dr. s. m. condren chapter 8 electron configuration, periodicity, and properties of the elements
TRANSCRIPT
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Dr. S. M. Condren
Chapter 8
Electron Configuration,
Periodicity, and
Properties of the Elements
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Dr. S. M. Condren
Electromagnetic Radiation
Electromagnetic wave• A wave of energy having a frequency
within the electromagnetic spectrum and propagated as a periodic disturbance of the electromagnetic field when an electric charge oscillates or accelerates.
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Dr. S. M. Condren
Electromagnetic Radiation
Electromagnetic wave
• wavelength
• frequency
• amplitude
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Dr. S. M. Condren
Quantum Mechanics
Quantum theory• the theory of the structure and behavior of
atoms and molecules.
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Dr. S. M. Condren
Black Body Radiation
http://www.cbu.edu/~mcondren/C11599/BBvis.mov
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Dr. S. M. Condren
Electromagnetic Radiation
= c
where=> frequency
=> wavelength
c => speed of light
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Dr. S. M. Condren
Electromagnetic Radiation
Ehi - Elo = hc/where E => energy
h => Planck's constant
c => speed of light
=> wavelength
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Dr. S. M. Condren
Photoelectric Effect
• the emission of electrons by substances, especially metals, when light falls on their surfaces.
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Photons
The quantum of electromagnetic energy, generally regarded as a discrete particle having zero mass, no electric charge, and an indefinitely long lifetime.
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Dr. S. M. Condren
Line Spectrum
A spectrum produced by a luminous gas or vapor and appearing as distinct lines characteristic of the various elements constituting the gas.
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Dr. S. M. Condren
Emission Spectrum
The spectrum of bright lines, bands, or continuous radiation characteristic of and determined by a specific emitting substance subjected to a specific kind of excitation.
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Dr. S. M. Condren
Ground State
The state of least possible energy in a physical system, as of elementary particles. Also called ground level.
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Excited State
Being at an energy level higher than the ground state.
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Absorption Spectrum
• Light shinning on a sample causes electrons to be excited from the ground state to an excited state
• wavelengths of that energy are removed from transmitted spectra
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Dr. S. M. Condren
Knowing diamond is transparent, which curve best represents the absorption spectrum of diamond (see below)?
A, B, C
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The Atomic Spectrum of Hydrogen and the Bohr Model
Bohr Model for the Hydrogen Atom
mnr = nh/2p
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Bohr Model
Netscape
• NCSU Materials Science site– Chapter 2 Atomic Bonding
• I Atoms and Electrons– slide 2
or
• http://odin.cbu.edu/~mcondren/bohr.html
or through the CHEM 115 homepage
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Bohr Atom
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Bohr Model
E = -B/n2
where n => quantum number
1, 2, 3, 4, 5, 6, 7, etc
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Bohr Model
E = (-2.179 X 10-18 J/part.)
(6.022 X 1023 part./mole)
(1 kJ/103 J)/n2
= (-1312 kJ/mol)(1/n2)
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Bohr Model
for hydrogen
ground state: n = 1
excited state: n > 1
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Line Spectra
Lyman series => ultraviolet
n > 1 ==> n = 1
Balmer series => visible light
n > 2 ==> n = 2
Paschen series => infrared
n > 3 ==> n = 3
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Dr. S. M. Condren
Line Spectra
See CHEMWORKS software
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According to the energy diagram below for the Bohr model of the hydrogen atom, if an electron jumps from E1 to E2, energy is
absorbed
emitted
not involved
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Heisenberg, Werner1901–76, German physicist
1932 Nobel Prize in physics
A founder of QUANTUM MECHANICS, he is famous for his uncertainty principle, which states that it is impossible to determine both the position and momentum of a subatomic particle (such as the electron) with arbitrarily high accuracy.
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Heissenberg Uncertainty Principle
“it is impossible to determine both the position and momentum of a subatomic particle (such as the electron) with arbitrarily high accuracy”
The effect of this principle is to convert the laws of physics into statements about relative, instead of absolute, certainties.
