Names and Formulas Ionic Compounds Binary Main Group M & NM Using Polyatomic ions
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Transcript of Names and Formulas Ionic Compounds Binary Main Group M & NM Using Polyatomic ions
Names and FormulasIonic Compounds
◦Binary Main Group M & NM ◦Using Polyatomic ions◦Transition metals with variable
charges Covalent Compounds
◦Names & Formulas
NC Essential Standards1.2: Understand the bonding that occurs in
simple compounds in terms of bond type, strength and properties.◦ 1.2.1: compare the relative strength of ionic, covalent,
and metallic bonds◦ 1.2.2: Infer the type of bond and its chemical formula
formed between atoms◦ 1.2.3: Compare inter- and intra- particle forces.◦ 1.2.4: Interpret the name and formula of compounds
using the IUPAC convention◦ 1.2.5: Compare the properties of ionic, covalent,
metallic, and network compounds.
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
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
Binary Ionic Compound with Representative Metals Example: Chlorine and
magnesiumRules for formula
◦Metal (cation)1st NM (anion) 2nd
◦Change number of each until charges = 0
◦Subscripts tell the number of atoms/moles
Rules for names:◦Metal 1st – metal’s element name◦NM 2nd – change ending to “-ide”◦No prefixes
Ionic compounds with polyatomic ions
Rules for formulas◦Cation 1st Anion 2nd
◦Use parentheses around the polyatomic ion◦Change number of each ion until charges =
0 ◦Check polyatomic ion: name, formula &
chargeRules for Names
◦Cation 1st Anion 2nd ◦Be careful about the ending (“-ate”, etc.) ◦No prefixes
Sodium + nitrate Ammonium + nitrideFormula
Name:
Using polyatomic ions:
Common Polyatomic IonsNAME FORMULA CHARGE
Nitrate
Acetate
NO₃⁻¹
C₂H₃O₂⁻¹
-1
-1Carbonate
Sulfate
CO₃⁻²
SO₄⁻²
-2
-2
Phosphate PO₄⁻³ -3Hydroxide OH ⁻¹ -1
Ammonium NH⁺¹ +1
Nick the Camel ate a clam for supper in Phoenix
http://www.youtube.com/watch?v=TZgv21FmEzk&list=PLs9HjZz1--dAB_gUIJJOhAu1Rrvaa56J6
Memorizing polyatomic ions
Criss – Cross methodUse the charges (oxidation numbers) to
help determine the number of atoms (moles)
Al⁺³(CO₃⁻²)Check if it the smallest (simplest) ratio
Cl¹⁻ CO₃²⁻ OH¹⁻ SO₄²⁻
PO₄³⁻
NO₃¹⁻
Na⁺¹
NH₄⁺¹
K⁺¹
Ca⁺²
Mg⁺²
Writing Formulas (criss –cross method)selected examples from worksheet
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 chlorideTin IV sulfideNote: Check for the smallest (simplest) ratio
Transition metals
Cl¹⁻ CO₃²⁻ OH¹⁻ SO₄²⁻
PO₄³⁻
NO₃¹⁻
Zn⁺²Fe⁺³Co⁺³Fe⁺²
Writing Formulas (criss –cross method)selected examples from worksheet
Sulfide Sulfate Oxide CarbonateMercury II
Iron III
Iron II
Formula Writing Practice – selected examples
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
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
Inorganic Covalent Compounds Names & Formulas
Binary
Diatomic
Acids
Note: Organic compounds different naming system
Inorganic Compoun
ds
Ionic
Binary Main
metalsTransition
metalsPolyatomi
c ions
Covalent (molecule
s)
Binary Diatomic Acids
Inorganic covalent compounds
Earth’s atmosphere
Names of Binary MoleculesFirst-element name2nd – 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
Practice:Complete the table in your notes.Write the names
Write the formula
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:
Acids: H + HalogenHydro + Halogen (ic) + AcidHBrHydrobromic acid
Oxyacids: common acidsContains oxygen (in a polyatomic
ion)◦Note the endings of the anion & the acid name
H + nitrate = Nitric AcidH + sulfate = H + phosphate = H + acetate =
7 Diatomic Molecules Heck No Halogens
Named with the element name
Common Names for 3 MoleculesMolecular name and formula: common
nameDihydrogen monoxide =Carbon tetrahydride =Nitrogen trihydride =
Methane: CH₄
Ammonia: NH₃
Water: H₂0