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Honors Physical Science Chemistry: Bell Work, Notes, Study Guides

Name: _____________________________________

Block: ______________________________________

Clicker Number: ______________________________

Mr. Banker

Fall 2014

[email protected]

http://wandohigh.ccsdschools.com/directory/science/banker_ian/physical_science/

Remind101.com Honors Reminders: text @MrBanker to (442)333-7101

mailto:[email protected]

http://wandohigh.ccsdschools.com/directory/science/banker_ian/physical_science/

Due Date: ______________

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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

Due Date: ______________

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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, ________________________________________________________

Notes for/from class

Due Date: ______________

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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 _____________

PRECISION AND ACCURACY

1. Precision is __________________________________________________________ ___________________________________________________________________

2. Accuracy is __________________________________________________________

___________________________________________________________________

3. Draw a picture of the following: Not accurate and not precise Accurate and not precise Not accurate, but precise both accurate and precise

4. Explain a scenario where you can be precise, but not accurate.

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


Due Date: ______________

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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)?

Due Date: ______________

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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)?


Due Date: ______________

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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:


Due Date: ______________

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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) _________________________________________________________


Due Date: ______________

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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: ___________________________________________________



3. Gasses:

a. Energy: _______________________________________

b. Movement: ___________________________________________________

i. Enough energy __________________________________________




Due Date: ______________

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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 ___________________


Due Date: ______________

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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. .


Due Date: ______________

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CHARLES LAW: 1. If the _____________________ is held constant, the _____________ and

_____________ vary directly.

a. Simply, as temperature _________ then volume _________



b. .

GAY-LUSSAC’S LAW: 1. If the _____________________ is held constant, the ___________ and

___________ vary directly.

a. Simply, as pressure _________ then temperature ________



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? ________ ________ ________ ________ ________ ________


Due Date: ______________

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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 ___________________________.


Due Date: ______________

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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


Due Date: ______________

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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 __________________________________


Due Date: ______________

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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 _______________________


Due Date: ______________

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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 ________________ 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:


Equation in words Equation in Symbols Units: Mass = _______________ (__) Volume (2 ways)

Ruler = ___________________ (__) Displacement = ___________________ (____)

Density (2 ways)

Ruler = ___________________ (__) Displacement = ___________________ (____)

Due Date: ______________

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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?


Due Date: ______________

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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


Due Date: ______________

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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 Atomic # Protons Neutrons Mass #

Boron – 11 B

Carbon – 12

6 6

Magnesium – 23

12 23

Copper – 64

29 35

20


Due Date: ______________

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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


Due Date: ______________

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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 39N+

8 16N-2

20 41N+2

Protons

Neutrons

Electrons


Due Date: ______________

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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. b. 1

st level = ______________

c. 2nd

level = ______________ d. 3

rd level = ______________

e. 4th

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 _______________ a. 1

st level = __________ electrons

b. 2nd

level = __________ electrons c. 3

rd level = __________ electrons

6. Draw the following Bohr Diagrams:

7. Valence electrons are electrons ___________________________

a. Valence electrons determine the ________________________________

b. Each column has a ______________________________

i. Sodium (Na) has ____________ valence electrons ii. Boron (B) has ____________ valence electrons

iii. Chlorine (Cl) has ____________ valence electrons iv. Neon (Ne) has ____________ valence electrons

H

B

F

Si


Due Date: ______________

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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:

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:

H

Al

Cl

Ne


Due Date: ______________

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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 ___________________________


Due Date: ______________

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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 _______


Due Date: ______________

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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.


Due Date: ______________

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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. Ranges from __________ to __________

2. 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


Due Date: ______________

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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. 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: __________, ___________, ___________

3. 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: a. 1

st – Determine the _________________

b. 2nd

– Draw the __________________ for each atom c. 3

rd – 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

Due Date: ______________

30 | P a g e

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?

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. ______ _______ _______ _______ _______ _______ _______

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

Due Date: ______________

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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: ____________________________________________________

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 ______________________________________


PreBalancing Practice: How many of each do you have?

2 H2O3 H = _______ O = _______

4 Fe2O3 Fe = _______ O = _______

6 NaCl Na = _______ Cl = _______

NO2 N = _______ O = _______

Due Date: ______________

32 | P a g e

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.


Due Date: ______________

33 | P a g e

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. _____________________


Due Date: ______________

34 | P a g e

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 _____________________ 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 ___________________

Show the formula for photosynthesis (without the coefficients!) _______________ + ______________ ____________ + _____________


Due Date: ______________

35 | P a g e

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:


c. Write a real world example found in your in the notes:

3. Single Displacement (Replacement) Reactions: a. Describe it in your own words:




Due Date: ______________

36 | P a g e

4. Double Displacement (Replacement) Reactions: a. Describe it in your own words:



5. Acid Base Reactions: a. Describe it in your own words:



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?


Due Date: ______________

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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.


Due Date: ______________

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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


Due Date: ______________

39 | P a g e

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 _____________

Fill in the table:

Substance (Formula) 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?


Due Date: ______________

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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


Due Date: ______________

41 | P a g e

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 _________________


Due Date: ______________

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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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