electronegative atom造句

• This electronegative atom is usually fluorine, oxygen, or nitrogen.
• When in doubt, lone pairs should be placed on more electronegative atoms first.
• In the bulky borates and aluminates, the negative charge is symmetrically distributed over many electronegative atoms.
• Normally, dipoles are associated with electronegative atoms, including oxygen, nitrogen, sulfur, and fluorine.
• A nucleus in the vicinity of an electronegative atom experiences reduced electron density and the nucleus is therefore deshielded.
• Also when the electronegative atom is removed further away the effect diminishes until it can be observed no longer.
• The atomic orbital energy correlates with electronegativity as more electronegative atoms hold their electrons more tightly, lowering their energies.
• A hydrogen atom attached to a relatively electronegative atom will play the role of the hydrogen bond " donor ".
• In the second sense, an oxidizing agent is a chemical species that transfers electronegative atoms, usually oxygen, to a substrate.
• We see that a similar situation occurs, but instead of iodine we now have fluorine, a relatively small highly electronegative atom.
• The hydrogen atoms each have oxidation state + 1, because they surrender their electron to the more electronegative atoms to which they are bonded.
• Increasing the number of electronegative atoms or groups on atom X decreases the electron density in the acidic bond, making the loss of the proton easier.
• Perchloric acid ( HClO 4 ) is an oxoacid and a strong acid . The number of electronegative atoms adjacent to an acidic bond also affects acid strength.
• A hydrogen attached to carbon can also participate in hydrogen bonding when the carbon atom is bound to electronegative atoms, as is the case in chloroform, CHCl 3.
• In a hydrogen bond, the electronegative atom not covalently attached to the hydrogen is named proton acceptor, whereas the one covalently bound to the hydrogen is named the proton donor.
• Nevertheless, peptide bonds can undergo chemical reactions, usually through an attack of an electronegative atom on the carbonyl carbon, breaking the carbonyl double bond and forming a tetrahedral intermediate.
• I mean, overall I guess with all these electronegative atoms the system is strongly electrophilic . . . but I guess the actual negative charge of the ion repels most electron donors away?
• A "'hydrogen bond "'is the attraction between the lone pair of an electronegative atom and a hydrogen atom that is bonded to either nitrogen, oxygen, or fluorine.
• In contrast to the " valency number ", the " oxidation state " can be positive ( for an electropositive atom ) or negative ( for an electronegative atom ).
• In the donor molecule, the electronegative atom attracts the electron cloud from around the hydrogen nucleus of the donor, and, by decentralizing the cloud, leaves the atom with a positive partial charge.