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Chemical Bonding I
Simple Models
| Question | Answer |
|---|---|
| ionic bond | attraction between oppositely-charged ions |
| Coulomb's law | describes the force of attraction between oppositely-charged particles |
| lattice energy | energy that is released by the formation of an ionic bond |
| can lattice energy be measured directly? | no |
| Lewis | created simple model for predicting the structures of covalent compounds |
| What do the atoms do in ionic compounds? | nonmetal atoms steal electrons from metal atoms |
| what do the electrons do in covalent compounds | electrons pairs are shared between atoms |
| 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 |
| 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. |
| how many electrons does hydrogen "need"? | two, so it is an exception to the octet rule |
| 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 |
| What are the elements are frequently make double bonds? | carbon (C), oxygen (O), sulfur (S), phosphorus (P) |
| Does chlorine, bromine, and iodine make double bonds? | yes, when they are the central atoms, not the terminal |
| Which elements never make double bonds? | fluorine and hydrogen |
| What does the charges on the polyatomic ions mean? | mean that there is an extra electron that we must count |
| which is shorter, double bond are single bond? | double bond. Triple bond are shorter than double bond |
| X-ray diffraction | a technique that allows us to determine bond lengths |
| Why are formal charges useful? | to help us determine which Lewis structure is the best |
| Formal for Formal Charge | FC = # of valence electron -(# unshared electrons + 1/2 # of shared electrons) |
| 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 |
| Electronegativity | the ability of an atom to attract shared electrons to itself |
| What element is the most electronegative? | Flourine (F) |
| the trend for electronegative | increase from left to right across a period, and decrease from top to bottom in a group |
| Atoms with higher electronegativity are more stable with what? | stable with a negative formal charge |
| atoms with a lower electronegativity are more stable with what? | a positive formal charge |
| What element is an exception to the octet rule? | Boron (only needs 6 electron); Be only needs 4 |
| radicals | when we get odd numbers of valence electrons |
| Where would the odd electron be place? | on the atom that has the odd # of valence electron |
| What is the reason that atoms can accomodate more than 8 electrons? | because they have empty d orbitals |
| What are the common elements that are central atoms that have more than 8 electrons around them? | Cl, Br, I, S, Se, P |
| What elements can never have more than 8 electrons? | C, N, O, F |
| strength | mean the amount of energy required to break a covalent bond between two atoms |
| Which is stronger, multiple bonds between two elements or single bonds between the same two element? | multiple bonds |
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