Section 10.1: The Mole (A Measurement of Matter) What is a Mole? A mole is a specific amount of particles. Atoms are very, very, very small. The fact that.

Slides:

Advertisements

Similar presentations

Counting units such as dozen or gross are commonly used to deal with large quantities of items. No matter what we are counting, a dozen means 12, whether.

Advertisements

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 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.

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

What is the molar mass of Calcium Chloride (CaCl2) (to the nearest tenth!)? 111.1g/mol.

What’s up with the Mole?. How do we measure matter? By weight: We buy bananas by the _______________. By volume: Milk is sold by the ____________________.

Quantities in Chemistry The Relationship Between Mole and Molar Mass.

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

I can calculate the molar mass of a compound Sometimes the molar mass is called the formula mass!

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.

Chapter 10 Chemical Quantities. A representative particle (RP) refers to the species present in a substance, usually atoms(S), molecules(SO 2 ), or formula.

IIIIIIIV The Mole I. Molar Conversions A. What is the Mole? n A counting unit n Similar to a dozen, except instead of 12, it’s 602 billion trillion 602,000,000,000,000,000,000,000.

Warm-Up Calculate Molar Mass K2O PCl5 LiF.

Regents Chemistry. What’s a Mole??? One mole of donuts contains x donuts One mole of H 2 O contains x molecules One mole of.

Unit 12 Mass and Moles.

The Mole Theory Molar Mass. Mass of a Mole o Molar Mass- the mass of a mole of any element or compound (in grams) o Also called: o Formula mass – sum.

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

Chapter 7: Chemical Formulas and Chemical Compounds

Chemical Quantities The Mole: A Measurement of Matter

The Mole and Avogadro’s Number

Molar Mass and Molar Conversions Chapter 3 part III.

Chemical Quantities Avogadro’s Number.

IIIIIIIV The Mole I. Molar Conversions A. What is the Mole? n A counting unit n Similar to a dozen, except instead of 12, it’s 602 billion trillion 602,000,000,000,000,000,000,000.

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

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:

The Mole Unit 5. Formula Mass Formula mass - also called: formula massmolecular mass molecular massformula weight formula weightmolecular weight molecular.

Quantities in Chemistry The Mole and Molar Mass. Mole Review A Mole is a unit of measurement in chemistry. It represents 6.02 x of an entity. One.

1 The Mole 6.02 X What is “The Mole??” A counting unit (similar to a dozen) 6.02 X (in scientific notation) = 602 billion trillion = 602,000,000,000,000,000,000,000.

10.1 THE MOLE Q4TP – CHEM MATT T.. THE MOLE: A MEASUREMENT OF MATTER What are three methods for measuring the amount of something? How is Avogadro’s number.

The Mole Mole Calculations. Molar Mass mass of one mole of a substance units: grams/mole equal to the ATOMIC MASS of the element, rounded to two numbers.

Moles COUNTING BY WEIGHING. Moles (is abbreviated: mol)  It is an amount, defined as the number of carbon atoms in exactly 12 grams of carbon-12.  1.

RR: How many ways can you count to 100?. Do you know how to count? In chemistry, the unit that helps us count is the mole (mol). The mole represents

Chemical quantities Chapter Ways to measure matter Length/width/height Volume Density Surface Area Etc.

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

The Mole Chemistry’s Unit of Convenience. Calling particles by the right name Particles of a type of a(n)… are called…  ion……………………  element………………..

The Mole  Just to clear up any misconceptions when we use the term “mole” we are not referring to this small blind fellow.

What is a Mole? A mole is a specific amount of atoms. Atoms are very, very, very small. The fact that atoms are so small makes it hard to take measurements.

Mole GRAM FORMULA MASS MOLES TO GRAMS AND GRAMS TO MOLES.

Chapter 10 “Chemical Quantities” Pequannock Township High School Chemistry Mrs. Munoz.

Stoichiometry and the Mole (Part 2) Converting—Particles and Grams.

WHAT IS A MOLE? SI unit for Amount of Substance A mole is a unit like “dozen” or “pair” or “gross”. It doesn’t represent a measured number, but a counted.

RR: How many ways can you count to 100?. Do you know how to count? In chemistry, the unit that helps us count is the mole (mol). The mole represents

Stoichiometry and the Mole (Part 1) Formula Mass and Molar Mass.

1 The Mole 6.02 X X STOICHIOMETRYSTOICHIOMETRY - the study of the quantitative aspects of chemical reactions.

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

Stoichiometry Review.

Molar Mass (M) Topic 1.2.

Warm-up March 16th What is the molar mass of: KCl CuSO4.

