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Acetone reacts with iodine to form iodoacetone, iodide, and a hydrogen ion:In water, ${\mathrm{H}}^{+}$ denotes a solvated hydrogen ion; added hydrochloric acid provides acidic conditions.

Moorpark College's protocol mixes acetone, hydrochloric acid and water from burets in matched test tubes; pipet in iodine, swirl and time colour loss against white paper. Use water, then reacted solution, as references. Duplicate each mixture; keep total volume $5.00\mathrm{mL}$ and run temperatures within $2{}^{\circ }\mathrm{C}$.^[ref]

The stock dilutions give $[\mathrm{acetone}{]}_0=0.800$, $[{\mathrm{H}}^{+}{]}_0=0.200$, and $[{\mathrm{I}}_2{]}_0=0.00100\mathrm{mol}{\mathrm{L}}^{-1}$. B and C separately double acetone and acid; D halves iodine. The manual supplies no measured times; it states zero partial order of reaction in iodine and asks students to determine the other exponents.^[ref]

The endpoint measurement is a time $\tau$ to an operational colour threshold, not direct observation of a reaction intermediate. If the iodine disappearance rate $r$ is approximately constant until that endpoint, $r\approx [{\mathrm{I}}_2{]}_0/\tau$. Halving $[{\mathrm{I}}_2{]}_0$ at fixed other concentrations then approximately halves $\tau$ without changing $r$. A longer or shorter endpoint time alone is not a comparison of reaction rates unless the starting concentration is included. For an observed power-form rate law, doubling only acetone gives a rate ratio $2^m$ and hence $m=\ln (r_B/r_A)/\ln 2$; doubling only acid similarly estimates its own partial order of reaction. Those are inference formulas, not asserted experimental results.

A useful proposed reaction mechanism would explain how iodine is consumed after an earlier transformation sets the throughput, making the observed reaction rate insensitive to iodine over a tested range. The observed zero exponent would contradict treating this net chemical equation as a single elementary reaction with directional rate law $k[\mathrm{acetone}][{\mathrm{I}}_2]$. It would not uniquely prove which reaction intermediate or earlier step is involved. Independently detecting a candidate reaction intermediate would provide another kind of evidence.

The excess-reactant approximation has an explicit scale: the baseline iodine inventory is only $0.00100/0.800=0.125\%$ of the initial acetone inventory, and its net hydrogen ion production is $0.00100/0.200=0.5\%$ of the initial acid inventory, assuming only the stated one-to-one chemical reaction. These are calculated bounds on composition change, not measured reaction orders. Mixing delay, a subjective colour threshold, and temperature drift limit the inference. Repeats and a fixed viewing geometry help; a calibrated absorbance trace could test linearity during conversion instead of relying on an endpoint alone. That extension would require a reference blank and a justified Beer-Lambert law calibration, rather than treating visible colour as an exact concentration. A zero-order reaction approximation in iodine must fail at depletion; it cannot imply consumption after no iodine remains.

Ferri Iodidum is the historical iron-iodide medicinal article. The salt differs from free iodine and from its syrup or pill formulations.^[ref]

The diatomic molecule containing one hydrogen atom and one iodine atom. Its measured spectroscopic wavenumbers include anharmonic corrections beyond the two-term Morse oscillator model.^[ref]

An iodide is an iodine anion with electric charge $-e$, where $e$ is the elementary charge.

Iodine is the chemical element with atomic number 53 and symbol $\mathrm{I}$. It is a halogen. Elemental iodine consists of ${\mathrm{I}}_2$ molecules and forms a dark molecular solid near room temperature. Iodide is the reduced anion ${\mathrm{I}}^{-}$; the different forms can interconvert in redox chemistry and have different spectroscopic behavior.^[ref]

An iodine cell places reference absorption on the same beam as stellar lines. A template and known cell transmission constrain stellar shift and instrumental line shape together. The observed spectrum is modelled by multiplying the stellar and cell spectra before instrumental convolution.

Iodine deficiency is insufficient iodine availability for normal physiology, especially production of thyroid hormones. Increased stimulation of the thyroid can produce a goitre; enlargement and reduced hormone output are distinct outcomes. During pregnancy, inadequate iodine can impair biological development, so nutritional timing matters as well as total intake.^[ref]

A reactive iodine oxide radical. Its gas-phase abundance need not represent total reactive iodine when particulate reservoirs and multiphase recycling are important.

