Chapter 2 Chemical Names and Formulas and Formulas.
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Transcript of Chapter 2 Chemical Names and Formulas and Formulas.
Chapter 2Chapter 2
Chemical NamesChemical Names
and Formulasand Formulas
Naming Ions
IE X + energy X+ + e-
Atom Ion
Cation
• CationCation• Positive IonPositive Ion
• MetalMetal
• Loses ElectronsLoses Electrons
Cation t looks like a + Cation t looks like a +
Naming Ions
EA X + e- X- + energy
Atom Ion
Anion
• AnionAnion • Negative IonNegative Ion
• NonmetalNonmetal
• Gains ElectronsGains Electrons
Anion n in middle stands for negativeAnion n in middle stands for negative
Monoatomic IonMonoatomic Ion
Monatomic IonMonatomic Ion – Ion that consists of a – Ion that consists of a single atomsingle atom• CationCation
• Positive IonPositive Ion
• MetalMetal
• Loses ElectronsLoses Electrons
• AnionAnion• Negative IonNegative Ion
• NonmetalNonmetal
• Gain ElectronsGain Electrons
Rules for Ion Names/Symbols: Cation
Metals = use element name
= use symbol with superscript charge
= superscript is written in air
Alkali Metals Transition Metals
Hydrogen H+1 Silver Ag+1
Lithium Li+1 Gold Au+1
Sodium Na+1
Potassium K+1
Rules for Ion Names/Symbols: Cation
Metals = use element name
= use symbol with superscript charge
= superscript is written in air
Alkaline Earth Metals Transition Metals
Magnesium Mg+2 Cobalt Co+2
Calcium Ca+2 Nickel Ni+2
Strontium Sr+2 Zinc Zn+2
Barium Ba+2
Rules for Ion Names/Symbols: Cation
Some metals have multiple charges.
Stock System uses Roman numerals.
Roman numerals = charge!!
1 I 6 VI
2 II 7 VII
3 III 8 VIII
4 IV 9 IX
5 V 10 X
.
Rules for Ion Names/Symbols: Cation
Copper (I) Cu+1 Tin (II) Sn+2
Copper (II) Cu+2 Tin (IV) Sn+4
Iron (II) Fe+2 Manganese (II) Mn+2
Iron (III) Fe+3 Manganese (IV) Mn+4
Lead (II) Pb+2
Lead (IV) Pb+4
Rules for Ion Names/Symbols: Anion
Nonmetals = use element name with ‘ide’
= use symbol with superscript charge
= superscript is written in air
Halogens
Fluorine Fluoride F-1
Chlorine Chloride Cl-1
Bromine Bromide Br-1
Iodine Iodide I-1
Rules for Ion Names/Symbols: Anion
Nonmetals = use element name with ‘ide’
= use symbol with superscript charge
= superscript is written in air
Oxygen Family Nitrogen Family
Oxygen Oxide O-2 Nitrogen Nitride N-3
Sulfur Sulfide S-2 Phosphorus
Carbon Family Phosphide P-3
Carbon Carbide C-4
Rules for Ion Names/Symbols: Cation or Anion ?
Multiples can be cation or anion.
It depends on what other ion is around it.
Cation Anion
Carbon C+4 Carbide C-4
Nitrogen N+5 Nitride N-3
Phosphorus P+5 Phosphide P-3
Binary CompoundsBinary Compounds
Composed of 2 elementsComposed of 2 elements• Can be either ionic or molecularCan be either ionic or molecular
Binary Ionic CompoundsBinary Ionic Compounds
Consist of IonsConsist of Ions• Metallic IonsMetallic Ions bonded to bonded to Nonmetal ionsNonmetal ions
oror
• CationsCations bonded to bonded to AnionsAnions
Writing Names forBinary Ionic Compounds
Steps
1. Use ION names.
2. Write the CATION name.
3. Then write the ANION name.
For example,
NaCl becomes Sodium Chloride
MgBr2 becomes Magnesium Bromide
CuO becomes Copper (II) Oxide
Writing Formulas for Writing Formulas for Binary Ionic CompoundsBinary Ionic Compounds
StepsSteps1.1. USEUSE the the IONS.IONS.
2.2. Write the symbol for the Write the symbol for the CATIONCATION..
3.3. Then write the symbol for the Then write the symbol for the ANION.ANION.
4.4. Balance the charges to zero. The Balance the charges to zero. The subscripts denotes the number of ions subscripts denotes the number of ions needed to balance the charges to zero.needed to balance the charges to zero.
