CHM 105 & 106 MO1 UNIT FOUR, LECTURE SIX 1 TODAY WE RE GOING TO SPEND OUR TIME LOOKING ONCE AGAIN AT NOMENCLATURE AND

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1 CHM 105 & 106 MO1 UNIT FOUR, LECTURE SIX 1 CHM 105/106 Program 35: Unit 4 Lecture 6 TODAY WE RE GOING TO SPEND OUR TIME LOOKING ONCE AGAIN AT NOMENCLATURE AND TRYING TO COMPLETE OUR DISCUSSION IN CHAPTER EIGHT RELATIVE TO NOMENCLATURE. THE LAST TIME WE TALKED ABOUT CHEMICAL NOMENCLATURE WE HAD JUST BEGUN LOOKING AT THREE RULES WHICH CAN BE APPLIED WHICH PROVIDE US WITH TOOLS TO ADD A LARGE NUMBER OF OTHER, ESPECIALLY ANIONS, TO OUR LIST. WE HAD THE LIST IN THE CHAPTER OF WHICH HAD THOSE WITH THE MINUS ONE CHARGE. WE HAD SIX OF THOSE. WE HAD THREE OR FOUR WITH A TWO MINUS CHARGE, AND WE HAD TWO THAT WERE MINUS THREE CHARGES. THESE THREE RULES THEN ALLOW US TO GREATLY INCREASE THE NAMES AND THE CHARGE AND THE CHEMICAL FORMULA OF A WHOLE BUNCH OF OTHER POLYATOMIC ANIONS, AND WE LL APPLY THOSE THEN AS WE GO THROUGH THE DAY, BUT ONCE AGAIN THIS CAN HIGHLIGHT RULE NUMBER ONE SAYS THAT IF WE HAVE ONE OXYGEN LESS THAN THE ATE ION, WHATEVER THE ATE IS NITRATE PHOSPHATE, ACETATE, CARBONATE, DOESN T MAKE ANY DIFFERENCE. IF THE ANION NORMALLY ENDS IN ATE WE REMOVE ONE OXYGEN FROM THAT IN THE CHEMICAL FORMULA. DOESN T CHANGE THE CHARGE, BUT WE CHANGE THE NAME THEN TO ITE, I-T-E, AND THE EXAMPLE THAT WE SEE HERE IS CHLORATE FROM OUR TABLE IN THE TEXT, IS ClO 3 WITH A MINUS CHARGE. IF WE REMOVE ONE OXYGEN IT STILL STAYS A MINUS ONE CHARGE BUT THE NAME OF THE ION NOW BECOMES CHLORITE. SO YOU SEE JUST THAT ONE SIMPLE RULE IN ITSELF NOW DOUBLES THE NUMBER OF POLYATOMIC ANIONS NAMEWISE, FORMULAWISE, AND CHARGEWISE WE WOULD KNOW IF WE KNEW THE TABLE ITSELF. SO KNOWING THE TABLE THEN IS IMPORTANT BECAUSE BY USING THAT TOOL OF COURSE WE CAN GREATLY INCREASE THE NUMBER OF IONS. RULE NUMBER TWO THEN AS WE LOOKED AT THE OTHER DAY SAYS IF WE ADD A HYDROGEN TO A TWO MINUS OR A THREE MINUS ATE OR ITE ION THEN IT GIVES US THE NAME HYDROGEN, WHATEVER THE NAME OF THE ION WAS BEFORE AS AN ATE OR AN ITE, HYDROGEN WHATEVER ATE OR ITE. THE EXAMPLE HERE IS CARBONATE. WHEN WE ADD A HYDROGEN TO THIS NOW WHEN WE ADD A HYDROGEN TO IT NOTICE THAT THE CHARGE IN FACT DID CHANGE. SO THAT S ONE THING WE HAVE TO KEEP IN MIND BECAUSE

2 CHM 105 & 106 MO1 UNIT FOUR, LECTURE SIX 2 WE RE ADDING A PLUS ONE HYDROGEN TO THE ION AND THAT S WHY ITS CHARGE DECREASED BY ONE. NOTICE CARBONATE IS TWO MINUS. THIS ION NOW WITH A HYDROGEN ON IT HAS ONLY A MINUS ONE CHARGE. HYDROGEN CARBONATE THEN WE CALL IT. NOW THE REASON THAT WE RE LIMITED TO THOSE IONS THAT HAVE A MINUS TWO OR A MINUS THREE CHARGE IS BECAUSE IF THEY HAD ONLY A MINUS ONE CHARGE WE WOULD HAVE A NEUTRAL MOLECULE. WE COULDN T ATTACH IT TO ANYTHING. IT WOULDN T BE AN ION ANYMORE. IT WOULD BE A NEUTRAL MOLECULE. AND IT WOULD BE NAMED THEN AS A COMPOUND. ALRIGHT, SO IT HAS TO BE THE IONS WITH A TWO MINUS OR A THREE MINUS CHARGE IN ORDER TO ADD THE HYDROGENS TO IT. AND THE THIRD RULE JUST TAKES US BACK TO OUR KNOWLEDGE OF THE PERIODIC TABLE AND CHEMICAL FAMILY SIMILARITY. WE RE SAYING THAT IF, IN FACT, WE MEMORIZE ONE OF THE POLYATOMIC IONS OF THE FAMILY THEN WE SHOULD BE ABLE TO PREDICT THE OTHER IONS IN THE FAMILY AS WELL. AN EXAMPLE HERE IS THAT THE TABLE GAVE US CHLORATE. ALRIGHT, THAT S THE TABLE IN THE TEXT GAVE US THE FORMULA ClO 3 WITH A MINUS CALLED CHLORATE. WELL, WE SEE THAT IN THAT SAME FAMILY NOW WE HAVE BROMINE, IODINE, ASTATINE. SO IF CHLORATE IS ClO 3 WITH A MINUS ONE CHARGE IT WOULD BE LOGICAL THAT BROMATE WOULD BE BrO 3 MINUS ONE, AND IODATE WOULD BE IO 3 MINUS ONE, AND FLUORATE WOULD BE FO 3 MINUS ONE. ALRIGHT, SO THAT THE FAMILY SIMILARITY, OR WE GO OVER HERE TO SULFATE. IT S SO 2-4. SELENIUM THEN SeO 2-4 IS SELENATE. SO AGAIN WE SEE THE FAMILY CHARACTERISTIC INVOLVED. NOW YOU SEE WITH THAT AND WITH RULE NUMBER ONE NOT ONLY DO WE KNOW THE FORMULA NOW OF CHLORATE AND ITS CHARGE, WE NOW KNOW CHLORATE, BROMATE, IODATE, BUT RULE NUMBER ONE, WHICH SAYS TAKE ONE OXYGEN AWAY, WE NOW KNOW CHLORITE, BROMITE, AND IODITE AS WELL. SO THESE THREE RULES GREATLY EXPAND THE IONS THAT WE SHOULD BE ABLE TO RECOGNIZE IF, IN FACT WE KNOW THOSE FROM THE TABLE IN THE CHAPTER. ALRIGHT, WELL LET S APPLY THESE PRINCIPLES THEN, NOW THESE RULES, TO NAMING SOME COMPOUNDS AND WRITING SOME CHEMICAL FORMULAS, AND AT FIRST WE LL LOOK AT THE NAMING PART. FIRST ONE, KNO 2. ALRIGHT, SO WE RE GONNA NAME THE METAL AND THEN WE RE GONNA NAME THE POLYATOMIC ION. THE METAL IS POTASSIUM. AND NOW WE HAVE TO DETERMINE WHAT NO 2 IS.

