IB Topic 1: Quantitative Chemistry 1.1: The mole concept and Avogadro s number

Oct 04, 2012

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2. Pre-IB Info: Naming Compounds and Writing Formulas . Inorganic Ionic CompoundsNaming: Ionic compounds consist of a positive ion (metal or NH4 (ammonium)) and a negative ion (nonmetal or polyatomic ion). Identify the two ions and name them.CaSO4: Calcium sulfateNa2S: Sodium sulfideFe(NO3)3

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IB Topic 1: Quantitative Chemistry 1.1: The mole concept and Avogadro s number

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Mole Day!!

Mole Day!!. Make your very own mole! Use the pattern handout. Reference: www.moleday.org Write Mole Day Jeopardy questions. Categories: History of Mole Day Avogadro Mole Jokes Mole Terms Randomole!. Mole Day!. Cut Here!. Index Cards w/ Jeopardy questions: Front Back. Cut Here!.

526 views • 9 slides

The Mole Concept

The Mole Concept. Avogadro’s Number. Avogadro’s Number (symbol N ) is the number of atoms in 12.01 grams of carbon. Its numerical value is 6.02 × 10 23 . Therefore, a 12.01 g sample of carbon contains 6.02 × 10 23 carbon atoms . The Mole.

699 views • 39 slides

Chemistry 20 Mole Conversions

Chemistry 20 Mole Conversions. What is a Mole?. A term of measurement A counting number Similar to saying 1 dozen = 12 things Avogadro's Number (N A ) 6.02 x 10 23 items A VERY LARGE NUMBER!!!. = 1 mole.

829 views • 33 slides

conquer the Chemistry EOC: Balancing Equations and Stoichiometry

conquer the Chemistry EOC: Balancing Equations and Stoichiometry. Chemistry TEKS 8 (A) define and use the concept of a mole; 8 (B) use the mole concept to calculate the number of atoms, ions, or molecules in a sample of material;

897 views • 70 slides

Quantitative Chemistry

Quantitative Chemistry. Topic 1 SL + HL. 1.1 Mole concept and Avogadro’s Constant. 1 mol = Avogadro’s Constant = N A = Number of atoms in 12 gram 12 C (def.) = 6.02*10 23 units Mole = n = Amount of substance, with the unit mol.

1.11k views • 58 slides

The mole, Avogadro’s number, and Molar Mass

The mole, Avogadro’s number, and Molar Mass. The Mole. How many items are in a dozen? 12 How many “items” are in a mole? 6.022 x 10 23 molecules, atoms, or some other unit. Represents a much larger number than 12. How big is a mole?.

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Read Section 5.3 before viewing the slide show.

Read Section 5.3 before viewing the slide show. Unit 18 Avogadro’s Number and the Mole. Significance of Avogadro’s Number (5.3) Size of Avogadro’s Number (5.3) Definition of a Mole (5.3) Formula Mass (and Molecular Mass) (5.3). Introduction to Avogadro’s Number.

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Avogadro's Law

Avogadro's Law. And the combined Gas Law. Mr. Shields Regents Chemistry U05 L08. Avogadro’s Law. V/n = k (Constant T and P). Amedeo Avogadro (1776 – 1856). Related the volume of a gas to the number of molecules ( moles ) present.

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Stoichiometry

Stoichiometry. Chemistry Dr. May. Moles. One mole of anything contains Avogadro’s number of particles: One mole of sodium (Na) contains 6.02 x 10 23 atoms with a mass of 23 grams One mole of water (H 2 O) contains 6.02 x 10 23 molecules and a mass of 18 grams.

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THE MOLE

THE MOLE. What a fun concept. WHAT IS A MOLE?. A burrowing critter? A skin pigmentation? A word that evokes an enormous number? 1 mole of any substance equals 6.02 x 10 23 representative particles of that substance 6.02 x 10 23 is known as Avogadro’s number.

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Avogadro’s Number

Avogadro’s Number. 6.02x10 23. mole = (mol) 602000000000000000000000. Mole. A mole is just a number like… Pair = 2 Trio = 3 Dozen = 12 Baker’s dozen = 13 Gross = 144 Score= 20 Century=100 Ream=500. How BIG is a mole?. There are ~ 6.6 billion people on Earth

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What is . . .

