Topic 4: Bonding
(Questions first, answers follow)
1. Define ionic bonding
2. Are ionic compounds molecules?
3. Are ionic bonds uni-directional?
4. How is an ionic compound structured?
5. How do electronegativity values relate to ionic compounds?
6. What are the physical properties of ionic compounds?
7. What do melting points of ionic compounds depend on?
8. How do ionic compounds dissolve in water?
9. Define covalent bonds
10. List covalent bonds in order of increasing strength
11. What is a coordinate bond?
12. Relationship between bond length and strength?
13. How do you determine bond polarity?
14. Is polarity permanent or temporary for covalent bonds?
15. How to draw Lewis structures?
16. What are some exceptions to the octet rule?
17. What are resonance structures? Examples?
18. List types of covalent structures
19. Name + Explain the giant covalent structures
20. Key ideas of VSEPR theory?
21. Distinction between electron domain geometry and molecular geometry?
22. List EDG names and MG names for different numbers of electron domains w and w/o
lone pairs (state their bond angle too)
23. Difference between bond polarity and molecular polarity?
24. How can you determine net dipole moment?
25. Is the C-H bond polar?
26. Name types of intermolecular forces (+ define intermolecular forces)
27. Explain London/dispersion forces (where are they found, how do they work)
28. What factors affect the magnitude of London forces?
29. Explain dipole-dipole forces
30. How do you determine what type of intermolecular forces are present?
31. Explain hydrogen bonding
32. Do hydrogen bonds occur in H-F?
33. List intermolecular forces in order of increasing strength
34. Relationship between solubility and intermolecular forces?
35. Define metallic bonds
36. Structure of metallic compounds?
37. What factors do the strength of metallic bonds depend on?
38. Define alloys and explain their properties
39. Properties of metals?
40. Why is the rearrangement of the shape of a metal possible?
41. Trends in melting points of metals?
, 42. Define ionic bonding
a. Electrostatic attraction between oppositely charged ions (positive and
negative ions)
43. Are ionic compounds molecules?
a. No
44. Are ionic bonds uni-directional?
a. No: all ions are bonded ionically to others
45. How is an ionic compound structured?
a. In giant regular lattices (to maximise attraction and minimise repulsion
between oppositely charged and like charged ions) [repeating units of cations
and anions, 3D]
46. How do electronegativity values relate to ionic compounds?
a. If the difference is greater than 1.8, it is ionic
47. What are the physical properties of ionic compounds?
a. Does not conduct electricity when solid: only when molten or in aqueous
solution
b. High melting and boiling points (because strong electrostatic forces of
attraction between ions in lattice structure, lots of energy needed to
overcome)
48. What do melting points of ionic compounds depend on?
a. Strength of electrostatic attraction between the oppositely charged ions (this
statement should be in your answer -> explain why a certain factor
increases / decreases strength of electrostatic attraction, hence MP is higher /
lower)
i. Ionic radius (smaller the radius the stronger the connection),
electronegativity, ionic charge (greater the charge, stronger the
attraction, higher the melting point), low volatility (because strong
electrostatic forces), solubility (dissolves in water + other polar
solvents), brittle (breaks easily because lattice structures repel)
49. How do ionic compounds dissolve in water?
a. H+ and OH- in water bond interact with oppositely charged ions in the ionic
compound (and overcome electrostatic attractions between ions in the lattice
structure by pulling out individual ions from lattice)
50. Define covalent bonds
a. Electrostatic attraction between a shared pair of electrons and the positively
charged nucleus of the atom/molecule
51. List covalent bonds in order of increasing strength
a. Single bond, double bond, triple bond (because increasing pair of electrons
shared)
52. What is a coordinate bond?
a. Also known as dative covalent bond; where one atom provides both shared
electrons
53. Relationship between bond length and strength?
a. Increase in bond length (distance between two covalently bonded nuclei) =
decrease in bond strength
i. Because as number of shared electrons increases, the length
decreases (as there is a stronger attraction)
54. How do you determine bond polarity?
a. Electronegativity values (ability of an atom to attract shared electrons in a
covalent bond)
(Questions first, answers follow)
