#HYDROGEN VALENCE ELECTRONS HOW TO#
#HYDROGEN VALENCE ELECTRONS FULL#
#HYDROGEN VALENCE ELECTRONS PLUS#

Remember that hydrogen is an exception to the rule though and stable with two electrons! Example Problems The hydrogen in CH 4 all have one covalent bond associated with them, giving them two total electrons. There are two electrons associated with each covalent bond, therefore carbon is following the octet rule. We will start with carbon which has four covalent bonds.

In methane (CH 4) there are two different atoms to look at. Therefore, the total number of electrons associated with each nitrogen atom is 8 and both atoms follow the rule. There are three covalent bonds between the nitrogen atoms and each nitrogen has a lone pair.

The molecules are drawn using Lewis dot structures.

#HYDROGEN VALENCE ELECTRONS HOW TO#

Here are several example problems explaining how to count electrons to determine if an atom is following the octet rule. The further down an atom is in the periodic table, the more likely it is to not have eight electrons in the valence shell and still be stable. For example, SF 6 and XeF 2 are two commonly made gasses in labs.

Some compounds disobey the octet rule.

Lithium often will lose an electron to have the same configuration as helium (2 electrons).

This is because they do not have p-orbitals, and just need the s 2 orbital filled.

Helium and hydrogen both do not follow the octet rule, but instead have two electrons in the valence shell to be stable.

Instead, because of the d-block electrons, they can have more electrons in the valence shell.

Transition metals do not normally follow the octet rule.

The further down you move in the periodic table the more exceptions to the octet rule there are. This trend of decreasing the number of bonds holds true for the rows below the one discussed above.

As you move across the row of the periodic table, the number of bonds tends to decrease for those elements (non-metals) that are covalently bonding.

#HYDROGEN VALENCE ELECTRONS PLUS#

Nitrogen will almost always have three bonds plus a lone pair. For example, carbon will almost always have four bonds. Non-metals tend to gain electrons to obtain eight electrons.Д¬ertain atoms tend to have a certain number of bonds to meet the octet rule. Generally, metals will lose electrons to achieve a valence shell of eight electrons. In ionic bonds, atoms transfer electrons between each other. In covalent bonds, atoms share electrons. The octet rule can be obtained through either ionic or covalent bonds.

#HYDROGEN VALENCE ELECTRONS FULL#

Therefore, the electron configuration ends with s 2 p 6 for all atoms with a full octet. The filled valence octet means that the s and p-orbitals are filled. Neon has a full octet of eight valence electrons and therefore tends not to bond with other atoms. The electron configuration of neon, a noble gas. Hence why other atoms with a full octet are referred to as in вЂnoble-gas configurationвЂ™. This lack of reaction is because they are already at their most stable state with a full octet of electrons. The noble gasses are the only atoms with eight valence electrons and therefore tend not to react or bond with other atoms and molecules. A configuration that has eight electrons is also referred to as the вЂnoble-gas configurationвЂ™. An atom that does not have eight electrons will bond with other atoms to have eight electrons. The octet rule is that an atom will be most stable when surrounded by 8 electrons in the valence shell. In this tutorial, you will learn what the octet rule is, the exceptions to the rule, and see examples and problems.

Hydrogen valence electrons