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- 1. Open EndedWhich of the following options correctly describes the shielding effects in a many-electron systems? a.) Shielding reduces the magnitude of the nuclear charge a given electron experiences. b.) Inner electrons are more effective at shielding outer electrons than electrons in the same level. c.) The shielding effect increases with an increasing number of electrons in a given sublevel. d.) Electrons in the same sublevel do not shield each other from the nucleus. e.) Shielding protects an electron so that it is harder to remove from the atom.
- 2. Open EndedWhich of the following statements correctly describes the changes that occur as we move from left to right across the periodic table? a.) Nuclear charge increases b.) The number of core electrons increases. c.) The nuclear charge felt by the outermost electrons decreases d.) The number of valence electrons increases for representative elements.
- 3. Open EndedOrder the following elements in terms of increasing effective nuclear charge (Zeff) Br Cs K As
- 4. Fill in the BlankRepulsions between electrons in a many-electron atom results in a phenomenon known as ______________, which leads to the electrons "experiencing" a lower____________ nuclear charge.
- 5. Open EndedWhich type of electrons are best at shielding a 3p electron? 3d 3p 3s 2p 4p
- 6. Fill in the BlankAs we move from left to right in the periodic table the effective nuclear charge (Zeff) __________ because the number of ___________ electrons remains the same while the actual nuclear charge increases.
- 7. Open EndedBased on their positions in the periodic table, match the elements that are most chemically similar. K Cs Mg Cl F Sr Ne Ar
- 8. Open EndedArrange the following elements in order of increasing atomic size, starting with the smallest atom at the top of the list. I Se S Br
- 9. Fill in the BlankElements such as Na and K are in the same ________________ of the periodic table. These elements have similar chemical properties because they have the same number of __________ electrons.
- 10. Fill in the BlankMatch the group number from the periodic table with the correct name. Elements in Groups 1A - 7A Group 8A Elements in Groups 18 and 3B f- block transition elements ____________________________________________ transition metals noble gases lanthanides and actinides main group elements
- 11. Open EndedWhich elements are removed first when forming cations of period 4 transition elements? 3d 4d 3p 4s
- 12. Open EndedWhich of the following groups contains elements that are chemically similar to each other because they have the same valence-electron config? Noble gases Transition metals Halogens Alkali metals
- 13. Open EndedWhich of the following species are isoelectronic w/ each other? Ar Sr^2+ Mg^2+ Br^- Cd^2+
- 14. Open EndedList the following elements in order of decreasing
- 15. Open EndedWhich element, Mg or Al, will have the higher first ionization energy, and why? Select the statement that best describes the reason for your choice. (Hint: in order to answer this question, first write out the electron config for both elements.) Removing an electron from Mg is more difficult because the outermost electron is in a lower-energy ns orbital. Mg will have a higher first ionization energy. Al is farther to the right in the periodic table and has a higher value for effective nuclear charge. Al will have a higher first ionization energy.
- 16. Fill in the BlankIn general for main group elements atomic radii __________ from left to right across a period and ____________ down a group of the period table.
- 17. Fill in the BlankMatch each type of ion with the correct description of its size relative to its parent atom. Cation Anion ___________________________________________ Smaller than its parent atom Larger than its percent atom
- 18. Fill in the BlankAtomic radius generally decreases from left to right across a period because the effective nuclear charge _______________ while electrons are being added to the same outer shell. These additional electrons are not shielded as well by inner electrons and are therefore attracted _____________ strongly by the nucleus.
- 19. Fill in the BlankThe energy required for the complete removal of 1 mol of electrons from 1 mol of gaseous atoms or ions is called _____________ energy. For a neutral element this energy is a measure of how easily the element forms a(n) _________________ , which is an ion w/ a net ________________ charge.
- 20. Open EndedMatch each of the following element with the correct number of electrons lost or gained to form its most common ion. K -> loses 1 electron Cl -> gains 1 electron Mg -> gains 2 electrons S -> loses 2 electrons
- 21. Open EndedWithout reference to the periodic table, match each atom (number of electrons given) with its block designation (s-, p-, or d-block) on the periodic tables. Hint: Write out the electron configuration for each example. 15 electrons -> d-block 20 electrons -> s-block 43 electrons -> p-block
- 22. Open EndedElectron configuration for Sn^4+
- 23. Open EndedWhich of the following statements correctly describe the trends in ionization energy (IE) Select all that apply. a.) Atoms w/ low ionization energies tend to form cations b.) Noble gases have high ionization energies. c.) Nonmetals tend to have low ionization energies d.) Second ionization energies are always less than first ionization energies.
- 24. Open EndedWhich of the following statements describes/define ionization energy correctly? Select all that apply. a.) The ionization energy of an element is a measure of how easily it forms a cation. b.) Ionization energy is the energy required for complete removal of 1 mol of core electrons from 1 mol of gaseous atoms or ions. c.) The ionization energy of an element is a measure of how easily it forms an anion. d.) Ionization energy is the energy (kJ) required for the complete removal of 1 mol of valence electrons from 1 mol of gaseous atoms or ions.
- 25. Open EndedIonization trends
- 26. Open EndedMetallic Character
- 27. Open EndedIsoelectronic
- 28. Open EndedAtomic Radius
- 29. Open EndedAtomic size
- 30. Fill in the BlankIons are most attracted to each other when their charges are ____________ and the distance between them is __________.
- 31. Open Endedwhich of the following ions are isoelectronic with Ar? Select all that apply. Br^- K^+ Cl^- Mg^2+ S^2-
- 32. Open EndedHalogens
- 33. Open EndedNoble gasses
- 34. Open EndedTransition Metals
- 35. Open EndedLanthanides and Actinides
- 36. Open Endedwhy do some elements (such as Li and Mg) exhibit diagonal relationships?
- 37. Fill in the BlankThe periodic table developed from the observation of ________________, which is the regular recurrence of the physical and chemical properties of the elements when they are arranged in order of increasing atomic mass.
- 38. Open EndedMetallic Radius
- 39. Open EndedCovalent Radius
- 40. Open EndedMendeleev's original periodic table
- 41. Open Endedionic radius
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