Honors Physical Science
Chemistry: Bell Work, Notes, Study Guides
Mr. Banker
Fall 2014
[email protected]
http://wandohigh.ccsdschools.com/directory/science/banker_ian/physical_science/
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Table of Contents
Bell Work……………………………………..……………………………..…………………………………. First 4 pages
Periodic Table ………………………..…………………………………..……………………… Following Bell Work
Syllabus ….…………………………….………………………………..………………………Following Periodic Table
Unit 1A.1: Metric System ......................................................................................................... 3
Unit 1A.2: Scientific Notation .................................................................................................. 5
Unit 1A.3: The Nature of Science ............................................................................................. 7
Unit 1B.1: States / Phases of Matter ....................................................................................... 9
Unit 1B.2: Gas Laws ............................................................................................................... 11
Unit 1B.3: Composition of Matter ......................................................................................... 13
Unit 1B.4: Chemical vs Physical: Properties and Changes ..................................................... 15
Unit 1B.5: Density .................................................................................................................. 17
Unit 2.1: Atomic Structure ..................................................................................................... 19
Unit 2.2: Isotopes and Ions .................................................................................................... 21
Unit 2.3: Electron Arrangement............................................................................................. 23
Unit 3.1: Periodic Table of Elements ..................................................................................... 26
Unit 3.2: Oxidation Numbers and Bonding ............................................................................ 28
Unit 3.3: Bonding: Ionic and Covalent Bonds ........................................................................ 29
Unit 4.1: Balancing Chemical Reactions................................................................................. 31
Unit 4.2: Chemical Reactions: Energy .................................................................................... 33
Unit 4.3: Types of Chemical Reactions................................................................................... 35
Unit 4.4: Translation .............................................................................................................. 37
Unit 5.1: Solutions and Saturation Level ............................................................................... 38
Unit 5.2: Acids and Bases ....................................................................................................... 40
Unit 5.3: The Mole ................................................................................................................. 42
Study Guides: Unit 1 thru Unit 5 ..………………………………………….……………Following Each Unit
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Unit 1A.1: Metric System
Further Reference: 1.2 The Way Science Works and 1.3 Organizing Data
THE BASICS
1. The 7 SI base units and what each measures:
a. ______________ (__) – a measure of _____________________
b. ______________ (__) – a measure of _____________________
c. ______________ (__) – a measure of _____________________
d. ______________ (__) – a measure of _____________________
e. ______________ (__) – a measure of _____________________
f.
______________ (__) – a measure of _____________________
g. ______________ (__) – a measure of _____________________
2. Every measurement will include _________________________
PREFIXES
1. The prefixes from largest to smallest:
a. ______________ (__) : one ____________ is equal to 1000 meters
b. ______________ (__) : one ____________ is equal to 100 liters
c. ______________ (__) : one ____________ is equal to 10 grams
d. ______________ (__) : one ____________ is equal to 1/10 meters
e. ______________ (__) : one ____________ is equal to 1/100 liters
f.
______________ (__) : one ____________ is equal to 1/1000 grams
2. Remember, these ______________ are always added to the __________________
3. Bases in order:
a. ________ ________ ________ ________ ________ ________ ________
4. And to help you remember:
a. ________ ________ ________ ________ ________ ________ ________
CONVERTING UNITS
1. When you are converting from on unit to another, you:
a. First, _________________________________________________________
b. Then, ________________________________________________________
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2. If you move to the _____________ (aka: ______ to ______) the you move the
decimal to the _____________
3. If you move to the _____________ (aka: ______ to ______) the you move the
decimal to the _____________
PRACTICE PROBLEMS:
1. 1 meter = ________________ hectometers
K H Da B D C M
2. 2.5 kilograms = ________________ grams
K H Da B D C M
3. 17.504 deciliters = ____________ decaliters
K H Da B D C M
4. 2.16 grams = _________________ kilograms
K H Da B D C M
5. 3.2 liters = ____________________ centiliters
K H Da B D C M
6. 1 meter = ____________________ centimeters
K H Da B D C M
7. 9.3 decameters = _______________ millimeters
K H Da B D C M
PRECISION AND ACCURACY
1. Precision is __________________________________________________________
___________________________________________________________________
2. Accuracy is __________________________________________________________
___________________________________________________________________
3. Draw a picture of the following:
Not accurate and not precise
Not accurate, but precise
Accurate and not precise
both accurate and precise
4. Explain a scenario where you can be precise, but not
accurate.
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Unit 1A.2: Scientific Notation
Further Reference: 1.3 Organizing Data
SCIENTIFIC NOTATION
1. Scientific notation is the way of writing ____________ or ______________
numbers that are hard to express ______________________.
a. A number is written in Scientific notation with the following form:
i. _____ x_______
ii. Where C is between ______ and ______ and ______ is an integer
PRACTICE PROBLEMS: Circle the numbers that are written in correct scientific notation
2.35 x 105
2.1203 x 10-16
5 x 10-9
45.9 x 10-6
3.214 x 101
10.3 x 109
-78.3 x 1023
6.09 x 107
12 x 100
1.9 x 10-22
-4.89 x 108
LARGE NUMBER PRACTICE PROBLEMS: Decimal notation to scientific notation
Decimal Notation:
Scientific Notation:
123,000,000,000 =
_________________
45,000,000 =
_________________
67,800,000,000,000 = _________________
LARGE NUMBER PRACTICE PROBLEMS: Scientific notation to decimal notation
Scientific Notation:
Decimal Notation:
7.82 x 103
=
_________________________
3.04 x 108
=
_________________________
5 x 104
=
_________________________
Q1 – Which direction did the decimal move if you are going from Sci Notation to
decimal notation for a VERY LARGE NUMBER (more than 1)?
