In complete sentences, describe the similarities and differences between: a. different isotopes of an element b. a neutral atom and an ion of the same element

Understanding atomic number and mass is fundamental to grasping the differences between various isotopes of an element. The atomic number is the number of protons found in the nucleus of an atom. This number is unique to each element and defines what the element is — for example, all carbon atoms have an atomic number of 6 because they have six protons.

On the other hand, atomic mass refers to the total number of protons and neutrons in an atom's nucleus. Isotopes of an element vary in atomic mass because they have the same number of protons but different numbers of neutrons. Despite these differences in mass, isotopes of an element will occupy the same position on the periodic table due to their consistent atomic number, hence, they showcase similar chemical behaviors.

Radioactive isotopes, or radioisotopes, are versions of an element that have unstable nuclei. This instability leads to a phenomenon known as radioactivity, where the isotopes can release particles and radiant energy to form more stable atoms. The types of radiation emitted may include alpha particles, beta particles, and gamma rays.

Radioisotopes have various applications. For instance, they are used in medicine to diagnose and treat certain illnesses. Carbon-14, a radioactive isotope of carbon, is used in radiocarbon dating to determine the age of archeological findings. The health and safety risks associated with radioisotopes are a topic of concern as well because exposure to radiation can be harmful to living organisms.

Comparing neutral atoms and ions highlights the effects of electron arrangements and charge on an atom's properties. Neutral atoms have a balanced number of protons and electrons, which results in no net electrical charge. Electrons are arranged in energy levels around the nucleus and the neutral atom is most stable when its outermost energy level is filled or follows an established electron configuration pattern.

An ion is formed when an atom gains or loses electrons, disrupting the balance and creating a net charge — positive for losing electrons (cation) or negative for gaining electrons (anion). The process of ionization alters an atom's chemical properties significantly, affecting how it bonds and interacts with other atoms or molecules. The ionic charge plays a pivotal role in the formation of ionic compounds and the behavior of atoms in a chemical reaction.

Electron configuration is the arrangement of electrons in an atom's orbitals, and it follows a set of rules often depicted by the quantum mechanical model. Electrons occupy orbitals starting from the lowest energy level to higher ones, and each orbital can hold a specific number of electrons before additional electrons begin to populate the next orbital.

The configuration determines how atoms interact in chemical reactions and contributes to their chemical properties. For instance, elements with a valence shell (outermost electron shell) that is full or near full tend to be less reactive, as they have a stable electron configuration. The understanding of electron configuration is not only important for predicting the reactivity of elements but also essential when it comes to determining the types of bonds that an atom can form with others.