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- As an alternative to "metal oxides," some sunscreens utilize "organic" (carbon-based) ingredients such as oxybenzone: 22. 6 HC 12 || HC :O: CH HC. HỌ: How many of the atoms in oxybenzone have electrons in unhybridized ("pure") p orbitals? 04 2 14 CH CH3 16Write out the ground-state electron configurations of Ti3+.Which of the following is the ground state electron configuration of a phosphorus atom? O [Ar]4s? O [Ne]3s²3p3 O [Ar]4s*3d1 O [Ne]3s? O [Ar]3d?
- Describe the shape of a 5p, orbital. O three balls O six balls O spherical dumbbell shaped O four ballsalthough we associate Pz 2. Now we will move on to diatomic molecules. In atoms all p-orbitals are equivalent with m/= 0, and px py with m/= ±1. In diatomic molecules these orbitals are in fact separated, with pz associated with o orbitals along the internuclear axis and px py associated with л orbitals (m/= ±1). In determining electron configurations we do indeed separate them: N₂ (KK¹ 0₂²). and O2 (KKogu ng *2). 4 a. Two excited states of N₂ are associated with Tu transitions. Tg and og → ou* i. Draw the MO energy level scheme (p-orbitals only) for the N₂ ground state and for these two excited states. ii. Obtain the term symbols for the two excited states and order them according to Hund's rules. iii. Write the wave functions for each of the terms obtained in ii) above. iv. Pick one wave function from each excited state and show it obeys the Pauli Principle.What is the ground-state electron configuration of the valence electrons ofiodine molecules (I2)? Is iodine paramagnetic or diamagnetic?
- What is the ground-state electron configuration of the sulfide ion S2−S2−? Express your answer in condensed form, in order of increasing orbital energy. For example, [He]2s22p2[He]2s22p2 should be entered as [He][He]2s^22p^2 .Give the ground-state electron configurations of (i) XeF, (ii) PN, and (iii) SO−.Photoelectron spectroscopy applies the principle of the pho-toelectric effect to study orbital energies of atoms and mol-ecules. High-energy radiation (usually UV or x-ray) is absorbedby a sample and an electron is ejected. The orbital energy can becalculated from the known energy of the radiation and the mea-sured energy of the electron lost. The following energy differ-ences were determined for several electron transitions:ΔE 2→1=4.098X10⁻¹⁷J, ΔE 3→1=4.854X10⁻¹⁷J, ΔE 5→1=5.242X10⁻¹⁷J, ΔE 4→2=1.024X10⁻¹⁷J Calculate the energy change and the wavelength of a photon emitted in the following transitions:(a) Level 3→2 (b) Level4→1 (c) Level5→4