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Chapter 9
Chemical Bonding I: Lewis Theory (Test 4)
| Question | Answer |
|---|---|
| ionic bonding | electrostatic attractions between oppositely charged particles; typically between a metal and a nonmetal |
| covalent bonding | involves the sharing of electrons; typically between two nonmetals |
| metallic bonding | consists of metal cations sitting in a "sea" of electrons; typically between two metals |
| the Octet Rule | Atoms tend to gain, lose, or share electrons in such a way as to attain a noble gas electron configuration. |
| ionic bonding | 1. involves complete electron transfer 2. infinite crystal lattices 3. solids with high melting points |
| polar covalent bonding | 1. involves unequal sharing of electrons 2. polarity is determined by electronegativity |
| nonpolar covalent bonding | 1. involves equal sharing of electrons 2. gases or liquids at room temperature, or solids with low melting points |
| lattice energy | the energy released when gaseous ions form 1 mole of the ionic crystal |
| the greater the lattice energy, | the higher the melting point and the harder the crystal |
| Bond breaking is always what? | endothermic |
| Bond forming is always what? | exothermic |
| Coulomb's Law is used to determine what? | lattice energy |
| What is Coulomb's Law? | F = k (q1q2)/(r^(2)) where q is the magnitude of the charges and r is distance between centers |
| Does charge or size impact lattice energy more? | charge |
| What are two ways to measure the strength of a bond? | 1. bond length 2. bond energy |
| The shorter the bond, | the stronger the bond |
| What is the first step in drawing Lewis Structures? | Sum the valence electrons from all atoms; take into account any positive or negative charge and add or subtract electrons from the total as necessary. |
| The central atom is usually either what? | 1. listed first 2. the less electronegative atom |
| Which atoms should you add electrons to first, after connecting the atoms with bonds? | the outer atoms |
| What should you do after all electrons are distributed? | Check to see if the central atom has an octet. |
| formal charges | the number of valence electrons on the atom minus the number of electrons assigned to the atom. (The number assigned corresponds to all the unshared electrons plus 1/2 of the shared electrons.) |
| Which atoms routinely have less than an octet? | Be, B, Al. |
| Which molecules will always violate the octet rule? | molecules with an odd number of electrons |
| Which elements can have more than an octet? | 3rd row elements and below |
| When is resonance used? | when one Lewis Structure does not adequately describe the molecule |
| resonance structure | any valid Lewis Structure |
| resonance hybrid | the "true molecule"; a hybrid of all valid Lewis Structures |
| If you add the formal charges of all atoms in a molecule, | you should get the overall charge of the molecule |
| What three things should you consider when evaluating resonance structures for validity? | 1. the less formal charge, the better 2. negative formal charge on the more electronegative element is favorable 3. avoid like charges on adjacent atoms |
| the more resonance structures that can be formed, | the more stable a molecule (due to charge delocalization) |
| electronegativity | the ability of an atom in a molecule to attract shared electrons |
| What is the most electronegative element? | F (fluorine) |
| What is the second most electronegative element? | O (oxygen) |
| bond energy | the energy required to break 1 mole of a covalent bond |
Created by:
2nenogirl
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