Chemistry Chemistry Chapter 7 Chapter 7 Chemical Formulas and Chemical Compounds
Elements combine to form bonds
Covalent Bonds
-Electrons are shared-Usually between two
non-metals
EXAMPLE: carbon dioxide
Ionic Bonds
-Electrons are transferred
-Usually between a metal and a non-metal or polyatomic ions
EXAMPLE: sodium chloride
Different systems of naming depending on the type of bond…BE CAREFUL!
IonsIonsIonsIons• Cation:Cation: A positive ion A positive ion
• MgMg2+2+, NH, NH44++
• Anion:Anion: A negative ionA negative ion • ClCl--, SO, SO44
2-2-
• Ionic Bonding:Ionic Bonding: Force of attraction Force of attraction between oppositely charged ions.between oppositely charged ions.
Predicting Ionic ChargesPredicting Ionic Charges
Group 1Group 1:: Lose 1 electron to formLose 1 electron to form 1+1+ ionsions
HH++ LiLi++ NaNa++ KK++
Na
How many valence electrons does Na have?Does Na satisfy the octet rule?
Bohr Model of Sodium
How can we satisfy the octet rule?Now does Na satisfy the octet rule?
How many protons does Na have?
Protons: 11
How many electrons does Na have?
Electrons: 11
What’s the net charge on Na?
× +1 = 11
× -1 = -11
0Now, how many electrons does Na have?
Electrons: 10 × -1 = -10
+1
+
Predicting Ionic Charges
Group 2Group 2::Loses 2 electrons to formLoses 2 electrons to form 2+2+ ionsions
BeBe2+2+ MgMg2+2+ CaCa2+2+ SrSr2+2+ BaBa2+2+
Mg
Bohr Model of Magnesium
How many valence electrons does Mg have?Does Mg satisfy the octet rule?How can we satisfy the octet rule?Now does Mg satisfy the octet rule?
What is the net charge of Mg?
Protons: 12 × +1 = 12
× -1 = -10Electrons: 10
+2
+2
Predicting Ionic ChargesPredicting Ionic ChargesGroup 13Group 13:: Loses 3 Loses 3
electrons to form electrons to form 3+ ions3+ ions
BB3+3+ AlAl3+3+ GaGa3+3+
Al
Bohr Model of Aluminum
How many valence electrons does Al have?Does Al satisfy the octet rule?How can we satisfy the octet rule?Now does Al satisfy the octet rule?
What is the net charge of Al?
Protons: 13 × +1 = 13
× -1 = -10Electrons: 10
+3
+3
Predicting Ionic ChargesGroup 14: Lose 4 electrons or
gain 4 electrons?Neither! Group 14 elements rarely form ions.
Predicting Ionic ChargesPredicting Ionic ChargesGroup 15Group 15:: Gains 3 electrons Gains 3 electrons
to formto form 3-3- ionsions
NN3-3-
PP3-3-
AsAs3-3-
Nitride
Phosphide
Arsenide
P
Bohr Model of Phosphorous
How many valence electrons does P have?Does P satisfy the octet rule?How can we satisfy the octet rule?Now does P satisfy the octet rule?
What is the net charge of P?
Protons: 15 × +1 = 15
× -1 = -18Electrons: 18
-3
-3
Predicting Ionic ChargesGroup 16: Gains 2 electrons
to form 2- ions
O2-
S2-
Se2-
Oxide
Sulfide
Selenide
S
Bohr Model of Sulfur
How many valence electrons does S have?Does S satisfy the octet rule?How can we satisfy the octet rule?Now does S satisfy the octet rule?
What is the net charge of S?
Protons: 16 × +1 = 16
× -1 = -18Electrons: 18
-2
-2
Predicting Ionic ChargesPredicting Ionic ChargesGroup 17Group 17:: Gains 1 electron Gains 1 electron
to formto form 1-1- ionsions
FF1-1-
ClCl1-1-
BrBr1-1-Fluoride
Chloride
Bromide
II1-1- Iodide
Cl
Bohr Model of Chlorine
How many valence electrons does Cl have?Does Cl satisfy the octet rule?How can we satisfy the octet rule?Now does Cl satisfy the octet rule?
