The Mole Unit 3 The Mole So far we have been dealing with numbers on the atomic scale… –Atomic Number = # of protons –Mass Number = # of protons + #

Slides:

Advertisements

Similar presentations

Chapter 11 The Mole Section 11.1 Please have a highlighter and your periodic table out.

Advertisements

The Mole Avogadro’s Number. What is a Mole? The mole is a counting unit, similar to 1 dozen. 1 dozen eggs = 12 eggs 1 mole of eggs = 6.02x10 23 eggs.

1 The Mole 2 Counting Without Counting If you had to count the number of coffee beans in this bag how would you do it? How long would it take?

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 ?

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

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.

The Mole. I. Why the Mole? A. Atomic Mass The mass of one atom of an element Measured in amu –1amu = mass of 1 proton = mass of 1 neutron amu is measured.

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.

Monday November 26, 2012 (Discussion and Worksheet – Moles and Molar Mass)

Chemical Measurements Unit 1: Stoichiometry Chapter 10 – The Mole.

The M & M Lab: What if we had 6.02 x M&M’s and we spread them out over the whole state of Washington, how deep would it be? Yum.

THE MOLE CONCEPT. Objects are measured by counting or by weight (mass) It’s easier to measure large objects by counting –Elephants, cars, eggs It’s easier.

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.

Relating Mass to Numbers of Atoms The mole, Avogadro’s number, and molar mass provide the basis for relating masses in grams to moles.

IIIIIIIV Ch. & 7 – The Mole I. Molar Conversions.

The Mole Chapter 11 – Chemistry L1 LSM High School Section 11.1: Measuring Matter Objectives: Describe how a mole is used in chemistry Relate a mole to.

1 The Mole A counting unit Similar to a dozen, but instead of 12, it’s 602 billion trillion 602,000,000,000,000,000,000, X (in.

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.

IIIIIIIV The Mole I. Molar Conversions A. What is the Mole? n A counting unit n Similar to a dozen, except instead of 12, it’s 602 billion trillion 602,000,000,000,000,000,000,000.

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.

A New Unit of Measurement A Chemistry Exclusive!!!

The Mole Chapter11. I. The mole and Avogadro’s number.

The Mole Chapter11. I. Atoms, Molecules, and Formula units.

Chapter 2 cont’ Atoms and Elements Recall: Atomic Number Number of protons Z Mass Number Protons + Neutrons Whole number A Abundance = relative amount.

A Chemist’s Dozen Today you will only need to copy slides that have a TEAL background.

The Mole A. What is the Mole? ► A counting number (like a dozen) ► Avogadro’s number (N A ) ► 1 mol = 6.02  items A large amount!!!!

Counting atoms. atomic number - # of protons in atom of an element identifies element tells also # of e- Au, K, C, V.

Italian lawyer turned scientist Famous for proposing that equal volumes of gases held at same temperature and pressure must have the same number of gas.

The Mole (and M&M’s) 1 1.

Chapter 8: The Mole – Part 1. What is Avogadro’s favorite saying from American History?

The Mole What's a mole? In chemistry, a mole is a counting unit.

Average Atomic Mass. Relative Atomic Masses  Masses of atoms (in grams) are very small, so for convenience we use relative masses.  Carbon-12 is our.

Chapter 8 Chemical Reactions and Physical Changes Part 3.

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

Tuesday 11/7/12 Bell Ringer 1) Get out your composition notebook to finish taking MOLE notes! *YOU WILL NEED A CALCULATOR ALSO Schedule 1.Bell Ringer—Go.

The Mole Chapter 11 – Honors Chemistry LSM High School.

Note: When doing calculations never clear your calculator.

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.

Chemical Composition … Moles Chemistry Mr. Lentz.

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.

Chapter 8 Earth Chemistry Part – Atomic Number  An atom of a specific element is different from other elements by the number of protons it has.

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.

The Mole Q: how long would it take to spend a mole of $1 coins if they were being spent at a rate of 1 billion per second?

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

Section 6.1 Atoms and Moles 1.Students will be able to describe the concept of average mass. 2.Students will be able to demonstrate how counting can be.

1 Warm Up Isotopes Mass of Isotope Abundance 24 Mg =24.0 amu 78.70% 25 Mg = 25.0 amu 10.13% 26 Mg = 26.0 amu 11.17% Calculate the mass average of magnesium.

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.

RR: How many ways can you count to 100?. Do you know how to count? In chemistry, the unit that helps us count is the mole (mol). The mole represents

The Mole Concept g of Carbon-12 contains x atoms (1 mole) Moles - How chemists count atoms.

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.

A New Unit of Measurement A Chemistry Exclusive!!.

The Mole Concept. How many particles are present? In chemistry, it is important to know the # of atoms (or molecules) that you have. In chemistry, it.

The Mole & Chemical Formulas

Chapter 3 Sec 3 Counting Atoms

The Mole Concept g of Carbon-12 contains x 1023 atoms (1 mole)

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

How We Can Accurately Measure Atoms

Calculating Average Atomic Mass

1. What are these two atoms of carbon called?

Ch. 3 Atoms 3.3 Counting Atoms.

1. What are these two atoms of carbon called?

THE “MOLE” A Mole (mol) is a unit of measurement used for counting very small things (atoms, molecules, etc.) A mole of something is similar to a dozen.

Chemical Reactions & Reaction Stoichiometry

Presentation transcript:

The Mole Unit 3

The Mole So far we have been dealing with numbers on the atomic scale… –Atomic Number = # of protons –Mass Number = # of protons + # of neutrons –Atomic Mass = # of amu in one average atom

The Mole This is a really small scale. Is it logical to try to measure out chemicals for labs this way? NO! We need a bigger scale to use for everyday measurements and calculations.

The Mole We need… The MOLE! The MOLE is a unit of measure – a unit of “how many”.

The Mole Just like a dozen eggs tells us “how many” eggs, a mole tells us “how many” particles. 1 dozen eggs = 12 eggs 1 mole = 6.02 x particles –Particles can be anything – atoms, molecules, eggs, etc.

The Mole This number (6.02 x ) is called Avogadro’s Number, in honor of Amedeo Avogadro’s contributions to chemistry. Unfortunately for him, his ideas weren’t really recognized as important until after he died.

The Mole But wait, where did we get this number? Scientists have found that there is exactly 1 mole of atoms in the atomic mass of an element when that mass is expressed in grams. Huh?

For example: What is the atomic mass of C-12? (Hint – there is only one isotope here, so think mass number) Atomic mass = 12 amu

The Mole Then express that mass in grams  12 g In exactly 12 grams of C-12, there is one mole (6.02 x ) of atoms. This also works for our average atomic masses (from the periodic table).

The Mole So, in exactly g of natural carbon there are 6.02 x atoms. AND, 6.02 x atoms = 1 mole. So 1 mole of carbon = g. Hmm…..those sounds suspiciously like conversion factors… Time for examples!

The Mole How many atoms are in 1.00 mole of gold? 1.00 mole Au 6.02 x atoms 1 mole = 6.02 x Atoms Au

The Mole How many molecules are in 2.00 moles of water? 2.00 mole H 2 O 6.02 x molecules 1 mole = 1.20 x Molecules H 2 O

The Mole How many marbles are in 1.00 mole of marbles? (Enough to cover the entire Earth to a depth of 50 miles!) 1.00 mole marbles 6.02 x marbles 1 mole = 6.02 x marbles

The Mole How many grams are in 1.00 mole of neon? 1.00 mole Ne 6.02 x atoms 1 mole Ne =20.2 g Ne 6.02 x atoms g Ne