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OAT - Chem
Chapter 1 - Atomic Structure
| Term | Definition |
|---|---|
| chemistry | study of the nature of matter |
| atom | basic building block of matter, smallest unit, made of subatomic particles |
| proton/neutron | make up the nucleus |
| protons | carry single positive charge; 1 amu |
| Z | atomic number, number of protons for an element |
| Neutrons | carry no charge, slightly larger than protons, isotopes have diff these but the same protons |
| A | mass number, protons + neutrons |
| Electrons | carry single negative charge, hella small mass |
| Valence electrons | electrons farthest from nucleus |
| reactivity | valence electrons and their activity determine ___ of an atom |
| atomic weight | weight in g/mol using avogadro's number |
| isotopes | species of atoms with same number of protons but diff number of neutrons |
| How to find atomic weight given percentages and amu | multiply percentage with correct amu and then add those numbers up |
| A-Z | amount of neutrons |
| Planck's Constant | h; 6.626x10^-34 Js |
| quanta | bundles of electromagnetic radiation E |
| The smaller the radius of an electron | the lower the E state of the electron |
| orbitals | representation of the probability of finding an electron within a given region |
| Heisenberg Uncertainty Principle | states that it is impossible to determine with perfect accuracy the position and momentum of an electron simultaneously |
| Pauli Exclusion Principle | no two electrons in a given atom can have the same set of 4 quantum numbers |
| energy state | position and E of an electron described by quantum numbers |
| Principle Quantum Number | n; the larger the number, the higher the E lvl and radius of electron's orbit |
| Azimuthal Quantum Number | L; angular momentum; sublevels of each E lvl; ranges from 0 to n-1; 0, 1, 2, 3 = s, p, d, f |
| Magnetic Quantum Number | m.e.; specifies the particular orbital within a sublevel where an electron is likely to be found; L to -L |
| Spin Quantum Number | m.s.; intrinsic angular momentum; two orientations 1/2 and -1/2 |
| How to determine what subshell is filled first | n + L, whichever is lower gets filled first |
| Hund's Rule | within a given subshell, orbitals are filled such that there are a max number of half-filled orbitals with parallel spins |
| Paramagnetic | if the material has unpaired electrons and attract atom |
| Diamagnetic | no unpaired electrons and slightly repelled |
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