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Inorganic Chemistry

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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 containerWhat makes the states

different? Amount of kinetic energy- The kinetic energy of an object is the energy it possesses because of its motion

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II. Atomic StructureA. 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).

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Because of attraction to the positive nucleus.

Fig. 2-1

Why do electrons stayIn their “orbits”?

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Atoms have a neutral charge. The electron(-) & proton(+) cancel each other out.

Fig. 2-1

What is the charge of an atom?

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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-)** Magnesium loses two electrons?

Mg+2

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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.

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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

Isotopes and Radiation Atoms of the same

element that differ in the number of neutrons

Some isotopes are unstable and breakdown over a predictable period of time and give off radiation in the process

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Isotopes have the same chemical properties because they have the same number of electrons!

Fig. 2-2

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Isotopes are identified by their mass numbers. Carbon has three isotopes: carbon-12, carbon-13, & carbon-14. Each has a different number of neutrons

Fig. 2-2

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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.

Do compounds have the same properties as the elements that formed them? Think Water

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IV. Chemical BondingC. Chemical bonds

are forces that hold two or more atomstogether.

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IV. Chemical BondingD. Two types of Chemical

bonds:1. 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)

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

covalent bonds are the most common in living systems.

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3. Also we talk about Hydrogen “Bonding” - a weak force of attraction between H and O, F or N.

Fig. 2-7

Water is a “polar” molecule

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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

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VI. Water and its propertiesA. Hydrogen bonding is responsible

for the following properties…1. High surface tension

What is this & How can it walk on water?

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VI. Water and its properties2. High specific heat capacity (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?

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VI. Water and its properties

3. Water demonstrates capillarity (capillary action).

Meniscus

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Capillary action

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VI. Water and its properties

4. Water has a high heat of fusion and vaporization (it takes a lot of heat to change the state of water… from solid to liquid and liquid to gas)

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5. Most dense at 4°C (39.2 F). *** What impact does this have on

life in a lake in the winter?

B. Water is a universal solvent & a great lubricant.

CoyoteOn Frozen Lake

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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.

What is the pH of Water?

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VII. pH - “Potential of Hydrogen”

B. Definitions of an acid and a base

1. 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.