Name: organic molecules in everyday chemistry
Uploaded: 2020-09-03T13:38:26.000Z
Duration: 3 min 2 s
Channel: JoVE

K12 Standards

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NC K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.3.3

Organic Compounds

Composants chimiques composé principalement d'atomes de carbone lié à l'hydrogène, l'oxygène, l'azote ou atomes de soufre sont appelés composés organiques. Les composés organiques forment une grande variété de molécules-des éléments fondamentaux de la vie comme l'ADN ou les parois cellulaires des plantes aux matériaux libérateurs d'énergie comme les combustibles. Ils sont généralement facilement décomposés.Les atomes de carbone constituent l'épine dorsale de chaque composé organique, qui peut prendre diverses structures avec des arrangements en forme d'anneau, ramifiés et à chaîne droite en raison de la polyvalence du carbone pour former quatre liaisons, soit simples, doubles ou triples. Les composés organiques peuvent être des hydrocarbures ou des hydrocarbures fonctionnalisés. Les hydrocarbures sont constitués entièrement d'atomes de carbone et d'hydrogène.Les alcanes sont des hydrocarbures contenant des liaisons simples. Les alcènes contiennent une ou plusieurs liaisons doubles, tandis que les alcynes contiennent une ou plusieurs liaisons triples. La nomenclature des hydrocarbures suit un modèle où le nom de base est mentionné en premier en utilisant un préfixe déterminé par le nombre d'atomes de carbone.Le nom se termine par le suffixe ane, ene ou yne selon la présence de liaisons simples, doubles ou triples, respectivement. Par exemple, l'alcane contenant une seule liaison avec trois atomes de carbone est le propane. La double liaison contenant l'alcène avec trois carbones est le propène, tandis qu'une triple liaison contenant l'alcyne avec trois atomes de carbone est le propyne.Hydrocarbures avec un ou plusieurs de ses atomes d'hydrogène substitué par un groupe spécifique d'atomes ou de groupes fonctionnels sont appelés fonctionnalisés hydrocarbures. La formule générale des hydrocarbures fonctionnalisés désigne la partie hydrocarbonée par la lettre R et le groupe fonctionnel spécifique. Groupes fonctionnels peuvent être de plusieurs types et avoir des propriétés physiques et chimiques.Tous les composés organiques portant un groupe fonctionnel commun appartiennent à la même famille d'hydrocarbures, présentent des propriétés similaires et suivent une nomenclature similaire. Par exemple, tous les composés organiques portant un groupe fonctionnel OH sont appelés alcools. La nomenclature mentionne le nom de base parent-alcane se terminant par le suffixe ol, spécifique au groupe fonctionnel alcool.Par conséquent, le propane ayant un groupe fonctionnel OH est dénommé propanol. En revanche, tous les composés organiques portant des groupes fonctionnels carboxyle sont denommés acides carboxyliques. La nomenclature indique le nom de base parent-alcane se terminant par le suffixe acide oic, unique au groupe fonctionnel carboxyle.Par conséquent, le propane avec un groupe fonctionnel carboxyle est denommé acide propanoïque.

composés organiques

Toutes les choses vivantes sont formées principalement de composés de carbone appelés composés organiques. La catégorie des composés organiques comprend à la fois des composés naturels et synthétiques qui contiennent du carbone. Bien qu'une définition unique et précise n'ait pas encore été identifiée par la communauté des chimistes, la plupart d'entre eux conviennent que la présence du carbone comme élément principal, lié à l'hydrogène et à d'autres atomes de carbone, est un trait déterminant des molécules organiques. Toutefois, certains composés contenant du carbone, tels que les carbonates, les cyanures et les oxydes simples (CO et CO2), ne sont pas classés comme composés organiques.  
 
 Les composés organiques sont des composants clés des matières plastiques, savons, parfums, édulcorants, tissus, produits pharmaceutiques et beaucoup d'autres substances utilisées quotidiennement. Les composés organiques comprennent les composés provenant d'organismes vivants et ceux synthétisés par les chimistes. L'existence d'un large éventail de molécules organiques est une conséquence de la capacité des atomes de carbone à former jusqu'à quatre liaisons fortes avec d'autres atomes de carbone, ce qui se traduit par des chaînes et des cycles de différentes tailles, formes et complexités. 
 
