Explain how valence electrons are responsible for the number of bonds an atom can form.
Specifically how is it that atoms that have 1-4 valence will make the same number
of
bonds
equal to the valence electrons and atoms that have 5-7 valence electrons will use
the
formula #
=
bonds 8-valence electrons? In addition, explain why elements that have 8 valence electrons
will not form any bonds?
mr with 1-4 valence eletrons will form a

Valence electrons dictate the number and type of chemical bonds atoms can form based on their octet rule. Elements with differing valence electron counts exhibit distinct bonding behaviors.

Explanation:

Chemical bonding is determined by the outermost shell of electrons, called the valence electrons (VE), of an atom. The number of VE is important when determining the number and type of chemical bonds an atom will form.

The number of bonds an atom can form is often predicted by the number of electrons needed to reach an octet (eight valence electrons). Elements within groups 4 through 7 of the periodic table tend to form bonds based on the number of valence electrons they possess.

Atoms with 1-4 valence electrons typically form a number of bonds equal to their valence electrons. Meanwhile, elements with 5-7 valence electrons tend to form bonds following the formula # = 8 - valence electrons. Elements with 8 valence electrons are already stable and do not form bonds.

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