Show:
Light and Energy
Electron Configurations
Trends
Quantum Mechanics
Bonding
100
The type of radiation which has a lower frequency than UV-Vis and a shorter wavelength than Infrared.
What is Visible light/radiation?
100
1s2 2s2 2p6 3s2 3p4
What is the electron configuration of sulfur?
100
The four trends which increase up a group and left to right across a period.
What are the trends for Electron Affinity, Ionization Energy, Electronegativity and Effective Nuclear Charge?
100
The elements whose last electron is described by these four quantum numbers: n=3 l=1 ml=-1 ms=-1/2
What is the last electron to fill sulfur's orbitals?
100
The amount of lone pairs on the nitrogen in ammonia
What is one lone pair?
200
The most polar of the following bonds (and why): H-O, C-O, C-F and N-S
What is C-F due to the largest change in electronegativity?
200
[Ar] 3d5 4s1
What is the electron configuration of chromium?
200
This element has a higher electronegativity than bismuth (Bi) and a smaller radius than tin (Sn).
What is Antimony (Sb)?
200
The number of electrons which can satisfy these quantum numbers: n=2 ml=-2
What is no electrons. At n=2, the only possible ml values are -1, 0 and +1.
200
A drawing of the Lewis structure of XeF2OH
What is 2 lone pairs on Xe and no double bonds? [(::)(F)(F)(OH)(Xe); 28e-]
300
This is why magnesium has a higher ionization energy than aluminum. (733 kJ/mol vs. 577 kJ/mol)
What is a full s-orbital in magnesium versus a lone p-electron in aluminum? (The s-orbital is completely satisfied and thus harder to break apart.)
300
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f1 5d1
What is the electron configuration of lanthanum?
300
The ion with the largest radius in the series Bi3-, Po2-, At-, Rn, Fr+, Ra2+
What is Bi3-? (All isoelectronic. Bismuth has the least amount of protons.)
300
The four quantum numbers describing the last electron to fill platinum's orbitals. (Hint: Pt is an exception to the rule!!)
What is n=5, l=2, ml=1, ms=-1/2? (The electron config. is 5d9)
300
The amount of lone pairs on As in [AsCl3] 2-
What is 2 lone pairs?
400
The frequency (in Hz) a hydrogen atom would emit when an electron transitions from ground state to the third energy level. (Remember to account for whether it is emission/absorption.)
What is 2.93x10^15 Hz?
400
The noble gas electron configuration of antimony (III).
What is [Kr] 5s2 4d10 that is deficient 3 electrons?
400
The terms referring to the total positive charge experienced by an atom or electron when the effect of shielding is taken into account, and the amount of energy a neutral atom or molecule releases when an electron is added to it.
What is effective nuclear charge and electron affinity?
400
The number of electrons in the complete valence shell of Sm3+ and the quantum numbers of the last electron in that shell.
What is 7 electrons and n=5, l=1, ml=0, ms=-1/2? (6s1, 6s2 and 5p6 are lost. The last electron becomes 5p5.)
400
The formal charges on each atom in the molecule [ClF2] +
What is 0 on each F and +1 on Cl?
500
The compound with the highest lattice energy out of the following (and why): MgO, CsI, CaO and LiI
What is MgO? (Due to the highly charged, small atoms. The trend is CsI<LiI<<<CaO<MgO)
500
There are these many electrons on the fourth energy level of erbium (Er).
What is 30 electrons?
500
The total effective nuclear charge experienced by the complete 4th energy level of molybdenum (Mo). (Hint: It might help to first write out the configuration and draw a model like we did in class)
What has an effective nuclear charge of 14?
500
The sets of Quantum numbers for the first four electrons hafnium ,Hf, loses when it ionizes. (In the order they are lost)
What is 1) n=6, l=0, ml=0, ms=-1/2 2) n=6, l=0, ml=0, ms=1/2 3) n=5, l=2, ml=-1, ms=1/2 4) n=5, l=2, ml=-2, ms=1/2
500
The amount of double and triple bonds in the compound CHCCH2CHCHCH2CHCHCCCHCH2
What is 3 double bonds and 2 triple bonds?