how are the following words related? ourozlato de oro aurum all are the word for the element...
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How are the following words How are the following words related?related?
ouroouro
zlatozlato
de orode oro
aurumaurum
• All are the word for the element “gold” All are the word for the element “gold” in Portuguese, Croatian, Spanish, and in Portuguese, Croatian, Spanish, and LatinLatin
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CHAPTER 9p. 252
CHEMICAL NAMES AND FORMULAS
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SECTION 9.1 p. 253SECTION 9.1 p. 253NAMING IONSNAMING IONS
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•Atoms - neutral
•same # + and e-•Ions are atoms, or groups of atoms, with a charge (positive or negative)
•different # + and e-•gain or lose e-’s•Monotomic IonsMonotomic Ions – 1 atom w/ + or - charge
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A Cation is…A Cation is… + ion formed by losing e-’s Metals lose e-’s Charge written as superscript
K1+ Has lost one electron (no name change for positive ions)
Ca2+ Has lost two electrons
An Anion is…An Anion is…• - ion•gains e-’s•Nonmetals can gain e-’s
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Ion High School
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Predicting Ionic ChargesGroupGroup 1A1A:: Lose 1 e- to form 1+ ionsLose 1 e- to form 1+ ions
HH1+1+ LiLi1+1+ NaNa1+1+ KK1+1+ RbRb1+1+
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Predicting Ionic ChargesGroup 2AGroup 2A:: Loses 2 e-’s to form 2+ ionsLoses 2 e-’s to form 2+ ions
BeBe2+2+ MgMg2+2+ CaCa2+2+ SrSr2+2+ BaBa2+2+
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Predicting Ionic ChargesGroup 3AGroup 3A:: Loses 3 Loses 3
e-’s to form e-’s to form 3+ ions3+ ions
BB3+3+ AlAl3+3+ GaGa3+3+
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Predicting Ionic ChargesGroup 4AGroup 4A:: Do they Do they
loselose 4 e-’s or 4 e-’s or gaingain 4 4 e-’s?e-’s?
Neither! Group 4A Neither! Group 4A elements rarely form elements rarely form ions ions (they tend to share)(they tend to share)
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Predicting Ionic ChargesGroup 5AGroup 5A:: Gains 3 Gains 3
e-’s to form e-’s to form 3- ions3- ions
NN3-3-
PP3-3-
AsAs3-3-
Nitride
Phosphide
Arsenide
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Predicting Ionic Charges
Group 6AGroup 6A:: Gains 2 Gains 2 e-’s to form e-’s to form 2- ions2- ions
OO2-2-
SS2-2-
SeSe2-2-
Oxide
Sulfide
Selenide
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Predicting Ionic ChargesGroup 7AGroup 7A:: Gains 1 Gains 1
e- to form e- to form 1- ions1- ions
FF1-1-
ClCl1-1-
BrBr1-1-Fluoride
Chloride
Bromide
II1-1- Iodide
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Predicting Ionic ChargesGroup 8AGroup 8A:: Stable Stable
noble gases noble gases do notdo not form ions!form ions!
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Predicting Ionic ChargesGroup B elementsGroup B elements:: Many transition elements Many transition elements
have have more than onemore than one possible oxidation state. possible oxidation state.Iron (II) = Fe2+
Iron (III) = Fe3+Roman numerals show charges
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Naming cations
1) Stock system – Roman numerals in () indicates numerical value
2) Classical method – root word w/ suffixes (-ous, -ic)• Doesn’t give true value
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Naming cations•Stock system.•Cation - if the charge is always the same (like in the Group A metals) just write the name of the metal.
