How many electrons must the atoms of the elements below share with other atoms in covalent bonding to achieve an octet of electrons?

Whether an atom gains or loses electrons is governed by two measurable quantities - ionization energy and electron affinity. Ionization energy (IE) is the energy required to remove the...

The main reason the noble gases do not need to bond with other is that their outermost subshells are filled. These are known as . Take helium for example. It...

The carbon atom has an electronic configuration of $1s^(2)2s^(2)2p^(2)$. The $2s$ and the $2p$ orbitals participate in ; a tetrahedral $sp^3$ hybridization scheme is commonly invoked in order to describe...

As a chalcogen, sulfur generally behaves as does oxygen. However, sulfur can form up to 6 covalent bonds: $SF_6$ is an example.

The for phosphorus is $1s^2 2s^2 2p^6 3s^2 3p^3$. The are usually the outermost s and p electrons and in this case, there are 2 3s electrons and 3 3p...

We formally invoke a triple bond in $:C-=O$, a double bond in $O=O$, and a single bond in $Cl-Cl$. Given these representations, there are $6$, $4$, and $2$ electrons in...

Carbon can form single bonds, double bonds and triple bonds. Each bond is an electron pair, so a triple bond would be the sharing of 3 electron pairs => $-C-=C-$...

I'm guessing that one element that never obeys the when is beryllium. Beryllium has only 2 for bonding. Another element that does not follow the octet rule is boron....

By sharing one or more electrons. Let's take Fluorine (F). It has 7 electrons in its outer shell, but it "wants" to have 8 (the octet rule). Now with another...

Consider ethylene, $H_2C=CH_2$. Each hydrogen atom has the one electron available for . Each carbon atom has 4 electrons available for bonding. (The remaining electrons $C, Z=6$ are inner core,...