Name: how bonding affects acid strength
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 3 min 5 s
Channel: JoVE

K12 Standards

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North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.6.3

Acid Strength and Molecular Structure

Hidroklorik asit güçlü bir asit iken, hidroflorik asit zayıf bir asittir. Peki asitlerin güçlerini belirleyen şey nedir? Yalnızca iki elemente sahip ikili asitlerin gücü, bağ enerjisi ve bağ polaritesi ile belirlenir.Daha yüksek bir bağ enerjisine sahip bir asit daha güçlü bir bağa sahiptir ve bu nedenle daha zayıf bir asit olacaktır. Bir gruptaki asitleri karşılaştırırsak, hidroflorik asit gibi zayıf bir asitteki bağın kırılması daha zordur, bu nedenle asidin proton verme olasılığı daha düşüktür. Aksine, daha düşük bağ enerjisine sahip bir asit daha zayıf bir bağa sahiptir ve bu nedenle daha güçlü bir asit olacaktır.Örneğin hidroklorik asit gibi güçlü bir asitteki bağ, hidroflorik asitten daha kolay parçalanır ve protonları daha kolay verir. Hidroklorik asitte olduğu gibi bir bağ, bir atom diğer atomdan daha elektronegatif olduğunda kutupsaldır. Hidrojene bağlı atom hidrojenden daha yüksek elektronegatifliğe sahip olduğunda bir bileşik asit görevi görebilir.Atomun hidrojenin kısmi bir pozitif yüke sahip olmasına izin verecek kısmi bir negatif yükü olacak ve böylece bir proton olarak salınabilecektir. Daha yüksek bağ polaritesine sahip bir asit daha zayıf bir bağa sahiptir ve bu nedenle daha güçlü bir asit olacaktır. Bir periyodik tabloda bileşikleri karşılaştırırken, hidroklorik asit, klor sülfürden daha elektronegatif olduğundan ve bu nedenle protonları daha kolay saldığından, hidrojen sülfürden daha güçlüdür.Hidrojenin diğer atoma eşit veya daha büyük bir elektronegatifliği varsa, bu molekül proton veremez ve bu nedenle bir asit görevi göremez. Oksiasitler, bir OH'nin hidrojenden daha elektronegatif olan üçüncü bir atoma eklendiği asitlerdir. Bir oksiasidin gücü, elektronegatifliğe ve üçüncü atoma bağlı oksijenlerin sayısına bağlıdır.Atomun elektronegatifliği ne kadar yüksekse, o kadar çok polarize olur ve oksijen ile hidrojen arasındaki bağı zayıflatır. Merkezi atom ek oksijen atomlarına bağlanırsa, oksijen ile hidrojen arasındaki bağın polaritesini daha da artırır. Örneğin, üç ilave oksijen atomuna sahip perklorik asit iki ilave oksijen atomlu klorik asitten daha güçlüdür.Klorik asit ise, yalnızca bir ek oksijen ve hipokloröz asite sahip olan ve oksijen atomu içermeyen klorlu asitten daha güçlüdür. Karboksilik asitler, bir karboksil grubu içeren zayıf asitlerdir. İkinci oksijen atomu, oksijen-hidrojen bağını daha polar hale getirir ve böylece molekülün bir proton vermesine izin verir.Asetik asit ve formik asit, karboksilik asitlerin örnekleridir.

asit gücü ve moleküler yapı

İkili Asitler ve Bazlar
 
 Herhangi bir tesviye etkisinin yokluğunda, H-A bağ kuvveti periyodik tablodaki bir grup aşağıya düştükçe, hidrojenin ametaller (A) ile ikili bileşiklerinin asit mukavemeti artar. Grup 7A için, asitlik artış sırası HF < HCl < HBr < HI'dır. Benzer şekilde, grup 6A için, asit kuvvetinin artış sırası H2O < H2S < H2Se < H2Te'dir. Periyodik tablodaki bir sıra boyunca, ikili hidrojen bileşiklerinin asit kuvveti, metal olmayan atomun artan elektronegatifliği ile artar, çünkü H-A bağının polaritesi artar. Bu nedenle, ikinci satır boyunca artan asitliğin (bir protonun çıkarılması için) sırası CH4 < NH3 < H2O < HF;'dir; üçüncü sırada ise SiH4 < PH3 < H2S < HCl'dir.
 
 Üçlü Asitler ve Bazlar
 
 Hidrojen, oksijen ve bazı üçüncü elementlerden ((“E”) oluşan üçlü bileşikler, aşağıdaki resimde gösterildiği gibi yapılandırılabilir. Bu bileşiklerde, merkezi E atomu bir veya daha fazla O atomuna bağlanır ve O atomlarından en az biri, genel moleküler formül OmE(OH)n'ya karşılık gelen bir H atomuna da bağlanır. Bu bileşikler, merkezi E atomunun özelliklerine bağlı olarak asidik, bazik veya amfoterik olabilir. Bu tür bileşiklerin örnekleri arasında sülfürik asit, O2S(OH)2, sülfüröz asit, OS(OH)2, nitrik asit, O2NOH, perklorik asit, O3ClOH, alüminyum hidroksit, Al(OH)3, kalsiyum hidroksit, Ca(OH)2 ve potasyum hidroksit, KOH bulunur.
 