 <h4>Hydrocarbures </h4>
 
 Les composés organiques les plus simples ne contiennent que les éléments carbone et hydrogène et sont appelés hydrocarbures. Les hydrocarbures peuvent différer selon les types de liaisons carbone-carbone présents dans leurs molécules. Ceux qui ne contiennent que des liaisons simples sont appelés alcanes, alors que ceux qui contiennent des liaisons doubles ou triples sont respectivement des alcènes et des alcynes. Bien que tous les hydrocarbures ne soient composés que de deux types d'atomes (carbone et hydrogène), il existe une grande variété d'hydrocarbures car ils peuvent être constitués de longueurs variables de chaînes, de chaînes ramifiées et de cycles d'atomes de carbone, ou de combinaisons de ces structures. 
 
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 <td style="color: black; border: 1px solid black; text-align: center;">Butane (C4H10) </td>
 <td style="color: black; border: 1px solid black; text-align: center;">Isobutane (C4H10) </td>
 <td style="color: black; border: 1px solid black; text-align: center;">Cyclobutane (C4H8) </td>
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 </table>
 
  
 
 Les hydrocarbures sont utilisés chaque jour, principalement comme combustibles, comme le gaz naturel, l'acétylène, le propane, le butane et les principaux composants de l'essence, du carburant diesel et du mazout de chauffage. Les alcanes, ou hydrocarbures saturés, ne contiennent qu'une seule liaison covalente entre leurs atomes de carbone. Les propriétés telles que le point de fusion et le point d'ébullition changent généralement de façon prévisible à mesure que le nombre d'atomes de carbone et d'hydrogène dans les molécules change.  
 
 Pour nommer un alcane simple, identifiez d'abord le nom de base en fonction du nombre d'atomes de carbone dans la chaîne (méth = 1, éth = 2, prop = 3, mais = 4, pent = 5, hex = 6, hept = 7, oct = 8, non = 9 et déc = 10). Le nom de base est suivi d'un suffixe — déterminé selon que l'hydrocarbure est un alcane (-ane ), un alcène (-ène ) ou un alcyne (-yne ). Par exemple, un alcane avec deux carbones est appelé éthane ; un alcane avec trois carbones est appelé propane ; et un alcane avec quatre carbones est appelé butane. Les chaînes plus longues sont nommées comme suit : pentane (chaîne à 5 carbones), hexane (6), heptane (7), octane (8), nonane (9), et décane (10).  
 
 Les alcènes et les alcynes sont des hydrocarbures insaturés contenant respectivement des liaisons doubles et des liaisons triples entre au moins deux atomes de carbone. Leur nomenclature suit les mêmes étapes que celle des alcanes : nom de base + suffixe. Par exemple, une chaîne d'alcènes avec deux carbones est appelée éthène, et un alcyne avec deux carbones est appelé éthyne ; un alcène avec trois carbones est appelé propène et un alcyne avec trois carbones est appelé propyne, et ainsi de suite.  
 
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 <td style="color: black; border: 1px solid black; text-align: center;">Éthane (C2H6) </td>
 <td style="color: black; border: 1px solid black; text-align: center;">Éthène (C2H4)  </td>
 <td style="color: black; border: 1px solid black; text-align: center;">Éthyne (C2H2) </td>
 </tr>
 </tbody>
 </table>
 
 <h4>Hydrocarbures fonctionnalisés </h4>
 
 L'incorporation d'un groupe fonctionnel dans des molécules contenant du carbone et de l'hydrogène conduit à de nouvelles familles de composés appelés hydrocarbures fonctionnalisés. Le groupe fonctionnel est un atome ou un groupe d'atomes caractéristique, qui détermine principalement les propriétés des dérivés d'hydrocarbures.  
 
 Un type de groupe fonctionnel est le groupe –OH. Les composés qui ont un groupe fonctionnel –OH sont des alcools. Le nom de l'alcool provient de l'hydrocarbure dont il est dérivé. Par convention, la partie hydrocarbonée de la molécule est désignée par 'R' ; ainsi, la formule générale d'un alcool est R–OH. Le dernier ‘ –e ’ du nom de l'hydrocarbure est remplacé par ‘ –ol ’. Dans le cas d'un alcool ramifié, l'atome de carbone auquel le groupe –OH est lié est indiqué par un nombre placé devant le nom. D'autres groupes fonctionnels courants sont répertoriés ci-dessous. Un groupe de composés comportant le même groupe fonctionnel forme une famille. 
 
