Name: acid and base strength in water
Uploaded: 2025-10-30T13:58:47.000Z
Duration: 3 min 2 s
Channel: JoVE

K12 Standards

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

NC K-12 Science Standard Course of Study

9-12

Physical Science

Matter and its Interactions

PS.PSc.2.5

acidbase-strengths-and-dissociation-constants

Acid/Base Strengths and Dissociation Constants

Les acides et les bases peuvent être classés selon qu'ils sont un acide fort, une base forte, un acide faible ou une base faible. Il y a très peu d'acides et de bases forts donc la majorité des acides et des bases sont faibles. Un acide fort, comme l'acide chlorhydrique, se dissocie complètement en ions hydrogène et en ions chlorure lorsqu'il est dissous dans l'eau.Une base forte, comme l'hydroxyde de sodium, se dissocie complètement en ions sodium et en ions hydroxyde. Les acides faibles et les bases se dissocient partiellement et sont présents sous des formes ionisées et non ionisées. Par exemple, à la fois l'acide acétique et sa faible base conjuguée, acétate, se trouvent dans une solution aqueuse.Le degré de dissociation d'un acide ou d'une base faible peut être mesurée en utilisant sa constante d'équilibre. La constante d'équilibre pour les acides faibles a un nom spécial, la constante de dissociation acide, ou, Ka.Pour un acide faible générique HA, Ka à une température donnée peut être calculée par une équation d'équilibre:divisant la concentration de produits, d'ion A et d'ion hydronium par la concentration de réactifs, HA et eau. Comme l'eau est liquide et sa concentration reste pratiquement inchangée dans la réaction, elle est exclue de l'équation.Plus le Ka est élevé, plus l'acide est fort. L'acide nitreux est plus fort que l'acide acétique parce que le Ka de l'acide nitreux est plus grand que le Ka de l'acide acétique. La constante d'équilibre pour les bases faibles, la base de constante de dissociation, ou Kb, agit de la même manière que Ka.Pour une base faible générique B, Kb à une température donnée peut être déterminée en divisant la concentration des produits, L'ion BH et l'ion hydroxyde, par la concentration du réactif, B.Comme les acides, la force des bases est également directement proportionnel au Kb.Par exemple, l'éthylamine est relativement plus forte que l'urée parce que le Kb de l'éthylamine est plus grand que le Kb de l'urée.La force d'un acide peut également être exprimée en termes de pourcentage d'ionisation. Le pourcentage d'ionisation de l'acide peut être calculé en divisant la concentration en ions hydronium à l'équilibre par la concentration d'acide initiale et en le multipliant par cent. De même, le pourcentage d'ionisation pour les bases peut être calculé en divisant la concentration en ions hydroxyde à l'équilibre par la concentration initiale de base et en le multipliant par cent.Plus le pourcentage d'ionisation est élevé, plus l'acide ou la base.

