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11 Nov 2019
For each of the compounds below determine if the oxygen or nitrogen atom in the molecule has a formal charge. If there is a charge, draw the charge near the atom and circle it. If the there is no formal charge, write "nc" near the molecule. In the next exercise you will encounter some atoms with a formal charge. Remember that carbon is in group 4 of the periodic table and is therefore usually seen with 4 bonds. If the carbon has a (+) charge, then it is because carbon only possesses 3 electrons so that means that there is one electron (and therefore one bond) missing. If the carbon has a (-) charge, then carbon must own 5 electrons which means it will have three bonds and one lone pair of electrons. A minus charge automatically signifies an extra lone pair of electrons. For each of the following problems, take a look at where the charges are located and draw in all missing lone pairs of electrons. The lone pairs of electrons will be on certain carbon, nitrogen and oxygen atoms. D: Resonance Structures In the next two questions, we will tackle resonance structures. A combination of resonance structures more accurately describes a particular molecule and helps us better understand the electronic nature of the compound of interest. Instead of just guessing what a resonance structure will look like, it is helpful to draw the arrows leading from one structure to the next. There are a few things you should keep in mind. There are two important "commandments" that you can never violate when pushing arrows. a Thou shall not break a single bond b. Thou shall not violate the octet rule.
For each of the compounds below determine if the oxygen or nitrogen atom in the molecule has a formal charge. If there is a charge, draw the charge near the atom and circle it. If the there is no formal charge, write "nc" near the molecule. In the next exercise you will encounter some atoms with a formal charge. Remember that carbon is in group 4 of the periodic table and is therefore usually seen with 4 bonds. If the carbon has a (+) charge, then it is because carbon only possesses 3 electrons so that means that there is one electron (and therefore one bond) missing. If the carbon has a (-) charge, then carbon must own 5 electrons which means it will have three bonds and one lone pair of electrons. A minus charge automatically signifies an extra lone pair of electrons. For each of the following problems, take a look at where the charges are located and draw in all missing lone pairs of electrons. The lone pairs of electrons will be on certain carbon, nitrogen and oxygen atoms. D: Resonance Structures In the next two questions, we will tackle resonance structures. A combination of resonance structures more accurately describes a particular molecule and helps us better understand the electronic nature of the compound of interest. Instead of just guessing what a resonance structure will look like, it is helpful to draw the arrows leading from one structure to the next. There are a few things you should keep in mind. There are two important "commandments" that you can never violate when pushing arrows. a Thou shall not break a single bond b. Thou shall not violate the octet rule.
Keith LeannonLv2
19 Feb 2019