Hydrocarbon Derivatives:
... Hydrocarbons • contain only carbon & hydrogen • carbon can also form strong covalent bonds with other elements such as: O, N, F, Cl, Br, I, S, & P ...
... Hydrocarbons • contain only carbon & hydrogen • carbon can also form strong covalent bonds with other elements such as: O, N, F, Cl, Br, I, S, & P ...
2.11 Analytical Techniques notes - A
... Most of the functional groups give characteristic absorptions in the region of the spectrum between 1500 and 3500 cm-1. It is this region that is typically used to identify the functional groups as there are few other peaks in this region (except the C-H peak which is easily identifiable). All the p ...
... Most of the functional groups give characteristic absorptions in the region of the spectrum between 1500 and 3500 cm-1. It is this region that is typically used to identify the functional groups as there are few other peaks in this region (except the C-H peak which is easily identifiable). All the p ...
Alkenes Key features sp -hybridized carbons, 120 bond angles
... Some reactions favor reaction to occur with a particular orientation, where a given region of the molecule is more likely to participate in bond formation. This regioselectivity occurs with hydrogen halide addition to alkenes, so products have predictable structures based on the pattern of reactivit ...
... Some reactions favor reaction to occur with a particular orientation, where a given region of the molecule is more likely to participate in bond formation. This regioselectivity occurs with hydrogen halide addition to alkenes, so products have predictable structures based on the pattern of reactivit ...
INTRODUCTION TO ORGANIC CHEMISTRY
... - Two stable isotops (13C and 12C) - electron configuration: 1s2 2s2 2p2 - four valence electrons - can form more compounds than any other element - able to form single, double and triple carboncarbon bonds, and to link up with each other in chains and ring structures ...
... - Two stable isotops (13C and 12C) - electron configuration: 1s2 2s2 2p2 - four valence electrons - can form more compounds than any other element - able to form single, double and triple carboncarbon bonds, and to link up with each other in chains and ring structures ...
Functional Group Isomerism
... These isomers are referred to as enantiomers. The central carbon atom to which four different atoms or groups are attached, is called an asymmetrical carbon atom. Enantiomers have identical physical constants, such as melting points and boiling points, but are said to be optically active since they ...
... These isomers are referred to as enantiomers. The central carbon atom to which four different atoms or groups are attached, is called an asymmetrical carbon atom. Enantiomers have identical physical constants, such as melting points and boiling points, but are said to be optically active since they ...
Study Guide for Chapter 22 - Hydrocarbon Compounds
... of rotation about a carbon-carbon double bond leads to geometric isomers. 68. Most cyclic hydrocarbons have higher boiling ...
... of rotation about a carbon-carbon double bond leads to geometric isomers. 68. Most cyclic hydrocarbons have higher boiling ...
Sheet #24 (archive) Medicinal Plants
... β Carotene it is monocyclic structure in both ends of the molecule and this cyclic structure has only one double bond , and these double bond either in agreement with double bonds of side chain then we get β ionene ring( conjugated between double bond of cycle and side chain [ [ ــــ = ـــــ = ـــ ...
... β Carotene it is monocyclic structure in both ends of the molecule and this cyclic structure has only one double bond , and these double bond either in agreement with double bonds of side chain then we get β ionene ring( conjugated between double bond of cycle and side chain [ [ ــــ = ـــــ = ـــ ...
Chapter 19
... – Carbon: normally forms four covalent bonds and has no unshared pairs of electrons. C – Hydrogen: forms one covalent bond and no unshared pairs of electrons. H – Nitrogen: normally forms three covalent bonds and has one unshared pair of electrons. ...
... – Carbon: normally forms four covalent bonds and has no unshared pairs of electrons. C – Hydrogen: forms one covalent bond and no unshared pairs of electrons. H – Nitrogen: normally forms three covalent bonds and has one unshared pair of electrons. ...
IUPAC nomenclature of organic chemistry
... 2. Has the lowest-numbered locants for multiple bonds (The locant of a multiple bond is the number of the adjacent carbon with a lower number). 3. Has the lowest-numbered locants for double bonds. 4. Has the lowest-numbered locants for prefixes. Numbering of the various substituents and bonds with t ...
... 2. Has the lowest-numbered locants for multiple bonds (The locant of a multiple bond is the number of the adjacent carbon with a lower number). 3. Has the lowest-numbered locants for double bonds. 4. Has the lowest-numbered locants for prefixes. Numbering of the various substituents and bonds with t ...
Naming Alkanes Handout.key
... After this lesson you should be able to Name alkanes using IUPAC rules ...
... After this lesson you should be able to Name alkanes using IUPAC rules ...
Ch. 14 Alcohols, Ethers, & Thiols
... Physical Properties of Alcohols • Because of increase london forces between larger molecules, the B.P. of all types of compounds, including alcohols, increase as molecular weight increases • Alcohols are much more soluble in H2O due to their H-bonding capacity. • As MW increases, the water solubili ...
... Physical Properties of Alcohols • Because of increase london forces between larger molecules, the B.P. of all types of compounds, including alcohols, increase as molecular weight increases • Alcohols are much more soluble in H2O due to their H-bonding capacity. • As MW increases, the water solubili ...
Guide_to_Life_in_Orgo_Ib
... Predict the products of electrophilic addition reactions of conjugated dienes, and explain why certain products are favored using the concept of the allylic carbocation. ...
... Predict the products of electrophilic addition reactions of conjugated dienes, and explain why certain products are favored using the concept of the allylic carbocation. ...
