Bohr Model of the Atom Quiz- general chem 2

<p>$E = \frac{hcR}{n^2_{Upper} - n^2_{Lower}}$ (B)</p> Signup and view all the answers

<p>It can only describe hydrogen-like atoms (A)</p> Signup and view all the answers

<p>Rydberg constant (C)</p> Signup and view all the answers

<p>Lyman series (D)</p> Signup and view all the answers

<p>They contain only one electron but can have a different nuclear charge (D)</p> Signup and view all the answers

<p>It does not account for electron spin. (A)</p> Signup and view all the answers

<p>The principal quantum number n (B)</p> Signup and view all the answers

<p>Rydberg constant (B)</p> Signup and view all the answers

<p>Balmer series (C)</p> Signup and view all the answers

<p>By allowing electrons to fall between defined energy levels (D)</p> Signup and view all the answers

<p>$p = nh/2\pi r$ (D)</p> Signup and view all the answers

<p>The size of the orbital. (D)</p> Signup and view all the answers

<p>Their energy levels can be predicted using the Bohr model. (D)</p> Signup and view all the answers

<p>The charge of the nucleus (B)</p> Signup and view all the answers

<p>The angular momentum must be a fraction of $h$ (B)</p> Signup and view all the answers

<p>Potential energy (Un) (A)</p> Signup and view all the answers

<p>The Bohr radius is directly proportional to 'n'. (A)</p> Signup and view all the answers

<p>656.3 nm (B)</p> Signup and view all the answers

<p>Hydrogen (H) (A)</p> Signup and view all the answers

<p>1.097 x 10^7 m^-1 (C)</p> Signup and view all the answers

<p>Energy levels are adjusted by Z². (B)</p> Signup and view all the answers

<p>Mass of the electron. (D)</p> Signup and view all the answers

<p>n=3 to n=2 (D)</p> Signup and view all the answers

<p>It only includes the Balmer series. (B)</p> Signup and view all the answers

<p>Davison series (D)</p> Signup and view all the answers

<p>Energy increases as n². (C)</p> Signup and view all the answers

<p>Energy emission and absorption in hydrogen. (C)</p> Signup and view all the answers

<p>The size of the energy gap (B)</p> Signup and view all the answers

<p>L = nh/2π (C)</p> Signup and view all the answers

<p>λ = h/p (C)</p> Signup and view all the answers

<p>$F_e = F_c$ (D)</p> Signup and view all the answers

<p>Hydrogen-like atoms (C)</p> Signup and view all the answers

<p>Orbital radius (r) (C)</p> Signup and view all the answers

<p>Quantization of angular momentum (D)</p> Signup and view all the answers

<p>An electron changing orbits (D)</p> Signup and view all the answers

<p>The spatial distribution of the electron (A)</p> Signup and view all the answers

<p>Speed increases with decreasing distance (A)</p> Signup and view all the answers

<p>Minimum radius of an electron orbital (D)</p> Signup and view all the answers

<p>Higher energy and larger radial distances (C)</p> Signup and view all the answers

<p>It relates to the energy levels of the hydrogen atom (A)</p> Signup and view all the answers

<p>$E = hcR( \frac{1}{n_{Upper}^2} - \frac{1}{n_{Lower}^2})$ (B)</p> Signup and view all the answers

<p>Energy is bound to the atom (B)</p> Signup and view all the answers

<p>$p = mvr = n \frac{h}{2\pi}$ (D)</p> Signup and view all the answers

<p>1.89 eV (D)</p> Signup and view all the answers

<p>By summing potential energy and kinetic energy (D)</p> Signup and view all the answers

<p>Potential Energy (D)</p> Signup and view all the answers

<p>Principal quantum number (A)</p> Signup and view all the answers

<p>656.3 nm (C)</p> Signup and view all the answers

<p>It fails to account for their complexities. (C)</p> Signup and view all the answers

<p>The quantum state of the electron (C)</p> Signup and view all the answers

<p>En → ZEn (D)</p> Signup and view all the answers

<p>Lyman series (A)</p> Signup and view all the answers

<p>Wavelength of the Balmer Hα line (B)</p> Signup and view all the answers

<p>Determines the wavelength of emitted light (D)</p> Signup and view all the answers

<p>It fails to indicate the rate of transitions. (D)</p> Signup and view all the answers

<p>Lithium (C)</p> Signup and view all the answers

<p>UV series (D)</p> Signup and view all the answers

A theoretical model that describes the structure of the hydrogen atom. It suggests electrons orbit the nucleus in specific, quantized energy levels.

