Simple Models
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| ionic bond | attraction between oppositely-charged ions
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| Coulomb's law | describes the force of attraction between oppositely-charged particles
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| lattice energy | energy that is released by the formation of an ionic bond
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| can lattice energy be measured directly? | no
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| Lewis | created simple model for predicting the structures of covalent compounds
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| What do the atoms do in ionic compounds? | nonmetal atoms steal electrons from metal atoms
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| what do the electrons do in covalent compounds | electrons pairs are shared between atoms
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| Why do atoms share electrons? | to attain a noble gas configuration; to have the same # of electrons in its outermost orbital as a nobel gas
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| Why are hydrogen diatomic instead of monatomic? | because the two hydrogen atoms become much more stable by sharing their electrons. They want to reach a noble gas state.
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| how many electrons does hydrogen "need"? | two, so it is an exception to the octet rule
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| Steps for drawing Lewis Structures | 1: find the # of valence electrons; 2) skeleton structure 3)satisfy the octet rule; remaining electrons go on central atom 4)make double bonds if necessary
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| What are the elements are frequently make double bonds? | carbon (C), oxygen (O), sulfur (S), phosphorus (P)
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| Does chlorine, bromine, and iodine make double bonds? | yes, when they are the central atoms, not the terminal
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| Which elements never make double bonds? | fluorine and hydrogen
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| What does the charges on the polyatomic ions mean? | mean that there is an extra electron that we must count
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| which is shorter, double bond are single bond? | double bond. Triple bond are shorter than double bond
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| X-ray diffraction | a technique that allows us to determine bond lengths
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| Why are formal charges useful? | to help us determine which Lewis structure is the best
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| Formal for Formal Charge | FC = # of valence electron -(# unshared electrons + 1/2 # of shared electrons)
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| The status of the formal charges | 0 is good; +1 and -1 aren't bad; +2 and -2 are pushing things; +3 and -3 (and higher) are terrible
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| Electronegativity | the ability of an atom to attract shared electrons to itself
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| What element is the most electronegative? | Flourine (F)
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| the trend for electronegative | increase from left to right across a period, and decrease from top to bottom in a group
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| Atoms with higher electronegativity are more stable with what? | stable with a negative formal charge
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| atoms with a lower electronegativity are more stable with what? | a positive formal charge
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| What element is an exception to the octet rule? | Boron (only needs 6 electron); Be only needs 4
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| radicals | when we get odd numbers of valence electrons
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| Where would the odd electron be place? | on the atom that has the odd # of valence electron
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| What is the reason that atoms can accomodate more than 8 electrons? | because they have empty d orbitals
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| What are the common elements that are central atoms that have more than 8 electrons around them? | Cl, Br, I, S, Se, P
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| What elements can never have more than 8 electrons? | C, N, O, F
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| strength | mean the amount of energy required to break a covalent bond between two atoms
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| Which is stronger, multiple bonds between two elements or single bonds between the same two element? | multiple bonds
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