IMFs & gases
Determine who has the smaller boiling points: Cl2 or Br2. Explain in terms of IMFs
Cl2 has a smaller electron cloud making it less polarizable. It's LDFs are weaker due to a more limited polarizability.
What is the angle between the three X atoms that are bonded to Boron in a trigonal planar geometry?
120 degrees
Intra: bonds/ attractions between atoms, holding them together in a molecule
Inter: forces in between two molecules
Determine the concentration of Mg+2 ions in a 2 mole sample of MgCl2 diluted in 500 mL of water.
4 M
Explain in terms of structure, why lithium has a larger radius than an atom of beryllium
lithium has fewer protons therefore a smaller nuclear charge
The total pressure in a gas tube is 800 mmHg. If the vapor pressure at that temperature is 100 mmHg, what is the pressure of the gas collected inside the tube?
700 mg
(800-100)
Determine which species requires greater strength to separate: O2 or Br2.
Oxygen has a higher bond order, with a stronger nonpolar covalent bond.
Identify the conjugate base of HNO2 (aq)
NO2 - (aq)
The plot of 1/x vs. time is a straight line with a positive slope. The order of the reaction must be
2nd order
In addition to the identity and mass of a sample of matter, this value is needed to determine the amount of atoms in the given sample.
Avogadro's number/ mole number/ 6.02 X 10 23
MM = dRT/P
Mg has a +2 charge while Li only has a +1 charge therefore MgO has the greater lattice energy
Explain why Boron would have a significant increase in it's 3rd ionization energy versus the 4th ionization energy: (draw an orbital diagram to support your explanation)
after the third ionization energy, Boron's electrons would have to be removed from a core shell
An experiment with blue dye is conducted using a spectrophotometer. The second experiment is done with red dye. What settings do the students have to adjust before completing experiment 2?
Change the wavelength on the spectrophotometer to be consistent with the optimum absorbance for red color
Explain in terms of structure why Po has a smaller first ionization energy than Se.
Po has additional shells making the farthest available electron more shielded from the nucleus than the valence electron in Se.
When conducting paper chromatography with water as the solvent, the final position of the dye has traveled almost to the opposite end of the paper from its original starting position. What does this suggest about the polarity of the dye? Support your answer by referencing attraction for the stationary phase versus attraction for the mobile phase.
The dye has greater attraction for the mobile phase, which is water and is polar. The dye must be polar. Having attraction for the stationary phase would imply a nonpolar substance.
Explain why a solid ionic substance cannot conduct electricity but in the liquid phase, that same substance can be a good conductor:
only as liquid does it have mobile ions
Explain why Ar(g) specifically deviates more than Ne(g) at high pressure?
The particle volume of Ar is greater than the particle volume of Ne, and therefore the concept of negligible particle volume becomes less likely.
Determine the concentration of Cl-1 ions in a 2 mole sample of MgCl2 diluted in 500 mL of water combined with 2 moles of KCl.
12 M
Determine the wavelength, in meters, of light with photons containing 3.3 x 10-19 J of energy.
6x 10 -7 meters
Explain if NH3 has a lower or higher boiling point than PH3 by identifying all types of imfs in each compound.
NH3 has higher bp due to hydrogen bonding and dipole dipole and LDFs while PH3 only has LDFs and dipole dipole
Give the geometry of the SO3 molecule as well as the bond order:
trigonal planer; 1.3 bond order or 1 1/3
Determine the number of grams of Carbon in a 2.2 grams sample of CO2 (g)
0.6 grams
Overall reaction: 2NO + O2 --> 2 NO2
Step 1(fast) 2NO <-> N2O2
Step 2 (slow) N2O2 + O2 --> 2NO2
Find the rate law
rate= k[NO]2[O2]
Find the energy of a photon of light with a frequency of 6 x 10 -14 s-1 and a wavelength of 510 nm.
4.0 x 10 -19 J