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Chapter 3
Molecules, Compounds, and Chemical Equations
| Term | Definition |
|---|---|
| Compound Different From Mixture of Elements | In a compound, elements combine in fixed, definite proportions; in a mixture, elements can mix in any proportions whatsoever |
| Ionic Bonds | Occur between metal and nonmetal. Involve the transfer of electrons from one atom to another(cation to anion) |
| Covalent Bonds | Occur between two or more nonmetals or mettaloids. Involve the sharing of electrons between two atoms |
| Cation | Positively charged ion |
| Anion | Negatively charged ion |
| Ionic Bond | Bond between a cation and anion. Forms ionic compound |
| Ionic Compound | A lattice - a regular three-dimensional array - of alternating cations and anions |
| Covalent Bond | The bond between two nonmetals. Form molecules |
| Molecular Compounds | Covalently bonded compounds |
| Chemical Formula | Indicates the elements present in the compound and the relative number of atoms or ions for each. There are 3 types of chemical formulas... 1. Empirical.. 2. Molecular.. 3. Structural |
| Empirical Formula | Gives the relative number of atoms of each element in a compound |
| Molecular Formula | Gives the actual number of atoms of each element in a molecule of a compound |
| Structural Formula | Uses lines to represent covalent bonds and show how atoms in a molecule are connected or bonded to each other |
| Molecular Model | A more accurate and complete way to specify a compound |
| Ball-and-stick molecular model | Represents atoms as balls and chemical bonds as sticks; how the two connect reflects a molecule's shape |
| Space-filling molecular model | Atoms fill the space between each other to more closely represent our best estimates for how a molecule might appear if scaled to visible size |
| Atomic Elements | Exist in nature with single atoms as their basic units |
| Molecular Elements | Do not normally exist in nature with single Atoms as their basic units; instead they exist as molecules - two or more atoms of the element bonded together |
| List of Molecular Elements To Memorize | 1. O2.. 2. I2.. 3. Br2.. 4. N2.. 5. Cl2.. 6. F2.. 7. H2.. |
| Molecular Compounds | Usually consist of two or more covalently bonded nonmetals. Ex: H2O, CO2, C3H8 |
| Ionic Compounds | Composed of cations(usually a metal) and anions(usually one or more nonmetals) bound together by ionic bonds |
| Formula Unit | Basic unit of an ionic compound. The smallest, electrically neutral collection of ions. Ex: Na+, Cl- |
| Polyatomic Ion | An ion composed of two or more atoms |
| Summarizing Ionic Compound Formulas | 1. Ionic compounds always contain + and - ions.. 2. In a chemical formula, the sum of the charges of the + ions(cations) must equal that of - ions(anions).. 3. The formula of an ionic compound reflects the smallest whole-number ratio of atoms |
| Ionic Compound Common Names | Nicknames of sorts learned by familiarity. Ex: NaCl(table salt), NaHCO3(baking soda) |
| Systematic Names | Names made by chemists for different types of compounds including ionic ones |
| Remember When Naming Compounds | Ionic compounds are usually composed of metals and nonmetals; any time you see a metal and one or more nonmetals together in a chemical formula, assume that you have an ionic compound |
| Binary Compounds | Contain only two different elements |
| Naming Ionic Binary Compounds | Name of cation(metal) + base name of anion(nonmetal) + -ide |
| Naming Binary Ionic Compounds Containing a Metal That Forms More Than One Kind of Cation | Name of cation(metal) + (charge of cation(metal) in roman numerals in parentheses) + base name of anion(nonmetal) + -ide |
| The following are Polyatomic Ions | |
| CO3^-2 | Carbonate |
| C2O4^-2 | Oxalate |
| CH3CO2^-1, CH3COO^-1, C2H3O2^-1 | Acetate |
| CN^-1 | Cyanide |
| O2^-2 | Peroxide |
| OH^-1 | Hydroxide |
| N3^-1 | Azide |
| NO3^-1 | Nitrate |
| NO2^-1 | Nitrite |
| NH4^+1 | Ammonium |
| PO4^-3 | Phosphate |
| (PO3^-3) | Phosphite |
| S2^-2 | Disulfide |
| SO4^-2 | Sulfate |
| SO3^-2 | Sulfite |
| SCN^-1 | Thiocyanate |
| ClO4^-1 | Perchlorate |
| ClO3^-1 | Chlorate |
| ClO2^-1 | Chlorite |
| ClO^-1 | Hypochlorite |
| BrO4^-1 | Perbromate |
| BrO3^-1 | Bromate |
| BrO2^-1 | Bromite |
| BrO^-1 | Hypobromite |
| IO4^-1 | Periodate |
| IO3^-1 | Iodate |
| IO2^-1 | Iodite |
| IO^-1 | Hypoiodite |
| CrO4^-2 | Chromate |
