Chapter 7- Chemical Formulas and Chemical Compounds
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Transcript of Chapter 7- Chemical Formulas and Chemical Compounds
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Chapter 7- Chemical Formulas and Chemical
Compounds
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Ban Dihydrogen Monoxide! Colorless, odorless, tasteless Kills uncounted thousands of people every year. Most deaths caused by accidental inhalation Prolonged exposure to its solid form causes severe
tissue damage. Symptoms of ingestion can include
excessive sweating and urination, a bloated feeling, nausea, vomiting body electrolyte imbalance.
For those who have become dependent, withdrawal means certain death.
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Ban Dihydrogen Monoxide! Also known as hydroxl acid Major component of acid rain Contributes to the "greenhouse effect." May cause severe burns. Contributes to the erosion of our natural landscape. Accelerates corrosion and rusting of many metals. May cause electrical failures and decreased
effectiveness of automobile brakes. Been found in excised tumors of terminal cancer
patients. Is now an ingredient in most foods and beverages
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Ban Dihydrogen Monoxide!Based on the evidence presented in the
previous two slides, do you support the banning of dihydrogen monoxide?
Write at least two sentences stating your reasoning.
Please sign the petition!
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What is Dihydrogen Monoxide?
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Chemical Formulas Indicate the relative number of atoms or
ions of each kind in a chemical compound
C8H18
MgCl2
Ca(OH)2
8 C atoms 18 H atoms
2 OH- ions
2 Cl- ions
1 Ca2+ ion
1 Mg2+ ion
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Monatomic Ions Ions formed from a single atomUsually have noble gas configurationsThat’s how we determine its chargeExample:
Li: 1s22s1
Li+: 1s2 or [He]Table on p.221 on monatomic ions
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Naming Monatomic CationsUse the element’s name!Yes, it’s that simple!Example:
Cs+ = cesiumAl3+ = aluminum
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Naming Monatomic AnionsDrop the ending of the element’s nameAdd the ending –ideExamples:
Cl- = chlorideN3- = nitride
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Naming Monatomic IonsK+
S2-
Rb+
O2-
I-
Ba2+
Cu+
potassiumsulfiderubidiumoxide iodidebariumcopper
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Binary Ionic CompoundsCompounds composed of two ionsTotal numbers of positive charges and
negative charges must be equalExamples:
NaClKBrCaF2
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Writing Binary Ionic CompoundsWrite the symbols for the ions side by
side. Write the cation first.Al3+ O2-
Cross over the charges to use as the subscript for the other ion.
Al3+ O2-
Al2 O3
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Writing Binary Ionic CompoundsCheck the subscripts and divide them to
give the smallest whole number ratio of ions.
Al2O3
Write the formula!Al2O3
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Writing Binary Ionic CompoundsZinc iodideBarium fluorideLithium oxideCalcium oxideMagnesium bromide
ZnI2
BaF2
Li2OCaOMgBr2
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Naming Binary Ionic Compounds
Give name of cation firstThen name the anionAl2O3
Name of cation: aluminumName of anion: oxideName of compound: aluminum oxide
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Naming Binary Ionic Compounds
BaI2
ZnF2
K2OMgOCaBr2
Barium iodideZinc fluoridePotassium oxideMagnesium oxideCalcium bromide
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Cations With Different ChargesSome elements form two or more cations
with different chargesFe2+ and Fe3+
Iron (II) and Iron (III)Naming compounds
FeO and Fe2O3
Iron (II) oxide and Iron (III) oxide
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Name the Following Compounds
CuOCoF3
SnI4
FeS
Copper (II) oxideCobalt (III) fluorideTin (IV) iodide Iron (II) sulfide
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Quiz- Name the Following Compounds
1. K2S2. AgBr3. Na2O4. FeCl25. BaS
6. Lithium fluoride7. Silver iodide8. Iron (III) oxide9. Magnesium iodide10. Gold chloride
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Polyatomic Ions Ions that contain two or more atomsMost are negatively chargedList of polyatomic ions is on handout
**MEMORIZE THEM!!!**Examples:
CN- cyanideHCO3
- hydrogen carbonate (bicarbonate)NH4
+ ammonium
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Polyatomic IonsYou will need to memorize the following:
Ammonium NH4+1
Acetate C2H3O2-1
Hydroxide OH-1
Nitrite NO2-1
Nitrate NO3-1
Bicarbonate HCO3-1
Carbonate CO3-2
Chromate CrO4-2
Sulfate SO4-2
Phosphate PO4-3
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OxyanionsPolyatomic ions that contain oxygenName depends on number of oxygen
atoms
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Oxyanions (cont.) If two oxyanions-
Most oxygens: -ateLeast oxygens: -ite
ExampleNO3
- : nitrateNO2
- : nitrite
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Oxyanions (cont.) If more than two oxyanions
Most oxygens: “Per- …. –ate” “-ate” “-ite” Least oxygens: “Hypo- …. –ite”
Example ClO4
- : perchlorate ClO3
- : chlorate ClO2
- : chlorite ClO- : hypochlorite
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Polyatomic Ion Quiz
Sodium hypochloritePotassium sulfateMagnesium peroxideAmmonium chlorideLithium nitratePotassium phosphate
NaClOK2SO4
MgO2
NH4ClLiNO3
K3PO4
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Polyatomic Ion Quiz1. Bicarbonate2. Acetate3. Bisulfite4. Permanganate5. Nitrite6. Cyanide7. Hydroxide8. Bisulfate9. Nitrate10. What’s your favorite polyatomic ion?
