Inorganic Chemistry

I. Matter A. Anything that has mass and takes up space. B. Matter exists in 3 states or phases: 1. Solid - have definite shape and volume 2. Liquid - have definite volume but shape depends on the container 3. Gas - both the shape and volume are determined by the container **What makes the states different? The amount of kinetic energy C. A chemical element is a substance made of one kind of atom that can’t be separated into simpler substances. 1. 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 Table A. Displays all known chemical elements B. Atomic number = the # of protons 1. 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+ #Nso 30 #N = 35

D. Isotopes have same atomic #, but different atomic mass. 1. Have same chemical properties, but different physical properties. How many protons does 12 C have? 14 C? How many neutrons does 12 C have? 14 C?

IV. Chemical Bonding A.Molecules are formed by combining 2 or more atoms, e.g. O 2, or H 2 B.Compounds are molecules that form from combining 2 or more different elements, e.g. H 2 O or NaCl. C. Chemical bonds are forces that holds two or more atoms together. D. 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)

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 Reactions A. 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 H 2 + O > 2 H 2 O

VI. Water and its properties A. Hydrogen bonding is responsible for the following properties… 1. High surface tension 2. High specific heat (its temperature is hard to change) and therefore: a) It’s a good coolant b) 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. 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? B. Water is a universal solvent C. Water is a great lubricant.

VII. pH - “Potential of Hydrogen” A. pH scale 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 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.

Oven cleaner Bleach Ammonia solution Soap Sea water Pure water Normal rainfall Tomato juice Lemon juice Stomach acid Increasingly Basic Increasingly Acidic Neutral Human blood