Chapter 7 - Quantum Theory and the Electronic Structure of Atoms Flashcards
Entities emit energy only in discrete quantities or ———
Quanta
Vibrating disturbance by which energy is transmitted
Wave
Distance between identical points in succesive waves
Wavelength
Symbol for wavelength
Lambda
The number of waves that pass through a particular point in 1 second
Frequency
Symbol for frequency
Nu
Vertical distance from the midline of a wave to the peak or trough
Amplitude
Product of wavelength and its frequency
Speed
Two components of electromagnetic wave that’s perpendicular to each other
Electric Field
Magnetic Field
The emission and transmission of energy in the form of electromagnetic waves
Electromagnetic radiation
Smallest quantity of energy that can be emitted (or absorbed) in the form of electromagnetic radiation
Quantum
Planck’s constant
6.63x10^-34 J•s
Electrons are ejected from the surface of certain metals exposed to light to at least a certain minimum frequency
Photoelectric effect
Particles of light
Photons
Either continuous or line spectra or radiation emitted by substances
Emission spectra
Light emission only at specific wavelengths
Line spectra
Rydberg constant
2.18x10^-18 J
Lowest energy state of a system
Ground state or ground level
Higher in energy than the ground state
Excited state or excited level
Bohr model only worked succesfully on ————-
Hydrogen and hydrogenlike ions
It is impossible to simultaneously both the momentum p and the position of a particle with certainty
Heisenberg uncertainty principle
Gives the provability that an electron will be found in a particular region of an atom
Electron density
Wave function of an electron in an atom
Atomic orbital
Tells the energy of an atom
Average distance of an electron to the nucleus from an orbital
Principal quantum number
Shape of the orbital
Angular momentum quantum number
Orientation of the orbital
Magnetic quantum number
Direction of the spin
Electron spin quantum number
Hydrogen orbital energy
Same number same energy
Many- electron orbital energy
See electronic configuration
How the electrons are distributed among the various atomic orbitals
Electronic configuration
No two electrons can have the same set of quantum number
Pauli’s exclusion principle
Contains unpaired spins and attracted by a magnet
Paramagnetic
Does not contain unpaired spins and slightly repelled by magnet
Diamagnetism
The most stable arrangement of electrons in subshells is the one with the greatest number of parellel spins
Hund’s rule
Protons are added one by one to the nucleus to build up the elements, electrons are similarly added to the atomic orbitals
Aufbau principle
Second last row
Lanthanides or rare earth series
Last row of elements
Actinides
Enables us to predict and understand the critical role that electrons play in chemistry
Quantum Theory
Proponent of Quantum Theory and when
1900
Max Planck
2 natures if light
Wave
Particle
Proponent of photoelectric effect
Einstein (1905)
Electron can only have specific energy values
Light is emitted when electrons move from one energy to lower energy
Bohr’s model of the atom
De broglie wavelength formula
Wavelength = h/(m)(u)
h = j•s m = kg u = m/s
Equation that describe both particle and wave nature of the electron
Schrodinger wave equation
Symbol for wave equation
Pitchfork na maarte yung sides tapos flat yung gitna
Electrons with the same value of:
A. n
B. n and l
C. n, m, and ml
Shell
Subshell
Orbital
