Atomic Structure and Models Quiz

The positively charged central core of an atom, containing protons and neutrons. Most of the atom's mass is concentrated in the nucleus.

The negatively charged particles that orbit the atom's nucleus. They have negligible mass compared to the nucleus.

The force that pulls electrons towards the nucleus due to their opposite charges.

The force that pushes electrons away from the nucleus due to their circular motion.

A model of the atom proposed by Rutherford, suggesting that the atom has a small, dense, positively charged nucleus at the center, with negatively charged electrons orbiting around it.

A unique set of colored lines observed when an element's atoms are heated or energized, representing the specific wavelengths of light emitted by them. Each element has its own distinct line spectrum.

It stated that electrons could only occupy specific orbits around the nucleus, each with a fixed energy level. Transitions between these orbits resulted in the emission or absorption of specific wavelengths of light, explaining atomic spectra.

The study of the properties of light emitted or absorbed by atoms, providing crucial insights into the structure and behavior of atoms.

The specific colors (or wavelengths) of light emitted by an excited element, appearing as distinct lines against a dark background.

Dark lines appearing at specific wavelengths within a continuous spectrum, indicating wavelengths that have been absorbed by an element.

Bohr's model described the atom as having a positively charged nucleus surrounded by electrons orbiting in specific energy levels.

Electrons can only exist in specific energy levels around the nucleus, and can jump between these levels by absorbing or releasing energy.

Electrons orbiting the nucleus don't lose energy continuously, but only when transitioning between energy levels.

The amount of energy absorbed or released when an electron jumps between energy levels.

The process where an electron absorbs energy and jumps to a higher energy level.

The process where an excited electron releases energy and returns to a lower energy level, emitting light of a specific wavelength.

Describes the distance of an electron from the nucleus.

Represents the different energy levels within an atom.

Indicates the shape of an electron's orbital.

The difference in energy between electron shells is not equal. This energy difference decreases as you move further from the nucleus.

Determines the number of orbitals within a sublevel and their orientation in space.

The region of space surrounding the nucleus where there's a high probability of finding an electron.

An electron can only move between energy levels by absorbing or emitting a specific amount of energy equal to the difference between the two levels.

A specific region within the electron cloud where there's a high probability of finding a single electron.

The Bohr model successfully explained the spectrum of the hydrogen atom. It introduced quantum numbers to describe electron energy levels and explained why electrons don't radiate energy in the ground state.

States that electrons can only exist in specific energy levels around the nucleus.

The Bohr model failed to explain the spectra of other elements beyond hydrogen. It treated electrons as particles without wave properties and assumed that both position and velocity could be measured simultaneously.

Sommerfeld improved the Bohr model by introducing elliptical orbits for electrons. Each energy level has multiple sub-levels, with one circular orbit and the rest elliptical.

To describe the energy of an electron in an elliptical orbit, Sommerfeld introduced a new quantum number called the azimuthal, or orbital, quantum number (K). It quantifies the energy of electrons in sub-levels.

Electrons in elliptical orbits move at different speeds, travelling faster when closer to the nucleus.

Each spectral line in a hydrogen atom spectrum actually consists of multiple closely spaced spectral lines, indicating that energy levels have sub-levels.

Describes the relationship between the major and minor axes of an oval orbit, using the values 'n' and 'K'.

A principle in quantum mechanics stating that it's impossible to know both the exact position and momentum (velocity) of an electron at the same time.

Regions around the nucleus where there is a high probability of finding an electron. They are described by specific energy levels and shapes, represented by quantum numbers.

A set of four numbers that describe the state of an electron in an atom: principal quantum number (n), azimuthal quantum number (l), magnetic quantum number (ml), and spin quantum number (ms).

The idea that electrons exhibit wave-like behavior, implying they can be both particles and waves.

Schrödinger's equation describes the wave-like behavior of electrons in atoms, allowing us to determine their energy levels and orbitals.

The idea that electrons can only occupy certain energy levels, like steps on a staircase, not continuously varying.

A theoretical model where electrons are constantly moving around the nucleus in specific orbitals, based on their energy levels and shapes.

A sublevel with 3 orbitals, each having a specific shape and orientation in space. They are labeled as Px, Py, and Pz and resemble dumbbells.

A sublevel with 5 orbitals, each having a unique shape and orientation. These orbitals are more complex than 'p' orbitals and have various shapes.

A sublevel with 7 orbitals, each with a distinct shape and spatial orientation. These orbitals are even more complex than 'd' orbitals.

Electrons can only occupy specific energy levels around the nucleus, and they fill up orbitals with lower energy levels first. This rule helps determine the electron configuration of an atom.

This rule states that electrons will individually occupy each orbital within a sublevel before pairing up in any one orbital. This minimizes electron-electron repulsion.

This is the quantum number that describes the direction of an electron's spin as it orbits the nucleus. It can be either +1/2 or -1/2, representing clockwise or counterclockwise spin.

This refers to the number of ways an electron can spin around its axis. This spin creates a magnetic field, and electrons in the same orbital spin in opposite directions to minimize repulsion.

A diagram showing the filling of orbitals in an element's electronic configuration. It helps visualize the distribution of electrons among various atomic orbitals.