A Lewis acid is a species that can accept an electron pair, whereas a Lewis base has an electron pair available for donation to a Lewis acid. Complex ions are examples of Lewis acid-base adducts and comprise central metal atoms or ions acting as Lewis acids bonded to molecules or ions called ligands that act as Lewis bases. An approach to the Lewis acid-base model. Shortly after Bronsted and Lowry proposed their definition of acids and bases, the American chemist Gilbert Newton Lewis, building upon his new understanding of the nature of the chemical bond, proposed the definition that an acid is an electron pair acceptor while a base is an electron pair donor.This definition …Illustrated Examples. 1. The reaction of Lewis acids and bases with H+ ions. Answer: The reaction between the water molecule and the protons tends to make a hydronium ion (H3O+) 2. The reaction between Ag+ and ammonia. Answer: In this reaction, two lewis bases form an adduct with one lewis acid. 3.Water is probably the most common amphiprotic substance we will encounter, but other substances are also amphiprotic. Example 7.2.1 7.2. 1. Identify the Brønsted-Lowry acid and the Brønsted-Lowry base in this chemical equation. C6H5OH +NH−2 C6H5O− +NH3 C 6 H 5 OH + NH 2 − C 6 H 5 O − + NH 3.The Lewis Theory of acids and bases. This theory extends well beyond the things you normally think of as acids and bases. An acid is an electron pair acceptor. A base is an electron pair donor. Lewis bases. It is easiest to see the relationship by looking at exactly what Brønsted-Lowry bases do when they accept hydrogen ions. Three …The interaction between a magnesium cation (Mg 2+) and a carbonyl oxygen is a common example of a Lewis acid-base reaction in enzyme-catalyzed biological reactions. The carbonyl oxygen (the Lewis base) donates a pair of electrons to the magnesium cation (the Lewis acid). Further reading. Very detailed review of Lewis acids and bases, covering …The two theories are distinct but complementary. A Lewis base is also a Brønsted–Lowry base, but a Lewis acid does not need to be a Brønsted–Lowry acid. The classification into hard and soft acids and bases (HSAB theory) followed in 1963. Figure 4.11.2 4.11. 2: Use of non-aqueous solvents allows the study of strong acids that are hindered by the "leveling" of the solvent. Lewis proposed that the electron pair is the dominant actor in acid-base chemistry. An Lewis acid is a substance that accepts a pair of electrons, and in doing so, forms a covalent bond with the ….Martinique Lewis talks about her new book "The ABC Travel Green Book," and its importance for modern Black travelers. In the 1930s, the great open road in the United States meant f...The Lewis base is (CH 3) 2 S, and the Lewis acid is BH 3. As in the reaction shown in Equation 8.21, CO 2 accepts a pair of electrons from the O 2− ion in CaO to form the carbonate ion. The oxygen in CaO is an electron-pair donor, so CaO is the Lewis base.Dec 16, 2021 · The product between Lewis acids and Lewis bases is usually a species that has the acid and base joined together, and the product is called the “LA-LB adduct”. Other examples of Lewis acids include electron-deficient species, such as H +, M +, M 2+, BH 3, BF 3, AlCl 3 etc. Lewis bases can be: amine, ether or other species that have lone pair ... A Lewis base is a substance that can donate a pair of electrons to form a new bond. They are sometimes referred to as nucleophiles, or seekers of a positive nucleus. Neutralization is the sharing of an electron pair between an acid and base. The product formed in a neutralization reaction is sometimes called an adduct or complex.Arrhenius Definition. "an acidic substance is one whose molecular unit contains at least one hydrogen atom that can dissociate, or ionize, when dissolved in water, producing a hydrated hydrogen ion and an anion." hydrochloric acid. HCl → H +(aq) + Cl –(aq) sulfuric acid. H 2 SO 4 → H +(aq) + HSO 4–(aq)Nov 13, 2022 · According to Lewis, An acid is a substance that accepts a pair of electrons, and in doing so, forms a covalent bond with the entity that supplies the electrons. A base is a substance that donates an unshared pair of electrons to a recipient species with which the electrons can be shared. The Brønsted-Lowry picture of acids and bases as proton donors and acceptors is not the only definition in common use. A broader definition is provided by the Lewis theory of acids and bases, in which a Lewis acid is an electron-pair acceptor and a Lewis base is an electron-pair donor. This definition covers