Chemistry SM-1131 Week 7 Lesson 1
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Transcript of Chemistry SM-1131 Week 7 Lesson 1
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Chemistry SM-1131Week 7 Lesson 1
Dr. Jesse ReichAssistant Professor of Chemistry
Massachusetts Maritime AcademyFall 2008
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Class Today• Polyatomic anions, Molecular Compounds, Acid
Names, Formula Mass • Grams, atoms, mols, avogadro’s number• Take home quiz for Friday
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Review• Polyatomic Ions• Ionic Compounds are between metals and
non-metals, AND metals and polyatomic atoms
• Poly=Many• Atomic= Atoms• Polyatomic= many atoms
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Polyatomic Anions• Compounds still work basically the same way• 1- Symbols (keep the parenthesis)• 2- Charges• 3- Switcheroo• 4- Reduce
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Example• Sodium and Carbonate combine to make a
compound. What’s the formula and charge?• Na & (CO3)
• Na+1 and CO3-2
• Na2(CO3)• Metal First polyatomic ion second• Sodium Carbonate
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Example 2• Magnesium and Phosphate come together to
form a compound. Formula and charge?• Mg & (PO4)
• Mg+2 & (PO4)-3
• Mg3(PO4)2
• Metal first polyatomic ion second• Magnesium Phosphate
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Example 2 cont.• Mg3(PO4)2• There are 3 Magnesium atoms• There are 2 PO4 groups• Each PO4 group has 1 P and 4 O• So, we have to multiply:• 2x 1P = 2P• 2x 4O = 8O• Total: Mg3P2O8
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Example 3• Iron (III) and Nitrate form a compound.
What’s the formula and name?• Fe(III) & (NO3)
• Fe(III)+3 & (NO3)-1
• Fe(III)1(NO3)3
• Iron (III) nitrate• Formula = Fe(III)1N3O9
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Example 4• Ammonium and Permanganate form a compound.
Formula and Name?• (NH4) & (MnO4)
• (NH4)+1 & (MnO4)-1
• (NH4)1(MnO4)1
• Ammonium Permanganate• This guy is a rarity because the non-metal thing is the
cation and the metal thing is the anion. Polyatomics can act a little differerntly than metals or non-metals that are just by themselves.
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Polyatomics to Memorize
• Table 5.6 page 138• Make note cards. They are all fair game.
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Molecular Compounds• Ionic compounds are between metals and
non-metals (or polyatomic ions)• Molecular compounds are between 2 or
more non-metals
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Molecular Compounds• Two different naming systems. DON’T
CONFUSE THEM!• This system is just for molecular compounds.• Molecular compounds have 2 or more non-
metals in them
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Molecular Nomenclature
• The naming systems for the simple ones works like this:
• 1-Prefix • 2-First element (somewhat alphabetical)• 3-Prefix• 4-Second element• 5-change the ending of the second element to
-ide.
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What are the prefixes• MEMORIZE THESE!• Mono-1• Di-2• Tri-3• Tetra-4• Penta-5• Hexa-6• Hepta-7• Octa-8
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Example
• Here’s a formula: N2O4. What’s the name?• Di• Nitrogen• Tetra• Oxygen• Oxide• Dinitrogen tetraoxide
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Example 2• SF6• Mono (If mono is the very first one you don’t
have to use it).• Sulfur• Hexa• Fluorine• Fluoride• Sulfur Hexafluoride
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Example 3
• CO2
• Mono (drop it)• Carbon• Di• Oxygen• Oxide• Carbon Dioxide
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Acids• Acids are things that create H+ ions when
dissolved in water. They are typically bitter and sour tasting. Most acids can dissolve metals.
• They are combinations of H+ atoms with anions
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Acid Types• Binary Acids• Oxyacids
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Binary Acid Names• Binary Acids are a combination of 2 things.
Hydrogen and one other non-metal• Naming them is simple• 1-Hydro• 2-Base name of non-metal• 3-change the ending of the non-metal to –ic• 4-Add the word acid at the end
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Binary Acid names• HBr• 1-Hydro• 2-Brom• 3-ic• 4-Acid• Name= Hydrobromic acid
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Binary Acid Names• HCl• 1-Hydro• 2-Chlor• 3-ic• 4- Acid• Name= Hydrochloric Acid
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Oxyacid Names• Oxy Acids are built around compounds that
have oxygen containing polyatomic anions in them.
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What polyatomic anions make sense?
• Phosphate (PO4)
• Phosphite (PO3)
• Chlorate (ClO3)
• Chlorite (ClO2)
• Nitrate (NO3)
• Sulfate (SO4)
• Sulfite (SO3)
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Oxyacid naming with-ate
• 1-Name of the polyatomic acid• 2-change the ending to –ic (sometimes needs
a fudge factor)• 3-add the word acid
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Oxyacid Naming• Phosphate makes an acid. What is the name and
formula?• 1-Phosphate• 2-turns into Phosphoric• 3- add acid• Name= Phosphoric Acid• 1-H (PO4)
• 2-H+1(PO4)-3
• 3-H3(PO4)1
• Can’t reduce
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Naming Oxyacids with -ite polyatomic anions• 1-Write the anion name• 2-Change the ending to –ous (might need a
fudge factor)• 3- add the word acid
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Oxyacid Naming with -ite polyatomic anions
• The polyatomic anion sulfite forms an oxyacid. What is the name and formula?
