Isotope l The average atomic mass of each element uses the masses of the various isotopes of an...
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![Page 1: Isotope l The average atomic mass of each element uses the masses of the various isotopes of an element l An isotope of an element is the same element.](https://reader035.fdocuments.in/reader035/viewer/2022062409/5697bf861a28abf838c8833e/html5/thumbnails/1.jpg)
Isotope
The average atomic mass of each element uses the masses of the various isotopes of an element
An isotope of an element is the same element with the same # of p+, but a varying number of neutrons and thus a varying atomic mass
NOT all elements contain isotopes
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Isotope Determinationex. H
There are 3 isotopes of Hydrogen
atomic mass atomic # #p+ #n
1.001H 1.00 1 1 0
2.001H 2.00 1 1 1
3.001H 3.00 1 1 2
The average atomic mass of H = 1.0079
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Isotope Determination
There are three isotopes of Carbon
12C Carbon 12
13C Carbon 13
14C Carbon 14
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Groups - # valence e- Periods - Size of atom
Noble gasesGroup VIII
HalogensGroup VII
AlkalliMetalsGroup I
MetalsNonmetals
Metalloids
Alkali EarthMetals
Group II
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Formula WeightsH2
N2 O2 F2
Cl2
Br2
I2
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Chemical EquationsSodium + Diatomic Chlorine ------> Sodium Chloride
Reactant(s) -----yields-----> Product(s)
Na + Cl2 ----------> NaCl
Equations must be balanced due to the
Law of Conservation of Matter
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Chemical EquationsBookkeep the Atoms
Count the individual atoms of reactants and products line up under each atom in separate rows:
Na + Cl2 NaCl
1 Na 1 Na
2 Cl 1 Cl
Use whole number multipliers to equalize the atoms of reactants and products.
Place these whole number prefixes before the element or the compound
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Chemical EquationsBookkeep the Atoms
Na + Cl2 NaCl
1 Na 1 Na
2 Cl 1 Cl
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Chemical Equations
2Na + Cl2 2NaCl
2 Sodium atoms react with 1 chlorine molecule to form 2 “Molecules” of Sodium Chloride
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Chemical Equations
1. (NH4)SO4 H2SO4 + NH3
5. Fe + H2O Fe3O4 + H2
TRY in groups
#6 and #9
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% of an Element in a Compound
(Elemental Analysis) Mass of Element x 100
FW of Compound
% H in H2O 2H x 100 = 2.00 amu x 100 = 11.1%
H2O 18.00 amu
% O in H2O O x 100 = 16.00 amu x 100 =
88.89% H2O 18.00 amu
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Group Work
Determine the Elemental Analysis of:
» C6H12O6
» NH3
» CO2
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Definition
Mole (mol or n)» 1 mole contain the same number of entities
(atoms, molecules, ions, particles) as there are in exactly 12.01 grams of Carbon and a mole contains 6.022 x 1023
number of entities. This number is called Avogadro’s Number.
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1.00 gH
12.01 gC
18.00gH2O
35.45 gCl-
180.06gC6H12O6
6.022 x1023
atoms
6.022 x1023
atoms6.022 x1023
molecules
6.022 x1023
ions6.022 x1023
molecules
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Analogy
1 pair = 2 1 trio = 3 1 dozen = 12 1 mol = 6.022 x 1023
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Molar Mass (MM)
To Determine the Molar Mass (MM):
For an element - it’s the atomic weight
in grams
For a compound - it’s the formula weight
in grams
A mole contains Avogadro’s Number
(6.022 x 1023) particles
(atoms, ions, molecules).
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Working with Moles
Formula given grams of a compound or element, determine the number of moles
Moles = grams MM
OR Dimensional Analysis
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Working with Moles
Formula given moles of a compound or element, determine the number of grams
moles (MM) = grams
OR Dimensional Analysis
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Multiply by Avogadro’s #, Divide by Molar Mass
Multiply by Molar Mass, Divide by Avogadro’s #
Number of Moles
Number of atoms, ions,
molecules
Mass in
grams