A formula used to calculate the wavelengths of spectral lines in hydrogen-like atoms.

A fundamental constant in physics, used in the Rydberg equation. It relates to the energy levels and wavelengths in Hydrogen-like atoms.

Distinct frequencies of light emitted by a hydrogen atom when its electrons transition between energy levels.

Atoms with a single electron, such as hydrogen and singly ionized helium.

A specific spectral line in the visible light spectrum of hydrogen, calculated using the Rydberg equation.

The Bohr model, while successful for hydrogen, fails to accurately predict the spectra of more complex atoms.

The pattern of spectral lines emitted by atoms, when electrons are excited and transition between energy levels.

The movement of an electron between different energy levels in an atom.

A more generalized and accurate theory that explains atomic and molecular behavior, and where the Bohr model is insufficient to fully explain.

The angular momentum of an electron in an atom can only take on certain discrete values. Specific amounts.

Electrons in atoms don't travel randomly, but in specific, pre-defined paths or orbits around the nucleus.

A spectrum with specific lines/colors representing energy levels.

Distinct energy states associated with the allowed electron orbits.

The concept that certain physical properties (in this case, energy and angular momentum) can only take on specific, distinct values, like steps on a staircase.

Waves associated with particles, in this case, the electron.

A wave that appears to stay in one place, not moving forward or backward, because its ends are fixed.

The force of attraction between opposite charges.

The force that keeps an object moving in a circular path.

The smallest possible radius of an electron's orbit in a hydrogen atom, according to the Bohr model.

An integer that determines the energy level and radius of an electron's orbit in the Bohr model. Higher 'n' means larger radius and higher energy.

It proposes that electrons orbit the nucleus in specific, quantized energy levels and can jump between these levels by absorbing or emitting photons of light.

The energy of an electron in a hydrogen atom is given by En = -me^4/(8ε0^2h^2n^2), where 'n' is the principal quantum number.

When an electron jumps from a higher energy level to a lower one, it emits a photon with energy equal to the difference between the two levels. These emitted photons correspond to specific spectral lines.

A fundamental constant that appears in the formula for calculating the energy of hydrogen's spectral lines.

The Bohr model predicts the specific frequencies of light that hydrogen emits when its electrons jump between energy levels. These frequencies correspond to the observed spectral lines.

It only applies to hydrogen-like atoms with one electron. It doesn't explain the spectra of multi-electron atoms, spin, or the Heisenberg Uncertainty Principle.

Each photon emitted during an electron transition between energy levels has a specific frequency. These frequencies correspond to the distinct spectral lines observed in the atomic spectra.

Use the formula: EUpper - ELower = hcR(1/nLower^2 - 1/nUpper^2), where 'n' is the principal quantum number, 'R' is the Rydberg constant, and 'h' and 'c' are Planck's constant and the speed of light.

A model of the atom where electrons orbit the nucleus in specific, quantized energy levels.

Electrons can only exist in specific energy states, not anywhere in between.

The energy of a photon is determined by the difference in energy between the two energy levels involved in an electron transition.

The Bohr model successfully explains the line spectrum of hydrogen, which is why it is important.

The de Broglie equation relates the momentum of a particle to its wavelength.

Distinct colors of light emitted by atoms when electrons transition between energy levels.

The Bohr model only works for simple atoms like hydrogen and cannot explain more complex atoms.

It's a fundamental constant used in the Rydberg equation, helping us calculate hydrogen's spectral lines.

When an electron jumps between energy levels, it emits or absorbs a photon with a specific energy, resulting in a spectral line.