Name: salt hydrolysis and ph in solutions
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 4 min 8 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

Physical Science

Matter and its Interactions

PS.PSc.2.5

Determining the pH of Salt Solutions

Las soluciones salinas pueden ser ácidas, básicas o neutras. Los iones individuales se pueden examinar para determinar si el pH de su solución será inferior, superior o igual a siete. Las sales que contienen cationes y aniones de pH neutro forman soluciones neutras.Estas sales están compuestas por contraiones de un ácido fuerte y una base fuerte. Una solución acuosa pura de nitrato de potasio tendrá un pH de 7, ya que ni el potasio ni el nitrato tienen propiedades ácidas o básicas. Las sales que contienen un catión que es el contraión de una base débil y un anión que es el contraión de un ácido fuerte tendrán un pH inferior a 7.En una solución de bromuro de amonio, los iones de bromuro tienen un pH neutro, mientras que los iones de amonio son ácidos y donan protones a las moléculas de agua. Las sales que contienen un catión que es el contraión de una base fuerte y un anión que es el contraión de un ácido débil tendrán un pH superior a 7. En una solución de acetato de sodio, los iones de sodio tienen un pH neutro, mientras que los iones de acetato son básicos y aceptan protones de las moléculas de agua.Algunas sales contienen un catión y un anión que son contraiones de un ácido débil y una base débil, respectivamente. La solución será ácida si el Ka del catión es mayor que el Kb del anión;y será básica si el Kb del anión es mayor que el Ka del catión;o neutral si Ka y Kb son iguales. En una solución de nitrito de amonio, el Ka para el amonio es más alto que el Kb para los iones de nitrito;por tanto, la solución será ácida.El pH exacto de una solución salina que contiene un ion ácido o básico se puede determinar usando la constante de disociación para el ácido o base conjugado de ese ion. El pH del cianuro de sodio 0, 35 molar se puede determinar calculando los Kb de cianuro a partir del Ka de su ácido conjugado y configurando una tabla ICE para determinar la concentración de equilibrio. Como los cationes de sodio no reaccionan con el agua, no afectan el pH y pueden omitirse.Por el contrario, los iones de cianuro aceptan protones de moléculas de agua y generan iones de hidróxido. El Kb para los iones de cianuro se puede determinar usando la ecuación Ka multiplicado por Kb es igual a Kw.Como el Ka para el ácido cianhídrico es 4, 90 10⁻¹⁰, el Kb para los iones de cianuro es 2, 04 10⁻⁵. El Kb es igual a la concentración de ácido cianhídrico multiplicada por la concentración de iones de hidróxido dividida por la concentración de iones de cianuro.Se puede construir una tabla ICE para expresar las concentraciones inicial y de equilibrio. Si se sustituyen las concentraciones de equilibrio en la expresión, Kb es igual a x por x dividido por 0, 35, lo que se puede verificar más adelante mediante la regla del 5 porciento. Al resolver la ecuación, x es igual a 2, 7 10⁻³ molar.Como x es solo el 0, 77 porciento de 0, 35 molar, la aproximación 0, 35 menos x es igual a 0, 35 es válida. El pOH de la solución se puede calcular tomando el logaritmo negativo de 2, 7 10⁻³ molar, que equivale a 2, 57. El pH de la solución se determina usando la ecuación pH más pOH es igual a 14;por lo tanto, el pH de esta solución de cianuro de sodio es 11, 43.

