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AP chem chapter 7
Question | Answer |
---|---|
Hund's rule | Every orbital in a subshell is occupied with only one electron before the electrons can be paired. |
Aufbau Principle | electrons fill lower levels before filling the higher levels. ex: 1s before 2s |
Heisenberg uncertainty principle | the more precisely one property is measured, the less precisely the other can be controlled, determined, or known. |
Pauli exclusion principle | an orbital can only hold up to two electrons. the two electrons must have opposite spins. Therefore, no two electrons in the same atom can have the same 4 Quantom numbers. |
Absorption and emmision spectra | the colors for each element. The lines that are left when the electron falls. |
Quantized | Energy can be gained or lost only in integer mulitples of hv. |
photoelectric effect | electrons are emitted from the surface of a metal when light strikes it. |
line spectrum | Hydrogen only, only certain energies are allowed for the electron in the hydrogen atom. |
Quantum model | the electron in a hydrogen atom, moves around the nucleus only in certain allowed circular orbits. |
polyelectronic atoms | atoms with more than one electron |
core electrons | inner electrons |
Metals | *shiny *ductile *good conductors of heat/energy |
nonmetals | *brittle *aborbs heat *dull |
___has more protons than ____ and a greater inward pull... | 1st explanation |
___ has more energy levels than ___ and it's outer electrons are farter from the inward pull of the nucleus... | 2nd explanation |
Exception 1: | S electrons sheild the P electrons from the inward pull |
exception 2: | paired up electrons have extra repulsion. |
IE dips in what groups? | 3 and 6 |
EA dips in what groups? | 2 and 5 |