Atomic Orbitals and Quantum Numbers Quiz

The number of protons within the atom's nucleus.

The sum of protons and neutrons in an atom, measured in atomic mass units (amu).

Atoms of the same element that have the same number of protons but different numbers of neutrons.

A notation used to represent isotopes, where the element's name is followed by a hyphen and its mass number. Example: Carbon-14.

The process by which an atom gains or loses neutrons, changing its atomic mass but not its atomic number.

The principal quantum number determines the energy level of an electron, with values ranging from 1 to 7. Higher numbers correspond to higher energy levels.

The total number of electrons in an atom is equal to its atomic number.

A weighted average of the masses of all the isotopes of an element, considering their relative abundance.

According to the Pauli Exclusion Principle, no two electrons in an atom can have the same set of four quantum numbers.

Hund's Rule states that electrons will occupy empty orbitals within a subshell before pairing up in the same orbital. This minimizes electron repulsion.

The Aufbau Principle states that electrons will fill orbitals in the lowest energy levels first, then move to higher ones, based on the order of subshell filling.

The 'd' orbitals are filled after the 'p' orbitals within the same energy level.

This quantum number (l) describes the shape and number of subshells within a principal energy level. The value of l can range from 0 (s subshell) to n-1.

The Aufbau Principle dictates the filling of lower energy levels before higher energy levels in electron configuration.

The spin quantum number (s) describes the intrinsic angular momentum of an electron, which is also related to the magnetic field generated by the electron.

Hund's Rule mandates that each orbital within a subshell is singly occupied before electrons start pairing up.

The first quantum number (n) in electron configuration represents the energy level of an electron.

The atomic number of an atom represents the number of protons within its nucleus.

When an atom has an unequal number of protons and neutrons, it forms an isotope.

In neutral atoms, the number of protons and electrons is equal.

Using the electron configuration of the previous row's noble gas to simplify the electron configuration of an element with many electrons.

Quantum numbers are used in electron configuration to define the probable location of electrons within an atom's structure.

Helium and other noble gases have full electron configurations and are stable, which is why they don't readily participate in bonding.

Hund's Rule dictates the specific order of filling orbitals in electron configuration.