3 CHM 105 & 106 MO1 UNIT FOUR, LECTURE SIX 3 WELL, IF WE REFER BACK TO THE TABLE WE FIND THAT NO 3 IS CALLED THE NITRATE ION. SO NO 2 IS GOING TO BE THE NITRITE ION. THAT S RIGHT, SO POTASSIUM NITRITE WILL BE THE NAME. THIS IS THE IMPORTANT PART THIS TIME, WHICH IS DIFFERENT OF COURSE THEN THAN NITRATES THAT WE NAMED BEFORE. ALRIGHT, WE GO THROUGH THIS ONE. THAT ACTUALLY WAS AN EXAMPLE INVOLVING RULE NUMBER TWO. THE NEXT ONE, NAME THE METAL LITHIUM, AND NOW WE HAVE TO NAME THE POLYATOMIC ION. IF WE LOOK AT THE CHART OF COURSE WE DON T SEE BrO 3, BUT WE SEE THE FAMILY MEMBER. WE SEE CHLORATE, ClOb3n. SO THEREFORE WE WOULD PREDICT THAT BASED ON RULE NUMBER THREE THE NAME OF THIS ION WILL BE BROMATE. CHLORATE, BROMATE. THE NEXT ONE, AGAIN WE NAME THE METAL. NOW, IN THIS PARTICULAR CASE OF COURSE WE SHOULD POINT OUT THAT THE METALS THAT WE RE DEALING WITH HERE ARE ALL THE METALS THAT HAVE ONLY ONE CHARGE. THAT S WHY WE RE NOT USING ANY ROMAN NUMERALS IN THE NAMES. THEY RE JUST MERELY THOSE THAT ARE IN COLUMN ONE, COLUMN TWO, OR THOSE OTHER FOUR THAT WE MENTIONED, ALUMINUM ALWAYS PLUS THREE; ZINC, CADMIUM ALWAYS PLUS TWO; AND SILVER ALWAYS PLUS ONE. SO THESE ARE THOSE THAT WE CALL UNIVALENT. THEY HAVE ONLY ONE CHARGE. MAGNESIUM AND NOW I NEED TO KNOW WHAT S THE NAME OF ClO 2? AGAIN WE LOOK AT THE TABLE. WE SEE THAT ClOb3n IS CHLORATE. SO THEREFORE ClOb2n WOULD BE CHLORITE. SO ONE OXYGEN LESS ONCE AGAIN, AND SO WE HAVE THE ITE ION IN THIS CASE, CHLORITE. THE NEXT ONE, Na IS SODIUM, AND THEN WE LOOK AT THE SO 3. AGAIN IF WE LOOK IN THE TABLE WE DON T FIND SO 3, WE FIND SO 4. SO 4, THE SULFATE ION, AND SO SO 3 MUST BE THE SULFITE ION, ITE ENDING. ALRIGHT, THE NEXT ONE, THE METAL IS ZINC, AND NOW WE NOTICE THAT WE HAVE A HYDROGEN-CONTAINING ION IN THERE, AND IN THAT PARTICULAR CASE THEN WE RE GOING TO CALL IT HYDROGEN AND WHATEVER THE ION IS THAT IT S ATTACHED TO AND CO 3 IS CARBONATE. SO THIS PARTICULAR ION THAT S IN THE PARENTHESES THERE, THIS HCO 3 IS CALLED HYDROGEN CARBONATE, ALL ONE WORD. HYDROGEN CARBONATE. NOW NOTICE I DIDN T SAY ANYTHING ABOUT THIS LITTLE SUBSCRIPT 2 HERE. I WE DON T NEED TO IN THESE BECAUSE OF COURSE THE ONLY WAY THAT ZINC, WHICH HAS A CHARGE OF PLUS TWO, CAN COMBINE WITH HYDROGEN CARBONATE, WHICH NOW HAS A CHARGE OF MINUS ONE, IS A ONE

4 CHM 105 & 106 MO1 UNIT FOUR, LECTURE SIX 4 TO TWO RATIO. SO WE DON T NEED TO SAY ANYTHING MORE ABOUT IT. SO IT IS JUST ZINC HYDROGEN CARBONATE. OKAY, NOW THE NEXT ONE, THE METAL OF COURSE IS ALUMINUM AND THEN WE NOW HAVE THIS ANION. WELL IN THE CASE OF THE PHOSPHATE, TAKE THIS AWAY JUST A SECOND, IN CASE OF THE PHOSPHATE ION PO 3-4 WE HA VE TWO DIFFERENT FORMS THAT WE CAN MAKE FORM THAT IN TERMS OF ADDING A HYDROGEN. WE CAN ADD ONE HYDROGEN AND THAT MAKES THE HPO 2-4. WE CAN ADD TWO HYDROGENS AND THAT MAKES H 2 PO 4 WITH A 1 MINUS. SO WE HAVE TO BE ABLE TO IDENTIFY WHICH ONE OF THESE HYDROGEN PHOSPHATES WE ARE TALKING ABOUT. NOW THIS ISN T A PROBLEM WITH THE CARBONATE ION BECAUSE WE CAN ONLY DO IT ONCE. IF WE PUT TWO HYDROGENS WE RE AT A NEUTRAL COMPOUND AND THAT S NOT GONNA BE NAMED AS AN ION. SO WITH THE NEGATIVE THREE CHARGE WE CAN MAKE TWO DIFFERENT TYPES OF HYDROGENS. SO WE HAVE TO SPECIFY WHICH HYDROGEN PHOSPHATE WE RE TALKING ABOUT, AND IN THAT CASE THEN WE USE A PREFIX TO SHOW HOW MANY HYDROGENS. THIS ONE WOULD BE CALLED MONOHYDROGEN PHOSPHATE. AND THIS ONE WOULD BE CALLED DIHYDROGEN PHOSPHATE. OKAY, BUT THOSE ARE ONLY GOING TO HAPPEN WHERE WE HAVE TO SPECIFY HOW MANY HYDROGENS IN THE TWO CASES OF 3 - IONS THAT WE TALKED ABOUT, PHOSPHATE AND BORATE. THOSE ARE THE ONLY TWO IN THE TABLE THAT WE HAVE THAT ARE THREE MINUS. OR WE COULD HAVE PO 3 PHOSPHITE. SO WE COULD HAVE A MONOHYDROGEN PHOSPHITE AND WE COULD HAVE A DIHYDROGEN