explain the formation of covalent compound molecules F2&NH3.using Lewis dot structure
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Two H atoms, each contributing an electron, share a pair of electrons.The former, known as a 'Lewis dot diagram,' indicates a pair of shared electrons between the atomic symbols, while the latter, known as a 'Lewis structure,' uses a dash to indicate the pair of shared electrons that form a covalent bond.
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The octet rule says that the noble gas electronic configuration is a particularly favorable one that can be achieved through formation of electron pair bonds between atoms.
In many atoms, not all of the electron pairs comprising the octet are shared between atoms. These unshared, non-bonding electrons are called ‘lone pairs’ of electrons.
Although lone pairs are not directly involved in bond formation, they should always be shown in Lewis structures.
There is a logical procedure that can be followed to draw the Lewis structure of a molecule or compound.
Terms
Lewis structureFormalism used to show the structure of a molecule or compound, in which shared electrons pairs between atoms are indicated by dashes. Non-bonding, lone pairs of electrons must also be shown.
covalent bondTwo atoms share valence electrons in order to achieve a noble gas electronic configuration.
exceptions to the octet ruleHydrogen (H) and helium (He) only need two electrons to have a full valence level.
octet ruleAtoms try to achieve the electronic configuration of the noble gas nearest to them in the periodic table by achieving a full valence level with eight electrons.
The Octet Rule
Noble gases like He, Ne, Ar, Kr, etc., are stable because their valence level is filled with as many electrons as possible. Eight electrons fill the valence level for all noble gases, except helium, which has two electrons in its full valence level. Other elements in the periodic table react to form bonds in which valence electrons are exchanged or shared in order to achieve a valence level which is filled, just like in the noble gases. We refer to this chemical tendency of atoms as ‘the octet rule,’ and it guides us in predicting how atoms combine to form molecules and compounds.
Covalent Bonds and Lewis Diagrams of Simple Molecules
The simplest example to consider is hydrogen (H), which is the smallest element in the periodic table with one proton and one electron. Hydrogen can become stable if it achieves a full valence level like the noble gas that is closest to it in the periodic table, helium (He). These are exceptions to the octet rule because they only require 2 electrons to have a full valence level.
Two H atoms can come together and share each of their electrons to create a ‘covalent bond.’ The shared pair of electrons can be thought of as belonging to either atom, and thus each atom now has two electrons in its valence level, like He. The molecule that results is H2, and it is the most abundant molecule in the universe.
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In many atoms, not all of the electron pairs comprising the octet are shared between atoms. These unshared, non-bonding electrons are called ‘lone pairs’ of electrons.
Although lone pairs are not directly involved in bond formation, they should always be shown in Lewis structures.
There is a logical procedure that can be followed to draw the Lewis structure of a molecule or compound.
Terms
Lewis structureFormalism used to show the structure of a molecule or compound, in which shared electrons pairs between atoms are indicated by dashes. Non-bonding, lone pairs of electrons must also be shown.
covalent bondTwo atoms share valence electrons in order to achieve a noble gas electronic configuration.
exceptions to the octet ruleHydrogen (H) and helium (He) only need two electrons to have a full valence level.
octet ruleAtoms try to achieve the electronic configuration of the noble gas nearest to them in the periodic table by achieving a full valence level with eight electrons.
The Octet Rule
Noble gases like He, Ne, Ar, Kr, etc., are stable because their valence level is filled with as many electrons as possible. Eight electrons fill the valence level for all noble gases, except helium, which has two electrons in its full valence level. Other elements in the periodic table react to form bonds in which valence electrons are exchanged or shared in order to achieve a valence level which is filled, just like in the noble gases. We refer to this chemical tendency of atoms as ‘the octet rule,’ and it guides us in predicting how atoms combine to form molecules and compounds.
Covalent Bonds and Lewis Diagrams of Simple Molecules
The simplest example to consider is hydrogen (H), which is the smallest element in the periodic table with one proton and one electron. Hydrogen can become stable if it achieves a full valence level like the noble gas that is closest to it in the periodic table, helium (He). These are exceptions to the octet rule because they only require 2 electrons to have a full valence level.
Two H atoms can come together and share each of their electrons to create a ‘covalent bond.’ The shared pair of electrons can be thought of as belonging to either atom, and thus each atom now has two electrons in its valence level, like He. The molecule that results is H2, and it is the most abundant molecule in the universe.
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