(a)
Interpretation:
The element having higher ionization energy in given pair should be selected.
Concept Introduction: The energy which is required to remove an electron from the gaseous state of an atom or ion is said to be the ionization energy.
(b)
Interpretation:
The element having higher ionization energy in given pair should be selected.
Concept Introduction: The energy which is required to remove an electron from the gaseous state of an atom or ion is said to be the ionization energy.
(c)
Interpretation:
The element having higher ionization energy in given pair should be selected.
Concept Introduction: The energy which is required to remove an electron from the gaseous state of an atom or ion is said to be the ionization energy.
(d)
Interpretation:
The element having higher ionization energy in given pair should be selected.
Concept Introduction: The energy which is required to remove an electron from the gaseous state of an atom or ion is said to be the ionization energy.
Want to see the full answer?
Check out a sample textbook solutionChapter 5 Solutions
EBK BASIC CHEMISTRY
- Compare the elements B. Al, C, and Si. (a) Which has the most metallic character? (b) Which has the largest atomic radius? (c) Which has the most negative electron attachment enthalpy? (d) Place the three elements B, Al, and C in order of increasing first ionization energy.arrow_forwardHow many valence electrons do each of the following elements have, and what are the specific valence electrons for each element? a. Ca b.O c. element 117 d. In e. Ar f. Biarrow_forwardWhat is the electron configuration of Mg2+? How does its reactivity compare with neutral Mg? How do the reactivities of F- and F compare?arrow_forward
- Explain why Al is a member of group 13 rather than group 3?arrow_forwardWhich main group atom would be expected to have the lowest second ionization energy?arrow_forwardGraph the atomic radii versus atomic number of the first 18 elements. Explain the trends in radii across the second period and down Group 1A.arrow_forward
- Choose the element with the higher first ionization energy in each pair.a. P or I b. Si or Cl c. P or Sb d. Ga or Gearrow_forwardChoose the element with the higher first ionization energy from each pair.a. Br or Bi b. Na or Rb c. As or At d. P or Snarrow_forward67.)Which of the following elements has the highest ionization energy? a. K b. Ca c. Rb d. Srarrow_forward
- Which element has the greatest first ionization energy? A. C B. B C. Narrow_forwardWhich one of these ions is not isoelectronic with Ar? A. S²- B. Ca2+ C. Fe2+ D. CH E. K+arrow_forwardConsider the elements: B, C, N, O, F.a. Which element has the highest first ionization energy?b. Which element has the largest atomic radius?c. Which element is most metallic?d. Which element has three unpaired electrons?arrow_forward
- Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning