Explanation: An ion is defined by an *unequal* number of electrons and protons, which results in a net electrical charge. If the numbers were equal, the atom or molecule would be electrically neutral.

Explanation: The net electrical charge of an ion is precisely the difference between the number of protons (positive charges) and electrons (negative charges). An imbalance results in a net positive or negative charge.

Explanation: For singly charged ions, the magnitude '1' is conventionally omitted in chemical formulas; for example, it is written as Na+ rather than Na1+.

Explanation: The fundamental definition of an ion is an atom or molecule that carries a net electrical charge due to an imbalance between its protons and electrons.

Explanation: In chemical formulas, the magnitude of the charge is placed before the sign for charges greater than one (e.g., 2+ for a doubly charged cation).

Explanation: The net electric charge on an ion is calculated by subtracting the total number of electrons (negative charges) from the total number of protons (positive charges).

Explanation: While William Whewell suggested the term 'ion', it was Michael Faraday who introduced it in 1834. The term is indeed based on the Greek word 'ienai'.

Explanation: Svante Arrhenius's 1884 dissertation proposed that solid crystalline salts dissociate into ions when dissolved, even without an electric current, a theory for which he received the Nobel Prize in Chemistry in 1903.

Explanation: Michael Faraday coined the term 'ion' but did not initially understand their precise nature as charged atoms. He observed them as moving substances conveying matter during electrolysis.

Explanation: The term 'ion' is derived from the Greek word 'ienai', meaning 'to go', reflecting the movement of these charged particles during electrolysis.

Explanation: Michael Faraday introduced the term 'ion' in 1834, following a suggestion from William Whewell.

Explanation: Faraday observed the movement of these species during electrolysis and named them 'ions' based on their 'going' nature, without a precise understanding of their atomic structure or charge.

Explanation: William Whewell, in correspondence with Michael Faraday, coined the terms 'anode,' 'cathode,' 'anion,' and 'cation' to describe the electrodes and the ions attracted to them.

Explanation: Svante Arrhenius's key contribution was his theory that solid crystalline salts dissociate into charged particles (ions) when dissolved in a solution, even in the absence of an electric current.

Explanation: Monatomic ions are formed by the gain or loss of electrons from the *valence shell* (outermost electron shell) of an atom, not the tightly bound inner shells.

Explanation: Ionization is the process of gaining or losing *electrons* from a neutral atom or molecule, not protons. Changes in the number of protons would change the element itself.

Explanation: Electron transfer during chemical ionization is primarily driven by atoms or molecules seeking to attain *stable*, 'closed shell' electronic configurations, which typically requires the least energy.

Explanation: Polyatomic ions are usually formed by gaining or losing elemental ions (like H+), rather than directly gaining or losing electrons, to preserve their stable electronic configuration and avoid the instability of radical ions.

Explanation: Atoms gain or lose electrons to achieve a stable electronic configuration, often resembling a noble gas with full orbital blocks, as this state is energetically favorable.

Explanation: During physical ionization in a fluid, an 'ion pair' is indeed formed, consisting of a free electron and the resulting positive ion from which the electron was detached.

Explanation: Monatomic ions are formed by the gain or loss of electrons from the *valence shell* (outermost electron shell), as inner-shell electrons are tightly bound and generally do not participate in chemical interactions.

Explanation: During physical ionization in a fluid, an 'ion pair' is formed, consisting of a free electron and the positive ion from which it was detached.

Explanation: Ions can be created through chemical interactions, such as the dissolution of a salt in liquids, in addition to physical ionization processes.

Explanation: Monatomic ions are formed by the gain or loss of electrons exclusively from the valence shell, which is the outermost electron shell involved in chemical bonding.

Explanation: The primary driving force for electron transfer during chemical ionization is the tendency of atoms or molecules to achieve stable, 'closed shell' electronic configurations, which are energetically favorable.

Explanation: Polyatomic ions often form by gaining or losing elemental ions (like H+) to avoid the formation of unstable radical ions and to maintain stable electronic configurations within the molecular structure.

