CH. 3.4 Counting Atoms. ATOMIC MASS  Atoms are really small and have really small masses  Cu atoms have average mass of 1.0552 x 10 -25 kg  Special.

Slides:

Advertisements

Similar presentations

Chemistry chapter 3 Sample Problems. Isotopes The number of neutrons is found by subtracting the atomic number from the mass number. Mass # (235)---atomic.

Advertisements

1 By definition: 1 atom 12 C “weighs” 12 amu On this scale 1 H = amu 16 O = amu Atomic mass is the mass of an atom in atomic mass units (amu)

 What is the percent composition of N and O in NO 2 ?

The Mole: A Shortcut for Chemists S-C-8-1_The Mole Presentation Source:

Calculating Moles and Number of Atoms

Topic: Counting Atoms and Formula Mass (the MOLE) Do Now: complete package page 2 Here is an example NaCl = 1 Na atom, 1 Cl atom H 2 SO 4 = 2 H atoms,

Atoms: The building blocks of Matter

#1) If 0.20 bushel is 1 dozen apples and a dozen

Chemical Composition.

The Mole Molar Masses.

isotope Are atoms of the same element that have different masses. Due to a different number of neutrons in the nucleus.

Wednesday, Nov. 6 th : “A” Day Thursday, Nov. 7 th : “B” Day (11:45 release) Agenda  Collect “Introduction to the Elements” Worksheet  Section 3.4:

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.

THE ATOM Counting. The Atom  Objectives Explain what isotopes are Define atomic number and mass number, and describe how they apply to isotopes Given.

MOLES!!!. Atomic mass Review the mass of an atom expressed in atomic mass units is an average of the isotopes for that element listed on the periodic.

Chemical Quantities The Mole: A Measurement of Matter

Law of Conservation of Mass Law of Definite Proportions.

THE MOLE 10/1/14 – CHAPTER 3. RELATIVE MASS VS AVERAGE ATOMIC MASS RM = the standard - atomic mass of carbon-12 is used - 1 amu = 1/12 mass of 1 carbon-12.

Counting Atoms 3.3. Counting Atoms Very difficult to count Atomic Number – # of p + of each atom of that element Whole numbers Elements arranged by atomic.

Counting Atoms Chapter 9. MOLE?? Moles of Particles In one mole of a substance, there are 6 x particles.

THE MOLE. Atomic and molecular mass Masses of atoms, molecules, and formula units are given in amu (atomic mass units). Example: Sodium chloride: (22.99.

Wake-up 1.Study Polyatomic Ions for about 5/10 minutes. Write NO WAKE-UP on Friday.

I. Atomic Mass 1.The unit of an element is an atomic mass unit (amu). 2.Carbon –12 has an atomic mass unit of 12. The atomic masses of other elements are.

T HE M OLE Chapter 7. C ONCEPT M AP The mole Can be converted to Similar to: Dozen/ Gross/ set/ pair 6.02x10 ^23 Particles- atoms, molecules, etc. Molar.

Chapter 11: The Mole Table of Contents 11.1: Measuring Matter 11.2: Mass and the Mole 11.3: Moles of Compounds.

Quantities in Chemistry

IIIIIIIV Molar Conversions & Calculations CH. 11 – THE MOLE C. JOHANNESSON.

Chemical Calculations Mole to Mass, Mass to Moles.

I. Atomic Mass 1.The unit of an element is an atomic mass unit (amu). 2.Carbon –12 has an atomic mass unit of 12. The atomic masses of other elements are.

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 Stoichiometry: The Mole Concept Mr. Forte Atascadero High School.

Learning Goal 3 : Determine the molar proportions of the reactants and products in a balanced chemical reaction.

7.1 Notes Continued…The Mole! Key Concepts Why do chemists use the mole? How can you calculate the mass of a reactant or product in a chemical reaction?

10/5-6 Starter A neutral atom contains 34 electrons and has an A of 59. Write the nuclear symbol notation and hyphen notation for this isotope.

THE MOLE. you know that certain quantities can be represented by various terms: dozen = pair = these terms make counting easier 12 2.

Molar Mass = mass in grams of one mole –Units grams/mole Molar Mass = atomic mass Why aren’t all atomic masses whole numbers? –Remember that atomic masses.

3.3 Counting Atoms. Counting Atoms Isotopes Atoms of the same element with different masses Isotopes do not differ significantly in their chemical behavior.

