Section 9.3—Analysis of a Chemical Formula

Slides:



Advertisements
Similar presentations
Section Percent Composition and Chemical Formulas
Advertisements

Percentage Composition and Empirical Formula
Percent Composition, Empirical, and Molecular Formulas
Empirical and Molecular Formulas
Percent Composition and Empirical Formulas Ch
Determining Chemical Formulas Experimentally % composition, empirical and molecular formula.
Percentage Composition
Empirical and Molecular Formulas
Molar Mass & Percent Composition
Chapter 3 Percent Compositions and Empirical Formulas
Mass Conservation in Chemical Reactions Mass and atoms are conserved in every chemical reaction. Molecules, formula units, moles and volumes are not always.
Empirical Formula The empirical formula indicates the ratio of the atoms of an element in a compound.
  I can determine the percent composition for each element in a compound or sample.
4.6 MOLECULAR FORMULAS. 1. Determine the percent composition of all elements. 2. Convert this information into an empirical formula 3. Find the true number.
1 Empirical Formulas Honors Chemistry. 2 Formulas The empirical formula for C 3 H 15 N 3 is CH 5 N. The empirical formula for C 3 H 15 N 3 is CH 5 N.
Empirical and Molecular Formulas
Percent Comp. Percentage composition Indicates the relative amount of each element present in a compound.
Section 9.3—Analysis of a Chemical Formula
Percent Composition (Section 11.4) Helps determine identity of unknown compound –Think CSI—they use a mass spectrometer Percent by mass of each element.
Empirical and Molecular Formulas. Empirical Formula What are we talking about??? Empirical Formula represents the smallest ratio of atoms in a formula.
Empirical and Molecular formulas. Empirical – lowest whole number ratio of elements in a compound Molecular – some multiple of the empirical formula Examples:
1 Percent Composition: Identifies the elements present in a compound as a mass percent of the total compound mass. The mass percent is obtained by dividing.
Percent Composition Like all percents: Part x 100 % whole Find the mass of each component, divide by the total mass.
1 Chapter 10 “Chemical Quantities” Yes, you will need a calculator for this chapter!
It’s time to learn about.... Stoichiometry: Percent Composition At the conclusion of our time together, you should be able to: 1. Determine the percent.
Unit 6: Chemical Quantities
Percent Composition and Empirical Formula
Section 10.3 Percent Composition and Chemical Formulas n n OBJECTIVES: – –Describe how to calculate the percent by mass of an element in a compound.
Unit Empirical and Molecular Formulas. Empirical Formulas Consists of the symbols for the elements combined in a compound, with subscripts showing.
Empirical Formula vs. Molecular Formula Empirical formula: the formula for a compound with the smallest whole-number mole ratio of the elements Molecular.
Ch. 11 The Mole The Mol House The Mol House Atoms in a molecule molecules molgrams Molar Mass Avogadro’s number Chemical formula.
Empirical & Molecular Formulas. Percent Composition Def – the percent by mass of each element in a compound Percent by mass = mass of element x 100 mass.
USING MOLAR CONVERSIONS TO DETERMINE EMPIRICAL AND MOLECULAR FORMULAS.
(4.6/4.7) Empirical and Molecular Formulas SCH 3U.
Calculating Empirical Formula Using percentage or mass to find the Empirical Formula.
Section 9.3—Analysis of a Chemical Formula How can we determine a chemical formula?
Calculating Empirical Formulas
Percent Composition What is the % mass composition (in grams) of the green markers compared to the all of the markers? % green markers = grams of green.
Empirical and Molecular Formulas Topic #20. Empirical and Molecular Formulas Empirical --The lowest whole number ratio of elements in a compound. Molecular.
Percent Composition.  We go to school for 180 days a year. What % of the year are we in school? Similar to finding % in any other situation.
Section 9.3—Analysis of a Chemical Formula
Empirical Formula.
EMPIRICAL FORMULA VS. MOLECULAR FORMULA .
% Composition & Empirical Formulas
Empirical and Molecular Formulas
DO NOW Pick up notes. Get out your periodic table and calculator.
Empirical Formulas.
Percent Composition and Molecular Vs. Empirical Formulas
You need a calculator AND periodic table for today’s notes
Empirical and Molecular Formulas
EMPIRICAL FORMULA The empirical formula represents the smallest ratio of atoms present in a compound. The molecular formula gives the total number of atoms.
Empirical and Molecular Formulas
Calculating Empirical and Molecular Formulas
From percentage to formula
Percent Composition Empirical Formula Molecular Formula
Percent Composition and Molecular Vs. Empirical Formulas
Empirical and Molecular Formulas
Section 9.3—Analysis of a Chemical Formula
Empirical and Molecular Formulas
TYPES OF FORMULA.
Empirical and Molecular Formulas
Empirical and Molecular Formulas
Percent Composition and Molecular Vs. Empirical Formulas
From percentage to formula
Empirical & Molecular Formulas
Empirical and Molecular Formulas
Empirical and Molecular Formulas
Percent Composition and Molecular Vs. Empirical Formulas
Empirical and Molecular Formulas
Molecular Formula.
Presentation transcript:

Section 9.3—Analysis of a Chemical Formula How can we determine a chemical formula?

Percent Composition How is percent composition found?

What is Percent Composition?

Example #1 Example: An 8.5 g sample is composed of carbon and hydrogen. If 5.5 g of the sample is found to be carbon, what is the percent composition by mass of the carbon and hydrogen in the sample?

