Download - Chemical Formulas Copy the text colored RED or Purple throughout the PPT. Also complete the TABLES
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Chemical Formulas
Copy the text colored RED or Purple throughout the PPT. Also complete the TABLES
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You have lists of:Common polyatomic ionsMultivalent metalsCovalent prefixes
Use your periodic table to determine the charges of common elements when they form ions
Reminders from Naming Chemicals
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Binary Ionic compounds
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Definitions- Review
Binary Ionic Compound- compound containing two elements—one metal and one non-metal
+Cation
+Cation
-Anion
-Anion Ionic Compound
Ionic bond- bond formed by attraction between + and - ions
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Metals & Non-Metals
Ionic Bonds are between metals & non-metals
H He
Li Be B C N O F Ne
Na Mg Al Si P S Cl Ar
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
Cs Ba Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Fr Ra Lr Rf Db Sg Bh Hs Mt Uun Uuu Uub Uut
Metals Metalloids Non-metals
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These compounds:End in “-ide” (except “hydroxide and cyanide”)Do NOT contain covalent prefixes
To write these formulas:Write the symbol & charge of the first element (the metal,
cation)Write the symbol & charge of the second element (the
non-metal, anion)Add more of the cations and/or anions to have a neutral
compoundUse subscripts to show how many of each type of ion is
there.
Identifying & Naming Binary Ionic
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Name Cation Anion Criss Cross Formula
Sodium Chloride
Calcium Bromide
Cesium Chloride
Aluminum Sulfide
Potassium Oxide
Calcium Sulfide
Lithium NItride
21
Na+1 Cl-1 None NaCl
Ca+2 Br-1 Ca+2 Br-1 CaBr2
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Example #1
Sodium chloride
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Example #1
Sodium chloride
Cation
Anion
Na+1
Cl-1
NaCl
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Example #1
Sodium chloride
Cation
Anion
Na+1
Cl-1
NaCl
Na+1Cl-1
The +1 and -1 cancel each other out
The compound is neutral…no subscripts are needed.
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Example #2
Calcium bromide
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Example #2
Calcium bromide
Cation
Anion
Ca+2
Br-1
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Example #2
Calcium bromide
Cation
Anion
Ca+2
Br-1
CaBr2
Ca+2Br-1
Criss Cross the charges down
Ca+2 Br-1
The subscript “1” is dropped because its redundant. The subscript “2” is used to show that 2 anions are needed.
Ca1Br2
1 2
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Example #3
Aluminum Sulfide
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Example #3
Aluminum Sulfide
Cation
Anion
Al+3
S-2
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Example #2
Aluminum Sulfide
Cation
Anion
Al+3
S-2
Al2S3
Al+3 S-2
Criss Cross the charges down
The subscript “2” is used to show that 2 cations are needed. The subscript “3” is used to show that 3 anions are needed.
Al2S3
2 3Al+3 S-2
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Let’s Practice
Example:Write the following chemical formulas
Cesium chloride
Potassium oxide
Calcium sulfide
Lithium nitride
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Let’s Practice
CsCl
K2O
CaS
Li3N
Example:Write the following chemical formulas
Cesium chloride
Potassium oxide
Calcium sulfide
Lithium nitride
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Polyatomic Ionic Compounds
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Definition-Review
Polyatomic Ion- more than one atom that together have a charge
+Cation
+Cation
Polyatomic Ionic Compound- compound containing at least one polyatomic ion
-Polyatomic
Anion
Polyatomic IonicCompound
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These compounds:Do not end with “-ide” (except hydroxide & cyanide)Do not use covalent prefixes
To write these formulas:Write the symbol & charge of the cation & anionAdd additional cations or anions to have a neutral
compoundUse subscripts to show the number of ions
When using subscripts with a polyatomic ion, you must put the polyatomic ion in parenthesis.
Identifying & Naming Polyatomic Ionic
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Name Cation Anion Criss Cross Formula
Sodium Carbonate
Magnesium Nitrate
Lithium Iodate
Sodium Nitrate
Calcium Chlorate
Potassium Sulfite
Calcium Hydroxide
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Example #4
Sodium carbonate
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Example #4
Sodium carbonate
Cation
PolyatomicAnion
Na+1
CO3-2
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Example #4
Sodium carbonate
Cation
PolyatomicAnion
Na+1
CO3-2
Na2CO3
Na+CO32-
Criss Cross the charges down
Na+ CO32-
The subscript “2” is used to show that 2 cations are needed.
Na2CO3
2 1
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Example #5
Magnesium nitrate
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Example #5
Magnesium nitrate
Cation
PolyatomicAnion
Mg+2
NO3-1
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Example #5
Magnesium nitrate
Cation
PolyatomicAnion
Mg+2
NO3-1
Mg(NO3)2 Use parenthesis when adding subscripts to polyatomic ions
Mg+2NO3-1
Criss Cross the charges down
Mg+2 NO3-1
The subscript “2” is used to show that 2 anions are needed.
