Name: proton transfer in acids and bases
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 2 min 58 s
Channel: JoVE

K12 Standards

north-carolina-k-12-science-standard-course-of-study

North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.6.3

Bronsted-Lowry Acids and Bases

Eine Arrhenius-Säure ist eine Substanz, die ein Wasserstoffion erzeugt, wenn sie in Wasser gelöst wird, und eine Arrhenius-Base ist eine Substanz, die ein OH−- oder Hydroxid-Ion erzeugt.
Salzsäure ist eine Arrheniussäure, da sie in Wasser gelöst in ein Wasserstoffion und ein Chloridion dissoziiert. Natriumhydroxid ist eine Arrhenius-Base, da es in Wasser gelöst in ein Natriumion und ein Hydroxidion dissoziiert.
Diese Definition kann jedoch nicht verwendet werden, um Säuren und Basen zu beschreiben, die sich nicht in einer wässrigen Lösung befinden, oder Basen, die keine Hydroxidionen enthalten.
Eine weiter gefasste Definition von Brønsted und Lowry definiert eine Säure als Wasserstoffionen- oder Protonendonor, während eine Base ein Protonenakzeptor ist.
Wenn Salzsäure in Wasser gelöst wird, wirkt sie wie eine Säure, indem sie ein Proton an Wasser abgibt, wodurch ein Hydroniumion und ein Chloridion entstehen. Wenn Ammoniak in Wasser gelöst wird, fungiert es als Base und nimmt ein Proton aus Wasser auf, wodurch ein Ammoniumion und ein Hydroxidion entstehen.
Eine Brønsted-Lowry-Säure reagiert immer mit einer Brønsted-Lowry-Base und umgekehrt. Wenn eine Säure, zum Beispiel Essigsäure, ihr Proton abgibt, fungiert Wasser als Base und nimmt das Proton auf. Essigsäure wird in eine konjugierte Base, Acetat, umgewandelt, und Wasser wird in eine konjugierte Säure, ein Hydronium-Ion, umgewandelt.
Säuren und Basen, die sich durch die Übertragung eines Protons voneinander unterscheiden, werden als konjugierte Säure-Basen-Paare bezeichnet. In der Umkehrreaktion fungiert die konjugierte Säure Hydronium als Protonendonor und die konjugierte Base Acetat nimmt ein Proton auf. 
Die Stärke einer Säure wird durch ihre Fähigkeit bestimmt, ein Proton zu spenden, während die Stärke einer Base durch ihre Fähigkeit bestimmt wird, ein Proton aufzunehmen. Eine stärkere Säure spendet mit größerer Wahrscheinlichkeit ein Proton als eine schwächere Säure. Ebenso ist es wahrscheinlicher, dass eine stärkere Base ein Proton aufnimmt als eine schwächere Base.
Die Stärke einer Säure und ihre konjugierte Base stehen in einem umgekehrten Verhältnis. Eine starke Säure dissoziiert in Lösung vollständig und die resultierende konjugierte Base ist zu schwach, um ein Proton aufzunehmen. Gleiches gilt für eine starke Base und deren konjugierte Säure.
Andererseits dissoziiert eine schwache Säure teilweise in Lösung. Die konjugierte Base einer schwachen Säure ist ebenfalls relativ schwach; Daher liegt ein Gemisch aus der undissoziierten schwachen Säure und ihrer schwachen konjugierten Base im Gleichgewicht vor. Das gleiche Phänomen tritt bei einer schwachen Base und ihrer schwachen konjugierten Säure auf.

<ol>
	<li>Geschichte, David A. "Bench-to-bedside review: Eine kurze Geschichte der klinischen Säure-Base." Critical Care 8, Nr. 4 (2004): 253.</li>
</ol>