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Orbitals
• region of probability of finding an electron around the nucleus
• 4 types => s p d f
• maximum of 2 electrons per orbital
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Dr. S. M. Condren
Pure Atomic Orbitals
shape # of orbitals / energy level
s spherical 1
p dumbbell 3
d complex 5
f very complex 7
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Shapes of Orbitals
http://www.colby.edu/chemistry/OChem/DEMOS/Orbitals.html
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Dr. S. M. Condren
Electronic Configurations
• The shorthand representation of the occupancy of the energy levels (shells and subshells) of an atom by electrons.
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Dr. S. M. Condren
Electronic Configuration
shells => energy levels
subshells => orbitals
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Dr. S. M. Condren
Electron Filling Order Diagram
1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f
6s 6p 6d
7s
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Dr. S. M. Condren
Electronic Configuration
H atom
1 electron
1s1
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Dr. S. M. Condren
Electronic Configuration
He atom
2 electrons
1s2
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Dr. S. M. Condren
Electronic Configuration
Li atom
3 electrons
1s2, 2s1
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Dr. S. M. Condren
Electronic Configuration
Cl atom
17 electrons
1s2, 2s2, 2p6, 3s2, 3p5
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Dr. S. M. Condren
Electronic Configuration
As atom
33 electons
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p3
or
[Ar] 4s2, 3d10, 4p3
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Mn: [Ar]4s2 3d?
How many d electrons does Mn have?
4, 5, 6
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Dr. S. M. Condren
Electronic Configuration
negative ions
add electron(s), 1 electron for each negative charge
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Dr. S. M. Condren
Electronic Configuration
S-2 ion
(16 + 2)electrons
1s2, 2s2, 2p6, 3s2, 3p6
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Dr. S. M. Condren
Electronic Configuration
positive ions
remove electron(s), 1 electron for each positive charge
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Electronic Configuration
Mg+2 ion
(12-2)electrons
1s2, 2s2, 2p6
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Dr. S. M. Condren
How many valence electrons are in Cl, [Ne]3s2 3p5?
2, 5, 7
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For Cl to achieve a noble gas configuration, it is more likely that
electrons would be added
electrons would be removed
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Dr. S. M. Condren
Magnetism
• Result of the spin of electrons
• diamagnetism - no unpaired electrons
• paramagnetism - one or more unpaired electrons
• ferromagentism - case of paramagnetism where the substance retains its magnetism
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paramagnetic ferromagnetic
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Trends in thePeriodic Table
• atomic radius
• ionic radius
• ionization energy
• electron affinity
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Dr. S. M. Condren
Atomic Radius
• decrease left to right across a period– as nuclear charge increases, number of
electrons increase; however, the nucleus acts as a unit charge while the electrons act independently, pulling electrons towards the nucleus, decreasing size
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Dr. S. M. Condren
Atomic Radius
• increase top to bottom down a group– each additional electron “shell” shields the
outer electrons from the nuclear charge
Zeff = Z - Swhere Zeff => effective nuclear charge
Z => nuclear charge, atomic numberS => shielding constant
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Dr. S. M. Condren
Atomic Radius
• increases from upper right corner to the lower left corner
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Ionic Radius
• same trends as for atomic radius
• positive ions smaller than atom
• negative ions larger than atom
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Ionic Radius
Isoelectronic Series
• series of negative ions, noble gas atom, and positive ions with the same electronic confiuration
• size decreases as “positive charge” of the nucleus increases
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Dr. S. M. Condren
Ge is a semiconductor. If half of the Ge atoms of a sample of Ge are replaced with Ga atoms, with what element should the other half of the Ga atoms be replaced in order for this new compound to be isoelectronic with Ge?
Sn, As, Se
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Dr. S. M. Condren
Ionization Energy
• energy necessary to remove an electron to form a positive ion
• low value for metals, electrons easily removed
• high value for non-metals, electrons difficult to remove
• increases from lower left corner of periodic table to the upper right corner
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Dr. S. M. Condren
Ionization Energies
first ionization energy
• energy to remove first electron from an atom
second ionization energy
• energy to remove second electron from a +1 ion
etc.
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Dr. S. M. Condren
Electron Affinity
• energy released when an electron is added to an atom
• same trends as ionization energy, increases from lower left corner to the upper right corner
• metals have low “EA”
• nonmetals have high “EA”