Brønsted-Lowry proton transfer reactions, but …Researchers are breeding beef cattle with more healthy fats. You’ve heard of the alpha dog. Get ready for the omega cow. Chinese researchers say they’ve reared beef rich in the ben...The Brønsted-Lowry picture of acids and bases as proton donors and acceptors is not the only definition in common use. A broader definition is provided by the Lewis theory of acids and bases, in which a Lewis acid is an electron-pair acceptor and a Lewis base is an electron-pair donor. This definition covers Brønsted-Lowry proton transfer reactions, but …Depending on the acid–base properties of its component ions, however, a salt can dissolve in water to produce a neutral solution, a basic solution, or an acidic solution. ... (H_3O^+\). Instead, a metal ion can act as a Lewis acid and interact with water, a Lewis base, by coordinating to a lone pair of electrons on the oxygen atom to form a …The Lewis theory of acids and bases states that acids act as electron pair acceptors and bases act as electron pair doners. This definition doesn't mention anything about the hydrogen atom at all, unlike the other definitions. It only talks about the transfer of electron pairs. To demonstrate this theory, consider the following example. This is a …HF + H2O -> H3O+ + F- Which is an acid-conjugate base pair?, What is the definition of a Lewis acid? and more. Study with Quizlet and memorize flashcards containing terms like Which term describes a substance that increases the concentration of hydroxide ions in solution?, Consider the reaction below. One of the most commonly-encountered kinds of Lewis acid-base reactions occurs when electron-donating ligands form coordination complexes with transition-metal ions. Figure 8.10.1 8.10. 1: The tin atom in SnCl 4 can expand its valence shell by utilizing a pair of d-orbitals, changing its hybridization from sp 3 to sp 3 d 2. The electrons donated from a Lewis base to a Lewis acid form a new bond. A new, larger compound is formed from the smaller Lewis acid and Lewis base. This compound is called a Lewis acid-base complex. A simple example of Lewis acid-base complexation involves ammonia and boron trifluoride. The nitrogen atom has a lone pair and is an electron donor.3 Jul 2018 ... The more free the lone pair is the stronger the base is, hence NI3 is the strongest base out of the trihalides. This is why NH3 is such a great ...Figure 3.8.2 3.8. 2: Use of non-aqueous solvents allows the study of strong acids that are hindered by the "leveling" of the solvent. 3.8: Lewis Acids and Bases is shared under a not declared license and was authored, remixed, and/or curated by LibreTexts. Lewis proposed that the electron pair is the dominant actor in acid-base …Lewis acids are the compounds which are electron deficient (less than 8 electrons in the central metal atom) and can accept the lone pair of electrons. Reason behind BF 3 acting as a Lewis Acid: BF 3 has 6 electrons in the central metal atom, boron. That's why, it is electron deficient and hence is a Lewis acid. Suggest Corrections.15.14: Lewis Acids and Bases. In 1923, G. N. Lewis proposed a generalized definition of acid-base behavior in which acids and bases are identified by their ability to accept or to donate a pair of electrons and form a coordinate covalent bond. A coordinate covalent bond (or dative bond) occurs when one of the atoms in the bond provides both ...Learn about the theory of Lewis acid and base, which is based on electron pairs rather than proton transfers. Find out the common examples, chemical reactions …Acid-base Reactions without Transferring Protons. The major utility of the Lewis definition is that it extends the concept of acids and bases beyond the realm of proton transfer reactions. The classic example is the reaction of boron trifluoride with ammonia to form an adduct: BF3 +NH3 → F3B−NH3 (2.9.1) (2.9.1) BF 3 + NH 3 → F 3 B …The Lewis acid-base reaction forms an additional bond with a relatively small energetic penalty of stretching the existing bonds: Because F-is a good Lewis base, and also a small anion, it can form stable octahedral anions with both main group elements and transition metals. For this reason, TiO 2 and SiO 2 dissolve in HF (but are unreactive …Denise asks "On one of your episodes, Joe Truini said that muriatic acid would remove scum and water deposits from tile in a bathroom. Where can I purchase muriatic acid?"Muriatic ...Martinique Lewis talks about her new book "The ABC Travel Green Book," and its importance for modern Black travelers. In the 