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 ________.