Example #1 If total = 8.5 g and C = 5.5 g - then H = 3.0 g Example: A 8.5 g sample is composed of carbon and hydrogen. If 5.5 g of the sample is found to be carbon, what is the percent composition by mass of the sample? If total = 8.5 g and C = 5.5 g - then H = 3.0 g

Let’s Practice #1 A sample is 57.0% by mass chlorine, how many grams of chlorine are present in a 27.5 g sample?

Let’s Practice #1 A sample is 57.0% by mass chlorine, how many grams of chlorine are present in a 27.5 g sample? 27.5 g   27.5 g 100 100

Example #2 Percent composition can also be determined from a chemical formula Example: Find the percent composition, by mass, of CaCl2

Example #2 Percent composition can also be determined from a chemical formula Example: Find the percent composition, by mass, of CaCl2 Ca Cl 1 2 40.08 g/mole 35.45 g/mole  = 70.90 g/mole + 110.98 g/mole So for 1 mole: total = 110.98 g Ca = 40.08 g Cl = 70.90 g

Let’s Practice #2 Find the percent composition, by mass, of NaNO3

Find the percent composition, by mass, of NaNO3 Let’s Practice #2 Find the percent composition, by mass, of NaNO3 Na N 1 22.99 g/mole 14.01 g/mole  = + 85.00 g/mole O 3 16.00 g/mole 48.00 g/mole

Empirical Formulas

What’s an Empirical Formula? Empirical Formula –Lowest possible ratio of atoms CH2 is the lowest ratio (and empirical formula) of the molecule C3H6

Ratio of Atoms in a Molecule If the subscripts give the ratio of atoms, then they also give the ratio of moles of atoms In CaCl2 There is 1 Ca atom to every 2 Cl atoms. THEREFORE: There is 1 mole of Ca atoms to every 2 moles of Cl atoms!

Using Mole Ratio of Atoms in a Molecule If you know the whole number ratio of the moles for each atom….. then the subscripts of the chemical formula are known 1 mole C 2 mole H CH2

Example If given percents, use those percents as grams (as if you assume you have a 100 g sample)—Remember %’s add up to 100! 1 2 Change grams to moles for each atom Divide all moles by the smallest # of moles. We do this to find the lowest possible whole number ratios of the atoms*** 3 4 Use the ratio as subscripts for writing the chemical formula Example: Find the empirical formula if a sample contains Ca and Cl and is 36.1% Ca ***If this step doesn’t give whole numbers – you will need to multiply by a factor that will give you a whole number – you will see this in an example 

Example If given percents, use those percents as grams (as if you assume you have a 100 g sample)—Remember %’s add up to 100! 1 2 Change grams to moles for each atom Find the lowest possible whole number ratio of the atom (divide all moles by the smallest # of moles) 3 4 Use the ratio as subscripts for writing the chemical formula Example: Find the empirical formula if a sample contains Ca and Cl and is 36.1% Ca 36.1 g Ca 1 mol Ca = _____ mol Ca 0.901 40.08 g Ca CaCl2 63.9 g Cl 1 mol Cl = _____ mol Cl 1.80 35.45 g Cl 0.901 mol Ca = 1 mol Ca 0.901 1.80 mol Cl = 2 mol Cl 0.901

Find the empirical formula if a sample contains Let’s Practice #3 Find the empirical formula if a sample contains 40.92 g C, 4.58 g H and 54.5 g O 40.92 g C = _____ mol C g C mol C 1 12.01 3.41 4.58 g H = _____ mol H g H mol H 1 1.01 4.53 54.5 g O = _____ mol O g O mol O 1 16.00 3.41 C3H4O3 3.41 mol C = 1 mol C 3.41 4.53 mol H = 1.33 mol H 3.41 3.41 mol O = 1 mol O 3.41 Multiply the ratio (1 : 1.33 : 1) by 3 to make a whole number ratio (3 : 4: 3)

Molecular Formulas

What’s a Molecular Formula? Empirical Formula –Lowest possible ratio of atoms Molecular Formula – Actual ratio of atoms in a molecule

Empirical versus Molecular Formula The empirical formula is the lowest possible ratio. The molecular formula is the actual ratio A molecule with the empirical formula: Could have one of the following molecular formulas: NO2 NO2, N2O4, N4O8… CH2 CH2, C2H4, C4H8…

Find the molecular formula. Example 1 Find the empirical formula, if not given 2 Find the molar mass of the empirical formula Find the ratio of the molecular formula’s molar mass (must be given to you) to the empirical formula’s molar mass 3 Multiply the empirical formula’s subscripts by the ratio found in step 3. 4 Example: Empirical formula = C3H4O3. The molecular formula’s molar mass = 176.14 g/mole. Find the molecular formula.

Find the molecular formula. Example 1 Find the empirical formula, if not given 2 Find the molar mass of the empirical formula Find the ratio of the molecular formula’s molar mass (must be given to you) to the empirical formula’s molar mass 3 Multiply the empirical formula’s subscripts by the ratio found in step 3. 4 Example: Empirical formula = C3H4O3. The molecular formula’s molar mass = 176.14 g/mole. Find the molecular formula. 176.14 g/mole = 2 88.07 g/mole C 3  12.01 g/mole = 36.03 g/mole H 4  1.01 g/mole = 4.04 g/mole C3H4O3  2 O 3  16.00 g/mole = + 48.00 g/mole C6H8O6 88.07 g/mole