PHOSPHITE AS WELL. OKAY, IF WE HAVE THE PO 3, THREE MINUS ION, RULE NUMBER ONE. NOW, KEEPING THIS IN MIND THEN NOW WE LL GO BACK AND FINISH UP THE ONE THAT W E WERE LOOKING AT HERE. WE THEN SEE THAT WE HAVE TWO HYDROGENS IN THIS POLYATOMIC ANION THIS TIME, SO THAT MUST BE CALLED DIHYDROGEN PHOSPHATE. JUST ABOUT RAN OUT OF ROOM THERE, DIALUMINUM DIHYDROGEN PHOSPHATE WOULD BE THE NAME. AGAIN, NOTICE I DON T HAVE TO SAY ANYTHING ABOUT THIS BECAUSE THE CHARGE ON THE DIHYDROGEN PHOSPHATE ANION IS A MINUS ONE, AND THE CHARGE ON ALUMINUM IS ALWAYS PLUS THREE, SO THE ONLY WAY I CAN PUT THOSE TOGETHER IS ONE TO THREE COMBINATION. NOW LET S REVERSE THE PROCESS. WE LL START WITH THE NAME AND WRITE THE CHEMICAL FORMULA FOR THESE NEW TYPE OF CATEGORY OF COMPOUNDS. ALRIGHT, THE

5 CHM 105 & 106 MO1 UNIT FOUR, LECTURE SIX 5 FIRST ONE WE RE GIVEN SODIUM HYDROGEN CARBONATE, SO WE WOULD WRITE DOWN Na, AND THEN WE WOULD WRITE DOWN THE FORMULA FOR HYDROGEN CARBONATE. THERE WOULD BE HCO 3. NOW WE HAVE TO LOOK AT THE CHARGES. THE SODIUM HAS A CHARGE OF PLUS ONE. IT S IN THE FIRST COLUMN OF THE PERIODIC TABLE. THE CARBONATE ION IS A TWO MINUS. SO WHEN I PUT A HYDROGEN WITH IT IT BECOMES A ONE MINUS. SO WE HAVE A PLUS ONE SODIUM AND A MINUS ONE HYDROGEN CARBONATE. SO THE CHARGES ALREADY CANCEL EACH OTHER AND THAT WOULD BE IT. SO WE HAVE A PLUS HERE AND A MINUS HERE. SO THE FORMULA IS JUST NaHCO 3, SODIUM HYDROGEN CARBONATE. LET S LOOK AT THE NEXT ONE HERE ALUMINUM SULFITE. ALRIGHT, SO ALUMINUM, AND IT HAS A CHARGE OF THREE PLUS. IT S ONE OF THOSE THAT HAS ONLY ONE CHARGE. SULFITE WELL, WE LOOK IN THE TABLE. WE FIND SULFATE IS SO 4, SO SULFITE WOULD BE SO 3 AND A TWO MINUS CHARGE. NOW IN THAT PARTICULAR CASE THEN, WHAT IS THE LEAST COMMON NUMBER TO THE THREE AND THE TWO? SIX. AND SO THEREFORE WE RE GONNA HAVE TO MAKE SURE WE HAVE A PLUS SIX CONTRIBUTION AND A MINUS SIX CONTRIBUTION SO WE WILL NEED TWO ALUMINUMS. SO AL 2 AND NOW REMEMBER ANYTIME YOU HAVE TO PUT A SUBSCRIPT FOR A POLYATOMIC ION YOU NEED TO PUT IT IN PARENTHESES FIRST. SO PARENTHESES (SO 3 ) AND THERE WOULD BE THREE OF THOSE. SO AL 2, SO 3 IN PARENTHESES SUBSCRIPT THREE [ AL 2 (SO 3 ) 3 ], ALUMINUM SULFITE. LET S LOOK AT THE NEXT ONE HERE, MAGNESIUM. WE FIND IT ONE THE CHART UP THERE, WE SEE ELEMENT NUMBER 12 IS A 2 +. BROMITE, WELL HERE WE HAVE TO APPLY TWO RULES. IF WE LOOK ATA THE TABLE WE DON T FIND BROMITE, WE DON T FIND BROMATE, BUT WE DO FIND CHLORATE, AND CHLORATE IS CLO 3. SO BROMATE WOULD BE BRO 3, AND THEN USING RULE NUMBER ONE, THE ITE IS ALWAYS ONE OXYGEN LESS SO IT WOULD BE BRO 2 AND THE ION HAS A MINUS CHARGE. WE SEE AGAIN THAT THE CHARGES AREN T BALANCED SO THEREFORE WE WOULD NEED TWO OF THE POLYATOMIC ANIONS. SO Mg PARENTHESES BrO 2 PARENTHESES SUBSCRIPT 2 [ Mg(Br0 2 ) 2 ] FOR MAGNESIUM BROMITE. YES, QUESTION? (STUDENT NOT AUDIBLE) THE QUESTION WAS AM I DECIDING I NEED TWO OF THE BROMITE BY USING THE CRISS-CROSS RULE THAT WE TALKED ABOUT THE OTHER DAY SO THAT THE CHARGE IS BALANCED? THAT IS CORRECT, AND WE DO NOT WRITE ONES. SO EVEN THOUGH WE RE

6 CHM 105 & 106 MO1 UNIT FOUR, LECTURE SIX 6 BRINGING A ONE OVER HERE FOR THE MAGNESIUM WE DON T WRITE THE ONE IN THE FORMULA. BUT THE TWO FROM UP HERE DOES SHOW UP DOWN HERE. OKAY, REMEMBER WE ONLY USE THE CRISS-CROSS IF THE CHARGES ARE NOT BALANCED. IF THEY RE ALREADY BALANCED THEN WE DON T USE IT. ALRIGHT, THE NEXT THREE THEN FINISHING UP HERE WE HAVE SODIUM DIHYDROGEN PHOSPHATE, SO SODIUM IS A PLUS ONE. FIRST COLUMN OF THE PERIODIC TABLE. DIHYDROGEN PHOSPHATE THEN IS H 2 PO 4. QUESTION IS WHAT IS THE CHARGE ON DIHYDROGEN PHOSPHATE? WELL THE PHOSPHATE IS THREE MINUS AND IF WE ADD TWO PLUSSES WE RE GOING TO END UP WITH A SINGLE MINUS CHARGE LEFT. THE CHARGES ARE THE SAME, SO WE LL