Chapter 11 Flashcards
Length of a wave (measured in nm); the distance between peaks
Wavelength (T)
Energy transmitted from one place to another by light in the form of waves
Electromagnetic radiation
The vertical distance from the middle of the wave to the crest/trough
Amplitude
The top of a wave
Peak/crest
The number of waves that pass through a specific point in a given amount of time (measured in waves/sec or hertz (Hz)
Frequency (V)
Waves of electromagnetic radiation from short to long
Gamma rays, x-rays, ultraviolet, visible light, infrared, microwaves, radio waves
Light shining on a metal emits electrons
Photoelectric effect
Packets of light (quantum); particles of electromagnetic radiation (have no mass)
Photons
Planck’s equation
E=h•V
H= 6.626•10^-34
Speed of light equation
C=T•V
C=3.0•10^8
Rainbow colors within a given range
Continuous spectrum (visible spectrum)
Consists of several distinct lines of color each with its own frequency; each element has one
Bright line spectrum (line emission spectrum)
Finite quantity of energy that can be gained or lost by an atom
Quantum
Lowest energy state
Ground state
Atom has higher potential energy than at ground state
Excited state
Describes mathematically the wave properties of electrons and other very small particles
Quantum Theory
Properties of orbitals and electrons in the orbitals
Quantum numbers
3-D place around the nucleus that indicates the probable location of an electron
Orbital
Main energy level occupied by an electron; as it increases so does electrons energy and distance (1-7)
Principle quantum number (n)
Sublevels (l) indicate the shape of the orbital (s,p,d,f)
Angular momentum quantum number
Orientation of an orbital around a nucleus
Magnetic quantum number
Two values (Clockwise or counterclockwise)
Spin quantum number
Arrangement of electrons in an atom
Electron configuration
It is impossible to determine simultaneously both the position and velocity of an electron or other particles
Heisenberg principle
An electron occupies the lowest energy level that can receive it
Aufbau principle
No two electrons in the same atom can have the same set of four quantum numbers
Pauli exclusion principle
Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron; all electrons in singly occupied orbitals have the same spin
Hund’s rule
Electron containing main energy level with highest principle quantum number
Highest occupied level
Not in highest energy level
Inner shell electrons
N=______
N^2=______
2N^2=______
Energy level
Number of orbitals on that energy level
Number of total electrons on that energy level
Electrons in the outermost s and p orbitals
Valence electrons
5-10 rule
Chromium and copper
The energy required to remove one outer electron from an atom
Ionization energy
The distance from the nucleus to the outer electron shell
Atomic radius
Energy associated with an atom gaining an electron
Electron affinity
A number that describes the relative ability of an atom (when bonded) to attract electrons
Electronegativity
__________decreases from left to right and increases from top to bottom
Atomic radius
__________increases from left to right and decreases from top to bottom
Ionization energy, electron affinity, and electronegativity
Nonmetal reactivity ______ from top to bottom
Decreases
Metal reactivity ______ from top to bottom
Increases
The left side of the electromagnetic radiation spectrum has ____ wavelength, ____ frequency, and ____ energy while the right side has ____ wavelength, ____ frequency, and ____ energy
Short High High Long Low Low
