SL Chemistry. Friday August 28th Monday, August 31, 15
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1 SL Chemistry Friday August 28th 2015
2 Agenda Warm Up: NONE Empirical and Molecular Formula Notes E & M handout (HW) Internal Assessment - Project Guides
3 HOMEWORK Topic 1.1 Introduction to Particulate Nature of Matter & Chemical Change vocabulary DUE September 4th 2015 The Mole Concept DUE September 2nd 2015 Empirical & Molecular Formulas DUE September 4th 2015
4 Electronic Copies I have access to electronic copies of the chemistry textbook and the course companion study guide... PLEASE give me your flash drive and I will give you both copies! You are more than welcome to have both the electronic and hard copy of the textbook if you prefer though
5 Stoichiometric Relationships Introduction to the Particulate Nature of Matter and Chemical Change The Mole Concept Reacting Masses and Volumes Ms. Thompson - SL Chemistry Wooster High School
6 Topic 1.2 The Mole Concept The mole is a fixed number of particles and refers to the amount, n, of substance. Masses of atoms are compared on a scale relative to 12 C and are expressed as relative atomic mass (A r ) and relative formula/molecular mass (M r ). Molar mass (M) has the units g mol -1. The empirical formula and molecular formula of a compound give the simplest ratio and the actual number of atoms present in a molecule respectively.
7 The Mole Concept Experimental empirical and molecular formula determination Empirical describes information that is derived through observation and/or investigation. Qualitative analysis focuses on determining which elements are present in a compound. It could also verify the purity of the substance. Quantitative analysis enables chemists to determine the relative masses of elements which allows them to work out their exact composition. The molecular formula is the actual number of atoms or amount of elements in one structural unit or one mole of the compound. The empirical formula of a compound is the simplest whole-number ratio of atoms or amount (in mol) of each element present in a compound. Substance Molecular Formula Empirical Formula Hydrogen Peroxide H2O2 HO
8 Classwork Work with a partner and identify the substances molecular formula and empirical formula Substance Molecular Formula Empirical Formula ethane water butanoic acid glucose naphthalene benzene C2H6 H2O H2O2 C4H8O2 C10H8 C6H12O6
9 Classwork Work with a partner and identify the substances molecular formula and empirical formula Substance Molecular Formula Empirical Formula ethane C2H6 CH3 water H2O H2O hydrogen peroxide H2O2 HO glucose C4H8O2 C2H4O naphthalene C10H8 C5H4 benzene C6H12O6 CH2O
10 The Mole Concept Empirical Formulas When a compound s percent composition is known, its formula can be calculated. First, determine the smallest whole-number ratio of the moles of elements in the compound. This ratio gives the subscripts in the empirical formula. The empirical formula might or might not be the same as the actual molecular formula! The empirical formula = molecular formula for IONIC COMPOUNDS - ALWAYS!
11 The Mole Concept Calculating Empirical Formulas Use the following poem to remember the steps: Percent to mass Mass to moles Divide by small Multiply til whole
12 Practice Problem Methyl acetate is a solvent commonly used in some paints, inks, and adhesives. Determine the empirical formula for methyl acetate, which has the following chemical analysis: 48.64% carbon, 8.16% hydrogen, and 43.20% oxygen.
13 Step One: % to g Let s assume we have a g sample of methyl acetate. This means that each element s percent is also the number of grams of that element % C = g C 8.16% H = 8.16 g H 43.20% O = g O
14 Step Two: g to mol Convert each mass into moles using the molar mass of each element g C x 1 mol C = mol C 12.0 g C 8.16 g H x 1 mol H = 8.08 mol H 1.01 g H g O x 1 mol O = mol O 16.0 g O
15 Step Three: by small Oxygen accounts for the smallest number of moles in the formula, so divide each element by oxygen s number of moles: mol Carbon: mol / mol = = 1.5 Hydrogen: 8.08 mol / mol = 2.99 = 3 Oxygen: mol / mol = = 1 Remember, we will want whole-number ratios...
16 Step Four: x til whole In the previous slide, the ratio of C:H:O is 1.5:3:1 We need a whole-number ratio, so we can multiply everything by 2 to get rid of the 1.5 C >3, H >6, O >2 So, the final empirical formula is C3H6O2
17 The Mole Concept Calculating Molecular Formulas Sorry, no silly poem here! Step 1 Calculate the empirical formula (if needed) Step 2 GIVEN molecular mass (experimental)/empirical formula molar mass = multiplier Step 3 Multiply the empirical formula subscripts by the multiplier found in Step 2
18 Practice Problem Succinic acid is a substance produced by lichens. Chemical analysis indicates it is composed of 40.68% carbon, 5.08% hydrogen, and 52.24% oxygen and has a molar mass of g mol -1. Determine the empirical and molecular formulas for succinic acid.
19 Step One: Find Empirical Formula % C = g C x 1mol C = mol C 12.0 g C 5.08 % H = 5.08 g H x 1 mol H = 5.03 mol H 1.01 g H 54.24% O = g O x 1 mol O = mol O 16.0 g O C: H: O mol: 5.03 mol: mol mol mol mol 1 : 1.48: 1 > 1 : 1.5 : 1, multiply by 2 > C2H3O2 Round up! Obtain a WHOLE number
20 Step Two: Divide Molar Masses Molar mass empirical formula = (2 x 12.0 g/mol) + (3 x 1.01 g/mol) + (2 x 16.0 g/mol) = 59.0 g/mol Given molar mass = g/mol Multiplier = g/mol = g/mol
21 Step Three: Use Multiplier Empirical Formula = C2H3O2 x 2 from step two Molecular formula = C4H6O4
22 Determination of the Empirical Formula of Magnesium Oxide You will have a lab next Friday (September 4th) Your job is to write a thorough and complete exploration section for this lab. To achieve this you must: Research the scientific content of this topic Write and define a workable research question Adapt or design a methodology (how you will carry out your investigation) Practice academic integrity and cite any sources you use for your research Must include safety, environmental, and ethical considerations, if applicable.
23 Determination of the Empirical Formula of Magnesium Oxide You will have a lab next Friday (September 4th) Requirements: Typed, single-spaced, 12-point Times New Roman font Include cover page List and identify your variables: Independent variables - ones you manipulate or change Dependent variables - ones that respond to the change Controlled variables - ones you do not change and hold constant throughout the experiment List of materials you will use (diagrams can be helpful to explain experimental set up) Methodology - the steps necessary to complete the experiment without you having to be there to explain it. BE CLEAR, CONCISE, AND TO THE POINT.
24 HOMEWORK Topic 1.1 Introduction to Particulate Nature of Matter & Chemical Change vocabulary DUE September 4th 2015 The Mole Concept DUE September 2nd 2015 Empirical & Molecular Formulas DUE September 4th 2015
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