What is the net charge of Cl?
Protons: 17 × +1 = 17
× -1 = -18Electrons: 18
-1
-1
Predicting Ionic ChargesPredicting Ionic ChargesGroup 18Group 18:: Stable Noble gasesStable Noble gases
do notdo not form ions!form ions!
Predicting Ionic ChargesGroups 3 - 12Groups 3 - 12:: Many Many transitiontransition elements have more elements have more
than one possible oxidation state.than one possible oxidation state.
Iron (II) = Fe2+ Iron (III) = Fe3+
Predicting Ionic ChargesPredicting Ionic ChargesGroups 3 - 12Groups 3 - 12:: SomeSome transitiontransition elements have only one elements have only one
possible oxidation state.possible oxidation state.
Zinc = Zn2+ Silver = Ag+ Cadmium = Cd2+
MemorizeMemorize
Polyvalent Elements and Their Chargesto Memorize
Copper
Polyvalent Element Symbol Charge
Cu +1,+2
Lead Pb +2,+4
Iron Fe +2,+3
Mercury Hg,Hg2 +1,+2
Tin Sn +2,+4
Chromium Cr +2,+3
Cobalt
Nickel
Co
NiManganese Mn
+2,+3
+2,+3+2,+3
Polyatomic Ions to Memorize!+1 -1 -2
Ammonium NH4 +1 Acetate C2H3O2 -1Bromate BrO3 -1Chlorate ClO3 -1Chlorite ClO2 -1Cyanide CN -1Bicarbonate HCO3 -1Hydroxide OH -1Nitrate NO3 -1Nitrite NO2 -1Iodate IO3 -1Permanganate MnO4
Hydrogen Sulfate HSO4
Carbonate CO3 -2Chromate CrO4 -2Dichromate Cr2O7 -2Oxalate C2O4 -2Peroxide O2 -2Sulfate SO4 -2Sulfite SO3 -2
Arsenate AsO4 -3Phosphate PO4 -3
-3
Hand out Table
Writing Ionic Compound FormulasWriting Ionic Compound Formulas
Example: Barium nitrate
1. Write the formulas for the cation and anion, including CHARGES!
BaBa NONO33
2. Check to see if charges are balanced. (If so, skip to step 5)
3. Balance charges , if necessary, using subscripts. A. Cross over the charges by using the absolute value of each ion’s charge as the subscript for the other ion. B. Use parentheses if you need more than one of a
polyatomic ion.
Not balanced!
(( )) 224. Check the subscripts and divide them by their largest common factor to give the smallest possible whole-number ratio.
5. Write the formula without the charges.
2+ -Ba(NO3)2
Writing Ionic Compound FormulasWriting Ionic Compound Formulas
Example: Ammonium sulfate
1. Write the formulas for the cation and anion, including CHARGES!
2. Check to see if charges are balanced. (If so, skip to step 5)3. Balance charges , if necessary, using
subscripts. A. Cross over the charges by using the absolute value of each ion’s charge as the subscript for the other ion. B. Use parentheses if you need more than
one of a polyatomic ion. 4. Check the subscripts and divide them by their largest common factor to give the smallest possible whole-number ratio.5. Write the formula without the charges.
NHNH44 SOSO44
Not balanced!
( )( )22
+ 2-(NH4)2SO4
Let’s Practice
1. potassium nitrate2. sodium sulfate3. calcium hydroxide4. ammonium sulfite5. calcium phosphate6. aluminum chromate7. lithium bromide8. sodium peroxide
Pause for a Cause #2Page 251
16. Write formulas for each of the following compounds:
a. sodium fluoride
b. calcium oxide
c. potassium sulfide
d. magnesium chloride
e. aluminum bromide
f. lithium nitride
Writing Ionic Compound Formulas
Example: Copper II carbonate
1. Write the formulas for the cation and anion, including CHARGES!
2. Check to see if charges are balanced. (If so, skip to step 5)
5. Write the formula without the charges.
Cu2+ CO32-
They are balanced!