Lick Observatory is an astronomical observing site associated with optical spectroscopy and precision measurements of stellar motion. In the Lick Observatory iodine-cell radial-velocity method, a cell places known iodine absorption on the stellar beam, allowing instrumental changes and a stellar Doppler shift to be fitted together.

This apparatus illustrates why a spectral shift cannot be read independently of calibration. The reference and stellar spectra pass through the same optical system, and their combined image must be modelled with the instrumental line profile. Repeated measurements then test an orbital signal rather than merely identifying one shifted spectral line.

At Lick Observatory, the Hamilton spectrograph records starlight with an imprinted iodine reference. The reference tracks instrumental wavelength and profile changes during the science exposure. Barycentric correction and a time series of relative stellar shifts then support a dynamical companion model.

In a 1982 experiment, purified nucleoplasmin was labeled with radioactive iodine and cleaved by proteolysis. Microinjection delivered cargo into Xenopus laevis oocyte cytoplasm. Manually separated cell nuclei and cytoplasm were compared by gel electrophoresis and autoradiography; section autoradiography checked internal localization. Tail-bearing cargo entered the cell nucleus; tailless cores did not. Direct nuclear microinjection retained the cores: the tails mattered for entry, but the assay did not identify a receptor.^[ref]

Direct nuclear microinjection bypassed entry, distinguishing failure to enter from failure to remain inside a cell nucleus.

First construct the energy cost for heterolysis from the molecular potential minimum. Dissociation to neutral atoms costs $D_e$, ionizing caesium costs $I$, and attachment of the electron to iodine releases EA. ThereforeFor the ground-state reference convention used above, the initial molecule already has vibrational zero-point energy. Thus its ground-state dissociation energy is $D_0=D_e-\frac{1}{2}{k}_B{\theta }_{\mathrm{vib}}$ andAt $3000\mathrm{K}$, $k_{B}T=0.258520\mathrm{eV}$, givingAlternatively, retaining the molecular minimum as reference gives $\Delta {\epsilon }_{\min }=4.36\mathrm{eV}$ and a Boltzmann factor $4.7372\times 10^{-8}$. That convention must use the full vibrational partition function, including $e^{-{\theta }_{\mathrm{vib}}/(2T)}$, in the next part. The ground-state convention instead uses $q_{\mathrm{vib}}^0$. Either consistent convention gives the same final equilibrium constant; using the ground-state reaction energy with the full zero-point factor would count the correction twice. The distinction between $D_e$ and $D_0$ is a distinction between initial states, not a change in the dissociation products.^[ref]

The hydroxyl group first binds aluminium, normally by deprotonation to an aluminium alkoxide with release of hydrogen. Coordination also brings aluminium close to the alkyne. directed trans-hydroalumination then puts hydride on the alkyne carbon proximal to CH2O and aluminium on the distal carbon.

One useful mechanistic description has external hydride attacking the coordinated alkyne opposite the aluminium-containing face. The resulting vinylaluminate is stabilized by a five-membered O–Al–C–C–CH2 chelate. This is not the ordinary undirected syn addition of a neutral dialkylaluminium hydride. Propargylic-alcohol-directed trans-hydroalumination with Red-Al gives vinylaluminate intermediates that can be intercepted by electrophiles.^[ref]

iodine replaces the distal C–Al bond with C–I without scrambling the alkene geometry; aqueous work-up releases the alcohol. hydride and iodine are consequently trans across the alkene, while iodine and the CH2OH group are on the same side.

By Cahn-Ingold-Prelog priority rules priority the product is therefore $Z$: CH2OH outranks H at one alkene carbon and I outranks CH2R' at the other. Describing the two carbon chains as trans would not make this an $E$ alkene, because the iodine changes which substituent has higher priority.

Oxidizing cobaltocene removes its antibonding nineteenth electron and gives the particularly favourable 18-electron cobaltocenium cation. iodine can accept the electrons, giving cobaltocenium iodide at the simple stoichiometryEach cobalt changes from Co(II), $d^7$, to Co(III), $d^6$; each iodine atom changes from 0 to $-1$. Excess iodine can change the isolated counterion to a polyiodide such as ${\mathrm{I}}_3^{-}$. In contrast, oxidation of 18-electron ferrocene would remove an electron from its occupied closed-shell manifold to form 17-electron ferrocenium. iodine is insufficient to drive that reaction under the conditions implicit here. ferrocene can still be oxidized by suitable stronger oxidants; an electron count is a useful rationale for the comparative redox behaviour, not a universal proof of a numerical electrode potential.

