Download - Representing Chemical Compounds
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Representing Chemical Compounds
Naming Compounds and Writing Chemical Formulas
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Chemical Formula• Shows the kinds and numbers of atoms in a
substance.• If only one atom of the element in a
compound, you only write the element’s symbol. (Ex: Lithium fluoride LiF)
• If the molecules of the element each have more than one atom, a number is used as a subscript. (Ex: Lithium oxide Li2O).
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Molecular Formulas• Chemical formula for a molecular compound
is called a molecular formula.
• Shows the kinds and numbers of atoms present in a molecule of a compound.
• Examples: CO, CO2
• Tells nothing about the structure of the molecule --- doesn’t show arrangement of the various atoms.
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Formula Units• Chemical formulas represent ionic
compounds.
• Formula units – lowest whole-number ratio of ions in the compound.
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Ionic Charges• For most of the Group A elements, the
Periodic Table can tell what kind of ion they will form from their location.
• Elements in the same group have similar properties.
• Including the charge when they are ions.
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+2+1
+3 -3 -2 -1
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Naming Cations
• Cation- if the charge is always the same (Group A) just write the name of the metal.
• Transition metals can have more than one type of charge.
• Indicate the charge with roman numerals in parentheses.
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Name These• Na+1
• Ca+1
• Al+3
• Fe+3
• Fe+2
• Pb+3
• Li+1
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Write Formulas for these
• Potassium ion
• Magnesium ion
• Copper (II) ion
• Chromium (VI) ion
• Barium ion
• Mercury (II) ion
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Naming Anions• Anions are always the same. Change the element ending to – ide. F-1 Fluorine
F-1 Fluoride
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Name These• N-3
• Br-1
• O-2
• Ga+3
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Write These• Sulfide ion
• iodide ion
• phosphide ion
• Strontium ion
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Polyatomic Ions• Groups of atoms that stay together and have
a charge.
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Ions in Ionic Compounds
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Naming Binary Ionic Compounds
• Binary Compounds - 2 elements.
• Ionic - a cation and an anion.
• To write the names just name the two ions.
• Easy with Representative elements.
• Group A
• NaCl = Na+ Cl- = sodium chloride
• MgBr2 = Mg+2 Br- = magnesium bromide
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Naming Binary Ionic Compounds
• The problem comes with the transition metals.
• Need to figure out their charges.
• The compound must be neutral.
• same number of + and – charges.
• Use the anion to determine the charge on the positive ion.
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Naming Binary Ionic Compounds
• Write the name of CuO • Need the charge of Cu • O is -2 • copper must be +2 • Copper (II) chloride • Name CoCl3 • Cl is -1 and there are three of them = -3 • Co must be +3 Cobalt (III) chloride
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Naming Binary Ionic Compounds
• Write the name of Cu2S.
• Since S is -2, the Cu2 must be +2, so each one is +1.
• copper (I) sulfide
• Fe2O3
• Each O is -2 3 x -2 = -6
• 3 Fe must = +6, so each is +2.
• iron (III) oxide
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Naming Binary Ionic Compounds
• Write the names of the following • KCl • Na3N • CrN • Sc3P2 • PbO • PbO2 • Na2Se
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Ternary Ionic Compounds
• Will have polyatomic ions • At least three elements • name the ions • NaNO3 • CaSO4 • CuSO3 • (NH4)2O
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Ternary Ionic Compounds
• LiCN
• Fe(OH)3
• (NH4)2CO3
• NiPO4
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Writing Formulas
• The charges have to add up to zero.
• Get charges on pieces.
• Cations from name of table.
• Anions from table or polyatomic.
• Balance the charges by adding subscripts.
• Put polyatomics in parenthesis.
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Writing Formulas
• Write the formula for calcium chloride.
• Calcium is Ca+2
• Chloride is Cl-1
• Ca+2 Cl-1 would have a +1 charge.
• Need another Cl-1
• Ca+2 Cl 2-
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Write the formulas for these
• Lithium sulfide • tin (II) oxide • tin (IV) oxide • Magnesium fluoride • Copper (II) sulfate • Iron (III) phosphide • gallium nitrate • Iron (III) sulfide
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Write the formulas for these
• Ammonium chloride
• ammonium sulfide
• barium nitrate
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Things to look for
• If cations have (), the number is their charge.
• If anions end in -ide they are probably off the periodic table (Monoatomic)
• If anion ends in -ate or -ite it is polyatomic
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Molecular Compounds
Writing names and Formulas
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Molecular compounds
• made of just nonmetals
• smallest piece is a molecule
• can’t be held together because of opposite charges.
• can’t use charges to figure out how many of each atom
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Easier
Ionic compounds use charges to determine how many of each.
– Have to figure out charges. – Have to figure out numbers.
• Molecular compounds name tells you the number of atoms.
• Uses prefixes to tell you the number
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Prefixes
• 1 mono- • 2 di- • 3 tri- • 4 tetra- • 5 penta- • 6 hexa- • 7 hepta- • 8 octa-
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Prefixes
• 9 nona-
• 10 deca-
• To write the name write two words
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Prefixes
• 9 nona-
• 10 deca-
• To write the name write two words
• Prefix name Prefix name -ide
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Prefixes
• 9 nona-
• 10 deca-
• To write the name write two words
• One exception is we don’t write mono- if there is only one of the first element.
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Prefixes
• 9 nona- • 10 deca- • To write the name write two words
• One exception is we don’t write mono- if there is only one of the first element.
• No double vowels when writing names (oa oo)
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Name These
• N2O
• NO2
• Cl2O7
• CBr4
• CO2
• BaCl2
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Write formulas for these
• diphosphorus pentoxide
• tetraiodide nonoxide
• sulfur hexaflouride
• nitrogen trioxide
• Carbon tetrahydride
• phosphorus trifluoride
• aluminum chloride
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Acids
Writing names and Formulas
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Acids
• Compounds that give off hydrogen ions when dissolved in water.
• Must have H in them.
• will always be some H next to an anion.
• The anion determines the name.
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Naming acids
• If the anion attached to hydrogen is ends in -ide, put the prefix hydro- and change -ide to -ic acid
• HCl - hydrogen ion and chloride ion
• hydrochloric acid
• H2S hydrogen ion and sulfide ion
• hydrosulfuric acid
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Naming Acids
• If the anion has oxygen in it • it ends in -ate of -ite • change the suffix -ate to -ic acid • HNO3 Hydrogen and nitrate ions • Nitric acid • change the suffix -ite to -ous acid • HNO2 Hydrogen and nitrite ions • Nitrous acid
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Name these
• HF
• H3P
• H2SO4
• H2SO3
• HCN
• H2CrO4
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Writing Formulas
• Hydrogen will always be first
• name will tell you the anion
• make the charges cancel out.
• Starts with hydro- no oxygen, -ide
• no hydro, -ate comes from -ic, -ite comes from -ous
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Write formulas for these
• hydroiodic acid
• acetic acid
• carbonic acid
• phosphorous acid
• hydrobromic acid