Name: carbon compounds in everyday life
Uploaded: 2023-04-30T18:28:31.000Z
Duration: 2 min 17 s
Channel: JoVE

K12 Standards

Minnesota Academic Standards in Science

9-12

Chemistry

3.2.2 9C.3.2.1.1

What is Organic Chemistry?

Organische Chemie ist die Lehre von chemischen Verbindungen, die hauptsächlich aus Kohlenstoffatomen bestehen, die an Wasserstoff-, Sauerstoff-, Stickstoff- oder Schwefelatome gebunden sind.
Organische Verbindungen bilden eine Vielzahl von Molekülen – von grundlegenden Bausteinen des Lebens wie DNA oder pflanzlichen Zellwänden bis hin zu energiefreisetzenden Materialien wie Kraftstoffen. Sie lassen sich in der Regel leicht abbauen.
Kohlenstoffatome bilden das Rückgrat jeder organischen Verbindung, die aufgrund der Vielseitigkeit von Kohlenstoff bei der Bildung von vier Bindungen als Einfach-, Doppel- oder Dreifachbindung unterschiedliche Strukturen mit ringförmigen, verzweigten und geradkettigen Anordnungen annehmen kann. 
Organische Verbindungen können entweder Kohlenwasserstoffe oder funktionalisierte Kohlenwasserstoffe sein.
Kohlenwasserstoffe bestehen ausschließlich aus Kohlenstoff- und Wasserstoffatomen. Alkane sind Kohlenwasserstoffe, die Einfachbindungen enthalten. Alkene enthalten eine oder mehrere Doppelbindungen, während Alkine eine oder mehrere Dreifachbindungen enthalten.
Kohlenwasserstoffe, bei denen eines oder mehrere ihrer Wasserstoffatome durch eine bestimmte Gruppe von Atomen oder funktionellen Gruppen substituiert sind, werden als "funktionalisierte Kohlenwasserstoffe" bezeichnet. Die allgemeine Formel für funktionalisierte Kohlenwasserstoffe bezeichnet den Kohlenwasserstoffanteil mit dem Buchstaben "R", gefolgt von der spezifischen funktionellen Gruppe.
Funktionelle Gruppen können von vielen Arten sein und spezifische physikalische und chemische Eigenschaften haben. Alle organischen Verbindungen, die eine gemeinsame funktionelle Gruppe tragen, fallen in die gleiche Familie der Kohlenwasserstoffe, weisen ähnliche Eigenschaften auf und folgen einer ähnlichen Nomenklatur.
Zum Beispiel werden alle organischen Verbindungen, deren Kohlenstoffatom eine -OH-funktionelle Gruppe trägt, als Alkohole bezeichnet. Im Gegensatz dazu werden alle organischen Verbindungen, die funktionelle Carboxylgruppen tragen, als Carbonsäuren bezeichnet.
Insgesamt ist das Verständnis der Struktur, der Bindung und der Reaktionen organischer Verbindungen, sowohl natürlicher als auch künstlicher Verbindungen, der Schlüssel zum Verständnis ihrer Funktionen im wirklichen Leben.

Dieser Text wurde von <a href="https://openstax.org/books/chemistry-2e/pages/20-introduction">Openstax, Chemie 2e, Abschnitt 20 übernommen</a>.

was ist organische chemie?

Die organische Chemie ist die Lehre von den Verbindungen des Kohlenstoffs, den so genannten organischen Verbindungen. Organische Verbindungen stammen entweder von lebenden Organismen oder werden von Chemikern synthetisiert. Ein charakteristisches Merkmal dieser Verbindungen ist das Vorhandensein von Kohlenstoff als Hauptelement, das an andere Kohlenstoffatome und andere Elemente wie Wasserstoff, Sauerstoff, Stickstoff und Schwefel gebunden ist. Die Existenz einer breiten Palette organischer Moleküle ist eine Folge der Fähigkeit von Kohlenstoffatomen, bis zu vier starke Bindungen mit anderen Kohlenstoffatomen einzugehen, was zu Ketten und Ringen unterschiedlicher Größe, Form und Komplexität führt. Einige kohlenstoffhaltige Verbindungen wie Carbonate, Cyanide und einfache Oxide (CO und CO_2) werden jedoch normalerweise nicht als organische Verbindungen klassifiziert.