1. Define ionic bonding
2. Are ionic compounds molecules?
3. Are ionic bonds uni-directional?
4. How is an ionic compound structured?
5. How do electronegativity values relate to ionic compounds?
6. What are the physical properties of ionic compounds?
7. What do melting points of ionic compounds depend on?
8. How do ionic compounds dissolve in water?
9. Define covalent bonds
10. List covalent bonds in order of increasing strength
11. What is a coordinate bond?
12. Relationship between bond length and strength?
13. How do you determine bond polarity?
14. Is polarity permanent or temporary for covalent bonds?
15. How to draw Lewis structures?
16. What are some exceptions to the octet rule?
17. What are resonance structures? Examples?
18. List types of covalent structures
19. Name + Explain the giant covalent structures
20. Key ideas of VSEPR theory?
21. Distinction between electron domain geometry and molecular geometry?
22. List EDG names and MG names for different numbers of electron domains w and w/o
lone pairs (state their bond angle too)
23. Difference between bond polarity and molecular polarity?
24. How can you determine net dipole moment?
25. Is the C-H bond polar?
26. Name types of intermolecular forces (+ define intermolecular forces)
27. Explain London/dispersion forces (where are they found, how do they work)
28. What factors affect the magnitude of London forces?
29. Explain dipole-dipole forces
30. How do you determine what type of intermolecular forces are present?
31. Explain hydrogen bonding
32. Do hydrogen bonds occur in H-F?
33. List intermolecular forces in order of increasing strength
34. Relationship between solubility and intermolecular forces?
35. Define metallic bonds
36. Structure of metallic compounds?
37. What factors do the strength of metallic bonds depend on?
38. Define alloys and explain their properties
39. Properties of metals?
40. Why is the rearrangement of the shape of a metal possible?
41. Trends in melting points of metals?
, 42. Define ionic bonding
a. Electrostatic attraction between oppositely charged ions (positive and
negative ions)
43. Are ionic compounds molecules?
a. No
44. Are ionic bonds uni-directional?
a. No: all ions are bonded ionically to others
45. How is an ionic compound structured?
a. In giant regular lattices (to maximise attraction and minimise repulsion
between oppositely charged and like charged ions) [repeating units of cations
and anions, 3D]
46. How do electronegativity values relate to ionic compounds?
a. If the difference is greater than 1.8, it is ionic
47. What are the physical properties of ionic compounds?
a. Does not conduct electricity when solid: only when molten or in aqueous
solution
b. High melting and boiling points (because strong electrostatic forces of
attraction between ions in lattice structure, lots of energy needed to
overcome)
48. What do melting points of ionic compounds depend on?
a. Strength of electrostatic attraction between the oppositely charged ions (this
statement should be in your answer -> explain why a certain factor
increases / decreases strength of electrostatic attraction, hence MP is higher /
lower)
i. Ionic radius (smaller the radius the stronger the connection),
electronegativity, ionic charge (greater the charge, stronger the
attraction, higher the melting point), low volatility (because strong
electrostatic forces), solubility (dissolves in water + other polar
solvents), brittle (breaks easily because lattice structures repel)
49. How do ionic compounds dissolve in water?
a. H+ and OH- in water bond interact with oppositely charged ions in the ionic
compound (and overcome electrostatic attractions between ions in the lattice
structure by pulling out individual ions from lattice)
50. Define covalent bonds
a. Electrostatic attraction between a shared pair of electrons and the positively
charged nucleus of the atom/molecule
51. List covalent bonds in order of increasing strength
a. Single bond, double bond, triple bond (because increasing pair of electrons
shared)
52. What is a coordinate bond?
a. Also known as dative covalent bond; where one atom provides both shared
electrons
53. Relationship between bond length and strength?
a. Increase in bond length (distance between two covalently bonded nuclei) =
decrease in bond strength
i. Because as number of shared electrons increases, the length
decreases (as there is a stronger attraction)
54. How do you determine bond polarity?
a. Electronegativity values (ability of an atom to attract shared electrons in a
covalent bond)