•Transition metals can have more than one charge.• Indicate their charge as Roman numeral in () after name of cation (Table 9.2, p.255)
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Predicting Ionic Charges Some of the Some of the post-transitionpost-transition elements also elements also have have more than onemore than one possible oxidation state. possible oxidation state.Tin (II) = Sn2+ Lead (II) = Pb2+
Tin (IV) = Sn4+ Lead (IV) = Pb 4+
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Predicting Ionic ChargesGroup B elementsGroup B elements:: Some transition elements Some transition elements
have have only oneonly one possible oxidation state, such possible oxidation state, such as these three:as these three:
Zinc = Zn2+Silver = Ag1+ Cadmium = Cd2+
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Exceptions:•Some transition metals have only one ionic charge:
•Do not use Roman numerals for these:
•Silver always 1+ (Ag1+)•Cadmium and Zinc always 2+ (Cd2+ and Zn2+)
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Practice by naming these:
•Na1+ •Ca2+ •Al3+ •Fe3+ •Pb2+ •Li1+
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Write symbols for these:
•Potassium ion•Magnesium ion •Copper (II) ion•Chromium (VI) ion•Barium ion•Mercury (II) ion
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Naming Anions
•Change monatomic element ending to – ide
•F1- a Fluorine atom becomes Fluoride ion.
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Practice by naming these:
•Cl1- •N3- •Br1- •O2-
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Write symbols for these:
•Sulfide ion•Iodide ion•Phosphide ion
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Polyatomic ions • Groups of atoms that stay together and have overall
charge• Usually end in –ate or -ite
• Acetate: C2H3O21-
• Nitrate: NO31-
• Nitrite: NO21-
• Permanganate: MnO41-
• Hydroxide: OH1- and Cyanide: CN1-?
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• Sulfate: SO42-
• Sulfite: SO32-
• Carbonate: CO32-
• Chromate: CrO42-
• Dichromate: Cr2O72-
• Phosphate: PO43-
• Phosphite: PO33-
• Ammonium: NH41+
Know Table 9.3 on page 257
If polyatomic ion begins with H, then combine the word hydrogen with the other polyatomic ion present:
H+ + CO32- → HCO3
-
hydrogen + carbonate → hydrogen carbonate ion
(One of the few positive polyatomic ions)
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Section 9.2 – Marble madness
• Pair up with someone• everyone gets a cup• The person in each pair whose birthday is closest to today gets to add 4 marbles in their cups
• The other person keeps an empty cup• Listen for further instructions
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SECTION 9.2 P. 260
NAMING & WRITING FORMULAS FOR IONIC
COMPOUNDS
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Example: Barium nitrate (note the 2 word name)
1. Write the formulas for cation and anion, including CHARGES!
BaBa2+2+ NONO33--2. Do charges balance?
3. Balance charges , if necessary, using subscripts. Use () if more than one polyatomic ion. Use criss-cross method to balance subscripts.
Not balanced!
( )( ) 22Now balanced.
= Ba(NO3)2
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Writing Ionic Compound Formulas
Example: Ammonium sulfate (note the 2 word name)
NHNH44++ SOSO44
2-2-
2. Do charges balance? Not balanced!
( )( )22
Now balanced.
= (NH4)2SO43. Balance charges , if necessary, using subscripts. Use () if more than one polyatomic ion. Use criss-cross method to balance subscripts.
1. Write the formulas for cation and anion, including CHARGES!
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Writing Ionic Compound Formulas
Example: Iron (III) chloride (note the 2 word name)
1. Write the formulas for cation and anion, including CHARGES!
FeFe3+3+ClCl--
2. Do charges balance?
3. Balance charges , if necessary, using subscripts. Use () if more than one polyatomic ion. Use criss-cross method to balance subscripts.
Not balanced!
33Now balanced.
= FeCl3
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Writing Ionic Compound Formulas
Example: Aluminum sulfide (note the 2 word name)
1. Write the formulas for cation and anion, including CHARGES!
AlAl3+3+ SS2-2-
2. Do charges balance?
3. Balance charges , if necessary, using subscripts. Use () if more than one polyatomic ion. Use criss-cross method to balance subscripts.
Not balanced!
22 33Now balanced.