1930s, the great open road in the United States meant f...Jun 30, 2023 · Lewis bases can be divided into two categories: hard bases contain small, relatively nonpolarizable donor atoms (such as N, O, and F), and. soft bases contain larger, relatively polarizable donor atoms (such as P, S, and Cl). Metal ions with the highest affinities for hard bases are hard acids, whereas metal ions with the highest affinity for ... The major utility of the Lewis definition is that it extends the concept of acids and bases beyond the realm of proton transfer reactions. The classic example is the reaction of boron trifluoride with ammonia to form an adduct: BF3 +NH3 → F3B−NH3 (8.6.1) (8.6.1) BF 3 + NH 3 → F 3 B − NH 3. One of the most commonly-encountered kinds of ...The Brønsted-Lowry picture of acids and bases as proton donors and acceptors is not the only definition in common use. A broader definition is provided by the Lewis theory of acids and bases, in which a Lewis acid is an electron-pair acceptor and a Lewis base is an electron-pair donor. This definition covers Brønsted-Lowry proton transfer reactions, but …3 Jul 2018 ... The more free the lone pair is the stronger the base is, hence NI3 is the strongest base out of the trihalides. This is why NH3 is such a great ..."The Fifth Risk" comes out Oct. 2. Outside the headlines that stream endlessly, about Trump’s possible ties to Russia, his Supreme Court nominee’s alleged sexual assault, his advis...FAQs on Lewis Acid and Base 1. Define Lewis Acid. A Lewis acid is a chemical species or molecule that can accept a pair of electrons to form a coordinate …Lewis acids and Lewis bases are defined in a more inclusive way that was first introduced by G.N. Lewis in 1923. Lewis Acid: a species that can accept an electron pair. Lewis Base: a species that can donate an electron pair. All Brønsted-Lowry acids and bases fit into the Lewis definition because the proton transfer process is essentially the reaction …The Lewis Acid definition is a broader one, so encompasses more compounds. A subset of these compounds would also qualify as Bronsted-Lowry Acids, since this definition is much …The hydrogen atom is not included in this theory's description of acids and bases. Lewis acids have electrophilic properties, while Lewis bases have nucleophilic properties. Cu 2+, BF 3, and Fe 3+ are examples of Lewis acids. F-, NH 3, and C 2 H 4 are examples of Lewis bases (ethylene). A Lewis acid absorbs an electron pair from a …The Lewis definitions are: “An acid is a substance which can accept an electron pair from a base; a base is a substance which can donate an electron pair” [13]. By this definition, every cation is an acid, in addition to chemical compounds such as BF 3 and SiO 2. The reaction of a Lewis acid and a Lewis base will produce a coordinate covalent bond, as shown in Figure 1.12.1 1.12. 1 above. A coordinate covalent bond is just a type of covalent bond in which one reactant gives it electron pair to another reactant. In this case the lewis base donates its electrons to the lewis acid.Lewis Acids and Bases. Gilbert Lewis (1875-1946) proposed a third theory of acids and bases that is even more general than either the Arrhenius or Brønsted-Lowry theories. A Lewis acid is a substance that accepts a pair of electrons to form a covalent bond. A Lewis base is a substance that donates a pair of electrons to form a covalent bond ...Illustrated Examples. 1. The reaction of Lewis acids and bases with H+ ions. Answer: The reaction between the water molecule and the protons tends to make a hydronium ion (H3O+) 2. The reaction between Ag+ and ammonia. Answer: In this reaction, two lewis bases form an adduct with one lewis acid. 3.Lewis Acid. It is a chemical species that consist of an empty orbital that is capable of accepting a pair of an electron from a Lewis base for making Lewis adduct. Trimethylborane is capable of accepting a lone pair, therefore, it is a Lewis acid. On the other hand, in a Lewis adduct, the Lewis acid and the Lewis base share a pair of an ...There are also Lewis acids and bases, which is a different theory about acid base chemistry. The Bronsted-Lowery definition refers to the loss or gain of an H+ (proton). The acid is a proton donor, and the base is a proton acceptor. The Arrhenius definition of an acid is an H+ producer and the base is an OH- producer. This approach is more limited …The Lewis Acid-Base definition is so broad that most (at least a very large group) organic reactions can be looked at as Lewis-Acid base reactions and the reacting species as acids and bases. Think about this; any chemical reaction involves electrons flowing from one species to another. That’s what we show with curved arrows and based on the ... Figure 3.8.2 3.8. 