determinando el ph de las soluciones salinas

El pH de una solución salina es determinado por sus aniones y cationes componentes. Las sales que contienen aniones pH-neutros y los cationes productores de iones hidronio forman una solución con un pH inferior a 7. Por ejemplo, en la solución de nitrato de amonio (NH4NO3), los iones NO3− no reaccionan con el agua, mientras que los iones NH4+ producen los iones hidronio que resultan en la solución ácida.  Por el contrario, las sales que contienen cationes pH-neutros y los aniones productores de iones hidróxido forman una solución con un pH superior a 7. Por ejemplo, en la solución de fluoruro de sodio (NaF), el Na+ es pH-neutro, pero el F- produce los iones hidróxido y forma la solución básica. Los contraiones de un ácido o base fuerte son pH-neutros y las sales formadas por tales contraiones forman una solución neutra con un pH igual a 7. Por ejemplo, en KBr, el catión K+ es inerte y no afectará al pH. El ion bromuro es la base conjugada de un ácido fuerte, y por lo tanto es de una fuerza de base insignificante (no hay una ionización de base apreciable). La solución es neutra.
 Algunas sales contienen tanto un catión ácido como un anión básico. La acidez o alcalinidad general de una solución está determinada por la fuerza relativa del catión y el anión, que se puede comparar con Ka y Kb. Por ejemplo, en el NH4F, el ion NH4+ es ácido y el ion F− es básico (base conjugada del ácido débil HF). Comparando las dos constantes de ionización: la Ka de NH4+ es 5,6 × 10−10 y la Kb del F− es 1,6 × 10−11, por lo que la solución es ácida, ya que Ka > Kb.
 Calcular el pH de una solución de sal ácida
 La anilina es una amina que se utiliza para fabricar colorantes. Se aísla como cloruro de anilinio, [C6H5NH3+], una sal preparada a partir de la reacción entre la base débil anilina y el ácido clorhídrico. ¿Cuál es el pH de una solución 0,233 M de cloruro de anilinio?
 <img alt="Eq1" src="/files/ftp_upload/11404/11404_Equation_1.png" style="height: 50px;" />
 La Ka para el ion anilinio se deriva de la Kb para su base conjugada, anilina:
 <img alt="Eq2" src="/files/ftp_upload/11404/11404_Equation_2.png" style="height: 90px;" />
 Con la información proporcionada, se prepara una tabla ICE para este sistema:
 <table style="margin-left: auto; margin-right: auto;">
 <tbody>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;"></td>
 <td style="color: black; border: 1px solid black; text-align: center;">C6H5NH3+ (aq)</td>
 <td style="color: black; border: 1px solid black; text-align: center;">H3O+ (aq)</td>
 <td style="color: black; border: 1px solid black; text-align: center;">C6H5NH2 (ac)</td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">Concentración inicial (M)</td>
 <td style="color: black; border: 1px solid black; text-align: center;">0,233</td>
 <td style="color: black; border: 1px solid black; text-align: center;">~0</td>
 <td style="color: black; border: 1px solid black; text-align: center;">0</td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">Cambio (M)</td>
 <td style="color: black; border: 1px solid black; text-align: center;">−x</td>
 <td style="color: black; border: 1px solid black; text-align: center;">+x</td>
 <td style="color: black; border: 1px solid black; text-align: center;">+x</td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">Concentración de equilibrio (M)</td>
 <td style="color: black; border: 1px solid black; text-align: center;">0,233 −x</td>
 <td style="color: black; border: 1px solid black; text-align: center;">x</td>
 <td style="color: black; border: 1px solid black; text-align: center;">x</td>
 </tr>
 </tbody>
 </table>
 Al sustituir estos términos de concentración de equilibrio en la expresión Ka queda
 <img alt="Eq3" src="/files/ftp_upload/11404/11404_Equation_3.png" style="height: 90px;" />
 Suponiendo que x << 0,233, la ecuación se simplifica y se resuelve para x:  
 <img alt="Eq4" src="/files/ftp_upload/11404/11404_Equation_4.png" style="height: 90px;" />
 <img alt="Eq5" src="/files/ftp_upload/11404/11404_Equation_5.png" style="height: 50px;" />
 La tabla ICE define x como la molaridad del ion hidronio, y por lo tanto el pH se calcula como
 <img alt="Eq6" src="/files/ftp_upload/11404/11404_Equation_6.png" style="height: 50px;" />
 Hidrólisis de [Al(H2O)6]3+ 
 Calcular el pH de una solución de cloruro de aluminio de 0,10 M, que se disuelve completamente para dar el ion de aluminio hidratado [Al(H2O)6]3+ en solución.
 La ecuación para la reacción y la Ka son: 
 <img alt="Eq7" src="/files/ftp_upload/11404/11404_Equation_7.png" style="height: 90px;" />
 Una tabla ICE con la información proporcionada es
 <table style="margin-left: auto; margin-right: auto;">
 <tbody>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;"></td>
 <td style="color: black; border: 1px solid black; text-align: center;">Al(H2O)63+(ac)</td>
 <td style="color: black; border: 1px solid black; text-align: center;">H3O+(ac)</td>
 <td style="color: black; border: 1px solid black; text-align: center;">Al(H2O)5(OH)2+ (ac)</td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">Concentración inicial (M)</td>
 <td style="color: black; border: 1px solid black; text-align: center;">0,10</td>
 <td style="color: black; border: 1px solid black; text-align: center;">~0</td>
 <td style="color: black; border: 1px solid black; text-align: center;">0</td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">Cambio (M) </td>
 <td style="color: black; border: 1px solid black; text-align: center;">−x</td>
 <td style="color: black; border: 1px solid black; text-align: center;">+x </td>
 <td style="color: black; border: 1px solid black; text-align: center;">+x </td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">Concentración de equilibrio (M)</td>
 <td style="color: black; border: 1px solid black; text-align: center;">0,10 − x</td>
 <td style="color: black; border: 1px solid black; text-align: center;">x</td>
 <td style="color: black; border: 1px solid black; text-align: center;">x</td>
 </tr>
 </tbody>
 </table>
 Si se sustituyen las expresiones de las concentraciones de equilibrio en la ecuación para la constante de ionización, se obtiene:
 <img alt="Eq8" src="/files/ftp_upload/11404/11404_Equation_8.png" style="height: 90px;" />
 Si se asume que x << 0,10 y se resuelve la ecuación simplificada, se obtiene:
 <img alt="Eq9" src="/files/ftp_upload/11404/11404_Equation_9.png" style="height: 50px;" />
 La tabla ICE define x como igual a la concentración de iones hidronio, y por lo que se calcula que el pH es 2,92, y la solución es ácida.
 <img alt="Eq10" src="/files/ftp_upload/11404/11404_Equation_10.png" style="height: 90px;" />
 Este texto es adaptado de<a href="https://openstax.org/books/chemistry-2e/pages/14-4-hydrolysis-of-salts"> Openstax, Química 2e, Sección 14.4: Hidrólisis de las Sales</a>.

