Chemistry Ch 6 Study Guide, Chemical Bonding2015-2016

NAME: ______DATE:_____ HR: ____ CHEMISTRY ~ CH 6 STUDY GUIDE, CHEMICAL BONDING2015-2016

1. Why do atoms want to bond with other atoms? 2. Define chemical bond. 3. What is the difference between covalent and ionic bonds? 4. KNOW PROPERTIES OF BOTH COVALENT AND IONIC COMPOUNDS.( conduct electricity, crystal lattice structure, dissolves in water, which compounds have high melting and boiling points.. etc) 5. What two types of covalent bonding are there? What is the difference between these two types of bonding? 6. Define bond energy. 7. Define bond length. 8. What is the relationship between bond length, strength, and energy? 9. What is the difference between a cation and an anion? In an ionic compound, which is found in the front of the formula? 10. In general, what types of elements create ionic bonds? In general, what types of elements create covalent bonds? 11. What types of elements create metallic bonds? 12. How are metallic bonds formed? 13. What is Hydrogen bonding and how does this occur? 14. If a compound has an electro negativity difference of 1.80 what type of bonding will be present? 15. If a compound has an electro negativity difference of .03 what type of bonding will be present? 16. If a compound has an electro negativity difference of 1.0 what type of bonding will be present? 17. What is the difference between inter and intra molecular forces? 18. If a substance is dissolved in water and it DOES conduct electricity, what two types of intra- molecular bonding could the substance have? 19. If a substance is solid at room temperature, is shiny, DOES NOT dissolve in water but it DOES conduct electricity, what type of bonding does it probably have? 20. What three things are found in a Lewis structure? 21. KNOW HOW TO MAKE Lewis STRUCTURES. 22. What does VSEPR stand for? 23. What does the VSEPR theory state ( AKA; what is the main idea of VSEPR)? 24. If there are 2 pairs of e’ present around an atom, what molecular structure and what bond angles are present in this structure? 25. If there are 3 pairs of e’ present around an atom, what molecular structure and what bond angles are present in this structure? 26. If there are 4 pairs of e’ present around an atom, what molecular structure and what bond angles are present in this structure? 27. Using Lewis structures, how can you determine if a molecule/compound is bonded together with polar or non-polar bonds? 28. List all 7 elements that form diatomic molecules if not found in a compound. 29. Diatomic molecules are held together with what type of covalent bonding? 30. In a Lewis structure, what is the difference between the central atom and terminal atoms? What are two ways to determine the central atom when building a Lewis structure? 31. In a Lewis structure what represents a single, double, and a triple bond? 32. In a Lewis structure which electrons are represented by lines and dots? 33. What are the two electron regions found in a molecule? 34. Define electronegativity. 35. What element has the highest electronegativity? 36. What are dipole-dipole forces? 37. Which bonding is weaker- ionic, covalent or dipole-dipole forces? 38. What are London dispersion forces? 39. Explain how Noble gases or other non-polar molecules can have temporary dipole moments. 40. What is an octet? What is a duet? 41. Which atoms reach duets to be stable? 42. Name three elements that have expanded octets. Where do the extra electrons come from to help in bonding in these cases? 43. What element bonded to three fluorine atoms is stable with six valence electrons? 44. In VSEPR notation, what letters represent the central atom, the lone pairs of e’, and the bonding pairs of atoms? 45. BE ABLE TO WRITE VSEPR NOTATION FROM A Lewis STRUCTURE. 46. Explain what a resonance structure is. Give an example of a molecule that shows resonance. 47. BE ABLE TO DETERMINE IF AN ATOM SHOWS RESONANCE. 48. Be able to assign formal charges to atoms in a resonance structure and determine if there is a best structure. 49. Be able to look at a 3-D molecular model and determine what molecular geometry it has. 50. Define polyatomic ion. 51. Which types of bonds hold polyatomic ions together? 52. Are most of the polyatomic ions cations or anions? 53. In regard to bond angles, if you have lone e’ off the central atom are the bond angles smaller or larger between the bonding pairs of electrons? 54. In Lewis structures how is the need for multiple bonds usually determined? 55. In Lewis structures, if you have extra electrons where should they be put?

56. Draw the Lewis structures, write the VSEPR notation, determine the molecular geometry, and indicate the bond angles of the following molecules.

2- SCl2 NH2Cl SO3

1+ PI3 SiCl3Br NH4

Cl2O ONCl

53. Determine the electronegativity difference between the following atoms and determine the probable bond types:

H and I S and O K and Br Si and Cl Se and S Zn and Cl

54. According to VSEPR what molecular geometries do the following notations represent?

AB2 AB3 AB2E AB3E AB2E2