Question

Which of the following statements is false concerning orbitals? a. An orbital is a region of space where an electron might be found with \(90 \%\) probability. b. As an electron absorbs more energy, the orbital in which it might be found becomes larger and/or more complex. c. For each successive energy level, a new type of orbital is added.

Short answer

The false statement concerning orbitals is: c. For each successive energy level, a new type of orbital is added.

Step-by-step solution

Statement A

An orbital is a region of space where an electron might be found with \(90 \%\) probability. An orbital represents the region of space around an atomic nucleus where there is a high probability (90% in this case) of finding an electron. This statement is true, as it accurately describes the nature of an orbital.

Statement B

As an electron absorbs more energy, the orbital in which it might be found becomes larger and/or more complex. When an electron absorbs energy, it can move to a higher energy level or a higher orbital. As we move to higher energy levels (principle quantum number), the orbitals become larger and more complex. This statement is also true.

Statement C

For each successive energy level, a new type of orbital is added. In an atom, orbitals are classified into different types, which are s, p, d, and f orbitals. For each energy level (n), the number of subshells or types of orbitals increases. The relation is given by n subshells for the nth energy level. However, it doesn't mean a "new" type of orbital is added at each energy level; rather, it refers to the number of subshells in each energy level. Therefore, this statement can be considered false. So, the false statement concerning orbitals is: c. For each successive energy level, a new type of orbital is added.

Key concepts

Atomic Orbitals

Atomic orbitals are fundamental for understanding the behavior of electrons in atoms. Imagine the nucleus of an atom as a central point, around which we have a cloud of probabilities where electrons are likely to be found. This cloud is what we refer to as the atomic orbital. Each orbital is shaped differently and has a unique energy associated with it. These shapes are not paths that the electron travels, but rather areas in space where the probability of finding an electron is the highest.

For example, the simplest type of orbital is the s-orbital, which is spherical around the nucleus. As we move to higher energy levels and orbitals like p, d, and f, the complexity increases. The p-orbitals are dumbbell-shaped, the d-orbitals are clover-shaped, and the f-orbitals are even more complex. The complexity and shape of the orbital are tied to the quantum numbers assigned to an electron, which describe its state and energy.

Electron Energy Levels

Electrons within an atom exist in areas called energy levels, which are a bit like the rungs of a ladder. The lower rungs represent lower energy levels, and as electrons gain energy, they can 'jump' to higher rungs or energy levels. These jumps are not random; they follow specific rules of quantum mechanics. When an electron absorbs energy, for example from a photon, it moves to a higher energy level. This process is known as excitation.

The energy levels are quantized, meaning that electrons can only exist in certain energy states and not in between. This is an important concept of quantum chemistry and explains why we see distinct lines in the emission spectra of elements. Each energy level can contain a set number of electrons, and starting with the second level, these can be further divided into sublevels, or orbitals, such as s, p, d, and f. As we move to higher levels, the energy difference between them decreases, and they become more closely spaced.

Quantum Chemistry

Quantum chemistry is the branch of chemistry that deals with the application of quantum mechanics to chemical problems. This field provides the theoretical framework for understanding the structure and behavior of atoms and molecules. It explains why atomic orbitals have specific shapes and why electrons occupy distinct energy levels.

One of the key tenets of quantum chemistry is the quantization of energy levels. Just like in our exercise, where electrons can exist in various orbitals with different probabilities, quantum chemistry explains these phenomena using mathematical equations and models. It also provides the principles that predict chemical bonding patterns, reaction rates, and the physical properties of materials. Quantum chemistry is the scientific basis for many advanced technologies in materials science, biomedical imaging, and quantum computing, bridging the gap between abstract quantum theories and practical chemical applications.