Avogadro’s and the Mole. Moles a mole is the number of carbon atoms in exactly 12g of carbon. a mole is a unit of measurement, just like grams…

The Mole Continued.  The mole is also defined as the number of protons in g of protons.

ATOMIC AND MOLAR MASS. Atomic Mass 2  Considers mass numbers of all isotopes  Natural abundance  Weighted average.

Counting Atoms and Moles Chapter 3.4 us us.

Isotope Practice sodium Na 11 protons, 11 electrons, 12 neutrons copper Cu 29 protons, 29 electrons, 35 neutrons silver Ag.

Avogadro’s Number and Molar Conversions Mole: the SI base unit used to measure the amount of a substance whose number of particles is the same as the number.

Daily Objective To perform calculations using mole (mol) as a unit.

MASS and MOLES Page 57 of INB.

Drill – 10/14 How many decigrams are in 3.0 lbs of potatoes? (1 lb = g)

Scientific Notation and moles  atoms

Chapter 10 Chemical Quantities 10.1 The Mole: A Measurement of Matter

Bell Work Name At Least 4 Types of Representative Particles….. Atom

The Mole Concept.

Chemistry I Mole Review.

Counting Atoms Section 3.3.

mass of one mole of particles

Avogadro’s number, the mole, molarity, molar mass

Counting Atoms Chapter 3 Section 3.

The Mole "Not everything that counts can be counted, and not everything that can be counted counts." Albert Einstein.

The Mole Avogadro’s Number.

Chemical Stoichiometry: The Mole Concept

Section 3 Counting Atoms

The Mole: A Shortcut for Chemists

Counting Atoms CHAPTER 3.3.

The Mole "Not everything that counts can be counted, and not everything that can be counted counts." Albert Einstein.

1 step: Mol to mass conversions

The Mass of a Mole of an Element and a Compound

Chemical Composition.

Measuring Matter Today you’ll need: Periodic Table Calculator

Chemistry Chapter 3 Section 3

Presentation transcript:

CH. 3.4 Counting Atoms

ATOMIC MASS  Atoms are really small and have really small masses  Cu atoms have average mass of x kg  Special unit created for atoms called atomic mass unit (amu) Copper-63 is amu Copper-65 is amu Periodic table says – this is the average of all the isotopes

THE MOLE!  Mole (mol): The # of atoms in exactly 12 grams of carbon-12 (How they decided on the number) x atoms – Avogadro’s number MEMORIZE x  Why do we do this? It’s like saying 1 dozen instead of 12 eggs Grouping things together to making counting easier

THE MOLE  Molar mass is the mass of 1 mole of an element  Same as the atomic mass number on the periodic table But atomic mass is really small and a mole is really big! Atomic mass is the # followed by units amu Molar mass is the # followed by units g/mol (grams per mol)

MOLAR MASS  Moving forward, we will stick to molar mass …and not really use atomic mass

CONVERTING MOLES, MASS, AND PARTICLES – OH MY!  Picket fence time!! x  Mass  Molar Mass  Moles  Avogadro’s number  Particles (atoms)

PRACTICE!  Determine the mass of 3.50 mol of copper  3.50 mol g=222 g 1 mol

YOUR TURN  What is the mass in grams of mol of uranium?  Calculate the number of moles of g of hydrogen atoms.

YOUR TURN  What is the mass in grams of mol of uranium? 1.2 g  Calculate the number of moles of 0.85 g of hydrogen atoms mol

PRACTICE!  Determine the number of atoms in 0.30 mol of fluorine atoms  0.30 mol6.022 x atoms=1.8 x atoms 1 mol

YOUR TURN!  How many atoms are in 0.70 mol of iron?  How many moles of silver are represented by x atoms?

YOUR TURN!  How many atoms are in 0.70 mol of iron? 4.2 x atoms  How many moles of silver are represented by x atoms? mol

PRACTICE!  Determine the number of atoms in 10.0 g of sodium atoms  10.0 g1 mol x atoms= 2.62 x atoms g 1 mol

YOUR TURN!  Determine the number of atoms in 5.05 g of sulfur atoms.  Determine the mass of 3.56 x phosphorous atoms.

YOUR TURN!  Determine the number of atoms in 5.05 g of sulfur atoms x atoms  Determine the mass of 3.56 x phosphorous atoms. 183 g of phosphorous atoms