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By bonding with another atom, either ionically (donates/receives electrons) or covalently (electron sharing).
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Explain what atoms are trying to achieve in there electron shells when they bond with each outher?
Atoms are trying achieve a stable electronic configuration i.e., stable arrangement of electrons in their electron shells. All configurations are not stable. Mostly stable configuration is attained by forming an octet of electrons in outer most shell. Sometimes octet rule is violated also.
How many electron must phosphorus gain in order to achieve an octet?
This atom must gain 3 electrons to achieve an octet.
Why do atoms forms bonds?
Atoms form bonds to achieve an octet of valence electrons.
What The octet rule is satisfied when two atoms acquire how many valence electrons?
Eight
How could oxygen achieve a stable octet?
Yes. The octet rule is a rule of thumb that states that atoms tend for form bonds that allow the bonded atoms to have eight electrons in their valence shells. This is a "driving force" in chemistry, and it explains many, many reactions. Use the link below to gather more information.
How many electrons must the atoms of S share with other atoms in covalent bonding to achieve an octet of electrons?
two electrons
How can atoms achieve octet rule?
by losing or gaining electrons to become stable
What states that atoms tend to gain lose or share electrons in order to achieve a full set of valence electrons typically?
The octet rule.
What two things can atoms do to achieve a stable octet of electrons?
They can either pick the electrons from around them, or start throwing them off in a measure of radioactivity.
How many electrons that an atom in the oxygen family gain or share?
Atoms in the oxygen family can gain or share two electrons in order to achieve an octet of electrons.
Why would two oxygen atoms want to form a double covalent bond?
A lone oxygen atom has 6 electrons in its outer shell which is not very stable, whereas as full octet (8 outer shell electrons) is stable. In order to achieve this two oxygen atoms will share 4 electrons, each contributing 2 electrons. Since these electrons exist within the orbitals of both atoms, to oxygen atoms essentially achieve a full octet.
How are the duet and octet rules used to describe the arrangement of electrons in a molecule?
The very simple duet and octet models of covalent chemical bonding describe the chemical bond as involving an electron pair situated between atoms and that atoms lighter than He (there is only H!) achieve a stable duet (2 electrons)-- atoms heavier than He achieve an octet. the duet and octet are the stable configurations of noble gases. Lewis dot diagrams are typically used to "place" the electrons in the appropriate positions.
Do metals gain electrons to have full octet?
No, metals tend to lose electrons to achieve a full octet.
Does lithium follow the octet rule?
Sort of. Lithium loses one electron in order to achieve the noble gas configuration of helium, which has only two valence electrons in its 1s sublevel. The octet rule refers to the fact that atoms share or transfer electrons in order to achieve a noble gas configuration with eight valence electrons, called an octet. Helium is an exception to the rule.
What is the formation of an ion from a metal and a nonmetal in terms of the octet rule?
Atoms of metals tend to lose their valence electrons,leaving a complete octect in the next-lowest energy level. Atoms of some non-metals tend to gain electrons or to share electrons with another nonmetal to achieve a complete octet.
Why do atoms gain loose or share electrons?
Atom loose or gain electron to make its octet complete. It is done to achieve inert state.
Explain what atoms are trying to achieve in there electron shells when they bond with each outher?
Atoms are trying achieve a stable electronic configuration i.e., stable arrangement of electrons in their electron shells. All configurations are not stable. Mostly stable configuration is attained by forming an octet of electrons in outer most shell. Sometimes octet rule is violated also.
