Inorganic Chemistry

I. MatterA. Anything that has mass and takes up

space.B. Matter exists in 3 states or phases:

1. Solid - have definite shape and volume2. Liquid - have definite volume but shape

depends on the container3. Gas - both the shape and volume are

determined by the container**What makes the states different?

The amount of kinetic energy

1. A chemical element is a substance made of one kind of atom that can’t be separated into simpler substances.

– There are 92 naturally occurring.

II. Atomic Structure

A. The atom is the building block of matter.B. Subatomic particles make up atoms:

1. Electrons - have a “-” charge and no mass.

2. Protons have a “+” charge and a mass of 1 AMU (atomic mass unit).

3. Neutrons have no charge and a mass of 1 AMU (atomic mass unit).

II. Atomic structure (cont)

C. When atoms gain or lose electrons then they are called “Ions.”

** What forms when a chlorine atom gains one electron?

A chlorine ion (Cl-)** Oxygen gains two electrons?

O-2

** Magnesium loses two electrons?Mg+2

III. Periodic TableA. Displays all known chemical elements

B. Atomic number = the # of protons1. Each element has its own atomic number and if

you add or remove protons you will have a different element.

C. Atomic Mass = #Protons + #neutrons.** How many protons does Calcium (Ca) have?** How many electrons are in a neutral atom of

sodium (Na)? ** How many neutrons are in an atom of zinc

(Zn)?

= 65#P + #N= Mass+ #N so 30 #N = 35

D. Isotopes have same atomic #, but different atomic mass.

1. Have same chemical properties, but different physical properties.

2. How many protons does 12C have? 14C?3. How many neutrons does 12C have? 14C?

IV. Chemical BondingA.Molecules are formed by

combining 2 or more atoms, e.g. O2, or H2

B.Compounds are molecules that form from combining 2 or more different elements, e.g. H2O or NaCl.

C. Chemical bonds are forces that holds two or more atoms together.

D.Types of Chemical bonds:A.Ionic – 2 or more atoms

exchange one or more electrons.A. Sodium loses an electron to

become Na+

B. Chlorine gains an electron to become Cl-

C. Na+ and Cl- the compound sodium chloride (NaCl)

2. Covalent Bond – 2 or more atoms share electrons.

- covalent bonds are the most common in living systems.

3. Hydrogen Bonding - a weak force of attraction between H and O, F or N.

V. Chemical ReactionsA. Chemical reactions occur when chemical

bonds are being broken and reformed.B. All reactions either produce or use energy.C. The reactants (ingredients) are usually on the

left D. The products are usually on the right. E. An arrow represents the progress of the reaction

2 H2 + O2 -----> 2 H2O

VI. Water and its propertiesA. Hydrogen bonding is responsible

for the following properties…1. High surface tension

QuickTime™ and aTIFF (Uncompressed) decompressor

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2. High specific heat (its temperature is hard to change) and therefore:a) It’s a good

coolantb) It’s a good

antifreeze How much does

the ocean temperature change during the year or in a day?

VI. Water and its properties

3. Water demonstrates capillarity.

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4. Water has a high heat of fusion and vaporization (it takes a lot of heat to boil and freezing occurs at a lower temperature.)

5. Most dense at 4°C. *** What impact does this have on

life in a lake in the winter?

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B. Water is a universal solvent

C. Water is a great lubricant.

VII.pH - “Potential of Hydrogen”

A. pH scale 0-141. Lower the number the more acidic (0-7)2. Higher numbers are more basic or alkaline

(7-14).3. Neutral is 7.

B. Definitions of an acid and a base1. Acid - Proton donor (H+) which lowers pH

of a solution and taste sour.2. Base (alkali) - Proton acceptor (OH-) that

raises pH of a solution and they taste bitter.

Oven cleaner

Bleach

Ammonia solution

Soap

Sea water

Pure water

Normalrainfall

Tomatojuice

Lemon juice

Stomach acid

Incr

easi

ng

ly B

asic

Incr

easi

ng

ly A

cid

ic

NeutralHuman blood