Chem Turn in Classification of Matter Mini-Lab from Friday

Slides:

Advertisements

Similar presentations

Mixtures and Pure Substances

Advertisements

Copyright Sautter EMPIRICAL FORMULAE An empirical formula is the simplest formula for a compound. For example, H 2 O 2 can be reduced to a simpler.

CHEMISTRY MATTER ELEMENT ATOM COMPOUND MOLECULE 1.A _____ is a substance made of atoms of more than one element bound together. 2.An _____ is the smallest.

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.

The Mole: A Measurement of Matter OBJECTIVES: Describe how Avogadro’s number is related to a mole of any substance.

Conversion factors. Moles to particles Particles are atoms, molecules or ions 1 mole = Avagadro’s number of particles 1 mole___ or x

Chapter 7 – The Mole and Chemical Composition

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.

Percent Composition. What is Percent Composition?  The percent composition by mass of a compound represents the percent that each element in a compound.

1. What is a mass spectrometer and how does it work? 2. What kind of ion is produced to create a mass spectrum? 3. What is a mass spectrum? End.

  I can determine the percent composition for each element in a compound or sample.

Ch. 11 The Mole.

 What is the molar mass of water?  What % of the mass comes from hydrogen?  What % of the mass comes from oxygen?

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.

Percent Composition and Empirical Formulas Last part of chapter 8, we have done the rest of it already.

Unit 10 – The Mole Essential Questions:

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: A Measurement of Matter

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.

Using the MOLE. Percentage composition Percentage composition is the mass of individual elements in a compound expressed as a percentage of the mass of.

Chapter 11 : Matter Notes. Mole (mol) is equal to 6.02x10 23 The mole was named in honor of Amedeo Avogadro. He determined the volume of one mole of gas.

7.1 and 7.2 Review Calculate the mass in grams of 3.42 x molecules of NaCl. Calculate the volume occupied by 100g of water vapor (H 2 O)

Percent Composition and Molecular Formulas.  Determining the percent composition of each element in a compound  H 2 O 1. Find the molar mass of the.

Percent Composition, Empirical and Molecular Formulas.

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.

Empirical Formula vs. Molecular Formula Empirical formula: the formula for a compound with the smallest whole-number mole ratio of the elements Molecular.

10.1 THE MOLE Q4TP – CHEM MATT T.. THE MOLE: A MEASUREMENT OF MATTER What are three methods for measuring the amount of something? How is Avogadro’s number.

Empirical & Molecular Formulas. Percent Composition Determine the elements present in a compound and their percent by mass. A 100g sample of a new compound.

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.

UNIT 1 Living organisms Natural Science 2. Secondary Education DO YOU REMEMBER WHAT A CHEMICAL COMPOUND IS?

Percent Composition What is the % mass composition (in grams) of the green markers compared to the all of the markers? % green markers = grams of green.

Warm-up Determine the molar mass of the following compounds: Magnesium sulfide Potassium fluoride Carbon tetrabromide Dinitrogen hexachloride.

Moles and Molar Mass. Counting with Moles Mole – amount of a substance that contains 6.02 x particles of that substance 1 mole of the following.

The Mole Chemistry – Chapter 11. Measuring Matter  What measurements do we use?  Pair  Dozen  Gross  Ream  Counting Particles  Atoms and molecules.

Classification and Properties of Matter

Glencoe: Chapter 11 Sections 11.1 & 11.2

Empirical Formulas.

EMPIRICAL FORMULA VS. MOLECULAR FORMULA .

Remembering Scientific Notation…..

Do Now & Announcements Keep your periodic table out for today. This is the only copy you’ll be getting from me! Today: Classification of Matter, Intro.

DO NOW Pick up review. Get out Hydrate lab from yesterday.

Section 3.1 The Mole and Molar Mass

Chemical Quantities.

Percent Composition and Chemical Formulas

Types of Chemical Formulas

Do Now & Announcements Take out HW to be checked if you did not get it stamped. Work on Molar Mass/%Comp Warm Up Problems Unit 2 Quiz WED 9/28 (A),

Unit 6 Mole Calculations

Molar Conversions.

Chem You can start coming in during help session to work on test corrections. Today: Introduction to the Mole.

Empirical Formulas Unit 5.

mole (symbolized mol) = 6.02 x particles

Percent Composition and Empirical Formulas

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.

AP Chem Turn in Chromatography Lab. Today: Mole, EF & MF Review

Molar Conversions.

Percent Composition & Empirical Formulas

Empirical & Molecular Formulas

Percentage Composition

Empirical and Molecular Formulas

Example Problems Ch

Calculating Empirical and Molecular Formulas

1 step: Mol to mass conversions

Unit 8 Stoichiometry.

Formulas/MOF Objectives

Chemical Composition.

Moles and Molar Masses.

2 Step Mole Conversions: particles to Mass/Mass to Particles

Calculating Empirical and Molecular Formulas

Molecular Formula.

Presentation transcript:

Chem Turn in Classification of Matter Mini-Lab from Friday Work on Do Now questions Unit 2A Quest Mon 10/2 (A), Tue 10/3(B)

What is a Mole? Watch the video (https://www.youtube.com/watch?v=EkXR QktVJN0) and answer the questions:

Molar Mass: The mass of one mole of a substance Percent Composition: Identifies the elements present in a compound as a mass % of the total compound mass

41.67% Mg 54.86% O 3.46% H 47.70 % Cr 52.30 % F 15.77% Al 28.11% S 56.12 % O 38.67% K 13.86% N 47.47% O 58.33 grams 108.996 grams 342.14 grams 101.11 grams

Grams <-> Moles Conversions

Atom vs. Molecule ATOM MOLECULE Atom= the smallest, simplest unit of matter. Can refer to individual elements only Molecule=the smallest, simplest unit of a pure substance Can refer to elements or compounds ATOM H H H H H MOLECULE MOLECULE

ATOM MOLECULE H H H H H MOLECULE A water molecule is represented by H2O A water molecule contains 2 atoms of hydrogen and 1 atom of oxygen A hydrogen molecule is represented by H2 (it’s diatomic) An oxygen molecule is made up of 2 hydrogen atoms

Remember: 1 mole = 6.02 x 1023 particles!

Molecules Conversions 1.51 x 1024 molecules 4.37 x 1023 molecules

Molar Conversions Exit Activity Turn in when done HW=right half of note sheet.