Your Guide for Success—Chemistry Unit
Name: __________________________
Chemistry Outline
I. Atoms
A. Structure of an Atom
1. Subatomic Particles
2. Different Form
b. Isotope
II. Periodic Table
1. Arranging
a. Mendeleev
b. Mosely
2. Grouping the Elements
III. Chemical Bonding
A. Ionic Bonding
1. Forming Ionic Bonds
2. Forming Positive Ions
3. Forming Negative Ions
4. Properties
B. Covalent and Metallic Bonds
1. Molecules
2. Movement of Electrons in Metallic Bonds
3. Properties of Metallic Bonds
4
6
8
10
12
1V. Chemical Reactions
A. Forming New Substances
14
B. Chemical Formulas and Equations
16
1. Chemical Formulas
2. Writing Formulas for Covalent and Ionic Compounds
3. Chemical Equations
4. Law of Conservation of Mass
5. Balancing Equations
2
3
The Atom vs. The Isotope
Chapter _4_ Section _2_ Pages _88-94_
Smallest unit of an _____________ that maintains the properties of that
element.
 Contains subatomic particles: Protons, _______________, and Electrons


us
Nucleus:

Tiny, ________ core of an atom

Contains ____________ and neutrons

Most of an atom’s ___________.

Very small and ____________.
Protons:

Most of an atom’s _______

Contains ______________

_____________ charged

MUCH _______________

VERY ________________
Neutrons

_________ charged

1 ________ = 1 amu

Atomic # = the number of ___________ 

Symbol: + or ____

Together:
Protons + _____________ = atomic mass


Electron Cloud:
_____________ the nucle-
1 ________ = 1 amu

Symbol: 0 or ____

# of Electrons = # of
________________
Symbol: - or _______
An ______________ that has the same number of _______________ (atomic number) but a
__________________ number
of ________________, therefore it has a different

4
5
Arranging the Elements
Chapter _5_ Section _1_ Pages _106-112_
History 101-The Periodic Table

Dmitri Mendeleev—______________ Chemist—____________

Discovered a ________________ in the elements properties.

His final arrangement—increasing atomic _____________.

He left gaps in the his table—for yet _______________ elements.

He could _________________ the properties of the undiscovered elements.
Our Current Periodic Table

Henry Mosely—___________________ Scientist—____________

Rearranged original table—Our current periodic table is by atomic
______________________.

This allowed all elements to fit the __________________________.
Classification of Elements on the Periodic Table

Metals
__________ of zig-zag line


________ valence elec-

trons
Metalloids
____________ zig-zag line
About _________ a complete set of valance electrons
Nonmetals
__________ of zig-zag line

___________ or almost
complete set of valence electrons

An element’s classification is determined by its number of _____________ electrons. The
____________ line helps you recognize where to locate each classification on the Periodic Table.
Decoding The Elements of the Periodic Table
Periods

Direction =

Period # = __________

There are ______
periods.
Groups/Families




Direction = _____________
Each group has _____________
properties.
If you know the group number
you can determine the number
of _______________ electrons.
There are ______ groups.
6
7
Grouping the Elements
Chapter _5_ Section _2_ Pages _114-120_
Group 2 (G2) —Alkaline-Earth Metals:
 ___________ reactive than G1
Group 1 (G1) —Alkali Metals:
 __________ reactive metals

1 ______________ electron

2 ________________ electrons

Often store in _____________


Found in nature in _________________
Physical Properties—Silver,
____________ density
ring
ct u
a
f
than G1
anu
_m
___
nt
___
_
me
_
e
_
c
_
and
___
__
n_
i
_
_
d
___
Use
___
n
i
nd
Fou
Physical Properties — Soft,
_______________, shiny, and low
__________________

Groups 3-12 (G3-12)—Transition Metals:
 1 or 2 ___________ electrons (Do not let them
go as easily as G1 or G2)
 Less _____________ than G1 and G2

Good ___________________

__________ density, ______________ melting point than G1 and G2
Lanthanide Series:


Appears at the bottom of the table to keep it from being too wide.