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 of water?. The Mole. Avogadro’s number. 1 mole = 6.02 x 10 23 particles. How big is a Avogadro’s number?.

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Chemical Quantities

Chemical Quantities. Describe the concept of the mole and its importance to measurement in chemistry. Calculate the mass of compounds in atomic mass units. Calculate the molar mass of various substances. Additional KEY Terms Avogadro’s number. Avogadro (1776-1856)

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The Mole & Chemical Composition

The Mole & Chemical Composition. Section 1 Avogadro’s Number & Molar Conversions. For Review. Mole SI unit for amount # of atoms in 12g of carbon-12 Avogadro’s Number # of particles in a mole 6.022 x 10 23 - # of (?) in 1.000 mole Used to count any kind of particle.

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Avogadro and the Mole

Avogadro and the Mole. Amadeo Avogadro 1776-1856. Italian lawyer turned scientist Famous for proposing that equal volumes of gases held at same temperature and pressure must have the same number of gas particles (Avogadro’s Hypothesis-1811)

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The Mole

The Mole. Standards. The Mole. 1 dozen =. 12. 1 gross =. 144. 1 ream =. 500. 1 mole =. 6.02 x 10 23. There are exactly 12 grams of carbon-12 in one mole of carbon-12. Avogadro’s Number.

209 views • 10 slides

The Mole

The Mole. Objective 3.02. What is a MOLE????. An amount of a substance A unit of measurement specific to chemistry mole mol n. The Mole. “like a dozen” Specific quantity Does not change Avogadro’s Number: The # of “things” in 1 mole 6.022 x 10 23. The Mole.

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The Mole

The Mole. Chapter 6. The Mole. Remember it is a measurement for anything 1 mole means 6.022 x 10 23 of anything This is called Avogadro’s Number A sample of an element with a mass equal to that element’s average atomic mass expressed in grams contains 1 mol of atoms

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Mole

Mole. Stoichiometry. The study of quantitative relationships between the amounts of reactants used and products formed by a chemical reactions; it is based on the law of conservation of mass. Mole. The SI base unit used to measure the amount of a substance. Avogadro’s Number.

453 views • 27 slides

The Mole

The Mole. Chapter 11 Chemistry. The Mole. The mole ( mol ) is the SI unit used to measure the amount of a substance. A mole of anything contains 6.02 x10 23 particles. This number is also known as Avogadro’s number. A mole is also equal to the atomic mass of an element in grams.

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Moles and Stoichiometry

Moles and Stoichiometry. By Avery Carrico and Nick Ponturo. Moles. Mole- used to convert from atomic mass units to grams Scientists use the mole as a unit of measurement Abbreviation= mol Amedeo Avogadro discovered the mole Avogadro ’ s number= 6.02 x 10 23. Stoichiometry.

353 views • 14 slides

The Mole We use a package for atoms and molecules called a mole A mole =

The Mole We use a package for atoms and molecules called a mole A mole = a. the number of Carbon atoms in 12 g of 12 C 6.022 x 10 23 units = Avogadro’s Number The amount of an element equal to its atomic mass 1 mole of natural C atoms weighs 12.01 g and has 6.022 x 10 23 atoms

229 views • 5 slides

More Related

IB Topic 1: Quantitative Chemistry 1.1: The mole concept and Avogadro s number

IB Topic 1: Quantitative Chemistry 1.1: The mole concept and Avogadro s number

Presentation Transcript

Mole Day!!

The Mole Concept

Chemistry 20 Mole Conversions

conquer the Chemistry EOC: Balancing Equations and Stoichiometry

Quantitative Chemistry

The mole, Avogadro’s number, and Molar Mass

Read Section 5.3 before viewing the slide show.

Avogadro's Law

Stoichiometry

THE MOLE

Avogadro’s Number

What is . . .

Chemical Quantities

The Mole &amp; Chemical Composition

Avogadro and the Mole

The Mole

The Mole

The Mole

Mole

The Mole

Moles and Stoichiometry

The Mole We use a package for atoms and molecules called a mole A mole =

The Mole & Chemical Composition