= Al2S3
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Writing Ionic Compound Formulas
Example: Zinc hydroxide (note the 2 word name)
1. Write the formulas for cation and anion, including CHARGES!
ZnZn2+2+ OHOH--
2. Do charges balance?
3. Balance charges , if necessary, using subscripts. Use () if more than one polyatomic ion. Use criss-cross method to balance subscripts.
Not balanced!
( )( )22
Now balanced.
= Zn(OH)2
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Naming Ionic CompoundsNaming Ionic Compounds•1. Name cation first, then anion
•2. Monatomic cation = name of element
Ca2+ = calcium ion
•3. Monatomic anion = root + -ide
Cl = chloride
CaCl2 = calcium chloride
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Naming Ionic CompoundsNaming Ionic Compounds
•some metals form more than one charge (usually transition metals)
•use Roman numeral in name:
PbCl2 – use anion to find charge on
cation (chloride always 1-)
Pb2+ is lead (II) cation
PbCl2 = lead (II) chloride
(Metals with multiple oxidation states)(Metals with multiple oxidation states)
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Things to look for:
1) If cation has ( ), the number in parenthesis is its charge.
2) If anion ends in –ide, likely monoatomic
3) If anion ends in -ate or –ite, it’s polyatomic
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Practice by writing formula or name
•Iron (II) Phosphate•Stannous Fluoride•Potassium Sulfide•Ammonium Chromate
•MgSO4
•FeCl3
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Section 9.3 p. 268Naming and Writing Formulas for Molecular Compounds
Molecular cmpds…•made of nonmetals•smallest piece… molecule•not bound by opposite charge attraction•can’t use charges to figure # of each atom (no charges present)
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Molecular v.s. Ionic Compounds• Ionic: use charges to determine # of each
•Molecular: name tells you # of atoms
•prefix tells exact # of each element
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Know these prefixes (Table 9.4 p. 269)
PrefixPrefix MonoMono DiDi TriTri TetraTetra PentaPenta HexaHexa HeptaHepta OctaOcta NonaNona decadeca
ValueValue 11 22 33 44 55 66 77 88 99 1010
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Formula Elements # atoms prefixes
N2O
PBr5
P4S3
CS2
IF7
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Using Prefixes to name covalent compounds
• To write the name, write two words:
•One exception…..don’t write mono when only one of first element
Prefix name Prefix name -ide
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Using Prefixes to name covalent compounds• To write the name, write two words:
•One exception is we don’t write mono if there is only one of the first element.
• Normally, we do not have double vowels when writing names (oa oo)
Prefix name Prefix name -ide
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Practice by naming these:
•NO2
•Cl2O7
•CBr4
•CO2
•BaCl2 (This one will not use prefixes, since it is an ionic compound!)
= nitrogen dioxide
= dichlorine heptoxide= carbon tetrabromide
= carbon dioxide
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Write formulas for these:•diphosphorus pentoxide•tetraiodine nonoxide•phosphorus trifluoride•carbon tetrahydride•sulfur hexafluoride
more SF6
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Section 9.4 p. 271Naming and Writing Formulas for Acids and Bases
Acids are…•Cmpds containing 1 or more H atoms & produces H ions (H1+) when dissolved in H2O•Chem formula starts with H followed by anion•anion determines acid name
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Rules for Naming acids: Name it as normal cmpd first
1) If anion ends in –ide:1) Acid name begins w/ prefix hydro- 2) change -ide to -ic acid
• HCl(aq) - hydrogen ion and chloride ion = hydrochloric acid
• H2S(aq) hydrogen ion and sulfide ion = hydrosulfuric acid
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Naming Acids• If anion has O, it ends in -ate or -ite2) change suffix -ate to -ic acid (no prefix)
• If you “ate” something acidic, you would probobaly say “ic”!If you “ate” something acidic, you would probobaly say “ic”!