CuCO3
Writing Ionic Compound FormulasWriting Ionic Compound Formulas
Example: Iron (III) chloride
1. Write the formulas for the cation and anion, including CHARGES!
2. Check to see if charges are balanced. (If so, skip to step 5)
3. Balance charges , if necessary, using subscripts. A. Cross over the charges by using the absolute value of each ion’s charge as the subscript for the other ion. B. Use parentheses if you need more than one of a
polyatomic ion.
4. Check the subscripts and divide them by their largest common factor to give the smallest possible whole-number ratio.
5. Write the formula without the charges.
FeFe ClCl
Not balanced!
33
3+ -FeCl3
Names ending in –ide usually, but not always, represent an element from the
periodic table.
Writing Ionic Compound Formulas
Example: Chromium III sulfide
1. Write the formulas for the cation and anion, including CHARGES!
2. Check to see if charges are balanced. (If so, skip to step 5)3. Balance charges , if necessary, using
subscripts. A. Cross over the charges by using the absolute value of each ion’s charge as the subscript for the other ion. B. Use parentheses if you need more than
one of a polyatomic ion. 4. Check the subscripts and divide them by their largest common factor to give the smallest possible whole-number ratio.5. Write the formula without the charges.
Cr S
Not balanced!
3
3+ 2-Cr2S32
Write formulas for each of the following compounds.
1. Chromium III hydroxide2. Mercury I chloride3. Tin IV chloride4. Iron II chromate5. Cobalt II sulfide6. Copper I sulfate7. Iron III oxide
Let’s Practice
Pause for a Cause #3Writing Formulas of Compounds that have Roman Numerals
Write the formulas for the following compounds: Lead II nitrate Iron II Sulfite Mercury I Chloride Tin II Chlorate Chromium III Dichromate Mercury II Phosphate Cobalt II Acetate
Naming Covalent Binary CompoundsNaming Covalent Binary Compounds Naming Covalent Binary CompoundsNaming Covalent Binary Compounds
• -- Compounds between twoCompounds between two nonmetalsnonmetals • -- First element First element in the formula isin the formula is named firstnamed first.. • -- Second element Second element is named as if it were anis named as if it were an
anionanion.. • -- Use prefixes Use prefixes • -- Only useOnly use monomono on second element - on second element -
PP22OO55 = =
COCO22 = =
CO =CO =
NN22O =O =
didiphosphorusphosphorus pentpentoxideoxide
carbon carbon didioxideoxide
carboncarbon monmonoxideoxidedidinitrogennitrogen monmonoxideoxide
1 – mono2 – di3 – tri4 – tetra5 - penta
6 – hexa7 – hepta8 – octa9 – nona10 – deca
If given the formula……..
• 1st determine if the compound is a binary (molecular) compound– If all the elements in the compound are non-metals
or metalloids the compound is a binary compound.– Use prefixes to name the compound.– CHARGES DON’T MATTER, DON’T WRITE
CHARGES!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!
– DON’T SWITCH THE PREFIXES!!!!!!!!!!!!!!!!!!!!
Pause for a Cause #4Write the formula of the following compounds(WRITE WHAT YOU SEE DO NOT CHECK OXIDATION STATE!)
a. Phosphorus Pentachloride
b. Carbon Tetrafluoride
c. Dinitrogen Pentaoxide
d. Tetraphosphorous Decaoxide
e. Carbon Monoxide
f. Carbon Disulfide
Sourvelis’s Rules For NamingLook at the first element in the compound.
