Mole-o-rama Chapter 3.4. Objectives Why did you have to have 602 beans in your mole? Weighing to count What is a mole?

Slides:

Advertisements

Similar presentations

Mr. Bimber Freedom High School

Advertisements

Chemistry chapter 3 Sample Problems. Isotopes The number of neutrons is found by subtracting the atomic number from the mass number. Mass # (235)---atomic.

1 By definition: 1 atom 12 C “weighs” 12 amu On this scale 1 H = amu 16 O = amu Atomic mass is the mass of an atom in atomic mass units (amu)

Mole Calculation Review. Objective/Warm-Up  SWBAT perform mole calculations. Explain the picture:

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

Topic: Counting Atoms and Formula Mass (the MOLE) Do Now: complete package page 2 Here is an example NaCl = 1 Na atom, 1 Cl atom H 2 SO 4 = 2 H atoms,

Warm Up #4 Look at Carbon on the Periodic Table. Why is Carbon’s atomic mass number and not a whole number? I am a mystery element. I have 32 protons.

Chapter 6 Chemical Composition 6.1 Counting by Weighing Bean Lab

isotope Are atoms of the same element that have different masses. Due to a different number of neutrons in the nucleus.

Moles Chapter The Mole A number of atoms, ions, or molecules that is large enough to see and handle. A mole = number of things – Just like a dozen.

THE ATOM Counting. The Atom  Objectives Explain what isotopes are Define atomic number and mass number, and describe how they apply to isotopes Given.

MOLES!!!. Atomic mass Review the mass of an atom expressed in atomic mass units is an average of the isotopes for that element listed on the periodic.

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

What is... the number of carbon atoms in 12 grams of carbon? the number of oxygen atoms in 16 grams of oxygen? the number of H 2 O molecules in 18grams.

Chemistry Chapter 11 The Mole.

Section 6.1 Atoms and Moles 1.To understand the concept of average mass 2.To learn how counting can be done by weighing 3.To understand atomic mass and.

(I have now prefaced the slides for my talk on Sept. 5 with the solution to the atomic mass problem from Sept. 3. The lecture on moles follows those slides.)

T HE M OLE Chapter 7. C ONCEPT M AP The mole Can be converted to Similar to: Dozen/ Gross/ set/ pair 6.02x10 ^23 Particles- atoms, molecules, etc. Molar.

Atomic Theory The Mole. Things that you already know Science measures a lot of things. Examples of what we measure include time, mass, temperature, volume,

Chapter 8 Chemical Composition Chemistry 101. Atomic mass unit (amu) = × g Atomic Weight Atoms are so tiny. We use a new unit of mass:

Chemical Stoichiometry: The Mole Concept Mr. Forte Atascadero High School.

How can atoms be counted? When we want to know how many atoms of a substance are in a sample of the substance that we can see, counting the atoms individually.

7.1 Notes Continued…The Mole! Key Concepts Why do chemists use the mole? How can you calculate the mass of a reactant or product in a chemical reaction?

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

Chapter 8 The Mole. 2 I say, “I have a dozen….” You say.... ✓ A dozen what? ✓ eggs, donuts, pencils, dogs, siblings....whatever. What is a dozen? ✓ 12.

CH. 3.4 Counting Atoms. ATOMIC MASS  Atoms are really small and have really small masses  Cu atoms have average mass of x kg  Special.

Solving Mole Problems 2 steps Section 3 Counting Atoms Chapter 3.

3.3 Counting Atoms. Counting Atoms Isotopes Atoms of the same element with different masses Isotopes do not differ significantly in their chemical behavior.

The Mole Continued.  The mole is also defined as the number of protons in g of protons.

Section 6.1 Atoms and Moles 1.Students will be able to describe the concept of average mass. 2.Students will be able to demonstrate how counting can be.

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

1 Warm Up Isotopes Mass of Isotope Abundance 24 Mg =24.0 amu 78.70% 25 Mg = 25.0 amu 10.13% 26 Mg = 26.0 amu 11.17% Calculate the mass average of magnesium.

