Chemistry I Unit IV Objectives Chapter 10

Slides:



Advertisements
Similar presentations
Chapter 12 “Stoichiometry” Chemistry Tutorial Stoichiometry Mr. Mole.
Advertisements

STOICHIOMETRY Study of the amount of substances consumed and produced in a chemical reaction.
Balancing Chemical Equations and Stoichiometry
Chemistry 101 Chapter 9 Chemical Quantities.
Chapter 3.  Reactants are left of the arrow  Products are right of the arrow  The symbol  is placed above the arrow to indicate that the rxn is being.
 CHEM.B Apply the mole concept to representative particles (e.g., counting, determining mass of atoms, ions, molecules, and/or formula units). 
Section 9.1 Using Chemical Equations 1.To understand the information given in a balanced equation 2.To use a balanced equation to determine relationships.
CHAPTER 3 AP CHEMISTRY. AMU Atomic masses come from the carbon-12 scale Mass of carbon-12 is exactly 12 amu Nitrogen-14 has an amu of this is.
1 mole = particles : Avogadro’s number Particles = molecules Molar mass of each element can be found on the periodic table. The unit is in grams/mol or.
Chapter 12 Stoichiometry
Chapter 9 Chemical Quantities Chemistry B2A Formula and Molecule Ionic & covalent compounds  Formulaformula of NaCl Covalent compounds  Molecule molecule.
“Stoichiometry” Original slides by Stephen L. Cotton Mr. Mole.
Chemistry Fall Chemical Reactions A chemical reaction is a process in which one or more substances are converted into new substances with different.
Chapter 3 - Stoichiometry It is important to be able to quantify the amount of reagent(s) that will be needed to produce a given amount of product(s).
Chapter 3. Atomic Mass  amu = Average Atomic Mass Unit  Based on 12 C as the standard.  12 C = exactly 12 amu  The average atomic mass (weight) of.
Chemical Quantities and Moles
1 Chapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations.
CHAP 3 Stoichiometry. Key terms Atomic mass – average mass of the atoms of an element. (aka average atomic mass) based on the standard mass of Carbon-12.
Stoichiometry Chapters 7 and 9.
Chemistry Chapter 10 Formula Based Calculations. a mole is 6.02 x particles like a dozen is 12 particles it is a large number, because we are counting.
Reactions and Equations.  Chemical Reaction - One or more substances change into one or more new substances.
Chapter12 Stoichiometry. I. What is Stoichiometry? The study of quantitative relationships between amounts of reactants used and products formed by a.
Chapter 12 “Stoichiometry” Mr. Mole. Stoichiometry is… u Greek for “measuring elements” Pronounced “stoy kee ahm uh tree” u Defined as: calculations of.
Stoichiometry and the mole Chapter 8 What is stoichiometry?  Quantitative aspects of chemistry  Stoicheon Greek root (element)  Metron Greek root(
Stoichiometry Section 1 – Introduction to Stoichiometry, and Quantitative Relationships of Chemical Formulas Section 2 – Mathematics of Chemical Equations.
Vocabulary of Mole Theory. ___ is the amount produced from a reaction in reality. actual yield.
Conceptual Statement #2: Units of Matter Communication in Chemistry Chemical Formulas Net charge = 0 (+) charged cation first (-) charged anion last Chemical.
1 Chapter 4 Chemical Equations and Stoichiometry.
Chapter 12 “Stoichiometry” Pre-AP Chemistry Charles Page High School Stephen L. Cotton Mr. Mole.
Chapter 9 “Stoichiometry” Chemistry Charles Page High School Stephen L. Cotton.
Stoichiometry is… Greek for “measuring elements” Defined as: calculations of the quantities in chemical reactions, based on a balanced equation. There.
Chapter 4 Chemical Reactions Chemistry B11 Chemical Reactions Chemical change = Chemical reaction Substance(s) is used up (disappear) New substance(s)
Topic 1 Quantitative Chemistry. Describe and Apply Mole [2-6] 1 mole = 6.02 x – Avogadro’s constant 1 mole is the number of particles contained.
PowerPoint Lectures to accompany Physical Science, 8e Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chapter.
 Calculate empirical formula from mass percent :  Find the molecular formula of a compound has 20 % H, 80 % C, if its Mw = 30 g/mol.
Chapter 3 Stoichiometry AP Chemistry. Finding atomic, molecular and formula masses. Atomic mass is the mass of an atom of an element These are the “red.
Stoichiometry: Calculations with Chemical Formulas and Equations
CHAPTER 3.
Stoichiometry Chapter 3
Chemistry for Changing Times 12th Edition Hill and Kolb
Chemistry II Objectives Unit II - Chapter 2-4
Chemistry I Objectives Chapter 11
Chemical Sentences: Equations
Law of Conservation of Mass
Unit 5: Stoichiometry and Chemical Reactions
Law of Conservation of Matter
MOLE AND STOIKIOMETRI We measure mass in grams. g
Stoichiometry Chapter 3.
12.1 – What is Stoichiometry?
Chapter 12 “Stoichiometry”
Chemical Reactions: Review
Section 9.2 Classifying Chemical Reactions
“Stoichiometry” Mr. Mole.
Ch. 9 Stoichiometry Stoichiometry is a branch of chemistry that deals with the mass relationships of elements in compounds and the mass relationships between.
Chapter 12 “Stoichiometry”
Stoichiometry – Mr. Mole.
Chapter 11 “Stoichiometry”
Ch 7 Chemical Reactions.
Unit Four Chemical Reactions.
Chemical Reactions, Chemical Equations, and Stoichiometry
Chapter 12 “Stoichiometry”
Unit 5 “Stoichiometry” Mr. Mole.
Ch. 8 Chemical Reactions Ch. 8.1 Describing Chemical Change
Chapter 12 Stoichiometry
Chapter 3 Stoichiometry
Ch. 9 Chemical Reactions Identifying a Chemical Change
Stoichiometry Chapter 11.
Chapter 9 “Stoichiometry”
Stoichiometry Presentation
Presentation transcript:

