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An ion is a chemical atom or a group of chemical atoms with a nonzero net electric charge. A positive ion is a cation; a negative ion is an anion. The whole entity carries the electric charge: a hydronium ion is a group of four chemical atoms with net charge $+e$. This definition agrees with ^[ref].

For an ordinary ion containing only atomic nuclei and Electrons, let $N_p$ count all its protons and $N_e$ all its Electrons. Each proton contributes the elementary charge $+e$, each Electron contributes $-e$, and neutrons contribute zero. ThereforeThe signed integer $z$ is the net electric charge number. Removing an Electron increases $z$ by one; adding an Electron decreases $z$ by one. Changing the Electron count leaves the atomic number, and therefore the identity of the chemical element, unchanged.

For example, a neutral sodium chemical atom has $11$ protons and $11$ Electrons. Its cation ${\mathrm{Na}}^{+}$ still has $11$ protons, but only $10$ Electrons, so $q=(11-10)e=+e$. A neutral chlorine chemical atom has $17$ protons and $17$ Electrons; its anion ${\mathrm{Cl}}^{-}$ has $17$ protons and $18$ Electrons, so $q=(17-18)e=-e$. These are particle inventories, not pictures of atomic orbitals. See 2.6 Ionic and Molecular Compounds (§2.6: ions and ionic compounds).

One sodium chloride formula unit accounts for one ${\mathrm{Na}}^{+}$ cation and one ${\mathrm{Cl}}^{-}$ anion, whose net electric charges sum to zero. Ordinary solid sodium chloride is an extended arrangement of ions, rather than discrete $\mathrm{NaCl}$ molecules. This is a useful distinction: a neutral material can contain charged constituents, and its chemical formula tells us their ratio without claiming that each pair is a separate molecule.

Ion bookkeeping connects chemistry to electric current: moving ions can transport electric charge, while stationary ions cannot supply a transport current density. In electrochemistry, both signs of ions can contribute to the same conventional current. An ion opposing a fixed electric charge is called a counterion.

Ionic bonding binds oppositely charged ions through attraction governed by electrostatics. In ordinary solid sodium chloride, each cation interacts with many anions, and also with other cations: attraction and repulsion together contribute to the binding of an extended ionic crystal. The chemical formula $\mathrm{NaCl}$ specifies equal numbers of the two kinds of ions; it does not divide the solid into isolated two-atom molecules.^[ref]

This distinction explains a striking combination of properties: ordinary dry sodium chloride conducts electric current poorly, while its molten form or a sufficiently concentrated chemical solution in water conducts well. The ions already exist in the solid; their ability to move through the sample changes. A conductivity experiment on salt solutions tests this transport picture, rather than simply asserting that charged constituents must make every material conductive.

An ion pair is an associated cation and anion. An isolated ion pair lacks the extended neighbourhood of an ionic crystal. In a chemical solution, ion pairs can coexist with more widely separated ions; their abundance depends on conditions. A neutral gas-phase sodium chloride molecule can be treated as a discrete entity, with its own quantum mechanics and dissociation products. That use of molecule does not describe the constituents of ordinary solid sodium chloride.^[ref][ref]

An isocyanate bears an $\mathrm{R}-\mathrm{N}=\mathrm{C}=\mathrm{O}$ group. A molecule bearing two such groups can react with a diol to form polyurethane connections.

The isoelectric point is the pH at which a specified molecule's mean net electric charge is zero. Different protonation states can still carry nonzero electric charges; their contributions cancel in the average. For the two-step glycine speciation model, this gives $\mathrm{pI}=(\mathrm{p}{K}_{a1}+\mathrm{p}{K}_{a2})/2$. Additional ionizable amino acid side chains require their own chemical equilibrium calculations; averaging every pKa is not a general rule. ^[ref]

Below its isoelectric point, free glycine has positive mean electric charge and an electric field drives it toward the negative electrode; above its isoelectric point, the mean electric charge is negative and the direction reverses. At its isoelectric point the charge-driven contribution vanishes. Diffusion and bulk movement of the chemical solution can still move the sample. Gel electrophoresis applies this charge dependence to separation, although protein size, shape and interactions also affect migration. The pKa values of free glycine do not determine a protein's isoelectric point: its free N-terminus, C-terminus and ionizable amino acid side chains supply a different inventory. ^[ref]

Before calculating electronic energy, ask a simpler question: where can the available valence electrons go? A Lewis structure makes that budget visible, and nitrate shows why a correct budget can still require several resonance structures.