NEED NO OTHER SUBSCRIPTS. SO JUST NaH 2 PO 4, THE SODIUM DIHYDROGEN PHOSPHATE. ALUMINUM NITRITE. Al, AGAIN IT S ONE THAT HAS ONLY THE ONCE CHARGE, THREE PLUS, NITRITE. AGAIN WE LOOKED IN THE TABLE WE SEE NITRATE, NO 3 WITH A MINUS CHARGE. NITRITE THEREFORE IS GOING TO BE NO 2 WITH A MINUS CHARGE. AND WE SEE THAT THE CHARGES AREN T BALANCED SO AGAIN WE WOULD BE USING THAT CRISS-CROSS IDEA. SO WE HAVE Al AND THEN WE LL HAVE TO HAVE PARENTHESES (NO 2 ) SUBSCRIPT THREE. THE LAST ONE, CALCIUM HYDROGEN PHOSPHATE. ALRIGHT, SO WE HAVE CALCIUM Ca LOCATED ON THE TABLE IT S A 2 PLUS, SECOND COLUMN, HYDROGEN PHOSPHATE. NOW, IF WE DON T SAY ANYTHING IT IMPLIES MON. SO YOU MIGHT SEE IT STATED EITHER WAY, MONOHYDROGEN PHOSPHATE OR JUST HYDROGEN PHOSPHATE. SO EITHER MEANS THE SAME THING. IT MEANS ONE HYDROGEN. IF IT DOESN T HAVE ONE IT HAS TO SAY DIHYDROGEN PHOSPHATE. SO THIS WILL BE JUST HPO 4. NOW GAIN, PHOSPHATE IS A THREE MINUS. IF WE ADD A HYDROGEN IT S GOING TO BECOME TWO MINUS. WE SEE THAT THE CHARGES ARE IN FACT THE SAME AND WE HAVE CaHPO 4. WE DON T NEED ANY OTHER FURTHER SUBSCRIPTS. NOW, IF WE WERE TO ENCOUNTER ONE OF THE METALS THAT ISN T IN THIS UNIVALENT WE WOULD STILL USE THE SAME PROCEDURE. LET S JUST TRY ONE HERE AS AN EXAMPLE FOR THAT. LET S SUPPOSE THAT I WAS GIVEN HE CHEMICAL FORMULA OF FeSO 3, AND I WAS GOING TO NAME THIS COMPOUND. NOW NAMING THIS COMPOUND OF COURSE WE COULD SEE THE TWO THINGS FIRST OF ALL WE RE GOING TO NAME IRON AND THEN WE RE GOING TO NAME THE POLYATOMIC ANION. AGAIN, THE TABLE SHOWS SO 4 AS SULFATE. SO SO 3 WOULD BE SULFITE. BUT THIS IS ONE OF

7 CHM 105 & 106 MO1 UNIT FOUR, LECTURE SIX 7 THOSE METALS NOW THAT WE HAVE TO SAY SOMETHING ABOUT ITS CHARGE. IT S ONE OF THOSE THAT S NOT A SINGLE CHARGED METAL, AND SO WE LL HAVE TO FIGURE OUT WHAT THE CHARGE IS. WELL WE LOOK AT THE SULFITE AND IT HAS A CHARGE OF MINUS TWO AND THERE S JUST ONE OF THEM SO WE HAVE TO HAVE PLUS TWO TO END UP WITH A NEUTRAL CHARGE AND THERE S ONLY ONE IRON ATOM THERE TO CONTRIBUTE THAT TWO, SO THEREFORE THIS IS IRON TWO SULFITE. SO THE NAMING OVERALL IS EXACTLY THE SAME OTHER THAN THE FACT THAT WE HAVE TO IDENTIFY THE CHARGE ON THE METAL. BUT THE SAME APPLIES AS FAR AS THE THREE RULES THAT WE LOOKED AT. ONE OXYGEN LESS IS THE ITE. WE ADD A HYDROGEN IT BECOMES HYDROGEN X-ATE OR HYDROGEN X-ITE, AND FAMILY SIMILARITY. SO ONE MORE HERE REAL QUICK AND THEN WE WILL CALL THIS TYPE GOOD AND WE LL GO ON TO LOOK AT SOMETHING ELSE. LET S SUPPOSE WE HAD THIS ONE. ALRIGHT WE WANNA NAME THIS COMPOUND. WELL AGAIN WE NAME THE METAL, THAT S COPPER, AND IF WE LOOK ON THERE WE SEE THAT COPPER S IN THAT AREA THAT WE HAVE TO SPECIFY THE CHARGE. SO IT TELLS US WE LL NEED A ROMAN NUMERAL, AND THEN WE SEE TeO 4. WELL GOSH, I LOOK AT THE TABLE, I DON T SEE ANY TeO 4, BUT I GO TO THE PERIODIC TABLE AND I SAY WELL Te IS IN THE SAME FAMILY AS S. AND IF SO 4 IS CALLED SULFATE, THEN TeO 4 IS GOING TO BE CALLED TELLERATE. SO WE HAVE THE ATE ENDING JUST LIKE SULFATE TELLERATE, AND NOW WE HAVE TO DETERMINE THE CHARGE ON THE COPPER. WELL ONCE AGAIN, IF WE LOOK AT THIS WE SEE THAT THIS ION IS A MINUS TWO AND OF COURSE THE CHARGE FOR THE METAL WOULD HAVE TO BE, OR CONTRIBUTE A PLUS TWO. THERE S ONLY ONE OF THOSE AND SO IT WOULD BE CALLED COPPER TWO TELLERATE. SO FAMILY SIMILARITY AND ASSIGNING OXIDATION NUMBER FOR VARIABLE METAL. NOW, WHAT HAPPENS IF WE ADD ENOUGH HYDROGEN TO AN ION, TO AN OXY-ANION TO MAKE A NEUTRAL COMPOUND INSTEAD OF A HYDROGEN ANION? WHEN WE DO THAT WE MAKE WHAT WE CALL THE POLYATOMIC ACIDS. WE VE ALREADY TALKED ABOUT BINARY ACIDS, AND BINARY ACIDS WERE HYDROGEN NON- METAL COMPOUNDS IN WATER, AQUEOUS SOLUTIONS. HYDROCHLORIC ACID HC AQUEOUS. THE POLYATOMIC ACIDS NOW ARE MADE WHEN WE ADD SUFFICIENT NUMBER OF HYDROGENS TO THE ANION TO MAKE A NEUTRAL MOLECULE. SO IF THE ANION HAS A MINUS ONE CHARGE IT

