By: Brendan Timm Jesse Durrant Braedan Fitzpatrick and Austin Penrose.
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Transcript of By: Brendan Timm Jesse Durrant Braedan Fitzpatrick and Austin Penrose.
![Page 1: By: Brendan Timm Jesse Durrant Braedan Fitzpatrick and Austin Penrose.](https://reader036.fdocuments.net/reader036/viewer/2022072116/56649d175503460f949ecf83/html5/thumbnails/1.jpg)
Chapter 4-Inorganic Nomenclature
By: Brendan Timm
Jesse Durrant
Braedan Fitzpatrick
and Austin Penrose
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Monovalent CompoundsCompound name to compound formula
Identify the two elements in the compound and the charges. (e.g. Lithium Oxide = Li+ O2-)
Criss cross your charges
Put the two symbols together and then remove charges.
Answer: Li2O
Li+ O2-
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Monovalent Compounds Compound formula to compound name
Name the metal in the compound Then name the non-metal in the
compound and change the ending to “ide”
e.g NaCl• Sodium• Chlorine to Chloride • Sodium Chloride
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Multivalent CompoundsCompound Name to Compound Formula
Identify element symbols and their ion charge
E.g. Chromium (iii) Oxide Criss cross charges Combine the two symbols and get
rid of their charges Then make into smallest possible
ratio• E.g. Cr3N3 = CrN
Cr3+ O2-
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Multivalent Compounds Compound formula to compound name
Multivalent element: element that can form more than one stable ion
Name the metal ion, see if it has more than one charge
Un criss cross the combining capacitye.g. (Cr2O3, O2- and Cr 3+)
Chromium (III) Chromium (III) Oxide
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Binary Molecular CompoundsCompound Name to Compound Formula
Memorize to prefix system for subscript values of elements (mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca).
Identify the prefix for both elements and their corresponding subscript. (e.g. dinitrogen tetraoxide=2, 4)
Use the corresponding subscripts of the prefixes after their symbols. (e.g. N2O4)
Don’t reduce the subscripts.
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Binary Molecular CompoundsCompound Formula to Compound Name
Identify the subscript values of the elements and their corresponding prefixes. (e.g. H2O, 2=di and 1=mono)
Write down the two elements with their prefixes before their name.
Change the ending of the second element to “ide”. (dihydrogen monoxide)
Don’t add the prefix mono if the first element has a subscript of one. (e.g. CO2=carbon monoxide)
Don’t reduce prefixes
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Polyatomic IonsFrom formula to name
Write the positive ions name, will be either metal or ammonium (NH4
+) Determine if metal is multivalent, if it
is, indicate ion charge in roman numerals
Identify the negative ion and name itCr3(PO4)2 1. Chromate (II) 2. Chromate (II) Phosphate
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Polyatomic IonsFrom name to formula
Identify each ion and its charge E.g. Chromium (III) sulphate = Cr3+
SO4-2
Criss cross charges Cr3+ SO4-2
Put the symbols together and get rid of charge values.
For Polyatomic ions, use brackets around the whole ion. The whole ion has the subscript value. E.g. Cr2(SO4)3
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Hydrates A hydrate is a solid compound that is
surrounded by water molecules
Prefixes are also associated with hydrates - prefixes are words that represent how much of something there is
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Hydrates cont.Naming Hydrates:
1. Name the compound as you would regularly name it2. After writing the compound name, add the correct prefix in front of the word hydrate Ex. Al2O3 3H2O - aluminum oxide trihydrate
Writing Chemical Formulas for Hydrates: 1. Write the Elements symbol and use criss cross rule for first half of hydrate2. Then write the prefix number in front of H20 Ex. iron (II) sulphate pentahydrate - FeSO4 5H2O
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Bibliography http://stpatschem11.files.wordpress.c
om/2009/10/numerical_prefixes_silberberg_table_2-61.jpg?w=235&h=300