Electronic Structure of the Atom Flashcards

Flashcards covering Unit 2: Electronic Structure of the Atom, based on Chem 1120 lecture notes.

What were John Dalton's and Ernest Rutherford's atomic models, and in what years were they proposed according to the lecture notes?

John Dalton proposed the billiard ball model in $1808$, and Rutherford proposed the nuclear model in $1911$.

How are frequency, wavelength, and amplitude related to the characteristics of light?

Frequency and wavelength are related to the color of light, while amplitude is related to light intensity.

What is the difference between constructive interference and destructive interference of waves?

Constructive interference occurs when waves are in phase, whereas destructive interference occurs when waves are out of phase.

Under what condition does the photoelectric effect occur?

only occurs when the light frequency is greater than the threshold frequency

When light frequency is above the threshold frequency ($\nu > \nu_0$), how do light intensity and light frequency affect the emitted electrons?

The number of emitted electrons depends on the intensity of light, while the kinetic energy of the emitted electrons depends on the frequency .

What is wave-particle duality?

a complete description of light includes both wavelike and particlelike properties.

In atomic emission spectra, what does each individual spectral line represent?

Each line represents an electronic transition from a higher energy level to a lower energy level.

What are the three main postulates of the Bohr Model of the atom?

electrons moves in circular orbits. electrons has a fixed set of allowable orbits electrons can change from one allowable orbit to another

Which spectral series in the hydrogen spectrum corresponds to visible light wavelengths?

The Balmer series, which corresponds to electronic transitions down to the n=2 energy level.

To which energy level do electron transitions fall to emit ultraviolet wavelengths in the hydrogen spectrum?

to the n=1 energy level the Lyman series

What does quantization of energy mean in the context of atomic energy levels?

the energy levels can only have certain specific energy values rather than a continuous spectrum.

How is $E = 0$ defined in the energy state system of a hydrogen atom?

$E = 0$ is defined as when the electron is completely removed from the nucleus.

What is the definition of ionization energy (IE)?

Ionization energy is the minimum amount of energy required to remove $1\text{ mole}$ of electrons from $1\text{ mole}$ of gaseous ground-state atoms.

What are two major limitations or flaws of the Bohr atomic model?

It only works for one-electron systems, and electrons do not actually move in circular orbits.

In two-slit interference, what path length differences lead to constructive and destructive interference?

path lengths differing by a whole wavelength cause constructive interference , while path lengths differing by a half integer wave length cause destructive interference

What concept is demonstrated by comparing these X-ray and electron diffraction patterns of metal foil?

The wave nature of matter (matter/electrons exhibit wave properties).

What does the Heisenberg Uncertainty Principle state?

It states that it is impossible to know simultaneously the exact position and momentum of a particle.