By: Ashlee Katie & Jaselyn Chapter 1-3 Introduction to AP Chemistry.

Slides:

Advertisements

Similar presentations

Compound Stoichiometry

Advertisements

General Stoichiometry

Show the Arrangement of Particles in Solid, Liquid and Gaseous Water

Mass Relationships in Chemical Reactions Chapter 3.

Chapter 7 – The Mole and Chemical Composition

Mole Gangnam Style

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

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.

Chapter 3 Percent Compositions and Empirical Formulas

Lesson 25 Percent Composition

What are different ways (measurements) or places to buy apples?

Chapter 10: Chemical Quantities

Chemistry Jeopardy Review!!!. Introduction to chemistry Atoms and Elements Molecules and Compounds Chemical Reactions Moles! Organic

The Mole and Chemical Composition

Jeopardy Molar Mass Avogadro’s Number Stoichiometry Limiting Reactant Emp/Molec Formula Q $100 Q $200 Q $300 Q $400 Q $500 Q $100 Q $200 Q $300 Q $400.

Choose Your Category The MoleAverage Atomic Mass and Molar Mass FormulasPercentage Composition Limiting Reactants Percentage Yield and Error Vocab 100.

Matter Unit.  A unit created to describe atoms because the gram and kilogram are too large to use to define an atom.  1amu = 1.66 x g  g.

Final Review On a new sheet of paper label the top: “Review Do Nows” and begin answering the questions. Be sure to write the questions AND answer!

Unit 5: The Mole.

The MOLE CH 11.

Stoichiometry By Ellis Benjamin. Definitions I Compounds - is a pure substance that is composed of two or more elements Molecules – is a combination of.

Chapter 10 review.

The Mole and Avogadro’s Number

Section 4: Moles of Compounds

Chemical Formulas and Moles. Example: 1.water (C) – every molecule of water contains 2 atoms of hydrogen & one atom of oxygen - 2 molecules of H 2 O would.

By: Ashlee Katie & Jaselyn Chapter 11 Gas Laws Ideal Gas Law Combined Gas Law Movement of Gases Potpourri Final Jeopardy.

Moles and Stoichiometry Chapters 11 & 12. Counting Particles Particles are counted in moles Types of representative particles Atoms- smallest unit of.

Quantitative Chemistry (Part 1) Isotopes Standard Atom for Mass Relative Atomic Mass Formula Mass Percentage Composition.

Molar Mass Practice Calculate the molar mass of the following: Hydrogen Fe Iron II sulfate.

Molar Mass Practice: Molar Mass Practice: 1. Find the molar mass of ammonium sulfate (also called the formula mass): 2. Find the molar mass of copper (II)

Instructions for using this template. Remember this is Jeopardy, so where I have written “Answer” this is the prompt the students will see, and where.

The Mole: A Measurement of Matter Describe how Avogadro’s number is related to a mole of any substance Solve problems involving mass in grams, amount in.

How is the mole concept related to chemical formulas?

THE MOLE Chapter 10: Chemical Quantities Measuring Matter What is a mole? It is the SI unit that measures the amount of substance.

Stoichiometry Chapter 11 & 12. I. Things you should remember From the Moles Unit: Identify particles as atoms, molecules (mc), and formula units (fun)

1 The Mole 6.02 X What is “The Mole??” A counting unit (similar to a dozen) 6.02 X (in scientific notation) = 602 billion trillion = 602,000,000,000,000,000,000,000.

Matter Unit.  A unit created to describe atoms because the gram and kilogram are too large to use to define an atom.  1amu = 1.66 x g  g.

CHEMICAL QUANTITIES Composition Stoichiometry Calculating Molar Mass Avogadro’s Number and the Mole Percentage Composition and Empirical Formulas Molecular.

  Review Chemical Reactions Atoms and the Periodic Table Matter Bonding and compounds FJ Chemistry.

By: Ashlee Katie & Jaselyn Chapter 4 Stoichiometry.

CHEMISTRY CHAPTER 7 SECTIONS 3-4 SECTION 3. USING CHEMICAL FORMULAS Introduction A chemical formula indicates: the elements present in a compound the relative.

Molecular Weight, Percent Composition, Empirical Formula.

Objective: To reintroduce the mole and introduce two mole conversions Do Now: Solve each proportion = x2. 10 = x.

