Electronic Structure of Atoms Flashcards
Refers to how electrons are arranged within an atom.
Electronic structure of atoms
Refers to the arrangement of electrons in an atom’s orbitals.
Electron configuration
A positively charged atomic element.
Proton
A neutrally charged atomic element.
Neutron
The center of an atom, composed of the proton(s) and the
neutron(s).
Nucleus
A negatively charged atomic element that orbits the nucleus.
Electron
An atom that has either gained or lost an electron causes the atom to become either negatively or positively charged,
respectively.
Ion
The outermost orbital shell of an atom.
Valance shell
The electron/s in the outermost orbital shell of an atom is called its ________________.
Valence electron/s
This model is also known as the nuclear model of an atom.
Rutherford’s atomic model
It describes the atom in a model wherein the center
is a nucleus composed of protons and neutrons, which contain most of its mass.
Rutherford’s atomic model
A model that shows that the nucleus is surrounded by electrons, which occupy most of its volume.
Rutherford’s atomic model
This model does not fully explain the behavior and arrangement of electrons in the space around the nucleus.
Rutherford’s atomic model
He suggested that electrons do not emit energy while orbiting the nucleus but instead exist in stationary states with constant energy.
Niels Bohr
In this model, it is proposed that the electrons encircle the nucleus in their respective orbits. The electrons are not allowed to occupy spaces in between the orbits. The farther
the orbits from the nucleus, the higher the energy.
Bohr’s Atomic Model
This is the pairing of electrons in electron configuration. Every orbital in a sublevel is singly occupied before any orbital is doubly occupied.
Hund’s rule
An electron configuration principle that states that as electrons are added to “build up” the elements, each electron is placed in the lowest energy orbital
available.
Aufbau principle
Aufbau means ________ in German.
Building up
An electron configuration principle that states that in an atom or molecule, no two (2) electrons can have the same four (4) electronic quantum numbers. As an orbital can contain a maximum of only two (2) electrons, the two (2) electrons must have opposing spins.
Pauli Exclusion principle
This describes the position and energy of the electron in an atom.
Quantum numbers
A quantum number that refers to the number of the energy level.
Principal quantum number (n)
This quantum number indicates the subshell in which an electron can be found. It corresponds to the shape of
the orbital.
Azimuthal (l)
Shape of s-orbital
Spherical
Shape of p-orbital
Dumbbell
Shape of d-orbital
Clover
Shape of f-orbital
Complex
A quantum number that describes the orientation in space of a particular orbital.
Magnetic quantum number (ml)
A quantum number that indicates the orientation of the angular momentum of an electron in an atom.
Electron spin quantum number (ms)
This theory was proposed by __________ in 19th century that states that energy is transferred in discrete packets, or quanta, and that the energy of a quantum is directly proportional to the frequency of radiation.
Max Planck
A theory that explains how energy is transferred in discrete packets, or quanta, and that the energy of a quantum is directly proportional to the frequency of radiation.
Planck’s Quantum Theory
Energy is always emitted in integral multiples of hv, postulated that the energy of a particular quantum
of radiant energy could be described by the equation:
E = h c/λ
Photoelectric effect was contributed by ______________, five years after Planck presented his Quantum Theory.
Albert Einstein
A phenomenon in which electrons are ejected from the surface of certain metals exposed to light of
at least a certain minimum frequency.
Photoelectric effects
Particles of light are called ________, which possess energy.
Photons
Formula for photoelectric effect
E = hv
Planck’s Constant
6.626×10^-34 J*s
Speed of light
3.0×10^8 m/s
