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.

Slides:



Advertisements
Similar presentations
Chapter 10 Chemical Quantities
Advertisements

Chapter 3 Stoichiometry
Chapter 7 Chemical Formula Relationships
Chapter 10: Chemical Quantities
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.
Mass Relationships in Chemical Reactions Chapter 3.
Section 10.1 Measuring Matter
Mole Notes.
 What is the percent composition of N and O in NO 2 ?
Chapter 8 Chemical Composition Chemistry B2A. Atomic mass unit (amu) = × g Atomic Weight Atoms are so tiny. We use a new unit of mass:
Molecular Weight and Atomic Weight Na Cl Molecular Weight or Molar Mass =
Percentage Composition
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 3b Stoichiometry.
Chapter 6 Chemical Quantities. How you measure how much?  You can measure mass, or volume, or you can count pieces.  We measure mass in grams.  We.
7.3 Using Chemical Formulas  Review  Mole: SI unit for the amount of a substance (contains avogadro’s number of particles)  Avogadro’s Number:
1 Chapter 12 Chemical Quantities. 2 How do you measure things? How do you measure things? n We measure mass in grams. n We measure volume in liters. n.
The Mole: A measurement of Matter
The Mole and Chemical Composition
The Mole and Chemical Composition
Chapter 11. Mole SI base unit for measuring the amount of substance The number of representative particles in exactly 12 grams of pure carbon-12 1 mole.
Chemical Calculations: The Mole Concept and Chemical Formulas
The Mole Objective What is a MOLE???? An amount of a substance A unit of measurement specific to chemistry mole mol n.
Unit 10 – The Mole Essential Questions:
Unit 5: The Mole.
Unit 6 Moles Conversions Formulas. Mole SI base unit for measuring the amount of substance The number of representative particles in exactly 12 grams.
Chapter 7 Chemical Quantities Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings.
Mole Concept. Counting Units  A pair refers to how many shoes?  A dozen refers to how many doughnuts or eggs?  How many pencils are in a gross?  How.
Chapter 11 The Mole A chemists best friend  Counting units in groups is common  Dozen  Case  Gross  Mole - a particular number of atoms, ions, molecules.
Chapter 7: Chemical Formulas and Chemical Compounds
Mole Jeopardy Moles and Grams Avagadro!Percent Composition Empirical Formula Molecular Formula
The Mole: A Measurement of Matter
 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.
Counting Atoms Chapter 9. MOLE?? Moles of Particles In one mole of a substance, there are 6 x particles.
Chapter 11 : Matter Notes. Mole (mol) is equal to 6.02x10 23 The mole was named in honor of Amedeo Avogadro. He determined the volume of one mole of gas.
Mole Calculations. The Mole Mole – measurement of the amount of a substance. –We know the amount of different substances in one mole of that substance.
Chapter 7 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Empirical Formula. Definition A formula that shows the simplest whole-number ratio of the atoms in a compound Ex: H 2 O Not an Ex: H 4 O 2.
Chapter 5 Chemical Quantities and Reactions 5.1 The Mole 1.
The Math of Chemistry Factor-Label Method the Mole gram formula weight Avogadro Number Scientific Notation Percent Composition Empirical Formulas Hydrates.
Empirical Formula vs. Molecular Formula Empirical formula: the formula for a compound with the smallest whole-number mole ratio of the elements Molecular.
The Mole & Chemical Quantities. The Mole Mole-the number of particles equal to the number of atoms in exactly 12.0 grams of carbon mol = 6.02 x.
Chapter 7 Chemical Quantities. The Mole  SI base unit to measure the amount of a substance  1 mole of anything = x representative particles.
12.1 Test Review. What is percent composition? the percent (by mass) of all the elements in a compound.
Topic 3 The Mathematics of Formulas and Equations
Formula (Molar) Mass Li Mn K. Formula (Molar) Mass Add atomic mass of each atom in formula Unit: g/mol Mass of one mole of a pure substance.
Chapter 8 Factor Label Method and the Mole. What is Avogadro’s Favorite Novel?
Empirical Formulas from Percents and Mass. Empirical Formula Definition: A formula that shows the simplest whole-number ratio of the atoms in a compound.
Chapter 7 Chemical Quantities or How you measure how much? You can measure mass, volume, or you can count pieces of a substance. We measure mass in grams.
Chemical Quantities: Introduction to the Mole Chapter 10.
Chapter Three Mass Relationships in Chemical Reactions.
The Mole Chemistry – Chapter 11. Measuring Matter  What measurements do we use?  Pair  Dozen  Gross  Ream  Counting Particles  Atoms and molecules.
Avogadro’s Number and Molar Conversions Mole: the SI base unit used to measure the amount of a substance whose number of particles is the same as the number.
Chapter 11 The Mole.
Chapter 7 Sec. 1 Avagadro’s # and Molar Calc.
Glencoe: Chapter 11 Sections 11.1 & 11.2
Chapter 5 Chemical Quantities and Reactions
The Mole Chapter 10.1.
Chemical Quantities.
Chapter 10 – Chemical Quantities
Molecular formulas.
Unit 6 Mole Calculations
Molar Conversions.
mole (symbolized mol) = 6.02 x particles
Chemical Composition Mole (mol) – The number equal to the number of carbon atoms in grams of carbon. Avogadro’s number – The number of atoms in exactly.
Ch. 7: Chemical Formulas and Compounds
Chapter 9 Key Terms Mole Molar Mass Avogadro's Number Percent Composition Stoichiometry Limiting Reactant Excess Reactant Actual Yield Theoretical Yield.
The Mole.
Ch. 7: Chemical Formulas and Compounds
The Mole and Mole Concepts
Presentation transcript:

