MIDTERMS (but like look at the other decks too) Flashcards
What wavelength causes vibration?
infrared radiation
What wavelength causes rotation?
microwave radiation
What wavelength causes electrons to transition/be ejected?
UV
Electrons in orbitals must be opposite spins
Pauli Exclusion Principle
Fill orbitals half way until all in subshell are filled before filling orbitals fully
Hund’s rule
Fill orbitals and subshells of lowest energy first
Aufbau Principle
Aufbau Principle exceptions and why:
Cu and Ag, taking an electron from an s subshell to finish the d subshell and have stability, and Cr and Mo take electrons from s subshell to be half-filled stable
Heisenberg Uncertainty Principle
Determining the speed or position of an electron/photon is impossible, responsible for “probabilities of distribution”/electron clouds instead of exact electron positions and speeds. Closer you get to precise location the less precise the speed is and vise versa
Dmitri Mendeleev
Ordered elements from increasing atomic mass, w/elements of similar properties in the same column (he was wrong)
stupid
Mosley
Ordered elements by atomic numbers (he was right)
Why do different elements emit different spectra?
Because each element has a different electron configuration, thus energy levels, and therefore energy (in wavelength/frequency of photons ejected)
Coulomb’s law
F=k((Q1 x Q2)/r^2)
Describes atomic radius size as a function of forces of attraction and repulsion between the nucleus and electrons and electrons and electrons, (shielding and different sized outer oribts of elements given same energy levels)
Electronegativity trend (give directions ex. left and down)
Right and up
Atomic size trend (give directions (ex. left and down are larger))
Left and down are larger
Does effective nuclear charge change as it moves down a group? Why?
No, as the same amount of valence electrons exist for each atom down a group. ( weirdly, as the electrons are still further away, down a group decreases electron affinity/binding energy even though the effective nuclear charge is technically the same (text for clarification if this is too confusing))
Order for determining an elements atomic size
- Energy level
a. Whether or not there are the same amount of full electron “shields” - Amount of protons
a. And effective nuclear charge acting on valence electrons - Amount of valence electrons
a. Electrons repel, protons in nucleus are less effective and attraction is more spread out thus making it bigger
4.
Metals are more prone to ______ electrons, whereas nonmetals usually _____ electrons. (gain, lose)
- lose
- gain
Cations are _____ than their original element, whereas anions are _____. Additionally, when a cation and anion are isoelectronic, the cation is substantially smaller. Why is this? (larger, smaller)
- smaller
- larger
because cations lose and electron, therefore decreasing electron-electron repulsion, whereas anions gain an electron, having the opposite effect. When isoelectronic, the cation has a much higher Zeff value (effective nuclear charge), increasing attraction and decreasing distance by Coulomb’s law.
Define isoelectronic
Having the same number of electrons (though often not protons)
In what direction does electron affinity increase? (ex. top left to bottom right)
up and to the right
Electronegativity
The tendency to pull on an electron in a bond
What changes going right on the periodic table? What changes moving down?
Effective nuclear charge increases right, energy level and thus shielding increases down
Where do metallic and nonmetallic character increase/decrease?
Metallic character increases inversely to nonmetallic character down and left
Name the Fundamental SI units (relevant to what we’ve learned so far) (possibly unnecessary but included just to be safe)
Kg, meter, second, kelvin, mole
What do the prefixes mega, kilo, hecto, deka, deci, centi, milli, micro, and nano mean?
Mega - 1,000,000
kilo - 1,000
hecto - 100
deka - 10
deci - .1
centi - .01
milli - .001 (1 thousanth)
micro - .0000001 (1 millionth)
nano - .0000000001 (1 billionth)
Charges of Ag, Zn, and Cd ions
Ag = +
Zn = 2+
Cd = 2+