The bromines ortho and para to OH are removed, leaving the meta bromine at C3. A suitable polar mechanism begins with electrophilic ipso protonation of a brominated carbon. protonation at C4 or C6 gives a Wheland intermediate stabilized by donation of the phenolic oxygen lone pair; an important contributor has an O-protonated cyclohexadienone-like framework. Corresponding protonation at C3 lacks this direct stabilization by resonance in chemistry from OH.

iodide can capture/reduce the departing electrophilic bromine as the C–Br bond electrons restore the aromatic pi system. Thus the incoming hydrogen remains on carbon while bromine is removed, unlike ordinary electrophilic substitution in which the incoming electrophile remains and a proton leaves. bromine trapping can be represented through IBr formation followed by reaction with further iodide to give iodine and bromide. For each replacement the balanced net reduction isApplying it at C4 and C6 gives 3-bromo-2,5-dimethylphenol, with formula ${\mathrm{C}}_8{\mathrm{H}}_9\mathrm{BrO}$. This explains why the position least activated by OH is the one at which bromine survives. It is a proposed acid-assisted protodebromination mechanism consistent with the selectivity; the preparative sequence alone does not prove every proton-transfer or halogen-transfer intermediate. It should not be drawn as iodide simply displacing bromide from an unactivated aryl carbon.

The molecule with the larger inferred dissociation energy is assigned the stronger hydrogen–halogen bond: $\mathrm{A}=\mathrm{HBr}$ and $\mathrm{B}=\mathrm{HI}$. Moving from bromine to the larger iodine atom generally lengthens the bond and reduces effective overlap with the compact hydrogen $1s$ orbital, so hydrogen iodide is more weakly bound. Independently, the tabulated ground-state harmonic constants near $2649\mathrm{c}{\mathrm{m}}^{-1}$ for hydrogen bromide and $2309\mathrm{c}{\mathrm{m}}^{-1}$ for hydrogen iodide agree with the inferred assignment.^[ref][ref] The ordering is the identification criterion; the low-level Morse oscillator extrapolations above should not be presented as measured dissociation energies.

For fluorine, the key is chemical sequestration, not an inability of free F to react. Fluorine atoms readily form very stable hydrogen fluoride through reaction with hydrogen-containing gases. Breaking hydrogen fluoride or regenerating a sustained free-fluorine radical population under ordinary stratospheric conditions is difficult, so an efficient analogous catalytic family is not maintained.

For iodine, the traditional approximation is limited delivery to the stratosphere. Many iodine source gases are short lived in the troposphere, and their reactive products are efficiently taken up or removed before slow large-scale ascent. This historically motivated omitting iodine from the major stratospheric chlorine/bromine budget. It does not establish that iodine atoms are intrinsically ineffective catalysts, or that stratospheric iodine is exactly zero.

Indeed, the blanket omission needs qualification even for this exam's date. Aircraft observations published in 2020 detected both IO and particulate iodine in stratospheric air and inferred continuing multiphase recycling and ozone loss. Gas/particle partitioning and measurement sensitivity must be considered together; a small gas-phase concentration alone can miss an active reservoir. Thus the traditional supply argument is the intended contrast with fluorine's stable-HF sink, but zero stratospheric iodine chemistry is not supported by those observations.^[ref]

Stellar reflex motion. A planet and its host orbit their common barycentre. The star's line-of-sight velocity shifts its absorption lines by $\Delta \lambda /\lambda \simeq v_r/c$ at low speeds. A time series can be fitted withHere $\nu (t)$ is true anomaly, $\varpi$ the argument of periastron and $\gamma$ an arbitrary systemic velocity offset. At small companion mass and known stellar mass, the orbit supplies $M_p\sin i$, not the true planet mass without an inclination constraint. Long monitoring helps distinguish a reproducible Keplerian signal from stellar oscillations, magnetic activity, spots and instrumental trends.

The Lick reference-cell implementation. Starlight passes through a temperature-controlled cell of molecular iodine before entering the Hamilton high-resolution echelle spectrograph. The cell imprints a dense pattern of reference absorption lines on the stellar spectrum, predominantly in the approximately $500$–$630\mathrm{nm}$ interval. These lines share the same exposure and downstream optical path as the stellar light. A calibrated high-resolution Fourier-transform iodine spectrum and an iodine-free stellar template allow the wavelength solution and instrumental line-spread function to be fitted along with the stellar Doppler shift. The method corrects shifts and line-shape changes that a separate calibration exposure would not necessarily follow.^[ref]

A useful forward model for one short spectral segment isfollowed by pixel integration, continuum scaling and a fitted wavelength calibration. Here $S$ is the intrinsic stellar spectrum, $T_{{\mathrm{I}}_2}$ the cell transmission and $\mathcal{P}$ the instrumental line-spread function. The spectra multiply before convolution; simply dividing a recorded blended spectrum by the laboratory iodine spectrum is not equivalent to this model. The iodine pattern is stationary in the observatory frame while stellar lines move relative to it. Separate spectral segments accommodate wavelength dependence of the instrumental profile.