Paper 41
... Results and Discussion In the temperature range of 1600 K - 2200 K, the investigated induction times for soot formation show no dependence on the oxygen content of the studied mixtures. The activation energy of the induction time for the pure C6H6 pyrolysis and for the C6H6 /O2 mixtures is about 229 ...
... Results and Discussion In the temperature range of 1600 K - 2200 K, the investigated induction times for soot formation show no dependence on the oxygen content of the studied mixtures. The activation energy of the induction time for the pure C6H6 pyrolysis and for the C6H6 /O2 mixtures is about 229 ...
Chapter 8. CARBONYL COMPOUNDS
... The aldol can be easily dehydrated on heating because it retains the acidic α-hydrogen. α,βUnsaturated aldehydes and ketones are formed when the reaction is performed at elevated temperature. Crotonaldehyde is obtained from the simplest aldol in this way, therefore reactions of this type are called ...
... The aldol can be easily dehydrated on heating because it retains the acidic α-hydrogen. α,βUnsaturated aldehydes and ketones are formed when the reaction is performed at elevated temperature. Crotonaldehyde is obtained from the simplest aldol in this way, therefore reactions of this type are called ...
Supramolecular Assemblies Built from Lanthanide
... bonds. Three complexes were obtained with the enantiopure α-amino acid L-methionine (L-me), all of which are chiral. In [Yb(L-me)(H2O)7]·CB6·3NO3·7H2O (3) and [Dy(L-me)(H2O)7]4[Dy(NO3)2(H2O)5]·4CB6·13NO3·29H2O (4), the metal ions are bound to one monodentate carboxylate and seven water molecules. Th ...
... bonds. Three complexes were obtained with the enantiopure α-amino acid L-methionine (L-me), all of which are chiral. In [Yb(L-me)(H2O)7]·CB6·3NO3·7H2O (3) and [Dy(L-me)(H2O)7]4[Dy(NO3)2(H2O)5]·4CB6·13NO3·29H2O (4), the metal ions are bound to one monodentate carboxylate and seven water molecules. Th ...
Chapter 12: Oxidations In order to discuss the oxidation
... Oxidation of alkenes usually results in the loss of the pi bond And formation of two new sigma bonds between the carbons of the alkene and atoms more electronegative than carbon ...
... Oxidation of alkenes usually results in the loss of the pi bond And formation of two new sigma bonds between the carbons of the alkene and atoms more electronegative than carbon ...
Polar Alignment of -Shaped Basic Building Units within Transition
... active crystals requires that the crystal belong to a noncentrosymmetric (NCS) crystal class.1−5 Previous attempts to create NCS crystals have used chiral organic molecules, as the chirality is necessarily preserved within the bulk structure.6 This method synthesizes organic molecular crystals that ...
... active crystals requires that the crystal belong to a noncentrosymmetric (NCS) crystal class.1−5 Previous attempts to create NCS crystals have used chiral organic molecules, as the chirality is necessarily preserved within the bulk structure.6 This method synthesizes organic molecular crystals that ...
Covalent Bonding and Molecular Structure
... The representation of H2 shown previously where the bonding electrons are represented with a line, H3H, is the Lewis structure of H2. In a Lewis structure, bonding pairs of electrons are represented as lines connecting atom symbols, and nonbonding electrons are shown as dots (Interactive Figure 8.2. ...
... The representation of H2 shown previously where the bonding electrons are represented with a line, H3H, is the Lewis structure of H2. In a Lewis structure, bonding pairs of electrons are represented as lines connecting atom symbols, and nonbonding electrons are shown as dots (Interactive Figure 8.2. ...
Aromaticity
In organic chemistry, the term aromaticity is formally used to describe an unusually stable nature of some flat rings of atoms. These structures contain a number of double bonds that interact with each other according to certain rules. As a result of their being so stable, such rings tend to form easily, and once formed, tend to be difficult to break in chemical reactions. Since one of the most commonly encountered aromatic system of compounds in organic chemistry is based on derivatives of the prototypical aromatic compound benzene (common in petroleum), the word “aromatic” is occasionally used to refer informally to benzene derivatives, and this is how it was first defined. Nevertheless, many non-benzene aromatic compounds exist. In living organisms, for example, the most common aromatic rings are the double-ringed bases in RNA and DNA.The earliest use of the term “aromatic” was in an article by August Wilhelm Hofmann in 1855. Hofmann used the term for a class of benzene compounds, many of which do have odors (unlike pure saturated hydrocarbons). Today, there is no general relationship between aromaticity as a chemical property and the olfactory properties of such compounds, although in 1855, before the structure of benzene or organic compounds was understood, chemists like Hofmann were beginning to understand that odiferous molecules from plants, such as terpenes, had chemical properties we recognize today are similar to unsaturated petroleum hydrocarbons like benzene.In terms of the electronic nature of the molecule, aromaticity describes the way a conjugated ring of unsaturated bonds, lone pairs of electrons, or empty molecular orbitals exhibit a stabilization stronger than would be expected by the stabilization of conjugation alone. Aromaticity can be considered a manifestation of cyclic delocalization and of resonance. This is usually considered to be because electrons are free to cycle around circular arrangements of atoms that are alternately single- and double-bonded to one another. These bonds may be seen as a hybrid of a single bond and a double bond, each bond in the ring identical to every other. This commonly seen model of aromatic rings, namely the idea that benzene was formed from a six-membered carbon ring with alternating single and double bonds (cyclohexatriene), was developed by August Kekulé (see History section below). The model for benzene consists of two resonance forms, which corresponds to the double and single bonds superimposing to produce six one-and-a-half bonds. Benzene is a more stable molecule than would be expected without accounting for charge delocalization.