Determinando el pH de las Soluciones Salinas

El pH de una solución salina está determinado por sus componentes aniones y cationes. Las sales que contienen aniones de pH neutro y los cationes productores de iones hidronio ...

Education

Educación

JoVE Core

Chemistry

Química

Acids and Bases

Ácidos y bases

KEY TERMS AND CONCEPTS

TÉRMINOS Y CONCEPTOS CLAVE

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 contain pH-neutral cations and anions that produce hydroxide ions. These salts form basic solutions with pH above 7. Sodium fluoride is an example. In NaF, Na+ is pH-neutral, while F− reacts with water to produce hydroxide ions.

Salts made from the counterions of a strong acid or a strong base are usually neutral. Their solutions have a pH of 7. In KBr, K+ is inert and does not change the pH. Br− is the conjugate base of a strong acid, so it has negligible base strength and does not appreciably ionize in water.

Some salts contain both an acidic cation and a basic anion. In those cases, the overall pH depends on which ion is stronger. The ionization constants Ka and Kb are used to compare them. For NH4F, NH4+ is acidic and F− is basic. Because Ka for NH4+ is 5.6 × 10−10 and Kb for F− is 1.6 × 10−11, the solution is acidic since Ka is greater than Kb.

The pH of an acidic salt solution can be calculated with an ICE table. Anilinium chloride, [C6H5NH3+]Cl, comes from the weak base aniline and hydrochloric acid. For a 0.233 M solution, the Ka value for the anilinium ion is found from the Kb of aniline. The ICE table gives x as the hydronium ion concentration, and the pH is then calculated from that value.

