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PERIODIC TABLE

PERIODIC TABLE. Kenneth E. Schnobrich. Atomic Mass. Oxidation State. Li. 6.941. +1. Atomic Number. 3. 1s 2 2s 1 or 2-1. Electron Configuration. GROUPS. H. VERTICAL COLUMNS - • Alkali Metals • Alkaline Earth Metals • Transition Elements • Chalcogens • Halogens

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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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