Actinide Series:

______________/Unstable
 After element number _______________ made in laboratories.
Group 13 (G13)—Boron Group:

____ metalloid and _____ metals

3 ______________ electrons
Group 14 (G14)—Carbon Group:
 _____ nonmetal, _____ metalloids, and
____ metals
 4 _____________ electrons

_______________ at RT


Most common = _____________

Varying _________________
______________ at RT

in
sed
___
___
___
_
_
___
___
_
_
_
ps
chi
U
8
Grouping the Elements…..continued
Chapter _5_ Section _2_ Pages _114-120_
Group 16 (G16)—Oxygen Group:
 _____ nonmetals, _____ metalloids, and
_____ metals
 6 ________________ electrons
Group 15 (G15)—Nitrogen Group:
 _____ nonmetals, _____ metalloids, and
_____ metals
 5 ______________
electrons
.
athe
o
___%
_
_
_
_
f the
___
____
_
_
_
_
e b re
gas w
____
__ r
____
.
athe
b re
s we
a
g
the
% of
_
_
_
____
ive
eact
Groups 17 G(17)—Halogens:
 All _______________________

7 ____________________ electrons

Very ____________________

Need to gain only __________ valence electron

Forms compounds with ______________very easily.

Chemical properties _____________________

Physical properties _______________ different
Group 18 (G18)—Noble Gases:
 All _____________________
Hydrogen:
8 _______________ electrons—
Exception is He—__________ valence
electrons.





STABLE!

1 _________________ electron



Set a part because the _______________ do
not ____________ any other group.
Is placed above ___________ because the
______________ of valence electrons is the
same.
Most __________________ element
9
Ionic Bonding
Chapter _1_ Section _2_ Pages _8-11_
Ionic Compounds


Forms when _______________ electrons are
transferred (gained or lost) from one atom to
first.

another to _______________ each others outer
energy level.


Forms between _________________ (+ ions)
When formed, the # of _______________ lost
equals the # of electrons ______________.

Therefore, ionic compounds are ____________.

The charges _____________ each other out.

Properties include; ______________ bond,
Write the ____ ion or the ____________ second.
Polyatomic ion—an ion that is made up of
more than one atom (2 capital letters—Ex
and nonmetals ( ____ ions)

Writing Ionic Formulas
Always write the ____ ion or __________
(NH4)+

When written name remains the same.

Use parentheses

____________ numerals show
_______________ number.

____________ melting and boiling points.
An oxidation number is the number of
_________________ electrons an atom gains
or loses to become ______________.

Make sure compounds are
_______________.
Forming + Ions - Cation

Occurs when an atom __________ valence
Forming - Ions— Anion

electrons.

An atom now has ___________ protons than
lence electrons.

negative electrons. (Unbalanced + and -)


(Unbalanced + and -)

Only takes a small amount of ______________
to lose their few ___________________ elec______ and _______ are examples of atoms
that form + ions.
___________________ form - ions because
they have an almost full outer level.

trons.

An atom now has move ______________
electrons than positive protons.
_______________ form + ions because they
have ________ valance electrons (1, 2, or 3)
Occurs when an atom ______________ va-
Ending of the elements name changes to
___________ (Ex. Fluorine —>Fluoride)

______ and _______ are examples that
form - ions.
10
Section A: Complete the chart using a periodic table to help you.
Section B: Answer these questions:
1. An atom that gains one or more electrons will have a _________________ charge.
2. An atom that loses one or more electrons will have a __________________ charge.
3. At atom that gains or loses one or more electrons is called an ________________.
4. A positive ion is called a ___________________ and a negative ion is called a
________________.
5. Atoms will transfer one or more ______________ to another to form the bond.
6. Each atom is left with at ____________________ outer shell.
7. An ionic bond forms between a _________________ ion with a positive charge and
a ___________________ ion with a negative charge.
Section C: Draw the ionic compounds below. Show the transfer, give the name of the
compound and give the formula.
Example #1: Sodium + Chlorine
Example #2: Magnesium + Iodine
Example #3: Sodium + Oxygen
Example #4: Aluminum + Chlorine
11
Covalent and Metallic Bonding
Chapter _1_ Section _3_ Pages _12-17_


Covalent Molecules
Forms when atoms _______________ valence

electrons to complete an atom’s outermost en-
_____________________ between positively
ergy level.
charged metal ions and the
Forms between 2 or more _______________.
__________________ in the metal.


May have ______________ bonds between the
atoms.


The metals outermost energy levels
_______________.

This overlapping allows the
Consist of individual particles called
________________ electrons to move
__________________.
throughout the metal.
Simplest type = ___________________

Example—Hydrogen H2 and Oxygen O2

Metallic Compounds
This type of bond is formed by the
The _______________ ____ cancel the
__________________ charge of the ions.
Properties: _______________ bond, ________
melting and boiling points.

