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Essential Information from the Periodic Table

Explore the key properties and trends of elements, including atomic mass, electron configuration, oxidation states, and more. Understand the periodic table through detailed explanations and typical questions for better comprehension.

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Essential Information from the Periodic Table

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  1. PERIODIC TABLE Kenneth E. Schnobrich

  2. Atomic Mass Oxidation State Li 6.941 +1 Atomic Number 3 1s22s1 or 2-1 Electron Configuration

  3. GROUPS H VERTICAL COLUMNS - • Alkali Metals • Alkaline Earth Metals • Transition Elements • Chalcogens • Halogens • Inert (Noble) Gases 1 2 3-12 16 17 18 Li Na K Rb

  4. PERIODS Li Be B C N O F Ne 1s22s1 1s22s2 1s22s22p1 1s22s22p2 1s22s22p3 1s22s22p4 1s22s22p5 1s22s22p6 HORIZONTAL ROWS - the Period Number indicates the Principal Energy Level that is filling as we move from left to right.

  5. PERIODS Li Be B C N O F Ne 2-1 2-2 2-3 2-4 2-5 2-6 2-7 2-8 HORIZONTAL ROWS - the Period Number indicates the Principal Energy Level that is filling as we move from left to right.

  6. METALS METALLOIDS NONMETALS INERT GASES

  7. Atomic Radius Table S* DECREASES *NYS Reference Tables for Chemistry

  8. COVALENT RADII - PERIOD 2

  9. Atomic Radius INCREASES

  10. COVALENT RADII - GROUP IA

  11. Types of Atomic Radii Covalent Radius - effective distance from the center of the nucleus to the outer valence shell in a covalent or coordinate covalent bond. Van der Waals Radius - half the closest distance between two nonbonded atoms.

  12. Metals + Loss of electrons - Nonmetals Gain of electrons

  13. IONIZATION ENERGYELECTRONEGATIVITY Ionization Energy – the amount of energy (usually in kilojoules) needed to remove the most loosely bound electron from a gaseous atom of an element. Definitions Electronegativity – the attractive force that an atom has for an electron(s) during the formation of a chemical bond. (no units are assigned)

  14. Ionization Energy & Electronegativity 496 Na 0.9 “PROPERTIES OF SELECTED ELEMENTS” Table S First Ionization Energy (kJ/mol) Electronegativity

  15. Ionization Energy INCREASES

  16. General Trend Across a Period

  17. Ionization Energy DECREASES

  18. General Trend Down a Group

  19. General Trend Down a Group

  20. ELECTRONEGATIVITY Table S* DECREASES *NYS Reference Tables for Chemistry

  21. Electronegativities of Group IA

  22. Electronegativity Across a Period INCREASES

  23. Electronegativities for Period 2

  24. REACTIVITY REACTIVITY INCREASES REACTIVITY INCREASES

  25. Transition Elements • Multiple Oxidation States • Form Colored Compounds • Incomplete Inner “d” Sublevels

  26. TYPICAL QUESTIONS

  27. The Most active metals are in Group - • 1 (IA) • 15 (VA) • 13 (IIIA) • 17 (VIIA)

  28. The elements known as Alkali metals are found in Group • 1 (IA) • 2 (IIA) • 13 (IIIA) • 17 (VIIA)

  29. What is the total number of electrons found in the valence shell of an Alkaline Earth element in the ground state • 1 • 2 • 3 • 4

  30. As the elements in Group IIA are considered from top to bottom, the # of electrons in the 2s subshell • increases • decreases • remains the same

  31. Which group contains atoms that form +1 ions having an inert gas configuration? • 1 (IA) • 11 (IB) • 17 (VIIA) • 7 (VIIB)

  32. Which Group 17(VIIA) elements listed below has the greatest nuclear charge? • F • Cl • Br • I

  33. Which element is most likely to form a compound with Kr? • Fluorine • Chlorine • Bromine • Iodine

  34. Which group on the Periodic Table contains solid, liquid, and gaseous elements at room temperature? • 18 (O) • 2 (IIA) • 16 (VIA) • 17 (VIIA)

  35. Which represents the correct order of activity for the Group VIIA(17) elements? • Br > I > F > Cl • F > Cl > Br > I • I > Br > Cl > F • F > Br > Cl > I

  36. If the elements are considered from top to bottom in Group 16(VIA), the number of electrons in the outermost shell will? • decrease • increase • remain the same

  37. Which Group contains and element that is a liquid at room temperature? • 18 (O) • 2 (IIA) • 11 (IB) • 12 (IIB)

  38. Which element has the greatest tendency to gain electrons? • Te • Se • S • O USE CHART S

  39. When atoms of the elements in Group 18 (0) are compared in order from top to bottom, the attractions between atoms? • increases and the boiling point decreases • decreases and the boiling point increases • increases and the boiling point increases • decreases and the boiling point decreases

  40. In the ground state, an atom of which element in Period 3 has the most loosely bound electron? • Si • Na • S • Ar USE CHART S

  41. Which Period contains elements that are all gases at STP? • 1 • 2 • 3 • 4

  42. Considered in succession, the elements in Period 2 of the Periodic Table show a decrease in atomic radius with increasing atomic charge increases? • nuclear charge increases • # of PEL increases • number of neutrons decreases • # of protons increases

  43. Which represents the electron configuration of a metalloid in the ground state? • 2-3 • 2-5 • 2-8-5 • 2-8-6

  44. In a given Period of the Periodic Table, the element with the lowest first ionization energy is always? • an Alkaline Earth Metal • an Alkali Metal • a Halogen • an Inert Gas USE CHART S

  45. As one goes from Li to F in Period 2 of the Periodic Table, the atomic radius of the elements? • decreases • increases • remains the same USE CHART S

  46. An element in which electrons from more than one energy level may be involved in bond formation? • potassium • calcium • copper • zinc

  47. Which element can form more than one binary compound with chlorine? • potassium • calcium • iron • zinc

  48. A pure compound is blue in color. It is most likely a compound of? • sodium • lithium • calcium • copper

  49. Which is the electron configuration of a transition element in the ground state? • 2-8-8 • 2-8-8-2 • 2-8-18-2 • 2-8-18-8 Ar Ca Zn Kr

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