Use valence bond theory to write a hybridization and bonding scheme for CO2. Match the words…
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Question “Use valence bond theory to write a hybridization and bonding scheme for CO2. Match the words…”
Use valence bond theory to write a hybridization and bonding
scheme for CO2.
Match the words in the left column to the appropriate blanks in
the sentences on the right. Make certain each sentence is complete
before submitting your answer.
you can only use the following words:
two C(s)-O(s) ; two C(p)-O(p) ; trigonal planar ; two
O(sp2)-C(sp) ; two O(sp)-C(sp2) ; carbon and oxygen ; sp2 ; a
single and a double bond ; oxygen ; two single bonds ; linear ;
tetrahydral ; carbon ; sp ; two double bonds ; sp3
Answer
Valence Bond Theory
The Valence Bond Theory describes covalent bonds between two atoms, and how they form. It assumes that all covalent bond formations are localized.
Hybridization:
Hybridization can be defined as the combination of different atomic orbitals in order to create a new hybrid orbital.
This is the idea of mixing atomic orbitals with different shapes and energies to create equal numbers of hybrid orbitals (to the number of mixed orbitals), that have the same shape and energy. This concept can explain molecular geometry, bond angles and molecular structure for molecules.
Theory of VSEPR
The Valance Shell Elektron Pair Repulsion Theory, (VSEPR), states that molecular geometry can change due to repulsions between the single pair of electrons and bonded pairs of electrons in the molecule.
You can count the number of groups around the central atom to determine if there has been hybridization.
Groups surround by the central atom | Hybridization | Molecular geometry |
2 | linear | |
3 | Trigonal planar | |
4 | tetrahedral | |
5 | Trigonal bipyramidal |
An electron pair is also known as a group.
The VSEPR theory states that molecular geometry can change because of the presence of repulsions among bonded pairs and lone electrons. They are as follows.
Carbon is the central atom.
Oxygen is the surrounding atoms.
It has a linear structure.
Carbon contains two sp hybridized orbitals, and two p-atomic orbitals.
Three sp 2 hybridized orbitals for oxygen and one p orbital for oxygen are available.
Ans:
structure has a central atom.
Attached to oxygen atoms via two triple bonds.
2. Carbon dioxide has a carbon geometry.
hybridized.
4. Carbon dioxide is available in two C(p-O)(p),
bonds, and two O (p)-C(sp),
bonds.
Conclusion
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