Mg(NO3)2
21
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Let’s Practice
Example:Write the following chemical formulas
Lithium Iodate
Sodium nitrate
Calcium chlorate
Potassium sulfite
Calcium hydroxide
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Let’s Practice
LiIO3
NaNO3
Ca(ClO3)2
K2SO3
Ca(OH)2
Example:Write the following chemical formulas
Lithium iodate
Sodium nitrate
Calcium chlorate
Potassium sulfite
Calcium hydroxide
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Multivalent Metals
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Definition-Review
Multivalent Metal- metal that has more than one possibility for cationic charge
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These compounds:Will have roman numerals
To write these formulas:Same as binary ionic or polyatomic ionic.The roman numerals tell the charge of the
metal (cation)
Identifying & Naming Multivalent Metals
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Name Cation Anion Criss Cross Formula
Iron (III) Oxide
Copper (II) Nitrate
Iron (II) Nitrate
Copper (I) Chloride
Lead (IV) Hydroxide
Tin (II) Oxide
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Example #5
Iron (III) oxide
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Example #5
Iron (III) oxide
Cation
Anion
Fe+3
O-2
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Example #6
Iron (III) oxide
Cation
Anion
Fe+3
O-2
Fe2O3
Fe+3O2-
Criss cross the charges
Fe+3 O2-
The subscript “2” and “3” are used to show the numbers of atoms needed.
Fe2O3
32
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Example #7
Copper (II) nitrate
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Example #7
Copper (II) nitrate
Cation
PolyatomicAnion
Cu+2
NO3-1
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Example #7
Copper (II) nitrate
Cation
PolyatomicAnion
Cu+2
NO3-1
Cu(NO3)2
Cu+2NO3-1
Criss cross the charges
Cu+2 NO3-1
Use parenthesis when adding subscripts to a polyatomic ion
Cu(NO3)2
1 2
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Let’s Practice
Example:Write the following chemical formulas
Iron (II) nitrate
Copper (I) chloride
Lead (IV) hydroxide
Tin (II) oxide
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Let’s Practice
Fe(NO3)2
CuCl
Pb(OH)4
SnO
Example:Write the following chemical formulas
Iron (II) nitrate
Copper (I) chloride
Lead (IV) hydroxide
Tin (II) oxide
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Binary Covalent Compounds
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Definition-Review
Binary Covalent Compound compound made from two non-metals that share electrons
Nonmetal
Nonmetal
Nonmetal
Nonmetal Covalent compound
Covalent bond atoms share electrons
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These compounds:Use covalent prefixes
To write these formulas:Write the symbols of the first and second
elementUse the covalent prefixes (assume the first
element is “1” if there’s no prefix) as the subscripts to show number of atoms.
Identifying & Naming Binary Covalent
Atoms do not form charges when bonding covalently…you DO NOT need to worry about charges with this type!
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Name Prefix First Element
Prefix Second Element
Formula
Dinitrogen Tetraoxide
Di- = 2 Nitrogen = N Tetra- = 4 Oxide = O N2O4
Silicon dioxide
Carbon monoxide
Nitrogen dioxide
Diphosphorus pentaoxide
Carbon Tetrachloride
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Example #7
Dinitrogen Tetraoxide
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Example #7
Dinitrogen Tetraoxide
N
O
“Di-” = 2
“Tetra-” = 4
N2O4
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Example #8
Silicon dioxide
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Example #8
Silicon dioxide
Si
O
“Mono-” is not written for the first element
“Di-” = 2
SiO2
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CAUTION!!!
bi-di-
Stands for “2” in covalent compounds
Means there’s a hydrogen in the polyatomic anion
“di” and “bi” do not mean the same thing!
Carbon dioxide = CO2
Sodium biphosphate = Na2HPO4
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Let’s Practice
Example:Write the following chemical formulas
Carbon monoxide
Nitrogen dioxide
Diphosphorus pentaoxide
Carbon tetrachloride
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Let’s Practice
CO
NO2
P2O5
CCl4
Example:Write the following chemical formulas
Carbon monoxide
Nitrogen dioxide
Diphosphorus pentaoxide
Carbon tetrachloride
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Nomenclature Summary
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Mixed Practice
Example:Write the following chemical formulas
Magnesium hydroxide
Copper (II) nitrate
Iron (III) oxide
Nitrogen dioxide
Sodium bicarbonate
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Mixed Practice
Mg(OH)2
Cu(NO3)2
Fe2O3
NO2
NaHCO3
Example:Write the following chemical formulas
Magnesium hydroxide
Copper (II) nitrate
Iron (III) oxide
Nitrogen dioxide
Sodium bicarbonate