• Example: HNO3 Hydrogen and nitrate ions = Nitric acid
3) change the suffix -ite to -ous acid (no prefix)
• Example: HNO2 Hydrogen and nitrite ions = Nitrous acid
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Anion ending Example Acid name Example
-ide Chlor ide, Cl - Hydro-(stem)-ic acid
Hydrochloric acid
-ite Sulf ite, SO3 2- (stem)-ous acid Sulfurous acid
-ate Nitrate, NO3 - (stem)-ic acid Nitric acid
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Naming AcidsNaming Acids
Normal ending
____-ide
____-ate
____-ite
Acid name is…
hydro-___-ic acid
_____-ic acid
_____-ous acid
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Practice by naming these:
•HF
•H3P
•H2SO4
•HCN
•H2CrO4
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Write formulas for these:
•hydroiodic acid•acetic acid•carbonic acid•phosphorous acid•hydrobromic acid
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Names and Formulas for Bases•A base is ionic cmpd producing hydroxide ions (OH1-) when dissolved in water
•Bases named same way as other ionic cmpds:•Name of cation (which is a metal) followed by name of anion (hydroxide)
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Names and Formulas for Bases• NaOH - sodium hydroxide
• Ca(OH)2 - calcium hydroxide
• To write the formula:
1) Write symbol for metal cation
2) followed by formula for hydroxide ion (OH1-)
3) use criss-cross method to balance charges
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Practice by writing the formula for the following:
•Magnesium hydroxide•Iron (III) hydroxide•Zinc hydroxide
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Practice by naming the following bases:
•NaOH
•NH4OH
•Ca(OH)2
•Al(OH)3
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Section 9.5 p. 274The Laws Governing Formulas and Names
• Review: Law of Conservation of Mass?Review: Law of Conservation of Mass?• Mass neither created or destroyed but is conserved during any chem rxn
Mass reactants = mass products
Mass cmpd = mass of SUM of elements in cmpd
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•1. Law of Definite Proportions (mass) - in a sample of a pure cmpd, masses of elements always in same proportions
•CO2 (carbon dioxide)
•CO (carbon monoxide)
Law of Definite ProportionsLaw of Definite Proportions
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Law of Multiple Proportions Law of Multiple Proportions (Dalton’s Law)(Dalton’s Law)
•2. Law of Multiple Proportions- Dalton stated whenever 2 elements form more than one cmpd, the different masses of 1 element that combine with the same mass of the other element are in the ratio of small whole numbers
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Same mass of oxygen
- Page 275
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Law of definite and multiple proportions
Guided Practice Problem 34 p. 275 (p. 90 #34 in workbook)
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p. 275 practice problem #34Lead forms two compounds with oxygen. One compound contains 2.98 g of Pb and 0.461 g of O. The other contains 9.89 g of Pb and 0.763 g of O. For a given mass of oxygen, what is the lowest whole number mass ratio of lead in the two compounds?
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Step 1. Write the ratio of lead to oxygen for each cmpd.
______g Pb 9.89 g Pb
0.461 g O ______g O
Step 2. Divide the numerator by the denominator in each ratio.
6.46 ______ _______g Pb
_________ g O
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Step 3. Write a ratio comparing the first compound to the second.
_____ g Pb/g O
13.0 g Pb/g O
Step 4. Simplify. Note that this ratio has no units (they cancel out)
0.497 = roughly 1
1 __
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The mass ratio of lead per gram of oxygen in the two compounds is:
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Summary of Naming and Formula Writing
•Naming formulas – flowchart - Figure 9.20, page 277
•Writing formulas – flowchart - Figure 9.22, page 278
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Helpful to remember...1. In an ionic compound, the net ionic charge is zero (criss-cross method)
2. An -ide ending generally indicates a binary compound
3. An -ite or -ate ending means there is a polyatomic ion that has oxygen
4. Prefixes generally mean molecular; they show the number of each atom
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Helpful to remember...5. A Roman numeral after the name of a cation is the ionic charge of the cation