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Periodic Table Trend Review

Periodic Table Trend Review. To which group of the periodic table do lithium and potassium belong?. alkali metals transition metals halogens noble gases. Trends in the properties of elements in a group or period can be explained in terms of. binding energy. atomic number.

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Periodic Table Trend Review

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  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

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