A Mole is an Unit.

Slides:

Advertisements

Similar presentations

Chapter 10 Chemical Quantities

Advertisements

THE MOLE... a unit of counting. Review How many oxygen atoms in the following? CaCO 3 Al 2 (SO 4 ) 3 How many ions in the following? CaCl 2 NaOH Al 2.

NOTES: Molar Volume, Density; and the Mole “Road Map”; NOTES: 10.3 Percent Composition.

Aim: How to convert from moles to volume and vice versa

Chapter 10: Chemical Quantities

1 Section 3.3 The Mole: A Measurement of Matter n OBJECTIVES: –Describe how Avogadro’s number is related to a mole of any substance.

1 Chapter 8 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.

The Mole – A measurement of matter

Unit 06 The Mole Theory Ch. 4 and 7.

The Mole–Mass Relationship How do you convert the mass of a substance to the number of moles of the substance? 10.2.

Molar & atomic Mass Mole  > particles Mass  > Mole Molar Volume of Gas Gas Density

The Mole Concept Chapter 9 CHM 130 GCC.

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.

Mole-Mass & Mole-Volume Relationships

Mole-Mass and Mole-Volume Relationships

Mole-Mass and Mole-Volume Relationships

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.

Section 7.1 The Mole: A Measurement of Matter

Chemical Quantities and The Mole

Unit 06 The Mole Theory Ch. 4 and 7. Dimensional Analysis ● just converting one thing to another Problem 1 : How many seconds are in a day? sec day What.

Unit 5: The Mole and Stoichiometry

MOLAR MASS What is molar mass? How do you calculate molar mass?

Unit 12 Mass and Moles.

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

Unit 2 Lesson #5 Avogadro’s Number & The Mole (p.14-16)

AP Notes Chapter 7 Mole Representative Particles Molecular Mass (mm) - gam used for atoms - gmm used for molecules - gfm used for formula units MoleVolume.

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

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

Mathematics of Chemical Formulas Chapter 8 P

The Mole The Basic Chemical Unit. A Mole is : A chemical quantity A Mole of any substance is Chemically equivalent to a mole of any other substance.

1 The Mole. 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. n We measure mass in.

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

1 Chapter 8 Chemical Composition 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 Calculations Mole to Mass, Mass to Moles.

1. 2 Chemical Quantities or 3 How you measure how much? How you measure how much? n You can measure mass, n or volume, n or you can count pieces. n We.

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.

The Mole Theory. Dimensional Analysis A way to solve problems by converting or using the units of the items involved Converting one thing to the another.

The Mole 6.02 X The Mole 1 pair = 2 representative particles1 pair = 2 representative particles 1 dozen = 12 representative particles1 dozen =

UNIT 6: CHEMICAL QUANTITIES Chapter 10: Mole and Volume Relationships.

Miss Fogg Spring 2016  A particle can refer to an individual atom OR a type of molecule ◦ Jellybean ◦ Baseball ◦ Carbon atoms ◦ Hydrogen atoms ◦ Water.

Objective: To reintroduce the mole and introduce two mole conversions Do Now: Solve each proportion = x2. 10 = x.

Chapter 7 Moles. What is a Representative Particle The smallest unit into which a substance can be broken down without changing the composition of the.

10.2 Mole-Mass and Mole- Volume Relationships 1 > Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.. Chapter 10 Chemical Quantities.

The Mole Introduction to Chemistry. The Mole Atoms and molecules are too small to count out individually Avogadro’s Number = 6.02 x particles /

What is a mole? A mole is a number. It is x This number is also called Avogadro’s number. How many atoms in 1 mole of copper atoms?

Chapter 10 The Mole. Chapter 10 The Mole Dimensional Analysis Write the equivalence statement needed. 2. Find the appropriate conversion factor. 3.

CHEMICAL QUANTITIES OR

Chemical Quantities Chapter 10.

Chapter 10 Chemical Quantities

Atomic Mass is the Mass of One Mole of an Element

Molar Mass and Molar Volume

The Basic Chemical Unit

Unit 3: Moles!!!.

