Chapter 6 Flashcards
The intensity of a light is a function of the waves______
Amplitude
A point of zero amplitude
A node
Unit of frequency
Cycles per second or hertz
As wavelength increases, frequency and energy ________
Decrease
Max Planck proposed that light waves existed as discrete packets of energy known as…
Quanta
Ultraviolet catastrophe
According to classical physics, the intensity of emitted light approaches infinity as the wavelength approves zero (incorrect)
Predictions failed in the UV region
Light acts as….
Waves and particles
An object can gain or lose energy by absorbing or emitting radiant energy in…..
Quanta
Quanta of energy
Smallest unit of energy that may be emitted as radiation
Electrons can only go up or down_____levels
Entire
Quantization is the….
Only specific energies that are allowed
Certain metals will____electrons when light strikes the metal surface
(Excited electrons, think of flame test)
Release (energy must exceed a threshold energy first)
Blackbody radiation
Theory that a body absorbs all of the radiation that falls on it
Packets of energy
Photons
There is a 1:1 correspondence between ejected electrons and______
Light waves
Credited with the first modern model of the hydrogen atom based on the “line spectra” of atomic emission sources
Bohr
Proposed a “planetary” structure for the atom where the electrons circled the nucleus in….
Defined orbitals
(Attractive electrostatic forces of the electron and nucleus were balanced by the centripetal forces of the orbiting electron)
When ______light passes through a prism, all of the colors of the rainbow are observed
White
When the light from a discharge tube containing a pure element is passed through the same prism….
Only certain colors are observed (emission spectrum)
Wavelength red presents the distance between one complete______
(Wavelength)
Cycle
The lines on the line spectrum indicate…
Jumps between allowed energy levels
Wave duality
Electron has the properties of lights and waves
De brogli
Heisenberg uncertainty principle
Impossible to determine exact position and velocity of electron
Schrodinger
Determined that matter could be described as a wave, came up with orbitals
The behavior of an electron in the atom can be described as….
Is standing wave
Pauli exclusion principal
No 2 electrons have the same quantum numbers
The importance of E =mc ^2
Energy has mass
Electromagnetic radiation can be thought of as..:
A stream of particles called photons
Diffraction results when…
Iight is scattered from a regular array of points or lines
T or F
All matter exhibits either particulate or wave properties exclusively
F
The 4 lines observed in the visible emission spectrum for hydrogen tell us that…
Only certain energies are allowed for the electron in a hydrogen atom
Criticism of the Bohr model of the atom
Does not adequately predict the ionization energy of the valence electrons for elements other than H
Bohr’s model correctly describes….
Only the H atom
Orbital
Space where electrons are most likely to be found
Can the movement of electrons be determined?
No
The size of an orbital is_____defined
Arbitrarily
How to find electrons in n=___
n^2 * 2 (electrons)
The lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli principle in a particular set of degenerate orbitals
Hund’s rule
n describes the….
Principle quantum number
Energy level, row on periodic table, size of orbital
n represents the…
Subshell
l is the_____quantum number
Angular momentum
l represents the
Subshell (shape of orbital)
l equals…
0 to n-1 values
The # of nodes (space that no electrons occupy)
ml represents the _______quantum number
Magnetic
ml equals
-l to +l
ms represents the_____quantum number
ms equals…
Spin
-1/2 or +1/2
The number of orbitals having a given value of l is equal to…
2l + 1