Die einfachsten organischen Verbindungen enthalten nur die Elemente Kohlenstoff und Wasserstoff und werden Kohlenwasserstoffe genannt. Kohlenwasserstoffe können sich durch die Art der Kohlenstoff-Kohlenstoff-Bindungen in ihren Molekülen unterscheiden. Dies können Alkane (die nur Einfachbindungen enthalten), Alkene (die eine oder mehrere Doppelbindungen enthalten) oder Alkine (die eine oder mehrere Dreifachbindungen enthalten) sein. Obwohl alle Kohlenwasserstoffe nur aus zwei Arten von Atomen (Kohlenstoff und Wasserstoff) bestehen, gibt es aufgrund der unterschiedlichen Längen der Ketten, verzweigten Ketten und Ringe von Kohlenstoffatomen oder aufgrund von Kombinationen dieser Strukturen eine große Vielfalt an Kohlenwasserstoffen. Eigenschaften wie der Schmelzpunkt und der Siedepunkt ändern sich normalerweise vorhersehbar, wenn sich die Anzahl der Kohlenstoff- und Wasserstoffatome in den Molekülen ändert.

Der Einbau einer funktionellen Gruppe in kohlenstoff- und wasserstoffhaltige Moleküle führt zu neuen Verbindungsfamilien, den sogenannten funktionalisierten Kohlenwasserstoffen. Die funktionelle Gruppe ist ein charakteristisches Atom oder eine Gruppe von Atomen, die in erster Linie die Eigenschaften von Kohlenwasserstoffderivaten bestimmt. Verbindungen, bei denen eine funktionelle Gruppe -OH an den Kohlenwasserstoffteil gebunden ist, sind zum Beispiel Alkohole. Die allgemeine Formel eines Alkohols lautet R-OH, wobei R der Kohlenwasserstoffanteil des Moleküls ist. Eine Gruppe von Verbindungen mit derselben funktionellen Gruppe bildet eine Familie.

Organische Verbindungen sind Hauptbestandteile von Kunststoffen, Seifen, Parfüms, Süßungsmitteln, Stoffen, Arzneimitteln und vielen anderen Substanzen, die täglich verwendet werden. Daher ist die Untersuchung ihrer Strukturen und Reaktionen von entscheidender Bedeutung, um ihre Funktionen im wirklichen Leben zu verstehen.

Was ist organische Chemie?

Organische Chemie ist die Lehre von Kohlenstoffverbindungen, die als organische Verbindungen bezeichnet werden. Organische Verbindungen stammen entweder aus lebenden Organismen oder sind ...

Education

Lehre

JoVE Core

Organic Chemistry

Organische Chemie

Unit 1

Einheit 1

Covalent Bonding and Structure

Kovalente Bindung und Struktur

KEY TERMS AND CONCEPTS

KERNBEGRIFFE UND KONZEPTE

carbon compounds in everyday life

Organic chemistry focuses on carbon compounds called organic compounds. These compounds may come from living things or be made by chemists. Carbon is the main element in them, and it bonds with other carbon atoms as well as hydrogen, oxygen, nitrogen, and sulfur.

Carbon can form up to four strong bonds. That ability lets carbon atoms build chains and rings of many sizes, shapes, and levels of complexity. Not every carbon-containing substance is classified as organic. Carbonates, cyanides, and simple oxides such as CO and CO2 are usually excluded.

The simplest organic compounds are hydrocarbons. Hydrocarbons contain only carbon and hydrogen. They can be alkanes with single bonds, alkenes with one or more double bonds, or alkynes with one or more triple bonds.

Hydrocarbons can vary a lot even though they use only two kinds of atoms. Their carbon atoms may form straight chains, branched chains, rings, or combinations of these structures. As the number of carbon and hydrogen atoms changes, properties such as melting point and boiling point usually change in a predictable way.

Adding a functional group creates a new family of compounds called functionalized hydrocarbons. A functional group is a specific atom or group of atoms that mostly controls the properties of the molecule. For example, compounds with an –OH group attached to the hydrocarbon part are alcohols. By convention, alcohols have the general formula R–OH, where R is the hydrocarbon portion.

Compounds with the same functional group belong to the same family. Organic compounds are important in plastics, soaps, perfumes, sweeteners, fabrics, pharmaceuticals, and many other everyday products. Learning their structures and reactions helps explain how these materials work in real life.