A Lewis structure records which chemical atoms are connected in a molecule or ion and how its valence electrons are allocated. One line represents one bond pair, two lines two bond pairs, and three lines three bond pairs; two dots beside a chemical atom represent one lone pair. The marks are a counting language, rather than measured Electron positions. See the IUPAC Gold Book, Lewis formula.

For water, ${\mathrm{H}}_2\mathrm{O}$, the budget is $6+2\times 1=8$ valence electrons. Two O–H lines use four Electrons; the other four form two lone pairs on oxygen. For ammonia, ${\mathrm{NH}}_3$, $5+3\times 1=8$ valence electrons give three N–H lines and one lone pair on nitrogen. Both molecules contain four electron pairs, but their allocations differ. Each shared bond pair is counted once in the total budget, even though both endpoints count it when checking the octet rule.

A practical construction method is:

For carbon dioxide, $4+2\times 6=16$ valence electrons. Starting with two single C–O connections leaves twelve Electrons, enough for three lone pairs on each oxygen, but only four Electrons around carbon. Converting one lone pair from each oxygen into a second bond pair gives $\mathrm{O}=\mathrm{C}=\mathrm{O}$. Eight Electrons are in the four bond pairs, and eight are in four lone pairs, two on each oxygen. Carbon has no lone pair; all three chemical atoms satisfy the octet rule, and all three formal charges vanish.

For the nitrate ion, ${\mathrm{NO}}_3^{-}$, the valence electron budget isNitrogen contributes five, the three oxygen chemical atoms contribute eighteen, and the negative electric charge adds one Electron. Start with nitrogen connected to each oxygen by one bond pair: those three lines use six Electrons. Put the remaining eighteen Electrons into three lone pairs on each oxygen. Each oxygen now satisfies the octet rule, but nitrogen counts only six Electrons. Reassign one oxygen lone pair as a second bond pair on its N–O connection. This changes the allocation without adding an Electron; it applies the construction procedure in Flowers et al., Chemistry 2e, 7.3: drawing Lewis structures.

The resulting nitrate Lewis structure has one N=O connection and two N–O connections. Its four bond pairs use eight Electrons, and its eight lone pairs use sixteen: $8+16=24$. The doubly connected oxygen has two lone pairs; each singly connected oxygen has three; nitrogen has none. All four chemical atoms satisfy the octet rule. Any of the three oxygen chemical atoms can supply the additional bond pair, giving the three equivalent resonance structures below.

Why not draw three N=O connections to make the ion look symmetric? With two lone pairs on each oxygen, that drawing still spends $12+12=24$ Electrons and has the right total formal charge, but places twelve Electrons around nitrogen. It fails the octet rule for this second-period chemical element. Three equivalent resonance structures express the symmetry without that invalid local count.

The economy is beautiful: a handful of dots and lines rules out many impossible counts and identifies lone pairs that can participate in acid-base chemistry. A Lewis structure helps choose rational candidate connections before a detailed quantum chemistry calculation. It does not specify a complete many-Electron wavefunction, actual electron density, or molecular geometry. Adding the separate VSEPR model, described in Chemistry 2e, 7.6: molecular structure and polarity, predicts bent water and pyramidal ammonia; the layouts above alone make no such prediction. Molecular orbital theory supplies a richer electronic description, including the unpaired Electrons of molecular oxygen that an all-paired Lewis structure misses.

In 1916 Gilbert N. Lewis proposed two-dot notation for the shared Electrons of a chemical bond and fuller dot formulae for the outer Electrons, explicitly relating a shared pair to the existing single-line notation. See Lewis, The Atom and the Molecule, JACS 38, 762–785 (1916), pp. 777–778, available as an ^[ref]; the relevant passage is also readable in a ^[ref]. The modern quantum mechanics interpretation should be distinguished from his historical model of fixed outer Electrons.

