atomic theory & atomic structure. tro, chapter 4 & 9 sections 4.1 – 4.4, 4.8, 4.9; 9.2 –...
TRANSCRIPT
![Page 1: Atomic Theory & Atomic Structure. Tro, Chapter 4 & 9 Sections 4.1 – 4.4, 4.8, 4.9; 9.2 – 9.9](https://reader035.vdocument.in/reader035/viewer/2022062423/5697bf941a28abf838c903cd/html5/thumbnails/1.jpg)
Atomic Theory &
Atomic Structure
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Tro, Chapter 4 & 9
Sections 4.1 – 4.4, 4.8, 4.9; 9.2 – 9.9
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Document BIG IDEAS about:
• Atomic structure– Electrons (mass, size, position)– Protons and neutrons (mass, position)– Isotopes
• Changes in (MODERN) thought – Dalton– Thomson, Rutherford and Bohr
• Quantum theory (CONTEMPORARY)
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Early Atomic Theories
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Democritis (400 BCE)
• First to propose idea of atom• Atom = “a” + “tomos” = cannot be
cut• Based solely on logic; not
supported by experiments
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Alchemy(12-1500 CE)
• Modern word ‘chemistry’ came from Arabic ‘alkimiya’
• recognized importance of experimentation
• Responsible for developing lab equipment & procedures still used today
NOTE: Alchemy is a field, NOT a person…
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Galileo(~1600 CE)
• Birth of modern science - combining logic, experimenting, publishing results
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Lavosier & Priestly(1700’s)
• Quantitative analysis of chemicals
Law of Conservation of Mass:
Matter can neither be created nor destroyed
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Proust(1700’s)
• Developed Law of Definite Proportions
Law of Definite Proportions:Different samples of the same compound always contain its
constituent elements in the same proportions by mass
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Law of Definite Proportions
• Copper carbonate always contains – 5.3 parts copper– 4 parts oxygen– 1 part carbon
by mass
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Dalton(1800’s)
• School teacher that proposed the first modern-day idea of atoms
Law of Multiple Proportions:If 2 elements combine to form more than one compound, the masses of one element that
combine with a fixed mass of the other element are in small whole # ratios
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Law of Multiple Proportions
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Dalton’s Atomic Theory - 1808• All matter is composed of atoms which
cannot be subdivided• Atoms of same element are identical
(size, mass, reactivity)• Atoms combine to form compounds in
simple, whole # ratios• Chemical reactions involve the
separation, combination, or rearrangement of atoms; it does not result in their creation or destruction
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Modern Atomic Theories
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General Principle #1 Electric Charges
Objects with an equal amount of positive and negative charge are said
to be electrically neutral
+ – positive negative
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General Principle #2Forces between Charges
• Objects with like charge repel
• Objects with opposite charge attract
+ + ++
– + – +
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Forces between Charges• Electrostatic force becomes
greater with more charge• Electrostatic force becomes
smaller the greater the distance between the charges
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Thomson’s Atomic Model (1904)
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Cathode Ray Experiments• Any metal worked
for anode• Negative electric
field repelled beam• Object placed in
path of glow blocked beam
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J.J. Thomson’s Contribution
• Discovered the electron (1897)• Plum Pudding model• Determined the charge-to-mass
ratio of an electron using data from cathode ray tube experiments
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Evidence & Conclusions• cathode rays consisted of subatomic
particles from atoms of anode• cathode rays are negatively charged
• must also be positive charge
• Millikan (oil drop experiment, 1909) calculated electron’s mass to be 9.11 x 10-31 kg
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Modern View of Atomic Structure
Particle
SymbolRelativ
e Charge
Mass (kg)
proton p+ +1 1.6726 x 10-27
neutron
n0 0 1.67510 x 10-27
electron
e- -1 9.1096 x 10-31
+
0
nucleons
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Modern View of Atomic Structure
Particle
Relative
ChargeMass (kg)
Relative mass (amu)
p+ +1 1.6726 x 10-27 ~1
n0 0 1.67510 x 10-
27 ~1
e- -1 9.1096 x 10-31 ~0
+
0
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Rutherford’s Problems• How is nucleus held together?• Why don’t electrons collapse into
nucleus?• H atom has 1 proton & He atom has
2 protons, mass ratio should be 2:1; instead the ratio is 4:1
…there must be another particle
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The Gold Foil Experiment: Hypothesis
• The α-particles will pass straight through the atoms
What is an () alpha particle?
