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Three of the term symbols that correspond to a nd3 electron configuration are 2P, 2F, and 4P. Rank these in terms of increasing energy.
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- Write out the ground-state electron configurations of Ti3+.Pauli exclusion principle specifies that each (1) can hold (2) two electrons, which must have (3) spins. (1) = electron state, (2) = more than, (3) = opposite. (1) = subshell, (2) = more than, (3) = the same. (1) = electron state, (2) = no more than, (3) = opposite. (1) = subshell, (2) = no more than, (3) = opposite.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?
- An atom Q has six valence electrons and forms a stable Q3+ ion. What is the electronic configuration of atom Q?Write the full ground state electron configuration of O2+. electron configuration:Use the periodic table to (i) predict electron configurations for the following species: Arsenic ion, As3– Magnesium ion, Mg2+ Vanadium(II) ion, V2+ (ii) Write the electron configurations of each species in the noble gas notation. (iii) Draw an orbital diagram to represent 1 c above. Draw the Lewis electron dot structures of the following chemical species. In each case you must say whether or not the central atom obeys the Octet Rule. CS2 and H2S CF4 and SiH4 NH2Cl CO32– and BF3 PCl5 ClF3, XeF2, Calculate the formal charge on the Sulphur atom in the Sulphate anion structure shown below(picture attatched) Give the electron-pair and molecular geometries for NF3 and XeF4.
- although 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.The gadolinium +3 ion (Gd3+) has advantageous magnetic properties for Magnetic Resonance Imaging (MRI) applications, specifically a high number of unpaired electrons. In fact, both neutral Gd and Gd3+ have a set of degenerate orbitals with seven unpaired electrons. a) Write the electron configuration for Gd and Gd3+ using the condensed noble gas notation. Identify which orbitals lose electrons to yield the +3 cation based on the above information. Explain your reasoning (2-3 sentences). b) Curium (Cm) is an actinide element named for Marie Curie. Cm is in the same group as Gd and also forms a +3 cation. Write the electron configuration for Cm and Cm3+. c) While +3 is the most common oxidation state for lanthanide elements, some can form +2 ions. Identify an isoelectronic ion to Gd3+ that has a +2 oxidation state and indicate which orbitals lose electrons to form that ion.The change in energy for which of the following processes corresponds to the firstionization energy of bromine?Br2(g)→ 2Br(g) Br(g) + e-→ Br-(g) Br+(g) + Br-(g) → Br2(l)Br(g) → Br+(g) + e- Br-(g) → Br(g) + e-