Hydrolysis of the hydrated aluminum ion works the same way. Aluminum chloride dissolves completely to give [Al(H2O)6]3+ in solution. For a 0.10 M solution, the reaction and Ka are set up in an ICE table. After assuming x is much smaller than 0.10 and solving the simplified equation, the hydronium ion concentration gives a pH of 2.92. The solution is acidic.

Salt Hydrolysis and pH in Solutions

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...

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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

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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 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

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Electron-Pair Reactions in Acid-Base Chemistry

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key terms and concepts

Learn how salt ions affect pH, from acidic ammonium salts and basic fluoride salts to neutral salts and pH calculations with ICE tables.

Salt Hydrolysis and pH in Solutions | JoVE K12

chemistry

JoVE Core Química da vida a los conceptos de química general mediante lecciones de vídeo basadas en animaciones, concisas y fáciles de entender. Además, en los vídeos de científicos en acción, se muestran experimentos de investigación clásicos y originales realizados en laboratorios de todo el mundo.

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Ohio’s Learning Standards and Model Curriculum

Interactions Of Matter

Chemical reactions

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CHEM.12.D

Alabama Course of Study Science

Matter and Its Interactions

9-12.C.1.6

9-12.C.1.6.d

9-12.PS.3.6.c

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 ...

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 ...

Molecules and Compounds

Atoms and Molecules

Everything in the universe is made up of matter, and matter is composed of a combination of elements. An atom is the smallest unit of ...

Solution Formation

There is no one solvent that can dissolve every type of solute. Some substances that readily dissolve in a certain solvent might be insoluble in a ...

Colloids

Children at play often make suspensions such as mixtures of mud and water, flour and water, or a suspension of solid pigments in water known as tempera ...

Construct an explanation to classify matter as a pure substance or mixture; homogeneous or heterogeneous; element or compound; solution, colloid or suspension.

PS.PSc.1.1

Phase Transitions

Whether solid, liquid, or gas, a substance&#39;s state depends on the order and arrangement of its particles (atoms, molecules, or ions). Particles in the ...

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Phase Transitions: Vaporization and Condensation

The physical form of a substance changes on changing its temperature. For example, raising the temperature of a liquid causes the liquid to vaporize ...

Vapor Pressure

When a liquid vaporizes in a closed container, gas molecules cannot escape. As these gas phase molecules move randomly about, they will occasionally ...

Clausius-Clapeyron Equation

The equilibrium between a liquid and its vapor depends on the temperature of the system; a rise in temperature causes a corresponding rise in the vapor ...

Phase Transitions: Melting and Freezing

Heating a crystalline solid increases the average energy of its atoms, molecules, or ions, and the solid gets hotter. At some point, the added energy ...

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Phase Transitions: Sublimation and Deposition

Some solids can transition directly into the gaseous state, bypassing the liquid state, via a process known as sublimation. At room temperature and ...

Heating and Cooling Curves

When a substance&#8212;isolated from its environment&#8212;is subjected to heat changes, corresponding changes in temperature and phase of the substance ...

Phase Diagrams

A phase diagram combines plots of pressure versus temperature for the liquid-gas, solid-liquid, and solid-gas phase-transition equilibria of a substance. ...

Use models to compare the phases of matter and the physical changes they undergo.

PS.PSc.1.2

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Physical and Chemical Properties of Matter

The characteristics that enable us to distinguish one substance from another are called properties.

Physical Properties of Matter

A physical property is ...

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Molecular Comparison of Gases, Liquids, and Solids

Particles in a solid are tightly packed together (fixed shape) and often arranged in a regular pattern; in a liquid, they are close together with no ...

Intermolecular vs Intramolecular Forces

Intermolecular forces (IMF) are electrostatic attractions arising from charge-charge interactions between molecules. The strength of the intermolecular ...

Intermolecular Forces

Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions ...