| Cr2O7^-2 | Dichromate |
| MnO4^-1 | Permanganate |
| The Following Are Monatomic Ions | |
| O^-2 | Oxide |
| N^-3 | Nitride |
| P^-3 | Phosphide |
| S^-2 | Sulfide |
| F^-1 | Fluoride |
| Cl^-1 | Chloride |
| Br^-1 | Bromide |
| I^-1 | Iodide |
| Binary Ionic Compounds Containing a Metal That Forms More Than One Kind of Cation | Name of cation(metal) + (charge of cation(metal) in roman numerals in parentheses) + base name of anion(nonmetal) + -ide |
| Oxyanions | Anions containing oxygen and another element |
| Hydrates | Ionic compounds containing a specific number of water molecules associated with each formula unit |
| Molecular Compound Composition | Molecular compounds are composed of two or more atoms |
| Naming Molecular Compounds | Prefix + name of 1st element + prefix + base name of 2nd element + -ide |
| Molecular Compound Prefixes | Prefixes given to each element indicate number of atoms present. Normally you don't use the prefix mono- if there is only 1 atom of first element. 1. Hemi 2. Mono 3. Di 4. Tri 5. Tetra 6. Penta 7. Hexa 8. Hepta 9. Octa 10. Nona 11. Deca |
| Hemi | 1/2 |
| Mono | 1 |
| Di | 2 |
| Tri | 3 |
| Tetra | 4 |
| Penta | 5 |
| Hexa | 6 |
| Hepta | 7 |
| Octa | 8 |
| Nona | 9 |
| Deca | 10 |
| Atomic Mass | The average mass of an atom of an element |
| Formula Mass(Molecular Mass/Weight) | The average mass of a molecule(or a formula unit) of a compound |
| Formula Mass Equation | Formula Mass = (Number of atoms of 1st element in chemical formula * atomic mass of 1st element) + (number of atoms of 2nd element in chemical formula * atomic mass of 2nd element) + ... |
| Molar Mass of a Compound | The molar mass of a compound - the mass in grams of 1 mol of its molecules of formula units - is numerically equivalent to its formula mass. Compound molar mass = formula mass(g)/1 mol |
| Mass Percent Composition(Mass Percent) | An element's percentage of the compound's total mass |
| Mass Percent Composition Formula | Mass Percent of element X = [(mass of element X in 1 mol of compound)/(mass of 1 mol of the compound)] * 100 |
| General Form for Solving Problems Where We Are Asked To Find The Mass of an Element Present in a Given Mass of A Compound | Mass compound --> moles compound --> moles element --> mass element |
| Molecular Formula is Always a Whole Number multiple of the Empirical Formula | Molecular Formula = empirical formula x n, where n = 1, 2, 3,..... n = (molar mass)/(empirical formula mass) |
| Empirical Formula Molar Mass | The sum of the masses of all the atoms in the empirical formula |
| Combustion Analysis | A method of obtaining empirical formulas for unknown compounds, especially those containing carbon and hydrogen, by burning a sample of the compound in pure oxygen and analyzing the products of the combustion reaction |
| Chemical Reaction | A process in which one or more substances are converted into one or more different ones |
| Combustion Reaction | A particular type of chemical reaction in which a substance combines with oxygen to form one or more oxygen containing compounds |
| Chemical Equation | A symbolic representation of a chemical reaction; a balanced equation contains equal numbers of the atoms of each element on both sides of the equation |
| Reactants | The substances on the left side of the chemical equation |
| Products | The substances on the right side of the chemical equation |
| Subscript 0.20 | Multiply by 5 |
| Subscript 0.25 | Multiply by 4 |
| Subscript 0.33 | Multiply by 3 |
| Subscript 0.40 | Multiply by 5 |
| Subscript 0.50 | Multiply by 2 |
| Subscript 0.66 | Multiply by 3 |
| Subscript 0.75 | Multiply by 4 |
| Subscript 0.80 | Multiply by 5 |
| The Following Are More Charges to Remember | P^-3.. Zn^+2.. Ag^+.. Ga^+3.. In^+3 |
| In Naming Acids | Ends in... 1. -ide(hydro___ic acid).. 2. -ate(___ic acid).. 3. -ite(___ous acid) |
| All Polyatomic Ions with N(except NH4-ammonium with +1 charge) | Have -1 charge(except NH4 ammonium) |
| All Polyatomic Ions with P | Have -3 charge |
| All Polyatomic Ions with S(except SCN - thoicyanide with -1 charge)) | Have -2 charge |
| All Polyatomic Ions with CL | Have -1 charge |
| All Polyatomic Ions with Br | Have -1 charge |
| All Polyatomic Ions with I | Have -1 charge |
| All Polyatomic Ions with Cr | Have -2 charge |
| All Polyatomic Ions with Mn | Have -1 charge |
Created by:
TimChemistry1
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