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Use of Formulae Masses and Moles (but no badgers)
Formula Mass Sum of all the average atomic masses of all the atoms in the formula for the compound Example: Find formula mass for potassium chlorate First: find formula!
Formula mass problem continued Then: Mass of K: 1 atom/mole x amu/atom = amu Mass of Cl: 1 atom/mole x amu/atom = amu Mass of O: 3 atoms/mole x amu/atom=48.00 amu Formula mass = amu amu amu = amu
Molar Mass Mass of one mole of the compound Numerical value is equal to formula mass Units are grams!
Problem: Find molar mass of barium nitrate First, find formula! Then: Barium: 1 mole x g/mole = g Nitrogen: 2 mole x g/mole = g Oxygen: 6 mole x g/mole = g Sum: g g g = g/mole
Conversion: Molar mass can be used to convert from grams to moles and back again Show all your work! Do Sample problem 7-8 and 7-9
Lesson Starter Write the stock system names for MnO, PbO 2 Write the stock system names for MnO, PbO 2 Manganese (II) Oxide Manganese (II) Oxide Lead.
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Chapter 7 Preview Lesson Starter Objectives Formula Masses Molar Masses Molar Mass as a Conversion Factor Percentage Composition Section 3 Using Chemical.
The Mole and Avogadro’s Number. Mole (n): the amount of substance 6.02x10 23 particles (atoms or molecules) of a substance The same number of particles.
The MOLE. The Mole Mole: the amount of a substance that contains as many particles as there are in exactly 12g of carbon-12 A mole is similar to a dozen.
Chapter 7-3: Using Chemical Formulas Coach Kelsoe Chemistry Pages
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.
How Scientists Determine Formulas You have learned how atoms form bonds how to write formulas how to name compounds how to count the atom in compounds.
IIIIIIIV Ch. 10 – The Mole I. Molar Conversions A. What is the Mole? n A counting number (like a dozen) n Avogadros number (N A ) n 1 mole =
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.
1 Chapter 7 Chemical Quantities Charles Page High School Dr. Stephen L. Cotton.
Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 7 USING CHEMICAL FORMULAS Section 3.
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.
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The Mole Theory Molar Mass. Mass of a Mole o Molar Mass- the mass of a mole of any element or compound (in grams) o Also called: o Formula mass – sum.
EMPIRICAL FORMULA empirical formulaThe empirical formula represents the smallest ratio of atoms present in a compound. molecular formulaThe molecular formula.
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.
Module 3.09 Literacy Molar Mass of Compounds. **Please make sure you have a periodic table, calculator and something to write with.
Chapter 10 The Mole. Chemical Measurements Atomic Mass Units (amu) – The mass of 1 atom – 1 oxygen atom has a mass of 16 amu Formula Mass (amu or fu)
IIIIIIIV Ch. 3 & 7 – The Mole I. Molar Conversions (p.80-85, )
I can calculate the molar mass of a compound Sometimes the molar mass is called the formula mass!
Thursday, April 7 th : A Day Friday, April 8 th : A Day Agenda Finish Section 7.1: Avogadros Number & Molar Conversions In-Class: Practice pg. 231: #1-4.
MOLAR MASS Molar mass of a substance = mass in grams of one mole of the substance. A compound’s molar mass is NUMERICALLY equal to its formula mass. Formula.
1 Chemical Quantities or. 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. n We measure.
Let’s use those mole conversions!. Empirical formula tells you the lowest ratio of atoms within a molecule Molecular formula tells you the actual.
Unit 2 The Atom (in general), Atomic Weights, The Mole, Stoichiometry.
Converting using molar mass Because the molar mass of a substance is equal to one mole, we can use it to convert between grams and moles. To do this we.
1. 2 Chapter 10 Chemical Quantities or 3 How you measure how much? How you measure how much? n You can measure mass, n or volume, n or you can count.
For chemists, a mole is NOT a small furry animal.
Moles of Compounds. A properly written compound shows the ratio of atoms in the compound. For example, sodium carbonate (Na 2 CO 3 ) shows that for every.
Calculations with Elements and Compounds The Mole Concept Rev Pisgah High School M. Jones.
Empirical Formula From percentage to formula. The Empirical Formula The lowest whole number ratio of elements in a compound. The molecular formula the.
Section 7.3 – Using Chemical Formulas They allow chemists to calculate a number of characteristic values for a given compound.
What does the little number below each Element mean? What are its units? amu/atom.
The MOLE CH 11. Mole (mol) SI base unit used to measure the amount of a substance One (1) mole of anything is 6.02 X Compare to other counting units:
Molar Mass of ionic compounds. Molar Mass Molar mass- same as atomic mass but for a compound rather than an atom. To determine the molar mass of any compound.
MOLE (mol) Mass (g) Particles (atoms,m’c or f.u.) Which conversion factors that allow you to convert from mass to moles and from particles to moles.
MOLE (mol) Particles (atoms or molecules) DO NOW: Which conversion factor allows you to convert from moles to particles? 1 mol x particles.
MOLE (mol) Mass (g) Particles (atoms,m’c or f.u.) DO NOW: Copy the conversion factors that allow you to convert from mass to moles and from particles.
Christopher G. Hamaker, Illinois State University, Normal IL © 2005, Prentice Hall The Mole Concept.
Chemical Formulas: Formula Mass & Molar Mass. Subscripts in Chemical Formulas subscripts show # atoms of each element subscripts show # atoms of each.
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MOLAR MASS The molar mass is the mass, in grams, of one mole ( particles) of an element (ion), a covalent molecule or a formula unit. molar.
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