8 CHM 105 & 106 MO1 UNIT FOUR, LECTURE SIX 8 MEANS WE HAVE TO ADD ONE HYDROGEN. IF THE ANION HAS A MINUS TWO CHARGE WE HAVE TO HAVE TWO HYDROGENS. IF THE ION HAS A MINUS THREE WE WOULD HAVE TO HAVE THREE HYDROGENS TO MAKE THEN THE NEUTRAL COMPOUND, AND THE HYDROGEN THIS IS AN EXAMPLE THEN OF A HYDROGEN POLYATOMIC ANION WE SOMETIMES CALLED THEM OXY- ANIONS. THAT S A TERM THAT YOU MIGHT RN ACROSS. ALL THAT MEANS IS THAT IT S A NEGATIVE ION WHICH HAS AN OXYGEN IN IT. WELL LOOK AT ALL THE CHEMICAL FORMULAS IN THE TABLE. EVERY ONE OF THEM HAS OXYGEN IN IT. ACETATE, CHROMATE, PHOSPHATE, NITRATE, NITRITE, SULFITE THEY RE ALL OXY-ANIONS. THEY RE ALL ANIONS THAT CONTAIN AT LEAST ONE OXYGEN. ALRIGHT, SO IF WE MAKE A HYDROGEN OXY-ANION COMPOUND NOW, NOT ANOTHER ION, THEY RE ALWAYS NAMED AS ACIDS. PERIOD. THEY RE ALWAYS NAMED AS ACIDS, AND THE NAMING IS PRETTY STRAIGHT-FORWARD. WE START WITH THIS FIRST ONE, WE HAVE THE ACETATE ION. THAT S ITS CHEMICAL FORMULA. IF WE ADD A HYDROGEN NOW, ONE HYDROGEN BECAUSE IT WAS A PLUS ONE CHARGE, THIS IS OUR NEW FORMULA. THAT S A POLYATOMIC ACID AND IT IS CALLED A CETIC ACID. THE ACID ENDS IN IC IF THE ION ENDS IN ATE. THAT S THE SAME FOR ALL OF THEM. IF I HAVE SULFATE IT S SULFURIC ACID. THESE ARE ALWAYS GOING TO BE NAMED AS ACIDS. IN THE BINARY CASE WE NAMED IT BOTH WAYS. WE TALKED ABOUT HYDROGEN CHLORIDE AS A COMPOUND, BUT IF WE DISSOLVED IT IN WATER WE CALLED IT HYDROCHLORIC ACID. IN THE CASE OF THE HYDROGEN POLYATOMIC IONS THEY ARE ALWAYS NAMED AS THE ACIDS SO WE DON T NEED TO WORRY ABOUT ANY OTHER POSSIBILITY. SO WE SEE HERE, NITRATE ION, NO 3. PUT A HYDROGEN ON TO MAKE THE NEUTRAL COMPOUND. WHAT DO WE CALL IT? NITRIC ACID, AFTER THE NITRATE. NOW ONE THING I MIGHT MENTION IS THAT NOTICE WE DON T SAY ANYTHING ABOUT HYDROGEN. IN THE BINARY ACIDS WE SAID HYDROCHLORIC ACID. SO WE PUT THE NAME HYDROGEN IN THE BINARY ACIDS. SO IF YOU SEE THE NAME OF AN ACID AND IT DOESN T SAY HYDRO IN THE BEGINNING THAT ALREADY TELLS YOU THAT WE RE TALKING ABUT A POLYATOMIC ACID. ALL BINARY ACIDS START WITH HYDRO. HYDROFLUORIC, HYDROBROMIC, HYDROSULFURIC, HYDROSELENIC, ALL START WITH THAT TERM HYDRO, BUT THE REST OF THESE ACIDS DON T SAY ANYTHING ABOUT HYDROGEN. IT S JUST THE NAME OF THE ION WITH THE ENDING

9 CHM 105 & 106 MO1 UNIT FOUR, LECTURE SIX 9 CHANGED FROM ATE TO IC AND NAMED ACID. NITRIC ACID. SO THE NEXT ONE WE HAVE HERE OF COURSE WE SEE SULFATE. NOW AND OF COURSE THAT S SO 2-4. WE HAVE TO PUT IN TWO HYDROGENS THIS TIME TO GET THE NEUTRAL MOLECULE AND WE RE GOING TO NAME IT SULFURIC ACID. ATE ENDING ION, IC ENDING ACID. PHOSPHATE ION IS PO 4 WITH A THREE MINUS. WE RE GONNA HAVE TO HAVE THREE HYDROGENS TO GET THE NEUTRAL MOLECULE. WE CALL IT PHOSPHORIC. AGAIN WE REPLACE THE ATE WITH THE IC. NOW WHAT ABOUT THE IONS THAT END IN ITE? WE JUST TALKED ABOUT THE RULE THAT WE COULD USE. WELL, IF THE ENDING OF THE ANION IS ITE THE ENDING OF THE ACID IS O-U-S. ATE IC, ITE-OUS. THAT S THE ONLY THINGS WE HAVE TO REMEMBER AS FAR NAMING THE ACIDS. IF THE ANION THAT WE STARTED WITH ENDS IN ATE THE ACID ENDS IN IC. IF THE ANION THAT WE RE STARTING WITH ENDS IN ITE, THE ACID NAME WILL END IN OUS. SO WE SEE THAT SULFITE ION. IT S STILL A TWO MINUS, SO WE PUT TWO HYDROGENS IN TO MAKE THE NEUTRAL MOLECULE. IT S CALLED THEN SULFUROUS ACID. OKAY, OR WE GO DOWN TO THE NEXT ONE, WE HAVE THE NITRITE ION. WE ADD THE ONE HYDROGEN BECAUSE IT S A MINUS ONE, AND THE ITE BECOMES OUS, AND IT S CALLED NITROUS ACID. OKAY, ALRIGHT, KEEPING THOSE RULES IN MIND THEN LET S DO A COUPLE OF EXAMPLES OF NAMES, SOME ACIDS AND WRITING SOME CHEMICAL FORMULAS FOR ACIDS. SO THE FIRST ONES HERE WE HAVE WE RE GOING TO