Name: how bonding affects acid strength
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 3 min 5 s
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PS.Chm.6.3

Acid Strength and Molecular Structure

Zoutzuur is een sterk zuur, terwijl fluorwaterstofzuur een zwak zuur is. Maar wat bepaalt hun sterkte? De sterkte van binaire zuren, met slechts twee elementen, wordt bepaald door bindingsenergie en bindingspolariteit.Een zuur met een hogere bindingsenergie heeft een sterkere binding en zal daarom een zwakker zuur zijn. Als je zuren in een groep vergelijkt, is de binding in een zwak zuur, zoals fluorwaterstofzuur, moeilijker te verbreken, dus het is minder waarschijnlijk dat het zuur protonen afstaat. Daarentegen heeft een zuur met lagere bindingsenergie een zwakkere binding en zal daarom een sterker zuur zijn.De binding in een sterk zuur, zoals zoutzuur, breekt bijvoorbeeld gemakkelijker en staat sneller protonen af dan fluorwaterstofzuur. Een binding, zoals die in zoutzuur, is polair als het ene atoom elektronegatiever is dan het andere. Een verbinding kan als een zuur werken wanneer het atoom dat aan waterstof is gebonden een hogere elektronegativiteit heeft dan waterstof.Het atoom zal een gedeeltelijke negatieve lading hebben, waardoor de waterstof een gedeeltelijke positieve lading kan hebben, zodat het kan worden vrijgegeven als een proton. Een zuur met een hogere bindingspolariteit heeft een zwakkere binding en zal daarom een sterker zuur zijn. Als men verbindingen over een bepaalde periode vergelijkt, is zoutzuur sterker dan waterstofsulfide, omdat chloor elektronegatiever is dan zwavel en daarom gemakkelijker protonen afgeeft.Als waterstof een gelijke of grotere elektronegativiteit heeft dan het andere atoom, kan dat molecuul geen protonen afstaan en kan het daarom niet als zuur werken. Oxyzuren zijn zuren waarbij een OH is gehecht aan een derde atoom dat elektronegatiever is dan waterstof. De sterkte van een oxyzuur hangt af van de elektronegativiteit en het aantal zuurstofatomen dat aan het derde atoom is gebonden.Hoe hoger de elektronegativiteit van het atoom, hoe meer het polariseert, waardoor de binding tussen zuurstof en waterstof verzwakt. Als het centrale atoom is bevestigd aan extra zuurstofatomen, verhoogt dit de polariteit van de binding tussen zuurstof en waterstof verder. Perchloorzuur met drie extra zuurstofatomen is bijvoorbeeld sterker dan chloorzuur met twee extra zuurstofatomen.Chloorzuur is op zijn beurt sterker dan chlorigzuur, dat slechts één extra zuurstof en hypochloorzuur heeft, zonder extra zuurstofatomen. Carbonzuren zijn zwakke zuren die een carboxylgroep bevatten. Het tweede zuurstofatoom maakt de zuurstof-waterstofbinding meer polair, waardoor het molecuul een proton kan afstaan.Azijnzuur en mierenzuur zijn voorbeelden van carbonzuren.