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 that contains the same number of particles as the number of atoms in exactly 12 g of carbon-12

 What is Avogadro’s number? 1. the number of particles in a mole 2. 1 mole = 6.02 x particles 3. particles are: atoms, ions, molecules, formula units

How do you use these numbers? 1. 1 mole of C = 6.02 x atoms C 2. 1 mole of NaCl = 6.02 x formula units NaCl 3. 1 mole of H 2 O = 6.02 x molecules H 2 O 4. 1 mole of Ca +2 = 6.02 x ions Ca +2

What is molar mass? 1. the mass in grams of one mole of a pure substance (element or compound) 2. use the periodic table to find the mass 3. What is the molar mass of helium? 4.0 g He mole 4. will be used as a conversion factor

5. Examples: a. What is the molar mass of 1 mole of Al? 27.0 g Al mole b. What is the molar mass of 1 mole of CO 2 ? C = (1)(12.0) = 12.0 O = (2)(16.0) = g/mole

 Converting from moles to grams 1. What is the grams of 3.50 mole of Cu? 2. There are 11.9 g of Al, how many moles of Al are there?

3. How many moles are in 25.0 grams of H 3 PO 4 ?

Converting moles to molecules 1.How many molecules are in 5.2 moles of NaCl? 2.How many moles are in 3.12 x Mg +2 ions?

Convert grams to molecules. 1.How many molecules are in 3.14 grams of NaOH? 2.How many grams are in 4.12 x molecules of Rh? 3. How many molecules are in 523 g of KI?

 Percent Composition 1. Definition – the percent by mass of each element in the compound 2. Formula: % composition = mass of element 100 mass of compound

3. Ex. Find the percent composition of copper (I) sulfide. Cu 2 S Cu = 2(63.5) = S = 1(32.1) = g/mole %Cu = = 79.8% 159.1

%S =

 Empirical Formula 1.Shows the simplest whole-number ratio of the atoms in a compound 2. Examples: a.) C 2 H 8 = b.) Al 2 O 3 =

3. Examples: Analysis shows a compound to contain 26.56% K, 35.41% Cr, 38.03% O. Find the empirical formula.

 Molecular Formula 1. Indicates the ratio of the atoms 2. Indicates the actual number of atoms 3. n = Molecular mass empirical mass 4. (empirical formula) n = molecular formula

5. Examples: An organic compound is found to contains 92.25% C and 7.75% H. If the molecular mass is 78, what is the molecular formula?

Feedback: Privacy Policy Feedback
Do Not Sell My Personal Information
About project: SlidePlayer Terms of Service

© 2025 SlidePlayer.com. Inc. All rights reserved.