+ ---> name = + ---> name = + ---> name =

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1 Nomenclature Guide (inorganic) Case 1 - Nonmetal + Nonmetal 1. First element retains its name. 2. Second element gets -ide ending. 3. Use Greek prefixes to identify the # of atoms Examples: (ignore the 1 st one if it's a '1') N2O = Greek prefixes: /2- SO3 = carbon dioxide BrF 3 diphosphorus pentasulfide N 2 O 4 Case 2 - fixed metal + nonmetal 1. Metal retains its name. make sure ions join to form a neutral compound 2. Non-metal retains its ionic name. Examples Na + + Cl - ---> name = Ca +2 + Cl - ---> name = + ---> name = + ---> name = + ---> name = lithium bromide Al 2 S 3 magnesium hydroxide (NH 4 ) 2 SO 3 aluminum acetate Ba(NO 3 ) 2

2 Case 3 - variable charge metal + nonmetal 1. Metal gets its charge written w/ Roman # in ( ) after name 2. Non-metal retains its ionic name. Examples: Fe +2 + Cl - ---> name = Fe +3 + Cl - ---> name = + ---> name = + ---> name = manganese (IV) chloride Cr(OH) 3 nickel (III) carbonate CuCO 3 Case 4 - Acids (positive ion = "H + ") 1. Drop the ending on the negative ion. The -ate ending changes to -ic acid. The -ite ending changes to -ous acid. The -ide ending uses the prefix hydro- and the suffix -ic acid Examples: H2CrO4 = HNO2 = HCl = hydrobromic acid H 3 PO 3 perchloric acid HI hydrates when ionic substances have water molecules attached, theyʼre called hydrates MgSO4 3 H2O = calcium phosphate tetrahydrate = NaC2H3O2 2 H20 =

3 Packet #3 Objectives (know these for quiz...) nomenclature (how to write names and formulas) for inorganic compounds (WS 3.1 ~ 3.2) similarities & differences between ionic and covalent bonding (WS 3.3 & powerpoint notes) know how to determine the # of e - transferred during ionic bonding how to use the formula on WS 3.4 to calculate the # of bonds in a Lewis dot structure (WS 3.4) how to draw Lewis dot structures (WS 3.4) the definition & developer of electronegativity, how to calculate Δ EN, how to draw dipole arrow (WS 3.5) how to determine molecular geometry & polarity from a Lewis dot structure (WS 3.6) how to calculate energy of a photon (flame test lab, packet 2) (commonly missed? from last quiz) WS 3.2 answer bank ammonium hydroxide, ammonium sulfide, boric acid, bromine trifluoride, calcium nitrite, calcium carbonate, calcium fluoride, carbon tetrachloride, copper (II) chloride hexahydrate, hydrosulphuric acid, iron (II) iodate, iron (II) phosphate, lithium oxalate, magnesium sulfate heptahydrate, magnesium thiosulfate, nitric acid, phosphite ion, phosphorus trioxide, potassium bicarbonate, potassium nitrate, sodium bisulfite, sulphur tetrachloride, sulphur trioxide, tin (II) iodide, tin (II) phosphate, vanadium (V) bromate Al(C2H3O2)3, AlI3, BCl3, Ba(CN)2, BrF7, CaH2, Co(NO3)3 4 H2O, CO, CO2, CS2, Cu3(PO4)2, H2C2O4, HClO3, HNO2, H3PO3, Hg3(BO3)2, KClO3, KCN, KOH, NaCl, NaC2H3O2 5 H2O, NH4C2H3O2, PbS, SeS2, Si2O3, Sr(NO3)2, ZnSO4 Video Questions- Bonding Name 1. Why are the noble gases chemically inert? 2. How many valence electrons are in sodium? 3. What charge does sodium get when it forms an ion? 4. Chlorine needs to (gain / lose) how many electrons in order to achieve a noble gas configuration? 5. When salt is viewed with an electron microscope, what basic shape does it have? 6. When the bulb slowly lights, what does Don Showalter say? (guess: ) (actual: ) a) "Wow!" b) "Look at that bulb!" c) "Here we go; the bulb is lit" d) "How about that!" 7. Which of the crystalline substances conducted electricity when in solution? 8. The formation of a covalent bond is an (endothermic / exothermic) process. 9. The N-N triple bond is (stronger / weaker) than the single N-I bonds in NI When the nitrogen triiodide ("small brownish pile") explodes, what does Don Showalter say? a) "There it goes!" b) "Wow, what a reaction!" c) "Did you see that!?!" d) "Now my eyebrows are really spiked!" 11. Today's explosive of choice, which is also a fertilizer, is.

4 Octet Rule: What Is An Ionic Bond? How Does An Ionic Bond Form? Ionic Bonding Diagrams NaCl CaCl 2 Al 2 O 3 Single Covalent Bond Double Covalent Bond Triple Covalent Bond

5 electronegativity: developed by: structure Δ EN bond type nonpolar covalent polar covalent ionic

6 # of e- pairs (regions) Valence Shell Electron Pair Repulsion Theory (VSPER) e- geometry bonding diagram molecular geometry (pull the ropes) polarity example bond angle: bond angle: bond angle:

7 Common Ions To Memorize For Quiz, Regular Chemistry: 1 + ions 1 - ions H +1 hydrogen Li +1 lithium Na +1 sodium K +1 potassium F -1 Cl -1 Br -1 I -1 fluoride chloride bromide iodide NH 4 +1 ammonium 2 + ions Mg 2+ magnesium Ca 2+ calcium Ba 2+ barium NO -1 2 NO -1 3 ClO -1 ClO -1 2 ClO -1 3 ClO -1 4 OH -1 CN -1 nitrite nitrate hypochlorite chlorite chlorate perchlorate hydroxide cyanide C 2 H 3 O -1 2 acetate Al ion aluminum 2 - ions O 2- S 2- oxide sulfide CO 3 2- SO 3 2- SO 4 2- carbonate sulfite sulfate 3 - ions N 3- P 3- nitride phosphide PO 3 3- PO 4 3- phosphite phosphate