Writing Covalent Formulas
Usually the name tells you the
_____________________.


However, many molecules have
Metallic bonding is what gives
______________ their particular properties.
________________ names
Example—dihydrogen monoxide = water

Properties of Metals

When metals are ______________________
electric current, the ___________________
Pay attention to __________________ used.
electrons are moving through the metal.

Because of the “__________________” elec-
Mono—
Hexa—
Di—
Hepta -
trons, metals may be
Tri—
Octa -
____________________. Malleability and
Tetra—
Nona-
______________________ describe how a
Penta—
Deca—
metal may be reshaped.
12
Section A: Answer these questions:
1. Atoms ________________ one or more electrons with each other to form the bond.
2. Each atom is left with a _______________________ outer shell.
3. A covalent bond form between two _________________________________.
Section B: Draw the molecular compounds below. Show how they share, give the
name of the molecule and give the formula.
Example #1: Hydrogen + Hydrogen
Example #2: Hydrogen + Oxygen
Example #3: Chlorine + Chlorine
Example #4: Oxygen + Oxygen
Example #5: Carbon + 2 Oxygen
gen
Example #6: Carbon + 4 Hydro-
Write the formulas for the following covalent compounds:
Write the names for the following covalent compounds:
1)
antimony tribromide ____________________
9)
P4S5- __________________________________
2)
hexaboron silicide ______________________
10)
O2 __________________________________
3)
chlorine dioxide ________________________
11)
SeF6 __________________________________
4)
hydrogen iodide ________________________
12)
Si2Br-6 __________________________________
5)
iodine pentafluoride _____________________
13)
SCl4 __________________________________
6)
dinitrogen trioxide ______________________
14)
CH4 __________________________________
7)
ammonia ______________________________
15)
B2Si __________________________________
8)
phosphorus triiodide _____________________
16)
NF3 __________________________________
13
Forming New Substances
Chapter _2_ Section _1_ Pages _28-31_
Chemical Reactions


A process in which one or more substances _______________ to make one or more
_________ substances.
The _____________ and physical properties ____________ from the original substances.
Some Signs of Chemical Reactions
Reactions often have more than one of these signs. And the more of these
signs you see, the more likely that a chemical reaction is taking place. However there is NO guarantee. The MOST important sign is
___________________ of a ________ substance!
How do new substances form in a chemical reaction?

Chemical bonds in the original substances must ________________.

The _____________ rearrange.

New ______________ form to make ___________ substances.
14



On your desk place the “Physical Change” card to your left and the
“Chemical Change” card to your right.
Using what you know about physical and chemical changes, place each
card into the correct category.
Record you data in the chart below.
Physical Change



Chemical Change
Were there any cards you had trouble classifying?
Give an example of a physical change that was not listed above.
Give an example of a chemical change that was not listed above.
15
Chemical Equations
Chapter _2_ Section _2_ Pages _32-36_

Use symbols and __________________ to describe a chemical reaction.

Starting materials = _____________________________

Ending materials = _____________________________
Accuracy is key when writing chemical equations!
Equations MUST BE Balanced!

Atoms are never ______________ or gained in a chemical reaction—just _______________.

The __________________ of reactants must equal the number of ____________________.

Based on the work of Antoine Lavoisier—Law of _______________________________ of
________________________.
Steps to balance a chemical equation.
1. Write symbols and ___________________ correctly.
2. Make 2 lists of ______________ - write it the
__________ on both sides of the arrow.
3. Count
4. Use _____________________ to balance
5. Recount/ __________________ if necessary.
Never Ever Balance by Changing a Subscript!
16
Balancing Equations Practice
Part A: Identify the following parts of each chemical formula by circling the subscripts and drawing a square around the coefficients.
H2
2HCl
4O2
CH4
3CO3
2NaOH
Part B: List the symbols for the atoms in each formula and give the number of each.
C2H6
2MgO
4P4O10
NH3
3Al(OH)3
2H2O
Part C: Balance each of the following equations following the procedure described in
class. Be sure to show your work.
P + O2 → P4O10
Mg + O2 → MgO
P=
O=
Mg =
O=
P=
O=
Mg =
O=
HgO → Hg + O2
Al2O3 → Al + O2
Hg =
O=
Al =
O=
Hg =
O=
Al =
O=
BaCl2 + H2SO4 → BaSO4 + HCl
Ba =
Ba =
Cl =
Cl =
H=
H=
S=
S=
O=
O=
17