2: Use of non-aqueous solvents allows the study of strong acids that are hindered by the "leveling" of the solvent. 3.8: Lewis Acids and Bases is shared under a not declared license and was authored, remixed, and/or curated by LibreTexts. Lewis proposed that the electron pair is the dominant actor in acid-base …Nov 13, 2022 · Arrhenius Definition. "an acidic substance is one whose molecular unit contains at least one hydrogen atom that can dissociate, or ionize, when dissolved in water, producing a hydrated hydrogen ion and an anion." hydrochloric acid. HCl → H +(aq) + Cl –(aq) sulfuric acid. H 2 SO 4 → H +(aq) + HSO 4–(aq) John Lewis is one of the UK’s leading retailers, offering a wide range of products from fashion to home furnishings. With so many products available, it can be difficult to find th...The Hard and Soft Bases Concept (HSAB) The hard and soft acid and base concept (HSAB) can be conceived as a refinement of the Lewis-acid and base concept. Its most useful feature is that it can …List of Hard and Soft Lewis Acids and Bases. List of Hard and Soft Lewis Acids and Bases. Title. Microsoft Word - Document1. Author. yuming. Created Date. 9/14/2006 11:17:47 AM.When it comes to finding the perfect recliner for your home, John Lewis is a great place to start. With a wide selection of styles and sizes, you’re sure to find something that fit...The Lewis acid–base force between a hydroxyl group and another polar molecule is also known as hydrogen bonding, one of the most important bond types found in nature, contributing to 90% of noncovalent bonding. In the presence of water, the sum of acid–base interactions describes the wettability of a surface. When a bacterium and a biomaterial …15.14: Lewis Acids and Bases. In 1923, G. N. Lewis proposed a generalized definition of acid-base behavior in which acids and bases are identified by their ability to accept or to donate a pair of electrons and form a coordinate covalent bond. A coordinate covalent bond (or dative bond) occurs when one of the atoms in the bond provides both ...According to Lewis, An acid is a substance that accepts a pair of electrons, and in doing so, forms a covalent bond with the entity that supplies the electrons. A base is a substance that donates an unshared pair of electrons to a recipient species with which the electrons can be shared. In modern chemistry, electron donors are often referred ...3. It is expected that Aluminum forms a coordinate covalent bond as it can participate in a Lewis acid and a Lewis base interaction. For example \(Al^{3+}+H_{2}O \rightleftharpoons [Al(OH_2)_{6}]^{3+}\) 4. a. \(AlCl_{3}\) is a Lewis acid as \(Al\) can accept an electron pair. b. \(CH_{3}N\) is a Lewis base as \(N\) can donate an electron pair.Examples of Lewis Acid and Base [6 – 9] Lewis acid can be. Any cation that can accept electron pair: H +, Mg 2+, Fe 3+, NH 4+, and H 3 O +. Any molecule with an incomplete octet of electrons: BF 3 and AlCl 3. Any molecule where the central atom can have more than 8 electrons in its valence shell: SiCl 4 and SiF 4.Jun 30, 2023 · Lewis bases can be divided into two categories: hard bases contain small, relatively nonpolarizable donor atoms (such as N, O, and F), and. soft bases contain larger, relatively polarizable donor atoms (such as P, S, and Cl). Metal ions with the highest affinities for hard bases are hard acids, whereas metal ions with the highest affinity for ... The interaction between a magnesium cation (Mg 2+) and a carbonyl oxygen is a common example of a Lewis acid-base reaction in enzyme-catalyzed biological reactions. The carbonyl oxygen (the Lewis base) donates a pair of electrons to the magnesium cation (the Lewis acid). Further reading. Very detailed review of Lewis acids and bases, covering …Aug 14, 2021 · The Hard and Soft Bases Concept (HSAB) The hard and soft acid and base concept (HSAB) can be conceived as a refinement of the Lewis-acid and base concept. Its most useful feature is that it can make predictions about the strength of the acid-base interactions. It can also estimate if the interactions are more ionic or more more covalent. Water is probably the most common amphiprotic substance we will encounter, but other substances are also amphiprotic. Example 7.2.1 7.2. 