If the first element is…
1. A group 1 or 2 metal, or if it is Ag, Zn, Al, Cd, simply name the compound. NaCl Sodium Chloride
2. A transitional metal all the way to the left of the metalloid line, use roman numerals. Fe2O3 Iron (III) Oxide
3. A metalloid or nonmetal use prefixes.
N2O5 Dinotrogen Pentoxide
4. is hydrogen name it like an acid. HCl Hydrochloric acid. Exception Acetic acid C2H3O2H
5. a carbon atom, name it as an organic molecule.
ex. C2H6 ethane
Mixed Review Sheet
Naming Ionic Compounds Using Rule 1Naming Ionic Compounds Using Rule 1Naming Ionic Compounds Using Rule 1Naming Ionic Compounds Using Rule 1• 1. 1. Cation first, then anionCation first, then anion
• 2. Monatomic cation = name of the element 2. Monatomic cation = name of the element • CaCa2+2+ = calcium= calcium ionion
• 3. Monatomic anion =3. Monatomic anion = rootroot ++ -ide-ide • ClCl-- = = chlorchlorideide
• CaClCaCl22 = calcium = calcium chlorchlorideide
4. For polyatomic ions, use the name of that polyatomic ion.
Let’s Practice!! Name the following compounds:
• MgCl2
• Ag2O
• Ca(OH)2
• SrS• KClO3
• NH4OH
• KClO2
• Magnesium Chloride• Silver Oxide• Calcium Hydroxide• Strontium Sulfide• Potassium Chlorate• Ammonium Hydroxide• Potassium Chlorite
Pause for a Cause #5 Name the following compounds:
K2CrO4
Ca(MnO4)2
Zn(HCO3)2
Mg3N2
Na2O2
Ba3(PO4)2
AgCl
If given the formula……..• And the compound is not a
binary compound, name the compound like an ionic compound.– Use roman numerals if the
first element is a transitional element or to the left of the metalloid line.
(Exceptions Ag, Zn, Cd)
Naming Ionic CompoundsUsing Roman Numerals
Naming Ionic CompoundsUsing Roman Numerals
Example:
• PbCl2
• Lead can be a Pb2+ or Pb4+ cation
• PbCl2 = lead (II) chloride
How do you know???
Some metals have multiple oxidation states (Groups 3-12 and to the left of the metalloid line)
How do we know that lead was +2?
PbCl2
What is the charge of chlorine ion?
-1
How many chlorine ions does PbCl2 have?
What’s the total charge of the chlorine ions?
-2
Compounds are neutral, so what must the charge of lead be in order to balance the -2 charge of chlorine?
+2The oxidation number of lead is
+2.
Let’s try Fe2O3
What is the charge of oxygen ion?
How many oxygen ions does Fe2O3 have?
What’s the total charge of the oxygen ions?
What must the charge of iron be in order to balance the -6 charge of the oxygens?
Fe O2 3
-2
-6+6
+3
Iron III OxideThe oxidation
number of iron is +3.
Let’s practice!!! Name the following compounds:• CuO• CoF3
• SnI4
• FeS
Copper II OxideCobalt III FluorideTin IV IodideIron II Sulfide
If given the name…..• If the compound is not a binary compound
(contains polyatomic ions), use the rules for writing ionic compounds.– Make sure to use the correct charges.– Make sure you don’t change the subscripts of the
polyatomic ions.– THE ANSWER DOES NOT HAVE ANY
CHARGES!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!
Name the following compounds:
Pb(ClO3)2
Co2O3
Fe2(Cr2O7)3
NiBr2
MnSO4
SnOHg2Cl2
Fe(HCO3)3
Pause for a Cause #6
If given the name…..• 1st check for prefixes.
– If prefixes are present, the compound is probably a binary compound.
– DON’T WORRY ABOUT CHARGES, DON’T WRITE CHARGES, JUST WRITE WHAT YOU SEE!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!
– ***Remember some polyatomic ions have prefixes (bicarbonate, dichromate, dimercury). Write these like ionic compounds.
Quiz: Write the Formulasulfur tetrachlorideammonium carbonatechromium (III) oxidesodium peroxideAntimony (III) Chloride
Acid Nomenclature• AcidsAcids
– Compounds that form HCompounds that form H++ in water. in water.
– Formulas usually begin with ‘H’.Formulas usually begin with ‘H’.
