Portage Chemistry Module 3
Lewis Dot Structure
The symbol of an element withdots around it to show number of outer shell
electrons, paired and unpaired.
Atomic size
Distance from the center of the nucleus to the outer shell of an atom, increases
as you go down elements, decreases as you go right as nuclear charge
increases.
Ionization energy
Measure of energy needed to remove an electron from an atom, decreases as
you go down and increases as you go right because of greater nuclear charge.
Electronegativity
Attraction an atom has for its outer shell electrons. Decreases as you go down
since elements are larger and outer electrons are more distant, increases as you
go right because of greater nuclear charge.
Magnetic quantum number (m sub l)
Orientation in space of an orbital and has values of -l to 0 to +l based on angular
momentum number. (which orbital the last electron lands in)
Spin quantum number (m sub s)
Describes direction of the electron spin with value of -1/2 and +1/2 (whether the
electron was 1st or 2nd to enter orbital)
, Angular quantum number (l)
Describes the shape of the orbital within a subshell and is a whole number, s=0
p=1 d=2 f=3 (# of nodal planes in subshell)
Principal quantum number (n)
Size and energy of an orbital (same as shell number)
Schrodinger equation
Erwin Schrodinger, 1926, quantum mechanical model of the atom. Calculated
electron properties of hydrogen in 3D. (Schrodinger equation derived 3 quantum
numbers: n, l, m sub l
de Broglie equation
Louis de Broglie, 1924, the wave theory of the elctron.
- Thought electrons behave as standing waves because they are held in place by
positively charge nucleus, are confined to a region of space and do not travel.
- Each electron orbit must be equal to a whole number times the wavelength of
an electron, otherwise the waves will self destruct.
Wave theory
Wave in orbits which are not equal to a whole number times the electron
wavelength will destroy themselves by interference
Photoelectric effect
Particle property of light which occurs when the visible light interacts with alkali
metals causing electrons (photoelectrons) to be emitted such as in automatic
door openers.
Lewis Dot Structure
The symbol of an element withdots around it to show number of outer shell
electrons, paired and unpaired.
Atomic size
Distance from the center of the nucleus to the outer shell of an atom, increases
as you go down elements, decreases as you go right as nuclear charge
increases.
Ionization energy
Measure of energy needed to remove an electron from an atom, decreases as
you go down and increases as you go right because of greater nuclear charge.
Electronegativity
Attraction an atom has for its outer shell electrons. Decreases as you go down
since elements are larger and outer electrons are more distant, increases as you
go right because of greater nuclear charge.
Magnetic quantum number (m sub l)
Orientation in space of an orbital and has values of -l to 0 to +l based on angular
momentum number. (which orbital the last electron lands in)
Spin quantum number (m sub s)
Describes direction of the electron spin with value of -1/2 and +1/2 (whether the
electron was 1st or 2nd to enter orbital)
, Angular quantum number (l)
Describes the shape of the orbital within a subshell and is a whole number, s=0
p=1 d=2 f=3 (# of nodal planes in subshell)
Principal quantum number (n)
Size and energy of an orbital (same as shell number)
Schrodinger equation
Erwin Schrodinger, 1926, quantum mechanical model of the atom. Calculated
electron properties of hydrogen in 3D. (Schrodinger equation derived 3 quantum
numbers: n, l, m sub l
de Broglie equation
Louis de Broglie, 1924, the wave theory of the elctron.
- Thought electrons behave as standing waves because they are held in place by
positively charge nucleus, are confined to a region of space and do not travel.
- Each electron orbit must be equal to a whole number times the wavelength of
an electron, otherwise the waves will self destruct.
Wave theory
Wave in orbits which are not equal to a whole number times the electron
wavelength will destroy themselves by interference
Photoelectric effect
Particle property of light which occurs when the visible light interacts with alkali
metals causing electrons (photoelectrons) to be emitted such as in automatic
door openers.