A biochemical ligand is an ion or molecule that binds a protein. For a receptor, a ligand may activate signaling, prevent activation, or have another effect. This usage concerns protein binding; it is distinct from the coordination-chemistry use of the word. See the protein-binding reference under receptor.

The limiting reagent is the reactant exhausted first if the specified chemical reaction proceeds to the maximum conversion permitted by stoichiometry. With initial values of amount of substance $n_{i,0}$ for the reactants and positive consumption coefficients $a_i$, the largest forward extent of reaction is ${\xi }_{\max }={\min }_i(n_{i,0}/a_i)$. Compare these quotients, rather than simply choosing the smallest initial quantity. This calculation predicts the maximum reaction product quantity and identifies which reactant supply must increase to raise it. See Flowers et al., Chemistry 2e, limiting reactants.

Start with $3\mathrm{mol}$ of molecular hydrogen, $1\mathrm{mol}$ of molecular oxygen and no water. Assume complete conversion by the displayed chemical reaction, without competing reactions. ThenThe molecular oxygen is the limiting reagent. Consumption of $2\mathrm{mol}$ of molecular hydrogen and $1\mathrm{mol}$ of molecular oxygen forms $2\mathrm{mol}$ of water, leaving $1\mathrm{mol}$ of molecular hydrogen. Initially there are $1.806642228\times 10^{24}$ molecular hydrogen molecules and $6.02214076\times 10^{23}$ molecular oxygen molecules; after conversion there are $1.204428152\times 10^{24}$ water molecules and $6.02214076\times 10^{23}$ leftover molecular hydrogen molecules.

As a check, the initial inventory has $6\mathrm{mol}$ of hydrogen chemical atoms and $2\mathrm{mol}$ of oxygen chemical atoms. The final water contains $4\mathrm{mol}$ of hydrogen chemical atoms, and leftover molecular hydrogen supplies the remaining $2\mathrm{mol}$. The atom totals balance even though the total amount of substance of molecules falls from four to three moles.

Lipids are a chemically diverse family of chemical substances, conventionally associated with biological origin and solubility in nonpolar solvents. They include triglycerides, phospholipids, and cholesterol. The name does not specify one molecular formula, one repeating monomer, or one kind of polymer. Some lipids have both hydrophilic and hydrophobic regions rather than being uniformly nonpolar. See IUPAC Gold Book: lipids.

Structure explains the different jobs. A triglyceride has three fatty acid-derived acyl groups attached to glycerol and serves as an energy store. A typical glycerophospholipid instead combines two such chains with a phosphate-containing head, making it an amphiphile suited to a lipid bilayer. Cholesterol has a different structure and also contributes to cell membrane properties. Thus a lipid is a chemical building material, while a lipid bilayer is an organization of many molecules. See Clark, Douglas and Choi, Biology 2e, 3.3: lipid structures and functions.

A metabotropic receptor couples ligand recognition to intracellular signal transduction, which can regulate a separate ion channel, alter enzyme activity or change gene expression. In the usual neurotransmitter context, metabotropic receptors are G protein-coupled receptors: receptor activation is relayed by a G protein. There need not be a change in membrane potential at all. ^[ref]

Two routes should be distinguished. An activated G protein can regulate an ion channel locally at the cell membrane, without an obligatory diffusible second messenger. Alternatively, it can regulate an enzyme that changes the availability of a second messenger, such as cAMP or inositol trisphosphate. Downstream proteins then change channel opening, phosphorylation or other cellular activities. The receptor, G protein, second messenger and final target are distinct components; an activated G protein is a relay protein, rather than itself a small-molecule second messenger.^[ref]

Do not turn this useful chemical synapse classification into the claim that every receptor is a GPCR, or that every indirect response must pass through a G protein. For example, the insulin receptor is an enzyme-linked cell-surface receptor whose intracellular catalytic activity initiates protein phosphorylation. Intracellular receptors supply another category. “Metabotropic” commonly names the GPCR branch in neuroscience; the broader idea of biochemical coupling does not make all non-channel receptors structurally identical. ^[ref]