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SMALL NUMBER PRACTICE PROBLEMS: Decimal notation to scientific notation
Decimal Notation:
Scientific Notation:
0.000000034 =
_________________
0.0000000005609 =
_________________
0.000000000064 =
_________________
SMALL NUMBER PRACTICE PROBLEMS: Scientific notation to decimal notation
Scientific Notation:
Decimal Notation:
4.8 x 10-6
=
_________________________
1.2 x 10-2
=
_________________________
9 x 10-8
=
_________________________
Q2 – Which direction did the decimal move if you are going from Sci Notation to
decimal notation for a VERY SMALL NUMBER (less than 1)?
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Unit 1A.3: The Nature of Science
Further Reference: 1.1 Nature of Science and 1.2 The Way Science Works
SCIENCE
1. The goal of science is to ________________________________________________
2. Scientists hypothesize in order to _______________________________________
in a certain situation
a. Long held assumptions ___________________________
3. Question everything, but make ________________________________
a. You must be able to create ____________________ based on that question
SCIENTIFIC INQUIRY:
1) _________________________________________________________
2) _________________________________________________________
3) _________________________________________________________
a. Hypothesis = _________________________________________
4) _________________________________________________________
WITHIN THE EXPERIMENT:
a. Independent variable is __________________________________________
i. Example:
ii. There can be ___________________ independent variable
b. Dependent variable is ___________________________________________
i. Example:
c. Constants are _____________________________________________
i. Example:
d. Control group is _____________________________________________
i. Example:
e. Experimental group is___________________________________________
i. Example:
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f.
Scientists ________________________
i. Repeat the experiment to _________________________________
ii. Average the results to ___________________________
5) _________________________________________________________
a. Your data is ________________
b. Evidence is _______________________ NOT ________________________
c. Evidence can be ____________ or _____________________________
d. Quantitative data is _____________________________________________
i. 4 examples of quantitative data:
e. Qualitative data is ______________________________________________
i. 4 examples of qualitative data:
6) _________________________________________________________
a. Restate your ____________, and state whether your data _____________
or ______________ your hypothesis.
7) _________________________________________________________
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Unit 1B.1: States / Phases of Matter
Further Reference: 3.2 Changes of State
MATTER
1. Matter is ____________________________________________________________
2. The 4 states of matter are:
a. ___________________
b. ___________________
c. ___________________
d. ___________________
i. Each state of matter is designated by the _________________,
________________, and behavior of the __________________
3. Each state of matter has a different:
a. _____________________________________
b. _____________________________________
c. _____________________________________
d. _____________________________________
4. _______________ determines the kinetic energy ( and thus the _______________)
of a substance.
KINETIC THEORY OF MATTER
1. The Kinetic Theory of Matter: (AKA _____________________)
1. ___________________________________________________
2. ___________________________________________________
3. ___________________________________________________
STATES / PHASES OF MATTER
1. Solids:
a. Energy: _______________________________________
b. Movement: ___________________________________________________
c. Particle Spacing _______________________________________________
d. Volume Shape: ___________________ volume, ______________ shape
2. Liquids:
a. Energy: _______________________________________
b. Movement: ___________________________________________________
c. Particle Spacing _______________________________________________
d. Volume Shape: ___________________ volume, ______________ shape
3. Gasses:
a. Energy: _______________________________________
b. Movement: ___________________________________________________
i. Enough energy __________________________________________
c. Particle Spacing _______________________________________________
d. Volume Shape: ___________________ volume, ______________ shape
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4. Plasma is ______________________________________
a. Created at __________________________________
i. Seen in ____________________________
b. It is the most abundant state of matter ___________________________
i. NOT the most abundant ________________
CHANGES IN STATES / PHASES OF MATTER
1. Increase in energy:
a. _____________________________________________
b. _____________________________________________
2. Decrease in energy:
a. _____________________________________________
b. _____________________________________________
3. Melting point _________________________________________________
a. Example:
4. Freezing point _________________________________________________
a. Example:
5. Boiling point ___________________________________________________
a. Example:
6. condensation __________________________________________________
a. Example:
7. Sublimation ___________________________________________________
a. Example:
8. Deposition ____________________________________________________
a. Example:
PHASE CHANGE DIAGRAM
1. When changing from
solid to liquid, the
substance isn’t entirely
___________ until the graph
has a ____________ slope
2. At point A the substance is ___________________
3. At point B the substance is ___________________
4. At point C the substance is ___________________
5. At point D the substance is ___________________
6. At point E the substance is ___________________
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Notes for/from class
Unit 1B.2: Gas Laws
Further Reference: 3.4 Behavior of Gasses
GAS LAWS
1. Gasses have no definite ______________ or ____________.
a. BUT, there is a distinct relationship between _____________,
___________, and ___________ that holds true for all gasses.
2. Our 3 gas laws are
a. _______________ Law
b. _______________ Law
c. _______________ Law
d. For each law, one condition is held ________________, while the
other two conditions will __________________
GAS LAW EQUATION
1. Standard units for temperature _________________
2. Standard units for pressure _________________
a. What causes pressure?
