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R2 Common Chemicals Chart
Type
Atomic
Elements
Organic
Inorganic
Acidity
All Gases
Solubility
Poorly
Poorly
(neutral)
All solids
Neutral
salts
Ionic
Compounds
Phase at
22o
All Solids
Inorganic
Insoluble
Insoluble
Soluble
Soluble
Soluble
Partially
Insoluble
Solids
Bases
Aqueous
Acids
Aqueous
Soluble
Soluble
Liquid
Totally!
Poorly
Poorly
Poorly
liquid
Molecules
Inorganic
Neutral
Gases
Neutral
Organic
(has
C-H)
Acids
Soluble
Soluble
Soluble
Gas
Liquid
Soft solid
Solid
Insoluble
Insoluble
Insoluble
Insoluble
Liquid
Solid
Soluble
Soluble
Aqueous
Solid
Soluble
Soluble
Insoluble
Unit and Name
Noble gases
1 Helium
1 Argon
Metals
1 Copper
1 Aluminum
1+ or 1- Salts
1 Sodium chloride
5 Ammonium nitrate
5 Calcium dihydrogenphosphate
2+ & 2- Salts or Bases
4 Calcium sulfate
1 Calcium carbonate
1+ & OH, HCO3, CO3
4 Sodium hydrogen carbonate
4 Sodium hydroxide
4 Ammonium hydroxide
Strong acids
4 Hydrochloric acid
4, 5 Sulfuric acid
Inorganic molecules
1 Water
1 Carbon dioxide (carbonic acid)
3 Oxygen
3 Nitrogen
Hydrocarbons
1 Methane
3 Octane
3 Paraffin wax
3 Polyvinyl chloride (PVC)
Alcohols
1 Ethanol
5 Sugar
Weak organic acids
3 Acetic acid (in water)
5 Amino acids
5 Fatty acids
Formula
Polymer
Example Use
He
Ar
0.93% of air
Tube lights
Cu (not Cu2+)
Al
Wire, pipes
Many
NaCl
NH4NO3
Ca(H2PO4)2
Eat
Fertilizer
Fertilizer
CaSO4
CaCO3
Plaster walls
Cement
NaHCO3
NaOH
NH4OH (in water)
Baking
Oven cleaner
Floor Cleaner
HCl (in water)
H2SO4 (in water)
Stomach, pool
Car batteries
H2O
CO2
O2
N2
Lots
0.04% Air
21% of Air
78 % of air
(H2CO3)
(in soda pop)
CH4
CH3(CH2)6CH3
CH3(CH2)18-38 CH3
(-CH2CHCl-)100
Plastics
Natural gas
Gasoline
Candles
PVC pipes
CH3CH2OH
Ring; lots C-OHs
Carbohydrate
Beer
Starch
CH3COOH
H2NCH“R”COOH
CH3(CH2)16COOH
Proteins
Vinegar
Meat, gelatin
Fats
Element/Atom-A single type of chemical; i.e., those chemicals shown on the periodic table. Ex of a pure element-copper in pipes
Atomic formula-The smallest unit of a pure element. Ex. Cu represents one copper atom
Metallic bond-Strong electrostatic attraction that joins atoms of metals to each other due to sharing of freely moving electrons
Ionic compound-A chemical consisting of two or more atoms of two or more different elements joined by ionic bonds. Ex. table salt
Ionic formula-The smallest unit of a single ionic compound. Ex. NaCl represents one sodium ion and one chloride ion
Ionic bond-Strong electrostatic attraction that joins an atom that has lost one or more electrons (positive ion) and an atom that has gained
one or more electrons (negative ion).
Molecule-A chemical consisting of two or more atoms joined by covalent bonds. Ex. alcohol, carbon dioxide, water, oxygen
Written formula-The smallest unit of a single molecule. Ex. CH3CH2OH ethanol, CO2 carbon dioxide, H2O water, O2 oxygen (same atoms)
Covalent bond-Strong electrostatic attraction that joins two atoms that share electrons to create a full, stable shell.
Organic-A chemical that exhibits the normal oxidation-reduction: combustion reaction (i.e. burning) (ex. CH3CH2OH ethanol); normally a
chemical that contains C-H somewhere in its formula. Historically, organic chemicals were made by living organisms. Since the chemical
synthesis of urea, chemists also have been able to synthesize organic chemicals.
Inorganic-A chemical that does not exhibit the normal oxidation-reduction: combustion reaction (i.e. burning) (ex. CO2 carbon dioxide and
H2O water); may have a carbon, but does not have a C-H. Includes all noble gases, metals, ionic compounds, and some molecules.
Acid-A chemical that when dissolved in water loses H+ ions, hence the solution has a pH less than 7. Pink or purple in cabbage juice.
Neutral-A chemical that when dissolved in water does not lose H+ or gain H+, hence the solution remains at pH 7. Blue in cabbage juice.
Base-A chemical that when dissolved in water gains H+ ions, hence the solution has a pH greater than 7. Green in cabbage juice.
Organic acids-Have a –COOH group that can lose a H+ ion, making an aqueous (water) solution acidic.
Alcohols-Have a –COH group that does not lose a H+ ion.
Hydrocarbon-Have only carbon chains with hydrogen atoms attached.
Hydrogen Bond-a 5% bond between the lone pair of an O or N atom and the partly positive hydrogen atom attached to an O or N “bully.”
Van der Waal’s Forces-a “1%” bond between temporarily negative and temporarily positive regions, especially of long CH2 chains.
Solids-Have strong metallic bonds, strong ionic bonds, many hydrogen bonds, or extensive Van der Waals forces that hold the atoms, ions, or
molecules to each other tightly; the melting point is above room temperature (22o C). The atoms, ions, or molecules form a rigid structure.
Liquids-Have a few hydrogen bonds or limited Van der Waals forces that hold the molecules to each other weakly (ex. water, ethanol);
hence, the melting point is below room temperature (0o C ice/water) and the boiling point is above room temperature (100oC water/water
vapor or steam). Mercury is the only liquid metal; there are no liquid ionic compounds. The molecules are close together but movable.
Gases-Have no interactions between atoms or molecules; hence, the melting and boiling points are below room temperature (ex. Noble gases
like neon or molecules like methane; i.e. natural gas). The atoms or molecules are far apart and moving quickly.
Soluble-A chemical is soluble in water when its ability to hydrogen bond to water is sufficient to overcome its preference to stick to itself.
Insoluble-A chemical is insoluble in water when its ability to hydrogen bond to water is not sufficient to overcome its preference to stick to
itself. Insoluble ionic compounds have stronger ionic bonds & long chains of CH2 groups, such as fats, have strong Van der Waals forces.