Which of the following atoms, in its ground state, does not have unpaired electrons? (Select all that apply.)
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Chemistry
- E) None of these represent the system referenced above. 48) 48) Which of the following quantum numbers describes the size and energy of an orbital? A) spin quantum number B) magnetic quantum number C) principal quantum number D) Schrödinger quantum number E) angular momentum quantum number 49) 49) What value of l is represented by a d orbital? A) 2 B) 0 C) 1 D) 3 50) 50) Calculate the wavelength of light associated with the transition from n=1 to n 3 in the hydrogen atom. B) 136 nm ) 971 nm D) 103 nm E) 646 nm A) 155 nmarrow_forwardWhich of the following điagrams represents orbitals spinning the Py subleve1? 30. a) c) X- y b) d) ofarrow_forward3) Electrons are filled in various sub-shells from higher energy to lower energy. Select one: True Falsearrow_forward
- 41) Why is an atom's second ionization energy always larger than its first ionization energy? Select all that apply. a) Removing the second electron involves pulling it away from a greater positive charge. b) The second electron removed is under a greater effective nuclear charge than the first electron removed. c) The second electron removed is much further away from the nucleus than the first electron removed. d) None of these.arrow_forwardOutcome • Demonstrate a working knowledge of the Bohr model in determining orbital radii and energy levels for electrons. (Outcome 1) Apply the quantum numbers to analyze the electron configurations for any atom, and relate the structure of the Periodic Table with Pauli's exclusion principle. (Outcome 2) • Explore x-ray production and the properties of a laser. (Outcome 3)arrow_forward10. Select the correct statement for n-5 Orbitals Electrons 10 a) b) 25 c) 10 d) 50 20 16 32arrow_forward
- a) Zn b) Mn Which orbital notation correctly represents the outermost principal energy level of a sulfur atom in the ground state? 27. P. a) b) c) d) 1k 1 28. In the electron dot symbol the dots represent electrons b) p sublevels, only d) s, p, and d sublevels located in a) s sublevels, only c) s and p sublevels, only sS units (u) that are based onarrow_forwardLabel each of these orbital designations as “possible” (exists) or “impossible” (does not exist). a) 1s b) 2s c) 1p d) 2p e) 2d f) 3d The answer: a) possible, b) possible, c) impossible, d) possible, e) impossible, f) possible? Can you help me, please?arrow_forward13: Which of the following statements is correct about the effective nuclear charge (Zeft)? A) Zeff increases with increasing the size of the atom. B) Zefrdecreases across a period and increases down a group. C) Zefr increases across a period. D) None of themarrow_forward
- Consider an oxygen atom. Which of the following electron orbitals would be unused for a ground state atom? a) 2s b) 2p c) 1s d) 3parrow_forwardWhich values of me are possible within the 4s subshell? [Select all that apply.] 4+ 3+ 2+ 1+ 1- 2- 3- 4-arrow_forward17) Sometimes, 4s orbital has slightly lower energy level than the 3d orbital. The reason is: a) The number of n+l for 4s is lower b) The I for 4s is lower c) 4s has more angular nodes than 3d d) 4s has more angular nodes than 3d 18) In the two elements P and S, the ionization energy varies as follows: a) Pis higher b) S is higher c) The two have exactly same values d) We cannot tell Part II: 19) Based on Pauling studies on the molecule H-F: a) Which Bond Energy is higher the theoretical or the experimental value? b) Why? (shirt answer only) (a) (b) 20) Consider the two systems i) I ion and ii) H2O2 molecule a) Draw the correct molecular geometries for each system b) On each system draw all symmetry operations c) For each system, write down the Symmetry Point Group (ii) ()arrow_forward
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