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IUnit 1
How do we distinguish substances?
M1. Searching for Differences Identifying differences that allow us to separate components.
M2. Modeling MatterUsing the particulate model of matter to explain differences.
M3. Comparing Masses Characterizing differences in particle’s mass and number.
M4. Determining Composition Characterizing differences in particle’s composition.
The central goal of this unit is to help you understand and apply basic ideas that can be used to distinguish
the different substances present in a system.
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Unit 1
How do we distinguish substances?
Module 4: Determining Composition
Central goal: To use experimental data to determine the atomic
composition of the particles that make up a
substance.
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The Challenge AnalysisWhat is this?
According to our models, differences between substances are the result of differences in the composition and structure of their particles.
N2
O2
H2O
CO2
C4H10
O3
How can we determine what atoms and how
many of each type comprise the
molecules of any given substance ?
C H O NColor Code
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IFinding the Mass
One first step could be determining the relative mass of the particles. For this purpose, we could
use a Mass Spectrometer.
1. Particles are vaporized and broken into ions (charged particles).
2. The ions are accelerated and separated using a magnetic field.
3. The ratio mass/charge is recorded (most ions have a 1+ charge).
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IElectrical Nature
Mass spectrometry is based on our knowledge and understanding of the
electrical nature of matter.
When atoms or molecules lose or gain electrons they become electrically charged. The charged particles are called ions.
We model
atoms as made by + and –
charges.
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Each type of atoms is characterized by the number of protons in the
nucleus (atomic number, Z).
In a neutral atom, the number of protons is equal to the
number of electrons.
q(e-) = q(p+)
Atomic Number
Most of the atomic mass is concentrated in the nucleus
m(p+) ~ m(n0) ~ 1800 m(e-)
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IMass Spectrometry
So, imagine we take a sample of a gas, like Neon (Ne), and we analyze it with a
mass spectrometer:
rel. int
m/z
90.48%
0.27%9.25%
Why do we get 3 peaks instead of one?
Let′s think!
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IAtomic Differences
All atoms of the same element have the same number of
protons in the nucleus, Z, but they may differ in the number
of neutrons.
To differentiate them we can use a quantity called
Mass Number A:
A = # p+ + # n0
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IIsotopes
We call isotopes to these atoms of an element with the same number of protons,
but a different number of neutrons
rel. int
m/z
20Ne90.48%
21Ne 0.27%
22Ne 9.25%
Average relative atomic mass
mr(Ne) =19.99 x 0.9048 +
20.99 x 0.0027 +
21.99 x 0.0925
mr(Ne) = 20.18 amu
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From Atoms to MoleculesMass spectrometry can also be used to determine the
mass of molecules and analyze their structure.
However, in this case it is
important to realize that the molecules will
break apart into several
fragments.
MethaneCH4
CH4+
CH3+
CH2+
CH+
C+
?
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From Atoms to Molecules
This is the mass spectrum for methanol (CH4O):
How do you explain the
different peaks?
Let′s think!
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This is the mass spectrum of an elemental gaseous substance (X2) collected from a tanker truck spill.
Let′s think!
Which is this element?
How do you explain all of the different peaks
in the spectrum?
75.78%
24.22%
34.97 amu 36.97 amu
What is the average relative atomic mass of this element?
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Combustion Analysis
Knowing the relative mass of the particles, we need a method to determine particle composition
Particle composition: Type and number of atoms of each type per particle
Elemental Analysis
Through elemental analysis we can find the percentage of each
element present in the substance
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I This is the substance’s mass
spectrum.M(X) = 78.1 g/mol
Consider this data:
The analysis of the exhaust gases from motor traffic reveals the presence of a carcinogenic
substance. Elemental Analysis reveals that the substance contains
92.26% C and 7.74% H.
Collecting Data
What is this?
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1. Take 100.0 g of your sample and calculate how much of each element you have: 92.26 g C 7.74 g H
2. Calculate the number of moles of each type of atom in the sample:
92.26 g C x 1 mole C/12.01 g = 7.68 mol C7.74 g H x 1 mole H/1.008 g = 7.68 mol H
3. Write a preliminary formula and convert to the the smallest integer subscripts that have the same proportion (divide by the smallest subscript):
C7.68H7.68 CH Empirical Formula
Finding the Formula92.26% C and 7.74% H M(X) = 78.1 g/mol
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4. Compare the actual molar mass of the compound (mass spectrum) with the molar mass calculated using the empirical formula (13.018 g/mol).
