There are different types of bonds based on electronegativity. One bond type is known as non-polar covalent. Which choice below
has this bond type? A. all of the compounds B. H2 C. H2O D. NaCl
2 answers:
Answer:
H₂ has a non-polar covalent bond.
Explanation:
First, remember that a covalent bond occurs when two atoms with zero or very low difference of electronegativity share one or more pair of electrons, that's why <u>covalent bonds are very common between atoms of the same elements</u>, for example in the case of H₂, where the difference of electronegativity is zero.
Also, covalent bonds are non-polar when the atoms in the bond has the same electronegativity so the electronic density is symmetric distributed.
The molecule that has those characteristics is the molecule of Hydrogen (H₂) so it has a non-polar covalent bond.
On the other side, the molecule of water (H₂O) has covalent bond between hydrogen and oxygen atoms but the oxigen atom has 2 pairs of non bonded electrons that creates a zone with high electronic density making this molecule polar (you can see those pair of non bonded electrons in red in the attachment).
Finally, the molecule of chloride sodium (NaCl) is a type of ionic bond.
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Answer:
Canonical structures of a chemical specie explain its observed properties from a valence bond theory perspective.
Explanation:
Resonance is a valence bond concept introduced by Linus Pauling to explain the observed properties of certain chemical species such as bond lengths, bond angles, bond order , etc.
There are certain chemical species for which a single chemical structure does not suffice in explaining its observed properties. For instance, the bond order in CO3^2- is about 1.33. Its bond length, shows that the C-O bond present in CO3^2- is neither a pure C-O single bond nor a pure C-O double bond. Hence the structure of CO3^2- is 'somewhere in between' three contributing canonical structures as shown in the image attached to this answer. The resonance structures of NO3^- are also shown.
