Catalyst 1. What is a mass spectrometer and how does it work? 2. What kind of ion is produced to create a mass spectrum? 3. What is a mass spectrum? En d
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1. What is a mass spectrometer and how does it work? 2. What kind of ion is produced to create a mass spectrum? 3. What is a mass spectrum? End.
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Slide 1
Slide 2
1. What is a mass spectrometer and how does it work? 2. What
kind of ion is produced to create a mass spectrum? 3. What is a
mass spectrum? End
Slide 3
Havent you always wanted to know whats actually going into your
body? Naming Practice Stations practice Naming big molecules Naming
little molecules Naming organic molecules Naming inorganic
molecules Name it all!
Slide 4
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Slide 9
LT 2.11 I can explain the concept of the mole and why it is an
adequate means by which to express the amount of given substance.
LT 2.12 I can determine the empirical and molecular formula for any
compound given its constituent parts. I can also calculate percent
composition for each element in that compound.
Slide 10
Slide 11
Recall that Avogadro proposed that 1 mole = 6.022 x 10 23
particles. If you have 1 mole this means you have 6.022 x 10 23 of
this substance. This works because particles are really small!
Slide 12
One mole of Carbon- 12 holds 6.022 x 10 23 particles. This can
be applied to any substance and always has the same number of
particles. This isotope was easier to use than Carbon-13 or
C-14.
Slide 13
We can convert between the amount of a substance to moles by
using the molar mass. To do this, use the atomic mass on the
periodic table.
Slide 14
You have 5.380 g of C 6 H 12 O 6, how many moles do you
have?
Slide 15
Slide 16
Percent composition - is the percent by mass of each element
present in a compound. How much of one thing is in another?
Slide 17
Water, H2O is a great example. One mole of water is 18.0152
grams In that compound there are two moles of H atoms and 1 mole of
O atoms.
Slide 18
Calculate the percent by weight of sodium (Na) and chlorine
(Cl) in sodium chloride (NaCl) molecule.
Slide 19
Slide 20
Molecular Formula is what the actual molecule is! Molecular
Formula - a formula giving the number of atoms of each of the
elements present in one molecule of a specific compound.
Slide 21
Empirical means observed, or determined from experimentation!
Empirical formula is the smallest whole number ratio of moles of
each element in a compound. CaCl 2 --> there is 1 mole of
calcium for every 2 moles of chlorine
Slide 22
1. If you have masses go onto step 2. If you have %. Assume the
mass to be 100g, so the % becomes grams. 2. Determine the moles of
each element. 3. Determine the mole ratio by dividing each elements
number of moles by the smallest value from step 2. 4. Double,
triple to get an integer if they are not all whole numbers
Slide 23
Turn each of the molecular formulas to the right into empirical
formulas.
Slide 24
The atomic weight of element X is 100. g/mol. 50.0 grams of X
combines with 32.0 g of oxygen. What is the simplest formula for
the resulting compound? The atomic weight of oxygen = 16.0
g/mol.
Slide 25
Which of the following substances has an empirical formula that
is different from that of the others? (a) Erythrose: C 4 H 8 O 4
(b) Propionic acid: C 3 H 6 O 2 (c) Acetic acid C 2 H 4 O 2 (d)
Glucose C 6 H 12 O 6
Slide 26
KHAN YOU DO IT? http://www.khanacademy.org/test-
prep/mcat/physical- processes/stoichiometry/v/molecular-and-
empirical-formulas http://www.khanacademy.org/test-
prep/mcat/physical- processes/stoichiometry/v/molecular-and-
empirical-formulas Watch video and answer Qs
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Complete the stations review independently or with your
table.
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Quantitative on Ch. 2 on Monday Answers to practices