Explanation: A neutral sodium atom becomes a positively charged sodium cation (Na+) by losing one electron from its valence shell to achieve a stable electron configuration.

Explanation: Ions tend to form with full orbital blocks because this electronic configuration mimics that of noble gases, which is a highly stable and energetically favorable state.

Explanation: A cation is a positively charged ion formed when an atom *loses* one or more electrons, resulting in fewer electrons than protons. Gaining electrons leads to a negative charge, forming an anion.

Explanation: Anions are formed by gaining electrons, which increases electron-electron repulsion and expands the electron cloud, making them *larger* than their parent neutral atoms. Cations, by contrast, are smaller due to electron loss.

Explanation: The hydrogen cation (H+) is indeed unique in its composition, being a bare proton without any electrons, which also accounts for its exceptionally small size.

Explanation: An ion with a -2 charge is a dianion, and an ion with a +2 charge is a dication. The question reverses these definitions.

Explanation: A zwitterion is a neutral molecule that contains both positive and negative charges at different locations within its structure, resulting in an *overall neutral* charge, not an overall positive charge.

Explanation: In a crystal lattice, anions are generally larger and occupy most of the space, while the smaller cations fit into the interstitial spaces between them.

Explanation: The presence of unpaired electrons in radical ions makes them highly reactive, similar to uncharged radicals, as they seek to achieve a more stable electron configuration.

Explanation: Oxyanions are polyatomic ions that contain oxygen, but they do not necessarily contain hydrogen. Examples include carbonate (CO3^2-) and sulfate (SO4^2-).

Explanation: As charged particles in motion, ions are subject to the Lorentz force, which causes their trajectories to be deflected by a magnetic field.

Explanation: Organic ions are molecular ions that contain at least one carbon-to-*hydrogen* bond, not necessarily a carbon-to-oxygen bond.

Explanation: A carbocation is a *positively* charged organic ion where the charge is formally centered on a carbon atom. A negatively charged organic ion centered on carbon is a carbanion.

Explanation: A cation is defined as a positively charged ion, meaning it has lost one or more electrons, resulting in fewer electrons than protons.

Explanation: An anion is a negatively charged ion formed when an atom or molecule gains one or more electrons, leading to an excess of electrons compared to protons.

Explanation: Ions composed of two or more atoms are classified as polyatomic ions, also known as molecular ions.

Explanation: When an atom gains electrons to form an anion, the increased electron-electron repulsion expands the electron cloud, making the anion larger than its neutral parent atom.

Explanation: The hydrogen cation (H+) is unique because it is composed entirely of a single proton, lacking any electrons, which also makes it exceptionally small.

Explanation: An ion with a +2 charge is specifically termed a dication, while an ion with a -2 charge is a dianion.

Explanation: A zwitterion is characterized by having both positive and negative charges within the same molecule, but these charges balance each other, resulting in an overall neutral molecular charge.

Explanation: Anions are typically larger than cations, and in crystal structures, they tend to define the overall lattice, with the smaller cations occupying the interstitial sites.

Explanation: A radical ion is distinguished by the presence of unpaired electrons, which typically makes it highly reactive.

Explanation: Oxyanions are polyatomic ions that are characterized by the presence of oxygen atoms within their structure, such as carbonate or sulfate.

Explanation: A carbocation is specifically defined as a positively charged organic ion where the formal charge resides on a carbon atom.

Explanation: Ions in their gas-like state are highly reactive and readily interact with oppositely charged ions to form neutral molecules or ionic salts, seeking a more stable, uncharged state.

Explanation: The formation of a solvation shell around ions in a liquid leads to favorable energy and entropy changes, making solvated ions more stable compared to their highly reactive gas-like counterparts.

Explanation: Nonpolar liquids are *not* ideal for ion formation. Their low dielectric constant *strengthens* the electrostatic attraction between ions, making it harder for them to dissociate and remain separated, unlike in polar solvents like water.

Explanation: According to Dukhin and Parlia, an amphiphilic solute is necessary for ion formation in nonpolar liquids, as its hydrophobic tail ensures solubility and its polar head provides a source for initial ion creation and self-solvation.

