Chemistry Chapter 4 "Arrangement of Electrons in Atoms" Flashcards
Continuous spectrum
The emission of a continuous range of frequencies of electromagnetic radiation
Electromagnetic radiation
Which is a form of energy that exhibits wavelike behavior as it travels through space.
Electromagnetic spectrum
Together, all of the forms of electromagnetic radiation form the electromagnetic spectrum
Excited state
A state in which an atom has a higher potential energy than it has ground state
Frequency
Frequency (v) is defined as the number of waves that pass a given point in a specific time, usually one second.
Ground state
The lowest energy state of an atom
Line-emission spectrum
When a narrow beam of the emitted light was shined through a prism it was sparated into a series of specific frequencies of visible light. The bands of light were part of what is known as hydrogen’s line-emission spectrum.
Photoelectric effect
The photelectric effects refers to the emission of electrons from a metal when light shines on the metal.
Photon
Is a particle of electromagnetic radiation having zero mass and carrying a quantum of energy.
Quantum
Is the minimum quantity of energy that can be lost or gained by an atom
Wavelength
is the distance between corresponding points on adjacent waves
Angular momentum quantum number
Symbolized by 1, indicates the shape of the orbital
Electron configuartion
The arrangement of electrons in an atom is known as the atom’s electron configuration
Heisenberg uncertainty principle
States that it is impossible to determine simultaneously both the position an velocity of an electron or any other particle
Magnetic quantum number
Symbolized by m, indicates the orientation of an orbital around the nubleus
Orbital
is a 3 dimensional region around the nucleus that indicates the probable location of an electron
Principal quantum number
Symbolized by n, indicates the main energy level occupied by the electron
Quantum number
Specify the properties of atomic orbitals and the properties of electrons in orbitals
Quantum theory
Describes mathematically the wave properties of electrons and other small particles.
Spin quantum number
Has only two possible values (+1/2-1/2) which indicates the two fundamental spin states of an electron in an orbital
Aufbau principle
An electron occupies the lowest-energy orbital that can receive it
Highest occupies level
Is the electron-containing main energy level with the highest principal quantum number
Hund’s rule
Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin.
Inner-shell electrons
which are electrons that are not in the highest occupied energy level
Noble gases
the group 18 elements
Noble-gas configuration
is an outer main energy level fully occupied in most cases by eight electrons
Pauli exclusion principle
No two electrons in the same atom can have the same set of four quantum numbers
