Tag: chemistry

Questions Related to chemistry

In which of the following molecules/ions are all the bonds not equal?

chemistry introduction to organic chemistry bonding in organic molecule tetravalence of carbon: shapes of organic compounds introduction to carbon and its compounds

  1. $BF _4^-$

  2. $SF _4$

  3. $SiF _4$

  4. $XeF _4$

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Correct Option: B

Strength of pi bonds are generally :

chemistry introduction to organic chemistry bonding in organic molecule tetravalence of carbon: shapes of organic compounds introduction to carbon and its compounds

  1. stronger than sigma bond

  2. weaker than sigma bond

  3. stronger than ionic bond

  4. weaker than hydrogen bond

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Correct Option: B
Explanation:

Strength of pi bond is weaker than sigma bond because it is formed due to lateral overlapping of atomic orbitals. 
Since, their is a sharing of electron between the two atoms, which is not in case of hydrogen bond, hence it is stronger than the hydrogen bond.
Ionic bonds are always stronger than the covalent bonds. Since, Pi bonds are covalent bonds hence, it is weaker than ionic bonds.

Pent -2-yne has how many $\sigma$ and $\pi$ bonds?

chemistry introduction to organic chemistry bonding in organic molecule tetravalence of carbon: shapes of organic compounds introduction to carbon and its compounds

  1. 10 $\sigma$, 2$\pi$

  2. 12 $\sigma$, 2$\pi$

  3. 15 $\sigma$, 2$\pi$

  4. 13 $\sigma$, 3$\pi$

Show answer
Correct Option: B
Explanation:

$CH _3-C\equiv C-CH _2-CH _3$
Pent-2-yne has 12$\sigma$ and 2$\pi$ bonds.
No. of $\sigma$ bonds = $C _1$ has 3 C-H bonds + $C _4$ has 2 C-H bonds + $C _5$ has 3 C-H bonds + 4 C-C bonds = 12$\sigma$ bonds.
No. of $\pi$ bonds = 2 bonds between $C _2$ and $C _3$.

The correct sequence of bond length in a single bond, a double bond and triple bond of $C$ is:

chemistry introduction to organic chemistry bonding in organic molecule tetravalence of carbon: shapes of organic compounds introduction to carbon and its compounds

  1. ${(C - C) = (C = C) = (C \equiv C)}$

  2. ${C \equiv C < C = C < C - C}$

  3. $C - C < C = C < C \equiv C$

  4. $C = C < C \equiv C < C - C$

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Correct Option: B
Explanation:

The bond length changes with the bond order like this:-

$Bond\ length\ \alpha \ \dfrac { 1 }{ Bond\ order } \ \alpha \ \dfrac { 1 }{ No.\ of\ bonds }$

As the number of bonds will increase, the bond order will increase and the bond length will decrease.
So, the correct option is $B$ 
${C \equiv C < C = C < C - C}$

$Mg _{2}C _{3}$ reacts with water forming propyne, $C _{2}^{4-}$ has

chemistry introduction to organic chemistry bonding in organic molecule tetravalence of carbon: shapes of organic compounds introduction to carbon and its compounds

  1. Two sigma and two pi bonds

  2. Three sigma and one pi bonds

  3. Two sigma and one pi bonds

  4. Two sigma and three pi bonds

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Correct Option: A

$\displaystyle:Mg _{2}C _{3}$ reacts with water forming propyne, $C _{3}^{4-}$ has:

chemistry introduction to organic chemistry bonding in organic molecule tetravalence of carbon: shapes of organic compounds introduction to carbon and its compounds

  1. two sigma and two pi bonds

  2. three sigma and one pi bonds

  3. two sigma and one pi bonds

  4. two sigma and three pi bonds

Show answer
Correct Option: A
Explanation:

Structure is: $^-C\equiv C-C^{-3}$
So it contains 2 sigma bond and 2 pi bonds.

Select correct statements about $C^{4-} _3$ ion.

chemistry introduction to organic chemistry bonding in organic molecule tetravalence of carbon: shapes of organic compounds introduction to carbon and its compounds

  1. It reacts with $H _2O$ forming $C _3H _6$.

  2. It reacts with $H _2O$ forming $C _3H _4$.

  3. It has two sigma and two pi bonds.

  4. It has three sigma and one pi bonds.

Show answer
Correct Option: B,C
Explanation:

The correct statements about $C^{4-} _3$ ion are

(B) It reacts with $H _2O$ forming $C _3H _4$

$\displaystyle  C^{4-} _3 + 2H _2O \rightarrow C _3H _4+O _2 + 4e^-$

(C) It has two sigma and two pi bonds $\displaystyle [C=C=C]^{4-} $

Which of the following molecule(s) has/have $d _n\, -\, p _{\pi}$ bonding?

chemistry introduction to organic chemistry bonding in organic molecule tetravalence of carbon: shapes of organic compounds introduction to carbon and its compounds

  1. $H _2S _2O _3$

  2. $P _4O _{10}$

  3. $SO _3$

  4. $P _4S _{10}$

Show answer
Correct Option: A,B,C,D
Explanation:

In ${ H } _{ 2 }{ S } _{ 2 }{ O } _{ 3 }$ $S$ empty $d$ orbital and $O$ has electrons in $P$ orbital.

Hence, it has ${ d } _{ n }$$-$${ P } _{ n }$ bonding.
In ${ P } _{ 4 }{ O } _{ 10 }$ $P$ have empty $d$ orbital and $O$ has electrons in $P$ orbital
Hence, it has ${ d } _{ n }$$-$${ P } _{ n }$ bonding.
In ${ SO } _{ 3 }$ $S$ have empty $d$ orbital and $O$ has electrons in $P$ orbital.
Hence, it has ${ d } _{ n }$$-$${ P } _{ n }$ orbital.
Similarly in ${ P } _{ 4 }{ S } _{ 10 }$

If "$n$" number of $H _3PO _4$ molecules are polymerized to produce chain molecule and ring molecule separately, then the number of $P - O - P$ linkages formed is, respectively :

chemistry introduction to organic chemistry bonding in organic molecule tetravalence of carbon: shapes of organic compounds introduction to carbon and its compounds

  1. $n$ and $(n - 1)$

  2. $(n - 1)$ and $(n - 1)$

  3. $(n - 1)$ and $n$

  4. $n$ and $n$

Show answer
Correct Option: C
Explanation:

In case of a ring, the number of linkages will be one less than the number of $P$ atoms because of the fact that each $P$ atom is shared by $2$ rings.
However, in case of a chain no sharing takes place and the number of linkages is equal to $n$.

In $Fe(CO) _5$, the $Fe-C$ bond possesses:

chemistry introduction to organic chemistry bonding in organic molecule tetravalence of carbon: shapes of organic compounds introduction to carbon and its compounds

  1. $\pi$ - character only

  2. both $\sigma$ and $\pi$ - characters

  3. ionic character

  4. $\sigma$ - character only

Show answer
Correct Option: B
Explanation:
It's called “synergic bonding”. The ligand (CO) donates it's lone pair of electrons to the vacant orbitals of the iron atom and forms the sigma-bond. Since the iron atom also possesses some electrons in it's d-orbitals, it back donates those electrons to the molecular orbitals of the ligand forming a π-bond. In this way, the metal-carbon bond length is reduced and the complex gets more stability. One important thing to keep in mind is that the metal atom donates it's electron pairs to the antibonding MO of CO, so the C-O bond is weakened by this synergic bonding, leading to a larger C-O bond length in the complex (as opposed to a free CO molecule).
Metal-C bond length reduces, C-O bond length increases, complex gets stability.
Hence, option $B$ is correct.