Explanation: Solvated ions are more commonly found in environments with *low* temperatures, such as seawater, where salts dissolve to form ions surrounded by solvent molecules.

Explanation: Ions in their gas-like state are highly reactive and will quickly interact with oppositely charged ions to achieve a more stable, neutral state by forming molecules or ionic salts.

Explanation: Solvated ions gain stability from favorable energy and entropy changes that occur when they interact with a solvent, forming a solvation shell that stabilizes their charge.

Explanation: Dukhin and Parlia's concept posits that for ion formation in nonpolar liquids, the solute must be amphiphilic, possessing both hydrophobic and polar components to facilitate solubility and initial dissociation.

Explanation: Nonpolar liquids have a low dielectric constant, which means they are less effective at screening electrostatic interactions, thereby strengthening the attraction between ions and making dissociation difficult.

Explanation: Ionic bonding results from the *mutual attraction* of oppositely charged ions, not repulsion. This attraction leads to the formation of stable crystal lattices.

Explanation: Ions of opposite charge attract each other strongly via electrostatic forces. Therefore, they rarely exist in isolation but instead bind together to form stable crystal lattices, minimizing their energy.

Explanation: Ionic bonding typically occurs between metals, which tend to lose electrons, and nonmetals (excluding noble gases), which tend to gain electrons, forming stable ionic compounds.

Explanation: Electropositivity is a property of *metals*, describing their strong tendency to *lose* electrons and form cations. The tendency of nonmetals to gain electrons and form anions is described by electronegativity.

Explanation: Electronegativity is indeed the measure of an atom's tendency to attract and gain electrons, a characteristic of nonmetals that leads to the formation of negatively charged anions to achieve stable electron configurations.

Explanation: In such a combination, electrons are transferred from the electropositive metal atoms (which tend to lose electrons) to the electronegative nonmetal atoms (which tend to gain electrons), forming metal cations and nonmetal anions.

Explanation: The strong electrostatic attraction between the positively charged sodium cations and negatively charged chloride anions results in the formation of stable ionic bonds, leading to the compound sodium chloride.

Explanation: Electrostatic force is the fundamental attraction between oppositely charged ions, which is the driving force behind the formation of stable ionic compounds.

Explanation: Ionic bonding is fundamentally characterized by the strong electrostatic attraction between oppositely charged ions, leading to the formation of stable compounds.

Explanation: Due to strong electrostatic forces, ions of opposite charge are mutually attracted and readily combine to form stable ionic compounds, typically arranged in crystal lattices, rather than existing in isolation.

Explanation: Ionic bonding is most prevalent in compounds formed between metals, which readily lose electrons, and nonmetals (excluding noble gases), which readily gain electrons, facilitating electron transfer and strong electrostatic attraction.

Explanation: Electropositivity is the characteristic property of metals that describes their strong inclination to lose valence electrons and form positively charged cations.

Explanation: In such a combination, the highly electropositive metal readily donates electrons, and the highly electronegative nonmetal readily accepts them, resulting in electron transfer from metal to nonmetal.

Explanation: Ionization potential (or ionization energy) is the energy required to *detach* an electron from an atom or molecule in its gaseous state, not to add an electron.

Explanation: Each successive ionization energy is *markedly greater* than the last, meaning it becomes progressively more difficult to remove additional electrons from an atom.

Explanation: The statement reverses the facts: Caesium has the *lowest* measured ionization energy, indicating it readily loses an electron, while helium has the *greatest*, making electron removal very difficult.

Explanation: Metals generally have lower ionization energies, meaning less energy is required to remove an electron, which explains their tendency to lose electrons and form positively charged cations.

Explanation: Ionization potential, or ionization energy, is defined as the minimum energy required to remove an electron from a gaseous atom or molecule in its ground state.

Explanation: Successive ionization energies increase significantly because removing an electron from an already positively charged ion requires more energy due to increased nuclear attraction on the remaining electrons.

Explanation: Caesium, an alkali metal, has the lowest measured ionization energy, indicating its strong tendency to lose its outermost electron.