Quiz 1 Unit 3 Flashcards
Attractions
Electrons to nucleus stronger as it gets closer
Electrons to protons
Protons to neutrons
Light
Comes from electrons
Electromagnetic waves
How Did Four Colors Appear From One Electroned Helium?
When its electron jumps from higher energy level to a lower one, it releases a photon
Those photons cause different colours of light of different wavelengths due to the different levels
Wavelength
Lambda
Upside down Y
Measured by crest to crest or trough to trough
Measured in nanometers
Frequencey
Nu
Fancy V
Number of waves that pass a point in a given time
Measured in cycles, Hertz (Hz), s^-1, or 1/s
Not speed, all waves move at the speed of light
Comparisons
Short wavelength, high frequency, high energy
Long wavelength, low frequency, low energy
Electromagnetic Radiation
Form of energy that exhibits wavelike behaviours as it travels through space
Amplitude
Determines intensity
Measured from middle to crest
Electromagnetic Spectrum
Arrangement of all electromagnetic waves by decreasing wavelength and increasing frequency
Spectrum From High Energy/Frequence to High Wavelength
Gamma, x-ray, ultraviolet, visible, infrared, microwave, TV radio, AM radio, long radio
Equations
C=YV
Y=C/V
V=C/Y
C=Speed of light or 3.00x10^8 m/s
Lambda must be converted to meters
Wavelength Spectrum in Meters
10^-9 X-Ray
10^-8 UV
10^-7 Visible
10^-6 Infra
10^-5 Micro
Photoelectric Effect
Emission of electrons from a metal when light of a certain frequency shines on metal
Quanta
Light does not produce energy continuously, but in packets called quanta
Quantum
Minimum amount of energy lost or gained by an atom due to its energy levels
Quantized Energy
Multiples of quanta in whole number multiples
Energy Equation
E=hv
E=hc/y
E=Energy in joules (J)
h=Planck’s constant (6.626x10^-34 J*s)
v=Frequency
Dual-Wave Particle
Wavelike properties while also a stream of particles
Photon
Particle of electromagnetic radiation having zero mass and carrying a quantum of energy
Moves like waves
Visible Light
Wavelength 10^-7m
Energy 10^19J
Frequency 10^14Hz
Line-Emission Spectrum
Bands of light
Ground State
Atom at its lowest energy level
Excited State
Atoms absorb energy and move energy levels equivalent to amount of energy absorbed
Continuous Spectra
White light that continuosly emits lines of all colors
Line-Emission Spectra
Only certain lines of color are seen
Absorption
Energy added to an atom in order to move an electron from a lower energy level to a higher energy level
Max Planck
Proposed that light emits energy in small packets called quanta
Albert Einstein
Stated that while light has wavelike properties, it is also a stream of particles called photons or the dual wave-particle nature
Emission
When an electron falls to a lower energy level, a photon is emitted
Bohr Model
The electron can only circle the nucleus in allowed paths, called orbits, and there is nothing in between
Electricity
Electrons absorb energy from various sources
