Wave/Particle Duality + Atomic Models Quiz

What is wave-particle duality?

material has certain wave-like characteristics and certain particle-like characteristics

Light is seen as a wave but can have ___ properties.

particle

Electrons are seen as particles but can have ___ properties.

wave

What are the two wave-like properties of light?

electromagnetic radiation and electromagnetic spectrum

What is electromagnetic radiation?

form of energy that exhibits wavelength behavior as it travels through space

What is electromagnetic spectrum?

all electromagnetic radiation arranged according to increasing wavelength

What is wavelength? What variable represents it?

distance between corresponding points (crest to crest, trough to trough), upside down y

What unit is used for wavelength?

m

What is frequency? What variable represents it?

number of waves that pass a given point in a specific time (ex. waves per second), cursive v

What is the SI Unit for frequency, and what is it equivalent to?

Hertz (Hz), 1 wave per second (also written as 1 s^-1)

What is the equation to relate frequency an wavelength?

c = upsidedownY x cursiveV

Wavelength and frequency are ___ of one another. What is another way to say this?

reciprocals, inversely proportional

What are the two phenomena that suggest particle-like characteristics of light (could not be explained by the wave theory of light)?

photoelectric effect, line-emission spectrum

What is the photoelectric effect?

light at a particular frequency shines on CERTAIN metals and electrons called photoelectrons are emitted

Referring to the photoelectric effect, no matter how long a light shines on metal, electrons are not emitted unless the light is of a certain ___.

frequency

To be emitted, electrons have to ___ a certain amount of ___. (In relation to photoelectric effect)

absorb, energy

What is a quantum (plural: quanta)?

specific amount of something (in this lesson's case, energy)

What is a quantum of light?

finite quantity of energy that can be gained or lost by an atom

What equation is used to show the relationship of energy and frequency?

E = h x cursiveV

What SI unit is used for energy?

Joules

What is h? What is its value?

Planck's constant, 6.63 x 10^-34 J*s

In 1905, ___ suggested wave-particle duality.

Einstein

What is a photon?

individual quantum of light

Photons are thought of as a "particle of electromagnetic radiation" having ___ mass and carrying a ___ _ ___.

zero, quantum of energy

What is emission spectrum?

spectrum of lines that represent the emissions of photons with certain energies

What is an atom's ground state?

lowest energy

When energy is shot through electrons, the energy is given off in the form of ___ when the atoms returns to the ___ ___. The light is passed through a ___ so the light is separated into different lines. (in relation to line-emission spectrum)

light, ground state, prism

Each line represents emissions of photons with certain ___.

energies

What is the Balmer series?

visible

What is the Lymen series?

ultraviolet

What is the Paschen series?

infrared

What is spectroscopy?

spectroscope used to separate light given off from substances into line spectra

Line spectra can be used to what?

identify atoms of a certain substance (like a fingerprint)

In Bohr's atomic model, there were ___ allowed paths.

specific

In Bohr's atomic model, the ___ energy orbit is ___ to the nucleus. Electrons must ___ energy to move up to another orbit.

lowest, closest, gain

In Bohr's atomic model, each orbit (or path) had a ___ amount of energy.

fixed

In Bohr's atomic model, atoms' electrons were connected with ___ ___. When electrons move down from higher to lower energy levels, they emitted ___.

line spectra, photons

What were the two main problems with Bohr's model?

only true with hydrogen atom, didn't explain chemical behaviors of atoms

___ ___ suggested that electrons have ___-like properties.

Louis DeBroglie, wave

What properties do electrons have that are similar to waves?

diffraction, interference

Many people would not accept that an electron could act like a wave until the what?

Heisenberg Uncertainty Principle

What did the Heisenberg Uncertainty Principle state?

impossible to measure the velocity, which highly depends on energy, and position of electron at the same time

What did Edwin Schrodinger do?

developed mathematical equation that described how electrons move around the nucleus as waves - quantum theory

Unlike Bohr's atomic model, Schrodinger's equations did what?

worked for all atoms (not just hydrogen)

Schrodinger's equation gives what?

probability of where to find electrons in atoms

Schrodinger also developed different possible whats that the electrons occupy?

cloud shapes

What is quantum theory?

describes mathematically the wave properties of electrons and other small particles

What are orbitals?

3D region around nucleus that indicates possible location of an electron

The shape and size of electron clouds depend on the ___ of the electrons that occupy them.

energies

What are four examples of electromagnetic radiation?

radio waves, microwaves, ultraviolet, gamma

Which travels at a greater speed, ultraviolet or infrared light?

neither, both travel at speed of light

Which has a longer wavelength, green or yellow light?

yellow