empirical formulas. methanal vs. acetic acid both substances have c:h:o in a 1:2:1 ratio, but they...
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EMPIRICAL FORMULAS
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Methanal vs. acetic acid
Both substances have C:H:O in a 1:2:1 ratio, but they are completely different substances.
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Methanal vs. acetic acid
The EMPIRICAL FORMULA for both these substances is CH2O.
The MOLECULAR FORMULA for acetic acid is C2H4O2.
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EMPIRICAL VS. MOLECULAR FORMULAS
EMPIRICAL FORMULAS show the simplest whole number ratio of elements in a compound.
MOLECULAR FORMULAS show the element symbols and the exact no. of each type of atom in a molecular compound.
**formulas for ionic compounds are ALWAYS empirical.
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Comparing Empirical & Molecular Formulas
• Sometime the empirical and molecular formulas are the same and sometimes they are different
Glucose Hydrogen peroxide
Hydrazine Water
Molecular Formula C6H12O6 H2O2 N2H4 H2O
Empirical Formula
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Finding the Empirical Formula from Percent Composition
1.Use a chart to organize your work\
2.Assume you have 100 g sample so that your mass % is the same as your mass in grams.
3.To get a whole number at the end…multiply.
Atom Assume 100g:Mass (g)
MM (g/mol) n (mol) Smallest Ratio
Whole Number
A rhyme to help you remember what goes in the chart:
Percent to massMass to moleDivide by smallMultiply til whole
If the decimal ends in…. Fraction Multiply by…...33 1/3 3…25 1/4 4... 1.5 ½ 2…,67….75
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EXAMPLE 1: Find the empirical formula of a compound with 35.4% sodium and the remainder nitrogen.
STEP 1: Always assume you are working with 100 g of the compound.
Atom Assume 100g:Mass (g)
MM (g/mol) n (mol) Smallest Ratio
Whole Number
Na 35.4g 22.99
N 64.6g 14.01
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EXAMPLE 1: Find the empirical formula of a compound with 35.4% sodium and the remainder nitrogen.
STEP 2: Calculate the amount of each element in moles using n=m/MM
Atom Assume 100g:Mass (g)
MM (g/mol) n (mol) Smallest Ratio
Whole Number
Na 35.4g 22.99 n=m/MM =35.4/22.99 =1.539…
N 64.6g 14.01 n=4.61…
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EXAMPLE 1: Find the empirical formula of a compound with 35.4% sodium and the remainder nitrogen.
STEP 3: Determine the whole number ratio by dividing each element mole value by the lowest number.
Atom Assume 100g:Mass (g)
MM (g/mol) n (mol) Smallest Ratio
Whole Number
Na 35.4g 22.99 n=m/MM =35.4/22.99 =1.539…
1
N 64.6g 14.01 n=4.61…3
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EXAMPLE 1: Find the empirical formula of a compound with 35.4% sodium and the remainder nitrogen.
STEP 4: Multiply each number by an integer to obtain all whole numbers.
Empirical Formula is NaN3**not needed this time
Atom Assume 100g:Mass (g)
MM (g/mol)
n (mol) Smallest Ratio
Whole Number
Na 35.4g 22.99 n=m/MM =35.4/22.99 =1.539…
1
N 64.6g 14.01 n=4.61…3
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EXAMPLE 2: Determine the empirical formula of a compound that contains 69.9% iron and 30.1% oxygen by mass.
***Assume 100g of substance***
STEP 1: Calculate the amount of each element in 100g.
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EXAMPLE 2: Determine the empirical formula of a compound that contains 69.9% iron and 30.1% oxygen by mass.
STEP 2: Divide the amount of each element by the smallest amount.
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EXAMPLE 2: Determine the empirical formula of a compound that contains 69.9% iron and 30.1% oxygen by mass.
STEP 3: Find an equivalent whole number ratio and write the empirical formula.
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Tips for Solving Empirical Formula Problems• Don’t round until the very end.
• If the value is 0.95 round to 1, if the value is 0.05 round to 0, if between 0.45 to 0.55 round to 0.5.
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Determining the Empirical Formula by Experiment • You can calculate a molecular formula
using the periodic table, for example you know that pure copper will oxidize to become CuO. But, as a scientist you need to confirm this by experimentation.
• This can be done using a variety of methods such as a synthesis reaction.
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HOMEWORK:pp. 292 #1 (practice)
pp. 293 #1-5, 7
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Molecular Formula
• The molecular formula (actual formula) can only be found if you have both the:o Molar mass of the compound &o Empirical Formula (or percent composition)
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Steps to Finding Molecular Formula1.Find the molar mass of the empirical formula
2.Find the ratio of the molar mass of the compound to the empirical formula using:
3. Multiply the empirical formula by the ratio to obtain the molecular formula.
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Example 1
• The empirical formula for Vitamin C is C5H4O3 and its molar mass is 176.17 g/mol. Find the molecular formula
• MMEF = 88.07 g/mol
• Ratio = MMMF = 176.17g/mol = 2
MMEF 88.07g/mol
• Molecular Formula = C5 x 2 H4 x 2 O3 x 2
= C10H8O6
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Learning Check A compound with an empirical formula of C2OH4 and a molar mass of 88g/mol. What is the molecular formula of the compound?
C4O2H8
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Exit Card
• A sample of indium chloride with a mass of 0.5000g is found to have 0.2404g of chlorine. What is the empirical formula of the indium compound?