The Pauli Exclusion Principle tells us that no two electrons in an atom can have the same four quantum numbers. For an electron in the 2p orbital shown above, enter a possible value for each quantum number. n Give ONE example. m, = Give ONE example. Though a given electron only has one value for my, there are ( m¡ = Submit Answer possible my values for electrons in 2p orbitals. Retry Entire Group 9 more group attempts remaining

The Pauli Exclusion Principle tells us that no two electrons in an atom can have the same four quantum numbers. For an electron in the 2p orbital shown above, enter a possible value for each quantum number. n Give ONE example. m, = Give ONE example. Though a given electron only has one value for my, there are ( m¡ = Submit Answer possible my values for electrons in 2p orbitals. Retry Entire Group 9 more group attempts remaining

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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a This question uses He to explore the ability of one electron to shield another from the positive charge of the nucleus. The ionization of an atom not experiencing shielding can be calculated from Bohr's equation for the electron energy. E = - (N₁Rhc) (Z²/n² where N₁ Rhc = 1312 kJ/mol and Z is the atomic number. Use this approach to calculate a possible ionization energy for helium assuming the electrons of the He experience the full 2+ nuclear charge. This gives us the upper limit for the ionization energy. Ionization energy = kJ/mol
Following successive ionization energies (IE in kJ/mol) are for which atom? IE1 = 1085 IE2 = 2355 IE3 = = 4620 IE4 = 6225 IES = 37830 %3! %3D Toan Не 1000 gen egm hore 10 Li Be N F Ne maetn 12 odm 11 13 14 15 16 17 18 Na Mg Al Si cI Ar 2430 200 3200 TOFIE 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 к Са Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te Хе ar Sate 56 atan 72 81 55 57-70 71 73 74 75 76 77 78 79 80 82 83 84 85 86 Cs Ba Lu Hf Ta W Re Os Ir Pt Au Hg TI Pb Bi Po At Rn 87 88 89-102 103 104 105 106 107 108 109 110 111 112 114 Fr Ra ** Lr Rf Db Sg Bh Hs Mt Uun Uuu Uub Uuq 57 58 63 64 65 *Lanthanide series La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb 1413 1 tie 1734 **Actinide series 92 95 96 97 100 101 102 Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Select one: O a. o b. Al O. P o d. Be O e. C
b) Given the set of quantum numbers for highest energy electrons in atom Y as shown below:(n, l, m, s)(2, 1, -1, +1/2)(2, 1, 0, +1/2) i. Draw the complete orbital diagram of atom Y.ii. How many unpaired electrons would be found?
Give only typing answer with explanation and conclusion 1. How many degenerate orbitals are in each of the following subshells? (Enter 0 if there are none.) a) n = 6, l = 0 2. Identify the subshell in which electrons with the following quantum numbers are found. (Enter your answers in the format 1s, 2p, etc.) a) n = 6, l = 4 b) n = 2, l = 0 c) n = 4, l = 3
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O Empower 2021 acatinykt.cnc neaCNiEIDENT BASEIOME CONTROL arks EL IXI Classes O Google Slides O Empower 2020 Google Docs s č Lindsay High SchoolR Physics Safety & Ski. E Guided practice 10 Vop lath by The La see she A Am Cm -- Fa Why does it take more energy to remove an electron from elements higher on the perlodic table? Higher on the periodic table the atoms have fewer rings, electrons are closer to the nucleus and held more tightly, so harder to O A. remove OR Higher on the periodic table the atoms have more rings, electrons are further from the nucleus and not held as tightly, and easier OB. to remove. OC. LOwer on the periodic table the atoms have more rings, electrons are closer to the nucleus and easier to remove. O D. Lower on the periodic table the atoms have more rings so electrons are harder to remove. Score Now Finish Later DELL F3 F4 FS Fア F8 F10 F11 Priscr F9 2# $ & 4 5 6 E T K 11 zi
D. Give the quantum numbers for the last electron of each element given in Part II following the table below. Element 1 subshell N - 7 1s22s22p3 70 Ga,17⁰ Ar 1840 Sb,1122 112 AU79197 n main energy level 2 s=0 p=1 d=2 f=3 1 m₁ orbital -1 to 0 to +1 -1, 0, +1 +1 m₂ magnetic spin (+1/2, -1/2) +1/2
3. A student was asked to write the electron configuration for a number of elements on an exam. Here is a sample of some of their answers: a) Ne s2 b) 1s²25³ c) [Kr] 4s1 Select any 2 of the answers above, and explain what is wrong. What element do you think they were describing? Write the correct electron configuration for that element.
Would you be able to fill in table 1?
please solve question 1 and 2, thanks alot sir
The Pauli Exclusion Principle tells us that no two electrons in an atom can have the same four quantum numbers. In progress For an electron in the 3s orbital shown above, enter a possible value for each quantum number. n = 1 = = Give ONE example. Give ONE example. Though a given electron only has one value for possible mi, there are my values for electrons in 3s orbitals. m₁ = ms = Submit Answer Retry Entire Group 9 more group attempts remaining
I which will form an ion with ä ctl charge? 3iunsi I ) Note: All eiements äte in the came period ( periad a) o 12 Nais 18 Ar40 7A a cl b. Al C Na d. Ar mumixom 2: Which of the following set Of quantum numbers is Impossible for any element to have? 0 This is an all-or-nothing queion- Either you get all four corre ct, or you get no points at all. to %3D m= 5´;s= - '/2 %3D to m=D3 %3D %3D m 3D0 h.n= 5 1= 2 m =2