NAME. ALRIGHT, THE ONLY THING I NEED OT LOOK AT IS WHAT IS THE ANION? PO 4. PO 4 IS THE PHOSPHATE ION. SO IF I M STARTING WITH A PHOSPHATE, I THINK I HAVE SOMETHING WRONG OUR OH, ph, THERE WE GO. PHOSPHATE ION WE RE GOING TO HAVE THEN PHOSPHORIC, AND WE HAVE THEN ENDING, PHOSPHORIC ACID. NO 2. THAT S THE NITRITE ION. AND IF IT S THE NITRITE ION IT WOULD BE CALLED NITROUS ACID. FIRST ONE SHOULD BE PHOSPHORIC ACID, I DIDN T WRITE IN THE ACID THERE. OUS ITE. ClO 3. WE LOOKED IN THE ABLE. WE SEE THAT ClO 3 IS THE CHLORATE ION, AND SO THIS WOULD BE CALLED CHLORIC, IC BECAUSE OF ATE, CHLORIC ACID. AND FINALLY H 2 CrO 4, WE LOOK FOR CrO 4 AND WE FIND IT IS CALLED THE CHROMATE ION. AND SO THE ACID IS GOING TO BE CALLED CHROMIC, CHROMIC ACID. SO IT S PRETTY STRAIGHTFORWARD IN NAMING THE ACIDS. ALL WE HAVE TO DO IS LOOK AT THE ANION, THE POLYATOMIC ANION. LET S REVERSE THE PROCESS. WE LL START WITH THE NAME AND WRITE THE CHEMICAL

10 CHM 105 & 106 MO1 UNIT FOUR, LECTURE SIX 10 FORMULA THIS TIME. SO WE HAVE SULFUROUS ACID. NOW AS SOON AS I SEE THAT THAT TELLS ME THAT I M WANTING THE SULFITE ION. AND IF I LOOK IN THE TABLE I DON T FIND SULFITE, I FIND THE SULFATE, SO 4. SO SULFITE IS SO 3. AND THE SULFITE HAS A CHARGE OF 2 MINUS, SO THEREFORE I WILL HAVE TO PUT TWO HYDROGENS TO MAKE THE NEUTRAL MOLECULE. EACH HYDROGEN IS A PLUS. SULFITE IS A NEGATIVE 2. WE PUT TWO HYDROGENS TO MAKE A NEUTRAL MOLECULE. IF THE ION ENDS IN ITE THE ACID ENDS IN OUS. THE NEXT ONE, ACETIC ACID. THAT MEANS THAT WE RE LOOKING FOR THE ACETATE ION BECAUSE OF THE IC ENDING ON THE ACID, AND THE CHEMICAL FORMULA FOR THE ACETATE ION IS C 2 H 3 O 2, HAS A MINUS ONE CHARGE. SO WE ONLY NEED TO ADD ONE HYDROGEN. WELL WE COULD PUT IT HERE, SOMETIMES IT S SHOWN WRITTEN OVER ON THE OTHER END, DOESN T MAKE ANY DIFFERENCE. THAT S ACETIC ACID. MAJOR COMPONENT AS WE VE MENTIONED BEFORE, OF VINEGAR. NITRIC ACID, IC MEANS THAT WE HAVE THE NITRATE ION, AND WE LOOKED IN THE TABLE. NITRATE IS NO 3 AND IT HAS A ONE MINUS CHARGE. SO IT MEANS THAT WE NEED ONE HYDROGEN. NITRIC ACID. BROMIC ACID. IC, THAT MEANS THAT WHATEVER IT IS WE NEED THE BROMATE ION. WE LOOK IN THE TABLE WE DON T FIND BROMATE, BUT AGAIN WE FIND CHLORATE GIVEN, AND IF WE HAVE CHLORATE, THEN USING THE FAMILY RELATIONSHIP WE CAN DO THE BROMATE. WELL CHLORATE IS ClO 3 MINUS, SO THE BROMATE THEREF ORE IS BrO 3 WITH A MINUS ONE CHARGE, MEANS WE NEED ONLY ONE HYDROGEN. NOW NOTICE IN WRITING ANY OF THESE I DID NOT USE THE PARENTHESES AQUEOUS. HYDROGEN POLYATOMIC COMPOUNDS ARE ALWAYS NAMED AS ACIDS. SO WE JUST NAME IT, WE DON T NEED TO SHOW AQUEOUS IN THE CHEMICAL FORMULA. THAT S THE ONE DIFFERENCE BETWEEN POLYATOMIC ACIDS AND BINARY ACIDS. IF YOU RE TALKING ABOUT BINARY ACID IT HAS TO SHOW THAT AQUEOUS, OTHERWISE IT S JUST NAMED AS A NORMAL COMPOUND, MANY OF WHICH ARE GASSES IN THE HYDROGEN COMPOUNDS. HYDROGEN SULFIDE, HYDROGEN IODIDE, ALL GASEOUS SPECIES. OKAY, ALRIGHT, THE ACIDS. ONE LAST GROUP OF COMPOUNDS THAT WE RE GOING TO LOOK AT HERE QUICKLY AND THAT DEALS WITH THE ONE CATION, THE ONE POLYATOMIC POSITIVE CHARGED ION THAT WE WORK WITH, AND THE ONE ION THAT WE WORK WITH THAT HAS A PLUS CHARGE IS NH 4 WITH A PLUS, AND THIS IS CALLED AMMONIUM ION. THAT IS THE ONLY

