chapter 19: molecules and compounds section 19.2 chemical formulas
TRANSCRIPT
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Chapter 19: Molecules and Compounds
Section 19.2
Chemical Formulas
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Chemical Formula:
Ratio of atoms bonded together in a compound, i.e. X:Y
General Form: AxBy
where x and y are called subscripts.
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Recall NaCl (sodium chloride)…
Formula shows that atoms combine in a 1:1 ratio. Na1Cl1 = 1:1
Why in that ratio?
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To be stable…the net electrical charge of compounds must be zero.
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Oxidation Number:Indicates how many valence e- are lost, gained, or shared when bonding.(+) or (–) symbol is written after the number, i.e. 1+ or 2-
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2+
1+
3+ 3- 2- 1-
Common Oxidation Numbers0
Copy on your Periodic Table
Transition Metals
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Transition metals have more than one oxidation #. Roman numerals show oxidation #.
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Writing Chemical Formulas – monatomic ions
1. Symbol of (+) ion always written 1st.
2. Symbol of (–) ion always written 2nd.
3. Add subscripts so sum of oxidation #’s is zero.
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Example:
Write formula for binary (2 element) compound made of iron(III) and oxygen.
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1. Find oxidation #’s of elements:
iron(III) = Fe3+
oxygen = O2-
How do you make a cmpd electrically neutral?
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Calculate Fe3+ ions needed to combine with O2- ions
to make electrical charges equal zero.
2 (3+) added to 3 (2-) = 0
2 (Fe3+) added to 3 (O2-) = 0
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2-
2. To determine ratios to write chemical formulas…Use the Criss-cross Method
Fe3+
O2-3+
2 3
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Writing Chemical Formulas with polyatomic ions“poly” means many.
See page 329: Oxidation #’s for polyatomic ions.
Each polyatomic ion is treated like a single ion.
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Rules for writing formulas for cmpds with polyatomic ions:
Symbol or formula & oxidation # of (+) ion 1st.
Use PT or Table 19.2, pg 329. Symbol or formula & oxidation # of (-) ion 2nd.
Again, use PT or Table 19.2.
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Add oxidation #’s of (+) and (-) ions. = 0? If yes, then write formula: (+)ion 1st/(-) ion 2nd. = 0? How many of each ion are needed so oxidation #’s = 0? HINT: Find LCM LeastCommonMultiple
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Example: Write formula for aluminum sulfate.
1st ion is always (+). Use PT to find oxidation #.Aluminum = Al3+
2nd ion is always (-). Use Table 19.2.Sulfate = SO4
2-
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LCM of 2 and 3?
0(Al3+) x 2 = 6+
6 How many of each ion are needed?
(SO42-) x 3 = 6-
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Write chemical formulaAl2(SO4)3
Don’t change subscripts in polyatomic ion!! Use ( )
Criss-cross method
Al3+ SO42-
2 3
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Naming binary ionic compounds
Write name of 1st element or polyatomic ion.Write root name of 2nd element and add -ide.Exs: chlor-ine = chlor-idephosph-orus = phosph-ide
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Naming ionic cmpds with polyatomic ions
Write name of (+) ion 1st. Use PT or Table 19.2
Write name of (-) ion 2nd. Use PT or Table 19.2
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Naming binary covalent compoundsSpecify number of each element by using prefixes (Figure 19.25, pg 332).
If only one atom of 1st element, don’t use mono-
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Examples:
CO carbon monoxide
CO2 carbon dioxide
PCl5 phosphorus pentachloride
N2S6 dinitrogen hexasulfide
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Empirical vs Molecular formulasEmpirical formula – simplest whole number ratio of elements in cmpd.Molecular formula – actual # of atoms of each element in a compound.
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Example:
Molecular formula -sugar
C6H12O6
Empirical formula -sugar
CH2O