Name: catalyst action in reaction rates
Uploaded: 2020-09-24T15:06:50.000Z
Duration: 2 min 50 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.5.1

Catalysis

L'étude des mécanismes de réaction et de la cinétique aide les chercheurs à optimiser la vitesse d'une réaction. Une augmentation de la température ou de la concentration accélérera le rythme mais peut aussi conduire à la décomposition ou aux produits secondaires lorsqu'il est trop augmenté. Alternativement, un produit chimique qui accélère la vitesse de réaction sans être altéré ou consommé en permanence peuvent être ajoutés au mélange réactionnel.Ces substances sont appelées catalyseurs et affectent la constante de vitesse en modifiant l'énergie d'activation. Rappelez-vous que plus l'énergie d'activation est élevée, plus la vitesse de réaction est lente. Par conséquent, de nombreuses réactions chimiques, comme la décomposition de peroxyde d'hydrogène aqueux, progressent lentement.L'ajout d'un catalyseur réduit l'énergie d'activation en fournissant un mécanisme de réaction alternatif, sans affecter les états énergétiques des réactifs et produits. Il existe deux types de catalyseurs homogènes et hétérogène. Un catalyseur homogène existe dans la même phase comme réactifs.Par exemple, du bromure de sodium est ajouté à l'hydrogène aqueux peroxyde pour accélérer sa décomposition en oxygène gazeux et en eau. Premièrement, les ions de bromure réagissent avec le peroxyde d'hydrogène en milieu acide pour former une solution orange de brome aqueux et d'eau. Ensuite, le brome aqueux et le peroxyde d'hydrogène réagissent et libérent les ions de bromure, indiqués par une solution incolore.Caractéristique d'un catalyseur, les ions de bromure accélèrent la réaction mais restent non consommés et n'apparaissent pas dans l'équation nette équilibrée. Un catalyseur hétérogène existe dans un état physique différent par rapport aux réactifs. La catalyse hétérogène est caractérisée par quatre étapes sous-jacentes adsorption, diffusion, réaction, et la désorption.Par exemple, la réaction d'hydrogénation de gaz éthène insaturé en éthane est accélérée par du palladium finement dispersé sur charbon de bois. Ici, le catalyseur existe à l'état solide, tandis que les réactifs sont sous leurs formes gazeuses. Au cours de cette catalyse hétérogène, les molécules d'éthène et d'hydrogène s'adsorbent à la surface du catalyseur.La liaison hydrogène-hydrogène se rompt permettant aux atomes d'hydrogène de se diffuser sur la surface du catalyseur. Lorsque des atomes d'hydrogène en diffusion d'hydrogène rencontrent des molécules d'éthylène absorbées, ils réagissent pour former de l'éthane saturé. Ensuite, les produits se désorbent et s'éloignent de la surface métallique, derrière eux le catalyseur intact.