3. Standard units for volume ___________________
BOYLES LAW:
1. If the _____________________ is held constant, the ______________ and
_____________ vary inversely.
a. Simply, as pressure __________ then volume __________
2. Equation ignoring the constant
3. List and explain 2 real world examples:
a. .
b. .
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CHARLES LAW:
1. If the _____________________ is held constant, the _____________ and
_____________ vary directly.
a. Simply, as temperature _________ then volume _________
2. Equation ignoring the constant
3. List and explain 2 real world examples:
a. .
b. .
GAY-LUSSAC’S LAW:
1. If the _____________________ is held constant, the ___________ and
___________ vary directly.
a. Simply, as pressure _________ then temperature ________
2. Equation ignoring the constant
3. List and explain 2 real world examples:
a. .
b. .
SOLVING PROBLEMS
1. Figure out ___________________________________
a. The law you are dealing with will dictate _______________
2. How can you remember which law keeps which variable constant?
________ ________ ________ ________ ________ ________
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Unit 1B.3: Composition of Matter
Further Reference: 2.1 Classifying Matter
MATTER
1. Matter is ____________________________________________________________
2. The two categories of matter are:
a. ___________________
b. ___________________
SUBSTANCES
1. The two categories of substances are:
a. ___________________
b. ___________________
2. Elements are _________________________________________________________
a. There are ___________ known elements, with ________ of them occurring
naturally.
b. It is only an element if _________________________________________
c. Element symbols are written with the 1st letter _______________, and the
2nd letter __________________
i. Ex: Hydrogen = _____ Carbon = _____
Calcium = _____
d. Atom is ______________________________________________________
i. All atoms for one element are ______________
3. Compounds are ______________________________________________________
a. They are ________________________________
i. Ex: CO2
H2O
NaCl C6H12O6
b. If you see 2 different _________________ written together with no spaces,
it is a ____________________
c. Physical processes ____________________ separate compounds
d. Compounds have a different _________________ and _______________
than the elements that make them up
e. Molecule is __________________________________________________
i. These atoms do not need to be ___________________________.
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Notes for/from class
1. Ex: H-H is a _______________. H2O is also a ____________
ii. Molecules are the ______________form of a compound that can
exist and still have the _____________________ of that compound
MIXTURES
1. Mixtures contain _____________________________________ that IS NOT
_______________________________ together.
2. Mixtures can be __________________________________________
3. The two categories of mixtures are:
a. ___________________
b. ___________________
4. Heterogenous Mixtures occur when matter is _____________________________
____________________________________________
a. Different parts have easily ____________________________
b. Example: ____________, ________________, _______________
c. CAN be ___________________________________
5. Homogenous Mixtures occur when matter is _____________________________
____________________________________________
a. Example: ____________, ________________, _______________
b. Homogenous mixtures are also called a __________________________
c. CAN be ___________________________________
RECAP
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Unit 1B.4: Chemical vs Physical: Properties and Changes
Further Reference: 2.1 Properties of Matter and 2.2 Properties of Matter
PHYSICAL
1. Physical properties are any observations that can be made ___________________
the composition of matter
b. Examples include:
i. _______________ _______________ _______________
ii. _______________ _______________ _______________
iii. __________________________ __________________________
iv. __________________________ __________________________
2. Physical changes are a change in ______________________________.
a. The identity of the element or compound ____________________
b. _________________ make or break bonds.
3. Examples include:
a. Any ________________________________ (________________________)
i. Rubbing alcohol ______________________________
ii. A juice box _____________________________
iii. Butter __________________________________
b. Any ________________________________ (________________________)
i. Aluminum foil ______________________________
ii. Clay _____________________________
iii. Chewing __________________________________
4. Signs of a Physical Change include:
a. Any ____________________
b. Change in the ______________________
c. What you started off with is __________________________________
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CHEMICAL
1. Chemical properties are any observations that are dependent upon
________________________________ of the object
a. Examples include:
i. __________________________ __________________________
ii. __________________________ __________________________
2. Chemical changes: The substances that are present at the beginning of the reaction
are ______________________________.
a. _________________ make or break bonds.
b. The change __________________
3. Examples include:
a. Gasoline _________________________________
b. Car _____________________________
c. Milk ____________________________
d. Bread _____________________________
e. Hydrogen peroxide __________________________________
f.
Food digesting ______________________________________________
g. Any ________________________________ (________________________)
4. Signs of a Chemical Change include:
a. Bubbles ____________________________
b. _______________ something.
c. A _____________ forms (solid appears)
d. A ____________________________
e. The ______________________ changes
f.
There is a different _______________________
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Unit 1B.5: Density
Further Reference: 2.2 Properties of Matter
DENSITY
1. Density is defined as ___________________________________
b. It is a measure of __________________________________ are in an object
c. Basically, it is the _________________________ within ________________
Equation in words
Equation in Symbols
Units:
Mass = _______________ (__)
Volume (2 ways)
Ruler = ___________________ (__)
Displacement = ___________________ (____)
Density (2 ways)
Ruler = ___________________ (__)
Displacement = ___________________ (____)
DIFFERENT OBJECTS HAVE DIFFERENT DENSITIES
1. Each substance __________________________________________
a. It does not matter _______________________________ you have, it will
have ______________________
b. Distilled water has a density of _________________________
c. Objects with different densities will always interact, with the more dense
object __________________ and the less dense __________________
2. Is Ice or Distilled Water more dense? ___________ because __________________
a. Objects with more than a density of ______________ will ____________ in
tap water
i. Example:
b. Objects with less than a density of ______________ will ______________
in tap water
i. Example:
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DETERMINING DENSITY
1. Step 1: __________________________________________
2. Step 2: __________________________________________
a. 2 ways to determine volume:
i. _______________________________
ii. _______________________________
3. Step 3: __________________________________________
PRACTICE PROBLEMS: Show: the formula, your work, and an answer, include units.
