Slide 1 / orbitals are spherically symmetrical. s p d
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1 Slide 1 / 58 1 orbitals are spherically symmetrical. s p d f g
2 Slide 2 / 58 2ll of the orbitals in a given electron shell have the same value of the quantum number. Principal ngular Magnetic Spin Psi
3 Slide 3 / 58 3The quantum number defines the shape of an orbital. Spin Magnetic Principal ngular Phi
4 Slide 4 / 58 4The n = 1 shell contains p suborbitals. ll the other shells contain p sub-orbitals. 3, 6 0, 3 6, 2 3, 3 0, 6
5 Slide 5 / 58 5There are orbitals in the second shell
6 Slide 6 / 58 6The lowest energy shell that contains d orbitals is the shell with n =
7 Slide 7 / 58 7The principal quantum number of the first d orbital is
8 Slide 8 / 58 8Which of the orbitals below do not exist due to the constraints upon the angular quantum number? 3f 2s 2p all of the above none of the above
9 Slide 9 / 58 9Which of the orbitals below do not exist due to the constraints upon the angular quantum number? 4f 4d 4p 4s none of the above
10 Slide 10 / 58 10Which one of the following is an incorrect orbital notation? 4f 2d 3s 2p 3d
11 Slide 11 / There are sub-orbitals in the 3rd shell
12 Slide 12 / ll of the sub-orbitals in a given orbital have the same value of the quantum number. Principal ngular Magnetic and and
13 Slide 13 / The p-orbital can accommodate a maximum of electrons
14 Slide 14 / How many quantum numbers are necessary to designate a particular electron in an atom?
15 Slide 15 / t maximum, an f-orbital can hold electrons, a d-orbital can hold electrons, and a p-orbital can hold electrons. 14, 10, 6 2, 8, 18 14, 8, 2 2, 12, 21 2, 6, 10
16 Slide 16 / The lowest orbital energy is reached when the number of electrons with the same spin is maximized. This statement describes. Pauli xclusion Principle Planck's constant deroglie hypothesis Heisenberg Uncertainty Principle Hund's rule
17 Slide 17 / Which one of the following is the correct electron configuration for a ground-state nitrogen atom? None of the above is correct.
18 Slide 18 / Which electron configuration denotes an atom in its ground state?
19 Slide 19 / Which electron configuration represents a violation of the ufbau Principle?
20 Slide 20 / Which electron configuration represents a violation of the ufbau Principle?
21 Slide 21 / Which electron configuration represents a violation of the Pauli xclusion Principle?
22 Slide 22 / Which electron configuration represents a violation of the Pauli xclusion Principle?
23 Slide 23 / Which electron configuration represents a violation of the Pauli xclusion Principle?
24 Slide 24 / Which electron configuration represents a violation of Hund's rule for an atom in its ground state?
25 Slide 25 / Which electron configuration represents a violation of Hund's rule for an atom in its ground state?
26 Slide 26 / Which electron configuration represents a violation of Hund's rule for an atom in its ground state?
27 Slide 27 / Which two elements have the same ground-state electron configuration? I and S u and g Li and Na l and r No two elements have the same ground-state electron configuration.
28 Slide 28 / How many different principal quantum numbers can be found in the ground state electron configuration of ruthenium?
