イオンとイオン電荷

An ion is a charged particle formed when an atom or molecule gains or loses one or more electrons. Atoms are normally neutral with equal numbers of protons and electrons. When electrons are transferred, the balance shifts, creating a net positive or negative charge. The element identity remains unchanged because the number of protons stays constant.

Cations form when atoms lose electrons, resulting in more protons than electrons and a positive charge. Anions form when atoms gain electrons, resulting in more electrons than protons and a negative charge. Cations are named the same as their element followed by 'ion,' while anions use the suffix '-ide' added to the element name.

The charge of an ion is written as a superscript on the right side of the chemical symbol. For example, a calcium ion that loses two electrons is written as Ca2+, and a fluoride ion that gains one electron is written as F−. The number one is typically omitted for ions with a single positive or negative charge.

The periodic table reveals predictable patterns for main-group elements. Metals on the left lose electrons to form cations: Group 1 metals lose one electron (1+ charge), Group 2 metals lose two electrons (2+ charge). Nonmetals on the right gain electrons to form anions: Group 17 elements gain one electron (1− charge), Group 16 elements gain two electrons (2− charge). Noble gases rarely form ions.

Atomic mass is determined primarily by protons and neutrons in the nucleus. Electrons contribute negligibly to atomic mass because they are much smaller in mass than protons. When an atom loses or gains electrons to form an ion, the nucleus remains unchanged, so the atomic mass of the ion is essentially the same as the neutral atom's atomic mass.

Unlike main-group elements, transition metals often form cations with variable charges that cannot be easily predicted from their periodic table position. For example, copper can form ions with either a 1+ or 2+ charge, and iron can form ions with either a 2+ or 3+ charge. This variability makes transition metal ion charges less predictable than those of main-group elements.

Main-group atoms gain or lose electrons to match the electron configuration of the nearest noble gas. Metals lose enough electrons to have the same electron count as the preceding noble gas, while nonmetals gain enough electrons to match the next noble gas. This electron transfer creates ions with stable, filled electron shells similar to noble gas configurations.