Example Example ((Level 1Level 1))
Sodium ChlorideSodium Chloride
NaNa+1+1 ClCl-1-1
NaNaClCl
Example Example (Level 1)(Level 1)
Magnesium OxideMagnesium Oxide
OO-2-2MgMg+2+2
MgMgOO
Example Example (Level 1)(Level 1)
Aluminum NitrideAluminum Nitride
AlAl+3+3
AlAlNN
NN-3-3
PracticePractice
1.1. Potassium IodidePotassium Iodide
2.2. Calcium SulfideCalcium Sulfide
3.3. Aluminum PhosphideAluminum Phosphide
4.4. Gold FluorideGold Fluoride
5.5. Barium OxideBarium Oxide
6.6. Sodium BromideSodium Bromide
7.7. Strontium SulfideStrontium Sulfide
Example Example (Level 2)(Level 2)
Lithium OxideLithium Oxide
LiLi+1+1 OO-2-2
LiLi22OO
LiLi+1+1
Example Example (Level 2)(Level 2)
Calcium FluorideCalcium Fluoride
CaCa+2+2 FF-1-1
CaCaFF22
FF-1-1
Example Example (Level 2)(Level 2)
Aluminum IodideAluminum Iodide
AlAl+3+3 II-1-1
AlAlII33
II-1-1II-1-1
Practice
1.1. Potassium OxidePotassium Oxide
2.2. Strontium BromideStrontium Bromide
3.3. Aluminum ChlorideAluminum Chloride
4.4. Gold SulfideGold Sulfide
5.5. Silver NitrideSilver Nitride
6.6. Barium FluorideBarium Fluoride
7.7. Calcium IodideCalcium Iodide
Example Example (Level 3)(Level 3)
Aluminum SulfideAluminum Sulfide
AlAl+3+3 SS-2-2
AlAl22SS33
SS-2-2 SS-2-2AlAl+3+3
Example Example (Level 3)(Level 3)
Tin (IV) NitrideTin (IV) Nitride
SnSn+4+4 NN-3-3
SnSn33NN44
NN-3-3 NN-3-3SnSn+4+4SnSn+4+4 NN-3-3
Polyatomic IonsPolyatomic Ions
Polyatomic IonsPolyatomic Ions – Ions composed of – Ions composed of more than one atommore than one atom • Most end in Most end in iteite or or ateate
Polyatomic Ions
Ammonium NH4+1
Cyanide CN-1
Hydroxide OH-1
Nitrite NO2-1 Nitrate NO3
-1
Carbonate CO3-2
Sulfite SO3-2 Sulfate SO4
-2
Phosphite PO3-3 Phosphate PO4
-3
Example Example (Level 1)(Level 1)
Ammonium ChlorideAmmonium Chloride
ClCl--
NHNH44ClCl
NHNH44+1+1
Example Example (level 1)(level 1)
Barium SulfateBarium Sulfate
BaBa+2+2 SOSO44-2-2
BaBaSOSO44
Polyatomic Ions OnlyPolyatomic Ions Only
When writing compounds if you need When writing compounds if you need more than one polyatomic ion you more than one polyatomic ion you must add must add parenthesisparenthesis
Example Example (Level 2)(Level 2)
Ammonium SulfateAmmonium Sulfate
NHNH44+1+1 SOSO44
-2-2
NHNH4422SOSO44
NHNH44+1+1
((NHNH44))22SOSO44
Example Example (Level 2)(Level 2)
Barium HydroxideBarium Hydroxide
BaBa+2+2 OHOH-1-1
BaBaOHOH22 BaBa((OHOH))22
OHOH-1-1
Practice
1. Ammonium Phosphate
2. Calcium Hydroxide
3. Aluminum Nitrate
4. Magnesium Sulfate
5. Tin (IV) Carbonate
6. Strontium Sulfate
7. Barium Nitrate
Nomenclature Nomenclature of Ionic Compoundsof Ionic Compounds
StepsSteps
1.1. Use the names of the Use the names of the ionsions..
2.2. Write the Write the metalmetal first followed by the first followed by the nonmetalnonmetal
3.3. The The subscriptssubscripts take care of themselves take care of themselves
Example Example
NaClNaCl
NaNa+1+1
SodiumSodium ChlorideChloride
ClCl-1-1
ExampleExample
CaClCaCl22
CaCa+2+2
CalciumCalcium ChlorideChloride
ClCl-1-1 ClCl-1-1
Example Example
CuSOCuSO44
CuCu+2+2
Copper (II) Copper (II) SulfateSulfate
SOSO44-2-2
Practice
1.1. NaINaI
2.2. (NH(NH44))22SOSO44
3.3. MgBrMgBr22
4.4. AlAl22(CO(CO33))33
5.5. CuOCuO
6.6. FeFe22OO33
7.7. CaCa33PP22
Formula Writing and NomenclatureFormula Writing and NomenclatureCovalent (Molecular) CompoundsCovalent (Molecular) Compounds
StepsSteps
1.1. Write the first Write the first nonmetalnonmetal symbol followed symbol followed by the second by the second nonmetal nonmetal symbolsymbol..
