1. 1. Chemical Bond -a. The simplest ratio of elements in an ionic compound that describes its composition 2. Octet Ruleb. A communal sharing of electrons between metal atoms. 3. Covalent Bondc. The tendency of an object to form two localized regions of opposite character; in chemistry it relates to electrical charge. 4. Ionic Bondd. A group of atoms that maintains a constant electrical charge while existing as a unit in a wide variety of chemical reactions. 5. Metallic Bonde. A force of attraction that holds atoms together in compounds; an attraction produced by the transferring or sharing of electrons 6. Polarityf. Two atoms held together in an ion or molecule by their attraction for the same pair of shared electrons. 7. Electrostatic Forceg. An atom tends to gain, lose or share electrons until its outer s and p orbitals are filled with eight electrons: the electron configuration of a noble gas. 8. Lewis Structureh. The electrostatic attraction between two oppositely charged ions in a solid. 9. Polyatomic Ioni. The field force exerted by electrical charges. It may be repulsive or attractive depending on the kinds of charges. 10. Formula Unitj. A two dimensional diagram that uses element symbols and dots to show the bonds between different atoms.

2. 1. Crystal latticek. Electrons that can move between several different bonds. 2. Electron Sea TheoryL. Atoms covalently bonded into a continuous three-dimensional network: for example, diamond. 3. Delocalized electronsm. An extensive three-dimensional structure of points or objects that represents the regular alternating pattern of atoms or ions. 4. Network Covalent Substance n. A mixture of atoms of a metal with another element where the mixture has metallic properties. 5. Alloyo. A theory that offers an explanation of how metals bond; the valence electrons of atoms are said to be freely shared among all atoms. Also called the free-electron theory.

3. 1. Chemical Bond - ea. The simplest ratio of elements in an ionic compound that describes its composition 2. Octet Rule g b. A communal sharing of electrons between metal atoms. 3. Covalent Bond f c. The tendency of an object to form two localized regions of opposite character; in chemistry it relates to electrical charge. 4. Ionic Bond h d. A group of atoms that maintains a constant electrical charge while existing as a unit in a wide variety of chemical reactions. 5. Metallic Bond b e. A force of attraction that holds atoms together in compounds; an attraction produced by the transferring or sharing of electrons 6. Polarity c f. Two atoms held together in an ion or molecule by their attraction for the same pair of shared electrons. 7. Electrostatic Force i g. An atom tends to gain, lose or share electrons until its outer s and p orbitals are filled with eight electrons: the electron configuration of a noble gas. 8. Lewis Structure j h. The electrostatic attraction between two oppositely charged ions in a solid. 9. Polyatomic Ion d i. The field force exerted by electrical charges. It may be repulsive or attractive depending on the kinds of charges interacting. 10. Formula Unit a j. A two dimensional diagram that uses element symbols and dots to show the bonds between different atoms.

4. 1. Crystal lattice - mk. Electrons that can move between several different bonds. 2. Electron Sea Theory - oL. Atoms covalently bonded into a continuous three-dimensional network: for example, diamond. 3. Delocalized electrons - km. An extensive three-dimensional structure of points or objects that represents the regular alternating pattern of atoms or ions. 4. Network Covalent Substance - L n. A mixture of atoms of a metal with another element where the mixture has metallic properties. 5. Alloy - no. A theory that offers an explanation of how metals bond; the valence electrons of atoms are said to be freely shared among all atoms. Also called the free-electron theory.

5. Bond Theories All about the ……? Lewis structure limitations Cannot show molecular shape – 2d Remember sublevels? Azimuthal shape S – 1 orbital P – 3 orbitals D – 5 orbitals F – 7 orbitals All because of electron repulsion

6. Bond Theories Remember sublevels? Azimuthal shape S – 1 orbital P – 3 orbitals

7. Bond Theories Remember sublevels? Azimuthal shape D – 5 orbitals

8. Bond Theories Remember sublevels? Azimuthal shape F – 7 orbitals All because of electron repulsion

9. Bond Theories Covalent bonds 2 electrons with opposite spin sharing overlapping orbitals Electrons available to both nuclei Effectively both atoms acquire the shared electrons Valence Bond Theory

10. Bond Theories Covalent bonds Sigma and Pi bonds Sigma ∂ bonds Overlapping orbitals S (side – side) or P (end- end) Or P – S – in line

11. Bond Theories Covalent bonds Pi ( π ) bonds P orbitals out of plane are drawn to each other and overlap Double and triple bonds

12. Bond Theories Covalent bonds Pi ( π ) bonds Triple bond in molecular nitrogen

13. Bond Theories Molecular Resonance Many bonds can be represented by more than one lewis struct. Should be diff. between 2 ends due to double and single bonds – BUT NO!! Completely symmetrical Resonance Electron wave function can occupy different regions of a molecule at same time Electron wave function can occupy different regions of a molecule at same time Example - Ozone

14. Bond Theories Odd # of valence electrons Extra is free radical – cause damage to cells Eat your fruits & veggies to combat

15. Bond Theories Fewer than 4 pairs Boron – 3Ve – content with 6 to fill occupied orbitals – Boron trifluoride

16. Bond Theories Expanded octet Extra electrons occupy empty d sublevels Sulfur hexafluoride

17. Bond Theories What happens when theories don’t explain observations? LOX

18. Bond Theories Time for a new theory E.g. valence bond theory – prohibits stray electrons that account for certain properties of molecule – answer? Resonance structures Also doesn’t account for properties of LOX Thus – Molecular Orbital Theory When bond forms, old orbitals replaced by totally new orbitals Each molecule has unique orbitals – equal in # to what sum of orbitals in original atoms Some encircle multiple atoms or entire molecule

19. Bond Theories Time for a new theory Some encircle multiple atoms or entire molecule S orbital hybridization