1. If the mass of an object is 35 grams and it takes up 7 cm3 of space, calculate the
density.
2. Osmium is a very dense metal. What is its density in g/cm3 if 50.00 g of the
metal occupies a volume of 2.22cm3?
3. What is the density (g/cm3) of 48 g of a metal if the metal raises the level of
water in a graduated cylinder from 25 mL to 33 mL?
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Due Date: ______________
Notes for/from class
Unit 2.1: Atomic Structure
Further Reference: 4.2 Structure of Atoms
THE ATOM
1. The atom is _________________________________________________________
d. It is the basic building block ______________________
e. The atom is made of the following 3 parts:
i. _______________, ___________________, _________________
4. The atom is composed of 2 parts: the ______________ and the ________________
a. The nucleus is ______________ charged
i. Contains ______________ and ______________
ii. Protons are _________________ charged
iii. Neutrons are _______________ charged
1. Neutrons act like____________ for the nucleus
b. The electrons are ______________ charged
i. Electrons occupy the ________________________ around the
nucleus
ii. Electrons are arranged into ____________ or ______________
iii. Electrons are _________ moving in _______________________
around the nucleus. Their movement is ___________________
iv. The electron cloud give us _____________________ location
Location
Charge
Mass
Special Fact
Protons
Neutrons
Electrons
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PROPERTIES OF ATOMS
5. Atomic number is __________________________________________________
a. Each element has its _________________________________________
b. In a NEUTRAL ATOM, this is also ________________________________
6. (Average) Atomic Mass is ____________________________________________
_________________________________________________________________
7. Mass number is the ________________________________________________
a. It is the sum of the ______________ and _____________ in the nucleus
b. Mass number = ___________________ + _____________________
8. Isotope Notation:
9. Isotope Name:
_____________________
PRACTICE WITH ELEMENT PARTS
Element
Symbol
Boron – 11
Atomic #
Protons
Neutrons
6
6
Mass #
B
Carbon – 12
Magnesium – 23
12
Copper – 64
29
23
35
20
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Unit 2.2: Isotopes and Ions
Further Reference: 4.2 Structure of Atoms
ISOTOPES
1. Isotopes are _________________________________________________________
a. Two isotopes of an element will have the same _________________ but
different _______________________ (and _____________________)
b. Looking at the carbon atoms to the right:
i. What is the mass number of the
carbon atom on the left _______
ii. What is the mass number of the
carbon atom on the right ______
iii. What is the atomic number of the carbon atom on the left ______
iv. What is the atomic number of the carbon atom on the right ______
2. Isotope notation you write the _________________ with the _________________
on the top left and the ___________________ on the bottom left
a. Write an example of carbon-14 __________________________
7
14
N
7
15
N
7
16
N
Protons
Neutrons
Electrons
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IONS
1. Ions are atoms or groups of atoms with a _____________ or a _____________
charge
a. Ions differ in the number of _____________
i. For neutral atoms are where the number of electrons are
____________ to the number of protons
ii. For ions, the __________ stay the same and the ____________ are
different. You can either _________ or ___________ electrons.
b. Examples of Neutral Atoms: _______, _______, _______, _______
c. Examples of Ions: ________, ________, ________, ________
2. Taking away an electron gives an atom a _____________ charge because there are
now more _______________
a. This is called a _______________
b. So if the Mg atom loses 2 electrons, it becomes _____________
3. Gaining an electron gives an atom a _____________ charge because there are now
more __________________
a. This is called a _______________
b. So if the F atom gains 1 electron, it becomes ________________
19
39
N+
8
16
N-2
20
41
N+2
Protons
Neutrons
Electrons
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Unit 2.3: Electron Arrangement
Further Reference: 4.3 Modern Atomic Theory
ENERGY LEVELS
1. Electrons that are closer to the nucleus have ____________ energy
a.
Further away from the nucleus means you have __________ energy
2.
The Electron Cloud is organized into _________________
3.
Each level (or shell) has a maximum number of __________ that it can hold.
st
b. 1 level = ______________
nd
c. 2 level = ______________
rd
d. 3 level = ______________
th
e. 4 level = ______________
3.
Electrons must occupy the __________________________________________ first
BOHR DIAGRAMS
4. Bohr diagrams show ______________________________________ of the atom
a.
They show __________________ that an atom has orbiting around it.
5.
These electrons are organized into different _____________ or _______________
st
a. 1 level = __________ electrons
nd
b. 2 level = __________ electrons
rd
c. 3 level = __________ electrons
6.
Draw the following Bohr Diagrams:
7.
H
B
F
Si
Valence electrons are electrons ___________________________
a.
Valence electrons determine the ________________________________
b.
Each column has a ______________________________
i.
ii.
iii.
iv.
