Periodic Table Trend Review

1. Periodic Table Trend Review

2. To which group of the periodic table do lithium and potassium belong? • alkali metals • transition metals • halogens • noble gases

3. Trends in the properties of elements in a group or period can be explained in terms of • binding energy. • atomic number. • electron configuration. • electron affinity.

4. Trends in the periodic table indicate that the element with the greatest ionization energy is in which of the following periods and groups? • Period 2, Group 1 • Period 7, Group 2 • Period 1, Group 18 • Period 6, Group 17

5. Going down a group in the periodic table, electron shielding generally causes the ionization energy to • increase. • remain the same. • decrease. • vary unpredictably.

6. Which is the best reason that the atomic radius generally increases with atomic number in each group of elements? • The nuclear charge increases. • The number of neutrons increases. • The number of energy levels increases. • A new octet forms.

7. What is the effective nuclear charge on sulfur? • +2 • +4 • +6 • +16 • -2

8. What is the effective nuclear charge alkaline earth metals? • +2 • +4 • +6 • +16 • +1

9. Trends in the periodic table indicate that an element in which of the following periods and groups will have the smallest anion (negative ion) radius? • Period 3, Group 17 • Period 7, Group 16 • Period 4, Group 16 • Period 2, Group 17

10. In many compounds, atoms of main-group elements form ions so that the number of electrons in the outermost energy levels of each ion is • 2. • 6. • 8. • 10.

11. Atoms of lithium and calcium • generally form stable bonds with transition elements. • have stable electron configurations. • tend to form cations. • tend to form anions.

12. When the octet rule is satisfied, the outermost _____ are filled. • d and f orbitals • s and p orbitals • s and d orbitals • d and p orbitals

13. Once an atom has full s and p orbitals in its outermost energy level, • it is highly reactive only with alkali metals. • it is highly reactive only with halogens. • it can be combined with most elements. • it has a stable octet and is unreactive.

14. The idea of arranging the elements in the periodic table according to their chemical and physical properties is attributed to • Mendeleev. • Moseley. • Bohr. • Ramsay.

15. Mendeleev predicted that the spaces in his periodic table represented • isotopes. • radioactive elements. • unstable elements. • undiscovered elements.

16. Argon, krypton, and xenon are • alkaline earth metals. • noble gases. • actinides. • lanthanides.

17. Elements in a group or column in the periodic table can be expected to have similar chemical • atomic masses. • atomic numbers. • numbers of neutrons. • properties.

18. In Period 3 there are 8 elements. What sublevel(s) is (are) being filled? • s • s and d • s and p • d and f

19. If n stands for the highest occupied energy level, the outer configuration for all Group 1 elements is • ns1. • 2n. • n – s. • np1.

20. Nitrogen's electron configuration is 1s2 2s2 2p3. To what group does nitrogen belong? • Group 2 • Group 7 • Group 15 • Group 17

21. Bromine, atomic number 35, belongs to Group 17. How many electrons does bromine have in its outermost energy level? • 7 • 17 • 18 • 35

22. Oxygen atoms form anions that have the same electron configuration as: • Ne • Ar • He • Xe • Kr

23. Potassium atoms form cations that have the same electron configuration as: • Ne • Ar • He • Xe • Kr

24. Which block in the periodic table contains the alkali metals? • s • p • d • f

25. The most characteristic property of the noble gases is that they • have low boiling points. • are radioactive. • are gases at ordinary temperatures. • are largely unreactive.

26. A measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound is called • electron affinity. • electron configuration. • electronegativity. • ionization energy.

27. What is removed when the ionization energy is supplied to an atom of an element? • the electron cloud • the nucleus • an electron • an ion

28. The element that has the greatest electronegativity is • oxygen. • helium • chlorine. • fluorine.

29. A negative ion is known as a(n) • ionic radius. • valence electron. • cation. • anion.

30. Within a group of elements, as the atomic number increases, the atomic radius • increases. • remains approximately constant. • decreases regularly. • varies unpredictably.

31. As you move up Group 14 in the periodic table from lead up to carbon, atomic radii • generally increase. • generally decrease. • do not change. • vary unpredictably.

32. Hoe does the energy required to remove an electron from an atom changer as you move left to right in Period 4 from potassium through iron? • It generally increases. • It generally decreases. • It does not change. • It varies unpredictably.

33. The electrons available to be lost, gained, or shared when atoms form compounds are called • ions. • valence electrons. • d electrons. • electron clouds.

34. The number of valence electrons in Group 1 elements is • 1. • 2. • 8. • equal to the period number.

35. The number of valence electrons in Group 17 elements is • 7. • 8. • 17. • equal to the period number.

36. Halogens tend to form ions with a charge of • -1 • +1 • -2 • -3

37. Which of the following definitely do not form cations? • Metals • Alkali metals • Alkaline earth metals • Group 13 elements • Group 16 elements