11 CHM 105 & 106 MO1 UNIT FOUR, LECTURE SIX 11 POSITIVE ION, POSITIVE POLYATOMIC EXCUSE ME, POSITIVE POLYATOMIC ION THAT WE WORK WITH AMMONIUM. NOW AMMONIUM ALWAYS HAS A PLUS ONE CHARGE. AS A MATTER OF FACT, WE NAME THE AMMONIUM COMPOUNDS JUST LIKE WE NAME THE FIRST COLUMN COMPOUNDS. WE NAME IT SO TAKE AMMONIUM JUST LIKE IT WAS A SODIUM AND WE GO THROUGH THE SAME NAMING SYSTEM AS WE DO FOR THOSE METALS THAT HAVE ONLY THE ONE POSITIVE CHARGE. OKAY, SO IT S PRETTY STRAIGHTFORWARD AS FAR AS NAMING AND WRITING FORMULAS BECAUSE ALL WE HAVE TO REMEMBER IS HOW WOULD WE HAVE DONE IT IF IT WAS A SODIUM INSTEAD OF THE NH 4? SO LET S TAKE A LOOK AT WRITING SOME CHEMICAL FORMULAS HERE. THE FIRST ONE, FIRST THING WE RECOGNIZE IS THE NH 4. SO WE SAY AMMONIUM, AND THEN WE HAVE TO NAME THE POLYATOMIC ANION THAT IT S ATTACHED TO. AND IF I LOOK IN THE TABLE I DON T FIND SO 3, BUT ONCE AGAIN WE FIND SO 4, WHICH IS SULFATE, SO SO 3 IS SULFITE. AND THAT S IT. WE DON T HAVE TO SAY ANYTHING ABOUT THIS LITTLE SUBSCRIPT, BECAUSE AMMONIUM, JUST LIKE SODIUM, ALWAYS IS A PLUS ONE. THE ONLY WAY AMMONIUM COULD COMBINE WITH SULFITE IS IN A TWO TO ONE RATIO. SO WE DON T NEED ANY PREFIXES, WE DON T NEED ANY ROMAN NUMERALS. WE JUST NEED THE NAME OF THE CATION FOLLOWED BY THE NAME OF THE ANION. NOTICE THIS ONE HERE, OKAY WE NAME AMMONIUM, WHOOPS I FORGOT AN M IN THERE, AMMONIUM, AND THEN IODINE, BUT WE CHANGE THE ENDING TO IDE. NOW NOTICE THAT WE NAMED THIS JUST LIKE WE WOULD VE IF THIS HAD BEEN Na. IF THAT HAD BEEN Na AS A BINARY COMPOUND WE WOULD HAVE CALLED IT WHAT? SODIUM IODIDE. AND WE NAME AMMONIUM COMPOUNDS JUST THE SAME WAY AMMONIUM IODIDE. ANOTHER EXAMPLE, AS I MENTIONED, ALL BINARY COMPOUNDS END IN IDE, BUT ALL COMPOUNDS ENDING IN IDE ARE NOT NECESSARILY BINARY COMPOUNDS. SO YOU HAVE TO BE CAREFUL. HYDROXIDES, THOSE COMPOUNDS END IN IDE, THEY RE NOT BINARY. AMMONIUM, IDE COMPOUNDS AREN T BINARY. SO YOU KNOW IF YOU RE NAMING A BINARY COMPOUND IT S GOING TO END IN IDE, BUT IF YOU LOOK AT THE CHEMICAL FORMULA AND SEE IDE IT DOES NOT NECESSARILY MEAN IT S BINARY. THE NEXT ONE, AMMONIUM, AND THEN WE NEED TO NAME THE BROMATE, UH, YEAH, WE NEED TO NAME THE BROMATE. WE NEED TO NAME THE BrO 3. I JUST NAMED THE BROMATE, AND THAT S BROMATE, AND AGAIN WE

12 CHM 105 & 106 MO1 UNIT FOUR, LECTURE SIX 12 WOULD USE THE FAMILY RULE TO DETERMINE THAT BrO 3 IS IN FACT BROMATE. NOW, GOING THE OTHER WAY, WHEN WE RE GIVEN THE CHEMICAL NAME AND ASKED TO WRITE THE CHEMICAL FORMULA, SO ALL OF THESE ARE GOING TO CONTAIN I M JUST GOING TO WRITE THIS DOWN ONCE, ALL OF THEM ARE GOING TO CONTAIN NH + 4. NITRATE, NOW LOOK ON THE TABLE, NO 3 WITH A MINUS ONE CHARGE. WE ALREADY SEE THAT ONE S A PLUS ONE, ONE S A MINUS ONE, SO THEREFORE WE DO NOT NEED ANY SUBSCRIPTS, WE DON T NEED ANY ADDITIONAL ONE TO ONE COMBINATION, AMMONIUM NITRATE. AMMONIUM NITRATE OF COURSE IS A COMMERCIAL FERTILIZER AND AS YOU MAY RECALL FROM PAST HISTORY, AMMONIUM NITRATE WAS THE MAJOR COMPONENT ALONG WITH KEROSENE TO CONSTRUCT THE BOMB THAT DESTROYED THE FEDERAL BUILDING IN OKLAHOMA CITY. SO THIS DOES HAVE AN EXPLOSIVE NATURE TO IT, BUT IT S FAIRLY STABLE. WE USE IT AS FERTILIZER AND IT S RELATIVELY COMFORTABLE AS A FERTILIZER WE DON T NEED TO WORRY ABOUT IT, BUT IT CAN BE MISUSED AS WELL BY COMBINING WITH SOMETHING LIKE A FUEL OIL OR SOMETHING LIKE THAT. ACTUALLY IT CAN BE MADE INTO AN EXPLOSIVE. UH- MANY OF THE EXPLOSIVES THAT WE HAVE CONTAIN NITRATES IN THEM. NITROGEN/OXYGEN COMPOUNDS. AMMONIUM CHLORATE, ClO - 3 IS THE CHLORATE. AGAIN WE SEE THAT EACH HAVE THE SAME CHARGE SO WE WOULD MERELY WRITE AMMONIUM ClO 3. WE DON T NEED ANY PARENTHESES OR SUBSCRIPTS. AMMONIUM SULFITE. SULFATE IS SO 4, SULFITE IS SO 3 AND IT HAS A TWO MINUS CHARGE. WELL THIS TIME WE SEE THAT AMMONIUM OF COURSE WITH A PLUS ONE AND SULFITE WITH A TWO MINUS WE RE GOING TO HAVE TO THEN HAVE TWO AMMONIUMS ATTACHED. SO WE LL HAVE TO WRITE NH 4 AND THEN A SET OF PARENTHESES WITH A TWO AND THEN SO 3. AMMONIUM SULFITE. ALRIGHT, THE LAST ONE OF THAT GROUP, SULFIDE, IDE, MEA NS THAT WE RE JUST TALKING ABOUT THE NON-METAL BY ITSELF, NOT A POLYATOMIC ANION, AND IF WE LOOK AT ITS LOCATION IN THE CHART, SULFUR S IN THAT SIXTH COLUMN, LIKE OXYGEN. TWO ELECTRONS AWAY FROM ARGON, SO WE WOULD EXPECT THERE WOULD BE A TWO MINUS ION. AND AMMONIUM AGAIN OF COURSE IS A PLUS ONE AND SULFIDE IS A TWO MINUS AND SO THEREFORE WE WOULD HAVE TO HAVE TWO AMMONIUMS. SO WE WOULD HAVE NH 4 2S FOR THE FORMULA FOR AMMONIUM SULFIDE. NOW IN NATURE THINGS AREN T ALWAYS

