Chemical Bonding Ch 6
Section 6-1 Introduction to Bonding
1. Nearly all substances made up of combinations of atoms are held together by
____________ ____________.
2. A chemical bond is a mutual ___________ attraction between the nuclei and
___________ __________ of different atoms that binds the atoms together.
3. By bonding with each other, atoms decrease in ____________ energy, thereby
creating more stable arrangements of matter.
4. When atoms bond, their __________ ___________ are redistributed in ways that
make the atoms more _____________.
5. Chemical bonding that results from the electrical attraction between large number
of ____________ and ____________ is called ionic bonding.
6. Define cation (look in glossary)________________________________________.
7. Define anion (look in glossary)________________________________________.
8. In pure ionic bonding, atoms completely ___________ _______ electrons to other
atoms.
9. Atoms joined by covalent bonding _____________ electrons.
10. What’s one difference between ionic and covalent bonding?_________________
_____________________________________________________________________
11. Covalent bonding results from the ___________ of electron pairs between two
atoms.
12. Look at the electronegativity chart on page 151 in your book. One way to find
which type of bond two elements will have is to subtract the two numbers found
on the chart.
13. What is the electronegativity range for ionic bonds?________________________
14. What is the electronegativity range for polar-covalent bonds?________________
15. What is the electronegativity range for nonpolar-covalent bonds?_____________
16. Hydrogen-Hydrogen bonds are ____________ __________ bonds. This means
the electrons are __________ ___________ by the bonded atoms, resulting in a
balanced distribution of charge.
17. Polar covalent bonds have an ________ attraction for the shared electrons.
18. What’s the difference between polar and nonpolar covalent bonds?____________
_____________________________________________________________________
19. The partial negative symbol is ______, and the partial positive symbol is ______.
20. Look at the chart on pg 151 to help you answer question 3 under the section
review on pg 163.___________________________________________________
Section 6-2 Covalent Bonding
21. A molecule is a neutral group of atoms held together by ___________ bonds.
22. A ___________ formula indicate the relative numbers of atoms of each kind in a
chemical compound by using atomic __________ and numerical ___________.
23. A _________molecule is a molecule containing only ______atoms. An example
is __________.
24. The distance between two bonded atoms is the _________ ________.
25. ________ energy is the energy required to _________ a chemical bond and form
neutral isolated atoms.
26. The ________ rule states the chemicals tend to form so that each atom has a
________ of electrons in its highest occupied energy level.
27. How many is an octet?___________
28. There are exceptions to the octet rule. Hydrogen only wants _____ electrons.
Boron tends to form bonds to get _____ electrons.
29. Electron-dot notation is an electron-configuration notation in which only the
___________ electrons of an atom of a particular element are shown, indicated by
________ placed around the element’s symbol.
30. Look at Figure 6-10. Draw the electron dot diagram for carbon._____________
31. What group number is carbon in?_____________
32. Look at Figure 6-10. Draw the electron dot diagram for fluorine.____________
33. What group number is fluorine in?______________
34. What is the connection between the group number and the valence electron
number?___________________________________________________________
35. Dots between the two symbols in a Lewis structure represents the _________ pair
of a covalent bond. Electrons that surround the symbols are called a _______ pair.
This means that the electrons are not involved in ___________ and belong
exclusively to that one atom.
36. Lewis structures are formulas in which atomic __________ represent nuclei and
inner-shell electrons, dot-pairs or _________ between two atomic symbols.
37. Look at the Lewis structure for fluorine on pg 171 and look at the structural
formula for fluorine. What’s the difference?______________________________
_________________________________________________________________
38. Look at pg 171-173. What’s the difference between the Lewis structures of single,
double, and triple bonded atoms?______________________________________
_________________________________________________________________
39. _____________ structures cannot be correctly represented by a single Lewis
structure.
Section 6-3 Ionic Bonding
40. An ____________ compound is composed of positive and negative charges that
are ____________.
41. Look on pg 177. Do the Lewis structures for ionic compounds have dashes like
the covalent ones on pg 175 had?________
42. A charged group of covalently bonded atoms is known as a _______________ion.
How do the Lewis structures for polyatomic compounds differ from the ionic and
covalent ones you have seen so far (compare pg 180, 177, and175)?___________
__________________________________________________________________
Section 6-4 Metallic Bonding
43. Chemical bonding is different in ____________ than it is in ionic, molecular, of
covalent compounds.
44. Metals are excellent ___________ conductors in the ________ state.
45. The chemical bonding that results from the attraction between ________ atoms
and the surrounding _______ of electrons is called ______________ bonding.
46. ___________ is the ability of a substance to be ______________ into thin sheets.
47. ___________ is the ability of a substance to be drawn, pulled, or extruded
through a small opening to produce a ________.