Atomic Mass is the Mass of One Mole of an Element

The Mole and Avogadro’s Number

Using Conversions.

Unit 7: The Mole.

10.1 Chemical Measurement.

Chapter 10 – Chemical Quantities

Molar Conversions (p.80-85, )

Molar Conversions (p.80-85, )

The Mole "Not everything that counts can be counted, and not everything that can be counted counts." Albert Einstein.

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

(moles of solute per liter of solution)

The Mole: A Shortcut for Chemists

Problem Solving.

Chapter 11 Honors Chemistry Glencoe

The Mole "Not everything that counts can be counted, and not everything that can be counted counts." Albert Einstein.

The Mole Molar Conversions.

Chemical Composition.

Moles practice Q’s Ch 10 Pearson.

Presentation transcript:

Section 10.1: The Mole (A Measurement of Matter) What is a Mole? A mole is a specific amount of particles. Atoms are very, very, very small. The fact that atoms are so small makes it hard to take measurements (such as mass, volume, density, etc.) of just one atom. So, instead of measuring individual atoms, we will group atoms into what we call a MOLE. 1 Mole = 602 billion trillion atoms or (6.02 x atoms) Avogadro’s Number It’s the same as saying: 1 mile = 5,280 feet 1 cup = 8 ounces 1 foot = 12 inches

Section 10.1: The Mole (A Measurement of Matter) What is a Mole? Moles don’t always have to be referring to atoms. They can also be referring to molecules, compounds, ions, or other particles. Just remember, 1 mole of anything is equal to 6.02 x Question: What number of chloride ions are present if there are 2 moles of chloride ions? 1 mole = 6.02 x ions 2 moles of chloride ions x 6.02 x chloride ions = x chloride ions 1 mole of chloride ions

Section 10.1: The Mole (A Measurement of Matter) Molar Mass vs. Formular Mass Formula Mass The mass of one compound of Na 2 O Molar Mass The mass of one mole of Na 2 O Na: 23 amu (atomic mass units) O: 16 amu 2 Na = 2 (23 amu) = 46 amu 1 O = 1 (16 amu) = +16 amu 62 amu Note: 1amu = 1.66 x grams 1 mole of Na: 23 grams 1 mole of O: 16 grams 2 moles of Na = 2 (23 g) = 46 grams 1 mole of O = 1 (16 g) = 16 grams 62 grams *We can use our measuring equipment to achieve this value.

Section 10.1: The Mole (A Measurement of Matter) Molar Mass vs. Formular Mass So, we realize now that when the atomic mass of an element is reported in AMU’s it is referring to 1 atom of that element. If the mass is reported in grams it is referring to 1mole of atoms of that element. 4 Be grams is the mass of 1 mole of Be atoms.

Section 10.1: The Mole (A Measurement of Matter) Molar Mass Determine the molar mass of Copper (II) Chloride. Step 1: Write the compound formula. Step 2: Using the periodic table, write down the molar mass of each element in the compound. (Round the mass to the nearest tenth) Step 3: Add together the molar masses of each element. CuCl g35.5 gX 2 = 71 g 63.5 g + 71 g = grams

Section 10.2: Molar Road and Unit Conversions Mole Conversion Chart

Section 10.2: Molar Road and Unit Conversions Mole Conversion Chart Particle – Mole Relationship How many atoms of oxygen are in this room if this room contains 0.5 moles of oxygen atoms? Answer:.5 moles O x 6.02 x atoms of O = 3.01 x atoms 1 mole of O

Section 10.2: Molar Road and Unit Conversions Mass – Mole Relationship Determine the mass of 5.5 moles of Potassium Carbonate. K 2 CO 3 (39.1gX 2)12.0g(16.0g X 3) + = g X 138.2g K 2 CO moles K 2 CO 3 1 mole K 2 CO 3 = grams K 2 CO 3

Section 10.2: Molar Road and Unit Conversions Mass – Particle Relationship Example: Determine the number of molecules of carbon monoxide in 75.0 grams of carbon monoxide. 75.0g CO x 1 mole CO 28.0 grams CO = 2.7 moles COX 6.02 x molecules 1 mole CO = 1.6 x molecules CO CO 12.0 g16.0g+= 28.0g

Section 10.2: Molar Road and Unit Conversions Mole – Volume Relationship Example: Determine the number of molecules of carbon monoxide in 75.0 liters of carbon monoxide at STP. 75.0L CO x 1 mole CO 22.4 liters CO = 3.5 moles COX 6.02 x molecules 1 mole CO = 2.1 x molecules CO