forces des acides/bases et constantes de dissociation

La force relative d'un acide ou d'une base est la mesure dans laquelle il s'ionise lorsqu'il est dissous dans l'eau. Si la réaction d'ionisation est essentiellement totale, on dit que l'acide ou la base est fort ; s'il se produit relativement peu d'ionisation, l'acide ou la base est faible. Il y a beaucoup plus d'acides et de bases faibles que de forts. Les acides forts et les bases fortes les plus courants sont énumérés ci-dessous : 
 <table style="margin-left: auto; margin-right: auto;">
 <tbody>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">Acides forts </td>
 <td style="color: black; border: 1px solid black; text-align: center;">Bases fortes </td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">HClO4</td>
 <td style="color: black; border: 1px solid black; text-align: center;">LiOH </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;">NaOH </td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">HBr </td>
 <td style="color: black; border: 1px solid black; text-align: center;">KOH </td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">HI </td>
 <td style="color: black; border: 1px solid black; text-align: center;">Ca(OH)2 </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;">Sr(OH)2 </td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">H2SO4</td>
 <td style="color: black; border: 1px solid black; text-align: center;">Ba(OH)2 </td>
 </tr>
 </tbody>
 </table>
 Les forces relatives des acides peuvent être quantifiées en mesurant leurs constantes d'équilibre dans des solutions aqueuses. Dans des solutions de même concentration, les acides plus forts s'ionisent de façon plus importante et produisent donc des concentrations plus élevées d'ions hydronium que les acides plus faibles. La constante d'équilibre d'un acide est appelée la constante d'ionisation de l’acide, Ka. Pour la réaction d'un acide HA :   
 <img alt="Eq1" src="/files/ftp_upload/11395/11395eq1.png" style="text-align: center; height: 50px;" />
 La constante d'ionisation de l’acide est écrite comme  
 <img alt="Eq2" src="/files/ftp_upload/11395/11395eq2.png" style="text-align: center; height: 90px;" />
 où les concentrations sont celles à l'équilibre. Bien que l'eau soit un réactif dans la réaction, c'est aussi le solvant, nous n'incluons donc pas [H2O] dans l'équation. Plus le Ka d'un acide est élevé, plus la concentration de H3O+ et de A− est importante par rapport à la concentration de l'acide non ionisé HA dans un mélange en équilibre, et plus l'acide est fort. Un acide est classé comme “ fort ” lorsqu'il subit une ionisation totale, auquel cas la concentration de HA est nulle et la constante d'ionisation de l’acide est infiniment grande (Ka ≈ ∞). On dit que les acides partiellement ionisés sont “ faibles ” et leurs constantes d'ionisation de l’acide peuvent être mesurées expérimentalement. 
 Pour illustrer cette idée, les équations de l'ionisation de trois acides et les valeurs de Ka sont présentées ci-dessous. Les constantes d'ionisation augmentent de la première à la dernière des équations dans la liste, indiquant que la force relative de l'acide augmente dans l'ordre CH3CO2 < HNO2 < HSO4−. 
 <img alt="Eq3-5" src="/files/ftp_upload/11395/11395eq3-5.png" style="text-align: center; height: 135px;" />
 Une autre mesure de la force d'un acide est son ionisation en pourcentage. L'ionisation en pourcentage d'un acide faible est définie du point de vue de la composition d'un mélange en équilibre :  
 <img alt="Eq6" src="/files/ftp_upload/11395/11395eq6.png" style="text-align: center; height: 90px;" />
 où le numérateur est équivalent à la concentration de la base conjuguée de l'acide (par stœchiométrie, [A−] = [H3O+]). Contrairement à la valeur de Ka, l'ionisation en pourcentage d'un acide faible varie avec la concentration initiale de l'acide, diminuant généralement à mesure que la concentration augmente. 
 Tout comme pour les acides, la force relative d'une base se reflète dans la taille de sa constante d'ionisation de la base (Kb) dans les solutions aqueuses. Dans des solutions de même concentration, les bases plus fortes s'ionisent de façon plus importante et produisent donc des concentrations d'ions hydroxyde plus élevées que les bases plus faibles. Une base plus forte a une constante d'ionisation plus grande qu'une base plus faible. Pour la réaction d'une base, B :  
 <img alt="Eq7" src="/files/ftp_upload/11395/11395eq7.png" style="text-align: center; height: 50px;" />
 la constante d'ionisation est écrite comme  
 <img alt="Eq8" src="/files/ftp_upload/11395/11395eq8.png" style="text-align: center; height: 90px;" />
 L'inspection des données pour trois bases faibles présentées ci-dessous montre les augmentations de la force des bases dans l'ordre NO2− < CH2CO2− < NH3. 
 <img alt="Eq9-11" src="/files/ftp_upload/11395/11395eq9-11.png" style="text-align: center; height: 135px;" />
 Comme pour les acides, la force relative d'une base se reflète également dans son ionisation en pourcentage, calculée comme 
 <img alt="Eq12" src="/files/ftp_upload/11395/11395eq12.png" style="text-align: center; height: 90px;" />
 mais varie en fonction de la constante d'ionisation de la base et de la concentration initiale de la solution. 
 Ce texte est adapté de<a href="https://openstax.org/books/chemistry-2e/pages/14-3-relative-strengths-of-acids-and-bases"> Openstax, Chimie 2e, Section 14.3 : Forces relatives des acides et des bases. </a>

Forces des acides/bases et constantes de dissociation

La force relative d’un acide ou d’une base est la mesure dans laquelle il s’ionise lorsqu’il est dissous dans l’eau. Si la réaction d’ionisation est essentiellement complète, ...

Education

Enseignement

JoVE Core

Chemistry

Chimie

Acids and Bases

Acides et bases

KEY TERMS AND CONCEPTS

TERMES ET CONCEPTS CLÉS

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.

Acid strength can be measured with the acid-ionization constant, Ka. For an acid HA in water, Ka compares the concentrations of the products and the nonionized acid at equilibrium. Water is a reactant in the reaction, but it is not included in the equation because it is the solvent. A larger Ka means more H3O+ and A− relative to HA, so the acid is stronger.

A strong acid is considered completely ionized. In that case, the concentration of HA is zero, and Ka is immeasurably large, or approximately infinite. Weak acids ionize only partially, so their Ka values can be measured in the lab. The relative acid strengths in the examples increase in the order CH3CO2H &lt; HNO2 &lt; HSO4−.

Percent ionization is another way to describe weak acid strength. It is based on the amount of acid that ionizes at equilibrium. For a weak acid, the percent ionization changes with the starting concentration and usually gets smaller as the concentration gets higher. This makes percent ionization different from Ka.

Base strength is measured in a similar way with the base-ionization constant, Kb. For a base B in water, a larger Kb means the base ionizes more and produces a higher hydroxide ion concentration. A stronger base has a larger ionization constant than a weaker base.

The examples of weak bases show the strength order NO2− &lt; CH2CO2− &lt; NH3. Base strength can also be described with percent ionization. As with weak acids, this value depends on both the base-ionization constant and the initial concentration of the solution.

Acid and Base Strength in Water

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

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 acid and base strength in water depends on ionization, Ka, Kb, and percent ionization, with examples of strong and weak acids and bases.

Acid and Base Strength in Water | JoVE K12

chemistry

JoVE Core Chimie anime les concepts de chimie générale en utilisant des leçons vidéo concises et faciles à comprendre. De plus, nos vidéos de scientifiques à l'action présentent des expériences de recherche, classiques ou insolites, effectuées dans des laboratoires modernes du monde entier.

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.

acids-and-bases-percent-dissociation-and-ph

Acids and Bases: Percent Dissociation and pH

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 ...

phase-transitions-vaporization-and-condensation

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 ...

phase-transitions-sublimation-and-deposition

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

physical-and-chemical-properties-of-matter

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 ...

molecular-comparison-of-gases-liquids-and-solids

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 ...

comparing-intermolecular-forces-melting-point-boiling-point

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 ...

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 ...

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 ...

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.

Acid and Base Strength in Water

Description

Transcript

Tags

More videos by Standards