2.2. The Greek prefixes denote the The Greek prefixes denote the subscriptssubscripts..
3.3. Do not need to balance the charges.Do not need to balance the charges.
Greek PrefixesGreek Prefixesfor Molecular Compoundsfor Molecular Compounds
1 Mono 6 Hexa
2 Di 7 Hepta3 Tri 8 Octa4 Tetra 9 Nona5 Penta 10 Deca
ExampleExampleCarbonCarbon DiDioxideoxide
CC
CCOO22
OO22
ExampleExample
Dinitrogen Monoxide
NN
NN22OO
OO22 11
PracticePractice
1.1. Sulfur DioxideSulfur Dioxide
2.2. Trichlorine TetraiodideTrichlorine Tetraiodide
3.3. Pentaphosphorus HexasulfidePentaphosphorus Hexasulfide
4.4. Heptaoxygen OctaselenideHeptaoxygen Octaselenide
5.5. Nonafluorine DecanitrideNonafluorine Decanitride
6.6. Dinitrogen PentoxideDinitrogen Pentoxide
7.7. Carbon TetrachlorideCarbon Tetrachloride
Naming Molecular CompoundsNaming Molecular Compounds
RulesRules
1.1. Write the 1Write the 1st st element name.element name.
2.2. Write the 2Write the 2ndnd element name with an element name with an ending of “ending of “ideide””
3.3. Add Add Greek prefixes Greek prefixes to both names. The to both names. The Greek prefix Greek prefix denotes the subscript.denotes the subscript.
4.4. Do not use a mono on the 1Do not use a mono on the 1stst element element name. name.
Example
SiSiOO22
SiliconSilicon OxygenOxygen
SiliconSilicon DiDioxideoxide
DiDiideide
ExampleExample
PP44FF66
PhosphorusPhosphorus FluorineFluorine
TetraTetraphosphorusphosphorus HexaHexafluoridefluoride
HexaHexaideide
TetraTetra
PracticePractice
1.1. COCO
2.2. SiSi22FF
3.3. OO33BrBr77
4.4. ISIS
5.5. ONON44
6.6. FF44HH33
7.7. PP77SS99
Halogenated Oxyanions
Name:
Prefix Suffix
Hypo root ite
root ite
root ate
Per root ate
Example:
Chlorine
Hypochlorite ClO-1
Chlorite ClO2-1
Chlorate ClO3-1
Perchlorate ClO4-1
Try Bromine and Iodine.
Polyatomic Oxyacids
Example:
Chlorine
Hypochlorite ClO-1
Chlorite ClO2-1
Chlorate ClO3-1
Perchlorate ClO4-1
Example:
Chlorine
Hypochlorous acid HClO
Chlorous acid HClO2
Chloric acid HClO3
Perchloric acid HClO4
Binary Acids
Formula: Hydrogen w Halogen
Name: Hydro+Root+ic Acid
HCl Hydrochloric Acid
HBr Hydrobromic Acid
HI Hydroiodic Acid
HF Hydrofluoric Acid
Alkanes
Methane Ethane Propane Butane Pentane
Alcohols
Methanol Ethanol Propanol Butanol Pentanol
Other functional groups?
Alcohols Ethers Aldehydes Ketones Carboxylic acid Ester Amine Amide
Formula weights/Molar Mass
The sum of atomic weights for a compound (in amu)
The number of grams in one mole of a substance (in g)
Lewis Dot Structures
For atoms For ionic
compounds For molecular
compounds
LDS: Neutral Molecules
Draw the dot structures of each atom Share one atom for each element (to make
a single bond between each element) Count electrons around each atom If octets are incomplete, share more
electrons between atoms
LDS: Negatively Charged Molecules
Repeat procedure for uncharged molecules Add one electron for each negative charged
atom
LDS: Positively charged molecules
Same procedure as negative… except remove one electron
Web Practice Site
http://www.fernbank.edu/Chemistry/nomen.html