The Structure The Structure of the Atomof the Atom
Chapter 4
4.1 - Early Theories of the Atom
4.2 - Subatomic Particles
4.3 - How Atoms Differ
4.4 - Unstable Nuclei & Radioactivity
– CHEMISTRY 112
History of the atom• Not the history of atom, but the idea of the
atom
• Original idea Ancient Greece (400 B.C..)
• Democritus and Leucippus Greek philosophers
• Atomos - not to be cut
Another Greek
• Aristotle - Famous philosopher
• All substances are made of 4 elements
• Fire - Hot
• Air - light
• Earth - cool, heavy
• Water - wet
• Blend these in different proportions to get all substances
Who Was Right?• Greek society was slave based• Beneath Famous to work with hands• did not experiment• Greeks settled disagreements by argument• Aristotle was more famous• He won• His ideas carried through middle ages.• Alchemists change lead to gold
4.1 Early Theories of Matter• Dalton’s Atomic Theory
1. All matter is composed of extremely small particles called atoms.
2. All atoms of a given element are identical. Atoms of different elements are different from one another.
3. Atoms cannot be created or divided into smaller particles or destroyed.
4. Different atoms combine in simple whole number ratios to form compounds.
5. In a chemical reaction, atoms are separated, combined, or rearranged.
Dalton’s Atomic ModelAtom - the smallest
particle of an element that retains the
properties of the element.
4.1 Early Theories of Matter
• E. Goldstein discovered the proton in 1886. • J.J. Thomson discovered the electron in
1897 during cathode ray tube experiments in the late 1890’s.
Thomson’s Experiment
Voltage source
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Vacuum tube
Metal Disks
Thomson’s Experiment
Voltage source
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Thomson’s Experiment
Voltage source
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Thomson’s Experiment
Voltage source
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Thomson’s Experiment
Voltage source
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Passing an electric current makes a Passing an electric current makes a beam appear to move from the negative beam appear to move from the negative to the positive endto the positive end
Thomson’s ExperimentThomson’s Experiment
Voltage source
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Passing an electric current makes a Passing an electric current makes a beam appear to move from the negative beam appear to move from the negative to the positive endto the positive end
Thomson’s ExperimentThomson’s Experiment
Voltage source
+-
Passing an electric current makes a Passing an electric current makes a beam appear to move from the negative beam appear to move from the negative to the positive endto the positive end
Thomson’s ExperimentThomson’s Experiment
Voltage source
+-
Passing an electric current makes a Passing an electric current makes a beam appear to move from the negative beam appear to move from the negative to the positive endto the positive end
Thomson’s ExperimentThomson’s Experiment
Voltage source
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Voltage source
Thomson’s Experiment
• By adding an electric field
Voltage source
Thomson’s ExperimentThomson’s Experiment
By adding an electric field By adding an electric field
+
-
Voltage source
Thomson’s ExperimentThomson’s Experiment
By adding an electric field By adding an electric field
+
-
Voltage source
Thomson’s ExperimentThomson’s Experiment
By adding an electric field By adding an electric field
+
-
Voltage source
Thomson’s ExperimentThomson’s Experiment
By adding an electric field By adding an electric field
+
-
Voltage source
Thomson’s ExperimentThomson’s Experiment
By adding an electric field By adding an electric field
+
-
Voltage source
Thomson’s ExperimentThomson’s Experiment
By adding an electric field he found that By adding an electric field he found that the moving pieces were negative the moving pieces were negative
+
-
Thomson’s Model• Found the electron• Couldn’t find
positive (for a while) • Said the atom was
like plum pudding• A bunch of positive
stuff, with the electrons able to be removed
4.1 Early Theories of Matter
• Robert A. Millikan determined the mass and charge of the electron in 1916.– one unit of negative charge– mass is 1/1840 of a hydrogen atom
4.1 Early Theories of Matter
• In 1911 Ernest Rutherford discovered the nucleus during his gold foil experiment.
4.1 Early Theories of Matter
Ernest Rutherford’s gold foil experiment.
Lead block
Uranium
Gold Foil
Florescent Screen
He Expected
• The alpha particles to pass through without changing direction very much
• Because
• The positive charges were spread out evenly. Alone they were not enough to stop the alpha particles
What he expected
Because
Because, he thought the mass was evenly distributed in the atom
Because, he thought the mass was evenly distributed in the atom
What he got
+
How he explained it
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• Atom is mostly empty
• Small dense, positive piece at center
• Alpha particles are deflected by it if they get close enough
Density and the Atom
• Since most of the particles went through, it was mostly empty.
• Because the pieces turned so much, the positive pieces were heavy.
• Small volume, big mass, big density
• This small dense positive area is the nucleus
4.1 Early Theories of Matter
• Neils Bohr developed the planetary model of the atom– Electrons are in a particular
path have a fixed energy
– Energy level-region around a nucleus where the electron is likely to be moving
4.1 Early Theories of Matter
• Erwin Schrodinger developed the Quantum Mechanical Model– Describes the electronic
structure of the atom as the probability of finding electrons within certain regions of space
4.1 Early Theories of Matter
• James Chadwick discovered the neutron in 1932.
