What element has an atom with the greatest attraction for electrons in a chemical bond? Chemistry Bonding Basics Bonding. Ernest Z. Dec 27, The element with greatest attraction for electrons in a double bond is number 9, fluorine.
Explanation: Fluorine has the greatest attraction for electrons in any bond that it forms. Related questions What is the Lennard-Jones potential? This electron exchange results in an electrostatic attraction between the two atoms called an ionic bond. An atom that loses one or more valence electrons to become a positively charged ion is known as a cation, while an atom that gains electrons and becomes negatively charged is known as an anion. This exchange of valence electrons allows ions to achieve electron configurations that mimic those of the noble gases, satisfying the octet rule.
The octet rule states that an atom is most stable when there are eight electrons in its valence shell. Atoms with less than eight electrons tend to satisfy the duet rule, having two electrons in their valence shell. By satisfying the duet rule or the octet rule, ions are more stable.
An anion is indicated by a negative superscript charge - something to the right of the atom. Similarly, if a chlorine atom gains an extra electron, it becomes the chloride ion, Cl —.
Both ions form because the ion is more stable than the atom due to the octet rule. Once the oppositely charged ions form, they are attracted by their positive and negative charges and form an ionic compound.
Ionic bonds are also formed when there is a large electronegativity difference between two atoms. This difference causes an unequal sharing of electrons such that one atom completely loses one or more electrons and the other atom gains one or more electrons, such as in the creation of an ionic bond between a metal atom sodium and a nonmetal fluorine. Formation of sodium fluoride : The transfer of electrons and subsequent attraction of oppositely charged ions. To determine the chemical formulas of ionic compounds, the following two conditions must be satisfied:.
This is because Mg has two valence electrons and it would like to get rid of those two ions to obey the octet rule. Fluorine has seven valence electrons and usually forms the F — ion because it gains one electron to satisfy the octet rule. Therefore, the formula of the compound is MgF 2. The subscript two indicates that there are two fluorines that are ionically bonded to magnesium. On the macroscopic scale, ionic compounds form crystalline lattice structures that are characterized by high melting and boiling points and good electrical conductivity when melted or solubilized.
Fluorine has seven valence electrons and as such, usually forms the F — ion because it gains one electron to satisfy the octet rule. Covalent bonds are a class of chemical bonds where valence electrons are shared between two atoms, typically two nonmetals. The formation of a covalent bond allows the nonmetals to obey the octet rule and thus become more stable. For example:. Covalent bonding requires a specific orientation between atoms in order to achieve the overlap between bonding orbitals.
Sigma bonds are the strongest type of covalent interaction and are formed via the overlap of atomic orbitals along the orbital axis. The overlapped orbitals allow the shared electrons to move freely between atoms. Pi bonds are a weaker type of covalent interactions and result from the overlap of two lobes of the interacting atomic orbitals above and below the orbital axis.
Unlike an ionic bond, a covalent bond is stronger between two atoms with similar electronegativity. For atoms with equal electronegativity, the bond between them will be a non- polar covalent interaction. In non-polar covalent bonds, the electrons are equally shared between the two atoms. For atoms with differing electronegativity, the bond will be a polar covalent interaction, where the electrons will not be shared equally.
Electronegativity increases from bottom to top in groups , and increases from left to right across periods. Thus, fluorine is the most electronegative element, while francium is one of the least electronegative. Helium, neon, and argon are not listed in the Pauling electronegativity scale, although in the Allred-Rochow scale, helium has the highest electronegativity. The trends are not very smooth among the transition metals and the inner transition metals, but are fairly regular for the main group elements, and can be seen in the charts below.
The difference in electronegativity between two bonded elements determines what type of bond they will form. When atoms with an electronegativity difference of greater than two units are joined together, the bond that is formed is an ionic bond , in which the more electronegative element has a negative charge, and the less electronegative element has a positive charge. As an analogy, you can think of it as a game of tug-of-war in which one team is strong enough to pull the rope away from the other team.
For example, sodium has an electronegativity of 0. Particular sodium and chloride ions are not "tied" together, but they attract each other very strong because of the opposite charges, and form a strong crystal lattice.
When atoms with an electronegativity difference of less than two units are joined together, the bond that is formed is a covalent bond , in which the electrons are shared by both atoms.
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