Sodium (Na) has ____________ valence electrons
Boron (B) has ____________ valence electrons
Chlorine (Cl) has ____________ valence electrons
Neon (Ne) has ____________ valence electrons
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Notes for/from class
LEWIS DOT DIAGRAMS
1. Lewis dot diagrams use the symbol and dots to represent _____________________
a. How to…
i. Write the ______________ of the element
ii. Figure out how many ______________________ it has
iii. Each side of the symbol can only hold ___________________
1. 1 dot = ___________________
2. Each side must get _______________ before any side can
get ________________
iv. Maximum number is __________dots
2. Draw the following Lewis Dot:
H
Al
Cl
Ne
ELECTRON ARRANGEMENT
1. An ORBITAL is the _____________________________________________________
a. Electrons do not ________________
b. An orbit is a __________________________________________________
c. The reason for the different shapes (or orbitals) is to get as many
_____________ as possible, as close to the _____________ as possible,
while keeping the electrons ____________________________.
ELECTRON CONFIGURATION
2. Each energy level (2, 8, 18, 32) contains different ___________________.
a. There are 4 types of sub-orbitals.
i. S orbital holds ______ electrons
ii. P orbital holds ______ electrons
iii. D orbital holds ______ electrons
iv. F orbital holds ______ electrons
b. The reason for the different shapes is to get as many electrons as possible,
______________________ as possible.
c. Label the
following picture:
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Notes for/from class
d. The purpose of electron configuration is to tell how many _____________
are in each ________________
3. Practice:
a. H = ________________________
b. He = _______________________
c. Li = _________________________
d. B = __________________________
e. Ar = ___________________________
ORBITAL DIAGRAMS / ELECTRON SPIN
1. Electrons have a ____________ charge
a. And you recall that like objects ______________
b. Meaning that the two electrons want to ____________ each other
2. Two electrons within the same orbital will spin _________________________
3. There are two options for arrows: __________ and __________
a. Rules:
i. Each orbital must be filled before ___________________________
ii. Within an orbital, you must fill _________________________
before you fill in the down arrows.
4. The number of arrows you have will equal the number of _____________________
5. Try the following:
Hydrogen
Helium
Carbon
6. If you have any up arrows with no down arrow partner, it is considered an
___________________________
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Notes for/from class
Unit 3.1: Periodic Table of Elements
Further Reference: 5.1, 5.2, and 5.3 – Exploring, Organizing, and Families of the PT
THREE MAIN CATEGORIES
1. The three main categories of the periodic table are
a. ___________________
b. ___________________
c. ___________________
2. Properties of METALS
b. Metals are found on the ____________ side of the periodic table
i. Except for _____________
c. Metals are:
i. Good ______________________________
ii. __________________
iii. ___________________ (can be stretched into thin wires)
iv. ___________________ (can be pounded into thin sheets)
d. A chemical property of metal is its reaction with _____________ which
results in _____________________
4. Properties of NON-METALS
a. Non-Metals are found on the ____________ side of the periodic table
i. Except for _____________
b. Non-Metals are:
i. Poor ______________________________
ii. Not __________________________________
iii. Solid nonmetals are ________________ and __________________
iv. Many non-metals are _________________
5. Properties of METALLOIDS
a. Metalloids are located __________________________________________
b. Have properties of both _________________ and _________________
c. Metalloids are:
i. Solids can be ______________________________
ii. They are __________________________________
iii. They conduct _________________________________ better than
_______________, but not as well as __________________
ORGANIZING THE PERIODIC TABLE
1. PERIODS
a. Each _________________ is called a ___________________
b. The elements in a period ___________________________ in properties
c. Each element in the same period has the same _______________________
d. The first elements in a period (the far left side of the PT) is always an
____________________________. The last element in a period (the far
right side of the PT) is always an ________________________.
e. As you travel right across a period, you increase the ___________________
in the nucleus by _______
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2. FAMILIES
a. Columns of elements are called ______________ or ______________
b. Elements in each family have ___________________
c. All elements in a family have the same number of _________________
d. As you moved down a family, each new elements has an extra
__________________________
3. HYDROGEN
a. The hydrogen square sits atop ________________, but it is _____________
of that family
i. Hydrogen is in a class of its own.
b. It is a ______________ at room temperature
c. It has _________________ in its one and only energy level.
d. Hydrogen only needs ___________________ to fill up its valence shell
4. SPECIFIC FAMILIES
a. Group 1: Alkali Metals have __________ valence electrons
i. Hydrogen is not a member; it is a _________________
ii. Often react with Halogens because they have ___ valence electrons
iii. Very _____________, especially with ________________
b. Group 2: Alkaline Earth Metals have __________ valence electrons
i. Often reactive with the _____________ family
c. Group 3-12: Transition Metals have __________ valence electrons
i. Valence electrons (and oxidation number) __________________
d. Group 13: Boron Family have __________ valence electrons
i. Most are ______________ ( Boron is a _____________ )
e. Group 14: Carbon Family have __________ valence electrons
i. Contains ______________, ______________, and ______________
f.
Group 15: Nitrogen Family have __________ valence electrons
i. Contains ______________, ______________, and ______________
g. Group 16: Oxygen Family have __________ valence electrons
i. Contains ______________, ______________, and ______________
ii. Reactive with _________________________
h. Group 17: Halogen Family have __________ valence electrons
i. All are ______________________
ii. Very reactive: both with elements from _________________
i.
Group 18: Nobel Gas Family have __________ valence electrons
i. Exist as ________________: All of them are ______________
ii. __________________ with other elements because their
____________________ is full.
1. __________________ in the outer shell means they are full
2. Helium(He) has only _______________ in the outer shell to
be full.
