chem final
how do u determine the electron domain of a molecule
# of bonding domains+ lone pairs
what is bond order of a molecule that has 2 bonding and 2 nonbonding electrons
0 1/2(2-2)
how many nonbonding electron pairs in PCL3
1
Which increases when a gas is heated at constant volume? 1. Pressure 2. Kinetic energy of molecules 3. Attractive forces between molecules
1 and 2 only
which factors affect the vapor pressure of a liquid? 1. Inter-molecular forces of attraction within the liquid 2. The volume and or surface area of the liquid present 3. the temperature of the liquid
1 and 3
a double bond has how many sigma/pi bonds?
1 sigma, 1 pi
bond angle present in CCl4
109.5
H2O2 in the presence of a catalyst decomposes into water and oxygen gas. How many liters of O2 at STP are produced from the decomposition of 34.0 g of H2O2. 2H2O2 --> 2H2O + O2
11.2
what is C-C-O angle in ethyl acetate (look up image online)
120
When 4.0 L of He (g), 6.0 L of N2 (g), and 10. L of Ar (g) all at 0C and 1 atm, are pumped into an evacuated 8.0 L rigid container, the final pressure in the container at 0C is?
2.5 atm
A gas is most likely to behave as an ideal gas in which instance?
At room temperature and pressure, because inter-molecular interactions are minimized and the particles are relatively far apart
Which compound is most likely to form inter-molecular hydrogen bonds? C2H5OH NaH C4H10 C2H5SH
C2H5OH Think FON
Which is the least soluble in water? CH3OH CH3CH2CH2CH2OH CH3CH2CH2OH CH3CH2CH2CH2CH2OH
CH3CH2CH2CH2CH2OH
Which is the least soluble in hexane (C6H14)? CH3OH CH3CH2CH2CH2OH CH3CH2CH2OH CH3CH2CH2CH2CH2OH
CH3OH
which of the following is not an alloy Brass Steel Ceramic 14 karat gold
Ceramic
When solid carbon dioxide sublimes what IMF must be overcome?
Dispersion forces
A 0.5 mol sample of He (g) of and a 0.5 mol sample Ne (g) are placed separately in two 10.0 L rigid containers at 25C. Each container has a pinhole opening. Which of the gases will escape faster through the pinhole and why?
He (g) b/c they move at a higher average speed than the Ne atoms.
what diatomic molecule did u calculate the bond order of in the previous question
He2
Which of the following is the best explanation for the difference in the boiling points of Cl2 and I2, which are -35C and 184 C
I2 molecules have electrons clouds that are more polarizable than those of Cl2 molecules, thus L
which of the following gases has the highest average molecular speed at 298K? NF3 HBr CO Ne
Ne
Which of the following statements is false? 1. nonpolar liquids tend to be insoluble in polar liquids 2. The weaker the attraction between the solute and solvent molecules, the greater the solubility 3. Substances w similar IMF tend to be soluble 4. Megadoses of water insoluble vitamins, such as A and D can be toxic
The weaker the attraction between the solute and solvent molecules, the greater the solubility
Which is the best indicator of polarity diff in electro negativity symmetry shape all of the above
all
the best explanation for the fact that diamond is extremely hard is that diamond crystals
are giant molecules in which each atoms forms strong covenant bonds with all of its neighboring atoms
what influence does the double bond in cl-c-cl have on its ideal bond angle of 120
becomes less than 120
for molecules w trigonal bypiramidal electron domain geometry which CANNOT be its molecular geometry? linear bent seesaw tshaped
bent
When the energy required to break the ionic bonds is greater than the energy released when the ion-dipole interactions are formed in the solution, the dissolving of the compound is
endothermic
Which of the following are immiscible liquids? CH3CH2OH and water sulfuric acid and water vinegar and water gasoline and water
gasoline and water
review #6 on chpt 12
hard to quizlet:(
study first 2 matching sets on chapter 12
idk how to quizlet those srry
didnt put in chp. 14,,, got lazy
lol srry
according to valence bond theory, covalent bonds form due to
overlapping of orbitals
the hybridization of trigonal planar molecule?
sp^2
In liquids, the attractive IMF are
strong enough to hold molecules relatively close together but not strong enough to keep molecules from moving past eachother
the property responsible for the "beading up" of water is...
surface tension
A vessel contains Ar (g) at a high pressure. Which of the following statements best helps to explain why the measured pressure is significantly greater than the pressure calculated using the ideal gas law? molar mass of Ar is large A significant # of Ar2 molecules form the attractive forces among Ar atoms cause them to collide w the walls of the container w less force the combined volume of the Ar atoms is too large to be negligible compared to the total volume of the container
the combined volume of the Ar atoms is too large to be negligible compared to the total volume of the container
Which statement is true of a measured pressure of nitrogen gas collected over water at constant temperature?
the total measured pressure is greater than the pressure of nitrogen
