'Whole number ratio' diaporamas de présentation

Chemical Equations and Stoichiometry

3. Chemical Equations and Stoichiometry. 3.1 Formulae of Compounds 3.2 Derivation of Empirical Formulae 3.3 Derivation of Molecular Formulae 3.4 Chemical Equations 3.5 Calculations Based on Chemical Equations 3.6 Simple Titrations. Stoichiometry ( ????? )p.19.

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Chapter 6 Chemical Names and Formulas

Chapter 6 Chemical Names and Formulas. Milbank High School. Section 6.1 Introduction to Chemical Bonding. OBJECTIVES: Distinguish between ionic and molecular compounds. Section 6.1 Introduction to Chemical Bonding. OBJECTIVES: Define cation and anion, and relate them to metal and nonmetal.

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Nomenclature Chemical Formulas Reactions

Nomenclature Chemical Formulas Reactions. Which is an example of a synthesis reaction?. A. HCl + KOH ? KCl + H 2 O B. Pb(NO 3 ) 2 + 2HBr ? PbBr 2 + 2HNO 3 C. C + O 2 ? CO 2 D. Mg + H 2 SO 4 ? MgSO 4 + H 2.

1.83k views • 79 slides

Nomenclature Chemical Formulas Reactions

Nomenclature Chemical Formulas Reactions. Which is an example of a synthesis reaction?. A. HCl + KOH ? KCl + H 2 O B. Pb(NO 3 ) 2 + 2HBr ? PbBr 2 + 2HNO 3 C. C + O 2 ? CO 2 D. Mg + H 2 SO 4 ? MgSO 4 + H 2.

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The Mole

1.19k views • 62 slides

Chapter 11

Chapter 11. Chemical Quantities Chemistry Tracy Bonza Sequoyah High School. How do you measure how much?. You can measure mass, or volume, or you can count pieces. We measure mass in grams. We measure volume in liters. We count pieces in MOLES. Moles.

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A: 16 Nov. 2010

A: 16 Nov. 2010. Objective: SWBAT calculate percent composition for a compound and determine the percentage of water in a hydrate using laboratory techniques Do now : Calculate the molar mass of calcium chloride. (Hint: Write the correct formula first!). Agenda. Do now

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Chapter 6

528 views • 39 slides

The Mole

481 views • 37 slides

Ionic Bonds

Ionic Bonds. Chemistry Mrs. Coyle. Part A:. Ions Lewis Dot Structure Stable Octet (or Duet). The Periodic Table and Atomic Radius. Valence Electrons. Valence electrons are the electrons in the highest occupied energy level of the atom.

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Chapter 11

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Meet the Mole.

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Chapter 10 Chemical Quantities

Chapter 10 Chemical Quantities. Measuring Matter. How much? How many? Chemistry is a quantitative science. How do you measure matter? You can measure the amount of something by count, by mass and by volume. Some units used for measuring indicate a specific number of items. (a pair, a dozen)

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Empirical Formula

Empirical Formula. From percentage to formula. The Empirical Formula. The lowest whole number ratio of elements in a compound. The molecular formula the actual ratio of elements in a compound The two can be the same. CH 2 empirical formula C 2 H 4 molecular formula

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Formulas and equations

Formulas and equations. Chemical symbols represent Chemical elements. Two or more Chemical symbols combined represent a Chemical compound. Chemical symbols when added and yield new arrangements chemical symbols represent chemical equations ( reactions ). Reference Tables.

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Law of Definite Composition and Law of Multiple Proportions

Law of Definite Composition and Law of Multiple Proportions. Chemistry Mrs. Coyle. Joseph Proust (France 1799). Law of Definite Proportions: A given compound always contains elements in a certain proportion by mass. (Constant composition).

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Chemical Equations

Chemical Equations. Parts of an equation and how to balance. Chemical Equation:. Set of directions for a chemical reaction. The directions tell us: What materials to use How much you need Amount of product you will get. Chemical Equations *. Give info about:

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E mpirical F ormulas

E mpirical F ormulas. The empirical formula of a chemical compound is the simplest whole number ratio of atoms of each element present in a compound.

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MOLECULAR FORMULAS

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