G IVE OR RECEIVE Jeralisse Gonzalez Katie Mayers 3 rd block.
Agenda: 3/17 – 3 rd block
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Transcript of Agenda: 3/17 – 3 rd block
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Objective: To interpret (correctly write) formulas and names for compounds – using IUPAC convention
Warm-up: review names & formulasReview: Binary Ionic CompoundsMore Complex Ionic CompoundsWith Polyatomic IonsWith Transition Metals
Covalent Compounds
Agenda: 3/17 – 3rd block
Homework: Re-write in paragraph form – notes pages 1 and 3. Add additional information learned in practice.
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Formula Type of Bond and Compound
Name
MgCl₂SO₂PCl₃AlBr₃K₃NBrO₃H₂O
Warm-up: Review names & formulas
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Inorganic Compound
sIoni
c
M & NM
With Roman
numeral
3 or more
elements
Covalent
(molecules)
NM & NM
Diatomic Molecule
sAcids
Language of chemistry: Standardize system to represent compounds
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Ionic CompoundsMetals lose valence electrons
Non-metals gain valence electrons
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Ionic bonding occurs when a metal loses 1 or more electrons to a non-metal in an effort to attain a stable octet of valence electrons.
Use Electron Dot Diagrams (Lewis diagrams) to show the ionic bonds for one formula unit.
Na Cl = Na⁺¹Cl⁻¹
Ionic Bonding: Transfer of valence electrons
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Cl Ca Cl
= Ca Cl
Electron Dot Diagram (Lewis)
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Some Ionic Compounds are more complex
Include polyatomic ions
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Ionic compounds: Found in minerals and rocks
Barite = BaSO₄Used to make paper & glassSource of barium used For x-rays of the digestivesystem
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Ionic compounds: Found in minerals and rocks
Gypsum = CaSO₄· 2H₂O
Used for plaster for walls, ceilings, sculptures
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Ionic compounds: Found in minerals and rocks
Calcite = CaCO₃Used in paint,Antacids, calciumSupplement for food
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Ionic compound with polyatomic ions
Sodium acetateIn Heat packs
Calcium sulfate in castsBarium sulfate to absorb x-rays
Acetate uses
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Sodium hydrogen carbonate(old name: sodium bicarbonate)
Medical: used in emergency situations to correct pH of blood
Baking soda: to make cakes rise
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Bleach
Dentistry: Clean and disinfectRoot canals
Rocket fuels:Source of oxygen
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POLYATOMIC IONS
Ions with -1 chargeperbromate BrO4
-
1
bromate BrO3-1
bromite BrO2-1
hypobromite BrO-1
perchlorate ClO4-1
chlorate ClO3-1
chlorite ClO2-1
hypochlorite ClO-
1
periodate IO4-1
iodate IO3-1
iodite IO2-1
hypoiodite IO-1
nitrate NO3-1
nitrite NO2-1
hydroxide OH-1
cyanide CN-1
thiocyanate SCN-
1
acetate C2H3O2-1
Permanganate MnO4
-1
bicarbonate HCO3-
1
Ions with a -2 Charge
carbonate CO3-2
phthalate C8H4O4-
2
sulfate SO4-2
sulfite SO3-2
chromate CrO4-2
dichromate Cr2O7-
2
oxalate C2O4-2
peroxide O2-2
Ions with a -3 Charge
phosphate PO4-3
phosphite PO3-3
arsenate AsO4-3
Ions with +1 chargeammonium ion
NH4+1
Examine the names & formulas: What is the pattern? Do they end in “–ide?”
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Compounds vs. Polyatomic Ions
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Polyatomic ions that you must know: NAME FORMULA CHARGE
Nitrate
AcetateCarbonate
Sulfate
Phosphate
Hydroxide
Ammonium
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Sodium + nitrate Calcium + nitrate
Formula
Name:
Using polyatomic ions:
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Cl¹⁻ CO₃²⁻
OH SO₄²⁻
PO₄³⁻
NO₃¹⁻
Na¹⁺
NH₄¹⁺
Zn²⁺
Co³⁺
Writing Formulas (criss –cross method)
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The transition metals are elements in Groups _____ to _______.
+ post transition metals: under the staircase.
Transition metals can have more than one charge.
Use Roman numerals after the name. Roman numbers: I = II = III = IV = V=
Ionic Compounds with Transition Metals
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Examples Iron II oxideIron III oxide
Write the formulas for:Copper I oxideCobalt III chlorideNickel II sulfide
Transition metals
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Sulfide Sulfate Oxide CarbonateMercury II
Iron III
Iron II
Formula Writing Practice
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Many transition and post transition metals have multiple oxidation numbers (charges)
Ni: oxidation numbers of _____ & _____ Fe: Find other examples:
Write formulas Write names
Practice: Writing Binary Formulas
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Inorganic Compounds
Ionic
M & NM
With Roman numera
l
3 or more
elements
Covalent (molecules
)
NM & NM
Diatomic Molecule
sAcids
Language of chemistry: Standardize system to represent compounds
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Covalent CompoundsMolecules
Names & Formulas for Inorganic Covalent Compounds
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Compounds-Stable-Most atoms are bonded in compounds-Separated with chemical reactions
-Usually need high heat or electricity
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Earth’s atmosphere
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Names of Binary Molecules First-element name 2nd – end in “ide”
Use prefixes-Always with 2nd
element -With 1st element except mono-
Element with lowest EN goes firstOn the Periodic Table – across /down
Prefix Numbermono- 1
di- 2tri- 3
tetra- 4penta- 5hexa- 6hepta- 7octa- 8nona- 9deca- 10
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Practice: Complete the table in your notes. Write the names
Write the formula
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Acids Acids are molecules that are in aqueous
solution (_________ in __________) and produce hydrogen ions (H¹⁺)
Typically start with H
Almost act as an ionic compound
Electronegativity Difference:
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Acids: H + Halogen Hydro + Halogen (ic) + Acid HBr Hydrobromic acid
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Oxyacids: common acids Contains oxygen (in a polyatomic ion)
◦ Note the endings of the anion & the acid name
H + nitrate = Nitric Acid H + sulfate = H + phosphate = H + acetate =
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Inorganic covalent compounds
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7 Diatomic Molecules Heck No Halogens
Named with the element name
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Common Names for 3 MoleculesMolecular name and formula: common
name Dihydrogen monoxide = Carbon tetrahydride = Nitrogen trihydride =
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Methane: CH₄
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Ammonia: NH₃
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Water: H₂0
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Element Chemical Symbol
Percent Weight in Earth's Crust
Oxygen O 46.60 Silicon Si 27.72 Aluminum Al 8.13 Iron Fe 5.00 Calcium Ca 3.63 Sodium Na 2.83 Potassium K 2.59 Magnesium Mg 2.09
Common elements found in the Earth's rocks.
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Group Typical Minerals Chemistry Compound Name
SulfidesCinnabar HgS
Galena PbSPyrite FeS2
Halides Fluorite CaF2
Halite NaCl
OxidesCorundum Al2O3
Cuprite Cu2OHematite Fe2O3
Carbonates(Nitrates and Borates)
Calcite CaCO3
Dolomite CaMg(CO3)2
Malachite Cu2(CO3)(OH)2
SulfatesAnhydrite CaSO4
Gypsum CaSO4 -2(H2O)
Phosphates Apatite Ca5(F,Cl,OH)(PO4 )
Silicates Quartz SiO₂ (metalloid & oxygen)
Important Minerals found in Rocks