Earth's rotational and orbital velocities must then be removed with a barycentric correction using accurate timing, ideally weighted by photon arrival rate. Many stellar lines constrain a shift smaller than one instrumental resolution element; spectral resolution alone is not the velocity error. Photon statistics, template quality, instrumental-profile modelling and intrinsic stellar variability limit the precision. The method measures changes relative to a template and does not by itself provide a perfectly absolute centre-of-mass velocity. No particular discovery, modern precision floor or historical observing performance is assumed here.

This is a C-centered orthorhombic lattice. The translation $(1/2,1/2,0)$ takes each A molecule to another A molecule and each B molecule to another B molecule. Thus the conventional cell has two lattice points.

A two-molecule crystal motif can be chosen as A at $(0,0,0)$ and B at $(1/2,0,1/2)$. Attaching that same motif to both C-centered lattice points produces all four molecules, hence eight iodine atoms per conventional cell.

The centers alone appear face-centered, but $(1/2,0,1/2)$ exchanges A and B orientations. It is not a translation symmetry of the oriented molecular solid. An F-centered assignment would discard essential motif information.

Starch granules can often be distinguished by their shape, size distribution, hilum and lamellae; dextrin and inulin are distinguished chiefly by their molecular constitution, solubility and chemical reactions. An isolated particle of uncertain origin cannot always be identified uniquely by one feature.

In a water-mounted preparation of unheated starch, potato granules are usually relatively large, oval or pear-shaped, often with an eccentric hilum near the narrower end and conspicuous curved growth markings. Wheat gives a characteristic mixture of larger flattened lenticular granules and small rounded granules; the hilum and rings are less conspicuous. Rice starch consists of very small angular or polyhedral granules, often still associated into compound groups. These are distributions rather than a guarantee that every potato granule is larger than every wheat granule.^[ref]

Maize commonly gives polygonal or rounded granules with a central point or fissured hilum; oats characteristically include aggregates of small angular granules. Arrowroot commonly has oval or elongated granules, sometimes with a transverse fissure towards one end. Preparation, variety and processing change the apparent population. Rotation between crossed polarizers shows the organized granule structure through a characteristic extinction cross in many intact granules. Swelling and loss of birefringence on heating with sufficient water help demonstrate starch gelatinization, although the precise temperature depends on the starch source.

Cold water normally leaves native starch granules as a suspension rather than a clear molecular solution. On heating, granules swell and a paste develops. With iodine in iodide solution, ordinary starch rich in sufficiently long amylose helices produces an intense blue or blue-black complex. Its intensity depends on chain structure and conditions; the response can weaken on heating and return on cooling if the chains remain suitable. Continued acid or enzymatic hydrolysis shortens chains and eventually destroys this characteristic blue response.

Dextrin denotes a range of shorter or modified glucose polymers derived from starch, rather than one pure substance. Many preparations dissolve or disperse in water more readily and no longer show intact native granules. Their iodine reactions vary with chain length: some give violet or reddish-brown colours, while extensively shortened material gives no characteristic colour. It is therefore too absolute to say that every dextrin is chemically identical or that no dextrin can react with iodine. The modern international specifications themselves distinguish starch modifications and their variable iodine colours.^[ref][ref]

Inulin is principally a fructose-based fructan, with a different linkage pattern from glucose-based starch. It occurs, for example, in chicory and related storage organs. It does not give starch's blue iodine complex. It dissolves more readily in hot water, and may separate as deposits on cooling or precipitation, but such deposits are not the characteristic native starch granules. Hydrolysis yields mainly fructose, whereas complete starch or dextrin hydrolysis yields glucose. A copper-reduction test after hydrolysis detects reducing products in both cases and is therefore insufficient by itself to distinguish them. Their different hydrolysis products, interpreted with iodine reaction and microscopy, give a more specific comparison.^[ref]

A sound comparison uses separately labelled reference preparations, equal iodine conditions and separate unheated and heated mounts. Inspecting an unknown mixture only after boiling destroys much of the morphological evidence. The combined observations distinguish source-related morphology from the effects of processing.