Write the electron configuration of tin.

The periodic table is a comprehensive chart that provides a systematic way to organize information about the elements. It is structured in rows, called periods, and columns, known as groups or families. Each element has its own unique spot, and the table is arranged so that elements with similar chemical behaviors are aligned in the same group. By looking at an element's position on the periodic table, one can infer a variety of its properties, including atomic mass, electronegativity, and, as with our exercise, the expected electron configuration.

For students struggling to understand the periodic table, it's essential to start by getting familiar with its basic organization. Recognize that the periods indicate the number of electron energy levels, and the groups give you insight into the number of valence electrons for the main group elements. This information is vital for predicting how an element will react chemically and physically.

Atomic orbitals can be thought of as the 'neighborhoods' for electrons within an atom. These are regions in space where the probability of finding an electron is highest. Orbitals are categorized into four main types: 's', 'p', 'd', and 'f'. Each type has a different shape and energy level, with 's' being the lowest energy and 'f' the highest.

In the context of an exercise, identifying which orbitals are filled can be done by following the electron configuration principles. It is crucial for students to remember that 's' orbitals can hold up to 2 electrons, 'p' up to 6, 'd' up to 10, and 'f' up to 14. This helps in constructing the orbital diagram basing on the hierarchy of energy levels. For an accessible understanding, visualize orbitals as distinct slots in an energy level, where the s orbitals are always filled first, followed by p, then d, and finally f as you move to higher energy levels.

Quantum numbers are like the address of an electron, describing its position within an atom. There are four types: the principal quantum number (n), angular momentum quantum number (l), magnetic quantum number (m), and spin quantum number (s). Each electron within an atom has a unique set of these numbers.

n indicates the electron's energy level, l defines the shape of the orbital (with 0 corresponding to s, 1 to p, 2 to d, and 3 to f orbitals), m specifies the orientation of the orbital in three-dimensional space, and s gives the direction of the electron's spin. Familiarizing themselves with these quantum numbers helps students not only understand the nuances of electron arrangements but also the broader concepts of atomic structure and chemical behavior.

Electron energy levels, or 'shells', are akin to the rungs of a ladder on which electrons reside. The first energy level is closest to the nucleus and has the lowest energy, while higher levels are progressively further away and higher in energy. Understanding how electrons fill these levels is integral to grasping electron configurations.

Electrons populate energy levels in a methodical way, following the Pauli exclusion principle, Hund's rule, and the Aufbau principle. The lowest energy levels are filled first, and electrons in the same subshell will not pair up until each orbital has one electron (Hund's rule). These guidelines ensure that when students write out the electron configuration, as with the exercise's tin example, they place electrons correctly and predict the most stable arrangement within an atom.