Chapter 10 The Mole. The atomic mass is found by checking the periodic table. The atomic mass is the number of grams of an element that is numerically.

Slides:

Advertisements

Similar presentations

Chapter 11 The Mole Section 11.1 Please have a highlighter and your periodic table out.

Advertisements

Molar Mass of Compounds

The Mole IV. CONVERTING BETWEEN PARTICLES AND MASS.

7.3. Formula Mass – for any molecule, formula unit, or ion, it is the ____ of the ________ masses of all atoms represented in its formula. H 2 O for example.

Chapter 8 Chemical Composition Chemistry B2A. Atomic mass unit (amu) = × g Atomic Weight Atoms are so tiny. We use a new unit of mass:

The Mole: A Shortcut for Chemists S-C-8-1_The Mole Presentation Source:

 Molar mass is the mass in grams of one mole of particles (atoms, ions, molecules, formula units).  Equal to the numerical value of the average atomic.

Chapter 7 Chemical Quantities

The Mole Chapter 9 What is a mole? A mole of a substance is the amount of that substance which contains 6 x particles of that substance.

Chapter 7 Lecture Basic Chemistry Fourth Edition Chapter 7 Chemical Quantities 7.2 Molar Mass Learning Goal Given the chemical formula of a substance,

Chemical Formulas and Compounds Using Chemical Formulas.

(4.3) The Mole and Molar Mass. THE MOLE IS THE SI UNIT FOR AMOUNT OF A SUBSTANCE. the mole represents 6.02 x particles. used for small particles.

The Mole Objective What is a MOLE???? An amount of a substance A unit of measurement specific to chemistry mole mol n.

1 Chapter 6 Chemical Quantities 6.2 The Mole Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings.

1 Chapter 10 Chemical Quantities 10.2 The Mole Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings.

Chapter 7: Chemical Formulas and Chemical Compounds

Chapter 7 Chemical Quantities. The Mole (Friend or foe)  What is a mole? 1. SI base unit to measure the amount of a substance 2. The amount of a substance.

Unit 6: Chemical Quantities

Chem Catalyst - What is the atomic mass of: - Cl? - Fe? - KCl? - H 2 O?

Chemistry Chapter 11 The Mole.

Conversion Factor Analysis practice Write down and answer these questions: 1)Molar Mass of C 6 H 12 O 6 = ____________ 2)How many C atoms in 1.74 mol of.

Counting Atoms Chapter 9. MOLE?? Moles of Particles In one mole of a substance, there are 6 x particles.

Chapter 7 Preview Lesson Starter Objectives Formula Masses Molar Masses Molar Mass as a Conversion Factor Percentage Composition Section 3 Using Chemical.

Moles and Molecules. Formula Mass Sum of the average atomic masses of all the atoms represented in a formula Measured in amu What is the formula mass.

Moles Notes. 1. Atomic Mass Unit amu – atomic mass unit, used to describe the mass of an atom Conversion factor: 1 amu = 1.66 x g Equivalence statement:

7.2 More Mole Conversions!!!. - Molecular Oxygen = O 2 - Atomic Oxygen = O from the periodic table 7 elements that exist as diatomic molecules (MEMORIZE)

Mole (symbolized mol) = 6.02 x particles (602,000,000,000,000,000,000,000) Avogadro’s Number (N A ) molar mass – mass (usually in grams) of one mole.

Chemical Calculations Mole to Mass, Mass to Moles.

Stoichiometry Chemical Quantities Chapter 9. What is stoichiometry? stoichiometry- method of determining the amounts of reactants needed to create a certain.

Once you know the number of particles in a mole (Avogadro’s number = 6.02 x ) and you can find the molar mass of a substance using the periodic table,

Section 3: Mass and the Mole Chapter 7: Chemical Composition.

Molar Mass, Moles, and Molecules 7.3 Using Chemical Formulas.

Tro's Introductory Chemistry, Chapter Counting Atoms or Molecules by Moles The number of atoms or molecules we will use is x and we.