catalyse

La présence d'un catalyseur influence la vitesse d'une réaction chimique. Un catalyseur est une substance qui peut augmenter la vitesse de réaction sans être consommée pendant le processus. Une compréhension de base du rôle des catalyseurs lors des réactions chimiques peut être interprétée à partir du concept des mécanismes de réaction et des profils énergétiques. 
 <img alt="Image1" src="/files/ftp_upload/11383/11383_Image_1.png" style="text-align: center; height: 350px;" />
 L'image illustrée représente les profils de réaction pour un processus chimique endothermique qui progresse en l'absence (courbe rouge) et en présence (courbe bleue) d'un catalyseur. 
 Les deux courbes représentent la même réaction globale : elles commencent et se terminent aux mêmes énergies (dans ce cas, les produits ont plus d'énergie que les réactifs ; par conséquent, la réaction est endothermique). Toutefois, leurs mécanismes de réaction sont différents. La réaction non catalysée se déroule via un mécanisme en une étape (avec un seul état de transition observé). En revanche, la réaction catalysée suit un mécanisme en deux étapes (deux états de transition sont observés) avec nettement moins d'énergie d'activation. Cette différence entre les chemins de réaction illustre le rôle du catalyseur en fournissant un autre mécanisme de réaction possible avec une énergie d'activation plus basse, accélérant ainsi les réactions. 
 Le mécanisme de réaction catalysée n'a pas besoin d'impliquer un nombre plus élevé d'étapes élémentaires que le mécanisme non catalysé. Cependant, il doit fournir un chemin de réaction alternatif dont l'étape déterminante de la vitesse est plus rapide (avec un Ea, ou une énergie d'activation, plus faible). 
 Une réaction catalytique peut être classée comme étant homogène ou hétérogène, en fonction des états physiques dans lesquels existent les catalyseurs et les réactifs au cours du processus catalytique. 
 Catalyse homogène 
 Dans une catalyse homogène, le catalyseur est présent dans la même phase que les réactifs – solide, liquide ou gaz. Au cours du processus, le catalyseur interagit avec le réactif pour former une substance intermédiaire, qui se décompose ou réagit avec un autre réactif en une ou plusieurs étapes pour régénérer le catalyseur d'origine et former le produit final. 
 Un exemple de catalyse homogène est le processus chimique impliquant la décomposition de l’ozone dans la haute atmosphère terrestre. L'ozone est une molécule relativement instable qui se décompose pour produire de l'oxygène diatomique. Cette réaction de décomposition est cohérente avec le mécanisme suivant en deux étapes : 
 <img alt="Eq1" src="/files/ftp_upload/11383/11383_Equation_1.png" style="text-align: center; height: 75px;" />
 De nombreuses substances peuvent catalyser la décomposition de l'ozone. Par exemple, on croit que la décomposition de l'ozone catalysée par l'oxyde nitrique se produit par le biais du mécanisme en trois étapes suivant : 
 <img alt="Eq2" src="/files/ftp_upload/11383/11383_Equation_2.png" style="text-align: center; height: 115px;" />
 Cependant, la réaction globale est la même pour le mécanisme non catalysé en deux étapes et pour le mécanisme catalysé par NO en trois étapes : 
 <img alt="Eq3" src="/files/ftp_upload/11383/11383_Equation_3.png" style="text-align: center; height: 50px;" />
 Dans la réaction catalysée, notez que NO est un réactif dans la première étape du mécanisme et un produit dans la dernière étape. C'est un autre trait caractéristique d'un catalyseur : bien qu'il participe à la réaction chimique, il n'est pas consommé par la réaction. De plus, dans cette catalyse homogène, le réactif et le catalyseur existent en phase gazeuse. 
 Catalyse hétérogène 
 Dans une catalyse hétérogène, le catalyseur est présent dans une phase différente (généralement un solide) que les réactifs. Ces catalyseurs fonctionnent généralement en fournissant une surface active sur laquelle une réaction peut se produire. Les réactions en phase gazeuse et liquide catalysées par des catalyseurs hétérogènes se produisent à la surface du catalyseur plutôt qu'à l'intérieur de la phase gazeuse ou liquide. 
 La catalyse hétérogène implique généralement les processus suivants : 
 <ol>
 <li>L'adsorption du ou des réactifs sur la surface du catalyseur </li>
 <li>L'activation du ou des réactifs adsorbés </li>
 <li>La réaction du ou des réactifs adsorbés </li>
 <li>La désorption du ou des produits de la surface du catalyseur </li>
 </ol>
 <img alt="Image2" src="/files/ftp_upload/11383/11383_Image_2.png" style="text-align: center; height: 250px;" />
 L'image illustrée représente le mécanisme réactionnel impliquant la catalyse hétérogène de l'éthylène et de l'hydrogène gazeux sur une surface solide de nickel, formant de l'éthane gazeux (C2H4 + H2 ⟶ C2H6) : 
 (a) L'hydrogène est adsorbé sur la surface du nickel. Au cours du processus, des liaisons hydrogène-hydrogène sont rompues pour former des liaisons nickel-hydrogène. 
 (b) L'éthylène s'adsorbe également sur la surface du nickel en rompant la liaison-pi carbone-carbone et en formant des liaisons nickel–carbone. 
 (c) Les atomes d'hydrogène se diffusent à travers la surface et forment de nouvelles liaisons carbone-hydrogène lorsqu'ils entrent en collision pour former de l'éthane (C2H6). 
 (d) Les molécules d'éthane se détachent de la surface du nickel. 
 La catalyse hétérogène est utilisée pour fabriquer industriellement des produits chimiques tels que l'ammoniac, l'acide nitrique, l'acide sulfurique et le méthanol. Des catalyseurs hétérogènes sont également utilisés dans les pots catalytiques de la plupart des automobiles à essence. 
 Ce texte est adapté de<a href="https://openstax.org/books/chemistry-2e/pages/12-7-catalysis"> Openstax, Chimie 2e, Section 12.7 : Catalyse</a>.

Catalyse

La présence d’un catalyseur affecte la vitesse d’une réaction chimique. Un catalyseur est une substance qui peut augmenter la vitesse de réaction sans être consommée...

