Honors Chemistry Chapter 6 Lecture Notes
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Created by:
12le on September 26, 2010
Subjects:
honors chemistry, chapter 6, sharon
Description:
Sharon
SFHS
Honors Chemistry Chapter 6 Lecture Notes Quiz
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33 terms
Terms | Definitions |
|---|---|
 if s and p sublevels are full | outer level is considered full |
| outer level full | most stable situation |
| 8 electrons in outer level | makes an atom become unreactive |
| helium | exception because it only has one full orbital |
| if it can't have full outer level, atoms likes to have half filled orbitals | these are slightlt more stable (less reactive) than other choices |
| Cr | [Ar] 4s1 3d5 |
| Cu | [Ar] s1 3d10 |
| cation | positive ion |
| anion | negative ion |
| why do atoms become ions | to become more stable (octet rule) |
| what does the 1st column do? | lose one election |
| what do metallic elements do when forming ions | lose electios |
| positive ions are | smaller then corresponding neutral atoms because it lost one energy level (goes down a shell energy level, decreasing the size) positive char (p) hasnt changed but pulling on fewer electrons |
| what do halogens do | gain 1 electron |
| nonmentals do what when forming ions | gain electrons |
| negative ions | bigger than corresponding neutral atoms because there are more electrons crowding |
| metal activity | inc toward bottom left (Fr) |
| nonmetal activity | inc toward top right but skips noble gases (F) |
| first ionization energy | energy required to remove electrons from gaseous atom |
| x(g) + E ~> | x+(g) + e- (E needed) units (KJ/mol) |
| ionzation energy to right | increases to right because inc nuclear charge (or more protons) |
| ionization energy column trend | decreases down a column because electron is greater distance from nucleus, valence electrons are shielded from pull of nucleus by core electron |
| ionization energy exception trend | electron from full or 1/2 full sublevel more stable than trend so greater ionization energy |
| metal ionization energy | low 1st IE; takes little E to remove e- |
| nonmetal ionization energy | high 1st IE |
| electronegativity | relative tendency of an atom to attract electrons to itself when it is chemically combined with another element |
| highest electronegativity | Flourine |
| electronegativity upper right | increases to upper right (not noble gases) b/c less distance from nucleus to outer reacting electrons, shielding effect less so it does not affect reacting electron so increases at top of group; more protons in nucleus so more pull for outer electron as go across row to right |
| electron affinities | the energy change that accompanies the addition of an electron to a gaseous atom |
| x(g) + e- ~> | x-(g) + E (usually energy given off) |
| electron affinity across a period | across a period inc to right because increased nuclear char (#p) but if stable will cause deviation |
| negative electron affinity means | more stable as is, does not want more electrons (must add E to force it to take that electron) |
| metals electron affinity | gives off less E so smaller electron affinity some even neg values |
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