7.3 Using Chemical Formulas  Review  Mole: SI unit for the amount of a substance (contains avogadro’s number of particles)  Avogadro’s Number: 6.022.

Slides:

Advertisements

Similar presentations

Chapter 10: Chemical Quantities

Advertisements

7.3 USING CHEMICAL FORMULAS APRIL 27, USING CHEMICAL FORMULAS Formula Masses: Sum of all the average atomic masses of all atoms represented.

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)

Mass Relationships in Chemical Reactions Chapter 3.

 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:

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

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.

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 7: Chemical Formulas and Chemical Compounds

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.

The Mole Ch.8. (8-1) Mole (mol): amt. of substance – # of atoms in 12g of carbon-12 Avogadro’s constant: 6.02 x particles / mol –Atoms, molecules.

Chemical Quantities The Mole: A Measurement of Matter

The Mole: A Measurement of Matter

The Mole and Avogadro’s Number

Chapter 10 The Mole. Chemical Measurements Atomic Mass Units (amu) – The mass of 1 atom – 1 oxygen atom has a mass of 16 amu Formula Mass (amu or fu)

THE MOLE 10/1/14 – CHAPTER 3. RELATIVE MASS VS AVERAGE ATOMIC MASS RM = the standard - atomic mass of carbon-12 is used - 1 amu = 1/12 mass of 1 carbon-12.

Using Molar Mass as a Conversion Factor.  A molar mass is the mass in grams of one mole of a substance.  One mole of any substance contains Avogadro’s.

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.

Wake-up 1.Study Polyatomic Ions for about 5/10 minutes. Write NO WAKE-UP on Friday.

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.

Stoichiometry The mathematics of Chemistry. What is Stoichiometry? The proportional relationship between two or more substances during a chemical reaction.

Mole (symbolized mol) = 6.02 x particles (602,000,000,000,000,000,000,000) Avogadro’s Number (N A ) molar mass – mass (usually in grams) of one mole.

CHEMICAL COMPOUNDS AND THE MOLE Chapter 7. Formula Mass  Mass of H 2 O?  Formula Mass: mass of molecule, formula unit, or ion is sum of masses of all.

Chemical Calculations Mole to Mass, Mass to Moles.

Topic 3 The Mathematics of Formulas and Equations

The Mole How We Count Atoms and Other Fundamental Particles.

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.

Mole Calculations I.Molar Mass II. Percent Composition III. Converting Mass to Moles IV. Converting Moles to Mass.

Section 3: Mass and the Mole Chapter 7: Chemical Composition.

Relating Mass to Numbers of Atoms The MOLE. Is the SI unit for amount of a substance Abbreviated as mol Amount of a substance that contains as many atoms.

The Mole. What is the a mole? A unit to measure the amount of a substance. Commonly abbreviated mol. The symbol is n.

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

Avogadro’s and the Mole. Moles a mole is the number of carbon atoms in exactly 12g of carbon. a mole is a unit of measurement, just like grams…

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.

Mass Relationships in Chemical Reactions Chapter 3.

Bell Ringer How many moles of Nitric acid are there in 250 g?

Ch 7 Mole & chemical composition

Chemistry The Mole: MAC NOTES:

Glencoe: Chapter 11 Sections 11.1 & 11.2

The Mole: A Measurement of Matter

The Mole and Avogadro’s Number

How many ions are in a mole of chloride, Cl- ?

Chapter 7 – Chemical Formulas and Chemical Compounds

III. Formula Calculations

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

Molecular formulas.

Molar Conversions.

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

10.1 What is a Mole? A mole of any substance contains Avogadro’s number of representative particles, or 6.02  1023 representative particles. The term.

Chapter 6 Chemical Composition.

The Mole Concept.

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.

Molar Conversions.

Ch. 7: Chemical Formulas and Compounds

The Mole the mole is the SI unit representing atomic amounts.

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

Ch. 7: Chemical Formulas and Compounds

The Mole Chapter 7-1.

Chapter 11 The Mole.

Chemical Composition.

Moles practice Q’s Ch 10 Pearson.

Molecular Formula.

Presentation transcript:

7.3 Using Chemical Formulas  Review  Mole: SI unit for the amount of a substance (contains avogadro’s number of particles)  Avogadro’s Number: x particles/molecules/formulas units per 1 mol  Formula Unit: smallest ratio of cations to anions

2) Formula Mass  Sum of the average atomic masses of all atoms represented in a formula (Units: amu)  Ex: What is the formula mass of Ca(NO 3 ) 2 ?

3) Molar Mass  mass of one mole of any substance (contains avogadro’s number of particles) Units: g/mol  Ex: calculate the molar mass of Al 2 S 3

4) Problem Solving Using Molar Mass  A) Mol to mass  Ex: What is the mass (grams) of 3.0 mol of NaOH?  1. determine molar mass of NaOH  2. # of moles of NaOH x molar mass

 B) mass to mol  How many moles are in 135 g of NaOH?  1. determine molar mass of NaOH  2. grams of NaOH / molar mass

 C) Moles to molecules / molecules to moles  How many molecules of H 2 0 are present in 1.5 mol?  1. mol NaOH x Avogadro’s #

6. Determining % Composition  A) from chemical formula  Ex – Find the % composition of copper (II) sulfate?  Formula -> molar mass -> mass of each element as %  (disregard letter 6.B)

6) Determing % Composition  B) from mass data