Education

Enseignement

JoVE Core

Chimie

Chemical Kinetics

Cinétique chimique

KEY TERMS AND CONCEPTS

TERMES ET CONCEPTS CLÉS

catalyst action in reaction rates

Catalysts change the rate of a chemical reaction by giving it a faster path. A catalyst increases reaction rate without being consumed during the process. Its effect is often explained with reaction mechanisms and energy diagrams.

For an endothermic reaction, the reactants and products start and end at the same energies in both cases. The uncatalyzed path is a one-step mechanism with one transition state. The catalyzed path follows a different mechanism with two transition states and a lower activation energy, or Ea. The lower rate-determining barrier is what makes the reaction faster.

Catalytic reactions are often grouped as homogeneous or heterogeneous. In homogeneous catalysis, the catalyst and reactants are in the same phase, which may be solid, liquid, or gas. The catalyst reacts with the reactant to form an intermediate, and that intermediate then breaks down or reacts again to form the product and regenerate the catalyst.

A good example of homogeneous catalysis is ozone decomposition in the upper atmosphere. Ozone breaks down to form diatomic oxygen, and nitric oxide can catalyze that process through a three-step mechanism. In this reaction, NO appears as a reactant in the first step and a product in the last step, which shows that it participates in the reaction but is not used up. Here, both the reactant and the catalyst are gases.

In heterogeneous catalysis, the catalyst is in a different phase from the reactants, usually a solid. These reactions happen on the catalyst surface. They typically include adsorption of reactants, activation on the surface, reaction of the adsorbed molecules, and desorption of the products.

The nickel-catalyzed reaction of ethene and hydrogen to form ethane shows this surface process. Hydrogen first adsorbs on nickel, and the H-H bond breaks to form nickel-hydrogen bonds. Ethene also adsorbs as its carbon-carbon pi bond breaks and nickel-carbon bonds form. Hydrogen atoms then move across the surface and make new carbon-hydrogen bonds, and the ethane product desorbs from the nickel surface.

Heterogeneous catalysts are important in industry. They help make ammonia, nitric acid, sulfuric acid, and methanol. They are also used in catalytic converters in most gasoline-powered cars.

Catalyst Action in Reaction Rates

reaction rate

Measuring Reaction Rates

Measuring reaction rates shows how fast reactants are used up or products are formed over time. The rate of reaction is the change in the amount of a reactant or product per unit time. Because of that, scientists measure how a property changes as the reaction proceeds and connect that change to reactant or product amounts. For reactions that make or use a gas, the rate can be followed by changes in volume or pressure. A rate expression is the mathematical way to write how concentration changes...

measuring reaction rates

Tracking Reaction Kinetics with Light and Pressure

Reaction kinetics can be tracked with polarimetry, spectrometry, and pressure measurements. These methods let scientists follow a reaction without disturbing the sample. They also help determine how reactant or product concentrations change over time. Polarimetry is used for optically active substances. These substances rotate the plane of polarized light, which is called optical rotation. The effect comes from molecular structure. Normal monochromatic light is unpolarized, but after it passes...

concentration and rate law

Reaction Order from Concentration

Reaction order from concentration shows how reactant amounts affect reaction rate. Rate laws, also called differential rate laws or rate equations, are mathematical expressions that connect reaction rate with the concentrations of reactants. For a generic reaction a A + b B → products, the rate law can be written using the reactant concentrations [A] and [B] and a rate constant k. In a rate law, k is the rate constant for one specific reaction at one specific temperature. The exponents m and n...

determining order of reaction

Finding Rate Law from Initial Rates

Rate laws connect the speed of a chemical reaction to the concentration of its reactants. The rate constant, k, and the reaction orders are not taken from the chemical equation. They are found experimentally by watching how the rate changes when the reactant concentrations change. One common way to do this is the method of initial rates. In this method, several trials are run with different starting concentrations. The measured rates are then compared to determine the reaction orders and,...

the integrated rate law: the dependence of concentration on time

the-integrated-rate-law-the-dependence-of-concentration-on-time

Reading Reaction Progress with Integrated Laws

Integrated rate laws connect reaction concentration to time. They help show how much reactant or product is present after a certain period. They can also help estimate how long a reaction must run to reach a given extent. A common use is finding how long radioactive material must be stored before its radioactivity drops to a safe level. These equations come from the differential rate law after it is integrated with respect to time. For a first-order reaction, where rate = k[A], the integrated...

