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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.