AI2CI6
CCI4
H3O+
NH + 4
Explanation
No explanation available
Video Explanation
No video available
Post your Contribution
Discussions (15)
CCl4 is a tetrahedral molecule in which each chlorine atom is covalently bonded to the central carbon atom through a single covalent bond. There are no lone pairs of electrons on the carbon or chlorine atoms, so there are no electrons available to form a coordinate bond.
In contrast, the other options contain coordinate bonds:
Al2Cl6 contains three coordinate bonds between the aluminum and chlorine atoms.
H3O+ contains one coordinate bond between the oxygen and hydrogen atoms.
NH4+ contains four coordinate bonds between the nitrogen and hydrogen atoms
Isn't Carbon tetrachloride ordinary covalent bonding
if so, then why is their answer CCl4
A coordinate bond (or dative covalent bond) is a type of covalent bond where one atom contributes both of the shared electrons to the bond.
Let's analyze each species:
* A. Al$_2Cl_6$: Aluminium chloride (AlCl$_3$) exists as a dimer, Al$_2Cl_6$, in the vapor phase and in non-polar solvents. In this dimer, two chlorine atoms act as bridging ligands, forming coordinate bonds by donating their lone pairs to the electron-deficient aluminum atoms. Each aluminum atom in AlCl$_3$ has only 6 valence electrons, making it a Lewis acid. When two AlCl$_3$ molecules dimerize, the chlorine atoms from one AlCl$_3$ donate lone pairs to the aluminum of the other, forming coordinate bonds to complete the octet around the aluminum atoms.
* B. CCl$_4$ (Carbon tetrachloride): In CCl$_4$, carbon is bonded to four chlorine atoms. Carbon has 4 valence electrons, and each chlorine atom has 7 valence electrons. Carbon forms four single covalent bonds with the four chlorine atoms to achieve a stable octet. All the bonds in CCl$_4$ are standard covalent bonds, where each atom contributes one electron to the shared pair. There are no lone pairs on the central carbon atom to donate, nor are there any atoms with vacant orbitals to accept a lone pair from carbon. Therefore, CCl$_4$ does not contain coordinate bonds.
* C. H$_3O^+$ (Hydronium ion): The hydronium ion is formed when a water molecule (H$_2O) accepts a proton (H^+).[span_9](end_span) [span_10](start_span)The oxygen atom in H_2O has two lone pairs of electrons.[span_10](end_span) When H^+$ (which has an empty 1s orbital) approaches, one of the lone pairs on the oxygen atom is donated to form a bond with the H$^+. This is a coordinate bond. Once formed, all three O-H bonds in H_3O^+$ become equivalent.
* D. NH$_4$$^+$ (Ammonium ion): The ammonium ion is formed when an ammonia molecule (NH$_3$) accepts a proton (H$^+). The nitrogen atom in NH_3$ has one lone pair of electrons. When H$^+$ approaches, this lone pair is donated to form a bond with the H$^+. This is a coordinate bond. Similar to H_3O^+, once formed, all four N-H bonds in NH_4$$^+$ become equivalent.
Therefore, the species that does not contain a coordinate bond is CCl$_4$.
The final answer is \boxed{B}
A coordinate (dative) bond is a type of covalent bond where both electrons come from one atom. Let's analyze the given options:
A. Al₂Cl₆ (Aluminum chloride dimer) → Contains a coordinate bond between aluminum and chlorine atoms. 
B. CCl₄ (Carbon tetrachloride) → Does not contain any coordinate bond; all bonds are normal covalent bonds. 
C. H₃O⁺ (Hydronium ion) → Contains a coordinate bond between oxygen and an extra hydrogen ion (H⁺).
D. NH₄⁺ (Ammonium ion) → Contains a coordinate bond where nitrogen donates a lone pair to bond with an H⁺ ion.
Answer: B. CCl₄ (Carbon tetrachloride does not contain a coordinate bond).
The correct answer is B. CCl
4
(Carbon tetrachloride).
Rationale
To identify which species lacks a co-ordinate (dative) bond, we look at how the atoms share electrons. A co-ordinate bond occurs when both electrons in the shared pair come from the same atom.
CCl
4
(Carbon Tetrachloride): Carbon has 4 valence electrons and forms 4 standard covalent bonds with 4 Chlorine atoms. Each atom (Carbon and Chlorine) contributes one electron to each bond. There is no need for a dative bond here.
Shutterstock
Explore
Al
2
Cl
6
(Aluminum Chloride Dimer): In its vapor phase, AlCl
3
molecules pair up. Two Chlorine atoms act as bridges by donating a lone pair of electrons to the empty p-orbitals of the Aluminum atoms, forming two co-ordinate bonds.
H
3
O
+
(Hydronium Ion): This is formed when a water molecule (H
2
O) reacts with a hydrogen ion (H
+
). The Oxygen atom in water provides both electrons from one of its lone pairs to bond with the electron-less H
+
ion.
NH
4
+
(Ammonium Ion): Similar to hydronium, ammonia (NH
3
) has a lone pair on the Nitrogen atom. It donates this lone pair to an H
+
ion to form a co-ordinate bond.
Summary Table
Species Type of Bonding
Al
2
Cl
6
Covalent and Co-ordinate
CCl
4
Purely Covalent
H
3
O
+
Covalent and Co-ordinate
NH
4
+
Covalent and Co-ordinate
Export to Sheets
A coordinate bond, also known as a dative covalent bond, occurs when one atom provides both electrons for the bond. Let's analyze each species to determine if it contains a coordinate bond:
A. Al₂Cl₆ (Aluminum chloride dimer): This molecule contains coordinate bonds. In the Al₂Cl₆ dimer, one aluminum atom donates a lone pair of electrons to form a bond with another aluminum atom.
B. CCl₄ (Carbon tetrachloride): This molecule does not contain any coordinate bonds. All bonds in CCl₄ are regular covalent bonds where each bond involves one electron from carbon and one electron from chlorine.
C. H₃O⁺ (Hydronium ion): This ion contains a coordinate bond. The oxygen atom in H₂O donates a lone pair of electrons to bond with a proton (H⁺) to form H₃O⁺.
D. NH₄⁺ (Ammonium ion): This ion contains a coordinate bond. The nitrogen atom in NH₃ donates a lone pair of electrons to bond with a proton (H⁺) to form NH₄⁺.
Thus, the species that does not contain a coordinate bond is:
B. CCl₄