zuursterkte en moleculaire structuur

Binaire zuren en basen Bij afwezigheid van enig nivellerend effect neemt de zuursterkte van binaire waterstofverbindingen met niet-metalen (A) toe naarmate de H-A-bindingssterkte afneemt in een groep in het periodiek systeem. Voor groep 17 is de volgorde van toenemende zuurgraad HF < HCl < HBr < HI. Op dezelfde manier is voor groep 16 de volgorde van toenemende zuursterkte H2O < H2S < H2Se < H2Te. Over een rij in het periodiek systeem neemt de zuursterkte van binaire waterstofverbindingen toe met toenemende elektronegativiteit van het niet-metaalatoom, omdat de polariteit van de H-A-binding toeneemt. De volgorde van toenemende zuurgraad (voor verwijdering van één proton) over de tweede rij is dus CH4 < NH3 < H2O < HF; op de derde rij is dit SiH4 < PH3 < H2S < HCl. Ternaire zuren en basen Ternaire verbindingen bestaande uit waterstof, zuurstof en een derde element (“E”) kunnen worden gestructureerd zoals weergegeven in de onderstaande afbeelding. In deze verbindingen is het centrale E-atoom gebonden aan een of meer O-atomen, en is ten minste één van de O-atomen ook gebonden aan een H-atoom, wat overeenkomt met de algemene molecuulformule OmE(OH)n. Deze verbindingen kunnen zuur, basisch of amfoteer zijn, afhankelijk van de eigenschappen van het centrale E-atoom. Voorbeelden van dergelijke verbindingen zijn onder meer zwavelzuur, O2S(OH)2, zwaveligzuur, OS(OH)2, salpeterzuur, O2NOH, perchloorzuur, O3ClOH, aluminiumhydroxide, Al(OH)3, calciumhydroxide, Ca(OH)2 en kaliumhydroxide, KOH. <img alt="Eq1" src="/files/ftp_upload/11406/11406_Figure_1.svg" style="height: 90px;"> Als het centrale atoom, E, een lage elektronegativiteit heeft, is de aantrekkingskracht voor elektronen laag. Er bestaat weinig neiging voor het centrale atoom om een sterke covalente binding te vormen met het zuurstofatoom, en binding a tussen het element en zuurstof wordt gemakkelijker verbroken dan binding b tussen zuurstof en waterstof. Daarom is binding a-ionisch, komen er hydroxide-ionen vrij in de oplossing en gedraagt het materiaal zich als een base – dit is het geval met Ca(OH)2 en KOH. Een lagere elektronegativiteit is kenmerkend voor de meer metalen elementen; vandaar dat de metaalelementen ionische hydroxiden vormen die per definitie basische verbindingen zijn. Als het atoom E daarentegen een relatief hoge elektronegativiteit heeft, trekt het de elektronen die het deelt met het zuurstofatoom sterk aan, waardoor een relatief sterke covalente binding ontstaat. De zuurstof-waterstofbinding, binding b, wordt daardoor verzwakt omdat elektronen naar E worden verplaatst. Binding b is polair en geeft gemakkelijk waterstofionen af aan de oplossing, zodat het materiaal zich als een zuur gedraagt. Hoge elektronegativiteiten zijn kenmerkend voor de meer niet-metalen elementen. Niet-metalen elementen vormen dus covalente verbindingen die zure −OH-groepen bevatten die oxyzuren worden genoemd. Het verhogen van het oxidatiegetal van het centrale atoom E verhoogt ook de zuurgraad van een oxyzuur omdat dit de aantrekkingskracht van E voor de elektronen die het deelt met zuurstof vergroot en daardoor de O-H-binding verzwakt. Zwavelzuur, H2SO4 of O2S(OH)2 (met een zwaveloxidatiegetal van +6), is zuurder dan zwaveligzuur, H2SO3 of OS(OH)2 (met een zwaveloxidatiegetal van +4). Op dezelfde manier is salpeterzuur, HNO3 of O2NOH (N-oxidatiegetal = +5), zuurder dan salpeterigzuur, HNO2 of ONOH (N-oxidatiegetal = +3). In elk van deze paren is het oxidatiegetal van het centrale atoom groter voor het sterkere zuur. Carbonzuren Carbonzuren bevatten een carboxylgroep. Carbonzuren zijn zwakke zuren, wat betekent dat ze niet 100% geïoniseerd zijn in water. Carbonzuur werkt als een zwak zuur omdat, zoals in het geval van oxyzuren, de tweede zuurstof die aan het koolstofatoom is gebonden de polariteit van de O-H-binding verhoogt en deze zwakker maakt. Verder wordt de carboxylgroep na het verlies van het proton omgezet in het carboxylaation, dat resonantie vertoont. De verschillende resonantiestructuren stabiliseren het carboxylaation terwijl de negatieve lading ervan over verschillende atomen wordt gedelokaliseerd.

Zuursterkte en moleculaire structuur

Binary Acids and Bases
In the absence of any leveling effect, the acid strength of binary compounds of hydrogen with nonmetals (A) increases as the H-A ...

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how bonding affects acid strength

Acid strength depends on bonding, electronegativity, and oxidation number. These factors help explain why some hydrogen compounds act as strong acids, while others behave as weak acids or bases.

