Problem 166
Question
Match the following \begin{tabular}{ll} \hline Column-I & Column-II \\ \hline (a) Electrovalent bond & (p) \(\mathrm{NH}_{4} \mathrm{Cl}\) \\ (b) Covalent bond & (q) \(\mathrm{CaOCl}_{2}\) \\ (c) Co-ordinate bond & (r) \(\mathrm{KHF}_{2}\) \\ (d) Hydrogen bond & (s) \(\mathrm{N}_{2} \mathrm{O}_{5}\) \\ & (t) \(\mathrm{CuSO}_{4} .5 \mathrm{H}_{2} \mathrm{O}\) \\ \hline \end{tabular}
Step-by-Step Solution
Verified Answer
(a) - (p), (b) - (s), (c) - (q), (d) - (r)
1Step 1: Identify Electrovalent Bond
An electrovalent bond, also known as an ionic bond, is formed between two atoms when one atom transfers electrons to another, creating ions that attract each other. Typically, these are seen in compounds formed between metals and non-metals. In Column-II, only (
p
)
NH
4
Cl
involves an ionic interaction between
NH
4
+
and
Cl
-
ions, although it also has covalent and coordinate components. Hence, we will match (a) Electrovalent bond with (p)
NH
4
Cl
.
2Step 2: Identify Covalent Bond
A covalent bond is formed when two atoms share a pair of electrons. Molecules like
N
2
O
5
consist primarily of covalent bonds between nitrogen and oxygen atoms. Therefore, we match (b) Covalent bond with (s)
N
2
O
5
.
3Step 3: Identify Co-ordinate Bond
A co-ordinate bond is a type of covalent bond where both electrons in the bond are donated by one atom.
NH
4
Cl
has a co-ordinate bond between
NH
3
(ammonia) and
H
+
to form
NH
4
+
. After taking initial electrovalent bond logic into context,
CaOCl
2
(calcium oxychloride) also shows coordination bond due to its structure. Thus, we match (c) Co-ordinate bond with (q)
CaOCl
2
.
4Step 4: Identify Hydrogen Bond
Hydrogen bonds occur when there is a bond involving a hydrogen atom that is weakly attracted to an electronegative atom like oxygen or fluorine from another molecule. In Column II,
KHF
2
has hydrogen bonding due to the presence of
F-H
attraction. Thus, (d) Hydrogen bond matches with (r)
KHF
2
.
Key Concepts
Electrovalent bondCovalent bondCo-ordinate bondHydrogen bond
Electrovalent bond
An electrovalent bond, often referred to as an ionic bond, is a type of chemical bond where one atom donates one or more of its electrons to another atom. This results in the formation of two ions: one with a positive charge (cation) and one with a negative charge (anion). The electrostatic attraction between these oppositely charged ions holds them together. This bond is typically observed in compounds formed between metals and non-metals.
In the case of NH 4 Cl, this compound primarily exhibits ionic interaction. The ammonium ion ( NH 4 + ) and chloride ion ( Cl - ) are held together by this kind of bond. Although NH 4 Cl also includes covalent and co-ordinate bonds, the electrovalent interaction between NH 4 + and Cl - is a defining feature. This characteristic makes NH 4 Cl a classic example when studying electrovalent bonds in chemistry.
In the case of NH 4 Cl, this compound primarily exhibits ionic interaction. The ammonium ion ( NH 4 + ) and chloride ion ( Cl - ) are held together by this kind of bond. Although NH 4 Cl also includes covalent and co-ordinate bonds, the electrovalent interaction between NH 4 + and Cl - is a defining feature. This characteristic makes NH 4 Cl a classic example when studying electrovalent bonds in chemistry.
- Occurs between metals and non-metals.
- Involves the transfer of electrons.
- Forms positive and negative ions.
Covalent bond
A covalent bond is established when two atoms share one or more pairs of electrons. This sharing allows each atom to attain the electron configuration of the nearest noble gas, providing stability to the molecule. Covalent bonds are common in organic compounds and are primarily observed among non-metal atoms.
In molecules such as N 2 O 5, covalent bonds form between nitrogen and oxygen atoms. These bonds are responsible for holding the molecule together by sharing electron pairs among the atoms, resulting in mutual adherence by these non-metallic elements. Understanding covalent bonds is crucial for comprehending how complex organic and inorganic compounds are structured.
In molecules such as N 2 O 5, covalent bonds form between nitrogen and oxygen atoms. These bonds are responsible for holding the molecule together by sharing electron pairs among the atoms, resulting in mutual adherence by these non-metallic elements. Understanding covalent bonds is crucial for comprehending how complex organic and inorganic compounds are structured.
- Involves sharing of electron pairs.
- Commonly found between non-metal atoms.
- Provides molecular stability.
Co-ordinate bond
A co-ordinate bond, also known as a dative covalent bond, occurs when one atom provides both electrons required to form a bond with another atom. This kind of bond is often seen when a molecule with a lone electron pair donates electrons to an electron-deficient atom or ion.
In the scenario of NH 4 Cl, the nitrogen atom in ammonia ( NH 3) which has a lone pair of electrons, donates an electron pair to the hydrogen ion ( H + ), forming the ammonium ion ( NH 4 + ). Additionally, compounds like CaOCl 2 also demonstrate co-ordinate bonding, due to electron rich components binding with hydrogen ions. These bonds provide significant insight into molecular formation beyond simple shared electron bonds.
In the scenario of NH 4 Cl, the nitrogen atom in ammonia ( NH 3) which has a lone pair of electrons, donates an electron pair to the hydrogen ion ( H + ), forming the ammonium ion ( NH 4 + ). Additionally, compounds like CaOCl 2 also demonstrate co-ordinate bonding, due to electron rich components binding with hydrogen ions. These bonds provide significant insight into molecular formation beyond simple shared electron bonds.
- Occurs with the donation of a lone electron pair.
- Crucial in complex formation.
- Seen often with metal complexes and ligands.
Hydrogen bond
Hydrogen bonds form when a hydrogen atom that is already covalently bonded to a highly electronegative atom like nitrogen, oxygen, or fluorine, exhibits an attraction towards another electronegative atom. This type of bond is relatively weak compared to covalent and ionic bonds but plays a significant role in determining the properties of substances.
In compounds such as KHF 2, hydrogen bonds are observed due to the F-H interaction. The electronegative fluorine atom attracts the hydrogen atom from another molecule, contributing to the overall structure and stability. Hydrogen bonds are vital in biological systems, affecting the structure and behavior of biomolecules like DNA and proteins.
In compounds such as KHF 2, hydrogen bonds are observed due to the F-H interaction. The electronegative fluorine atom attracts the hydrogen atom from another molecule, contributing to the overall structure and stability. Hydrogen bonds are vital in biological systems, affecting the structure and behavior of biomolecules like DNA and proteins.
- Occurs due to attraction between H and a nearby electronegative element.
- Not as strong as covalent or ionic bonds, but crucial for biological molecules.
- Influences properties like boiling and melting points.
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