Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Transcribed Image Text:Arrange the following chemical species in order of
increasing radius: Be
Na +, Ne
O Na +
< Be
O Be
2+
2+
O Te< Be < Na
+
O Te < Na < Be
2+
< Te
Save Answer
+
2+
+
< Na <Te
2+
"
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- What would you predict the charge of an ion from column 1A (or column 1 from ptable) to be? O a 2- O b 1- Oc 1+ Od 2+arrow_forwardArrange the following atoms in the order of increasing ionization energy: CI, S, Ar, Ne You may need to use the periodic table below. 1A 7A 8A Metals 3A 4A 5A 6A H He B C NO F Ne H 2A Metalloids Li Be Nonmetals Na Mg зв 4в 58 6B 7B — 88 — 1в 28 Al si P S CI Ar K Ca Sc Tiv Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Hf Ta w Re Os Ir Pt Au Hg TI Pb Bi Po At Rn Fr Ra Ac Rf Db Lanthanides Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Actinides Th Pa u Np Pu Am Cm Bk Cf Es Fm Md No Lr Increasing ionization energy Drag and drop your selection from the following list to complete the answer: Ne CI Ar Sarrow_forwardArrange the following in order of decreasing atomic radius: Al, Mg, Na, O O > Na > Mg > Al O Al > Mg > O > Na O > Al > Mg > Na O Al > Mg > Na > O Na > Mg > Al > Oarrow_forward
- Og is the noble gas after Rn. To go from [Rn] to [Og], you must fill four subshells (s, p, d, and f) with a total of 32 electrons. Thus, the atomic numbers of sixth and seventh period elements of the same group differ by 32. To go from [Og] to the next noble gas, however, you would theoretically fill five subshells (s, p, d, f, and g). How many electrons are needed to fill all five subshells? number of electrons: Element 106 in the periodic table is Sg. Determine the atomic number of the element just below Sg in the periodic table. atomic number:arrow_forwardWhich element would have the greatest ionization energy? S, Ge, Al, K, or Sr Which equation below illustrates the first ionization energy for strontium? A, B, C, D, E, or F A) Sr (g) + 2e– → Sr–2 (g) B) Sr (g) → Sr+2 (g) + 2e– C) Sr+ (g) →Sr+2(g) + e– D) Sr (g) → Sr+ (g) + e– E) Sr+2 (g) + 2e– → Sr (g) F) Sr (g) + e– → Sr– (g)arrow_forwardcan you help me with this question?arrow_forward
- Rank the following isoelectronic species in order of decreasing size: Argon atom (Ar), Calcium ion (Ca+2), chloride ion (Cl-1), Potassium ion (K+1), Sulfide ion (S-2).arrow_forwardTwo sets of ionizations are shown in the tables below. Complete the tables by ordering each set of ionizations by increasing amount of energy required. In other words, for each set choose "1" next to the ionization that would require the least energy, "2" next to the ionization that would require the next least energy, and so on. ionization + F → F + e + Bi → Bi + e Te → Te + e energy required ? ? ? î ↑ ŷ ionization + PbPb te + CI + e Cl → Cl Sb Sb + e X energy required ? ? ? S ↑ ↑arrow_forwardTwo sets of ionizations are shown in the tables below. Complete the tables by ordering each set of ionizations by increasing amount of energy required. In other words, for each set choose "1" next to the ionization that would require the least energy, "2" next to the ionization that would require the next lea energy, and so on. ionization Ar Ar+e Ba Ba +e Fr Fre energy required [? ? ? ionization F→ F + e Si Si + e Ra Ra +e X energy required ? ? ?arrow_forward
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