For binary acids, which are hydrogen compounds with one other nonmetal, acidity increases as the H-A bond gets weaker down a group. That is why the order for group 17 is HF &lt; HCl &lt; HBr &lt; HI, and for group 16 it is H2O &lt; H2S &lt; H2Se &lt; H2Te. Across a period, acid strength increases as the nonmetal becomes more electronegative because the H-A bond becomes more polar. The second row follows CH4 &lt; NH3 &lt; H2O &lt; HF, and the third row follows SiH4 &lt; PH3 &lt; H2S &lt; HCl.

Ternary acids and bases contain hydrogen, oxygen, and a third element E. Their general form is OmE(OH)n, and they may be acidic, basic, or amphoteric. Examples include sulfuric acid, sulfurous acid, nitric acid, perchloric acid, aluminum hydroxide, calcium hydroxide, and potassium hydroxide.

If E has low electronegativity, it does not hold electrons strongly. In that case, the bond between E and oxygen is more likely to break than the O-H bond, so hydroxide ions are released and the compound acts as a base. This is typical of more metallic elements, which form ionic hydroxides such as Ca(OH)2 and KOH.

If E has high electronegativity, it pulls electron density toward itself. That weakens the O-H bond and makes it easier to release H+ ions, so the compound behaves as an acid. These nonmetal compounds are called oxyacids. A higher oxidation number on E also increases oxyacid strength because it pulls harder on shared electrons. For example, H2SO4 is more acidic than H2SO3, and HNO3 is more acidic than HNO2.

Carboxylic acids also show weak-acid behavior. They contain a carboxyl group, and they are not fully ionized in water. The second oxygen attached to carbon makes the O-H bond more polar and weaker. After the proton leaves, the carboxylate ion is stabilized by resonance, which spreads the negative charge over several atoms.

How Bonding Affects Acid Strength

bronsted-lowry acids and bases

Proton Transfer in Acids and Bases

Acids and bases can be understood through proton transfer. Early scientists described acids by their sour taste, their effect on dyes, and their reaction with limestone, which releases carbon dioxide. Robert Boyle also noted that acid solutions can lose these properties after contact with alkali, or base, solutions. The modern view developed step by step. Humphry Davy showed that hydrogen is the essential part of acids. Joseph Louis Gay-Lussac then described acids as substances that neutralize...

water: a bronsted-lowry acid and base

Water as an Amphiprotic Substance

Water can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base. When hydrogen fluoride dissolves in water, it donates protons to water. This is acid ionization. The products are hydronium ions and fluoride ions. Water can also accept protons from another substance. When pyridine dissolves in water, it accepts a proton from water molecules. This is base ionization. The products are hydroxide ions and pyridinium ions. These reactions show that water can play either role. A substance that...

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pH and pOH in Water

pH and pOH show how hydronium and hydroxide ions behave in water and other aqueous solutions. These ion concentrations are linked by the ion product of water, K w , so when one goes up, the other goes down. Because ion concentrations can differ by huge amounts, a logarithmic scale is used to describe them. pH is defined from the hydronium ion concentration, [H3O+], and pOH is the matching p-function for hydroxide ion concentration. These two values are also connected through the K w...

relative strengths of conjugate acid-base pairs

relative-strengths-of-conjugate-acid-base-pairs

How Ka and Kb Show Acid-Base Strength

Brønsted-Lowry acid-base chemistry is based on proton transfer. That idea helps show how the strength of an acid is linked to the strength of its conjugate base, and vice versa. Acid and base strength is measured with ionization constants, Ka and Kb, which tell how far an ionization reaction goes. For the conjugate pair HA and A−, the acid ionizes in water and the base reaction can be written for the partner species. When the two reactions are added, they give the autoionization of water. The...

strong acid and base solutions

Strong Acids, Strong Bases, and pH

Strong acids and strong bases change the pH of a solution by dissociating completely in water. A strong acid produces hydronium ions, which are H3O+ ions, and a strong base produces hydroxide ions, OH-. Because the dissociation is complete, the ion concentration can be found from the starting concentration and the molar ratio. For example, 0.20 M hydrobromic acid dissociates fully in water. It produces 0.20 M hydronium ions and 0.20 M bromide ions. A 0.015 M KOH solution also dissociates...

weak acid solutions

Weak Acid Equilibrium in Water

Weak acid equilibrium in water explains why many acids only partially react when dissolved. Most weak acid molecules stay in their original form, and only a small amount of hydronium ions forms. Weak acids are common in nature. They help create the tangy taste of citrus fruits, the stinging sensation from insect bites, and the smells linked to body odor. Acetic acid is a familiar weak acid. It is the main ingredient in vinegar. Its equation uses a double arrow to show that the reaction with...

