CHM 11500 Lecture Notes - Lecture 10: Electron Configuration, Probability Distribution, Bohr Model

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CHM 11500 Full Course Notes

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Chm 115 - lecture 10 - quantum theory continued. Electron energies are quantized, this is what causes them to only inhabit constrained orbitals. Electrons moving from one orbital to another requires the absorption of energy (when moving to a higher energy orbital) or the release of energy (when moving to a lower energy orbital) Electrons fill orbitals in order of increasing energies. Each orbital can contain up to two electrons. Two electrons sharing an orbital must have opposite spins. Spins are indicated by spin quantum number, which has values of + or. In a set of orbitals (e. g. 2s, 2p, 3d) each orbital must have one electron in it before any orbital can have two. The above diagram of the periodic table can be used to determine the electron configuration of different elements. Electrons fill orbitals according to the rows in this version of the table.

Related Questions

A--Galena (also known as lead (II) sulfide) is the ore from which elemental lead is extracted. In the first step of the extraction process, galena is heated in oxygen to form lead (II) oxide and sulfur dioxide.

--Write a balanced equation for the reaction. (2 points)
--What mass of galena is converted to lead (II) oxide if 975 kJ of heat is produced? (3 points)

B--Tungsten(VI) oxide reacts with hydrogen gas (H₂) to produce tungsten metal and water vapor. The equations below represent the enthalpy change for the formation of the two compounds from their elements.

2 W (s) + 3 O₂ (g) ---> 2 WO₃ (s) ÎH = -1685.4 kJ

2 H₂ (g) + O₂ (g)---> 2 H₂O (g) ÎH = -477.84 kJ

--Write a balanced equation for the reaction. (1 point)

--What is the enthalpy change for the overall reaction written in (a)? (4 points)

C---An important step in the synthesis of nitric acid is the reaction of ammonia (NH₃) and molecular oxygen to form nitrogen monoxide gas and water vapor.

--Write a balanced equation for this reaction. (2 points)

--Calculate DH^o for this reaction, using standard heat of formation values from Appendix G in the Open Stax Chemistry text. (3 points)

D----When an electron in a 2p orbital of a particular atom makes a transition to the 2s orbital, a photon of approximate wavelength 629.1 nm is emitted. What is the energy difference between these 2p and 2s orbitals?

E---Provide a numerical value (whole number) for each of the following questions. Briefly explain your reasoning (1 point each).

How many electrons can be contained in all of the orbitals with n = 4?

Among the orbitals with n = 4 (see part a), which one has the highest energy and how do you know this?

What is the l quantum number for a 4s orbital?

How many electrons can be described by the quantum numbers n = 3, l = 3, m_l = 1?

l = 3, how many electrons can be contained in all the possible orbitals of a given principal quantum number?

Are these correct? And how do you do #5 and #6?

CHM 11500 Lecture Notes - Lecture 10: Electron Configuration, Probability Distribution, Bohr Model

CHM 11500 Full Course Notes

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