1)Which substance ( Ar or F2 ) has the higher boiling point?
Select the two most important reasons below to justify your choice should have the higher boiling point
*Both substances are nonpolar but the higher boiling includes hydrogen bonding *Both substances are nonpolar but the higher boiling is more polarizable
*The higher boiling substance is polar and the other is not
*The lower boiling substance is polar and the other is not
*The higher boiling substance has smaller vander Waals forces than the lower boiling
*The higher boiling substance has greater vander Waals forces than the lower boiling
*The higher boiling substance is ionic and the other is not
*The lower boiling substance is ionic and the other is not
*The higher boiling substance has hydrogen bonds and the other does not The lower boiling substance has hydrogen bonds and the other does not
*Both substances are ionic but the higher boiling has a larger cohesive energy
*Both substances are ionic but the lower boiling has a larger cohesive energy
*The higher boiling substance is ionic and the other is not.
*Ionic bonds are stronger than hydrogen bonds The lower boiling substance is ionic and the other is not.
*Ionic bonds are weaker than hydrogen bonds
*The higher boiling substance is ionic and the other is not.
*Ionic bonds are stronger than vander Waals forces
*The lower boiling substance is ionic and the other is not.
*Ionic bonds are weaker than vander Waals forces
2)Which substance ( HI or Xe ) has the higher boiling point?
Select the single most important reason below to justify your choice should have the higher boiling point
*Both substances are nonpolar but the higher boiling includes hydrogen bonding *Both substances are nonpolar but the higher boiling is more polarizable
*The higher boiling substance is polar and the other is not
*The lower boiling substance is polar and the other is not
*The higher boiling substance has smaller vander Waals forces than the lower boiling
*The higher boiling substance has greater vander Waals forces than the lower boiling
*The higher boiling substance is ionic and the other is not
*The lower boiling substance is ionic and the other is not
*The higher boiling substance has hydrogen bonds and the other does not *The lower boiling substance has hydrogen bonds and the other does not *Both substances are ionic but the higher boiling has a larger cohesive energy
*Both substances are ionic but the lower boiling has a larger cohesive energy
*The higher boiling substance is ionic and the other is not.
*Ionic bonds are stronger than hydrogen bonds
*The lower boiling substance is ionic and the other is not.
*Ionic bonds are weaker than hydrogen bonds
*The higher boiling substance is ionic and the other is not.
*Ionic bonds are stronger than vander Waals forces
*The lower boiling substance is ionic and the other is not.
*Ionic bonds are weaker than vander Waals forces
3)Which substance ( HBr or HF ) has the higher boiling point?
Select the single most important reason below to justify your choice should have the higher boiling point
*Both substances are nonpolar but the higher boiling includes hydrogen bonding *Both substances are nonpolar but the higher boiling is more polarizable
*The higher boiling substance is polar and the other is not
*The lower boiling substance is polar and the other is not
*The higher boiling substance has smaller vander Waals forces than the lower boiling
*The higher boiling substance has greater vander Waals forces than the lower boiling
*The higher boiling substance is ionic and the other is not
*The lower boiling substance is ionic and the other is not
*The higher boiling substance has hydrogen bonds and the other does not *The lower boiling substance has hydrogen bonds and the other does not *Both substances are ionic but the higher boiling has a larger cohesive energy
*Both substances are ionic but the lower boiling has a larger cohesive energy
*The higher boiling substance is ionic and the other is not.
*Ionic bonds are stronger than hydrogen bonds
*The lower boiling substance is ionic and the other is not.
*Ionic bonds are weaker than hydrogen bonds
*The higher boiling substance is ionic and the other is not.
*Ionic bonds are stronger than vander Waals forces
*The lower boiling substance is ionic and the other is not.
*Ionic bonds are weaker than vander Waals forces
dude i got this one
did you got other questions?
Hmmm its Ar HI HF
but what are the reasons
ss01 are you there?
for 3rd
The higher boiling substance has hydrogen bonds and the other does not
for 2d 3 optin
please tell any other ans you got?
Using molecular orbital diagrams of CN- and NO+, solve the following questions
The occupied orbital(s) with the highest energy in CN- is(are)
1.sigma-2s
2.sigma*-2s
3.sigma-2p
4.pi-2p
5.sigma*-2p
6.pi*2p
The occupied orbital(s) with the highest energy in NO+ is(are)
1.sigma-2s
2.sigma*-2s
3.sigma-2p
4.pi-2p
5.sigma*-2p
6.pi*2p
Which of these two molecules has the longer bond length?
1.NO+
2.CN-
3.they have equal length
1#6
2#6
3#1
I think so
answer for
Using molecular orbital diagrams of CN- and NO+, solve the following questions
The occupied orbital(s) with the highest energy in CN- is(are)
1.sigma-2s
2.sigma*-2s
3.sigma-2p
4.pi-2p
5.sigma*-2p
6.pi*2p
The occupied orbital(s) with the highest energy in NO+ is(are)
1.sigma-2s
2.sigma*-2s
3.sigma-2p
4.pi-2p
5.sigma*-2p
6.pi*2p
Which of these two molecules has the longer bond length?
1.NO+
2.CN-
3.they have equal lengt
sigma-2p
sigma-2p
CN-
right answers
The pi-2p orbitals are lower in energy than the sigma-2p in NO+ because of nitrogen, so they fill before the sigma-2p. The same configuration applies to CN- because both carbon and nitrogen are small atoms.
The 2s and 2p orbitals on carbon are higher in energy than on oxygen. Thus, the pi-2p and sigma-2p bonding orbitals in CN- are higher in energy. This means the bond strength of CN- is less than NO+, resulting in a longer bond length for CN-
What were your answers for these ones?
Determine the minimum potential that must be applied to a proton so that, on interaction with a hydrogen atom, it can excite the ground state electron to a state of n=5
Electron exhibiting a particle wavelength of 5.84 x 10-9 are emitted from hydrogen atoms after interaction with high energy photons. Assuming that the electrons in the hydrogen atom were in their ground state prior to interaction, determine the wavelength of the photon which generated the free electrons
Why is the Ge-F bond energy so much more than the Ge-Cl bond energy?
Covalent bond energies generally increase as you go down the periodic table Covalent bond energies generally decrease as you go down the periodic table The Ge-F bond is more polarizable than the Ge-Cl bond The Ge-F bond is more ionic than the Ge-Cl bond The Ge-F bond is more covalent than the Ge-Cl bond The Ge-F has a smaller dipole moment than the Ge-Cl bond
Why do the bond energies decrease in the order Ge-Cl, Ge-Br, Ge-I?
Covalent bond energies generally increase as you go down the periodic table Covalent bond energies generally decrease as you go down the periodic table Ionic bond energies generally decrease as you go down the periodic table Ionic bond energies generally increase as you go down the periodic table The polarizability of bonds generally decreases as you go down the periodic table The polarizability of bonds generally increases as you go down the periodic table