PERIODIC TABLE
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| With principal quantum number, how many electrons are there per shell? | 2n^2
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| Absorption spectrum vs. emission spectrum | -absorption spectrum shows what is absorbed (black lines on rainbow)
-emission spectrum shows what is emitted (colored lines on black background)
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| How many electrons does each orbital hold? | 2
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| What are l, m, s? | -l = subshell (0 -> n-1)
-m = magnetic quantum number (-l to l)
-s = spin quantum number (+/-1/2)
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| What does magnetic quantum number tell us? | particular orbital within a subshell where an electron is highly likely to be found (orientation of orbital in space)
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| Aufbau principle | shells/subshells of lower energy get filled first
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| Hund's rule | fill each orbital with a single electron with same spin
--> e-e repulsion in double occupied orbitals creates high energy
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| Pauli exclusion principle | 2 electrons in same orbital must be of different spins
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| Bohr atom | electron orbiting positive nucleus
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| Effective nuclear charge increases as you move...? | left to right across periodic table
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| Higher effective nuclear charge, more / less stable? | more stable --> higher ionization energy
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| Do alkali metals / alkaline earth metals increase / decrease in reactivity as you go down a group? | increase (increasing radii)
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| Are halogens more / less reactive as you go down a group? | less (increasing radii)
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| What is oxidation state of noble gases? | 0
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| WHy do transition metals have high conductivity? | loosely bound outer d electrons
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| Transition metals vs. representative elements | -transition metals are d-block
-representative elements are s and p block
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| Metals like to (gain/lose) electrons and nonmetals like to (gain/lose) electrons | lose / gain
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| Metals form basic / acidic oxides, nonmetals form basic / acidic oxides. | basic / acidic
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| What is ionization energy? | energy needed to knock off first valence electron
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| What is ionization energy trend? | decreases as you go down because of increasing radii, increases as you go right because of decreasing radii
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| Which group has the lowest ionization energy? Highest? | alkali metals / noble gases
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| Is second ionization higher / lower for first ionization energy? | much higher
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| What is electron affinity | amount of energy released when something gain an electron
--> how easily it can gain an electron
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| What is electron affinity trend? | decreases down a group because of larger radii, increases as you go right
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| Which group has highest electron affinity? lowest? | halogens / noble gases
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| What creates an ionic bond? | complete transfer of electrons from electropositive element to the electronegative element
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| What is a covalent bond? | sharing of electrons between elements
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| What is electronegativity? | how much something hordes electrons in a covalent bond
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| What is the most electronegative element? | fluorine
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| Can noble gases be electronegative? | YES --> Kr and Xe
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| The more electronegative,... | the more it hordes electrons
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| Why does atom size decrease across the period? | increasing Zeff and electrostatic interaction
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| What does Zeff refer to in relation to protons and electrons? | strength through which protons in nucleus can pull additional electrons
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| What is trend for Zeff? | increases left to right and stays the same going down a group
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| The higher the Zeff,... | the more tightly electrons are bound to atom
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| Atomic radii trend? | size increases as you go down a column, size decreases as you go across a row
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| Is hydrogen a metal or nonmetal? | nonmetal
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| Where is the most metallic element found? least metallic? | lower right / upper left
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| What is a nucleon? | one of the particle that makes up a nucleus
--> either a proton or a neutron
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| Nucleus with a net spin will have odd / even number of nucleons? | odd
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| How many times bigger are ions than electrons? | thousand times
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| What is the lightest ion? | hydrogen
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| Thomson Experiment | existence of opposite charges
--> charge is a fixed quantity
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| What is a positron? | has the same mass as an electron but opposite charge
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| What formula to use for mass spectrometry? | mv^2/r = qvB
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| Millikan oil drop experiment? | -charge of electron has fixed value
-charge of proton has opposite value
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| What is charge of electron | 1.6E-9C
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| What is the charge of a proton? | opposite of electron
1.6E-9C
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| Rutherford experiment | atoms have dense nuclei with all atomic mass centrally concentrated (uniformly spaced)
--> lattice structure
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| Rutherford showed that an atom is mostly? | empty space
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| What is inside the nucleus? | protons and neutrons
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| Heisenberg uncertainty principle | not possible simultaneously to identify a particle's position and velocity at the same time
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| Energy of a photon | E = hv
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| Is more or less energy required to carry out transitions when electrons are close to nucleus? | more energy
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| Hydrogen transitions formula | (1/nf^2 - 1/ni^2)
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| Number of electrons in each shell | 2(n)^2
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| Mg2+ has 2 more or 2 less electrons? | 2 less electrons
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| What is Zeff? | moving left --> right across a period, add electrons and protons one at a time
--> electrons more attracted to positive nucleus and size decreases
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| Calculate Zeff? | #protons - shielding electrons
-only electrons in shells below one of interest contribute
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| How does more protons affect size? | smaller
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| What does a shell represent? | energy level an electron can occupy
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| What does an orbital represent? | region in which electron is likely to be found
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| What is a paramagnetic species? | something with one unpaired electron
--> susect to B-fields
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| Which elements are diamagnetic? | alkaline earth metals and noble gases
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| What is a cation? | -deficit in at least one electron
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| What is an anion? | -excess of at least one electron
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| What is an excited state electron configuration? | electrons are in an energy level higher than what is standard for ground state
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| Quantum numbers formula | -n / l = n-1 / m=-l to l / up or down
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| What are the possibilities for angular quantum number, l? | 0 --> n-1
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| What increases from going from left --> right? | ionization energy, electron affinity, eN
--> atomic radius decreases
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| Are cations smaller or larger than neutral atoms? Are anions smaller or larger than neutral atoms | -smaller --> more compact
-larger --> electron repulsion
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| Within a period, are anions bigger than cations? | YES
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| What defines the radius of an atom? | electrons
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| Is He bigger or smaller than H? | bigger
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| What does an atom become when it is ionized? | a cation
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| Why are the d-elements exceptions to several periodic trends? | half-filled and filled d-shell stability
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| Does the atomic radius of d-elements change a lot? | NO
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| The more protons... | the greater the attractive interactions, smaller the atom
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| What creates higher ionization energy? | less willing to give it up
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| Does increasing valence electrons affect shells? | NO
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| Is I.E. trend clean or erratic? | erratic
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| Trend in eN increases with what? | number of valence electrons
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| What happens when a quantum of energy less than what is required to ionize element is absorbed by element? | electron excited to higher energy state
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| Lyman, Balmer, Paschen, Brackett? | UV, visible, Infrared, Microwave
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| What does it mean to have the lowest threshold frequency for photoelectric effect? | material that is easiest to ionize
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| What does electron capture create? | decrease number in atomic number
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| What does positron capture create? | increase number in atomic number
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| A beta particle is positive or negative? | negative
--> positive = positron
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| For a first order decay, what is constant? | half-life regardless of concentration
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