Chapter 10 review.

Slides:

Advertisements

Similar presentations

Aim: How to calculate Percent Composition

Advertisements

Section Percent Composition and Chemical Formulas

1 Chapter 6 Chemical Quantities. 2 How you measure how much? How you measure how much? n You can measure mass, n or volume, n or you can count pieces.

Chemical Quantities Chapter 7 (10)

Chapter 7 – The Mole and Chemical Composition

Chemistry Notes Empirical & Molecular Formulas. Empirical Formula The empirical formula gives you the lowest, whole number ratio of elements in the compound.

Percent Composition, Empirical Formulas, Molecular Formulas.

Calculating Moles and Number of Atoms

Empirical and Molecular Formulas

APPLICATIONS OF THE MOLE

Molar Mass & Percent Composition

MOLECULAR AND EMPIRICAL FORMULA OF A HYDRATE Section: 6.2.

What is a Mole How many socks come in a pair? 2 How many eggs are in a dozen? 12 How many eggs come in a gross? 144 How many pencils come in a ream? 500.

Chapter 10: Chemical Quantities

Chemical Quantities Chapter 10:The Mole

Chapter 10 II. Formula Calculations

The Mole and Chemical Composition

The Mole Chapter 11 Chemistry RiverDell High School Ms. C. Militano

Stoichiometry Balancing Equations Molecular and Empirical Formulas Percent Composition Mole Conversions

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.

Formula Stoichiometry. What is stoichiometry? Deals with the specifics of QUANTITY in chemical formula or chemical reaction. Deals with the specifics.

Mole Jeopardy Moles and Grams Avagadro!Percent Composition Empirical Formula Molecular Formula

The Mole and Avogadro’s Number

Chemical Formulas and Moles. Example: 1.water (C) – every molecule of water contains 2 atoms of hydrogen & one atom of oxygen - 2 molecules of H 2 O would.

 Dalton used the percentages of elements in compounds and the chemical formulas to deduce the relative masses of atoms  Unit is the amu(atomic mass.

Percent Composition Empirical & Molecular Formulas.

Molecular Formula Represents the actual number of atoms of each element in compound – Not necessary for ionic compounds – Necessary for covalent compounds.

Atoms and Molecules Formula Unit Mass The formula unit mass of a substance is a sum of the atomic masses of all atoms in a formula unit of a compound.

Review for chapter 8 Problem-solving practice. Calculating masses 1) Calculate the molecular mass of pentane 2) Calculate the formula mass of calcium.

THE MOLE Chapter 10: Chemical Quantities Measuring Matter What is a mole? It is the SI unit that measures the amount of substance.

Percent Composition and Molecular Formulas.  Determining the percent composition of each element in a compound  H 2 O 1. Find the molar mass of the.

MOL Concept Warmups. 1. The gram-formula mass of a compound is 48 grams. The mass of 1.0 mole of this compound is – A. 1.0 g B. 4.8 g C. 48 g D. 480 g.

The Formula for a Hydrate Objectives: 6.0 Solve stoichiometric problems involving relationships among the number of particles, moles, and masses of reactants.

IIIIII Formula Calculations The Mole. A. Percentage Composition n the percentage by mass of each element in a compound.

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.

Chapter 7 “Chemical Formulas and Chemical Compounds” Yes, you will need a calculator for this chapter!

Aim: How to calculate Percent Composition  DO NOW: 1. What is the number of moles of potassium chloride present in 148 g? 2. What is the molar mass of.

Calculating Empirical and Molecular Formulas. Calculating empirical formula A compound contains 79.80% carbon and 20.20% hydrogen. What is the empirical.

USING MOLAR CONVERSIONS TO DETERMINE EMPIRICAL AND MOLECULAR FORMULAS.

NOTES: Quantifying Chemical Compounds Chapter 11.

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

Calculating Empirical Formulas

Percent Composition Molar Mass Molar Conversions Empirical Formulas Random

C. Johannesson Ch. 11 – The Mole Molar Conversions & Calculations.

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.

Students type their answers here

Empirical Formulae The empirical formula of a compound is the simplest ratio of the different atoms in it. For example, for ethane (C2H6)it is CH3. You.

ATOMIC MASS – The mass of an individual atom ATOMIC MASS UNIT (amu or u) – One twelfth the mass of a carbon-12 atom, equal to 1.66 x g Atomic masses.

Formulas and the Mole.

Chapter 7 “Chemical Formulas and Chemical Compounds”

Jeopardy Empirical Formulas Molecular Formulas Nomenclature Hydrates

The Mole and Avogadro’s Number

Section 9.3—Analysis of a Chemical Formula

Aim: How to calculate Percent Composition

Molar Conversions & Calculations

Mole problems with compounds

Section 9.3—Analysis of a Chemical Formula

Percent Composition, Empirical Formulas, and Molecular Formulas

Bell Work 1 / Mole Map 1. Draw the Mole Map and include the relationships that exist between each section.

Bell Work 1 / Mole Map 1. Draw the Mole Map and include the relationships that exist between each section.

Empirical and Molecular Formulas

What is the mass of 1 mole of Uranium?

Review Game MOLES MOLES MOLES.

Chapter 10: Chemical Quantities

Introduction to the Mole and Math Concepts

Empirical and Molecular Formulas

Warm Ups- The Mole January 10-January 20.

Chapter 7- Sec. 3 and 4 “Chemical Formulas and Chemical Compounds”

Presentation transcript:

Chapter 10 review

Define the following: Hydrate Molecular formula Empirical formula Percent composition Mole

Find the atomic mass for the following atoms: 11. Cl 12. O 13. Fe

Find the molar mass for the following compounds: 14. CH2O 15. CaSO4 16. Na3PO4

Identify if the following problems are 1 or 2 steps 17. How many atoms are in 0.750 moles of zinc? 18. How many moles of magnesium is 3.01 x 1022 atoms of magnesium? 19. How many atoms of nitrogen are in 1.2 grams of aspartame 20. Find the number of moles of argon in 452 g of argon 21. Find the mass of 1.00 x 1023 molecules of N2 22. What is the mass of 5 moles of Fe2O3

Solve the following molar conversions: 23. How many atoms are in 0.750 moles of zinc? 24. How many moles of magnesium is 3.01 x 1022 atoms of magnesium? 25. Find the mass of 1.00 x 1023 molecules of N2

Solve the following percent composition problems for Nitrogen: 26. Mg(NO3)2 27. (NH4)2S

Solve the following empirical formula problem: What’s the empirical formula of a molecule containing 65.5% carbon, 5.5% hydrogen, and 29.0% oxygen. Element Percent Composition C 65.5% H 5.5% O 29.0%

Solve the following molecular formula problem: A compound with an empirical formula of C2H8N and a molar mass of 46 grams per mole. Find the molecular formula.

Determine the empirical formula for the compound whose percent composition.

Which samples have the same empirical formula? Which substances have the same empirical formula? Which samples have the same empirical formula? Sample Formula 1 CH3OH 2 CH2O 3 C6H12O6 4 C2H4O2

A hydrate of calcium chloride has a mass of 8. 52 g A hydrate of calcium chloride has a mass of 8.52 g. This sample is heated until no water remains. The CaCl2 anhydrate has a mass of 5.60g. How many water molecules were attached to calcium chloride?