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Due Date: ______________
Notes for/from class
Unit 3.2: Oxidation Numbers and Bonding
Further Reference: 6.2 Ionic and Covalent Bonding
“HAPPY” ELEMENTS
1. All elements want to be happy
2.
An atom wants ______________________________________ to make them happy
a.
Atoms will _______________________________ in order to become stable
b.
The most stable configuration involves having ________ valence electrons
c.
8 valence electrons = _____________________
d.
__________________ do not need to transfer/share any electrons because
they already have __________________________ and are _____________
iv. OCTET RULE means that atoms will _________________ with other atoms
in order to have ___________________________.
1.
Atoms can ___________ or ____________ electrons with other
elements
2.
Elements will not just _________________ electrons. They will
give to _________________ or take from _______________.
OXIDATION NUMBERS
1. The oxidation number indicated how many ______________ are going to be ___________
or ___________ during bonding
a.
2.
Ranges from __________ to __________
Steps to predicting oxidation numbers:
a. First, determine how many ___________________ the neutral atom has
b.
Determine if the atom will ______________________________
i. Will it be faster to ____________________ or _________________
c.
Count the number of electrons ______________________
i. If you lose electrons, the charge will be ______________
ii. If you gain electrons, the charge will be ______________
3.
Practice!
a. Lithium = ___________
b. Sulfur = ___________
c. Aluminum = ___________
d. Iodine = ___________
e. Phosphorous = ___________
f. Carbon = ___________
g. Neon = ___________
4.
Transition metals have _________________ oxidation number
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Due Date: ______________
Notes for/from class
Unit 3.3: Bonding: Ionic and Covalent Bonds
Further Reference: 6.2 Ionic and Covalent Bonding
CHEMICAL STABILITY
1. Nobel gases are the ___________________ elements
a. They have _____ valence electrons and don’t want to ________ or _______ any
electrons
CHEMICAL BONDS
1. Involve only _______________. The nucleus ___________________.
2.
3.
Elements will not just _______________________________.
a.
They will ________________________________________________ OR
__________________________________________________
b.
There will always be at least ______________ involved in this process
c.
Binary compound = compound with __________________________ in it
i. Example: __________, ___________, ___________
When atoms bond, they will always form new ________________ with
________________________
a.
The final product has _____________________ than either of the
___________________________________
IONIC BONDS
1. Form when one atom ___________________ and another atom _______________
a. One atom _____________ their _____________ to another atom
2.
Occur between _____________ and _______________
a. Two ______________ charged ______________
3.
The product of an ionic bond is a ________________________
a. The oxidation numbers must add up to _____________
4. Properties of Ionic Bonds
a. ______________ bonds
b. ______________ melting points
c. ______________ electricity when _______________
d. ____________________ at room temperature
5.
Drawing:
st
a. 1 – Determine the _________________
nd
b. 2 – Draw the __________________ for each atom
rd
c. 3 – Draw the _______________ being transferred in the _____________
d. DOUBLE CHECK: Does each atom have a ________________ orbital?
Drawing Practice: Draw the ionic bonding structure for Na and Cl
Oxidation number
Lewis Dot
Electrons being Transferred
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Due Date: ______________
Notes for/from class
COVALENT BONDS
1. Occur between _________________________
a. Formed when two atoms _____________________ with one another.
2. Can be between two _______________________, or two atoms of
_________________________________
a. Covalent Bonds are also called _______________________ (aka Molecule)
3. Properties of Covalent Bonds
a. ______________ bonds
b. ______________ melting points and boiling points
c. ___________________ electricity when _______________
d. _________________________ at room temperature
4. Drawing:
a. 1st – Draw the __________________ for each atom
b. 2nd – Draw the ________________ being ________________
c. 3rd – Draw each __________________ as a _________ between two atoms
d. DOUBLE CHECK: Does each atom have a ________________ orbital?
Drawing Practice: Draw the covalent bonding structure for H and Cl.
Lewis Dot
Electrons being Shared
Bonds as Lines
Drawing Practice: Draw the covalent bonding structure for H2O
Lewis Dot
Electrons being Shared
Bonds as Lines
Drawing Practice: Draw the covalent bonding structure for CH4
Lewis Dot
Electrons being Shared
Bonds as Lines
5. DIATOMIC MOLECULES
a. Two atoms __________________________ covalently bonded together.
i. Cannot exist as ________________ and must bond together
ii. Called ___________________
b. The 7 diatomic molecules are:
i. ______ _______ _______ _______ _______ _______ _______
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Due Date: ______________
Notes for/from class
Unit 4.1: Balancing Chemical Reactions
Further Reference: 7.1 and 7.2 – Chemical Equations
CHEMICAL CHANGES
1. In a chemical change, you are going to ___________ bonds, ______________ those
atoms, and _______________________.
2. All chemical changes are a result of _______________________
d. Happen when you _______________________ bonds.
e. Involve _____________________ of atoms
f. One set of compounds (_________________) forms another set of
compounds (________________________)
LAW OF CONSERVATION OF MATTER
1. The law of conservation of matter states that matter cannot be _____________ or
______________, but it can only ____________________.
a. The number of each type of atom ________________________ must be
___________ to the number of each type of atom ____________________
BEFORE WE BALANCE
1. Complete the following figure:
a. Coefficient: ___________________________________________________
b. Subscript: ____________________________________________________
PreBalancing Practice: How many of each do you have?
