Draw Lewis structures for the following molecules and ions:...

Key Concepts

Polyatomic Ions

When drawing Lewis structures for polyatomic ions, it is important to adjust the total count of electrons to include the extra electrons gained or lost due to the ionic charge. This adjustment ensures that the structure accurately reflects the distribution of electrons, the resulting formal charges, and the overall ionic character of the species.

Resonance

Resonance refers to the situation in which more than one valid Lewis structure can represent the bonding in a molecule. These structures, known as resonance forms, differ only in the distribution of electrons. The actual electronic structure of the molecule is a hybrid of these forms, which can provide a better description of the electron delocalization within the molecule.

Formal Charge

Formal charge is a bookkeeping method for electrons in a Lewis structure that helps determine the most stable arrangement of electrons. It is calculated by comparing the number of valence electrons in the free atom with the number assigned to it in the molecule. Minimizing formal charges across atoms in a molecule generally leads to a more stable structure.

Octet Rule

The octet rule states that atoms tend to form structures in which they have eight electrons in their valence shell, achieving a stable electronic configuration similar to the noble gases. While this rule holds for many elements, it has exceptions such as in molecules with incomplete octets or atoms capable of an expanded valence shell.

Valence Electrons

Counting valence electrons is a crucial step in drawing Lewis structures. It involves summing the outer electrons of each atom based on the periodic table and adjusting for any ionic charges. This count is used to determine how electrons can be allocated to bonds and lone pairs, thereby ensuring the structure adheres to known bonding patterns.

Lewis Structures

Lewis structures are diagrams that depict the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule. They are fundamental tools in chemistry for visualizing molecular structure, predicting the shape of molecules, and understanding reactivity by showing how electrons are shared, transferred, or arranged around atoms.

Transcript

00:01 So lavish structures are the structures in which the atoms are shown bonded together by bonds and if we have any lone pair of electron any unbonded electron then we show that also okay so now in a part we have given of2 so the lavish structure will be like so whenever you are drawing the lavish structure you should make sure that the lavish electronegative atom should be in the center so this is oxygen as comparison to fluorine so being less electronegative it will have more tendency to share the electron okay so now that is bonded to two fluorine atoms so oxygen has six valence electron two of its electron are involved in bonding okay and rest are unbonded okay so these are the unbonded electron for oxygen and similarly for fluorine so they are from group 17 they have seven valence electron one of their electron are involved in bonding rest are unbonded okay so that is the structure we have now b part we have given n2 f2 so here we have nitrogen atom and nitrogen atom is pentavalent in nature so that has five valence electrons so what happen that they will be bond together by triple bond okay so now see what happen when that we have to bind here fluorine also okay so now if i bind fluorine and of course nitrogen and fluorine will share one their electron to form single bond so in this case we will have odd electron present on this nitrogen so this odd electron makes the compound unstable so that's why for this reason we can't afford this triple bond here so now let me draw this structure again so what if we have the nitrogen atom bonded together by double bond now this time what happened that nitrogen that has five valence electrons so two of its electron is involved in bonding and now one of its electron is involved in bonding with fluorine and now we have three electrons involved in bonding now and we have a pair of electron so now this pair of unbonded electron that is stable okay and this similarly this nitrogen so that has two electrons involved in double bond with another nitrogen and one electron to form single bond with fluorine now again so fluorine so that is from group 17 seven valence electron one electron is involved in bonding rest are unbonded so that is the structure okay now moving on to c part so we have si2h6 so we have silicon here so now silicon can bond with another silicon atom okay like carbon it can also possess some amount of some property of catenation and now silicon has four valence electrons so one electron is involved in bonding with…

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