It is a positively charged Helium nucleus
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Rutherford’s Gold Foil Experiment
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The Gold Foil Experiment: Outcome
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What’s happening?
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The Gold Foil Experiment: Conclusions
Atoms :• must be mostly
space• must have a very
small, dense area of + charge
• Protons have same charge as e-, but almost 2000x more mass!
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The Neutron• Discovered by James Chadwick in
1932.• Neutron is electrically neutral &
has slightly greater mass than a proton
Mystery solved.
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Atomic theory timeline
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Updating Dalton’s Atomic Theory
3 major differences between modern atomic theory & Dalton’s atomic theory:
• Atoms are NOT indivisible – they are made up of protons, neutrons, and electrons
• Atoms of the same element are NOT exactly alike – they can have different masses (isotopes)
• Atoms CAN be changed from one element to another, but not by chemical reactions (nuclear reactions)
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Atomic Structure & Isotopes
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Atomic Mass Unit (amu)• defined as a more convenient unit
for reporting mass of small numbers of atoms
• 12C is used as the reference• 1 amu is defined as exactly 1/12 of
a 12C atom
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Getting Information from the Periodic Table
6C
12.0111
Atomic # = # p+ in nucleus
Elemental symbol
Atomic mass (more on this later)
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Isotopic Notation• Atomic number (Z) = # of p+ in the nucleus• Mass number (A) = sum of # p+ & n0 in
nucleus• For a neutral atom, # e- = # p+
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H11 He4
2 C126 O16
8 Zn6330
Mass number (A)
Examples
Atomic number (Z)
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Isotopes• All atoms in an element have the
same atomic number• However, 2 atoms of the same
element can have different mass numbers – called isotopes
• Isotopes have:– Same # of p+
– Different # of no
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Some Common Isotopes
H
H
H
11
21
31
C
C
C
126
136
146
U
U
23592
23892
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Relative Abundance
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Mass Spectrometry• Technique used to determine
atomic mass
e-
Atom bombarded by stream of high energy electrons
e-
e- collides with atom, “bounces” off, but transfers some energy to it
e-
+Atom dissipates excess energy by expelling an electron
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Mass Spectrometry, cont.• Ions are accelerated through a magnetic field• Amount of deflection depends on the ion’s mass• Highest mass deflected least
• Lowest mass deflected most
N
S
++ +
+
++++
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Mass Spectrometry, cont.
Mass (amu)
Sample mass spec for chlorine
Relative abundance of each isotope can be determined from relative peak heights
35 37
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Relative Abundance & Atomic Mass
• Relative isotopic abundance is then used to calculate atomic mass
• Atomic mass is the weighted average of the mixture of isotopes
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Example
average atomic mass = (atomic mass 35Cl)(fraction 35Cl) + (atomic mass 37Cl)(fraction 37Cl)= (34.968 amu)(0.7577) + (36.965 amu)(0.2423)= 35.45 amu
Calculate the atomic mass of Cl given the relative abundances of its isotopes:35Cl – 75.77%37Cl – 24.23%
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PracticeCopper, a metal known since ancient times, is used in electrical cables & pennies, among other things. The atomic masses of its 2 stable isotopes, 63Cu (69.09%) and 65Cu (30.91%) are 62.93 amu and 64.9278 amu, respectively. Calculate the average atomic mass of copper – the relative abundances of each ion is given in parentheses. Answer: 63.54 amu
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The Bohr Model
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Electromagnetic Spectrum
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Light
c =
c = speed of light (3.0 x 108 m)= wavelength= frequency
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Frequency vs. Wavelength
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Light
• Energy as frequency • Energy as wavelength • Light behaves like a particle
(photon) as well as a wave
c =
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Emission Spectrums• When electricity is run through a
sample of hydrogen gas, hydrogen atoms gain energy
• H atoms loose that energy by emitting photons
• Resulting spectrum is discontinuouscontinuous
discontinuous
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Bohr Model• Electrons move in
circular orbits around the nucleus
• Only certain energy levels are “permitted ” (this explains the discrete lines for the emission spectrum of hydrogen)
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Schroedinger/Heisenburg• Experiments used mathematics
(probability) to predict behavior of electrons– Schroedinger equation
approximated the probability of finding a single electron for H within a region close to the nucleus
– Heisenburg [Uncertainty Principle] reinforces the idea that we just don’t know!
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Math in Context: Blackbody Experiments