naming ii smart
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Unit 7Nomenclature IIHow to get the formula from the
name
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Binary covalent compounds are compounds with two (2) nonmetals (Ex. CO, SF6, P2O5).
Binary Covalent Compounds
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Binary Covalent Compounds
Determining the formula: Identify the elements in the compound. Confirm they are both nonmetals. Use the prefix to tell how many atoms of each element there are in the compound.
mono = 1 • di = 2 • tri = 3 • tetra = 4 • penta = 5
hexa = 6 • hepta = 7 • octo = 8 • nona = 9 • deca = 10
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Binary Covalent Compounds
Determining the formula: To indicate how many atoms of each element are in the formula, use subscripts.
Example: carbon dioxide has1 carbon and 2 oxygens = C1O2 = CO2
(carbon’s 1 subscript is understood)
mono = 1 • di = 2 • tri = 3 • tetra = 4 • penta = 5
hexa = 6 • hepta = 7 • octo = 8 • nona = 9 • deca = 10
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Binary Covalent Compounds
Practice: selenium tetrafluoride __________________________________ octaphosphorus pentabromide__________________________________ heptanitrogen hexachloride__________________________________ iodine trifluoride__________________________________
mono = 1 • di = 2 • tri = 3 • tetra = 4 • penta = 5
hexa = 6 • hepta = 7 • octo = 8 • nona = 9 • deca = 10
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Acids
Acid - a compound that produces hydrogen ions, (H+) when dissolved in water. An acid will always end in the word "acid"! Also, an acid formula will always begin with hydrogen!
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Acids
Finding the formula of an acid1) What kind of acid is it?
a. If it begins with “hydro”, it is binary, meaning hydrogen bound to a nonmetal.
b. If it does not begin with “hydro”, it is ternary, meaning hydrogen bound to a polyatomic ion.
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Acids
Finding the formula of an acid2) Find the formula of a binary acid!
a. First, identify the nonmetal from the root of the word before acid.
Example: Hydrochloric Acidthe nonmetal is
chlorine.
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Acids
Finding the formula of an acid2) Find the formula of a binary acid!
b. Then, find the oxidation number of hydrogen (always 1+) and the nonmetal and write them as superscripts of each ion. This makes a cation(+) and an anion(–)
Example: H+1
Cl–1
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Acids
Finding the formula of an acid2) Find the formula of a binary acid!
c. Next, CRISS-CROSS the number of each oxidation number (NOT the charge!) down to the subscript of the opposite ion to indicate how many atoms you have of each ion in the compound.
Example:
H+1
Cl–1
= H1 Cl1
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Acids
Finding the formula of an acid2) Find the formula of a binary acid!
d. Reduce subscripts to lowest whole number ratio.
Example HCl(1 subscripts are understood)
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Acids
Finding the formula of an acid2) Find the formula of a binary acid!
Practice: Hydrochloric Acid_________________________________ Hydroselenic Acid_________________________________ Hydroiodic Acid_________________________________
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Acids
Finding the formula of an acid3) Find the formula of a Ternary Acid!
a. Identify the polyatomic ion.i. If it ends in “-ous” acid,
change the end to “-ite”, look up on polyatomic ion list.
ii. If it ends in “-ic” acid, change the end to “-ate”, look up on polyatomic ion list.
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Acids
Finding the formula of an acid3) Find the formula of a Ternary Acid!
b. Write the oxidation numbers of H and the polyatomic anion as superscripts
c. Criss cross the numbers only (not the charge!)
d. Reduce subscripts to lowest whole number ratio.
SAME AS
BINARY ACIDS
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Acids
Finding the formula of an acid3) Find the formula of a Ternary Acid!
Practice: Chlorous Acid____________________________________ Sulfuric Acid____________________________________ Perchloric Acid____________________________________
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Ionic Compounds
Ionic Compounds are made of a metal and a nonmetal (KCl, NaCl, NaI, CaCl2, BeF2).
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Ionic Compounds
Determining the Formula of an Ionic Compound1) Identify the elements that make up the compound
a. The first term, the metal, is the cation (+) and will look the same as it does on the periodic table.
b. The second term, the nonmetal, is the anion (–) and its ending has been changed to"-ide”. Determine the element name from the root of the word.
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Ionic Compounds
Determining the Formula of an Ionic Compound2) Form the cation and anion by looking at oxidation numbers.
3) Use the criss-cross method to form the compound.
4) Reduce subscripts to lowest whole numbers.
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Ionic Compounds
Practice: sodium chloride ____________________________________________
magnesium fluoride ____________________________________________
aluminum iodide____________________________________________
calcium sulfide____________________________________________
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Compounds withPolyatomic Ions
Polyatomic ions are groups of covalently bonded atoms that function as ions.
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Compounds w/Polyatomic Ions
Determining the Formula:1) Identify the first term, the cation (+), and the second term, the anion (–)
a. the cation, anion, or BOTH may be polyatomic ions.
2) Form the cation and anion by looking at oxidation numbers.
3) Use the criss-cross method to form the compound.
4) Reduce subscripts to lowest whole numbers.
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Compounds w/Polyatomic Ions
Practice: Sodium cyanide________________________________
Aluminum nitrite________________________________
Ammonium silicate________________________________
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Ionic Compounds w/ Transition Metals
Transition metals are the d block on the periodic table!
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Ionic Compounds w/ Transition Metals
Determining the Formula from the Name:1) Identify the transition metal and the anion.
2) Form the cation and anion by finding the oxidation numbers of the ions.
a. transition metal - the Roman numeral
b. anion - periodic table groups or polyatomic ions
3) Use the criss-cross method to form the compound.
4) Reduce subscripts to lowest whole numbers.
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Ionic Compounds w/ Transition Metals
Practice: tin (IV) iodide__________________
mercury (II) sulfide______________
iron (III) oxide__________________
nickel (III) sulfate________________
chromium (VI) phosphate__________
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Compounds w/Polyatomic IonsIon Name Ion Name
HCO3- hydrogen carbonate
CO32- carbonate
CN- cyanide CrO42-
chromate
C2H3O2-
acetate Cr2O72-
dichromate
ClO- hypochlorite SiO32- silicate
ClO2- chlorite SO32- sulfite
ClO3- chlorate SO42- sulfate
ClO4- perchlorate PO33- phosphite
MnO4- permanganate PO43- phosphate
NO2- nitrite NO3- nitrate
NH4+ ammonium OH- hydroxide