Bonding and Structure Questions PDF

1. What type of bonding involves the transfer of electrons from a metal to a non-metal? * (A) Covalent * (B) Ionic * (C) Metallic * (D) Dative covalent 2. What type of bonding involves the sharing of a pair of electrons between two non-metal atoms? * (A) Covalent * (B) Ionic * (C) Metallic * (D) Da...

1. What type of bonding involves the transfer of electrons from a metal to a non-metal? * (A) Covalent * (B) Ionic * (C) Metallic * (D) Dative covalent 2. What type of bonding involves the sharing of a pair of electrons between two non-metal atoms? * (A) Covalent * (B) Ionic * (C) Metallic * (D) Dative Covalent 3. What is the electrostatic attraction in metallic bonding between? * (A) Positive ions and negative ions * (B) Positive ions and delocalized electrons * (C) Shared pairs of electrons and nuclei * (D) Atoms and delocalised electrons 4. What is a dative covalent bond? * (A) A bond formed by transferring electrons * (B) A bond where both electrons are donated from the same atom * (C) A bond between a metal and a non-metal * (D) A bond between positive and negative ions 5. Which of the following is NOT a giant lattice structure? * (A) Diamond * (B) Graphite * (C) Ice * (D) Sodium Chloride 6. Which of the following molecules contains polar bonds but is a non- polar molecule overall? * (A) H₂O * (B) NH₃ * (C) CCl₄ * (D) HCl 7. What is electronegativity? * (A) The ability of an atom to attract electrons in a covalent bond * (B) The ability of an atom to lose electrons * (C) The ability of an atom to form positive ions * (D) The charge on an ion 8. Which of the following is the most electronegative element? * (A) Chlorine * (B) Oxygen * (C) Fluorine * (D) Nitrogen 9. In a polar bond, the more electronegative atom will have a: * (A) δ+ charge * (B) δ- charge * (C) Full positive charge * (D) No charge 10. Which of the following types of intermolecular forces is the strongest? * (A) Van der Waals' forces * (B) Permanent dipole - permanent dipole * (C) Hydrogen bonding * (D) Ionic bonding 11. Hydrogen bonding occurs when hydrogen is bonded to which elements? * (A) N, O, F *(B) C, H, O * (C) Cl, Br, I * (D) Any electronegative element 12. What is the approximate bond angle in a tetrahedral molecule like methane (CH₄)? * (A) 90° *(B) 104.5° * (C) 109.5° *(D) 120° 13. What is the approximate bond angle in a water molecule (H₂O)? * (A) 104.5° * (B) 107° * (C) 109.5° * (D) 180° 14. What is the shape of an ammonia molecule (NH₃)? * (A) Linear * (B) Trigonal planar * (C) Trigonal pyramidal * (D) Tetrahedral 15. How many lone pairs of electrons are there on the central oxygen atom in a water molecule? * (A) 0 * (B) 1 * (C) 2 * (D) 3 16. What is the shape of a BF₃ molecule? * (A) Linear * (B) Trigonal pyramidal * (C) Trigonal planar *(D) Tetrahedral 17. How many bonding pairs of electrons are in a molecule of carbon dioxide? * (A) 1 *(B) 2 *(C) 3 *(D) 4 18. What is the shape of a molecule of carbon dioxide? * (A) Linear * (B) Bent * (C) Trigonal planar * (D) Tetrahedral 19. Why does diamond have a very high melting point? * (A) It has weak intermolecular forces. * (B) It has strong covalent bonds throughout the structure. * (C) It has delocalized electrons. *(D) It has ionic bonds 20. Why is graphite a good conductor of electricity? * (A) It has strong covalent bonds. * (B) It has layers that can slide over each other. * (C) It has delocalized electrons. * (D) It has a giant ionic structure. 21. Why can graphite be used as a lubricant? * (A) It has strong covalent bonds in each layer * (B) It has delocalised electrons * (C) It has weak forces between the layers * (D) It forms a giant covalent structure. 22. What type of structure does sodium chloride (NaCl) have? * (A) Simple molecular * (B) Giant ionic lattice * (C) Giant covalent *(D) Metallic 23. Why do ionic compounds have high melting and boiling points? * (A) They have weak intermolecular forces. * (B) They have strong electrostatic forces between oppositely charged ions. * (C) They have delocalized electrons. * (D) They have covalent bonds. 24. Why are metals good conductors of electricity? * (A) They have strong covalent bonds. * (B) They have delocalized electrons. * (C) They have a giant ionic structure. * (D) They have weak intermolecular forces. 25. Why are metals malleable? * (A) The layers of ions can slide over each other. * (B) They have strong covalent bonds. * (C) They have delocalized electrons. * (D) They have weak intermolecular forces. 26. In a covalent bond, the bond strength _______ as the bond gets shorter. * (A) increases * (B) decreases * (C) stays the same *(D) varies depending on the atoms 27. In a covalent bond, the bond strength _______ as the number of shared electrons increases. * (A) increases * (B) decreases * (C) stays the same * (D) varies depending on the atoms. 28. What is the approximate H-N-H bond angle in ammonia? * (A) 104.5 * (B) 107 * (C) 109.5 * (D) 120 29. What is the approximate F-B-F bond angle in boron tri uoride? * (A) 104.5 * (B) 109.5 * (C) 120 * (D) 180 30. Which intermolecular force exists between *all* molecules? * (A) Hydrogen bonding * (B) Permanent dipole-permanent dipole * (C) Van der Waals' forces * (D) Ionic Bonding fl