Finding the Formula
78.1 /13.018 = 6.00
Molecular Formula = 6 x Empirical Formula
C6H6
92.26% C and 7.74% H. M(X) = 78.1 g/mol
Benzene
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M(X) = 410. g/mol
The analysis of indoor air in some Tucson homes treated for termites reveals the presence of a harmful substance that affects the nervous system. Elemental analysis provides the following percent composition:
29.31% C, 1.476% H, and 69.22% Cl.
Let′s think!
Find the empirical and
molecular formulas of this
compound.
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I Assess what you know
Let′s apply!
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ILet′s apply!
Environmental analysis of air samples is often performed using a combined analytical technique
called GC/MS (Gas Chromatography-Mass Spectrometry)
Other applications include drug detection,
explosives investigation, and identification of unknown samples
GC/MS
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Gas ChromatographyLet′s apply!
GC is used to separate the
components of the mixture.
What differentiating
characteristics is used to separate
substances?
Why some substances move faster than others
inside the column?
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After the components are separated, their masses are analyzed by mass spectrometry.
Mass SpectrometryLet′s apply!
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A sample of Tucson’s air is analyzed by
GC/MS, followed by elemental analysis. Among the various substances in the sample, two major
pollutants are found.
Tucson AirLet′s apply!
30.4% N 69.6% O
50.0% O 50.0% S
Find the empirical and molecular
formulas of these two substances.
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If you had to describe what this module was about,
what would you say?
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Determining Composition
Summary
We take advantage of the electrical nature of matter to explore its properties and composition.
Mass spectrometry, an analytical technique that exploits the electrical nature of matter, can be used to compare the relative masses of different atoms and differentiate one from another.
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We can use MS and elemental analysis to determine the number of atoms of each type that make up the
particles of a given chemical compound.
Determining Composition
Empirical Formula
C5H3Cl4
Molecular Formula
C10H6Cl8
Chlordane
M(X) = 410. g/mol
29.31% C, 1.476% H, 69.22% Cl.
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Are You Ready?
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The central goal of this unit was to help you understand and apply basic ideas that can be used to distinguish the different substances present in a
system.
Unit 1How do we distinguish substances?
Can you use measurements and models to separate
and identify the different substances present in a system?
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The Challenge
Bombardier beetles seem to store aqueous solutions of two
different substances.
When they are threatened, the two solutions are squirted
through two tubes, where they are mixed and undergo a violent
chemical reaction.
The reaction releases a gas (O2) and generates enough heat to bring the mixture to the boiling
point and vaporize about a fifth of it.
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Analysis of the reaction mixture (an homogeneous solution) has revealed the presence of two major substances. One of them is hydrogen peroxide,
H2O2, which is a liquid (Tb = 150.2 oC) fully miscible in water. H2O2 easily decomposes into H2O and O2
when heated up.
Let′s think!
How would you propose to separate the other component?
What additional information would help you better answer this question?
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Let′s think!The analysis of the phase behavior of the isolated substance produces the following phase diagram:
What is the stable phase of this
substance at room temperature (20 oC)?
What are the normal melting and boiling
points of this substance?
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Let′s think!What would you propose to do to determine the
chemical composition of the unknown substance?
Elemental analysis of the
unknown reveals the following composition:
65.45% C, 5.49% H, 29.06% O.
What is the molecular formula
and the molar mass?
M = 110.1 g/mol
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Let′s think!The separation process yields 0.028 g of C6H6O2 and 0.25 g of H2O2 per mL of aqueous solution.
If the density of water (H2O) is close to 1.0 g/mL,how many moles of water are there per mole
of C6H6O2 and H2O2 in the solution?
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Let′s think!
Use all of the information provided to build a microscopic representation of the reacting
solution inside the bombardier beetle.
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Let′s think!
Use the particulate model of matter to
explain how the defense
mechanism of the bombardier beetle
works.
The reaction between C6H6O2 and H2O2 in a closed chamber inside the beetle releases a gas (O2) and generates enough heat to bring the mixture to the
boiling point and vaporize about a fifth of it.