13 CHM 105 & 106 MO1 UNIT FOUR, LECTURE SIX 13 THIS CLEAN AND NEAT AS JUST BEING SINGLE THINGS HOOKED TOGETHER. MANY TIMES IN ORES THINGS LIKE THAT IN NATURE WE HAVE MIXTURES OF COMPOUNDS, AND IF WE ENCOUNTER THOSE THE NAMING PROCESS WE CAN USE IS PRETTY STRAIGHTFORWARD. AS A MIXTURE WE NAME THE METALS, WHICHEVER ONES ARE IN THERE, AND THEN WE NAME THE POLYATOMIC ANIONS. SO LOOKING AT THIS COMPOUND HERE THIS WOULD BE CALLED CALCIUM, POTASSIUM, AND THEN NAMING THE PO 4, PHOSPHATE. CALCIUM POTASSIUM PHOSPHATE. THAT WOULD BE THE NAMING SYSTEM THAT WE WOULD USE. THEN GOING DOWN HERE WOULD BE LITHIUM, AND THEN Al ALUMINUM, SULFATE. NOW IF WE WERE SHOWN THE NAME AND ASKED TO WRITE THE CHEMICAL FORMULA WE MIGHT SAY GOSH HOW ARE WE GONNA DO THAT? WELL IF LOOK LITHIUM HAS A POSITIVE ONE CHARGE. ALUMINUM HAS A THREE PLUS CHARGE. WE RE GOING TO HOOK AN SO 4 ON HERE, AND SO 4 HAS A TWO MINUS CHARGE. WELL WE CAN SEE THAT THE TWO METALS COMBINED GIVE US A TOTAL CHARGE OF PLUS FOUR, WHEREAS THE ANION HAS ONLY A CHARGE OF TWO MINUS. SO TO GET THE CHARGES TO EQUAL WE WOULD HAVE TO HAVE THEN TWO OF THE SULFATES, AND THAT S WHY THE CHEMICAL FORMULA APPEARS THE WAY THAT IT DOES. NOW IN NATURE SEVERAL OF THE COMPOUNDS, OR SEVERAL OF THE ORES CONTAINING ALUMINUM OXIDE, ALUMINUM OXIDE IS A RATHER STANDARD COMPOUND IN NATURE, SILICON DIOXIDE, WHICH IS SAND, ALUMINUM OXIDE WHICH IS THE OTHER MAJOR COMPONENT MAKING UP SOILS AND ORES, AND SOMETIMES IF WE HAVE SMALL AMOUNTS OF IMPURITIES TO ALUMINUM OXIDE WE GET SOME VERY NICE LOOKING COLORED COMPOUNDS OR ORES, AND IN THIS PARTICULAR CASE THE COLOR, WELL LET ME MOVE THIS ONE OVER MAYBE WE CAN SEE IT A LITTLE BIT BETTER. ALUMINUM OXIDE WITH JUST A SMALL AMOUNT OF IRON AND TITANIUM METALS ATOMS IN THERE THEN MAKE UP THIS NICE BLUE COLOR THAT IS KNOWN AS SAPPHIRE. SO VERY SMALL AMOUNT OF THE TRACE ELEMENTS, IN THIS CASE IRON AND TITANIUM CONVERTS ALUMINUM OXIDE WHICH ITSELF IS COLORLESS INTO THEN THIS BLUE COLOR WHICH IS CALLED SAPPHIRE. IF WE HAVE A CHROMIUM IMPURITY, ALUMINUM OXIDE WITH A LITTLE BIT OF CHROMIUM IN IT WE GET THIS BEAUTIFUL RED COLOR AND THAT S THE RUBY, AND OF COURSE THE REASON THAT THESE HAVE SUCH HIGH VALUE IS BECAUSE IN NATURE THIS ENTRAPMENT OF THESE IMPURITIES

14 CHM 105 & 106 MO1 UNIT FOUR, LECTURE SIX 14 OCCUR ONLY ON AN INFREQUENT BASIS AND SO WE DON T FIND TONS OF ALUMINUM OXIDE WITH CHROMIUM IN IT, ONLY SMALL AMOUNTS AND IN RATHER SMALL AREAS AND SO THAT S WHY THEY RE SO VALUABLE. AND OF COURSE THEY RE VERY HARD, AND SO JEWELRY STANDPOINT THEY HAVE THE COLOR, THE INTERACTION WITH LIGHT AND CRYSTALLINE. ALL OF THESE THEN LEAD TO THEIR USEFULNESS AS JEWELRY. AND ONE OTHER ONE HERE, A REAL BIG MIXTURE, THIS ONE IS BERYLLIUM ALUMINUM SILICATE, SILICON DIOXIDE OR SILICON TRIOXIDE IS WHAT GLASS OR SAND IS AND WITH BERYLLIUM AND ALUMINUM IN THERE WE GET THIS BEAUTIFUL GREEN COLOR, INTENSE GREEN CALLED EMERALD, AND THAT S WHAT AN EMERALD IS THEN, IS A BASICALLY AN ALUMINUM SILICATE WITH SOME TRACE BERYLLIUM IN IT TO GIVE US THAT PARTICULAR JEWEL. OKAY AND ONE LAST THING HERE REAL QUICK, OUR SOURCE OF MOST OF OUR MERCURY IN NATURE COMES FROM THIS REDDISH COLORED MATERIAL CALLED MERCURY II SULFIDE. CHEMICAL FORMULA HgS, AND WHERE IT APPEARS IT S IN A SOIL ROCK ORE AREAS, AND IT HAS THIS VERY REDDISH COLOR, AND IF WE HEAT IT UP TO A HIGH ENOUGH TEMPERATURE THE MERCURY SULFITE DECOMPOSES AND WE GET MERCURY COMING OFF AS A VAPOR AND WE COLLECT IT THEN BECOMES A LIQUID AND THAT S WHERE WE GET OUR SUPPLY OF MERCURY METAL.