 <img alt=""Eq1"" src=""/files/ftp_upload/11406/11406_Figure_1.svg"" style=""height: 90px;"" />
 
 Merkez atom E'nin elektronegatifliği düşükse, elektron çekiciliği düşüktür. Merkezi atomun oksijen atomu ile güçlü bir kovalent bağ oluşturma eğilimi azdır ve element ile oksijen arasındaki a bağı, oksijen ve hidrojen arasındaki b bağından daha kolay kırılır. Dolayısıyla bağ a iyoniktir, hidroksit iyonları çözeltiye salınır ve malzeme bir baz görevi görür —bu, Ca(OH)2 ve KOH içeren durumdur. Daha düşük elektronegatiflik, daha metalik elementlerin karakteristiğidir; dolayısıyla metalik elementler, tanımları gereği temel bileşikler olan iyonik hidroksitleri oluşturur.
 
 Öte yandan, E atomu nispeten yüksek bir elektronegatifliğe sahipse, oksijen atomuyla paylaştığı elektronları güçlü bir şekilde çekerek nispeten güçlü bir kovalent bağ oluşturur. Oksijen-hidrojen bağı, bağ b, böylece zayıflatılır çünkü elektronlar E'ye doğru yer değiştirir. Bağ b polar olup, hidrojen iyonlarını çözeltiye kolayca salar, böylece malzeme bir asit gibi davranır. Yüksek elektronegatiflikler, daha metalik olmayan elementlerin karakteristiğidir. Böylece, metal olmayan elementler, oksiasitler adı verilen asidik−OH grupları içeren kovalent bileşikler oluşturur.
 
 Merkez atom E'nin oksidasyon sayısını artırmak, bir oksiasitin asitliğini de arttırır çünkü bu, E'nin oksijenle paylaştığı elektronlar için çekiciliğini artırır ve dolayısıyla O-H bağını zayıflatır. Sülfürik asit, H2SO4 veya O2S(OH)2 (sülfür oksidasyon sayısı +6), sülfüröz asitten, H2SO3 veya OS(OH)2'den (sülfür oksidasyon numarası +4) daha asidiktir. Benzer şekilde, nitrik asit, HNO3 veya O2NOH (N oksidasyon numarası = +5), nitröz asitten, HNO2 veya ONOH'den (N oksidasyon numarası = +3) daha asidiktir. Bu çiftlerin her birinde, merkez atomunun yükseltgenme sayısı, daha güçlü asit için daha büyüktür.
 
 Karboksilik Asitler
 
 Karboksilik asitler bir karboksil grubu içerir. Karboksilik asitler zayıf asitlerdir, yani suda % 100 iyonize olmazlar.
 
 Karboksilik asit, oksiasitlerde olduğu gibi, karbon atomuna bağlanan ikinci oksijen O-H bağının polaritesini arttırdığı ve onu zayıflattığı için zayıf bir asit görevi görür. Ayrıca, proton kaybından sonra karboksil grubu, rezonans sergileyen karboksilat iyonuna dönüştürülür. Negatif yükü birkaç atom üzerinde yer değiştirdiği için, farklı rezonans yapıları karboksilat iyonunu stabilize eder.
 
 Bu metin bu kaynaklardan uyarlanmıştır: <a href=""https://openstax.org/books/chemistry-2e/pages/14-3-relative-strengths-of-acids-and-bases""> Openstax, Chemistry 2e, Section 14.3: Relative Strengths of Acids and Bases</a> ve <a href=""https://openstax.org/books/chemistry-2e/pages/20-3-aldehydes-ketones-carboxylic-acids-and-esters"">Openstax, Chemistry 2e, Section 20.3 Aldehydes, Ketones, Carboxylic Acids, and Esters</a>.

Asit Gücü ve Moleküler Yapı

İkili Asitler ve Bazlar
Herhangi bir tesviye etkisinin yokluğunda, ametaller (A) ile ikili hidrojen bileşiklerinin asit mukavemeti, H-A ...

Education

JoVE Core

Kimya

Acids and Bases

Asitler ve Bazlar

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

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...

ph scale

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...

weak base solutions

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

acidbase-strengths-and-dissociation-constants

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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JoVE Core Kimya, özlü ve kolay anlaşılır animasyon video derslerini kullanarak genel kimya kavramlarına hayat veriyor. Ek olarak, bilim insanı uygulama videolarımız ile klasik ve orijinal araştırma deneylerini dünya çapında günümüz laboratuvarlarında görselleştiriyoruz.

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Construct an explanation to infer the atomic size, reactivity, electronegativity, and ionization energy of an element based on its position in the Periodic Table.

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Trends in Lattice Energy: Ion Size and Charge

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Resonance

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	...

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Molecular Comparison of Gases, Liquids, and Solids

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Intermolecular vs Intramolecular Forces

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Surface Tension, Capillary Action, and Viscosity

Surface Tension
The various IMFs between identical molecules of a substance are examples of cohesive forces. The molecules within a liquid are surrounded ...

Construct an explanation to summarize the influences intermolecular forces have on the properties of chemical compounds.

PS.Chm.3.2

Analyze the structure of atoms and isotopes.

How Bonding Affects Acid Strength

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