Agenda: 10/23
Warm-up: Ionic Bonds
Ionic Compounds – names & formulas◦ Binary◦ With Roman numerals◦ With 3 or more elements
Covalent Compounds (molecules)
Homework:
Read
Ionic Bonds (Black Study Guide)
Compounds-Stable (do not easily change)-Most atoms are bonded into compounds-Separated with chemical reactions
-Usually need high heat or electricity
Ionic CompoundsMetals lose valence electrons
Non-metals gain valence electrons
Ionic bonding occurs when a metal loses 1+ 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
Cl Ca Cl
= Ca Cl
Electron Dot Diagram (Lewis)
Ionic CompoundsNames and Formulas
Inorganic Compounds
Ionic
M & NM
With Roman numer
al
3 or more
elements
Covalent (molecul
es)
NM & NM
Diatomic Molecule
sAcids
Language of chemistry: Standardize system to represent compounds
Inorganic Compounds
Ionic
Binary - representative metals
Formulas
Names
Transition & post
transition metals
Formulas
Names
Polyatomic ions
Formulas
Names
Covalent (molecul
es)
Binary
Formulas
Names
Diatomic molecules
Formulas
Names
Acids
Formulas
Names
Ionic Compounds
Ionic compounds: Found in minerals and rocks Granite: rock (combination of minerals)
Halite: NaCl Use as source of table salt
Ionic compounds: rocks & minerals
Al₂O₃Aluminum oxide
Pyrite (Fool’s gold)
Iron sulfide
FeS₂Used to produce sulfuric acid for the chemical industry
Ionic Compounds - Opposites Attract
Separate cations and anions to bond◦ Use only the single element ions (not the polyatomic ions)
Write the symbol and the charge
Write the new compound formed by combining the ions. Write the formula showing that the charges (oxidation numbers) add up to 0 (cancel out)
Name the compound. Write at least 15 compounds.
◦ Ten should include subscripts.
a. The formula for ionic compounds are determined by the charges (oxidation numbers). The overall charge of the compound must equal 0.
b. The charges are determine by the number of valence electrons that the element loses or gains to reach 8 valence electrons. This is the octet rule that makes the compound stable (does not easily react.)
Ionic Compounds: Names & Formulas
c.Metals always _______ electrons to form a ____ ion.
Non-metals always _______ electrons to form a ______ ion .
Group 1 2 13 14 15 16 17 18
Charge=Oxid. #
e. Since Aluminum has a charge (oxidation number) of 3⁺,- It must have __________ chlorine atoms (ions) to make a stable compound.
-It must have __________ nitrogen atoms (ions) to make a stable compound.
-It must have _______ aluminum and ________ oxygen atoms (ions) to make a
stable compound.
Write the correct formula for compounds composed of:
Sodium and bromine
Sodium and sulfur
Sodium and phosphorus
Calcium and bromine
Calcium and sulfur
Calcium and phosphorus
Rules for naming:◦Metals are written first.◦Non-metals change their name to an “-ide” ending.
Prefixes are ________ ___________.
Names for Ionic compounds
Ionic Compounds- Formulas
Salt is a commonly used term for all ionic compounds
Some Ionic Compounds are more complex
Include polyatomic ions
Ionic compounds: Found in minerals and rocks
Barite = BaSO₄Used to make paper & glassSource of barium used For x-rays of the digestivesystem
Ionic compounds: Found in minerals and rocks
Gypsum = CaSO₄· 2H₂O
Used for plaster for walls, ceilings, sculptures
Ionic compounds: Found in minerals and rocks
Calcite = CaCO₃Used in paint,Antacids, calciumSupplement for food
Ionic compound with polyatomic ions
Sodium acetateIn Heat packs
Calcium sulfate in castsBarium sulfate to absorb x-rays
Acetate uses
Sodium hydrogen carbonate(old name: sodium bicarbonate)
Medical: used in emergency situations to correct pH of blood
Baking soda: to make cakes rise
Bleach
Dentistry: Clean and disinfectRoot canals
Rocket fuels:Source of oxygen
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?”
Compounds vs. Polyatomic Ions
Polyatomic ions that you must know: NAME FORMULA CHARGE
Nitrate
AcetateCarbonate
Sulfate
Phosphate
Hydroxide
Ammonium
Sodium + nitrate Calcium + nitrate
Formula
Name:
Using polyatomic ions:
Cl¹⁻ CO₃²⁻
OH SO₄²⁻
PO₄³⁻
NO₃¹⁻
Na¹⁺
NH₄¹⁺
Zn²⁺
Co³⁺
Writing Formulas (criss –cross method)
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
Examples Iron II oxideIron III oxide
Write the formulas for:Copper I oxideCobalt III chlorideNickel II sulfide
Transition metals
Sulfide Sulfate Oxide CarbonateMercury II
Iron III
Iron II
Formula Writing Practice
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