1. Identify the Brønsted-Lowry acid and the Brønsted-Lowry base in this chemical equation. C6H5OH +NH−2 C6H5O− +NH3 C 6 H 5 OH + NH 2 − C 6 H 5 O − + NH 3.A Lewis acid-base reaction occurs when a base donates a pair of electrons to an acid. In many Lewis acid-base reactions, a Lewis acid-base adduct, a compound that contains a coordinate covalent bond between the Lewis acid and the Lewis base, is formed. Example 5. 6.1 – Id entifying Lewis Acids & Bases. Identify the acid and the base in each Lewis …Write equations for the formation of adducts and complex ions. In 1923, G. N. Lewis proposed a generalized definition of acid-base behavior in which acids and bases are identified by their ability to accept or to donate a pair of electrons and form a coordinate covalent bond. A coordinate covalent bond (or dative bond) occurs when one of the ...In 1923, G.N. Lewis from UC Berkeley proposed an alternate theory to describe acids and bases. His theory gave a generalized explanation of acids and bases based on …There are three primary theories of acid-base chemistry that are often taught together: Arrhenius theory, Brønsted-Lowry theory, and Lewis acid-base theory. Each theory is introduced below. Figure 7.1A. 1 7.1 A. 1: Hierarchal definitions of acids and bases via the three primary theories. These theories are designed to be "superset" of the ... When it comes to finding the perfect recliner for your home, John Lewis is a great place to start. With a wide selection of styles and sizes, you’re sure to find something that fit...Mar 6, 2017 · Example Lewis Acid-Base Reaction. While Brønsted theory cannot explain the formation of complex ions with a central metal ion, Lewis acid-base theory sees the metal as the Lewis Acid and the ligand of the coordination compound as a Lewis Base. Al 3+ + 6H 2 O ⇌ [Al (H 2 O) 6] 3+. The aluminum metal ion has an unfilled valence shell, so it ... Learn about the theory of Lewis acid and base, which is based on electron pairs rather than proton transfers. Find out the common examples, chemical reactions …Water is probably the most common amphiprotic substance we will encounter, but other substances are also amphiprotic. Example 7.2.1 7.2. 1. Identify the Brønsted-Lowry acid and the Brønsted-Lowry base in this chemical equation. C6H5OH +NH−2 C6H5O− +NH3 C 6 H 5 OH + NH 2 − C 6 H 5 O − + NH 3.Alpha-Lipoic Acid (Alpha Lipoic) received an overall rating of 5 out of 10 stars from 13 reviews. See what others have said about Alpha-Lipoic Acid (Alpha Lipoic), including the ef...The combined use of Lewis acids (electron-pair acceptors) and Lewis bases (electron-pair donors) for simultaneous activation of electrophiles and nucleophiles has proven to be a synthetically highly versatile concept. Catalytic systems consisting of Lewis acid and Lewis base functions, present in a single molecule or in separate molecules ...Dec 25, 2022 · Figure 3.11.2 3.11. 2: Use of non-aqueous solvents allows the study of strong acids that are hindered by the "leveling" of the solvent. 3.11: Lewis Acids and Bases is shared under a not declared license and was authored, remixed, and/or curated by LibreTexts. Lewis proposed that the electron pair is the dominant actor in acid-base chemistry. In the Lewis acid-base complexation reaction, these two entities (an acid and a base) come together, resulting in a more substantial molecule. So for instance let me illustrate it on the example I have BF3 which is a good Lewis acid because it can accept electrons and I have let’s say a diethyl ether molecule over here which can donate electron density and …Jul 17, 2023 · An acid and a base which differ only by the presence or absence of a proton are called a conjugate acid-base pair. Thus NH 3 is called the conjugate base of NH 4+, and NH 4+ is the conjugate acid of NH 3. Similarly, HF is the conjugate acid of F –, and F – the conjugate base of HF. Example 11.13.1 11.13. 1 : Conjugate Pairs. A Lewis acid-base reaction occurs when a base donates a pair of electrons to an acid. A Lewis acid-base adduct, a compound that contains a coordinate covalent bond between the Lewis acid and the Lewis base, is formed. The following equations illustrate the general application of the Lewis concept. The boron atom in boron …Nov 13, 2022 · Arrhenius Definition. "an acidic substance is one whose molecular unit contains at least one hydrogen atom that can dissociate, or ionize, when dissolved in water, producing a hydrated hydrogen ion and an anion." hydrochloric acid. HCl → H +(aq) + Cl –(aq) sulfuric acid. H 2 SO 4 → H +(aq) + HSO 4–(aq) Classify the following species into Lewis acids and Lewis bases and show how these act as Lewis