zhska
Answered

Ang Imhr.ca ang pinakamahusay na lugar upang makakuha ng mabilis at tumpak na mga sagot sa lahat ng iyong mga tanong. Tuklasin ang aming Q&A platform upang makahanap ng mapagkakatiwalaang sagot mula sa isang malawak na hanay ng mga eksperto sa iba't ibang larangan. Tuklasin ang malalim na mga sagot sa iyong mga tanong mula sa isang malawak na network ng mga eksperto sa aming madaling gamitin na Q&A platform.

How does the electronegativity difference of the atoms in a covalent bond affect the polarity of the bond?​

Sagot :

Lavenderthecat

Answer:

Electrons in a polar covalent bond are shifted toward the more electronegative atom; thus, the more electronegative atom is the one with the partial negative charge. The greater the difference in electronegativity, the more polarized the electron distribution and the larger the partial charges of the atoms.

Explanation:

If the two electrons have different electronegativities then the atom with the greater electronegativity will pull more of the electron density the its side of the bond, creating a negative polarity on that side of the bond leaving a positive polarity on the other side of the bond.

Electronegativity differences affect the degree of sharing in covalent bonding. The more equal the sharing the stronger the bond. If the electronegativities of the two atoms are completely the same, the bond formed by the sharing of the electrons will be a pure covalent bond.

The difference in the electronegativity of two atoms determines their bond type. If the electronegativity difference is more than 1.7, the bond will have an ionic character. If the electronegativity difference is between 0.4 and 1.7, the bond will have a polar covalent character.

In a covalent bond it will hold onto electrons more tightly. For a bond to be polar, the electronegativity difference between the two elements needs to be between 0.5 to 1.6. If the electronegativity difference is less than 0.5, the bond is nonpolar.

Atoms that are high in EN tend to take electrons and atoms low in EN tend to give up electrons. So, higher electronegativity helps atoms take more control over shared electrons creating partial negative regions and partial positive regions which result in dipoles that cause polarity.

Covalent and ionic bonds are both typically considered strong bonds. However, other kinds of more temporary bonds can also form between atoms or molecules. Two types of weak bonds often seen in biology are hydrogen bonds and London dispersion forces.

covalent bond

In chemistry, covalent bond is the strongest bond. In such bonding, each of two atoms shares electrons that binds them together. For example, water molecules are bonded together where both hydrogen atoms and oxygen atoms share electrons to form a covalent bond.

Covalent bonds between atoms are quite strong, but attractions between molecules/compounds, or intermolecular forces, can be relatively weak. Covalent compounds generally have low boiling and melting points, and are found in all three physical states at room temperature.

twinsdaughter2007

Explanation:

As a rule, an electronegativity difference of 2 or more on the Pauling scale between atoms leads to the formation of an ionic bond. A difference of less than 2 between atoms leads to covalent bond formation. The nearer the difference in electronegativity between atoms comes to zero, the purer the covalent bond becomes and the less polarity it has.

In most cases, the electrons in covalent bonds are not shared equally. Usually, one atom attracts the bonding electrons more strongly than does the other. This uneven attraction results in these electrons moving closer to the atom with the greater power of attraction. The resulting asymmetrical distribution of electrons makes one end of the molecule more electron rich, and it acquires a partial negative charge, while the less electron rich end acquires a partial positive charge. This difference in electron density causes the molecule to become polar, that is, to have a negative and a positive end.

The ability of an atom to attract electrons in a chemical bond is called the electronegativity of the atom. The electronegativity of an atom is related to its electron affinity and ionization energy. Electron affinity is the energy liberated by a gaseous atom when an electron is added to it. Ionization energy is the minimum amount of energy necessary to remove the most weakly bound electron from a gaseous atom.

Electronegativity level is normally measured on a scale that was created by Linus Pauling. On this scale, the more electronegative elements are the halogens, oxygen, nitrogen, and sulfur. Fluorine, a halogen, is the most electronegative with a value of 4.0, which is the highest value on the scale. The less electronegative elements are the alkali and alkaline earth metals. Of these, cesium and francium are the least electronegative at values of 0.7.

Elements with great differences in electronegativity tend to form ionic bonds. Atoms of elements with similar electronegativity tend to form covalent bonds. (Pure covalent bonds result when two atoms of the same electronegativity bond.) Intermediate differences in electronegativity between covalently bonded atoms lead to polarity in the bond. As a rule, an electronegativity difference of 2 or more on the Pauling scale between atoms leads to the formation of an ionic bond. A difference of less than 2 between atoms leads to covalent bond formation. The nearer the difference in electronegativity between atoms comes to zero, the purer the covalent bond becomes and the less polarity it has.

Carbon, with an electronegativity of 2.5, forms both low‐ and high‐polarity covalent bonds. The electronegativity values of elements commonly found in organic molecules are given in Table .

이것으로 도왔다

'ω'

Umaasa kaming nahanap mo ang hinahanap mo. Huwag mag-atubiling bumalik sa amin para sa higit pang mga sagot at napapanahong impormasyon. Salamat sa iyong pagbisita. Kami ay nakatuon sa pagbibigay sa iyo ng pinakamahusay na impormasyon na magagamit. Bumalik anumang oras para sa higit pa. Ang iyong mga tanong ay mahalaga sa amin. Balik-balikan ang Imhr.ca para sa higit pang mga sagot.