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Questions and Answers
In the following electron-dot structure, calculate the formal charge on each nitrogen atom from left to right.
In the following electron-dot structure, calculate the formal charge on each nitrogen atom from left to right.
- +1, -1, -1
- +1, -1, +1
- -1, -1, +1
- -1, +1, -1 (correct)
Which of the following is the correct electron dot structure of N2O molecule?
Which of the following is the correct electron dot structure of N2O molecule?
- : N̈ − N = Ö :
- : N ≡ N − Ö : (correct)
- : N̈ = N = Ö
- : N = N = Ö :
In which of the following molecules does the central atom have more than 8 electrons in the outermost orbit?
In which of the following molecules does the central atom have more than 8 electrons in the outermost orbit?
- All of these (correct)
- P2O5
- SO3
- SO2
Which one of the following elements will never obey the octet rule?
Which one of the following elements will never obey the octet rule?
The number of lone pairs present in N-atom in NF3 molecule is:
The number of lone pairs present in N-atom in NF3 molecule is:
Maximum number of bonds in:
Maximum number of bonds in:
Electron deficient species among the following is:
Electron deficient species among the following is:
In PO4^3− ion the formal charge on the oxygen atom of P − O bond is:
In PO4^3− ion the formal charge on the oxygen atom of P − O bond is:
Formal charge present on carbon atom in CO is:
Formal charge present on carbon atom in CO is:
Molecule which follows the octet rule is:
Molecule which follows the octet rule is:
The average formal charge on the oxygen atom in carbonate ion is:
The average formal charge on the oxygen atom in carbonate ion is:
In which of the following molecules does the central atom have less than 8 electrons in the outermost orbit?
In which of the following molecules does the central atom have less than 8 electrons in the outermost orbit?
Study Notes
Chemical Bonding and Molecular Structure
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Formal Charge calculation - The formal charge on an atom can be calculated using the following formula: Formal Charge = Valence Electrons - Non-bonding Electrons - (1/2) Bonding Electrons.
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Electron Dot Structures - The electron dot structure of a molecule shows the arrangement of valence electrons around each atom in the molecule.
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Octet Rule - Atoms tend to gain, lose, or share electrons to achieve a stable configuration with eight electrons in their outermost shell (valence shell). Except for elements in the second row of the periodic table (H, Li, Be, and boron family) can have less than eight electrons in their valence shell.
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Exception to Octet rule - Some elements, like sulfur and phosphorus, can have more than eight electrons in their valence shell because of the availability of d-orbitals.
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Lone pair of electrons - Lone pairs are valence electrons that are not involved in bonding.
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Electron deficient species - Species that do not have eight electrons in their valence shell, such as BH3, are electron deficient.
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Description
Test your understanding of chemical bonding concepts including formal charge calculation, electron dot structures, and the octet rule. This quiz will cover essential topics such as exceptions to the octet rule and the role of lone pairs of electrons in molecular structures.
