This quiz works best with JavaScript enabled. Home > Cbse > Class 11 > Science > Chemistry Part I > Class 11 Chemistry (Part I) Chapter 4 Chemical Bonding And Molecular Structure – Quiz 2 🏠 Homepage 📘 Download PDF Books 📕 Premium PDF Books Class 11 Chemistry (Part I) Chapter 4 Chemical Bonding And Molecular Structure Quiz 2 (60 MCQs) Quiz Instructions Select an option to see the correct answer instantly. 1. Which of the following hybridisation leads to square planer geometry? A) Sp3d. B) Sp3. C) Dsp2. D) Sp3. Show Answer Correct Answer: C) Dsp2. 2. The elevtrovalence is thus ..... (a) ..... to the number of unit charge on ..... (b) ..... ? A) A:half ; b:stable atom. B) A:equal ; b:ion. C) A:equal ; b:anion. D) None of the above. Show Answer Correct Answer: B) A:equal ; b:ion. 3. A three-dimensional arrangement of particles in an ionic solid is called a(n): A) Electrolyte. B) Formula unit. C) Sea of electrons. D) Crystal lattice. Show Answer Correct Answer: D) Crystal lattice. 4. A lone pair is defined as A) A pair of electrons on the central atom. B) A pair of bonding electrons. C) One non-bonding electron. D) A pair of non-bonding electrons. Show Answer Correct Answer: D) A pair of non-bonding electrons. 5. Which type of bond is formed by an overlap of p orbitals? A) Pi. B) Sigma. C) Both. D) Neither. Show Answer Correct Answer: C) Both. 6. What is the electron configuration of sodium? A) 11. B) 2.8. C) 2.8.1. D) 2.8.2. Show Answer Correct Answer: C) 2.8.1. 7. If the boiling point of ethanol (molecular weight-46) is 78$^\circ$C. What is the boiling point of diethyl ether (molecular weight=74)? (2004-M) A) 78$^\circ$C. B) 100$^\circ$C. C) 34$^\circ$C. D) 86$^\circ$C. Show Answer Correct Answer: C) 34$^\circ$C. 8. Salts are examples of: A) Nonmetals. B) Metals. C) Ionic compounds. D) Nonionic compounds. Show Answer Correct Answer: C) Ionic compounds. 9. What is the geometry of a molecule in which the central atom has no lone pair and 3 bonding pairs? A) Bent. B) Tetrahedral. C) Trigonal Planar. D) Linear. Show Answer Correct Answer: C) Trigonal Planar. 10. Structural Formula A) A chemical formula that shows the arrangement of atoms in a molecule or a polyatomic ion. B) A property that describes the ability of the material to be pulled into thin wire without breaking. C) The arrangement of electrons in relation to the central atom of the molecule. D) The valence electrons in an atom that are bonded or shared with other atoms. Show Answer Correct Answer: A) A chemical formula that shows the arrangement of atoms in a molecule or a polyatomic ion. 11. In NO$_{3}$$^{-}$ ion, the number of bond pairs and lone pairs of electrons on nitrogen atom are A) 4, 0. B) 3, 3. C) 2, 2. D) 1, 3. Show Answer Correct Answer: A) 4, 0. 12. What is the concept that atoms combine either by transfer of valence electrons or by sharing of valence electrons to have an octet in their valence shells? A) Molecular Orbital Theory. B) Lewis Structure. C) Octet Rule. D) Hybridization. Show Answer Correct Answer: C) Octet Rule. 13. What is the primary characteristic of an ionic bond? A) Attraction of atoms for electrons they share. B) A force that holds together atoms of the same charge. C) A force that holds together atoms that are oppositely charged. D) Attraction of an atom for its electrons. Show Answer Correct Answer: C) A force that holds together atoms that are oppositely charged. 14. Which of the following species has tetrahedral geometry? A) NH$_{2}$$^{-}$. B) BH$_{4}$$^{-}$. C) CO$_{3}$$^{2-}$. D) H$_{3}$O$^{+}$. Show Answer Correct Answer: B) BH$_{4}$$^{-}$. 