• 1-Sulfite• 2- Change to Sulferous• 3- add Acid• Name= Sulferous Acid• H (SO3)• H+1 (SO3)-2• H2(SO3)1
• Can’t reduce
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Molecular Mass• To figure out molecular mass you have to
know the atomic mass.• Let’s start easily• Ne- it exists by itself and doesn’t form
molecules. It’s mass is just the atomic mass of Ne, which is 20.18
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Simple Molecule Mass
• The mass of N2 is going to be twice the mass of 1 atom of N
• So, if N has an atomic mass of 14.01, then N2 must have a mass of 2x14.01 or 28.02
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Molecular Mass• Ozone has the formula O3, what is it’s
molecular mass• 1 Oxygen has a mass of 16.00• 3x(16.00) has a mass of 48.00 amu
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More Complex Masses
• Water has the formula H2O• The molecular mass is going to be from 2H
atoms and 1 O atom, so• 2x(1.0079) + 1x(16.00)= 18.0158amu
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Sugar
• C6H12O6
• 6(12.01) + 12(1.0079) + 6(16.00)= ???
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New Material• Moles, Atoms, Molecules, grams• IT’S MATH HEAVY TODAY! PAY ATTENTION
YOU SCURVEY DOGS!
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Moles• Dozen: 12 somethings• Baker’s Dozen: 13 Somethings• A Score: 20 Somethings • Avogadro’s number: 1 mol= 6.022e23
somethings
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See how it works• A dozen atoms = 12 atoms• A baker’s dozen atoms = 13 atoms• A score of atoms = 20 atoms• A mole of atoms = 6.022e23 atoms
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Moles• 1 mole of atoms = 6.022e23 atoms• 2 moles of atoms= 2(6.022e23)atoms=
1.2044e24 atoms• 3 moles of atoms = 3(6.022e23)atoms=
1.8066e24
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Moles• 1 mole of kittens = 6.022e23 kittens• 2 moles of kittens= 2(6.022e23)kittens=
1.2044e24 kittens• 3 moles of kittens = 3(6.022e23)kittens=
1.8066e24
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Moles• It just means a big number.• 602,200,000,000,000,000,000,000,000• But we do this because it converts amu to
grams
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Why a 6.022e23• 1 amu = 1.66e-24 grams• So, 1.66e-24gx6.022e23= 0.99652g which is very
similar to 1g.• The point is that if you multiply the mass of
something in amu you can convert amu into a mass in grams
• We don’t weigh anything in amu, but we do in grams so this is useful.
• So, if we multiply the atomic mass of something by 1 mol it turns from amu into grams.
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If you have 1 mole of N2 how much would it weigh?• Atomic Mass of N= 14.01 amu• Molecular Mass of N2= 28.02 amu• 6.022e23 atoms of N2 x 28.02 amu x 1.66e-24g =
1 atom 1 amu
Which equals 28.02g. So, 1 mol x molecular mass = # of grams
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What do we do with this?
• Chemists generally convert moles into atoms.• Atoms into Moles• Moles into grams• Grams into Moles
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Moles into atoms• 1 mole has 6.022e23 atoms in it• 5 moles of Ne x 6.022e23 atoms = 3.011e24 atoms 1 mole
• 24.00 moles of He 6.022e23 atoms = 1.445e25 atoms
1 mole
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Atoms into Moles• You have 18.066 e23 atoms of Cu many many
moles of Cu do you have?18.066e23 atoms x 1 mol = 3.0000 mol 6.022e23 atoms
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So• Atoms x 1 mole = moles 6.022e23 atoms• Moles x 6.022e23 atoms = atoms 1 mole
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Moles to grams• We also convert moles into grams• You can’t weigh a mole, you weigh a gram• Moles x molecular mass in grams = grams 1 mole
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Moles to Grams Example 1
• 5 moles of N2 is how many grams?Copy the given5.000 moles x grams = grams 1 molesHow many grams in 1 mole? Use the atomic
mass. N= 14.01amu, so N2= 28.02amu5.000 moles x 28.02 g = 140.1 g 1 mole
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Moles to Grams Example 2
• 8 moles of O3 is how many grams?Copy the given8.000 moles x atomic mass in grams = grams 1 molesHow many grams in 1 mole? Use the atomic
mass. O= 16.00 amu, so O3= 48.00amu8.000 moles x 48.00 g = 384.0 g 1 mole
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Moles to Grams Example 3
• 10 moles of H2O is how many grams?Copy the given10.0 moles H2O x molecular mass in grams = grams 1 molesHow many grams in 1 mole? Use the atomic
mass. O= 16.00 amu, H = 1.0079 so H2O= 18.0158amu10.0 moles H2O x 18.00158 g = 180.0158 g = 180g 1 mole
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Grams to Moles• Grams -> Moles• Xgrams x moles = moles Atomic mass
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Grams to Moles example 1
• 2000 g of He into moles• 2000 g x 1 mole He = X moles Atomic Mass• Molecular mass of He 4.00• 2000 g x 1 mole H2O = 500 moles 4g
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Grams to Moles example 2
• 450 g of O3 into moles
• 450g x 1 mole O3 = X moles Molecular Mass• Molecular mass of O3 3(16)= 48 amu• 450g x 1 mole O3 = 9.375 moles= 9.4 moles 48g
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Grams to Moles example 3
• 270 g of H2O into moles
• 270g x 1 mole H2O = 15 moles Molecular Mass• Molecular mass of H2O 16+1+1= 18
• 270g x 1 mole H2O = 15 moles 18g
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If there is time• Convert the following• 15 moles N2 into atoms
• 15 moles of N2 into grams
• 28g of N2 in moles
• 28g of N2 into atoms (2 conversion factors)