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