Chemistry I Unit IV Objectives Chapter 10 I.   What is a mole? Define and describe its importance. II.  Memorize and use Avogadro’s number to calculate the number of particles from moles or the number of moles from particles.  III.  Define and be able to calculate molar mass of an element and formula mass of a compound (gram atomic/formula mass). Use this to calculate moles from mass or mass from moles. IV.    Use molar volume (22.4 dm3) to calculate the number of moles in a gas sample at standard conditions of temperature (0C / 273 K) and pressure (1 atm / 760 Torr / 101.3 kpa).

Objectives Unit IV Chapter 10 cont.. V.   Use the mole diagram to convert from and to mass, volume, particles or moles of an element or compound given any one of those properties.  VI.  Calculate % composition of a given formula. VII.  Use percent composition to determine the empirical formula of an unknown substance. VIII.  Be able to use the empirical formula and molar mass to calculate the molecular formula of a given compound. Remember HOFBrINCl

Chemistry I Unit IV Objectives Ch.11 I.  What is a chemical reaction? Describe the characteristics of chemical reactions. II.  Be able to write and balance chemical equations, including word and formula equations.   III. Identify the reactant and products in chemical equations and use correct chemical notation to show the physical state. (s) (l) (g) (aq) IV. Recognize and identify the characteristics of the six types of chemical reactions: a. Direct Combination (Synthesis) ex.      A + B  AB b.  Decomposition (Analysis) ex.      AB  A + B c.   Single Replacement 1.   Cation (metal) replacement ex.   A + BX  AX + B 2.   Anion (nonmetal) replacement ex.    AY + Z  AZ + Y d.  Double Replacement ex.      AX + BY  AY + BX e.  Combustion ex.      CH4 + 2O2  CO2 + 2H2O   f. Neutralization ex. Acid + Base  Salt + Water V.   Be able to predict products of chemical reactions based on type of reaction. VI. Be able to identify spectator ions and write the net ionic equation for replacement reactions   Remember HOFBrINCl

Chemistry I Unit IV Objectives Chapter 12 I.      What is stoichiometry? Define and describe its importance.   II.     Relate stoichiometry to the coefficients in balanced chemical equations and conservation of mass. III.   Be able to solve the following types of stoichiometry problems. a. Mass – Mass b. Volume – Volume c.  Particle – Particle d. Any combination of mass, volume & particles

Objectives Unit IV Chapter 12 cont… IV.     Determine the limiting reactant in a chemical reaction and the reactant in excess. Explain how the limiting reactant controls the amount of product(s).   V.   Use the limiting reactant concept to determine the amount(s) of product(s) (theoretical yield) if reactants are not present in stoichiometric proportion VI.  Calculate theoretical yield and use the actual yield to find the percent (%) yield. Remember HOFBrINCl