• View Available Hint(s)configurations.Reset Helpomic orbitals. Electron configurations can be目日11 11s2s2p3s3pn of an element. Orbital diagrams are filled usings are added to an orbital diagram one at a time toowever, due to shielding of the nucleus, the- orbital is lower in energy than the 3d orbital forrbitals, draw a diagram (Figure 1)with the energylevel across in rows, with each row offset by oneFll, read the diagram from top to bottom, left toed the "aufbau order."1Gt G1G1G1 G1 G11s282pG2G2ue of all four quantum numbers (n, l, mi, and m).is 1s. The fourth quantum number (m;) specifiesd3 p:), for a total of up to six electrons in a given pconsists of seven separate orbitals.), only two electrons can occupy any givenom is one having the maximum number of electronsegin to fill a p subshell (which consists of threenergy configuration consists of one electron in each pPrevious Answersv CorrectPart BComplete an orbital diagram for scandium (Sc)Drag the appropriate labels to their respective targets. Labels can be used once, more than once, or not at alI.> View Available Hint(s)ResetHelp1125203s3p3d4s4p151L11 1L 111111 11 11G1 G1 G1 G111152s2p353p453dPrevious Answersv CorrectPart CElectron configurations are a shorthand fom of an orbital diagram, descrting which orbita are accupied for a given sloment For ssample La 2 2p is the electron configuration of boronEnter the complate electron configuration for arsenic (As)Express your answer in complete lom in the order of orbital filling es a suing without blank space beteeen orbitals. For example, 1s should be entered as 1s 22s 2.> View Available Hintis)< 1 of 1paSubmit Electron configurations are a shorthand form of an orbital diagram, describing which orbitals are occupied for a given element. For example, 1s 2s 2p is the electron configuration of boron.Enter the complete electron configuration for arsenic (As).Express your answer in complete form in the order of orbital filling as a string without blank space between orbitals. For example, 1s22s? should be entered as 1s^22s^2.• View Available Hint(s)

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Reset Help Previous Answer v Correct • Part B Complete an orbital dagram for scandium (Sc) Drag the appropriate labels to their respective targets. Labels can be used once, more than once, or not at all. View Available Hints) Reset Helo 11 1 he s * Corect Part C cond n ot h Eledn conigations are a shothnd fu of an l degam des g wh coed r e for Le2 Ente the cample coiro a A Express your an complte oin e der of urbal ng en ng wout kspce bete orale For emle, le'esde dan V lle 1of1 Submal

Reset Help Previous Answer v Correct • Part B Complete an orbital dagram for scandium (Sc) Drag the appropriate labels to their respective targets. Labels can be used once, more than once, or not at all. View Available Hints) Reset Helo 11 1 he s * Corect Part C cond n ot h Eledn conigations are a shothnd fu of an l degam des g wh coed r e for Le2 Ente the cample coiro a A Express your an complte oin e der of urbal ng en ng wout kspce bete orale For emle, le'esde dan V lle 1of1 Submal

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter11: Modern Atomic Theory

Section: Chapter Questions

Problem 126CP

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Similar questions

Construct an energy level diagram showing all orbitals for the hydrogen atom up to n=5, labeling each orbital with its appropriate quantum numbers. How many different orbitals are in each shell?
What evidence do we have that energy levels in an atom are quantized? State and explain the evidence.
Discuss briefly the difference between an orbit (as described by Bohr for hydrogen) and an orbital (as described by the more modern, wave mechanical picture of the atom).
Quantum mechanics predicts that the energy of the ground state of the H atom is 13.6eV . Insight into the magnitude of this quantity is gained by considering several methods by which it can be measured. (a) Calculate the longest wavelength of light that will ionize H atoms in their ground state. (b) Assume the atom is ionized by collision with an electron that transfers all its kinetic energy to the atom in the ionization process. Calculate the speed of the electron before the collision. Express your answer in meters per second (ms1) and miles per hour (milesh1) . (c) Calculate the temperature required to ionize a H atom in its ground state by thermal excitation. (Hint: Recall the criterion for thermal excitation of an oscillator in Planck’s theory of blackbody radiation is that hvkBT .)
The first ionization energy of helium is 2370kJmol1 , the highest for any element. (a) Define ionization energy and discuss why for helium it should be so high. (b) Which element would you expect to have the highest second ionization energy? Why? (c) Suppose that you wished to ionize some helium by shining electromagnetic radiation on it. What is the maximum wavelength you could use?
The outermost electron in an alkali-metal atom is sometimes described as resembling an electron in the corresponding state of a one-electron atom. Compare the first ionization energy of lithium with the binding energy of a 2s electron in a one-electron atom that has nuclear charge Zeff , and determine the value of Zeff that is necessary for the two energies to agree. Repeat the calculation for the 3s electron of sodium and the 4s electron of potassium.
When metallic sodium is dissolved in liquid sodium chloride, electrons are released into the liquid. These dissolved electrons absorb light with a wavelength near 800 nm. Suppose we treat the positive ions surrounding an electron crudely as defining a three-dimensional cubic box of edge L, and we assume that the absorbed light excites the electron from its ground state to the first excited state. Calculate the edge length L in this simple model.
r Questions 11—13, you will need to consider ionizations beyond the first ionization energy. For example, the second ionization energy is the energy to remove a second electron from an element. Compare the first ionization energy of helium to its second ionization energy, remembering that both electrons come from the 1s orbital. l> X Y First 170 200 second 350 400 Third 1800 3500 fouth 2500 5000 entify the elements X and Y. There may be more than one answer. so explain completely.
Suppose that the spin quantum number could have the values 12,0 and 12 . Assuming that the rules governing the values of the other quantum numbers and the order of filling sublevels were unchanged, (a) what would be the electron capacity of an s sublevel? a p sublevel? a d sublevel? (b) how many electrons could fit in the n=3 level? (c) what would be the electron configuration of the element with atomic number 8? 17?
Although we may draw the 4s orbital with the shape of a ball, there is some probability of finding the electron outside the ball we draw. Is this statement true or false? Comment on this statement.
Until recently, it was thought that Ca was unstable, and that the Ca atom therefore had a negative electron affinity. Some new experiments have now measured an electron affinity of +2.0kJmol1 for calcium. What is the longest wavelength of light that could remove an electron from Ca ? In which region of the electromagnetic spectrum does this light fall?
6.47 Depict two ways to place electrons in the 2p orbitals for a nitrogen atom. Which depiction is correct according to Hund’s rule?