29 Slide 29 / The ground state electron configuration of Fe is. 1s 2 2s 2 3s 2 3p 6 3d 6 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 6 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 4d 6 1s 2 2s 2 3s 2 3p 10
30 Slide 30 / The ground state electron configuration of Ga is. 1s 2 2s 2 3s 2 3p 6 3d 10 4s 2 4p 1 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 4d 10 4p 1 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 1 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4d 1 [r] 4s 2 3d 11
31 Slide 31 / The 2p orbital in the ground state of atomic Neon contains electrons
32 Slide 32 / The second shell in the ground state of atomic argon contains electrons
33 Slide 33 / The orbital is partially filled in Manganese atom. 3s 4s 4p 3d 4d
34 Slide 34 / The ground state configuration of Ne is. [He] 2s 2 2p 2 [He] 2s 2 2p 3 [He] 2s 2 2p 4 [He] 2s 2 2p 6 [F] 2s 2 2p 6
35 Slide 35 / The ground state configuration of iodine is. [r] 4s 2 3d 3 [Xe] 6s 2 4f 14 5d 4 [Ne] 3s 1 [Xe] 6s 2 4f 7 [Kr] 5s 2 4d 10 5p 5
36 Slide 36 / Which is the correct ground-state electron configuration for silver? [Kr] 5s 2 4d 9 [Kr] 5s 1 4d 10 [Kr] 5s 2 4d 10 [Xe] 5s 2 4d 9 [Xe] 5s 1 4d 10
37 Slide 37 / The ground-state electron configuration of the element is [Kr] 5s 1 4d 5. Nb Mo r Mn Tc
38 Slide 38 / The ground-state electron configuration of is [r] 4s 1 3d 5. V Mn Fe r K
39 Slide 39 / The principal quantum number for the outermost electrons in a Iodine atom in the ground state is
40 Slide 40 / Which of the following elements has a groundstate electron configuration different from the predicted one? u a Xe l Ti
41 Slide 41 / Horizontal rows of the periodic table are known as. Periods Groups Metalloids Metals Nonmetals
42 Slide 42 / Vertical columns of the periodic table are known as. Metals Periods Nonmetals Groups Metalloids
43 Slide 43 / lements exhibit similar physical and chemical properties. with similar chemical symbols with similar atomic masses in the same period of the periodic table on opposite sides of the periodic table in the same group of the periodic table
44 Slide 44 / Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties? H, Li s, Sr, Si Ga, Ge, O
45 Slide 45 / Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties? s, Sb, N K, a H, He Si, P
46 Slide 46 / Which pair of elements below should be the most similar in chemical properties? and O and s I and r K and Kr s and He
47 Slide 47 / In the periodic table, the elements are arranged in. alphabetical order order of increasing atomic number order of increasing metallic properties order of increasing neutron content reverse alphabetical order
48 Slide 48 / lements in Group 1 are known as the. halcogens lkaline arth Metals lkali Metals Halogens Noble Gases
49 Slide 49 / lements in Group 2 are known as the. lkaline arth Metals lkali Metals halcogens Halogens Noble Gases
50 Slide 50 / lements in Group 17 are known as the. halcogens lkali Metals lkaline arth Metals Halogens Noble Gases
51 Slide 51 / lements in Group 18 are known as the. Halogens lkali Metals lkaline arth Metals halcogens Noble Gases
52 Slide 52 / The elements in groups 1, 16, and 17 are called,, respectively. lkaline arth Metals, Halogens, and halcogens lkali Metals, halcogens, and Halogens lkali Metals, Halogens, and Noble Gases lkaline arth Metals, Transition Metals, and Halogens Halogens, Transition Metals, and lkali Metals
53 Slide 53 / Which of the following elements is a metalloid? Ga Se In
54 Slide 54 / opper is a and helium is a. Metal, Nonmetal Metal, Metal Metal, Metalloid Metalloid, Nonmetal Nonmetal, Metal
55 Slide 55 / Sulfur is a and nitrogen is a. Metal, Metalloid Nonmetal, Metal Metalloid, Metalloid Nonmetal, Nonmetal Nonmetal, Metalloid
56 Slide 56 / alcium is a and silver is a. Nonmetal, Metal Metal, Metal Metalloid, Metal Metal, Metalloid Nonmetal, Metalloid
57 Slide 57 / lements in group have an ns 2 np 6 electron configuration in the outer shell
58 Slide 58 / Which group in the periodic table contains elements with the valence electron configuration of ns 2 np 1?
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