Here below some basic MCQ’s about “Coordination compound” which is well explained for exam practice. Let’s check one by one.
1. Which of the following is the correct IUPAC name for the compound CH3CH2CH2OH?
a) Propanol
b) Ethanol
c) Butanol
d) Methanol
Answer: a) Propanol
Explanation: The compound has three carbon atoms and an alcohol group (-OH). According to IUPAC nomenclature, the parent chain is propane, and the suffix “ol” is added to indicate the presence of the -OH group. Thus, the name is propanol.
2. Which of the following compounds exhibits hydrogen bonding?
a) CH4
b) HCl
c) H2O
d) CCl4
Answer: c) H2O
Explanation: Water (H2O) can form hydrogen bonds due to the highly electronegative oxygen atom and the presence of hydrogen atoms. Hydrogen bonds occur when hydrogen is attached to highly electronegative atoms like oxygen, nitrogen, or fluorine.
3. What is the hybridization of carbon in methane (CH4)?
a) sp
b) sp2
c) sp3
d) dsp3
Answer: c) sp3
Explanation: In methane (CH4), the central carbon atom forms four single bonds with hydrogen atoms. To accommodate these four bonds, carbon undergoes sp3 hybridization, where one s orbital and three p orbitals combine to form four equivalent sp3 hybrid orbitals.
4. Which of the following molecules has a trigonal planar structure?
a) BF3
b) CH4
c) NH3
d) H2O
Answer: a) BF3
Explanation: Boron trifluoride (BF3) has three bonding pairs of electrons around the central boron atom, which results in a trigonal planar structure with a bond angle of 120°. There are no lone pairs on the boron atom, making the geometry trigonal planar.
5. What type of bonding is present in sodium chloride (NaCl)?
a) Covalent bond
b) Ionic bond
c) Metallic bond
d) Coordinate bond
Answer: b) Ionic bond
Explanation: Sodium (Na) donates one electron to chlorine (Cl) to form Na+ and Cl− ions, which are held together by electrostatic forces of attraction. This type of bond is called an ionic bond.
6. Which of the following compounds has a bent or V-shaped molecular geometry?
a) CO2
b) H2O
c) BeCl2
d) BF3
Answer: b) H2O
Explanation: Water (H2O) has two lone pairs of electrons on the oxygen atom and two bond pairs. The repulsion between the lone pairs causes the bond angle to reduce, giving the molecule a bent or V-shaped geometry with a bond angle of approximately 104.5°.
7. Which type of hybridization is present in ethylene (C2H4)?
a) sp
b) sp2
c) sp3
d) sp3d
Answer: b) sp2
Explanation: In ethylene (C2H4), each carbon atom forms three sigma bonds (two with hydrogen and one with the other carbon atom). The carbon atoms are sp2 hybridized, where one s orbital and two p orbitals mix to form three sp2 hybrid orbitals, leaving one unhybridized p orbital that forms a π bond.
8. Which of the following is an example of a polar covalent bond?
a) H-H
b) O=O
c) H-F
d) Cl-Cl
Answer: c) H-F
Explanation: In the H-F molecule, fluorine is much more electronegative than hydrogen, causing a significant difference in electronegativity. As a result, the electron pair is shared unequally, creating a polar covalent bond.
9. Which bond angle is closest to that found in a molecule with tetrahedral geometry?
a) 90°
b) 109.5°
c) 120°
d) 180°
Answer: b) 109.5°
Explanation: A tetrahedral molecule, like methane (CH4), has four bonding pairs of electrons that are equally spaced around the central atom. The bond angle between these bonds is 109.5°.
10. Which of the following molecules has a dipole moment?
a) CO2
b) CH4
c) NH3
d) BF3
Answer: c) NH3
Explanation: Ammonia (NH3) has a trigonal pyramidal structure with a lone pair of electrons on nitrogen. Due to this asymmetric distribution of electrons, NH3 has a net dipole moment. The lone pair-bond pair repulsion gives the molecule polarity.
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