J OURNAL #67 What is a chemical formula? Provide an example of a chemical formula.

Slides:

Advertisements

Similar presentations

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.

Advertisements

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

Unit 7: The Mole (Chapter 10). The Mole (Ch. 10) I. Chemical Measurements (10-1) A. Atomic Mass & Formula Mass A. Atomic Mass & Formula Mass 1. The mass.

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.

7.3. Formula Mass – for any molecule, formula unit, or ion, it is the ____ of the ________ masses of all atoms represented in its formula. H 2 O for example.

Quantities in Chemistry The Relationship Between Mole and Molar Mass.

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

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.

Honors Chemistry Section 7.3. A chemical formula indicates: ◦the elements present in a compound ◦the relative number of atoms or ions of each element.

Chemical Formulas and Compounds Using Chemical Formulas.

T HE M OLE The Chemist’s Package. H OW DO WE GROUP THINGS ? Pairs, Dozen, ??? Chemists group chemicals into moles. A mole of any chemical is the same.

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.

Formula Mass and Composition of Compounds

Mathematical Chemistry

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 7 USING CHEMICAL FORMULAS Section 3.

The Mole and Chemical Composition

Wednesday, November Compound Naming Problems: Questions?

Unit 10 – The Mole Essential Questions:

Modern Chemistry Chapter 7 Chemical Formulas and Chemical Compounds

The MOLE CH 11.

Chapter 7: Chemical Formulas and Chemical Compounds

Unit 6: Chemical Quantities

The Mole and Avogadro’s Number

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu How to Use This Presentation To View the presentation as a slideshow.

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 7 Table of Contents Chapter 7 Section 3 Using Chemical Formulas.

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.

Section 7.3 – Using Chemical Formulas

Chapter 7 Preview Lesson Starter Objectives Formula Masses Molar Masses Molar Mass as a Conversion Factor Percentage Composition Section 3 Using Chemical.

F LASHBACK In your notes … answer the following question to the best of your ability: 1.) How many atoms would there be in one mole? 2.) What would be.

The mole (abbreviation: mol) is the amount of substance equal to 6.02 x particles These particles can be atoms, ions, formula units,molecules, electrons,

Moles and Molecules. Formula Mass Sum of the average atomic masses of all the atoms represented in a formula Measured in amu What is the formula mass.

The Mole. Atomic Mass Relative weight - the atomic mass unit (amu) is used to describe the mass of an atom relative to a carbon-12 isotope. 1mole of any.

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.

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.

Flashback In your notes … answer the following question to the best of your ability: 1.) How many atoms would there be in one mole? 2.) What would be the.

The chemical formula for water is H 2 O. How many atoms of hydrogen and oxygen are there in one water molecule? H2OH2O 2 hydrogen atoms 1 oxygen atom.

Chemical Calculations Mole to Mass, Mass to Moles.

Chapter 3: Calculations with Chemical Formulas and Equations MASS AND MOLES OF SUBSTANCE 3.1 MOLECULAR WEIGHT AND FORMULA WEIGHT -Molecular weight: (MW)

The Mole Intro to Stoichiometry. Measurements in Chemistry Atomic Mass: the mass of an atom of a certain element in atomic mass units (amu). 1 amu = 1.66.

The Mole Calculating -Molecular Weight -Formula Weight -Molar Mass.

Chapter 7-3: Using Chemical Formulas Coach Kelsoe Chemistry Pages

SOL R EVIEW 5 The Mole A M OLE OF P ARTICLES A M OLE OF P ARTICLES C ONTAINS 6.02 X PARTICLES = 6.02 x C atoms = 6.02 x H 2 O molecules.

Section 7.3 – Using Chemical Formulas   They allow chemists to calculate a number of characteristic values for a given compound.   Formula mass  

Mass Relationships in Chemical Reactions Chapter 3.

Using Chemical Formulas

Chapter 7 Objectives Explain the significance of a chemical formula.

MOLAR MASS CHAPTER 7-2.

Chemistry 200 Fundamentals D Chemical Composition.

Mathematics of Chemical Formulas

Formula Mass of Compounds

The Mole: A Measurement of Matter

The Mole and Avogadro’s Number

Using Chemical Formulas

Ch 7.3 Using Chemical Formulas

Chapter 7 – Chemical Formulas and Chemical Compounds

average mass of H2O molecule: amu

Chemistry 100 Chapter 6 Chemical Composition.

The Mole Unit 3.

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

2.3 الوزن الجزيئي Molecular Mass

Unit 6 Mole Calculations

Ch. 7: Chemical Formulas and Compounds

The Mole Mole: convenient measure of chemical quantities.

1 step: Mol to mass conversions

Unit 8 Stoichiometry.

Ch. 7: Chemical Formulas and Compounds

Chemical Composition.

Chemical Reactions & Reaction Stoichiometry

Presentation transcript:

J OURNAL #67 What is a chemical formula? Provide an example of a chemical formula.

T ODAY WE WILL LEARN HOW TO USE CHEMICAL FORMULAS

M OLAR M ASS R EVIEW : Give the molar mass of the following elements: 1. Na 2. C 3. O 4. Xe

C AN YOU GUESS THE MOLAR MASS OF A COMPOUND ? 1. H 2 O 2. NaCl

F ORMULA M ASSES Previously, we saw that hydrogen atoms have an average atomic mass of amu and oxygen has an average atomic mass of amu. Like individual atoms, molecules or ions have characteristic average masses Example: H2O is composed of 2 hydrogens and 1 oxygen. The average atomic mass can be calculated: 2 H atoms x = 2.02 amu 1 O atom x = amu average atomic mass of H20 = amu 1.01 amu H atom amu O atom

F ORMULA M ASS The mass of a water molecule can be referred to as a molecular mass. The mass of one NaCl formula unit, is not a molecular mass because NaCl is an ionic compound. The mass of any unit represented by a chemical formula, where the unit is a molecule, a formula unit, or an ion is known as the formula mass.

F IND THE FORMULA MASS OF THE FOLLOWING : 1. KClO 3 2. H 2 SO 4 3. Ca(NO 3 ) 2 4. PO MgCl 2

M OLAR M ASS Molar mass of a substance is qual to the mass in grams of one mole (or x 10 ^23 particles) Example: molar mass of Ca is 40.08g/mol because calcium atoms has a mass of 40.08g The molar mass of a compound is calculated by summing the masses of the elements present in a mole of the molecules or formula units that make up the compound.

M OLAR M ASS A compounds molar mass is numerically equal to its formula mass. Example: 2 H atoms x = 2.02 g H 1 O atom x = g O molar mass of H20 = g/mol 1.01 g H 1 mol H g O 1 mol O

W HAT IS THE MOLAR MASS OF THE FOLLOWING : 1. Ba(NO 3 ) 2 2. Al 2 S 3 3. NaNO 3 4. Ba(OH) 2

C ONVERSION F ACTOR Molar mass of a compound can be used as a conversion factor to relate the amount in moles to a mass in grams for a given substance. To convert a known amount of a compound in moles to a mass in grams, multiply the amount in moles by the molar mass. Example: what is the mass in grams of 2.50 mol of oxygen gas?

E XAMPLE : Ibuprofen, C13H18O2 is the active ingredient in many nonprescription pain relievers. Its molar mass is g/mol. If the tablets in a bottle contain a total of 33g of ibuprofen, how many moles of ibuprofen are in the bottle? How many molecules of ibuprofen are in the bottle? What is the total mass in grams of carbon in 33g of ibuprofen?