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Binary Molecular CompoundsComposed of molecules (covalently
bonded!)A nonmetal bonded to another nonmetalExamples:
SO3
ICl3CH4
H2O
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Prefixes for Naming Binary Molecular Compounds
1 mono- 2 di- 3 tri- 4 tetra- 5 penta- 6 hexa- 7 hepta- 8 octa- 9 nona- 10 deca
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Naming Binary Molecular Compounds
Which element goes first? Smaller group number If same group- greater period number Use prefix only if there is more than one atom
Second element Prefix indicating number of atoms + root of the name
of the element + -ide General order of elements in binary compounds:
C, P, N, H, S, I, Br, Cl, O, F
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Naming Binary Molecular Compounds
Examples:SO3 – sulfur trioxideBrCl3 – bromine trichloridePBr5 – phosphorus pentabromideN2O5 – dinitrogen pentoxide
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Naming Binary Molecular Compounds
N2OCCl4NOCO2
N2O3
P4O10
Dinitrogen monoxideCarbon tetrachlorideNitrogen monoxideCarbon dioxideDinitrogen trioxideTetraphosphorus decoxide
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Naming Binary Molecular Compounds- More Practice!
Disulfur dioxideSilicon tetrafluorideSulfur monoxidePhosphorus trioxideBoron trifluorideDiphosphorus pentoxide
S2O2 SiF4
SOPO3
BF3
P2O5
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Acids Acid- a type of molecular compound
Two types Binary acids- made up of two elements- hydrogen, and one
of the halogens (F, Cl, Br, I) Oxyacids- contain hydrogen, oxygen, and a third element
Examples Binary acids:
HCl- hydrochloric acid; HF- hydrofluoric acid Oxyacids:
H2SO4: sulfuric acid HNO3: nitric acid
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Formula MassThe sum of the atomic masses of all
atoms represented in its formulaUnits = amu (atomic mass units)Example: What is the formula mass of
water?2 H atoms @ 1.01 amu each = 2.02 amu1 O atom @ 16.00 amu each = 16.00 amuTotal mass of water = 16.00 + 2.02 = 18.02
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Formula MassFind the formula mass of the following:
KClO3
H2SO4
Mg(NO3)2
C12H22O11
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Molar MassThe mass in grams of one mole of a
substance If we have 1 mole of H2O, we have
2 moles of H atoms1 mole of O atoms
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Molar Mass (cont.)How many moles of each atom are in the
following?CaCl2NaOHKMnO4
NH4OHMg(NO3)2
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Molar Mass (cont.)Once we know the number of moles of
each atom, we can calculate the molar mass.
In H2O:2 moles H x 1.01 g H = 2.02 g H
1 mole H
1 mole O x 16.00 g O = 16.00 g O 1 mole O
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Molar Mass (cont.)
Total mass of 1 mole H2O 2.02 g + 16.00 g = 18.02 g/mol
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Molar Mass (cont.)Determine the molar mass of the following:
CaCl2NaOHKMnO4
NH4OHMg(NO3)2
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Molar Mass as a Conversion Factor
Can use molar mass as a conversion factor to determine number of moles
How many moles of H2O are in 34.32 g?
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Molar Mass as a Conversion Factor
How many molecules of NaCl can be found in a sample containing 45.43 g?
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Molar Mass as a Conversion Factor
How many carbon atoms are in a 23.43 g sample of CO2?
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Fun With Conversions! Ibuprofen, C13H18O2, is the active
ingredient in Advil. Find its molar massIf the tablets in the bottle contain a total of 33
g of ibuprofen, how many moles of ibuprofen are in the bottle?
How many molecules of ibuprofen are in the bottle?
What is the total mass in grams of carbon in 33 g of ibuprofen?