 What do you call the following phase changes?  Solid to a liquid  Melting  Liquid to a solid  freezing  Liquid to a gas  vaporization  Gas to.

The Mole Honors Chem. -How do we measure chemical quantities? -What units of measure do we use?

ATOMIC MASS – The mass of an individual atom ATOMIC MASS UNIT (amu or u) – One twelfth the mass of a carbon-12 atom, equal to 1.66 x g Atomic masses.

THE MOLE. STANDARDS Use the mole concept to determine the number of particles and mass in a chemical compound. (includes gram to mole to atom conversions)

1 Chapter 7 Chemistry Empirical Formulas/molecular formulas LOOK AT: Pages

Chemical Quantities Chapter 10. The Mole  a mole is an amount of matter  mass is also an amount of matter, however the mole is much more useful to chemists,

EF, MF, Hydrates & % Comp notes

AP Chemistry Chapters 1-3 Review

Jeopardy Empirical Formulas Molecular Formulas Nomenclature Hydrates

Molar Mass Chapter 7 Review

The Mole and Avogadro’s Number

Chemical Compostition

Practice questions All of the following are examples of mixtures except a) soft water. b) hard water. c) distilled water. d) supermarket salt. e) drugstore.

Isotopes and Average Atomic Mass

MIDTERM REVIEW.

Bell Work 1 / Mole Map 1. Draw the Mole Map and include the relationships that exist between each section.

Bell Work 1 / Mole Map 1. Draw the Mole Map and include the relationships that exist between each section.

Using Chemical Formulas

Chapter 10: Chemical Quantities

1 step: Mol to mass conversions

The Mass of a Mole of an Element and a Compound

Combustion analysis Combustion analysis is a method used in both organic chemistry and analytical chemistry to determine the elemental composition (more.

Chemistry Chapter 3 Section 3

Presentation transcript:

By: Ashlee Katie & Jaselyn Chapter 1-3 Introduction to AP Chemistry

CompoundsIsotopesPotpourri Math Review Final Jeopardy

100 Compounds Are all compounds molecules? Give an example to support your answer.

200 Compounds What are allotropes? Give two examples of allotropes

300 Compounds Name the following compounds: Pb(C2H3O2)2 SnCr2O7 Cl2O7

400 Compounds Write formulas for: Aluminum sulfate Beryllium phosphate

A compound was analyzed and found to contain 63.15% carbon, 5.30% hydrogen, and 31.55% oxygen by mass. If the molar mass of the compounds is g/ mol, what is the molecular formula of the compound 500 Compounds

What is different about isotopes of the same element? 100 Isotopes

200 Isotopes What do the atomic masses written on the periodic table represent?

300 Isotopes What is the result of the alpha decay of Carbon-14?

400 Isotopes What is the result of the beta decay of protactinium-234? (Pa is the symbol for protactinium.)

500 Isotopes Europium as two isotopes. Eu-151 has a mass of amu and Eu-153 has a mass of amu. The average atomic mass of Eu is amu. Calculate the relative abundance of the two europium isotopes.

100 Potpourri What is the meaning of 0 Kelvin?

Convert from 25 C to Kelvin. 200 Potpourri

300 Potpourri Use Coulomb’s Law to explain which compound melts at a higher temperature: lithium fluoride or calcium sulide

400 Potpourri The density of ethanol is g/mL. How many moles of ethanol are present in 27 mL of ethanol?

Explain whether each of the following reactions will occur or not: Zinc combined with cupric sulfate Potassium chloride combined with silver 500 Potpourri

Express your answer in scientific notation with correct sig figs and units: g / (1.376 cm x 2.45 cm x 3.78 cm) 100 Math Review

200 Math Review What is the percent by mass of nitrogen in ammonium nitrate?

300 Math Review Use your graphing calculators! The density of pure water at various temperatures is given in degrees Celcius: g/mL g/mL g/mL g/mL What is the density at 47 C?

400 Math Review What mass of lead has the same number of atoms as 50 g of oxygen?

A g sample of a hydrate of magnesium carbonate was carefully heated without decomposing the carbonate to drive off the water. The mass was reduced to 7.58 g. What is the formula of the hydrate? 500 Math Review

Daily Double

Final Jeopardy Make Your Wager

Final Jeopardy How many atoms of iron are in 3.58 grams of ferric carbonate?