bronsted-lowry-säuren und basen

Die Klasse der Säure-Base-Reaktionen wird seit geraumer Zeit untersucht. Im Jahr 1680 berichtete Robert Boyle über die Eigenschaften saurer Lösungen, darunter ihre Fähigkeit, viele Substanzen aufzulösen, die Farben bestimmter natürlicher Farbstoffe zu ändern und diese Eigenschaften nach dem Kontakt mit alkalischen (basischen) Lösungen zu verlieren. Im 18. Jahrhundert erkannte man, dass Säuren einen säuerlichen Geschmack haben, mit Kalkstein reagieren und eine gasförmige Substanz (heute bekannt als CO2) freisetzen und mit Alkalien interagieren, um neutrale Substanzen zu bilden. Im Jahr 1815 trug Humphry Davy maßgeblich zur Entwicklung des modernen Säure-Base-Konzepts bei, indem er zeigte, dass Wasserstoff der wesentliche Bestandteil von Säuren ist. Ungefähr zur gleichen Zeit kam Joseph Louis Gay-Lussac zu dem Schluss, dass Säuren Substanzen sind, die Basen neutralisieren können, und dass diese beiden Substanzklassen nur voneinander definiert werden können. Die Bedeutung von Wasserstoff wurde 1884 erneut betont, als Svante Arrhenius eine Säure als eine Verbindung definierte, die sich in Wasser auflöst und Wasserstoffkationen (heute als Hydroniumionen bekannt) ergibt, und eine Base als eine Verbindung, die sich in Wasser auflöst und Hydroxidanionen ergibt. Brønsted-Lowry-Säuren und Basen Johannes Brønsted und Thomas Lowry schlugen 1923 eine allgemeinere Beschreibung vor, in der Säuren und Basen anhand der Übertragung von Wasserstoffionen, H+, definiert wurden. (Beachten Sie, dass diese Wasserstoffionen oft einfach als Protonen bezeichnet werden, da dieses subatomare Teilchen die einzige Komponente von Kationen ist, die vom am häufigsten vorkommenden Wasserstoffisotop, 1H, abgeleitet sind.) Eine Verbindung, die ein Proton an eine andere Verbindung abgibt, wird Brønsted-Lowry genannt Säure, und eine Verbindung, die ein Proton aufnimmt, wird Brønsted-Lowry-Base genannt. Eine Säure-Base-Reaktion ist also die Übertragung eines Protons von einem Donor (Säure) auf einen Akzeptor (Base). Das Konzept der konjugierten Paare ist nützlich bei der Beschreibung von Brønsted-Lowry-Säure-Base-Reaktionen (und auch anderen reversiblen Reaktionen). Wenn eine Säure H+ abgibt, wird die verbleibende Spezies als konjugierte Base der Säure bezeichnet, da sie in der Rückreaktion als Protonenakzeptor reagiert. Wenn eine Base H+ aufnimmt, wird sie ebenfalls in die entsprechende Säure umgewandelt. Die Reaktion zwischen Wasser und Ammoniak veranschaulicht diese Idee wie unten gezeigt.  <img alt="Eq1" src="/files/ftp_upload/11394/11394_Equation_1.png" style="height: 50px;"> In Vorwärtsrichtung wirkt Wasser als Säure, indem es ein Proton an Ammoniak abgibt und anschließend zu einem Hydroxidion, OH−, der konjugierten Base von Wasser, wird. Das Ammoniak fungiert als Base bei der Aufnahme dieses Protons und wird zu einem Ammoniumion, NH4+, der konjugierten Säure von Ammoniak. In der umgekehrten Richtung fungiert ein Hydroxidion als Base, indem es ein Proton vom Ammoniumion aufnimmt, das als Säure wirkt. Starke Säuren und Basen dissoziieren in einer Lösung vollständig. Ihre konjugierten Säuren und Basen sind extrem schwach und können die Protonen nicht abgeben bzw. aufnehmen, um die Rückreaktion durchzuführen; Daher verlaufen Reaktionen mit starken Säuren und Basen in einer wässrigen Lösung im Wesentlichen vollständig. Andererseits dissoziieren schwache Säuren und Basen teilweise in Lösungen und erzeugen schwache konjugierte Basen bzw. Säuren. Diese schwachen konjugierten Säuren oder Basen können die Rückreaktion durchführen, und so erreichen Reaktionen schwacher Säuren und Basen ein Gleichgewicht, abhängig von den relativen Stärken der schwachen Säuren und Basen. Zusammenfassend lässt sich sagen, dass eine stärkere Säure die ebenso schwächere konjugierte Base erzeugt, während eine stärkere Base die ebenso schwächere konjugierte Säure erzeugt und umgekehrt. Tabelle 1 zeigt die Beziehung zwischen verschiedenen konjugierten Säure-Base-Paaren. <table style="margin-left: auto; margin-right: auto;"> <tbody> <tr> <td style="color: black; border: 1px solid black; text-align: center;">Strong Acid</td> <td style="color: black; border: 1px solid black; text-align: center;">Very Weak Conjugate Base</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">HCl</td> <td style="color: black; border: 1px solid black; text-align: center;">Cl−</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">HNO3</td> <td style="color: black; border: 1px solid black; text-align: center;">NO3−</td> </tr> <tr> <td colspan="2"></td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">Weak Acid</td> <td style="color: black; border: 1px solid black; text-align: center;">Weak Conjugate Base</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">HF</td> <td style="color: black; border: 1px solid black; text-align: center;">F−</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">NH4+</td> <td style="color: black; border: 1px solid black; text-align: center;">NH3</td> </tr> <tr> <td colspan="2"></td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">Very Weak Acid</td> <td style="color: black; border: 1px solid black; text-align: center;">Strong Conjugate Base</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">OH−</td> <td style="color: black; border: 1px solid black; text-align: center;">O2−</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">CH4</td> <td style="color: black; border: 1px solid black; text-align: center;">CH3−</td> </tr> </tbody> </table> Tabelle 1: Relative Stärke einiger konjugierter Säure-Base-Paare. Dieser Text ist adaptiert von <a href="https://openstax.org/books/chemistry-2e/pages/14-1-bronsted-lowry-acids-and-bases">Openstax, Chemistry 2e, Section 14.4 Brønsted-Lowry Acid and Bases</a>

