Four main-group elements a, b, c and d are highlighted in the outline of the Periodic Table below:abdList these elements below by increasing ionization energy. For example, if a has the lowest ionization energy and b the next highest, then your list should starta, b, ...Important: don't try to figure out exactly which elements are marked, and then use your knowledge of the properties of each specific element. You don't needto. You will also be marked wrong for any answer, correct or not, that can't be determined from only the rough location of each marked element in the PeriodicTable.1-1-0-1×

Step 1: Step 2: Step 3: Step 4:

Answered: Four main-group elements a, b, c and d…

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 13ALQ

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Similar questions

For each of the following pairs of elements, choose the one that correctly completes the following table.
In each of the following sets of elements, which element would he expected to have the highest ionization energy? msp;a.Cs,K,Lic.l,Br,Clb.Ba,Sr,Cad.Mg,Si,S
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?
Calcium metal reacts with cold water as follows: Ca+2H2OCa(OH)2+H2 Magnesium metal does not react with cold water. What behavior toward cold water would you predict for strontium and barium? Write equations to represent any predicted reactions.
Which of the following atoms and ions is (are) isoelectronic with S2+:Si4+,Ar,As3+,Si,Al3+?
Which atom and/or ion is (are) isoelectronic with Br+:Se2+,Se,As,Kr,Ga3+,Cl?
6.84 Which graph correctly depicts the first ionization energy of three elements in groups 14 (dashed line) and 17 (solid line)? Explain the reasoning you used to make your choice.
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.
Without looking at the figures for the periodic properties, compare the three elements B, AI and C. (a) Place the three elements in order of increasing atomic radius. (b) Rank the elements in order of increasing ionization energy. (c) Which element, B or C, is expected to have the more negative electron attachment enthalpy value?
How are the electron arrangements in a given group (vertical column) of the periodic table related? How is this relationship manifested in the properties of the elements in the given group?
lement X, which has a valence shell configuration of ns2np4 , was isolated in a laboratory. Which of the following statements is(are) true concerning element X? Element X has chemical properties similar to those of the halogens. Element X has six valence electrons. When element X is reacted with calcium, the compound formed would most likely have the formula Ca2X . Element X needs to gain two electrons to attain a noble gas electron configuration. mg src=Images/HTML_99425-11-106AP_image001.jpg alt="" align="top"/>

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