 <table style="margin-left: auto; margin-right: auto;">
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 <td style="color: black; border: 1px solid black; text-align: center;">Famille </td>
 <td style="color: black; border: 1px solid black; text-align: center;">Groupe fonctionnel </td>
 <td style="color: black; border: 1px solid black; text-align: center;">Exemple </td>
 <td style="color: black; border: 1px solid black; text-align: center;">Formule </td>
 <td style="color: black; border: 1px solid black; text-align: center;">Nom </td>
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 <td style="color: black; border: 1px solid black; text-align: center;">Alcools </td>
 <td style="color: black; border: 1px solid black; text-align: center;"><img alt="Eq3" src="https://www.jovecore.com/CDNSource/lessons/1290/1290_Image 3.svg" style="height: 15px;" /></td>
 <td style="color: black; border: 1px solid black; text-align: center;"><img alt="Eq4" src="https://www.jovecore.com/CDNSource/lessons/1290/1290_Image 4.svg" style="height: 75px;" /></td>
 <td style="color: black; border: 1px solid black; text-align: center;">C3H8O</td>
 <td style="color: black; border: 1px solid black; text-align: center;">Propanol </td>
 </tr>
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 <td style="color: black; border: 1px solid black; text-align: center;">Éthers </td>
 <td style="color: black; border: 1px solid black; text-align: center;"><img alt="Eq5" src="https://www.jovecore.com/CDNSource/lessons/1290/1290_Image 5.svg" style="height: 15px;" /></td>
 <td style="color: black; border: 1px solid black; text-align: center;"><img alt="Eq6" src="https://www.jovecore.com/CDNSource/lessons/1290/1290_Image 6.svg" style="height: 75px;" /></td>
 <td style="color: black; border: 1px solid black; text-align: center;">C 2H6O</td>
 <td style="color: black; border: 1px solid black; text-align: center;">Éther diméthylique </td>
 </tr>
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 <td style="color: black; border: 1px solid black; text-align: center;">Aldéhydes </td>
 <td style="color: black; border: 1px solid black; text-align: center;"><img alt="Eq7" src="https://www.jovecore.com/CDNSource/lessons/1290/1290_image 7.svg" style="height: 45px;" /></td>
 <td style="color: black; border: 1px solid black; text-align: center;"><img alt="Eq8" src="https://www.jovecore.com/CDNSource/lessons/1290/1290_Image 8.svg" style="height: 75px;" /></td>
 <td style="color: black; border: 1px solid black; text-align: center;">C3H6O</td>
 <td style="color: black; border: 1px solid black; text-align: center;">Propanal </td>
 </tr>
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 <td style="color: black; border: 1px solid black; text-align: center;">Cétones </td>
 <td style="color: black; border: 1px solid black; text-align: center;"><img alt="Eq9" src="https://www.jovecore.com/CDNSource/lessons/1290/1290_Image 9.svg" style="height: 45px;" /></td>
 <td style="color: black; border: 1px solid black; text-align: center;"><img alt="Eq10" src="https://www.jovecore.com/CDNSource/lessons/1290/1290_Image 10.svg" style="height: 75px;" /></td>
 <td style="color: black; border: 1px solid black; text-align: center;">C3H6O</td>
 <td style="color: black; border: 1px solid black; text-align: center;">Propanone (acétone) </td>
 </tr>
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 <td style="color: black; border: 1px solid black; text-align: center;">Acides carboxyliques </td>
 <td style="color: black; border: 1px solid black; text-align: center;"><img alt="Eq11" src="https://www.jovecore.com/CDNSource/lessons/1290/1290_Image 11.svg" style="height: 45px;" /></td>
 <td style="color: black; border: 1px solid black; text-align: center;"><img alt="Eq12" src="https://www.jovecore.com/CDNSource/lessons/1290/1290_Image 12.svg" style="height: 75px;" /></td>
 <td style="color: black; border: 1px solid black; text-align: center;">C3H6O2</td>
 <td style="color: black; border: 1px solid black; text-align: center;">Acide propanoïque </td>
 </tr>
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 <td style="color: black; border: 1px solid black; text-align: center;">Esters </td>
 <td style="color: black; border: 1px solid black; text-align: center;"><img alt="Eq13" src="https://www.jovecore.com/CDNSource/lessons/1290/1290_Image 13.svg" style="height: 45px;" /></td>
 <td style="color: black; border: 1px solid black; text-align: center;"><img alt="Eq14" src="https://www.jovecore.com/CDNSource/lessons/1290/1290_Image 14.svg" style="height: 75px;" /></td>
 <td style="color: black; border: 1px solid black; text-align: center;">C4H8O2</td>
 <td style="color: black; border: 1px solid black; text-align: center;">Acétate d'éthyle </td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">Amines </td>
 <td style="color: black; border: 1px solid black; text-align: center;"><img alt="Eq15" src="https://www.jovecore.com/CDNSource/lessons/1290/1290_Image 15.svg" style="height: 17px;" /></td>
 <td style="color: black; border: 1px solid black; text-align: center;"><img alt="Eq16" src="https://www.jovecore.com/CDNSource/lessons/1290/1290_Image 16.svg" style="height: 75px;" /></td>
 <td style="color: black; border: 1px solid black; text-align: center;">C3H9N</td>
 <td style="color: black; border: 1px solid black; text-align: center;">Propylamine </td>
 </tr>
 </tbody>
 </table>
 