Bronsted-Lowry-Säuren und Basen

Die Säure-Base-Reaktionsklasse wird schon seit geraumer Zeit untersucht. Im Jahr 1680 berichtete Robert Boyle über Eigenschaften von sauren Lösungen, zu denen ihre Fähigkeit gehörte, ...

Education

Lehre

JoVE Core

Chemie

Eins

Acids and Bases

Säuren und Basen

KEY TERMS AND CONCEPTS

KERNBEGRIFFE UND KONZEPTE

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 bases. In 1884, Svante Arrhenius defined acids as compounds that produce hydrogen cations in water and bases as compounds that produce hydroxide anions.

Brønsted and Lowry gave a broader definition in 1923. A Brønsted-Lowry acid donates a proton, and a Brønsted-Lowry base accepts a proton. An acid-base reaction is the transfer of that proton from the donor to the acceptor. The hydrogen ion, H+, is often called a proton because it is the only particle in the most common hydrogen isotope.

Conjugate pairs help describe these reactions. After an acid donates H+, the species left behind is its conjugate base. After a base accepts H+, it becomes its conjugate acid. Water and ammonia show this clearly. In the forward direction, water donates a proton to ammonia, so water acts as an acid and becomes hydroxide, OH−, while ammonia acts as a base and becomes ammonium, NH4+.

The reverse reaction also fits the same pattern. Hydroxide can accept a proton, so it acts as a base. Ammonium can donate a proton, so it acts as an acid. Strong acids and strong bases dissociate completely in solution, and their conjugate acids and bases are extremely weak. That is why reactions with strong acids and bases in water usually go to completion.

Weak acids and weak bases behave differently. They only partially dissociate in solution and form weak conjugate bases or weak conjugate acids. These conjugate species can take part in the reverse reaction, so weak acid-base reactions reach equilibrium. In general, a stronger acid gives a weaker conjugate base, and a stronger base gives a weaker conjugate acid.

Proton Transfer in Acids and Bases

bronsted-lowry 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

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...

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 Brønsted-Lowry acids and bases work through proton transfer, conjugate pairs, and the difference between strong and weak acid-base reactions.

Proton Transfer in Acids and Bases | JoVE K12

chemistry

JoVE Core Chemie erweckt allgemeine Konzepte der Chemie durch kompakte und leicht verständliche animierte Videolektionen zum Leben. Außerdem zeigen wir in den Videos Wissenschaftler in Aktion bei klassischen und neuartigen Forschungsexperimenten, wie sie heutzutage in Laboren weltweit durchgeführt wurden.

