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What is the charge of iron in Fe2O3? Determine the charge on a multi-charge ion Total ion charge 1. 2. 3. 4. +6 +3 Fe2 -6 -2 O3 Determine the charge on the other atom Multiply the charge by the subscript ie. 2 x 3 = 6 This is the total charge for the other ion. Divide this number by the subscript and that is the charge on each of that ion. Charge of each ion H –hydrogen N – nitrogen O – oxygen F – fluorine Cl – chlorine Br – bromine I – iodine At- astatine All written as diatomic molecules in elemental state Creation of oxidation numbers 1. If the atom has less than 3 electrons then the atom will give them up. 2. If the atom has more than 5 electrons then the atom will gain up to a total of 8 electrons 3. If the atom has 4 it can go either way. 4. The transition metals are exceptions to these rules and they can follow them or not. 1- mono 2- di 3- tri 4- tetra 5- penta 6- hexa 7- hepta 8- oct 9- nano 10 - deca If the polyatomic ion ends in ate, replace with -ic + acid If the polyatomic ion ends in ite, replace with –ous + acid If the acid is binary – start with hydro, then use the anion & end with – ic if name ends in ic, then look for a polyatomic ion ending in ate if the name has the prefix hydro- it is a binary acidanion is probably a halogen. HCO3-1 -bicarbonate SO4 –2 –sulfate -2 SO3 -sulfite –2 CO3 - carbonate -1 ClO4 -perchlorate -1 ClO3 -chlorate -1 ClO2 -chlorite –1 ClO –hypochlorate –1 OH – hydroxide –1 NO3 – nitrate -1 NO2 - nitrite -1 CN cyanide PO4 –3 – phosphate +1 NH4 - ammonium -2 S2O3 -thiosulfate –1 C2H3O2 – acetate MnO4 -permanganate -2 CrO4 -chromate Cr2O7 -dichromate Yes Is it ionic Does the cation have more than 1 oxidation number? Yes No 1) determine charge on cation 2) write full name followed by a Roman numeral 3) write anion name if polyatomic – if only 2 atoms, then name ends in ide 1. Write full name of cation. 2. Write full name of anion if polyatomic 3. Use an ide ending if only two atoms present. Yes Is it ionic No 1. Convert subscript after first element to a Greek prefix & attach to full name of first element 2. If only two elements present apply #1 to the second element and end name in ide. No Does the cation have a Roman numeral? Yes No 1. use the Roman numeral as the charge on the cation 2. balance the formula 3. use an ide ending if only two elements present. 1. Write cation symbol first, anion symbol second. 2. Use the most common charge to balance the formula 3. Subscripts should be written in lowest whole number ratio. 1. Use prefix as a subscript for each element. 2. If only2 elements present end second in ide. 3. First element name will not have a prefix if only 1 atom present. 1. 2. 3. 4. Write out rough formulas with reactants and products. Balance formulas using the flow charts. Use subscripts to balance formulas Write the elements on both sides (you may delete this step later). Starting with the left side use coefficients to obtain equal number of the same element on both sides of the equation. Use coefficients to balance equations. 5. Leave H & O until the end. 6. If you get an odd-even coefficient result, go back an double all coefficients assigned to that point. Total mass in grams = 1 mole Particles 6.02 x1023 particles = 1 mole Moles of 1st substance Grams Liters Ratio of coefficients Particles Moles of 2nd substance @ STP 22.4 L = 1 mole Grams Liters Metals NonMetals 1. 2. 3. 4. Electron Configuration Electronic configuration is under the element name The symbol in square brackets is the inner core of electrons Usually only the electrons outside of the core are involved in bonding. You remove highest level electrons first, then the next level electrons Na = [Ar] 3s1 Na+ = [Ar] notice the 3s1 electron is gone. If you remove all of the electrons from either a level or type you do not write that location in the final configuration.