.6 X 105 dg
7.6 X 10-5dg
69
Woops! This is a biggie! You better study hard!
I cant believe you missed this!
70
Naming Compounds

• If only 2 elements name will end in ide
• If the first element is a metal there will be no
  prefixes.
• If there are more than 2 elements then it will
  end in ite or ate.
• If the metal is a transition or a Family IV metal
  you will need a Roman Numeral in parenthesis
  after the name of the metal.
• If the first element is a nonmetal you will use
  prefixes telling the of atoms of each there are
  in the formula.
• No prefix if only 1 of the first element.
• Mono, di, tri, tetra, penta, hexa, hepta, octa,
  nona, and deca
• There are 3 covalent compounds but you are not
  responsible for knowing how to name them.

Name the following compound. Cl2O7
Chlorine oxide
Dichloride heptoxide
Dichlorine heptoxide
Chloride oxide
71
Use this chart to name the following compounds
Click on various parts of the chart for more
explanation
H3PO4 N2O5 Mn2O7 CaSO4 Fe3(PO4)2
Click here to check your answers
72
Back
73
Answers

• Phosphoric Acid
• Dinitrogen pentoxide
• Manganese (VII) oxide
• Calcium Sulfate
• Iron (II) phosphate

What is the Name of Al(OH)3 ?
Aluminum Triosygenhydride
Aluminum Hydroxide
Aluminum Trihydroxide
Aluminum Hydrate
74
Roman Numerals

• Transition Metals and Family IV metals have
  charges that vary
• The name of all compounds containing these metals
  must contain a roman numeral to tell what the
  charge is on the cation in this compound
• You determine the Roman Numeral by using algebra
• Assign an X as the charge for the variable
  charged cation if there is more than one you must
  multiply the X by the number of the cations in
  the formula
• Add that to the total charge of the anion(s)
• Set the total to zero and solve for X
• For example Name Co2(SO4)3
• 2X 3(-2) 0
• 2X -6 0
• 2X 6
• X 3
• Cobalt (III)
  Sulfate

Back to Naming Chart
What is the name of the following compound?
Mn2(CO3)3
Manganate Cobalt
Magnesium carbonate
Manganese(II)Carbonate
Manganese(III)Carbonate
75
Naming Covalent Compounds

• Use prefixes to tell how many atoms of each
  element are in the compound. Mono, di, tri,
  tetra, penta, hexa hepta, octa, nona, deca.
• Do not use a prefix if there is only 1 atom of
  the first element ex. Carbon Monoxide
• Change the ending on the second element to ide
• Covalent compounds are made up of 2 or more
  nonmetals.

Name the following. N2O4
Back to Naming Chart
76
I thought that you knew this stuff!
I promise I will Learn all about representative
particles
77
Representative Particles - smallest unit into
which a pure substance can be broken into without
a change in its composition.

• Formula Unit-if it is the smallest unit of an
  ionic compound (metal-nonmetal combination)
• Molecule-if it is the smallest unit of a covalent
  compound (two nonmetals bonded together
• Atom-if it is the smallest unit of an element

What is the representative particle for the
compound carbon monoxide?
Atom
Molecule
Formula Unit
Unit
78
Finals are coming! You better study.
I will never procrastinate on studying again.
79
You have been detoured. Lets review ions.

• Protons are positive and electrons are negative
• Protons are equal to electrons in an atom or a
  molecule. They are neutral by definition.
• If an atom or a molecule loses an electron it
  will have more positive protons than negative
  electrons, therefore it will be a cation. A
  molecule would become a polyatomic cation.
• If an atom or a molecule gains an electron it
  will have more negatives than positives. It will
  be a negative ion or an anion. If it is a
  molecule it will be a polyatomic anion.

A nonmetal atom will gain electrons until it has
an octet (8 valence electrons). It will become
a_____?
Polyatomic cation
Polyatomic anion
Monatomic cation
Monatomic anion
80
Only Three Rules for Naming Acids
Acid Naming
81
Acid Naming Formula Writing

• Acids start with a Hydrogen as a positive
  hydrogen ion
• The number of hydrogen atoms needed is determined
  by the charge on the anion, the positives must
  equal the negatives.
• The ending of the anion will determine the name
  of the acid.
• Anion ending Acid Name
• ide Hydro Anion
  Root ic Acid
• ate Anion Root
  ic Acid
• ite Anion Root
  ous Acid

Back to Naming
Name the following compound. HBr
Hydrobromic Acid
Hydrobromous Acid
Bromic Acid
Bromous Acid
82
Wrong! Lets review Density
I am not Dense!
83
Mass Volume

• Weigh the object to determine the mass in grams
• Calculate the volume usually in cm3 or mL
• By measuring and calculating if it is a regular
  shaped object
• By water displacement if the object is irregular
  in shape
• Divide the Mass by the volume and label the
  answer in g/cm3 or g/mL.
• Objects that have a density greater than 1 will
  sink and less than 1 will float

What is the mass of goofium it has a density of
1.6 g/cm3 and a volume of 14.4 cm3?
24 g
9 g
23.04 g
14.4 g