15. What is the attractive force that holds atoms together in a molecule called? A) Hydrogen bond. B) Chemical bond. C) Ionic bond. D) Covalent bond. Show Answer Correct Answer: B) Chemical bond. 16. What is the shape of PF$_{5}$? A) Trigonal pyramidal. B) Square planar. C) T-shape. D) Trigonal bipyramidal. Show Answer Correct Answer: D) Trigonal bipyramidal. 17. Each atom will achieve a geometry that minimizes the repulsion between electrons A) Double bond. B) VSEPR Theory. C) Molecular formula. D) Single bond. Show Answer Correct Answer: B) VSEPR Theory. 18. What is the bond angle in a tetrahedral molecule like CH4? A) 90$^\circ$. B) 120$^\circ$. C) 180$^\circ$. D) 109.5$^\circ$. Show Answer Correct Answer: D) 109.5$^\circ$. 19. Ionization occurs when valence electrons are transferred between atoms until they reach the electron configuration of a noble gas. Writing the formula for the ionic compound therefore involves balancing the total number of positive and negative charges, taking into account the different charges on each ion. Using this knowledge, find out the product of Mg and F. A) Mg$_{2}$F$_{2}$. B) Mg$_{2}$F. C) MgF. D) MgF$_{2}$. Show Answer Correct Answer: D) MgF$_{2}$. 20. Is luster a characteristic of most metals? If yes, explain how metallic bonding accounts for this property. A) No, because metals absorb light. B) No, because metals are opaque. C) Yes, because delocalized electrons reflect light. D) Yes, because metals are transparent. Show Answer Correct Answer: C) Yes, because delocalized electrons reflect light. 21. Is ductility a characteristic of most metals? If yes, explain how metallic bonding accounts for this property. A) Yes, because metallic bonds allow atoms to slide past each other. B) No, because metallic bonds are rigid. C) Yes, because metallic bonds are ionic. D) No, because metallic bonds are covalent. Show Answer Correct Answer: A) Yes, because metallic bonds allow atoms to slide past each other. 22. What does the Valence Bond Theory explain? A) The shapes of polyatomic molecules. B) The formation of chemical bonds based on atomic orbitals, electronic configurations, and overlap criteria. C) The shapes of simple molecules based on lone pairs and bonding pairs. D) The energy released when a bond is formed between two atoms. Show Answer Correct Answer: B) The formation of chemical bonds based on atomic orbitals, electronic configurations, and overlap criteria. 23. What is the term used to describe the energy required to completely separate one mole of a solid ionic compound into gaseous constituent ions? A) Bond Energy. B) Electron Affinity. C) Lattice Energy. D) Ionization Energy. Show Answer Correct Answer: C) Lattice Energy. 24. The geometry of a molecule with 3 bonded pairs of electrons and 1 lone pair of electrons A) Linear. B) Trigonal Planar. C) Bent. D) Tetrahedral. E) Trigonal Pyramidal. Show Answer Correct Answer: E) Trigonal Pyramidal. 25. A covalent bond is A) A bond that shares electrons metallicaly. B) A bond that shares electrons with non metals. C) Metalloids bonding. D) Metals and nonmetals bonding. Show Answer Correct Answer: B) A bond that shares electrons with non metals. 26. An ionic bond results from electrical attraction between A) Cations and anions. B) Atoms. C) Dipoles. D) Orbital. Show Answer Correct Answer: A) Cations and anions. 27. How many electrons are involved in a double bond? A) 8. B) 2. C) 6. D) 4. Show Answer Correct Answer: D) 4. 28. Which of the following statements about bond angles is true? A) They are the same for all molecules. B) They cannot be measured experimentally. C) They are determined by the arrangement of orbitals around the central atom. D) They are always 90 degrees. Show Answer Correct Answer: C) They are determined by the arrangement of orbitals around the central atom. 29. Hybridization of Central carbon in the following molecule isH$_{3}$C-CH = C = CH-CH$_{3}$ A) Sp$^{2}$. B) Sp$^{3}$. C) Sp. D) None of the above. Show Answer Correct Answer: A) Sp$^{2}$. 