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Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility

Intermolecular forces are attractive forces that exist between molecules. They dictate several bulk properties, such as melting points, boiling points, ...

Carry out investigations to compare physical and chemical properties of matter.

PS.PSc.1.3

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 ...

The Bohr Model

Following the work of Ernest Rutherford and his colleagues in the early twentieth century, the picture of atoms consisting of tiny dense nuclei surrounded ...

Emission Spectra

When solids, liquids, or condensed gases are heated sufficiently, they radiate some of the excess energy as light. Photons produced in this manner have a ...

The de Broglie Wavelength

In the macroscopic world, objects that are large enough to be seen by the naked eye follow the rules of classical physics. A billiard ball moving on a ...

The Uncertainty Principle

Werner Heisenberg considered the limits of how accurately one can measure properties of an electron or other microscopic particles. He determined that ...

Use models to interpret the data presented in Bohr diagrams and electron dot diagrams for neutral atoms of elements 1 through 18.

PS.PSc.1.4

Ions and Ionic Charges

In ordinary chemical reactions, the nucleus &mdash; which contains the protons and neutrons of each atom and thus identifies the element &mdash; remains ...

Use models to compare representations of atoms, ions, and isotopes.

PS.PSc.1.5

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 ...

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 ...

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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 ...

Alkali Metals

Group 1 elements are soft and shiny metallic solids. They are malleable, ductile, and good conductors of heat and electricity. The melting points of the ...

Halogens

Group 17 elements, known as halogens, are nonmetals. At room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine a solid. ...

Noble Gases


The elements in group 18 are noble gases (helium, neon, argon, krypton, xenon, and radon). They earned the name &ldquo;noble&rdquo; because they were ...

Use the Periodic Table as a model to predict the relative properties (metallic/nonmetallic character, ionic charge, and reactivity) and arrangement of elements based on the pattern of valence electrons in the outermost energy levels of atoms.

PS.PSc.1.6

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 ...

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 ...

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 ...

Bonding in Metals

Metallic bonds are formed between two metal atoms. A simplified model to describe metallic bonding has been developed by Paul Dr&#xFC;de called the ...

Construct an explanation to classify the type of chemical bond that occurs (covalent, ionic, or metallic) in a given substance.

PS.PSc.2.1

Nomenclature of Alkanes

In the late 19th-century, the number of new chemical compounds discovered increased tremendously. Hence, the necessity arose to develop a naming system ...

Nomenclature of Alkenes

The IUPAC naming system for alkenes replaces -an- with -en- in the corresponding parent alkanes. Accordingly, a simple alkene replaces the -ane suffix of ...

Nomenclature of Alkynes

Alkynes are unsaturated hydrocarbons characterized by the presence of carbon-carbon triple bonds and have a general formula CnH2n-2. The nomenclature of ...

structure-and-nomenclature-of-alcohols-and-phenols

Structure and Nomenclature of Alcohols and Phenols

Overview 
Alcohols are one of the most important functional groups in organic chemistry. The name of alcohol comes from the hydrocarbon from which it is ...

Structure and Nomenclature of Ethers

Structure and Bonding
Ethers are organic compounds with an ether functional group which is characterized by an oxygen atom connected to two &#8212; ...

IUPAC Nomenclature of Aldehydes

Aldehydes are named based on the systematic nomenclature rules set by the IUPAC. For acyclic aldehydes, the longest carbon chain containing the aldehydic ...

IUPAC Nomenclature of Ketones

Like aldehydes, ketones are named using IUPAC rules; in this case, by replacing &#8220;e&#8221; in the name of the longest hydrocarbon chain with ...

IUPAC Nomenclature of Carboxylic Acids

IUPAC names of carboxylic acids are systematically derived following a few rules discussed below.
For acyclic saturated monocarboxylic acids, the longest ...

Use models to apply International Union of Pure and Applied Chemistry (IUPAC) conventions to name and write formulas for simple compounds.

PS.PSc.2.2

Understand types, properties, and structure of matter.

Salt Hydrolysis and pH in Solutions

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