Your Guide for Success—Chemistry Unit

Name: __________________________

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Chemistry Outline

I. Atoms

A. Structure of an Atom 4

1. Subatomic Particles

2. Different Form

b. Isotope

II. Periodic Table

1. Arranging 6

a. Mendeleev

b. Mosely

2. Grouping the Elements 8

III. Chemical Bonding

A. Ionic Bonding 10

1. Forming Ionic Bonds

2. Forming Positive Ions

3. Forming Negative Ions 4. Properties

B. Covalent and Metallic Bonds 12

1. Molecules

2. Movement of Electrons in Metallic Bonds

3. Properties of Metallic Bonds

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

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The Atom vs. The Isotope Chapter _4_ Section _2_ Pages _88-94_

Nucleus: Tiny, ________ core of an atom

Contains ____________ and neutrons

Most of an atom’s ___________.

Very small and ____________.

Protons:

_________ charged

1 ________ = 1 amu

Atomic # = the num-

ber of ___________

Symbol: + or ____

Neutrons

1 ________ = 1 amu

Symbol: 0 or ____

Together:

Protons + _____________ = atomic mass

Electron Cloud:

_____________ the nucle-

us

Most of an atom’s _______

Contains ______________

_____________ charged

MUCH _______________

VERY ________________

# of Electrons = # of

________________

Symbol: - or _______

Smallest unit of an _____________ that maintains the properties of that

element.

Contains subatomic particles: Protons, _______________, and Electrons

An ______________ that has the same number of _______________ (atomic num-

ber) but a

__________________ number

of ________________, there-

fore it has a different

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Arranging the Elements Chapter _5_ Section _1_ Pages _106-112_

History 101-The Periodic Table

Henry Mosely—___________________ Scientist—____________

Rearranged original table—Our current periodic table is by atomic

______________________.

This allowed all elements to fit the __________________________.

Our Current 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.

Classification of Elements on the Periodic Table Metals

__________ of zig-zag line

________ valence elec-

trons

Metalloids

____________ zig-zag line

About _________ a com-

plete set of valance elec-

trons

Nonmetals

__________ of zig-zag line

___________ or almost

complete set of valence elec-

trons

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.

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.

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Grouping the Elements Chapter _5_ Section _2_ Pages _114-120_

Group 1 (G1) —Alkali Metals:

__________ reactive metals

1 ______________ electron

Often store in _____________

Found in nature in _________________

Physical Properties — Soft,

_______________, shiny, and low

__________________

Group 2 (G2) —Alkaline-Earth Metals:

___________ reactive than G1

2 ________________ electrons

Physical Properties—Silver,

____________ density

than G1

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:

Actinide Series:

______________/Unstable

After element number _______________ made in laboratories.

Group 13 (G13)—Boron Group:

____ metalloid and _____ metals

3 ______________ electrons

_______________ at RT

Most common = _____________

Group 14 (G14)—Carbon Group:

_____ nonmetal, _____ metalloids, and

____ metals

4 _____________ electrons

Varying _________________

______________ at RT

Used in _______________ manufacturing

Used in ____________________ chips

Appears at the bottom of the table to keep it from being too wide.

Found in __________ and cement

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Grouping the Elements…..continued Chapter _5_ Section _2_ Pages _114-120_

Group 15 (G15)—Nitrogen Group:

_____ nonmetals, _____ metalloids, and

_____ metals

5 ______________ electrons

Group 16 (G16)—Oxygen Group:

_____ nonmetals, _____ metalloids, and

_____ metals

6 ________________ electrons

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 _____________________

8 _______________ electrons—

Exception is He—__________ valence

electrons.

STABLE!

Hydrogen:

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

_______% of the gas we breathe.

_____________________ reactive

_______% of the gas we breathe.

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Ionic Bonding Chapter _1_ Section _2_ Pages _8-11_

Ionic Compounds

Forms when _______________ electrons are

transferred (gained or lost) from one atom to

another to _______________ each others outer

energy level.

Forms between _________________ (+ ions)

and nonmetals ( ____ ions)

When formed, the # of _______________ lost

equals the # of electrons ______________.

Therefore, ionic compounds are ____________.

The charges _____________ each other out.

Properties include; ______________ bond,

____________ melting and boiling points.

Writing Ionic Formulas Always write the ____ ion or __________

first.

Write the ____ ion or the ____________ sec-

ond.

Polyatomic ion—an ion that is made up of

more than one atom (2 capital letters—Ex

(NH4)+

When written name remains the same.

Use parentheses

____________ numerals show

_______________ number.

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

electrons.

An atom now has ___________ protons than

negative electrons. (Unbalanced + and -)

_______________ form + ions because they

have ________ valance electrons (1, 2, or 3)

Only takes a small amount of ______________

to lose their few ___________________ elec-

trons.

______ and _______ are examples of atoms

that form + ions.

Forming - Ions— Anion

Occurs when an atom ______________ va-

lence electrons.

An atom now has move ______________

electrons than positive protons.

(Unbalanced + and -)

___________________ form - ions because

they have an almost full outer level.

Ending of the elements name changes to

___________ (Ex. Fluorine —>Fluoride)

______ and _______ are examples that

form - ions.

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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

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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-

ergy level.

Forms between 2 or more _______________.

May have ______________ bonds between the

atoms.

Consist of individual particles called

__________________.

Simplest type = ___________________

Example—Hydrogen H2 and Oxygen O2

Properties: _______________ bond, ________

melting and boiling points.

Writing Covalent Formulas Usually the name tells you the

_____________________.

However, many molecules have

________________ names

Example—dihydrogen monoxide = water

Pay attention to __________________ used.

Mono— Hexa—

Di— Hepta -

Tri— Octa -

Tetra— Nona-

Penta— Deca—

Metallic Compounds This type of bond is formed by the

_____________________ between positively

charged metal ions and the

__________________ in the metal.

The metals outermost energy levels

_______________.

This overlapping allows the

________________ electrons to move

throughout the metal.

The _______________ ____ cancel the

__________________ charge of the ions.

Properties of Metals

Metallic bonding is what gives

______________ their particular properties.

When metals are ______________________

electric current, the ___________________

electrons are moving through the metal.

Because of the “__________________” elec-

trons, metals may be

____________________. Malleability and

______________________ describe how a

metal may be reshaped.

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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 Example #6: Carbon + 4 Hydro-

gen

Write the formulas for the following covalent compounds:

1) antimony tribromide ____________________

2) hexaboron silicide ______________________

3) chlorine dioxide ________________________

4) hydrogen iodide ________________________

5) iodine pentafluoride _____________________

6) dinitrogen trioxide ______________________

7) ammonia ______________________________

8) phosphorus triiodide _____________________

Write the names for the following covalent compounds:

9) P4S5- __________________________________

10) O2 __________________________________

11) SeF6 __________________________________

12) Si2Br-6 __________________________________

13) SCl4 __________________________________

14) CH4 __________________________________

15) B2Si __________________________________

16) NF3 __________________________________

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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. How-

ever 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.

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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.

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Chemical Equations Chapter _2_ Section _2_ Pages _32-36_

Use symbols and __________________ to describe a chemi-

cal 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!

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Balancing Equations Practice

Part A: Identify the following parts of each chemical formula by circling the sub-

scripts 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 = P = Mg = Mg =

O = O = O = O =

HgO → Hg + O2 Al2O3 → Al + O2

Hg = Hg = Al = Al =

O = O = O = O =

BaCl2 + H2SO4 → BaSO4 + HCl

Ba = Ba =

Cl = Cl =

H = H =

S = S =

O = O =