half-life of a reaction

Reaction Half-Life in Kinetics

Reaction half-life is the time needed for half of a reactant to be consumed. After each half-life, half of the remaining reactant is used up. A hydrogen peroxide decomposition example shows this pattern clearly. The concentration drops from 1.000 M to 0.500 M in the first 6.00 hours, then to 0.250 M in the next 6.00 hours, and then to 0.125 M in the third period. Each later 6.00-hour interval removes half of what is left. For first-order reactions, the half-life does not depend on the reactant...

temperature dependence on reaction rate

Collision Theory and Reaction Speed

Collision theory explains why reaction speed depends on how particles collide. Atoms, molecules, or ions must come close together before they can react. The theory says the reaction rate depends on the collision rate, the orientation of the colliding species, and whether the collision has enough energy for bonds to change. A gas-phase reaction between carbon monoxide and oxygen shows why orientation matters. The molecules can collide in more than one way. If the oxygen side of carbon monoxide...

arrhenius plots

Determining Activation Energy from Temperature

The Arrhenius equation links activation energy and the rate constant, k, for chemical reactions. It is written as k = Ae−Ea/RT. In this equation, R is the ideal gas constant with a value of 8.314 J/mol·K, T is the temperature on the kelvin scale, Ea is the activation energy in J/mole, e is the constant 2.7183, and A is the frequency factor. The frequency factor depends on collision frequency and the orientation of reacting molecules. Experimental kinetic data can be used to find the activation...

reaction mechanisms

Elementary Steps in Reaction Mechanisms

Chemical reactions can happen in steps, and a balanced equation does not show the full path at the molecular level. A reaction mechanism, also called a reaction path, gives the step-by-step process that explains how reactants become products. The decomposition of ozone is one example of a reaction that can be described by a sequence of steps. Each step in a mechanism is an elementary reaction. These elementary reactions happen in order, and when they are added together, they give the balanced...

rate-determining steps

Reaction Bottlenecks in Chemical Kinetics

Reaction bottlenecks help explain rate-determining steps in multistep reaction mechanisms. In a mechanism with several elementary steps, one step is often much slower than the others. That slowest step is called the rate-limiting step, or rate-determining step. A reaction cannot move faster than its slowest step, so this step controls the overall reaction rate. The idea is like traffic on a four-lane freeway with one lane closed. Cars can only move as fast as the bottleneck allows. In the same...

catalysis

Catalysts change the rate of a chemical reaction by giving it a faster path. A catalyst increases reaction rate without being consumed during the process. Its effect is often explained with reaction mechanisms and energy diagrams. For an endothermic reaction, the reactants and products start and end at the same energies in both cases. The uncatalyzed path is a one-step mechanism with one transition state. The catalyzed path follows a different mechanism with two transition states and a lower...

enzymes

Enzyme Action and Inhibition

Enzymes are biological catalysts that speed up many reactions in living organisms. They help control cellular metabolism by lowering the activation energy needed for biochemical reactions. When activation energy drops, reaction rates can increase. Enzyme problems can also lead to serious disease. A genetic abnormality that causes G6PD, or glucose-6-phosphate dehydrogenase, deficiency can disrupt the pathway that supplies NADPH to cells. In red blood cells, this can reduce glutathione and...

key terms and concepts

Explore how catalysts speed up reactions by lowering activation energy, with clear examples of homogeneous and heterogeneous catalysis for high school chemistry.

Catalyst Action in Reaction Rates | 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.

Pennsylvania State Academic Standards

Physical Science

Chemical Reactions

3.2.9-12.D

3.2.9-12.E

ohios-learning-standards-and-model-curriculum

Ohio’s Learning Standards and Model Curriculum

Interactions Of Matter

Chemical reactions

Virginia  Standards of Learning

HIgh School

CH.7

CH.7.f

Arizona Science Standards

High School

HS.P1

HS.P1U1.3

Next Generation Science Standards

Matter and Its Interactions

HS-PS1-4

HS-PS1-5

Florida Department of Education

SC.912.P.12

SC.912.P.12.12

new-york-state-science-learning-standards

New York State Science Learning Standards

HS. Chemical Reactions

HS-PS1-5.

Georgia Standards of Excellence

SC4.

Catalysts in Chemical Reactions

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:


	...

Bond Energies and Bond Lengths

Stable molecules exist because covalent bonds hold the atoms together. The strength of a covalent bond is measured by the energy required to break it, ...

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

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 ...

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

PS.Chm.3.2

Analyze the structure of atoms and isotopes.

Catalyst Action in Reaction Rates

Description

Transcript

Tags

More videos by Standards