Separating recognition from execution allows signal amplification and branching. A persistently activated receptor can activate several relay proteins; a regulated enzyme can produce many second messenger molecules. As an explicitly invented count example, suppose one activated receptor activates four relay proteins during one interval, and each relay activates a distinct enzyme that produces fifteen second messenger molecules during the next interval. With sufficient substrates and no loss, this gives $4\times 15=60$ molecules. Those counts do not specify a physiological gain or response duration. A directly gated ion channel also passes many ions while open, so amplification is not an exclusive property of metabotropic receptors: always name the input and output being compared. ^[ref]

A particularly instructive electrophysiology experiment separated a chemical trigger from the ion channel carrying its eventual electric current. In 1987, Hirono, Ito and Sugiyama injected messenger RNA from rat brain into frog egg cells, then tested acquired responses to neurotensin and muscarinic acetylcholine stimulation. Under voltage clamp at $-60\mathrm{mV}$, neurotensin elicited transient, oscillatory inward electric currents after a delay of several tens of seconds. This delay refers to that response and preparation. Reversal potential measurements implicated increased permeability to chloride anions, rather than a pore specific to the applied ligand. Both neurotensin and acetylcholine responses were inhibited by pertussis toxin, which interferes with susceptible G proteins, and by intracellular EGTA, which binds free calcium. Injecting inositol trisphosphate mimicked the responses; a large prior dose of inositol trisphosphate reduced subsequent responses to either extracellular signal. These interventions implicate a shared intracellular relay and calcium-dependent channel opening.^[ref]

The informative comparison with the nicotinic acetylcholine receptor experiment is mechanistic: an extracellular ligand can produce an inward electric current either by directly gating the pore or by mobilizing an intracellular second messenger and stored calcium that activate another pore. Intracellular inositol trisphosphate bypasses reception, whereas EGTA tests the need for free calcium. However, neither inhibition nor mimicry alone identifies every molecular connection: a perturbation can affect several targets, and an injected mediator can activate a pathway without proving that it is the only natural route. The egg cell's endogenous machinery and the mixed messenger RNA preparation also limit extrapolation to an intact neuron. The experiment establishes functional coupling in its preparation, rather than the exact molecular composition or timing of every metabotropic receptor.

Even G protein-dependent channel regulation need not involve a lengthy second messenger cascade. Pfaffinger and colleagues reported in 1985 that acetylcholine-evoked potassium channel activation in embryonic chick atrial cells required intracellular GTP, a guanine-containing nucleotide, and was abolished by pertussis-toxin pretreatment. Changes in cyclic nucleotides, including cAMP, did not account for the channel response. The report discusses intrinsic activation delays of roughly $30$–$100\mathrm{ms}$, illustrating relatively rapid metabotropic receptor action. These observations support a G protein coupling step without cyclic-nucleotide second messengers; they do not by themselves exclude every possible intermediary or prove the specific subunit-channel interaction.^[ref]

A small timing model makes the extra steps visible without inventing an experimental trace. Let $u(t)$ jump from zero to one at $t=0$ and remain on. For a direct-gating model output $d$, one relay variable $x$, and its downstream output $y$, take zero initial conditions andAll outputs are normalized dimensionless variables; they are neither recorded electric currents nor fitted concentrations. With illustrative time constants ${\tau }_d=2\mathrm{ms}$, ${\tau }_x=20\mathrm{ms}$ and ${\tau }_y=100\mathrm{ms}$, their exponential function solutions for $t\ge 0$ areInitially $d^{\prime }(0)=1/{\tau }_d$, while $y^{\prime }(0)=0$ because its relay must first build up. Both outputs eventually approach one. Equal normalized final values do not imply equal biological amplitudes or absence of signal amplification; normalization deliberately removes that question.

The model's useful feature is the delayed buildup created by sequential relaxation, not its arbitrary numbers. Actual kinetics also depend on ligand delivery, relay deactivation, neurotransmitter clearance and the final target. A local G protein route can act promptly, while an ionotropic receptor can remain active during continued exposure or feed a longer-lasting intracellular response. The beauty of metabotropic receptor coupling is its flexibility: the same recognition event can adjust electrical responsiveness and other cellular tasks through different targets. To classify an observed response, combine timing with molecular identity and controlled perturbations.