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6
...
99792458 * 108 m/s or 3
...
• λ units are meters
• ν units are reciprocal seconds (s-1)
• c = speed
*Nanometer = 10-9m
*Centimeter =
10-2m
Electromagnetic Wave: a wave that has an electric field component and a magnetic field
component
• These two components have the same wavelength and frequency, and hence
component
• These two components have the same wavelength and frequency, and hence
the same speed, but they travel in mutually perpendicular planes
...
6
...
Quantum: the smallest quantity of energy that can be emitted (or absorbed) in the form of
electromagnetic radiation
• E = energy
• h = Planck’s constant (6
...
Photoelectric Effect: a phenomenon in which electrons are ejected from the surface of a metal
exposed to light of at least a certain minimum frequency called the threshold frequency
...
602 * 10-19J
*The more energetic the photon (i
...
the higher its frequency), the greater the kinetic energy of
the ejected electron
...
*Light possesses properties characteristic of both particles and waves
...
6
...
• λ = wavelength of a line in the spectrum
• R∞ = Rydberg constant (1
...
*The energy of a free electron is assigned the value of 0
...
*The most negative value is reached when n = 1, which corresponds to the most stable energy
state
...
Excited State: a state that is higher than the ground state
*The radius of each circular orbit in Bohr’s model depends on n2
...
*The higher the excited state, the farther away the electron is from the nucleus
...
4: Wave Properties of Matter
Nodes: a collection of points at which electron density in an atom is 0; amplitude of the wave at
this point is 0
• r = radius of the orbit
• λ = wavelength of the electron wave
• n = a positive integer
*Because n is an integer, r can only have certain values (integral multiples of λ) as n increases
...
*de Broglie’s reasoning led to the conclusion that waves can behave like particles and particles
can exhibit wavelike properties
...
9)
6
...
*Even in the most favorable conditions for measuring the position and velocity, the product of
the uncertainties can never be less than h/4π, hence the = sign
...
*The Schrodinger equation specifies the possible energy states the electron can occupy in a
hydrogen atom and identifies the corresponding wave functions
...
6: Quantum Numbers
Quantum Numbers: numbers required to describe arrangement of electrons in an atom
1
...
The larger n is, the greater the average distance of an electron in the
orbital from the nucleus and therefore the larger the orbital
...
n can have integral values of 1, 2, 3, …
2
...
For a given value of n, the possible values of ℓ range from 0 to n-1
...
The value of ℓ is designated by the letters s, p, d, and f
...
A collection of orbitals with the same value of n is frequently called a
shell
...
One or more orbitals with the same n and ℓ values are referred to as a
subshell
...
Magnetic Quantum Number (mℓ): describes
the orientation of an orbital in space; depends on the value of ℓ
...
The number of mℓ values indicates the number of orbitals in a subshell
with a particular ℓ value; each mℓ value refers to a different orbital
...
The number of subshells in a shell is equal to n
...
The number of orbitals in a subshell is equal to
2ℓ+1
...
Electronic Spin Quantum Number (ms): the fourth quantum number that
differentiates two electrons in the same orbital
a
...
Because there are two possible directions of a spin (counterclockwise
and clockwise), opposite each other, ms, has two possible values: +½
and -½
...
Two electrons in the same orbital with opposite spins are referred to as
“paired
...
These three quantum numbers indicate the size (n), shape (ℓ), and orientation (mℓ) of the orbital
...
6
...
p Orbital: atomic orbital in which the angular momentum quantum number (ℓ) is 1
• There is a p subshell in every shell for which n > 2, and each p subshell
contains three p orbitals (px, py, and pz)
• 3 subshells are identical in size, shape, and energy; they differ in orientation
d Orbital: atomic orbital in which the angular momentum quantum number (ℓ) is 2
• All the 3d orbitals are identical in energy and are labeled with subscripts
denoting their orientation with respect to the x, y, and z axes
...
And as
energy increases, n increases
...
ℓ = 0 → s orbital, one per shell
ℓ = 1 → p orbital, 3 per shell
ℓ = 2 → d orbital, 5 per shell
ℓ = 3 → f orbital, 7 per shell
6
...
*Orbital energies in a one-electron system depend only on the value of n
...
*In a many-electron atom, for a given value of n, the energy of an orbital increases with
increasing value of ℓ
...
*A maximum of two electrons may occupy an atomic orbital, and the two electrons must have
opposite spins, referred to as paired spins
...
General Rules for Writing Electron Configurations
1
...
2
...
3
...
4
...
9: Electron
Configuration and the
Periodic Table
Noble Gas Core: a representation in
an electron configuration that shows
in brackets the most recently
completed noble gas
• All elements except hydrogen and
helium
*Transition Metals either have incompletely filled d subshells or readily give rise to cations that
have incompletely filled d subshells