It’s time to learn about.... Stoichiometry: Conversions At the conclusion of our time together, you should be able to: 1. Convert a mole of a chemical.

Unit 5A Chapter 10: Chemical Quantities Mole-Mass Relationships ABClark-Grubb.

UNIT 5A Chapter 10: Chemical Quantities Molar Mass ABClark-Grubb.

Chapter 11.  1. Describe how a mole is used in chemistry.  2. Relate a mole to common counting units.  3. Convert the number of moles to the number.

MOLAR MASS Molar mass of a substance = mass in grams of one mole of the substance. A compound’s molar mass is NUMERICALLY equal to its formula mass. Formula.

The Mole Molar Mass 1. Units you already know… 1 trio of singers= 1 pair socks= 1 dozen donuts= 1 gross of pencils= 2 3 singers 2 socks 12 donuts 144.

Chapter 7-3: Using Chemical Formulas Coach Kelsoe Chemistry Pages

MOLAR MASS CHAPTER 7-2.

MASS and MOLES Page 57 of INB.

The Mole A counting unit

Stoichiometry Review.

Chapter 7 Chemical Quantities

Formula Mass of Compounds

Using Conversions.

Unit: Chemical Quantities

average mass of H2O molecule: amu

Moles and Mass -The molar mass of a compound (aka molecular mass or molecular weight) is the sum of the atomic masses of each atom in the compound -Molar.

Section 3.1 The Mole and Molar Mass

Chemical Reactions Unit

mass of one mole of particles

Chapter 7 Chemical Quantities

Molar Conversions.

Molar Conversions (p.80-85, )

Chapter 7 Chemical Quantities

Chapter 7.3 molar mass of a compound –

mass of one mole of particles

The Mole: A Shortcut for Chemists

Molar Conversions.

1/9/18 Opener How many moles are there if you have 3.08 x 1024 particles of Ag? Please get out your weekend homework assignment, periodic table, & a calculator.

Chapter 11 Honors Chemistry Glencoe

The Mole Mole: convenient measure of chemical quantities.

UNIT 5A Chapter 10: Chemical Quantities Molar Mass

Presentation transcript:

Chapter 10 The Mole

The atomic mass is found by checking the periodic table. The atomic mass is the number of grams of an element that is numerically equal to the mass of an atomic mass unit. atomic mass of C = 12.0 g The atomic mass is the mass of one mole of atoms.

MOLAR MASS Mole – quantity such that there are as many atoms as in 12 g of carbon The mass of a mole of NaCl is the molar mass. 1 atom 1 mole C 12.0 u 12.0 g Fe 55.8 u 55.8 g Cu 63.5 u 63.5 g

MOLAR MASS 1 molecule 1 mole Cl 2 2Cl 2 X 35.5u = 71.0u 71.0 g H 2 O 2H 2 X 1.0u = 2.0u 1O 1 X 16.0u = 16.0u 18.0u 18.0 g

MOLAR MASS C 3 H u 42.0 g per mole Al 2 (SO 4 ) u g per mole

Converting grams to moles To convert first write what you are given. Then “times sign draw a line”. Place what you want above the line and the given below the line. “mol” always has a coefficient of 1. Where you see “g”, go to the periodic table to find the value.

Ex. 1: How many grams are in 6.50 moles of H 2 SO 4 ? 2H 2 X 1.0 = 2.0g 1S 1 X 32.1 = 32.1g 4 O 4 X 16.0 = 64.0g 98.1g

Ex. 2: What is the mass in grams of 5.90 mol C 8 H 18 ? 8C 8 X 12.0 = 96.0g 18H 18 X 1.0 = 18.0g 114.0g

Ex. 3: What is the number of moles in 432 g Ba(NO 3 ) 2 ? 1 Ba 1 X = 137.3g 2 N 2 X 14.0 = 28.0g 6 O 6 X 16.0 = 96.0g 261.3g