Physical Science

PS.PSc.2.5

ohios-learning-standards-and-model-curriculum

Ohio’s Learning Standards and Model Curriculum

Interactions Of Matter

Chemical reactions

Tennessee Academic Standards

High School

Matter and Its Interactions

CHEM1.PS1.8

Texas Essential Knowledge and Skills

CHEM.12

CHEM.12.B

Alabama Course of Study Science

9-12.C.1.6

9-12.C.1.6.a

9-12.C.1.6.c

9-12.PS.3.6.c

Florida Department of Education

SC.912.P.8

SC.912.P.8.11

new-york-state-science-learning-standards

New York State Science Learning Standards

HS. Chemical Reactions

HS-PS1-11.

Georgia Standards of Excellence

SPS6.

Acid and Base Structure

SC6.

acid-base-models-arrhenius-vs-bronsted-lowry

Acid-Base Models: Arrhenius vs. Bronsted-Lowry

Scientific Laws and Theories

Scientific Laws

In science, a law is defined as a concise, verbal or mathematical, statement that summarizes a vast number of experimental observations. ...

The Scientific Method

Chemistry is an empirical science. Scientists often pose questions to understand the chemistry in everyday life and seek answers to these questions. To ...

Classifying Matter by State

Chemistry is the study of matter and the changes it undergoes. Matter is anything that has mass and occupies space. Matter is all around us; the air, ...

Classifying Matter by Composition

Matter: Pure Substances and Mixtures
According to its composition, the matter can be classified into two broad categories &mdash; pure substances and ...

The Atomic Theory of Matter

The earliest recorded discussion of the basic structure of matter comes from ancient Greek philosophers. Leucippus and Democritus argued that all matter ...

Subatomic Particles

Dalton was only partially correct about the particles that make up matter. All matter is composed of atoms, and atoms are composed of three smaller ...

Elements: Chemical Symbols and Isotopes

A chemical symbol is an abbreviation used to indicate an element or an atom of an element. For example, the symbol for mercury is Hg. The same symbol is ...

Use models to explain how the scientific understanding of atomic structure has evolved.

PS.Chm.1.1

Radioactivity and Nuclear Equations

Nuclear chemistry is the study of reactions that involve changes in nuclear structure. The nucleus of an atom is composed of protons and, except for ...

Types of Radioactivity

The most common types of radioactivity are &#945; decay, &#946; decay, &#947; decay, neutron emission, and electron capture.
Alpha (&#945;) decay is the ...

Nuclear Stability

Protons and neutrons, collectively called nucleons, are packed together tightly in a nucleus. With a radius of about 10&#8722;15 meters, a nucleus is ...

Nuclear Binding Energy

The difference between the calculated and experimentally measured masses is known as the mass defect of the atom. In the case of helium-4, the mass defect ...

Radioactive Decay and Radiometric Dating

Radioactivity is a spontaneous disintegration of an unstable nuclide and is a random process, as all the nuclei in the sample do not decay simultaneously. ...

Nuclear Fission

Many heavier elements with smaller binding energies per nucleon can decompose into more stable elements that have intermediate mass numbers and larger ...

Nuclear Power

Controlled nuclear fission reactions are used to generate electricity. Any nuclear reactor that produces power via the fission of uranium or plutonium by ...

Nuclear Fusion

The process of converting very light nuclei into heavier nuclei is also accompanied by the conversion of mass into large amounts of energy, a process ...

Nuclear Transmutation

Nuclear transmutation is the conversion of one nuclide into another. It can occur by the radioactive decay of a nucleus, or the reaction of a nucleus with ...

Use models to compare nuclear reactions including alpha decay, beta decay and gamma decay; nuclear fusion and nuclear fission.

PS.Chm.1.2

Atomic Orbitals

An atomic orbital represents the three-dimensional regions in an atom where an electron has the highest probability to reside. The radial distribution ...

The Pauli Exclusion Principle

The arrangement of electrons in the orbitals of an atom is called its electron configuration. We describe an electron configuration with a symbol that ...