2 H2O3
H = _______
O = _______
4 Fe2O3
Fe = _______
O = _______
6 NaCl
Na = _______ Cl = _______
NO2
N = _______
O = _______
BALANCING EQUATIONS
1. _________________ on the left, _______________ on the right
2. Symbols:
a. + means ______________________________________
b.  means ______________________________________
c. g means ______________________________________
d. s means ______________________________________
e. l means ______________________________________
f.
aq means ______________________________________
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Due Date: ______________
Notes for/from class
3. When balancing chemical equations, you are not allowed to change the
____________________________
a. You CAN’T _____________________________
4. You can only change the _______________________________ on each side of the
equation
a. You CAN _________________________
5. Practice: Use the T Chart below to balance the following equation
a. Magnesium (solid) + Oxygen (gas)

Magnesium Oxide (solid)
Balancing Practice: Using the provided T Charts, balance the following equations.
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Due Date: ______________
Notes for/from class
Unit 4.2: Chemical Reactions: Energy
Further Reference: 7.1 and 7.2 and 7.4 – Chemical Equations and Reaction Rates
ENERGY IN CHEMICAL REACTIONS
1. All chemical reactions involve _____________________
2. Every time a bond is ___________ or _____________, energy is used
g. Breaking bonds ______________ energy
i. Chemical reactions require energy _______________
h. Forming bonds ______________ energy
3. Chemical energy is stored inside ______________________
a. The stronger the bond is, the ____________ it is to start the chemical
reaction
4. Energy is _________________________________
a. The energy within the _________________ and the __________________
must be the same as the energy within the ____________
HEAT ENERGY IN CHEMICAL REACTIONS
1. Exothermic reactions _______________ energy and the temperature __________
a. They _______________ heat!
b. Examples:
i. ___________________
ii. ___________________
iii. ___________________
2. Endothermic reactions _______________ energy and the temperature __________
a. They _______________ heat!
b. Examples:
i. _____________________
ii. _____________________
iii. _____________________
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Due Date: ______________
Notes for/from class
PHOTOSYNTHESIS
1. Photosynthesis is a _______________ reaction
a. Reactants are __________________ and __________________
b. Products are ___________________ and __________________
2. Energy from the ___________ is being transformed into __________________,
which is being stored as _____________________
Show the formula for photosynthesis (without the coefficients!)
_______________ + ______________  ____________ + _____________
SPEEDING UP REACTIONS
1. The following actions __________________ the rate of reactions because they
___________________________!
a. Increasing ________________________________
b. Increasing ________________________________
c. Increasing ________________________________
d. Increasing ________________________________
e. AND ______________________.
CATALYST
2. A CATALYST is a substance that _______________________________________
a. It does this by lowering the ________________________ of a chem rxn.
b. A catalyst is never ________________ and never__________________
c. Think of it as a _____________, like a _______________
i. Each catalyst has only _____________________________
3. Enzymes are merely ________________ that work ____________________
a. Just like catalysts, each enzyme has _______________________
b. Substrate: the ________________ an enzyme _________________
c. Essentially, the enzyme and substrate are like a ___________________
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Due Date: ______________
Notes for/from class
Unit 4.3: Types of Chemical Reactions
Future Reference: 7.3 Nature of Chemical Reactions
Classifying Reactions
1. Synthesis (Addition) Reactions:
a. Describe it in your own words:
b. Write the example using A, B, C, D, X, etc…
c. Write a real world example found in the notes:
2. Decomposition Reactions:
a. Describe it in your own words:
b. Write the example using A, B, C, D, X, etc…
c. Write a real world example found in your in the notes:
3. Single Displacement (Replacement) Reactions:
a. Describe it in your own words:
b. Write the example using A, B, C, D, X, etc…
c. Write a real world example found in the notes:
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Due Date: ______________
Notes for/from class
4. Double Displacement (Replacement) Reactions:
a. Describe it in your own words:
b. Write the example using A, B, C, D, X, etc…
c. Write a real world example found in the notes:
5. Acid Base Reactions:
a. Describe it in your own words:
b. Write the example using A, B, C, D, X, etc…
c. Write a real world example found in the notes:
Q1 – What 2 things does an Acid Base Reaction ALWAYS result in?
6. Combustion Reactions:
a. Describe it in your own words:
b. Write a real world example:
c. What are the two products of combustion EVERY TIME?
Q2 – What is ALWAYS going to be the non chemical product of a combustion reaction?
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Due Date: ______________
Notes for/from class
Unit 4.4: Translation
Further Reference: Google.
TRANSLATION
1. Translating is when I give you a __________________ that you have to turn into an
equation written _______________________
2. Hints:
a. Diatomic molecules are always written as:
i. ____________________________________
b. Words like ___________, _____________, ____________ mean put a +
into the equation
c. Words like ___________, ______________, ___________ mean put a 
into the equation
TRANSLATING PRACTICE (DO NOT BALANCE)
1. Potassium bromide  potassium metal + bromide
2. Calcium fluoride  Calcium + fluoride
3. Hydrogen reacts with oxygen to produce water.
4. Silicon tetrachloride decomposes into silicon and chlorine.
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Due Date: ______________
Notes for/from class
Unit 5.1: Solutions and Saturation Level
Further Reference: 8.1 Solutions and 8.2 How Substances Dissolve
HOMOGENEOUS MIXTURES
1. Solution is a ___________________________________________
a. Solutions are ________________ mixtures
2. 2 parts that make up a solution:
a. Solute is ________________________________________
i. Examples: _________________________
b. Solvent is ______________________________________
i. Examples: _________________________
THE DISSOLVING PROCESS
Q1 – Restate the 3 parts of the kinetic theory that you previously learned:
1)
2)
3)
1. Explain how a sugar molecule is broken down when it is put into water.
a. Dissolving works from the ____________  __________
2. Increasing ______________ between ____________ and ____________ will
increase the speed molecules dissolve.
