Question

How many \(2 p\) orbitals are there, and what is the total number of electrons they can hold?

Short answer

There are 3 '2p' orbitals, and they can hold a total of 6 electrons.

Step-by-step solution

Understanding Atomic Orbitals

Orbitals are regions around an atom's nucleus where electrons are likely to be found. Each orbital can hold a specific number of electrons. The '2' denotes the principal quantum number, which indicates the electron's energy level, and the 'p' denotes the type of orbital.

Identify the Number of 2p Orbitals

For a given principal quantum number, the possible types of orbitals are labeled as s, p, d, and f. The 'p' orbitals arise when the principal quantum number is 2 or greater. There are three 'p' orbitals for each energy level where 'p' orbitals exist.

Calculate Electron Capacity

Each 'p' orbital can hold a maximum of 2 electrons. Hence, for 3 'p' orbitals, the total number of electrons they can hold is given by: \[3 ext{ orbitals} imes 2 ext{ electrons/orbital} = 6 ext{ electrons}\]

Key concepts

Electron Configuration

The electron configuration of an atom describes the distribution of electrons in the atomic orbitals. It is a way to understand where, and how, electrons are organized within an atom.

• Electrons fill orbitals in a specific order, from lower to higher energy levels.
• The Aufbau principle suggests electrons start filling from the closest (lowest energy) orbitals and move outward.
• Electron configurations are typically represented in notations like 1s, 2s, 2p, etc.

This configuration influences the atom's chemical properties. For instance, the electron configuration can determine how an element will react with others. Electrons in outermost shells, or valence shells, are particularly important, as they are the most likely to participate in chemical bonding.
Understanding electron configurations helps in predicting the structure and stability of atoms and molecules.

p Orbitals

The 'p' orbitals are a type of atomic orbital depicted by their complex shape. These orbitals are fundamental in understanding atomic structure and chemistry.

• 'p' orbitals appear starting from the second energy level, where the principal quantum number is 2.
• They are shaped like dumbbells and are oriented along the x, y, and z axes in a Cartesian coordinate system. This is why there are three 'p' orbitals at any given energy level.
• Each 'p' orbital can hold a maximum of two electrons, following the quantum mechanical principle that electrons should have opposite spins within the same orbital.

Understanding 'p' orbitals is crucial for explaining how atoms form bonds and their magnetic properties. These orbitals significantly contribute to an atom's ability to form covalent bonds in molecules. For example, in covalent bonds, the overlap of 'p' orbitals from different atoms can lead to the formation of strong directional bonds.

Quantum Numbers

Quantum numbers are sets of numerical values that describe the distinctive quantum state of an electron in an atom. They provide a roadmap to understanding electron arrangement within atoms.

• The principal quantum number (n) relates to the energy level of an electron within an atom. It is always a positive integer.
• The angular momentum quantum number (l), for a 'p' orbital, is 1, which describes the shape of the orbital.
• The magnetic quantum number (m_l) designates the orientation of the orbital in space. For 'p' orbitals, it can be -1, 0, or +1.
• Lastly, the spin quantum number (m_s) indicates the spin direction of the electron, either +1/2 or -1/2.

These numbers are critical for predicting electron probability distributions and their interactions. By knowing the quantum numbers, chemists can predict the behavior of atoms in different types of chemical reactions, further providing insight into the electronic structure of atoms.