– Exception is acetic acid CHException is acetic acid CH33C00C00HH
• Examples:Examples:
– HCl HCl (aq)(aq) – hydrochloric acid – hydrochloric acid
– HNOHNO33 – nitric acid – nitric acid
– HH22SOSO44 – sulfuric acid – sulfuric acid
Anion Ending Acid Name
-ide hydro-(stem)-ic acid
-ate (stem)-ic acid
-ite (stem)-ous acid
Acid Nomenclature
Binary Binary
Ternary Ternary
An easy way to remember which goes with which…An easy way to remember which goes with which…
““In the cafeteria, you In the cafeteria, you ATEATE something something ICICky”ky”
Acid Nomenclature Flowchart
h yd ro - p re fix-ic en d in g
2 e lem en ts
-a te en d in gb ecom es-ic en d in g
-ite en d in gb ecom es
-o u s en d in g
n o h yd ro - p re fix
3 e lem en ts
AC ID Ss ta rt w ith 'H '
• HBr HBr (aq)(aq)
• HH22COCO33
• HH22SOSO33
• 2 elements, 2 elements, --ideide
• 3 elements, 3 elements, -ate-ate
• 3 elements, 3 elements, -ite-ite
hydrohydrobromic acidbromic acid
carboncarbonicic acid acid
sulfursulfurousous acid acid
Acid Nomenclature
• hydrofluoric acidhydrofluoric acid
• sulfuric acidsulfuric acid
• nitrous acidnitrous acid
• 2 elements2 elements
• 3 elements, 3 elements, -ic-ic
• 3 elements, 3 elements, -ous-ous
HF HF (aq)(aq)
HH22SOSO44
HNOHNO22
Acid Nomenclature
HH++ F- F-
HH++ SO SO442-2-
HH++ NO NO22--
Binary Acids
HF(aq) - HCl(aq) -HBr(aq) - HI(aq) - H2S(aq) -
hydrofluoric acidhydrochloric acidhydrobromic acidhydriodic acidhydrosulfuric acid
Exception, HI the “o” in hydro is left off for HI(aq), so its name is hydriodic acid.HCl(aq) HCl(gas)
Name ‘Em!• HH22SOSO33
• HNOHNO33
• H3PO4
• CH3COOH
sulfurous acidnitric acidphosphoric acidacetic acid
Write the Formula!
• Hydrobromic acidHydrobromic acid
• Nitrous acidNitrous acid
• Carbonic acidCarbonic acid
• Phosphoric acidPhosphoric acid
HBr
HNO2
H2CO3
H3PO4
• Straight Chains– Hydrocarbons linked in a straight chain
• C8H18
• Cyclochains– Hydrocarbon interlinked in a ring structure
• C6H12
Hydrocarbons - molecules that possess hydrogen and carbon
Alkanes – hydrocarbons with only C-C single bonds.
Example: Butane CH3CH2CH2CH3 C4H10 CnH2n+2
Alkenes – hydrocarbons with C=C double bonds.
Example: Butene CH3CH=CHCH3 C4H8 CnH2n
Alkynes – hydrocarbons with C C triple bonds.
Example: Butyne CH3C CCH3 C4H6 CnH2n-2
Alcohols – R-OH (-OH is hydroxyl group, NOT hydroxide)
Example: CH3OH Methanol
Basic Naming of HydrocarbonsHydrocarbon names are based on: 1) type,
2) # of carbons, 3) side chain type and position 1) name will end in -ane, -ene, or -yne2) the number of carbons is given by a “prefix”
1 meth- 2 eth- 3 prop- 4 but- 5 pent- 6 hex- 7 hept- 8 oct- 9 non- 10 dec-
Actually, all end in a, but a is dropped when next to a vowel. E.g. a 6 C alkene is hexene
Q - What names would be given to these:7C, 9C alkane2C, 4C alkyne1C, 3C alkene
heptane, nonaneethyne, butynemethene, propene
Mnemonic for First Four Prefixes
First four prefixes• Meth-
• Eth-
• Prop-
• But-
MonkeysEatPeeledBananas
Organic Compounds Containing Oxygen
• An alcohol is a compound obtained by substituting a hydroxyl group (-OH) for an –H atom on a carbon atom of a hydrocarbon group.• Some examples are
CH3 OH CH2CH3 OH CH3CHCH3
OH
methanol ethanol propanol