  
 
 Les éthers sont des composés qui contiennent le groupe fonctionnel –O–, avec la formule générale R–O–R’.  
 
 Une autre classe de molécules organiques contient un atome de carbone relié à un atome d'oxygène par une double liaison, communément appelé groupe carbonyle. Le carbone du groupe carbonyle peut se fixer à deux autres substituants conduisant à plusieurs sous-familles (aldéhydes, cétones, acides carboxyliques et esters).  
 
 Les groupes fonctionnels liés au groupe carbonyle comprennent le groupe –CHO d'un aldéhyde, le groupe –CO– d'une cétone, le groupe –CO2H d'un acide carboxylique et le groupe –CO2R d'un ester. Le groupe carbonyle, une double liaison carbone-oxygène, est la structure clé de ces classes de molécules organiques. Les aldéhydes contiennent au moins un atome d'hydrogène attaché à l'atome de carbone du carbonyle, les cétones contiennent deux groupes carbonés attachés à l'atome de carbone du carbonyle, les acides carboxyliques contiennent un groupe hydroxyle attaché à l'atome de carbone du carbonyle, et les esters contiennent un atome d'oxygène attaché à un autre groupe carboné relié à l'atome de carbone du carbonyle. Tous ces composés contiennent des atomes de carbone oxydés par rapport à l'atome de carbone d'un groupe alcool. 
 
 L'addition d'azote dans une structure organique conduit à deux familles de molécules, à savoir les amines et les amides. Les composés contenant un atome d'azote lié dans une structure hydrocarbonée sont classés en tant qu'amines. Les composés qui ont un atome d'azote lié à un côté d'un groupe carbonyle sont classés en tant qu'amides. Les amines sont un groupe fonctionnel de base. Les amines et les acides carboxyliques peuvent se combiner dans une réaction de condensation pour former des amides. 
 
 Ce texte est adapté de <a href="https://openstax.org/books/chemistry-2e/pages/20-introduction">Openstax, Chimie 2e, Section 20: Introduction, Openstax, Chimie 2e, Section 20.1 : Hydrocarbures, Openstax, chimie 2e, section 20.2 : Alcools et éthers, Openstax, chimie 2e, section 20.2 : Aldéhydes, cétones, Acides carboxyliques, et esters,</a> et <a href="https://openstax.org/books/chemistry-2e/pages/20-4-amines-and-amides">Openstax, Chimie 2e, Section 20.2 : Amines et amides</a>.

Composés organiques

Tous les êtres vivants sont formés principalement de composés carbonés appelés composés organiques. La catégorie des composés organiques comprend à la fois les composés naturels et synthétiques ...

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Molécules, composés et équations chimiques

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TERMES ET CONCEPTS CLÉS

organic molecules in everyday chemistry

Organic molecules are carbon-based compounds found in living things and in many everyday products. Most organic compounds have carbon as the main element, bonded to hydrogen and other carbon atoms. Some carbon-containing substances, such as carbonates, cyanides, and simple oxides like CO and CO2, are not classified as organic.

Carbon can form up to four strong bonds, which helps explain why organic compounds can make chains and rings of many sizes and shapes. These molecules appear in plastics, soaps, perfumes, sweeteners, fabrics, pharmaceuticals, and many other materials used daily. Organic compounds may come from living organisms, or they may be made by chemists.

The simplest organic compounds are hydrocarbons, which contain only carbon and hydrogen. Hydrocarbons can have only single bonds, only double bonds, or only triple bonds. Those with single bonds are called alkanes, while those with double or triple bonds are called alkenes and alkynes.

Hydrocarbons vary because their carbon atoms can form straight chains, branched chains, rings, or combinations of these structures. Examples include butane, isobutane, and cyclobutane. Hydrocarbons are widely used as fuels, including natural gas, acetylene, propane, butane, and the main components of gasoline, diesel fuel, and heating oil.