Carbon Compounds in Everyday Life

what is organic chemistry?

Organic chemistry focuses on carbon compounds called organic compounds. These compounds may come from living things or be made by chemists. Carbon is the main element in them, and it bonds with other carbon atoms as well as hydrogen, oxygen, nitrogen, and sulfur. Carbon can form up to four strong bonds. That ability lets carbon atoms build chains and rings of many sizes, shapes, and levels of complexity. Not every carbon-containing substance is classified as organic. Carbonates, cyanides, and...

electronic structure of atoms

Atomic Orbitals and Quantum Numbers

Atomic orbitals and quantum numbers describe how electrons are arranged around the nucleus. An atom has a small, positively charged nucleus with electrons surrounding it. The nucleus contains protons and neutrons, and the quantum mechanical model gives a better picture of this structure than older models. Protons carry a +1 charge and have a mass of 1.0073 amu. Neutrons have no charge and have a mass of 1.0087 amu. Electrons carry a −1 charge and have a mass of 0.00055 amu. The number of...

electron configurations

How Electrons Fill Atomic Orbitals

Electron filling in atoms follows a set order based on orbital energy. The Aufbau principle says each new electron enters the lowest-energy subshell available. The Pauli exclusion principle says no two electrons can share the same set of four quantum numbers. Hund’s rule of maximum multiplicity says electrons stay unpaired in equal-energy orbitals when possible. The order of filling follows the relative energies of the subshells. A common sequence is 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, and so on.

chemical bonds

Chemical Bonds: Types and Strength

Chemical bonds help atoms reach a full valence shell like the nearest noble gas. The main bond types are ionic, covalent, and metallic. Bond energy and bond length also help explain how strong a bond is. An ionic bond forms from electrostatic attraction between cations and anions. In many cases, one atom transfers electrons to another atom, and the ions form from that transfer. Ionic bonds have no defined direction because the attraction spreads evenly through three-dimensional space. A...

polar covalent bonds

Electronegativity in Polar Covalent Bonds

Polar covalent bonds form when atoms share electrons unevenly. This happens in covalent bonds between atoms that have similar, but not identical, tendencies to attract electrons. Nonmetal atoms often make these bonds with other nonmetals. Hydrogen gas, H2, is a simple example of a covalent bond between two hydrogen atoms. A covalent bond begins when two atoms move close enough for their valence orbitals to overlap. In hydrogen, the 1s orbitals overlap and the single electrons on each atom...

lewis structures and formal charges

Lewis Structures, Bonds, and Formal Charge

Lewis structures show how atoms share electrons in covalent bonds and in polyatomic ions. Lewis symbols help draw these structures, and the periodic table helps predict how many valence electrons an atom has and how many bonds it can form to reach an octet. Group 18 elements, such as argon and helium, already have filled electron configurations. They rarely take part in chemical bonding. Atoms in group 17, such as bromine and iodine, need one more electron to reach an octet, so they can form...

vsepr theory

Molecular Shapes from Electron Pairs

Molecular shape can be predicted from the way electron pairs arrange around a central atom. Valence shell electron-pair repulsion theory, or VSEPR theory, uses a Lewis structure to count bonding pairs and lone electron pairs. The main idea is simple: electron pairs spread out as far as possible to reduce repulsion. In a molecule, the valence electrons around the central atom can be bonding pairs or lone pairs. Bonding pairs are found mainly between bonded atoms. Lone pairs stay on one atom and...

molecular geometry and dipole moments

Predicting Shape and Molecular Polarity

Molecular shape and molecular polarity can be predicted with VSEPR theory and dipole moments. Start by writing the Lewis structure of the molecule or polyatomic ion. Then count the electron groups around the central atom. Lone pairs and bonds both count as electron groups, and a single, double, or triple bond each counts as one region of electron density. Use that count to identify the electron-pair geometry. Next, use the number of lone pairs to determine the molecular structure. If more than...

resonance and hybrid structures

Resonance in Nitrite and Carbonate Ions

Resonance explains why some Lewis structures do not match the measured properties of a molecule or ion. When two or more Lewis structures have the same atom arrangement, the real electron distribution is an average of the structures shown. The nitrite anion, NO2−, is one example. It can be drawn in two ways, with the N–O and N=O bonds in different places. If nitrite had one single bond and one double bond, the two bond lengths should be different, because a double bond is shorter and stronger...

