Which of the outrageous claims below is justified?

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Presentation transcript:

Which of the outrageous claims below is justified? (A) MO theory explains important aspects of our immune system. (B) MO theory explains why the sky is blue. (C) MO theory is the basis for the income tax return. (D) MO theory explains evolution. (E) MO theory explains why the sun generates heat.

Which of the outrageous claims below is justified? (A) MO theory explains important aspects of our immune system. … why is N2 inert, but O2 reactive? (B) MO theory explains why the sky is blue. (C) MO theory is the basis for the income tax return. (D) MO theory explains evolution. (E) MO theory explains why the sun generates heat.

Recall how atomic orbitals look like, and that they are labeled with +/- signs. The atomic orbital shown here is a p orbital. Which of the statements below is/are right? (A) The signs stand for charges. The electron is negatively charged, therefore it is in the “-” region. (B) The numerical value of the wave function of the electron is positive in the “+” region, negative in the “-” region. The signs do not make any statement about where the probability of finding the electron is higher. (C) The signs symbolize the phase of the wave function and will actually change over time, where the time dependence is given by e-iEt/ħ. (D) ... (A) and (C) (E) ... (B) and (C)

Recall how atomic orbitals look like, and that they are labeled with +/- signs. The atomic orbital shown here is a p orbital. Which of the statements below is/are right? (A) The signs stand for charges. The electron is negatively charged, therefore it is in the “-” region. (B) The numerical value of the wave function of the electron is positive in the “+” region, negative in the “-” region. The signs do not make any statement about where the probability of finding the electron is higher. (C) The signs symbolize the phase of the wave function and will actually change over time, where the time dependence is given by e-iEt/ħ. (D) ...(A) and (C) (E) ...(B) and (C)

In diatomic molecules, the p orbitals (pu2px, pu2py, pg. 2px and pg In diatomic molecules, the p orbitals (pu2px, pu2py, pg*2px and pg*2py) molecular orbitals constructed by the 2px and 2py AOs are degenerate in energy. They are often collectively labeled as just one set of p orbitals, pu2p, pg*2p. How many electrons can be placed into the pu2p (or the pg*2p) orbital? (A) The atomic 2p subshell can have 6 electrons. Since we have 2 atoms, we can fill 12 electrons into the pu2p orbital. Each atomic 2px and 2py orbital can carry 2 electrons, making a total of 4 per atom. Therefore, the pu2p orbital can have 8 electrons. (C) Each atomic 2px and 2py orbital can carry 2 electrons, making a total of 4 per atom. Since we have to distribute the orbitals into the bonding pu2p orbital and the antibonding pg*2p orbital, the pu2p orbital and the pg*2p orbital can take 4 electrons each. (D) The atomic 2p subshell can have 6 electrons per atom. Since we have to distribute the orbitals into the bonding pu2p orbital and the antibonding pg*2p orbital, the pu2p orbital and the pg*2p orbital can take 6 electrons each.

In diatomic molecules, the p orbitals (pu2px, pu2py, pg. 2px and pg In diatomic molecules, the p orbitals (pu2px, pu2py, pg*2px and pg*2py) molecular orbitals constructed by the 2px and 2py AOs are degenerate in energy. They are often collectively labeled as just one set of p orbitals, pu2p, pg*2p. How many electrons can be placed into the pu2p (or the pg*2p) orbital? (A) The atomic 2p subshell can have 6 electrons. Since we have 2 atoms, we can fill 12 electrons into the pu2p orbital. Each atomic 2px and 2py orbital can carry 2 electrons, making a total of 4 per atom. Therefore, the pu2p orbital can have 8 electrons. (C) Each atomic 2px and 2py orbital can carry 2 electrons, making a total of 4 per atom. Since we have to distribute the orbitals into the bonding pu2p orbital and the antibonding pg*2p orbital, the pu2p orbital and the pg*2p orbital can take 4 electrons each. (D) The atomic 2p subshell can have 6 electrons per atom. Since we have to distribute the orbitals into the bonding pu2p orbital and the antibonding pg*2p orbital, the pu2p orbital and the pg*2p orbital can take 6 electrons each.