Alkanes are saturated hydrocarbons because they contain only single covalent bonds between carbon atoms. Their melting point and boiling point usually change in a regular way as the number of carbon and hydrogen atoms changes. Simple alkane names use a prefix based on the number of carbon atoms, such as meth, eth, prop, but, pent, hex, hept, oct, non, and dec, followed by the ending -ane.

This naming pattern also helps identify alkenes and alkynes. The suffix changes to -ene for alkenes and -yne for alkynes. A two-carbon alkane is ethane, a three-carbon alkane is propane, and a four-carbon alkane is butane. The matching alkene and alkyne names are ethene and ethyne, then propene and propyne.

Adding a functional group to a hydrocarbon creates a functionalized hydrocarbon. A functional group is a specific atom or group of atoms that largely controls the properties of the compound. One common example is the -OH group, which makes a molecule an alcohol. Alcohol names come from the hydrocarbon name, with the final -e changed to -ol, and a branched alcohol may need a number to show where the -OH group is attached.

Other families of functionalized hydrocarbons include ethers, aldehydes, ketones, carboxylic acids, esters, amines, and amides. Ethers contain an -O- group and have the general formula R-O-R'. Carbonyl compounds contain a carbon-oxygen double bond. In aldehydes, the carbonyl carbon has at least one hydrogen attached. In ketones, it has two carbon groups attached. In carboxylic acids, a hydroxyl group is attached to the carbonyl carbon. In esters, an oxygen atom is attached to another carbon group connected to the carbonyl carbon.

These carbonyl families all have carbon atoms that are more oxidized than the carbon atom in an alcohol group. Nitrogen can also be part of organic molecules. Compounds with nitrogen in a hydrocarbon framework are called amines, and compounds with nitrogen on one side of a carbonyl group are called amides. Amines are basic, and amines can react with carboxylic acids in a condensation reaction to form amides.

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Organic molecules are carbon-based compounds found in living things and in many everyday products. Most organic compounds have carbon as the main element, bonded to hydrogen and other carbon atoms. Some carbon-containing substances, such as carbonates, cyanides, and simple oxides like CO and CO2, are not classified as organic. Carbon can form up to four strong bonds, which helps explain why organic compounds can make chains and rings of many sizes and shapes. These molecules appear in...

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Chemical formula mass and percent composition help describe the makeup of compounds. A chemical formula shows which atoms are present and how many of each atom appear in a substance. For covalent compounds, the formula shows the atoms in one molecule. That is why formula mass can also be called molecular mass. Chloroform, CHCl3, is one example. Its formula shows one carbon atom, one hydrogen atom, and three chlorine atoms. The molecular mass is the sum of their average atomic masses. Ionic...

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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 ...

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, ...

surface-tension-capillary-action-and-viscosity

Surface Tension, Capillary Action, and Viscosity

Surface Tension
The various IMFs between identical molecules of a substance are examples of cohesive forces. The molecules within a liquid are surrounded ...

Hydrogen Bonds

Hydrogen BondsHydrogen bonds are weak attractions between atoms that have formed other chemical bonds. One of these atoms is electronegative, like oxygen, ...

Van der Waals Interactions

Atoms and molecules interact with each other through intermolecular forces. These electrostatic forces arise from attractive or repulsive interactions ...

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

PS.Chm.3.2

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 ...

Chemical Formulas

A chemical formula presents information about the proportions of atoms constituting a particular chemical compound or molecule, mainly using symbols of ...

Molecular Models

Physical models representing molecular architectures of chemical compounds play essential roles in understanding chemistry. The use of molecular models ...

Classification of Elements and Compounds

Pure substances consist of only one type of matter. A pure substance can be an element or a compound. An element consists of only one type of atom, while ...

ionic-compounds-formulas-and-nomenclature

Ionic Compounds: Formulas and Nomenclature

An element composed of atoms that readily lose electrons (a metal) can react with an element composed of atoms that readily gain electrons (a nonmetal) to ...

molecular-compounds-formulas-and-nomenclature

Molecular Compounds: Formulas and Nomenclature

Molecular compounds or covalent compounds result when atoms share electrons to form covalent bonds. Since there is no electron transfer, molecular ...

Use models to predict chemical names and formulas including ionic (binary & ternary), acidic, and binary covalent compounds.

Analyze the structure of atoms and isotopes.

Organic Molecules in Everyday Chemistry

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