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A DOZEN roses = 12 roses - PowerPoint PPT Presentation


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A DOZEN roses = 12 roses. A PAIR of shoes = 2 shoes. a DOZEN eggs = 12 eggs. a REAM of paper = 500 sheets. A GROSS of pencils = 144 pencils. A SIX –PACK of beer = 6 cans. TRIO. QUARTET.

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Presentation Transcript
when you have a dozen of something no matter what you are talking about you have 12 of that thing
When you have a dozen of something, no matter what you are talking about, you have12 of that thing.
  • A dozen donuts- a dozen eggs
  • a dozen cars,
  • a dozen chemistry problems are all 12 of that material.
slide10
The mole is the exact same concept.
  • You can have:
  • a mole of eggs
  • a mole of donuts
  • a mole of cars
  • a mole of chemistry problems.

However a mole is MUCH bigger than 12

...it is 602 sextillion.

Obviously a mole of chemistry problems is way too many problems.

slide11
The mole is typically used for counting or grouping

very very small things, like

atoms

a mole mol
a MOLE (mol)

1. The mole is an SI unit that allows us to count # of:

  • Atoms
  • molecules
  • formula units
  • without actually seeing them

Representative

particles

2 1 mol 6 02 x 10 23 representative particles
2. 1 mol = 6.02 x 1023 representative particles

3. The number is called “Avogadro’s number”

in honor of the Italian scientist

Amadeo Avogadro

avogadro s number
Avogadro’s number

1 mole of anything=6.02 x 1023

Atoms or

Molecules or

FUNs

4 representetive particles
4. REPRESENTETIVE particles:
  • ATOMs (elements on the PT)

2. MOLECULES (_______compounds –

all elements are non metals)

EX: CO2, NO2, C12H22O11

covalent

3. Formula Units(_____compounds – at leastone element must be a metal)

EX: NaCl, CuCl2, FeO

ionic

a dozen
A DOZEN

MASS of a dozen limes = MASS of a dozen cars

a mole
A MOLE

CARBON

COPPER

MASS of a mole carbon = MASS of a mole copper

6.02 x 1023 Catoms = 6.02 x1023 Cu atoms

molar mass the mass of 1 mole of any pure substance element and compound
MOLAR MASS – the mass of 1 mole of any pure substance (element and compound)

Molar Mass (MM) = Atomic mass (AM)

  • MM units - g/mol
  • AM - Atomic Mass units - amu (atomic mass units)

EX: Mn - 54.94 amu = 54.94 g/mol

examples
EXAMPLES:
  • 1 mole of Al :

AM 26.98 g =

MM 26.98 g/mol

# of atoms = # of moles

2. 1 mole of CO2:

AM (C) = 12.011 amu = MM

AM (O) = 16.00 amu x 2 = MM

12.011 + 2 (16.00) = 44.01 g/mole

3 1 mole of cu no 2 2
3. 1 mole of Cu(NO2)2:

AM (Cu) 63.546 amu = MM g/mole

AM (N) 14 x 2 amu = MM g/mole

AM (O) 16 x 4 amu = MM g/mole

63.546 + 2(14) + 4 (16) =

155.5 g/mole

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