valence bond theory and hybridized orbitals

valence-bond-theory-and-hybridized-orbitals

Covalent Bond Overlap and Orbital Hybridization

Covalent bonds form when orbitals on two atoms overlap and their single electrons pair up. The bond is stronger when the overlap is greater. Maximum overlap happens when the orbitals meet along a direct line between the two nuclei. A sigma bond, or σ bond, is the kind of covalent bond found in a single bond in a Lewis structure. In a σ bond, electron density is concentrated along the internuclear axis. A pi bond, or π bond, forms when two p orbitals overlap side by side. In a π bond, the...

mo theory and covalent bonding

Bond Order and Molecular Orbitals

Molecular orbital theory explains how electrons are arranged in molecules. It treats electron regions in a molecule much like atomic orbitals in an atom. A molecular orbital is the region of space where a valence electron is most likely to be found. Molecular orbitals form through the linear combination of atomic orbitals, or LCAO. When atomic wave functions combine in phase, they create regions with high electron density. When they combine out of phase, they create nodes, or regions with no...

intermolecular forces and physical properties

intermolecular-forces-and-physical-properties

How Intermolecular Forces Affect Matter

Intermolecular forces are the attractions between molecules, and they help explain how matter behaves. These forces influence melting points, boiling points, and whether substances mix with one another. Water has a much higher boiling point than hexane, which shows that water has stronger intermolecular forces. Three main kinds of intermolecular interactions are covered here. They include ion-dipole forces, dipole-dipole interactions, and van der Waals forces, which include London dispersion...

solubility

Why Some Substances Dissolve in Water

Solution formation depends on how solutes and solvents interact. A solution is a homogeneous mixture made of a solvent, which is the larger part, and a solute, which is the smaller part. The physical state of a solution is usually the same as the solvent. Concentration is often described as dilute for a low amount of solute or concentrated for a high amount of solute. When a solute dissolves, its particles are surrounded by solvent species. This process is called solvation. If water is the...

introduction to functional groups

Functional Groups and Organic Molecules

Functional groups are groups of atoms with specific chemical properties that appear within organic molecules. They are sometimes shown as "R." These groups sit along the carbon backbone of macromolecules, which can form chains or rings of carbon atoms. Functional groups help functionalize a compound. That means they can give the molecule different physical and chemical properties. In organic chemistry, this change in group structure can strongly affect how a compound behaves. Common...

overview of advanced functional groups

Advanced Functional Groups in Organic Chemistry

Advanced functional groups are atom clusters in organic molecules that give those molecules specific chemical properties. They are sometimes shown as "R" in formulas. By changing the atoms attached to a carbon skeleton, a functional group can make a compound behave differently in physical and chemical reactions. This topic covers several major classes of organic compounds with advanced functional groups. Aromatic hydrocarbons include benzene. Phenol is another example and is also called...

key terms and concepts

Explore carbon-based organic compounds, from hydrocarbons to alcohols, and see how carbon structures and functional groups shape everyday materials.

Carbon Compounds in Everyday Life | JoVE K12

organic chemistry

JoVE Core Organic Chemistry explains basic concepts of stereochemistry, reactions, and mechanisms using concise and easy-to-understand animated video lessons. Additionally, the scientist-in-action videos demonstrate the application of related concepts in classical and original research experiments performed in today's laboratories worldwide.

Florida Department of Education

High School

Physical Science

SC.912.P.8

SC.912.P.8.12

SC.912.P.8.13

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Overview of Advanced Functional Groups


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Polymer Classification: Architecture

Polymers are classified as linear or branched on the basis of their chain architecture. The polymer chains in linear polymers have a long chain-like ...

Matter and Its Interactions: Construct and revise an explanation for the outcome of a simple chemical reaction based on the outermost electron states of atoms, trends in the periodic table, and knowledge of the patterns of chemical properties. (P: 6, CC: 1, CI: PS1)

3 Developing possible explanations of phenomena or designing solutions to engineering problems
 3.2 Constructing explanations and designing solutions 
  3.2.2 Students will be able to use their understanding of scientific principles and the engineering design process to design solutions that meet established criteria and constraints.*  

Carbon Compounds in Everyday Life

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