The Energies of Atomic Orbitals

In an atom, the negatively charged electrons are attracted to the positively charged nucleus. In a multielectron atom, electron-electron repulsions are ...

The Aufbau Principle and Hund's Rule

To determine the electron configuration for any particular atom, we can build the structures in the order of atomic numbers. Beginning with hydrogen, and ...

electron-configuration-of-multielectron-atoms

Electron Configuration of Multielectron Atoms

The alkali metal sodium (atomic number 11) has one more electron than the neon atom. This electron must go into the lowest-energy subshell available, the ...

Use models to explain how electrons are distributed in atoms.

PS.Chm.1.3

Periodic Classification of the Elements

The periodic table arranges atoms based on increasing atomic number so that elements with the same chemical properties recur periodically. When their ...

The Periodic Table

As early chemists discovered more elements, they realized that various elements could be grouped by their similar chemical behaviors. One such grouping ...

Atomic Mass

Atoms &mdash; and the protons, neutrons, and electrons that compose them &mdash; are extremely small. For example, a carbon atom weighs less than 2 ...

Molar Mass

The identity of a substance is defined not only by the types of atoms or ions it contains but by the quantity of each type of atom or ion. For example, ...

Use the Periodic Table as a model to predict the relative properties of elements based on the pattern of valence electrons in the outermost energy levels of atoms.

PS.Chm.2.1

atomic-radii-and-effective-nuclear-charge

Atomic Radii and Effective Nuclear Charge

The elements in groups of the periodic table exhibit similar chemical behavior. This similarity occurs because the members of a group have the same number ...

Ionic Radii

Ionic radius is the measure used to describe the size of an ion. A cation always has fewer electrons and the same number of protons as the parent atom; it ...

Ionization Energy

The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called its first ionization energy ...

Electron Affinity

The electron affinity (EA) is the energy change for adding an electron to a gaseous atom to form an anion (negative ion).



This process can be either ...

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

PS.Chm.2.2

Types of Chemical Bonds

Chemical bonding theories were pioneered by American chemist Gilbert&#xA0;N. Lewis. He developed a model called the Lewis model to explain the type and ...

Lewis Symbols and the Octet Rule

Chemical bonds are complex interactions between two or more atoms or ions, which reduce the potential energy of the molecule. Gilbert N. Lewis developed a ...

Ionic Bonding and Electron Transfer

Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence ...

The Born-Haber Cycle

Lattice Energy&#xA0;

An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a ...

trends-in-lattice-energy-ion-size-and-charge

Trends in Lattice Energy: Ion Size and Charge

An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a compound is a measure ...

Covalent Bonding and Lewis Structures

Compared to ionic bonds, which results from the transfer of electrons between metallic and nonmetallic atoms, covalent bonds result from the mutual ...

Electronegativity

Whether a bond is nonpolar or polar covalent is determined by a property of the bonding atoms called electronegativity.&#xA0;

Electronegativity values of ...

bond-polarity-dipole-moment-and-percent-ionic-character

Bond Polarity, Dipole Moment, and Percent Ionic Character

Bond Polarity

The absolute value of the difference in electronegativity (&Delta;EN) of two bonded atoms provides a rough measure of the polarity to be ...

lewis-structures-of-molecular-compounds-and-polyatomic-ions

Lewis Structures of Molecular Compounds and Polyatomic Ions

To draw Lewis structures for complicated molecules and molecular ions, it is helpful to follow a step-by-step procedure as outlined:


	Determine the ...

Resonance

The Lewis structure of a nitrite anion (NO2&minus;) may actually be drawn in two different ways, distinguished by the locations of the N-O and N=O ...

Formal Charges

In some cases, there are seemingly more than one valid Lewis structures for molecules and polyatomic ions. The concept of formal charges can be used to ...

Exceptions to the Octet Rule

Many covalent molecules have central atoms that do not have eight electrons in their Lewis structures. These molecules fall into three categories:


	...

Analyze and interpret data to explain the mechanisms and properties of the two main types of intramolecular (ionic and covalent) bonds.

PS.Chm.3.1

Analyze the structure of atoms and isotopes.

Proton Transfer in Acids and Bases

Description

Transcript

Tags

More videos by Standards