1) Which of the following statements is correct for an electron that has the quantum numbers n = 4 and ml = -2? A. the electron may be in a p orbital B. the electron may be in a d orbital C. the electron is in the second principal shell D. the electron must have a spin quantum number ms = + ½ 2) The set of quant
Explain how the attraction that the nucleus exerts on an electron changes, with the principal energy of the electron.
Which of the following is true? A. The 3s level in hydrogen has a lower energy than the3d level in hydrogen. B. The 4s level in multielctron atoms is equal in energy to the 3d level in multielectron atoms. C. The 2s level in multielectron atoms has a greater energy than the 2s level in hydrogen. D. The 2s level in multiele
Whichis not true? A. In the hydrogen atom, all subshells of a principle shell are at the same energy level. B. Orbital energies are higher in multielectron atoms than in hydrogen atomes. C. In a multielectron atom, the various subshells of a principle shell are at a different energy levels. D. All orbitals within a subshel
Each element has a different set of energy levels. Explain why the colour of the light emitted by an element in the gaseous state is characteristic of the element & explain with a sketch diagram how a hydrogen atom, which has only one electron, has so many spectral lines.
1. Give the number of electrons, Protons and neutrons in 24NA (small 24 to the top) 2. Give the electron configuration of the following A: A1 B: F- (- is at the top) 3. Give a set of four quantum numbers that describe the last electron to be placed in the electron configuration of the following atoms. A: Ar B: Rb C
Calculate the first-order correction to the ground-state energy of a particle in a three dimensional box with the perturbation: H^1 = V in the range a/4 < x < 3a/4, b/4 < y < 3b/4 , c/4 < z < 3c/4 where H^1=0 otherwise V=hv (See attached file for full problem description)
Set up your own character table for the ammonia molecule and use it to determine the number and kinds of infrared and Raman active bands predicted by GOT. Make the C3 operation along the z axis. (See attached file for full problem description)
Set up the secular determinant for benzene pi electrons as done in class for ethene. Label the energy level diagram shown below with the correct terms in alpha and beta. (See attached file for full problem description and diagram)
#1 You dissolve 12.6352 g of potassium iodide in water and bring the volume of solution to 250.0 ml. What is the molar concentration of KI? #2 What volume of 0.0436 molar hydrochloric acid is required to react with 30.0 ml of 0.0278 molar LiOH? #3 An AM radio station broadcasts using electromagnetic radiation at 1490 kiloh
Write electron configurations and count the number of unpaired electrons in: O, Si, Ni, I, Ir, Bi, Gd
2. For each of the following orbitals, provide a perspective sketch of the orbital in the Cartesian x, y, z coordinate system. Determine the number of angular nodes and the number of radial nodes in the orbital, and describe where those nodes fall. For instance, the 2px orbital has an angular node in the yz-plane. a) 1s b)
I need some help in determining the number of protons and the number of neutrons in the nucleus of the following atoms and the number of electrons in their first and quantum shells: 10/5B 14/6C 3/2He 40/19K 16/8O
Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si and Ar? a. Si > P > Ar > Na > Mg b. Ar > Si > P > Na > Mg c. Ar > P > Si > Mg > Na d. Mg > Na > P > Si > Ar e. Na > Mg > Si > P > Ar A tin atom has 50 electrons. Electrons in the ___________ subshell experience the lowest effecti
Hi, I need some assistance with the following questions: In the Bohr model of the atom, _____. a) electrons travel in circular paths called orbitals b) electrons can have any energy c) electron energies are quantized d) electron paths are controlled by probability e) both a and c The de Broglie wavelength of a bullet
1) Of the following transitions in the Bohr hydrogen atom, the __________ transition results in the emission of the highest-energy photon. a. n = 3 -> n = 6 b. n = 6 -> n = 3 c. n = 1 ->n = 4 d. n = 6 ->n = 1 e. n = 1 ->n = 6 2) The frequency of elect
Question 6 True/False 20 points The number of electrons in orbital 5f6 is 5 electons. True False Question 7 Multiple Choice 20 points Beginning at Argon, Ar, the electron configuration of a Copper atom (Cu) is: [Ar]4s24d4 [Ar]4s24p63d3 [Ar]4s23d7 [Ar]3d104s1 Question 8
A) Write one set of quantum numbers for an electron in that orbital 4d 5p B) Sketch picture of orbital. C) List an element whose outer most electron occupies this orbit. Also: Write one set of quantum numbers for the 2d orbital. I was told that it cannot happen - Why? n=2, l=0,1,2,msubl = 0, -1,0,1, -2...........
1. When an electrical discharged is passed through hydrogen gas, a unique four line spectrum is observed. One of the two blue wavelengths is observed at 411 nm. Calculate the frequency of this blue line. {See attachment for multiple choice options} 2. Calculate the engergy if 3 moles of photons are produced if the frequency o
An aqeuous solutino of Ni(No3)2 is green. Addition of aqueous solution Nh3 causes the color of the solution to change blue. If the ethylenediamine is added to the green solution, the color changes to violet. What causes the colors of these complexes? How do these colors relate to the expected positions of these ligands in the sp
For the isoelectronic series[V(CO)6]-, Cr(CO)6, and [Mn(Co)6]+, does the energy of the metal to ligand charge-transfer bands increase or decrease with increasing charge on the complex? Why?
1. Why is the peroxide anion such a strong oxidizing agent? 2. Describe qualitatively how the conclusions of Bohr and Rydberg are essentially the same? 3. Which property of the hydrogen atom does the Zeeman Effect illustrate? Explain this.
Elements in the first short period are limited by the octect rule whereas those in the higher period can expand their valence shells. Describe what this means, account for this phenomenon and give an example of each.
Consider the electronic structure of the element bismuth. a) The first ionization energy of bismuth is Ei1 = +703 kJ / mol. What is the longest possible wavelength of light that could ionize an atom of bismuth? b) Write the electronic configurations of neutral Bi and Bi+ cation. c) What are the n and l quantum numbers of the
Which of the following combinations of quantum numbers can refer to an electron in a ground-state cobalt atom (Z=27) ? a) n = 3, l = 0, m1 = 2 b) n = 4, l = 2, m1 = -2 c) n = 3, l = 1, m1 = 0
How would I find/identify the expected electron configuration for: Cr3+, Au3+, Ru2+ Cu+, Mn4+, and Ir3+?
An electron microscope employs a beam of electrons to obtain an image of an object. What energy must be imparted to each electron of the beam to obtain a wavelength of 10.0pm? Obtain the energy in electron volts (eV) (1eV= 1.602x10^-19J )
For each line in the hydrogen spectrum, how do you deduce n2 (the upper state) and n1 (lower state)? If you could record the absorption spectrum of hydrogen gas, what would it look like? What is the vapour (or gas) present in fluorescent lights? How do you know?
Write the electron configurations for Mg and Ar, using both the spdf notation and orbital box diagrams. Describe the relation of the atom's electron configuration to its position in the periodic table. electron configuration for Mg___________ spdf____________________ orbital box diagram: electron configuration for A
If energy is absorbed by a hydrogen atom in its general state, the atom is excited to a higher energy state. For example, the excitation of an electron from the level with n=1 to the level n=3 requires radiation with a wavelength of 102.6 nm. Which of the following transitions would require radiation of longer wavelength then