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Weak Base pH and Kb Calculations

Weak base pH and Kb calculations show how partially reacting bases change water chemistry. Weak bases produce hydroxide ions when they dissolve by reacting with water molecules. Because the reaction only happens partly, these compounds are classified as weak bases. Weak bases are common in nature and in technology. Ammonia is one major example. Global production of ammonia is typically well over 100 metric tons each year. It is used as an agricultural fertilizer, a starting material for...

mixtures of acids

pH of Acid Mixtures

The pH of acid mixtures depends on the acids present, their dissociation constants, and their starting concentrations. When a solution contains two different acids, the pH can be found by choosing the method that fits their relative strengths. This makes acid mixtures a useful case for applying acid-base rules in chemistry. In a mixture of a strong acid and a weak acid, the strong acid dissociates completely and supplies almost all of the hydronium ions in the solution. The weak acid...

ions as acids and bases

Salt Hydrolysis and pH of Solutions

Salt hydrolysis explains why some salt solutions are acidic, basic, or neutral. Salts are ionic compounds made of cations and anions. In water, either ion may react with water through an acid or base ionization reaction. The pH of the solution depends on the relative acid-base strength of the ions in the salt. Ammonium chloride is a good example of an acidic salt. When it dissolves, it separates into ammonium ions and chloride ions. The ammonium ion is the conjugate acid of ammonia, so it can...

determining the ph of salt solutions

Salt Hydrolysis and pH in Solutions

Salt hydrolysis and pH in solutions depend on the ions released when a salt dissolves. Some ions react with water, while others do not. The balance between the cation and anion helps show whether the solution becomes acidic, basic, or neutral. Salts with pH-neutral anions and cations that produce hydronium ions give acidic solutions with pH below 7. Ammonium nitrate is one example. In NH4NO3, NO3− does not react with water, but NH4+ forms hydronium ions, so the solution is acidic. Other salts...

acid/base strengths and dissociation constants

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Acid and Base Strength in Water

Acid and base strength in water depends on how much a substance ionizes after it dissolves. If ionization is nearly complete, the substance is called strong. If only a small amount ionizes, it is called weak. Weak acids and weak bases are much more common than strong ones. The most common strong acids are HClO4, HCl, HBr, HI, HNO3, and H2SO4. The most common strong bases are LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. These strong acids and bases ionize essentially completely in water. <br...

polyprotic acids

Stepwise Ionization of Polyprotic Acids

Polyprotic acids lose hydrogen ions in steps. The number of ionizable protons in a molecule determines whether an acid is monoprotic, diprotic, or triprotic. This video also shows that polyprotic bases can accept more than one proton. Monoprotic acids have one ionizable hydrogen atom per molecule. Examples include HCl, HNO3, and HCN. Their reactions with water form hydronium ions and the matching anion. Acetic acid, CH3CO2H, is also monoprotic because only the hydrogen in the carboxyl group...

acid strength and molecular structure

Acid strength depends on bonding, electronegativity, and oxidation number. These factors help explain why some hydrogen compounds act as strong acids, while others behave as weak acids or bases. For binary acids, which are hydrogen compounds with one other nonmetal, acidity increases as the H-A bond gets weaker down a group. That is why the order for group 17 is HF &lt; HCl &lt; HBr &lt; HI, and for group 16 it is H2O &lt; H2S &lt; H2Se &lt; H2Te. Across a period, acid strength increases as...

lewis acids and bases

Electron-Pair Reactions in Acid-Base Chemistry

Electron-pair reactions explain Lewis acid-base chemistry. In 1923, G. N. Lewis described acids and bases by how they accept or donate a pair of electrons. When that electron pair forms a coordinate covalent bond, one atom supplies both bonding electrons. This bond is also called a dative bond. A simple example is the reaction of water with a hydrogen ion to make a hydronium ion. Ammonia can also combine with a hydrogen ion to form an ammonium ion. In both cases, the reaction creates a Lewis...

key terms and concepts

Learn how bond strength, electronegativity, oxidation number, and resonance help explain acid strength in binary acids, oxyacids, and carboxylic acids.

How Bonding Affects Acid Strength | JoVE K12

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How Bonding Affects Acid Strength

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