acid/base: (a) O H − (b) F − (c) H + (d) B C l 3. View Solution Q 2The Brønsted-Lowry picture of acids and bases as proton donors and acceptors is not the only definition in common use. A broader definition is provided by the Lewis theory of acids and bases, in which a Lewis acid is an electron-pair acceptor and a Lewis base is an electron-pair donor. This definition covers Brønsted-Lowry proton …Lewis Acids and Bases ( Read ) | Chemistry | CK-12 Foundation. Click Create Assignment to assign this modality to your LMS. We have a new and improved read on this topic. Click here to view. We have moved all content for this concept to for better organization. Please update your bookmarks accordingly. To better organize out content, …
acid–base reaction, a type of chemical process typified by the exchange of one or more hydrogen ions, H +, between species that may be neutral ( molecules, such as water, H 2 O; or acetic acid, CH 3 CO 2 H) or electrically charged (ions, such as ammonium, NH 4+; hydroxide, OH −; or carbonate, CO 32− ). It also includes analogous behaviour ... . Nearest domino's pizza near me
A Lewis acid is an electron pair acceptor; a Lewis base is an electron pair donor (see below). Some metal oxides (like aluminium oxide) are amphoteric - they react both as acids and bases. For example, they react as bases because the oxide ions accept hydrogen ions to make water. Lewis acids are electrophilic in nature whereas Lewis Bases possess nucleophilic qualities. Examples of Lewis acids: Cu 2+, BF 3, and Fe 3+. Examples of Lewis bases: …9 years ago. Acids and Bases are on the reactants side of an equation. There conjugate acid or base will be on the products side of the equation. Acids will have a conjugate base and Bases will have a conjugate acid. For example: HCl-->H (+) + Cl (-) You have an acid on the reactants side. The Lewis acid/base theme is one of the most widely used theories, and it goes beyond the H+ and OH- ions to define acids and bases. Apart from academics, we have also encountered several uses of acid and base in our daily life. So, go thoroughly through lewis acid and base study material to better understand the topic. Lewis Acid.In Lewis's doctrinal explanations, acids and bases are divided on the basis of electrons. Lewis acid can be defined as receiving an electron pair that receives ...A Lewis acid is a species that can accept an electron pair, whereas a Lewis base has an electron pair available for donation to a Lewis acid. Complex ions are examples of Lewis acid-base adducts and comprise central metal atoms or ions acting as Lewis acids bonded to molecules or ions called ligands that act as Lewis bases.The Hard Soft Acid Base Principle is a Conceptual Tool for Thinking About Patterns of Lewis Acid-Base Reactivity. The explanation of the trends in metal distribution, halide salt solubility, and preferred metal coordination patterns is rooted in Arland, Chatt, and Davies' observation that Lewis acids and bases could be classified into two groups based on …Jul 17, 2023 · An acid and a base which differ only by the presence or absence of a proton are called a conjugate acid-base pair. Thus NH 3 is called the conjugate base of NH 4+, and NH 4+ is the conjugate acid of NH 3. Similarly, HF is the conjugate acid of F –, and F – the conjugate base of HF. Example 11.13.1 11.13. 1 : Conjugate Pairs. A Lewis acid-base reaction occurs when a base donates a pair of electrons to an acid. A Lewis acid-base adduct, a compound that contains a coordinate covalent bond between the Lewis acid and the Lewis base, is formed. The following equations illustrate the general application of the Lewis concept. The boron atom in boron trifluoride, BF 3, has only six …21 Jul 2022 ... For example, trimethyl boron is an electron pair acceptor, a lewis acid whereas ammonia being electron-rich (with nitrogen), is a lewis base.The Lewis definition of acids and bases is more encompassing than the Brønsted–Lowry definition because it’s not limited to substances that donate or accept just protons. A Lewis acid is a substance that accepts an electron pair, and a Lewis base is a substance that donates an electron pair. The donated electron pair is shared between the ...The Lewis definition of acids and bases is more encompassing than the Brønsted–Lowry definition because it’s not limited to substances that donate or accept just protons. A Lewis acid is a substance that accepts an electron pair, and a Lewis base is a substance that donates an electron pair. The donated electron pair is shared between the ....