Part B How many bonding electrons are in the structure? Express your answer as an integer. ΑΣφ electrons Submit Request Answer Part C Would you expect the O-O bond in O2 to be shorter or longer than the O O bond in compounds that contain an O O single bond? Explain. Check all that apply. U As O2 has two bonding electron pairs, the O-O distance will be shorter than the O O single bond distance. O The greater the number of shared electron pairs between two atoms, the shorter the distance between the atoms. O As O2 has two bonding electron pairs, the O-O distance will be longer than the 0-O single bond distance. O The greater the number of shared electron pairs between two atoms, the longer the distance between the atoms. Submit Request Answer amazon Formal. B. P Type here to search 立
Formal Charges
Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be neutral atoms.
Polarity Of Water
In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in the electronegativities of the bonded atoms. Water, as we all know has two hydrogen atoms bonded to an oxygen atom. As oxygen is more electronegative than hydrogen thus, there exists polarity in the bonds which is why water is known as a polar solvent.
Valence Bond Theory Vbt
Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the formation of covalent bonds with the help of wavefunctions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.
![Construct a Lewis structure for O, in which each atom achieves an octet of electrons.
Draw the Lewis dot structure for O2. Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all lone pairs of electrons.
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