Question | Answer |
Which form of energy exhibits wavelike behavior as it travels through space? | Electromagnetic radiation |
What do all the forms of electromagnetic radiation form? | The Electromagnetic spectrum |
Define Wavelength. | Wavelength is the the distance between corresponding points on adjacent waves. |
Define Frequency | Frequency is the number of waves that pass a given point in a specific time, usually one second. |
What is the wavelength of Visible Light? | Visible light is elctromagnetic radiation with a wavelength of 400-750nm. |
What is the velocity of all electromagnectic radiation in a vacuum? | 300000 kilometers per second |
photoelectric effect=the emission of electrons from a metal when light shines on the metal. | |
quantum =the minimum quanity of energy that can be gained or lost by an atom. | |
Planck’s Constant =E=hv it is the h. it is a fundamental physical constant. | |
Photon =a particle of electromagnetic radiation that has zero rest mass and carries a quantum of energy. | |
Energy of a Photon=6.5 x 1014 Hz | |
Ground State=the lowest energy state of an atom. | |
Excited State=a state in which an atom has a higher potential energy than it has in its ground state. | |
Line=emission spectrum-a series of specific wavelengths of emitted light created when the visible portion of light from excited atoms is is shined through a prism. | |
continuous spectrum = the emission of a continuous range of frequencies of electromagnetic radiation. | |
Bohr radius= Atomic fundamental physical constant used as atomic unit of length | |
Interference=This occurs when waves overlap. | |
Heisenberg Uncertainty Principle=it is impossible to determine simultaneously both the position and velocity of an electron or any other particle. | |
Quantum Theory or Quantum Mechanics=a mathematical description of the wave properties of electrons and other small particles. | |
Orbital =a three dimensional region around the nucleus that indicates the probable location of an electron. | |
Quantum numbers=a number that specifies the properties of atomic orbitals and the properties of electrons in orbitals. | |
Principle Quantum number (n)=the quantum number that indicates the main energy level occupied by the electron. | |
Angular momentum quantum number (l )=the quantum number that indicates the shape of the orbital. | |
Magnetic quantum number (m)=the quantum number that indicates the orientation of an orbital around the nucleus. | |
Spin quantum number (s)=the quantum number that has only two possible values, +1/2 and -1/2, which indicate the two fundamental spin states of an electron in orbital. | |
Aufban Principle=an electron occupies the lowest energy orbital that can receive it. | |
Electron Configuration =the arrangement of electrons in an atom. | |
Pauli Exclusion Principle=no two electrons in the same atom can have the same set of four quantom numbers. | |
Hund’s Rule=orbital of equal energy are occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupies orbitals must have the same spin. | |
Valence Electron =an electron that is available to be lost, gained, or shared in the formation of chemical compounds. | |
Inner-shell electrons=an electron that is not in the highest occupied energy level. | |
Highest occupied level =the electron containing main energy level with the highest principal quantum number. | |
Noble Gas Configuration= an outer main energy level fully occupied, in most cses, by eight electrons. | |
s sublevel or sub-orbital =An “s” orbital occurs alone,The shape of an “s” orbital is spherical | |
p sublevel or sub-orbital=The shape of a “p” orbital is like a dumbbell, they are two lobes arranged along a straight line with the nucleus between the lobes | |
f sublevel or sub-orbital -=hey occur in group of seven,These orbitals have complex shapes | |