Asked 8 years, 3 months ago. Active 3 years, 8 months ago. Viewed 20k times. Improve this question. Gerard Gerard 3, 13 13 gold badges 36 36 silver badges 47 47 bronze badges. Add a comment. Active Oldest Votes. Improve this answer. The point is, what makes things metallic is not as simple and brute force as ionization energy. Strictly speaking, metal bonding is a kind of covalent bonding in a sense.
In bulk metals, similar bonding bond is working for valence electron. Even more strictly speaking, to fully understand the matter you have to consider the matter from position of theory of molecular orbitals.
Let's assume we have a nanocrystal of 3d row element atoms. From orbitals of said atoms molecular orbitals are formed, with strict distribution of their energies depending on shape and size of the crystal and crystal cell. Related questions Are polyatomic ions molecular compounds or ionic compounds? What type of atoms tend to form covalent bonds?
What is an example of a covalent bonds practice problem? What are some examples of stable electronic configurations? How are covalent bonds named? How can elements achieve a stable electron configurations? It's not trivial at all, and in truth you probably don't need to care about these exotic examples until you have enough experience to understand the bonding. See the following references: M.
Evans, M. Polanyi, Transactions Faraday Society 35, ; C. Bawn, Ann. Your textbook is right. Lots of metals form covalent bonds.
In the case of lithium chloride such bonding is one explanation for the solubility of this compound in organic solvents see this answer. One additional example you might want to know about is Grignard reagents , a class of highly basic compounds in which carbon is covalently bonded to magnesium.
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A Nonpolar Covalent Bond is created when atoms share their electrons equally. This usually occurs when two atoms have similar or the same electron affinity.
The closer the values of their electron affinity , the stronger the attraction. This occurs in gas molecules; also known as diatomic elements. Nonpolar covalent bonds have a similar concept as polar covalent bonds; the atom with the higher electronegativity will draw away the electron from the weaker one.
Since this statement is true--if we apply this to our diatomic molecules--all the atoms will have the same electronegativity since they are the same kind of element; thus, the electronegativities will cancel each other out and will have a charge of 0 i. Examples of gas molecules that have a nonpolar covalent bond: Hydrogen gas atom, Nitrogen gas atoms, etc. As you can see from the picture above, Hydrogen gas has a total of 2 Hydrogen atoms. Each Hydrogen atom has 1 valence electron.
Since Hydrogen can only fit a max of 2 valence electrons in its orbital, each Hydrogen atom only needs 1 electron. Each atom has 1 valence electron, so they can just share, giving each atom two electrons each.
Write the electron configuration and determine how many electrons are needed to achieve the nearest noble-gas configuration for the following:. Introduction Only when two atoms of the same element form a covalent bond are the shared electrons actually shared equally between the atoms.
Octet Rule The Octet Rule requires all atoms in a molecule to have 8 valence electrons--either by sharing, losing or gaining electrons--to become stable. More examples can be found here. Single Bonds A single bond is when two electrons--one pair of electrons--are shared between two atoms. Double Bonds A Double bond is when two atoms share two pairs of electrons with each other.
Triple Bond A Triple bond is when three pairs of electrons are shared between two atoms in a molecule. Example 3: Acetylene Below is a Lewis dot structure of Acetylene demonstrating a triple bond. Example: Water, Sulfide, Ozone, etc. References Petrucci, Ralph H. New Jersey: Pearson Education, Inc. Vaczek, Louis. Pickering, H.
Kotz, Treichel, Townsend.
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