30. What is the main postulate of the Valence Shell Electron Pair Repulsion (VSEPR) theory? A) The shape of a molecule depends upon the number of protons in the nucleus. B) The shape of a molecule depends upon the number of lone pairs around the central atom. C) The shape of a molecule depends upon the number of bonding pairs around the central atom. D) The shape of a molecule depends upon the number of valence shell electron pairs around the central atom. Show Answer Correct Answer: D) The shape of a molecule depends upon the number of valence shell electron pairs around the central atom. 31. Which of the following is an example of a molecule with an odd number of electrons? A) Nitric oxide. B) Carbon dioxide. C) Methane. D) Ozone. Show Answer Correct Answer: A) Nitric oxide. 32. State whether the given statement is true or false "Ionic bonds are non-directional" . A) True. B) False. C) All the above. D) None of the above. Show Answer Correct Answer: A) True. 33. What type of overlap occurs in the formation of a pi bond? A) No overlap. B) Sidewise overlap. C) End-to-end overlap. D) Complete overlap. Show Answer Correct Answer: B) Sidewise overlap. 34. What is the crystal structure of Cesium Chloride? (2000 E) A) Octahedral. B) Face centered cubic. C) Tetrahedral. D) Body centered cubic. Show Answer Correct Answer: D) Body centered cubic. 35. The negative and positive ions are stabilised by ..... A) Electrostatic attraction. B) Electrostatic repulsion. C) Chemical bonds. D) None of the above. Show Answer Correct Answer: A) Electrostatic attraction. 36. The molecular formula of the compound formed from B and C will be A) BC. B) B$_{2}$C. C) BC$_{2}$. D) BC$_{3}$. Show Answer Correct Answer: D) BC$_{3}$. 37. Which of the following element neither looses nor gains electrons? A) Carbon. B) Chlorine. C) Sodium. D) Nitrogen. Show Answer Correct Answer: A) Carbon. 38. An ionic bond forms when atoms ..... electrons. A) Share. B) Transfer. C) Increase. D) Gain. Show Answer Correct Answer: B) Transfer. 39. How do the metallic ions differ from the ions that exist in ionic solids? A) Metallic ions are surrounded by delocalized electrons, while ionic solid ions are not. B) Metallic ions are neutral, while ionic solid ions are charged. C) Metallic ions are smaller than ionic solid ions. D) Metallic ions are bonded covalently, while ionic solid ions are bonded ionically. Show Answer Correct Answer: A) Metallic ions are surrounded by delocalized electrons, while ionic solid ions are not. 40. In periodic table, the highly electronegative halogens and the highly electropositive alkali metals are separated by ..... A) Actinoids and lanthanides. B) Noble gases. C) D-block elements. D) None of the above. Show Answer Correct Answer: B) Noble gases. 41. What is the term for the bond formed due to the electrostatic attraction between positive and negative ions? A) Hydrogen bond. B) Covalent bond. C) Ionic bond. D) Metallic bond. Show Answer Correct Answer: C) Ionic bond. 42. Calculate the total no of sigma and pi bonds in-CH3-CH2-CH=CH-CHO A) Sigma= 12, pi=1. B) Sigma=13, pi=2. C) Sigma=13, pi=1. D) None of the above. Show Answer Correct Answer: B) Sigma=13, pi=2. 43. The overall charge of a formula unit for an ionic compound: A) Is always positive. B) Is always zero. C) May have any value. D) Is always negative. Show Answer Correct Answer: B) Is always zero. 44. The bond energies (in KJmol-1) of P-H, As-H and N-H respectively are (2002-E) A) 247, 318 and 389. B) 247, 389 and 318. C) 318, 389 and 247. D) 318, 247 and 389. Show Answer Correct Answer: D) 318, 247 and 389. 