Chapter 10 Chemical Quantities

CELEBRITY CHEMIST of THE DAY

Mole-Mass and Mole-Volume Relationships

Avogadro’s Number: 1 mole = 6.02 x 1023 particles

Chapter 19 Avogadro’s Principle.

Chapter 10 Chemical Quantities

Chapter 10 Chemical Quantities

Moles and Gas Volume (3.4) Avogadro’s Hypothesis: equal volumes of different gases at the same temperature and pressure contain the same number of particles.

Practice: Determine the molar mass for the following:

Counting Atoms How many atoms are in: NaCl? H2O? MgSO4? Pb(SO4)2?

10.2 Molar Relationships.

Two Relationships 1 mole = molar mass in grams of any element or compound (use periodic table) 1 mole = x 1023 particles (molecules, atoms, formula.

C2H6 CH3 B. Empirical Formula

The Mole Molar Conversions.

Presentation transcript:

A Mole is an Unit

Representative Particles Type of Substance Description R.P. ( UNIT) Element 1 symbol ATOM Covalent Molecule 2 or more NM MOLECULE Ionic Compound Cation-Anion M -NM FORMULA UNIT

Caribbean Monkeys Eat Avocados In Forest Caribbean = Covalent Monkeys = Molecules

Caribbean Monkeys Eat Avocados In Forest Eat = Element Avocados = Atoms

Caribbean Monkeys Eat Avocados In Forest In = Ionic Forest = Formula Unit

or 1 mole = 6.02 x 1023 molecule 1 mole = 6.02 x 1023 formula unit 1 mole = 6.02 x 1023 atom or 1 mole = 6.02 x 1023 molecule 1 mole = 6.02 x 1023 formula unit

Determine the type of Representative Particle 1. Mg 2. C3H8 3.NaCl 4. CBr4 5. Li 6. K2O 7. Cl2 8. H2O

Using Representative Particles Example Problems Using Representative Particles

How many moles of magnesium is 1.25 x 1023 atoms? Given Info: Conversions: Work: Looking for? Answer:

How many molecules are in 2.12 mole of propane-C3H8 ? Given Info: Conversions: Work: Looking for? Answer:

How many molecules are in 2.12 mole of propane-C3H8 ? Given Info: 2.12 mole C3H8 Conversions: 1 mole = 6.02x1023 molecule Work: 2.12 mole 6.02 x 1023 molecule C3H8 C3H8 1 mole C3H8 Looking for? molecules C3H8 Answer: 1.28 x 1024 molecule C3H8

Example Problems Using Molar Mass

How many grams are in 2 moles of calcium hydroxide? Given Info: Conversions: Work: Looking for? Answer:

How many molecules are in 4.42 x 106g of water molecules? Given Info: Conversions: Work: Looking for? Answer

How many molecules are in 4.42 x 106g of water molecules? Given Info: 4.42 x 106g Conversions: MM = 18.02g H2O 1 mole 1mole = 6.02x1023 molecule Work: 4.42x106g 1 mole 6.02x1023 molecules H2O H2O H2O 18.02 g 1 mole H2O H2O Looking for? molecules Answer: 1.48 x 1029 molecules

Example Problems Using Molar Volume

Molar Volume @ STP only Standard Temperature and Pressure: STP Standard Temperature: 273K Standard Pressure: 1 atmosphere (atm) At these 2 conditions: Molar Volume 1 mole = 22.4L

How many liters are 2.78 x 1031 molecules? Given Info: Conversions: Work: Looking for? Answer: How many liters are 2.78 x 1031 molecules?

How many liters are 2.78 x 1031 molecules? Given Info: 2.78 x 1031 molecules Conversions: 1 mole =6.02x1023 molecules Work: 2.78 x1031 molecules 1 mole 22.4L 6.02 x 1023 1 mole molecules Looking for? liters Answer: 1.03 x 109 L How many liters are 2.78 x 1031 molecules?

The density of a gaseous compound containing carbon and oxygen is 1 The density of a gaseous compound containing carbon and oxygen is 1.964 g/L @ STP. Determine the molar mass of the compound. Given Info: Conversions: Work: Looking for? Answer: