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Chemistry311/312 Name: CovalentBonding UnitReviewPacket LearningTargets Identifytheinformationamolecularformulaprovides. Describetherepresentativeunitsthatdefinemolecularcompoundsandioniccompounds.
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How to Fill Out Covalent Bonding - MS:

01
Start by understanding the concept of covalent bonding, which is a type of chemical bond formed when two atoms share electrons.
02
Identify the elements involved in the covalent bond and determine their valence electron configurations. This will help you determine the number of electrons each atom needs to complete its outermost energy level.
03
Determine the number of electrons each atom in the bond already has, and calculate the number of electrons it needs to gain or lose to achieve stability.
04
Determine the central atom in the molecule. This is usually the least electronegative element.
05
Use Lewis dot structures to represent each atom's valence electrons. Place one dot for each valence electron around the symbol of each element.
06
Connect the atoms with a single bond by sharing one pair of electrons between them. This is done by drawing a line between the symbols of the atoms.
07
Arrange any remaining electrons around the atoms to satisfy the octet rule, where each atom (except hydrogen) should have eight electrons around it.
08
If necessary, convert any unshared electron pairs into multiple bonds (double or triple bonds) to achieve the octet rule for all atoms.
09
Double-check your work to ensure all electrons are accounted for, and the number of valence electrons for each atom matches its needs.
10
Finally, label the type of bond formed (single, double, or triple bond) in the molecule.

Who Needs Covalent Bonding - MS:

01
Students studying chemistry or chemical bonding will benefit from learning about covalent bonding - MS to understand how atoms form stable molecules by sharing electrons.
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Covalent bonding - ms refers to the sharing of electron pairs between atoms.
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