Going from the left to right in the periodic table, the size changes among the transition elements are more gradual than those among the representative elements. Select all that help explain why this is true. O The electrons that are added from one element to another enter an outer (n - 1)d subshell. O The electrons that are added from one element to another enter an inner (n - 1)d subshell. O The outer electrons for the transition elements are in the ns orbital. O The inner electrons for the transition elements are in the ns orbital. eTextbook and Media Attempts: 0 of 15 used Submit Answer Save for Later

Going from the left to right in the periodic table, the size changes among the transition elements are more gradual than those among the representative elements. Select all that help explain why this is true. O The electrons that are added from one element to another enter an outer (n - 1)d subshell. O The electrons that are added from one element to another enter an inner (n - 1)d subshell. O The outer electrons for the transition elements are in the ns orbital. O The inner electrons for the transition elements are in the ns orbital. eTextbook and Media Attempts: 0 of 15 used Submit Answer Save for Later

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Without using a periodic table, give the ground-state electron configuration and block designation (s-, p-, d-, or f-block) of an atom with (a) 17 electrons, (b) 37 electrons, and (c) 22 electrons. Classify each atom as a main group element or transition metal.
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How many electrons are in the outermost shell of the Cl- ion in its ground state? 6 0 8 2
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Which are the representative elements? (also known as main group elements) These elements have incompletely filled s or p subshells of the highest principal quantum number. O1. Hydrogen O 2. Helium O 3. Lithium 04. Beryllium 5. Boron 6. Carbon 7. Nitrogen 8. Oxygen O 9. Fluorine O 10. Neon O 11. Sodium O 12. Magnesium 13. Aluminum O 14. Silicon 15. Phosphorus O 16. Sulfur O17. Chlorine O18. Argon O 19. Potassium 20. Calcium O 21. Scandium 22. Titanium 23. Vanadium O 24. Chromium 25. Manganese 26. Iron O 27. Cobalt O 28. Nickel 29. Copper 30. Zinc 31. Gallium 32. Germanium 33. Arsenic 34. Selenium O35. Bromine O36. Krypton O37. Rubidium O38. Strontium O39. Yttrium O40. Zirconium NAVAM YA
The electron configuration of an element is: 1s? 2s? 2p6 3s? 3p6 4s? 3d10 4p6 5s2 The Group and Period of the element are: Group 5 Period 1A Group 2B Period 5 Group 5 Period 1B Group 2A Period 5
this question has two parts A and B. Part A: How does atomic radius change going down the group and why? Decreases because there are less energy levels decreases because the nucleus is stronger Increases because more energy levels are being added down the group Increases because the nucleus is weaker Part B: How does atomic radius change moving across the period? Increases because there are more energy levels Increases because the nucleus is less efficient (weaker) Decreases because the nucleus is stronger and more efficient Decreases because there are less energy levels