1. Chemical Bond - a. The simplest ratio of elements in an ionic compound that describes its composition

2. Octet Rule b. A communal sharing of electrons between metal atoms.

3. Covalent Bond c. The tendency of an object to form two localized regions of opposite character; in chemistry it relates to electrical charge.

4. Ionic Bond 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 e. A force of attraction that holds atoms together in compounds; an attraction produced by the transferring or sharing of electrons

6. Polarity f. Two atoms held together in an ion or molecule by their attraction for the same pair of shared electrons.

7. Electrostatic Force 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 h. The electrostatic attraction between two oppositely charged ions in a solid.

9. Polyatomic Ion i. The field force exerted by electrical charges. It may be repulsive or attractive depending on the kinds of charges.

10. Formula Unit j. A two dimensional diagram that uses element symbols and dots to show the bonds between different atoms.

1. Crystal lattice k. Electrons that can move between several different bonds.

2. Electron Sea Theory L. Atoms covalently bonded into a continuous three-dimensional network: for example, diamond.

3. Delocalized electrons

m. 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. Alloy o. 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.

1. Chemical Bond - e

a. The simplest ratio of elements in an ionic compound that describes its composition

2. Octet Ruleg

b. A communal sharing of electrons between metal atoms.

3. Covalent Bondf

c. The tendency of an object to form two localized regions of opposite character; in chemistry it relates to electrical charge.

4. Ionic Bondh

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 Bondb

e. A force of attraction that holds atoms together in compounds; an attraction produced by the transferring or sharing of electrons

6. Polarityc

f. Two atoms held together in an ion or molecule by their attraction for the same pair of shared electrons.

7. Electrostatic Forcei

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 Structurej

h. The electrostatic attraction between two oppositely charged ions in a solid.

9. Polyatomic Iond

i. The field force exerted by electrical charges. It may be repulsive or attractive depending on the kinds of charges interacting.

10. Formula Unita

j. A two dimensional diagram that uses element symbols and dots to show the bonds between different atoms.

1. Crystal lattice - m

k. Electrons that can move between several different bonds.

2. Electron Sea Theory - o

L. Atoms covalently bonded into a continuous three-dimensional network: for example, diamond.

3. Delocalized electrons - k

m. 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 - n o. 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.

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

Bond Theories• Remember

sublevels? • Azimuthal

shape• S – 1 orbital• P – 3 orbitals

Bond Theories• Remember sublevels? • Azimuthal shape• D – 5 orbitals

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

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

Bond Theories• Covalent bonds• Sigma and Pi

bonds• Sigma ∂ bonds• Overlapping orbitals• S (side – side) or P

(end-end)• Or P – S – in line

Bond Theories• Covalent bonds• Pi (π) bonds• P orbitals out of

plane are drawn to each other and overlap• Double and triple

bonds

Bond Theories• Covalent

bonds• Pi (π) bonds• Triple bond in

molecular nitrogen

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 functio

n can occupy different regions of a molecule at same time• Example - Ozone

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

Bond Theories• Fewer than 4 pairs• Boron – 3Ve – content with 6 to fill

occupied orbitals – Boron trifluoride

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

Bond Theories• What happens when theories don’t

explain observations?• LOX

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

Bond Theories• Time for a new theory

• Some encircle multiple atoms or entire molecule• S orbital hybridization