The model of the ping-pong balls that are thrown at the window increases the number of lowenergy photons but does not produce any photon with enough energy.
A high-frequency photon is like a baseball thrown at a glass window, breaking it.
The excess energy of the photon is transferred to the electron by the light's frequencies.
The wave explanation of light continued to have explanatory power even though the quantization of light explained the photoelectric effect.
At times light behaves like a particle and at other times it behaves like a wave.
The particular experiment affects which behavior we observe.
No photoelectrons were observed.
The photoelectrons had a kinetic energy of 155 kJ>mol.
The photoelectrons had a kinetic energy of 51 kJ>mol.
The discovery of the particle nature of light broke down the division that existed in nineteenth-century physics between the wave phenomenon and the small particles that compose atoms.
The photoelectric effect suggested the particle nature of light, and certain observations about atoms suggested a wave nature for particles.
In the form of heat, light, or electricity, an atom absorbs energy.
A neon sign is made of glass tubes filled with neon gas.
When an electric current is passed through the tube, the red light from neon atoms absorb some of the electrical energy and reemit it as the familiar red light of sign is emitted by neon atoms that a neon sign.
If the atoms in the tube are different, they emit light that is different in color.
The wavelength of visible light determines its color.
The light emitted by various atoms contains several different wavelength.
The emission spectrum of a particular element is always the same, with bright lines at the same wavelength.
The emission spectrum can be used to identify the element.
Light coming from a distant star has the emission spectrum of the elements that compose the star.
We can identify elements in the star by analyzing the light.
The emission spectrum of hydrogen, helium, and barium is not continuous and consists of bright lines at specific wavelength.
Only certain wavelength of light are present.
Classical physics couldn't explain why the spectrum consisted of lines.
Classical physics says that an atom composed of an electron around a nucleus should emit a white light spectrum.
An atom shouldn't be stable according to classical physics.
Johannes Rydberg, a Swedish mathematician, analyzed many atomic elements.
The component wavelengths are separated by the scurvy.
The light emitted from a hydrogen, helium, or barium lamp has a specific wavelength that can be separated.
The emission spectrum is a characteristic of the element that produced it.
There are only fixed distances from the nucleus for red to exist at any distance from the sun.
When an electron falls from one stable state to another, each line is produced.
The bar code on the items you buy can be read by a laser scanning device.
Each item has a unique code that identifies it.
Each element in the periodic table has a different spectrum.
The emission spectrum of oxygen and neon is shown in Figure 8.13V.
Each spectrum can be used to identify the substance.
There are two bright yellow lines in the emission spectrum of sodium.
When a drop of a solution containing a sodium salt is put into a flame, it glows bright yellow.
Other metals have similar colors in flame tests.
A combination of two or more such lines are represented by each color.
The colors seen in fireworks are formed by similar emissions.
The emission and absorption of calcium, strontium, barium, and strontium have bright lines on a dim background.
The processes that produce them are mirror images.
An electron makes a transition from a higher energy level to a lower one in emission.
The transition from the lower level to the higher one is called absorption.
We can use the emission spectrum to identify the element.
The characteristic color of the light they produce can be used to identify elements.