Quantum Mechanical Model of an Atom

Tiny particles smaller than an atom, each having different charges and locations within an atom.

A positively charged subatomic particle.

A neutrally charged subatomic particle.

A negatively charged subatomic particle.

The number of protons in an atom.

The mass of an atom.

The specific way electrons are organized around an atom's nucleus.

A substance composed of atoms of the same type.

The process where certain elements (metals) produce specific colors of light when heated in a flame.

Compounds containing a metal and another element. They cause characteristic colors when heated.

Different elements produce different colors of light when heated in a flame.

An instrument that precisely analyzes the light emitted by elements. It reveals narrow spectral lines.

A series of distinct lines found in the light emitted by an (heated) element.

Different energy states within an atom that produce the spectral lines when excited.

A chemical element that produces a yellow flame color.

A chemical element that produces a yellow-green flame color.

This table displays contact information, likely for different individuals or organizations.

A sequence of digits used to reach a specific person or organization by phone.

The first few digits of a phone number, often indicating a specific region or area code.

A wireless phone that can be used to make calls and send text messages from different locations.

A traditional wired phone connected to a fixed location, often used in homes or offices.

The s-orbital has a spherical shape.

The p-orbital has a dumbbell shape (bilobate).

The d-orbital has a clover or quadrilobate shape.

The f-orbital has a more complex shape, like a d-orbital but split.

Describes the main energy level of an orbital (n=1 to 7).

Describes the subshell (s, p, d, f).

Describes the orbital within a subshell.

Describes the electron spin (+1/2 or -1/2).

A method to visually represent the probability of finding electrons at different distances from the nucleus using a random drop experiment.

The midpoint between the inner and outer edges of a circle, measuring the distance of each circle from the center.

The space enclosed within a circle, calculated using the formula πr² where 'r' is the radius.

The difference between the areas of two consecutive circles, representing the increase in space between each circle.

The total count of marked dots that land within a specific circle in the simulation.

The density of dots within a circle, calculated by dividing the number of dots in a circle by its area.

The likelihood of finding a dot within a specific area of the simulation, expressed as a percentage.

The simulation models the probabilistic nature of electron location, showing that electrons are more likely to be found closer to the nucleus and less likely farther away.

The distance from the center of the circle where the density of dots is greatest, indicating the highest probability of finding a dot.

The arrangement of electrons around an atom's nucleus, influenced by quantized energy levels and orbital shapes.

Describes the shape of an electron's orbital, ranging from 0 (spherical) to n-1 (more complex shapes).

Specific combinations of quantum numbers that are physically possible for an electron in an atom, following the rules of atomic structure.

A principle stating that no two electrons in an atom can have the same set of all four quantum numbers. Each orbital can hold a maximum of two electrons with opposite spins.

A visual representation of how electrons fill orbitals in an atom, following the Aufbau principle and Hund's rule.