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