ATOMIC AND MOLAR MASS. Atomic Mass 2  Considers mass numbers of all isotopes  Natural abundance  Weighted average.

Counting Atoms and Moles Chapter 3.4 us us.

1 Chemical Quantities Chapter How to measure matter? Three ways to measure matter 1. By counting 2. By mass 3. By volume.

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

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.

Average atomic mass of isotopes Calculating the average atomic mass Element “X” Natural abundance of isotope X 10% = 4 amu 30 % = 5 amu 60 % = 6 amu.

Moles and Calculating Molar Mass. The mole is the S.I. unit for the amount of a substance. A mole is the amount of a substance that contains as many particles.

Daily Objective To perform calculations using mole (mol) as a unit.

MASS and MOLES Page 57 of INB.

Chemistry 200 Fundamentals D Chemical Composition.

Unit 5 ~ The Mole (Chapter 8)

Unit 5 ~ The Mole (Chapter 8)

“The Mole” and Avogadro’s Number

Unit 5 ~ The Mole (Chapter 8)

Converting Grams To Moles and Moles To Grams

Atomic Weights The mass of an individual atom, ion, or molecule is very small. Scientists use the atomic mass unit (amu) to express the mass of atoms or.

4.5 – NOTES Moles.

The Mole Discovery Purpose: to discover the mole

Chapter 8 The Mole.

Atoms and Moles.

Chemistry 100 Chapter 6 Chemical Composition.

Avogadro’s number, the mole, molarity, molar mass

chapter 6 chemical composition

Counting Atoms Chapter 3 Section 3.

Moles are a Chemist best friend.

Molar Conversions.

Chapter 6 Chemical Composition.

Calculating Average Atomic Mass

Section 3 Counting Atoms

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 2 Atoms and Elements

Introducing the Mole A mole is a chemistry unit used like a dozen or a gross Groups large numbers of objects together For example, 3 dozen eggs is 36 (3.

THE “MOLE” A Mole (mol) is a unit of measurement used for counting very small things (atoms, molecules, etc.) A mole of something is similar to a dozen.

Presentation transcript:

Mole-o-rama Chapter 3.4

Objectives Why did you have to have 602 beans in your mole? Weighing to count What is a mole?

Count Option 1: Count 602 beans Option 2: Say you counted Option 3: Mass a bean » Multiply by 602 » Collect that mass of beans!

Even better… Beans are different… Use average value Mass 10 beans … Divide by 10 = average

More beans… 6.0 g 8.0 g 5.0 g 4.0 g 5.0 g ABCDEABCDE Average bean here is 5.6 g 602 bean B = 4800 grams 602 bean D = 2400 grams 602 average = 3400 grams

Use averages!! Periodic TableIsotope Isotope Average Atomic Mass: Average mass of all atoms of an element Found on periodic tables everywhere

What is the average? 35 Cl Cl

What is the average? 35 Cl Cl 35 Cl

What is the average? 35 Cl Cl 35 Cl

Use averages!! Periodic TableIsotope Isotope is the average atomic mass of Cl

Back to the beans… If we had a dozen beans… what would they weigh? 12 beans 5.6 g 1 bean = 67 grams

Back to the beans… If we had a dozen bean burritos*… what would they weigh? 12 burritos 440 g 1 burrito = 5280 grams *Bean burrito is not pictured due to boring-ness … this is the Baja Fresh Baja Burrito…

Molé Tasty sauce for burritos, etc.

Mole

Mole Aside from being a small rodent and fun project…

Avogadro’s Number … the Mole! The Mole is a counting number Chemist’s Dozen 6.02 x things

If we had a mole of beans… It would have the mass of 3 billion billion CVN 76’s

By the way Enough aircraft carriers (which are about 3 ½ football fields long) to reach the sun and back almost 4 BILLION times

Why do we need the mole? This paperclip is 1.18 g 23 of them have 1 mole of Al atoms 6.02 x atoms

Next time… The name is Mole. James Mole.