45. Which of the following is correct pair? (2000 E) A) BF3, octahedral. B) NH3, linear. C) BeCl2, linear. D) CO2, tetrahedral. Show Answer Correct Answer: C) BeCl2, linear. 46. Is low boiling point a characteristic of most metals? If yes, explain how metallic bonding accounts for this property. A) Yes, because metallic bonds are weak. B) No, because metallic bonds are strong. C) Yes, because metallic bonds are ionic. D) No, because metallic bonds are covalent. Show Answer Correct Answer: B) No, because metallic bonds are strong. 47. Why NH3 has distorted shape? Choose the most appropriate option: A) Because nitrogen makes three bonds only. B) Because of presence of lone pair. C) None of the above. D) None of the above. Show Answer Correct Answer: B) Because of presence of lone pair. 48. Hybrid orbitals are more stable bond than atomic orbitals A) True. B) False. C) All the above. D) None of the above. Show Answer Correct Answer: A) True. 49. The types of hybrid orbitals of nitrogen in NO2$^{+}$, NO3$^{-}$ and NH4$^{+ respectively are expected to be }$ A) Sp2, sp3, Sp. B) Sp3, Sp, sp2. C) Sp, Sp2, Sp3. D) Sp, Sp3, Sp2. Show Answer Correct Answer: C) Sp, Sp2, Sp3. 50. What is the shape of the H2O molecule? A) Linear. B) Trigonal Planar. C) Bent. D) Tetrahedral. Show Answer Correct Answer: C) Bent. 51. Molecular Geometry A) A property that describes the ability of a material to be permanently reshaped without breaking or cracking. B) The arrangement of electrons in relation to the central atom of the molecule. C) The angle that is formed between adjacent bonds on the same atom. D) The valence electrons in an atom that are bonded or shared with other atoms. Show Answer Correct Answer: B) The arrangement of electrons in relation to the central atom of the molecule. 52. Which among the following is diamagnetic? A) N2. B) N2$^{2-}$. C) O2$^{-}$. D) O2. Show Answer Correct Answer: A) N2. 53. What is the VSEPR theory used to predict? A) Molecular Shape. B) Bond Strength. C) Electronegativity. D) Polarity. Show Answer Correct Answer: A) Molecular Shape. 54. What is the shape of a molecule with four bonding pairs and no lone pairs? A) Linear. B) Octahedral. C) Trigonal planar. D) Tetrahedral. Show Answer Correct Answer: D) Tetrahedral. 55. In nitrogen molecule, number of electrons shared by each nitrogen are A) 2. B) 3. C) 4. D) None of the above. Show Answer Correct Answer: B) 3. 56. In electron transfer involving a metallic atom and a nonmetallic atom during ion formation, which of the following is correct? A) The metallic atom gains electrons from the nonmetallic atom. B) The nonmetallic atom gains electrons from the metallic atom. C) Both atoms gain electrons. D) Neither atom gains electrons. Show Answer Correct Answer: B) The nonmetallic atom gains electrons from the metallic atom. 57. H-O-H bond angle is H2O is 104.5$^\circ$ and not 109$^\circ$28 because of A) Bond pair-bond pair repulsion. B) Lone pair-lone pair repulsion. C) High electronegativity of oxygen. D) Lone pair-bond pair repulsion. Show Answer Correct Answer: B) Lone pair-lone pair repulsion. 58. Why are the electrons in a metallic solid described as delocalized? A) They are bound to individual atoms. B) They are free to move throughout the entire solid. C) They are fixed in place within the metal lattice. D) They are shared between two specific atoms. Show Answer Correct Answer: B) They are free to move throughout the entire solid. 59. What is the primary reason for the formation of a covalent bond? A) Transfer of electrons. B) Sharing of electrons. C) Repulsion between electrons. D) Attraction between ions. Show Answer Correct Answer: B) Sharing of electrons. 60. The maximum number of hydrogen bond that a water molecule can have are A) 1. B) 3. C) 2. D) 4. 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