• In 1913 Henry Mosley used X-rays to count the number of protons in the atomic nuclei of different atoms.
4.2 Subatomic Particles & the Nuclear Atom
• Located within the Nucleus– Proton (p+)
• Positively charged particle (each carries a charge of +1)• Relative mass = 1 amu• Actual mass = 1.673 X 10-27 kg
– Neutron (n0)• Neutrally charged particle• Relative mass = 1 amu• Actual mass = 1.675 X 10-27 kg• Serves as the glue that holds the nucleus together as well as a buffer
between the charges of protons and electrons
Subatomic Particles
• Located outside the nucleus in the electron cloud– Electron
• Negatively charged particle (each carries a charge of -1)• Relative mass = 1/1840 amu• Actual mass = 9.11 X 10-31 kg• The electron is the part of the atom that will function in
bonding and reactions
4.3 How Atoms Differ
• Atomic Number– the number of protons in the nucleus of an atom– indicated at the top of the element’s block on the
periodic table 88
OO15.99915.999
1212
MgMg24.30524.305
Oxygen has an atomic number of 8
There are 8 protons in an atom of Oxygen
Magnesium has an atomic number of 12
There are 12 protons in an atom of Magnesium
Isotopes
• Atoms of the same element with the same number of protons, but different numbers of neutrons
• Since the atoms have different numbers of neutrons, they also have different mass numbers– Mass number = # of protons + # of neutrons
Abbreviating Isotopes
• Hyphen Notation– Simply write the Name of the atom, put a
hyphen, and then write the mass number• Carbon-12 vs. Carbon-14
– Carbon 12 has 6 protons and 6 neutrons– Carbon 14 has 6 protons and 8 neutrons
• Nuclear Designation– Element symbol is written in the center– Mass number goes in the upper left corner– Atomic number goes in the lower left corner C
12
6
Different Isotopes• Identify the number of protons, neutrons, and
electrons each of the following have.
Boron-10
Boron 11
35Cl 66Zn17 30
35
Br79.904
p+: ________ no: ________ e-: ________
p+: ________ no: ________ e-: ________
p+: ________ no: ________ e-: ________
p+: ________
no: ________
e-: ________
p+: ________
no: ________
e-: ________
Calculating Atomic Mass
• Mass Number– the number of protons + neutrons in a given isotope
• Atomic Mass– The weighted average mass of all of the isotopes of
that element[(Mass of isotope A)(percent abundance )] + [(Mass of isotope B)(percent abundance)]
Practice Calculating Atomic Mass
Calculate the atomic mass of helium given the following information:
There are two naturally occurring isotopes of helium:
Isotope % Abundance Mass
helium-3 0.0001 3.0160
helium-4 99.9999 4.0026
Practice Calculating Atomic Mass
There are two naturally occurring isotopes of helium:Isotope % Abundance Mass
helium-3 0.0001 3.0160 helium-4 99.9999 4.0026
(3.0160 x 0.000 001) + (4.0026 x 0.999999) 0.000 003 0160 + 4.002595997 0.000 003 0160 + 4.0026
= 4.002603016 = 4.0026
Practice Calculating Atomic Mass
There are three naturally existing isotopes of silicon: silicon-28, silicon-29, and silicon-30. Their percents of natural abundance is listed respectfully: 92.21 %, 4.70 %, and 3.09 %.
Calculate the average atomic mass of silicon and express your answer in 4 significant digits.
4.4 Unstable Nuclei & Radioactive Decay
• Nuclear Reactions– reactions that involve a change in the nucleus of an atom.
• Radioactivity– the spontaneous release of radiation.
• Radiation– rays and particles emitted by radioactive materials
• Radioactive atoms emit radiation because their nuclei are unstable.
• There are three main types of radiation– Alpha decay– Beta decay– Gamma decay
Alpha (α) radiation
• two protons and 2 neutrons
• Positive charge
• Symbols: 4 4He
2
2
• reduces the atomic number by 2
• reduces the mass by 4
Beta (β) radiation
• Fast moving electron
• Negative charge
• Symbols: 0 -1
• increases the atomic number by 1
• does not change the mass
Gamma (γ) radiation
• high energy radiation
• released with alpha and beta radiation
• symbol: 0 0
• does not change the mass or atomic number
Half lives
• The time it takes for 1/2 of the mass of the isotope to be decayed.
• If I have a 60g sample and the half life is 2 years, how long will it take for there to be 7.5g left of the sample?
60g 30g 15g 7.5g 2 years 4 years 6 years
So, it takes 6 years for the 60g sample to decay into 7.5g.So, it takes 6 years for the 60g sample to decay into 7.5g.