3. What are the 3 ways that we can increase the speed that a solute will dissolve into
solution?
1)
2)
3)
4. Concentration is the quantity of ____________________________ a quantity of
_____________
a. Dilute:
b. Concentrated
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Due Date: ______________
Notes for/from class
SATURATED SOLUTIONS
1. Saturated Solution is ____________________________________
2. Unsaturated Solution is __________________________________
3. Supersaturated Solution is _______________________________
a. Having too much solute means that some will ___________
4. Each substance has a _______________________________ value
c. That value tells us how much of a substance will ______________ under a
certain temperature.
d. Raising the temperature _____________ the solubility value
e. The solute stops dissolving once the solution reaches _____________
Substance (Formula)
Fill in the table:
Solubility in 100ml of
Water at 20oC
Solubility in 100ml of
Water at 30oC
Table Salt (NaCl)
Sugar (C6H12O6)
Baking Soda (NaHCO3)
PRACTICE PROBLEMS:
How much table salt will dissolve in 250ml of water at 20oC?
How much water would you need to dissolve 150g of sugar at 20oC?
How water would you need to dissolve 150g of sugar at 30oC?
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Due Date: ______________
Notes for/from class
Unit 5.2: Acids and Bases
Further Reference: 9.1 Chemical Reactions and 9.2 Acids and Bases
CLASSIFICATION
1. Nothing itself can be an acid or base until it ________________in water
2. Acids:
a. __________ + ____________ (ex: __________)
i. Produce _______________ in solution
3. Bases:
a. __________ + ____________ (ex: __________)
i. Produce _______________ in solution
ACIDS Side Note
(H+) Hydrogen ion
(H3O+) Hydronium ion
1. Acids form __________ when in solution (or ________)
a. Acids conduct ________________________
b. Acids ________ corrosive
c. Acids taste _________
d. Acids react with _________
2. List 4 examples of Acids:
BASES Hydroxide ion (OH-)
1. Bases form ______________ when in solution
a. Bases feel _________
b. Bases conduct ____________________
c. Bases taste _________
d. ___________________
2. List 4 examples of Bases:
pH OF SOLUTIONS
1. pH indicates the concentration of _______________ in solution
a. The more ___________ in a solution, the more _________ the solution is,
the_______________ of the solution
b. The fewer ___________ in a solution, the more _________ the solution is,
the_______________ of the solution
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Due Date: ______________
Notes for/from class
2. Scale of pH values range from ___________ to ___________:
a. Neutral pH value ___________
Example of Neutral pH ______________________
b. Acid pH value range __________
Examples of Acid _______________________
c. Base pH value range ___________
Examples of Base _______________________
3. The ____________ you get from 7, the _______________ the acid or base is.
a. HCl (pH 1) is much _________an acid than a banana (pH 5)
INDICATORS
1. Litmus paper is an _____________
a. An indicator _________________________________________________
i. When litmus paper turns red, that indicates ___________
ii. When litmus paper turns blue, that indicates ___________
iii. When litmus paper stays yellow, that indicates __________
b. Some indicators are
i. Standard litmus paper (_______________)
ii. blue paper (_________________)
iii. red paper(________________)
ACID AND BASE REACTIONS
2. If equal ________________ and equal _____________ are mixed, the acid and
basic properties _____________
a. The remaining ions form ____________ and __________
b. Write me a real life acid base reaction (in the notes)
3. If a strong acid is mixed with a weak base, the resulting solution is a
________________
4. If a strong base is mixed with a weak acid, the resulting solution is a
_________________
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Due Date: ______________
Notes for/from class
Unit 5.3: The Mole
Further Reference: 4.2 and 6.3
WHAT IS THE MOLE?
1. It is a counting unit, similar to ______________, except instead of 12, it is
______________________________
2. The number:
a. In standard notation _______________________________
b. In scientific notation _______________________________
3. 1 mol = _______________ particles
a. If I had 1 mol of cookies, I would have __________ cookies
b. If I had 1 mol of cars, I would have __________ cars
c. If I had 1 mol of Al, I would have __________ atoms of Al.
4. Note that the _______________ is always the same, but the ____________ is
always different
5. A mole of ANYTHING contains _______________ particles
a. 1 mol C = _______________ carbon atoms
b. 1 mol H2O = _______________ water molecules
c. 1 mol NaCl = _______________ salt crystals
AVAGADRO’S NUMBER
1. That means that in ___________grams of Hydrogen, there are ____________
atoms of Hydrogen
2. And in _______________ grams of Fluorine, there are ___________ atoms of
Fluorine.
MOLAR MASS
1. The molar mass describes the mass of _____________ of an element or compound.
2. Atomic mass tells the _______________ (g/mol)
MOLAR MASS EXAMPLES (USE THE PERIODIC TABLE I GAVE YOU, NOT THE ONE ON THE
WALL)
1. Carbon = _________________________
2. Aluminum = ______________________
3. Zinc = ___________________________
4. Water (H2O) = _____________________________________
5. Sodium Chloride (NaCl) = ____________________________
6. Sodium bicarbonate (NaHCO3) = __________________________
7. Sucrose (C12H22O11) = ___________________________________
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