ࡱ>  x*bjbjO O  -a-aj" rr8<T|$:V$X$X$X$X$X$X$$&(|$g@|$$'!'!'! V$'!V$'!'!Z##pNNjr#B$$0$z#,i)i)##i)#'!|$|$! $i)r : Periodic Table Worksheet #1 A. Write the electron configurations (all 3 ways) for the following elements: 1. Sulfur ______ 1s ______ ______ ______ ______ 2s 2p ______ ______ ______ ______ ______ ______ ______ _____ ____ 3s 3p 3d 2. Calcium ______ 1s ______ ______ ______ ______ 2s 2p ______ ______ ______ ______ ______ ______ ______ _____ ____ 3s 3p 3d ______ ______ ______ ______ ______ ______ ______ _____ ____ ____ ____ ____ ____ ____ ____ ____ 4s 4p 4d 4f Write the standard and noble gas electron configurations for the following elements: 3. Silver 4. Gold 5. Radium B. Periodic Table Group Properties 1. Define valence electrons: 2. Label the group numbers, period numbers, alkali metals, alkaline earth metals, transition metals, inner transition metals, halogens, noble gases, s-block, p-block, d-block, f-block, main group elements, and number of valence electrons on the following periodic table.  ____________3. How do the electron configurations within the same group of elements compare? ____________4. What information is provided by the specific block location of an element? ____________5. Which group of elements are the alkali metals? List four characteristic properties: _________________, _________________, _________________, _________________ ____________6. Which group of elements are the alkaline earth metals? List four characteristic properties: _________________, _________________, _________________, _________________ ____________7. What name is used to refer to the entire d-block elements? ____________8. Which group of elements are the halogens? List three characteristic properties: _________________, _________________, _________________ ____________10. Which groups of elements are the main group elements? ____________11. Which group of elements are the noble gases? List three characteristic properties: _________________, _________________, _________________ 12. Identify the period, block, and group in which the elements with the following electron configurations are located. Period_____ Block_____ Group_____ a. [Ne]3s23p4 Period_____ Block_____ Group_____ b. [Kr]5s24d105p2 Period_____ Block_____ Group_____ c. [Xe]6s24f145d106p5 13. Write the expected outer electron configuration for each of the following elements. _______________a. Group 7, Period 4 _______________b. Group 3, Period 5 _______________c. Group 12, Period 6 ____________15. Which main group elements have 1 valence electron? ____________16. Which main group elements have 6 valence electrons? _______________17. Write the nuclear symbol for an ion with a charge of +2, 20 protons, and 24 neutrons. ______________a. How many electrons are in this ion? ______________b. Is it an anion or cation? _______________18. Write the nuclear symbol for an ion with a charge of -2, 18 electrons, and 18 neutrons. ______________a. How many protons are in this ion? ______________b. Is it an anion or cation? _______________19. Write the nuclear symbol for an ion with a charge of +3, 13 protons, and 15 neutrons. ______________a. How many electrons are in this ion? ______________b. Is it an anion or cation? Periodic Trends Worksheet #2 Trends-Atomic Radii (size), Ionization Energy, Electronegativity 1. Circle the one from each pair that would have the larger atomic radius (larger in size): (A) F atom or O atom (B) Ba atom or Ra atom (C) Hf atom or Ti atom (D) Ta atom or At atom (E) Cu atom or K atom (F) Np atom or Cf atom (G) Mn atom or Re atom (H) Dy atom or Cf atom (I) As atom or Cl atom (J) B atom or In atom (K) Mg atom or S atom (L) Tl atom or Y atom (M) Cl atom or I atom (N) Ar atom or Xe atom (O) Ca atom or Ga atom 3. Circle the atom with the greater ionization energy (IE): (A) Pb or Sn (B) B or C (C) Ba or At (D) Lr or Ra (E) Cs or V (F) Si or Ag (G) F atom or O atom (H) Ba atom or Ra atom (I) S or Te (J) F or Cl (K) Sr or Rb (L) Os or Co (M) Am or Eu (N) Pb or Sn (O) Ba or At 4. Circle the atom with the lower electronegativity (EN): (A) C or N (B) Na or K (C) Ta or Cu (D) Pd or Mo (E) Lr or Ra (F) Cs or V (G) Si or Ag (H) F atom or O atom (I) Ba atom or Ra atom 5. Dont forget that atoms will lose or gain valence electrons in order to have either 0 or 8 valence electrons. (Whichever is closer, for example if an atom has 2 valence electrons it will lose 2 valence electrons instead of gaining 6 valence electrons.) When sodium becomes an ion will electrons be lost or gained?__________ How many?__________ When calcium becomes an ion will electrons be lost or gained?__________ How many?__________ When aluminum becomes an ion will electrons be lost or gained?__________ How many?__________ When phosphorus becomes an ion will electrons be lost or gained?__________ How many?__________ When sulfur becomes an ion will electrons be lost or gained?__________ How many?__________ When chlorine becomes an ion will electrons be lost or gained?_________ How many?__________ Periodic Trends Test Review _______________1. Who and how was the first periodic table constructed and how has our present day periodic table changed from the original? 2. As you move across the periodic table, from left to right, (A) do the atoms get smaller or larger? __________ (B) are the ionization energies increasing or decreasing?_____________ (C) are the metals becoming more or less reactive? ________________ (D) are the metals getting harder or softer? ___________________ 3. Explain the trends involving ionization energy, atomic radii, and electronegativity that are evident in the various groups and periods of the periodic table. 4. Which main group elements have 1 valence electron? _____ 6 valence electrons?____ 5. Determine the group, period, and block for the following elements: a. [Ne]3s1 block____ group____period____ b. [Ar]4s23d10 block____ group____period____ c. [Ar]4s23d104p2 block____ group____period____ d. [Kr]5s24d2 block____ group____period____ e. [Kr]5s24d10 block____ group____period____ 6. Use their placement on the periodic table to arrange the following elements based on their size (atomic radii) from largest to smallest. a. Ca, Ge, Br, K, Kr b. Sr, Mg, Be, Ba, Ra c. F, Cl, Fr, Cs 7. Use their placement on the periodic table to arrange the following elements from highest ionization energy to lowest ionization energy. a. Ca, Ge, Br, K, Kr b. Sr, Mg, Be, Ba, Ra c. F, Cl, Fr, Cs 8. Use their placement on the periodic table to determine which of the following has the lowest ionization energy. a. F or Sn b. Si or Y c. Fe or K d. Bi or N e. Ho or Br f. Rb or Cl 9. Use their placement on the periodic table to determine which of the following has a lower electronegativity. a. F or Sn b. Si or Y c. Fe or K d. Bi or N e. Ho or Br f. Rb or Cl 10. When sodium becomes an ion will it lose or gain electrons?_______ How many electrons?_______ Write the nuclear symbol for an ion of sodium (assume it has 11 neutrons)._____________ 11. When aluminum ionizes will it lose or gain electrons?_______ How many electrons?_______ Write the nuclear symbol for an ion of aluminum (assume it has 14 neutrons)._____________ 12. When nitrogen becomes an ion will it lose or gain electrons?_______ How many electrons?_______ Write the nuclear symbol for an ion of nitrogen (assume it has 7 neutrons)._____________ _______________13. Write the nuclear symbol for an ion with a charge of +2, 20 protons, and 24 neutrons. ______________a. How many electrons are in this ion? ______________b. Is it an anion or cation? _______________14. Write the nuclear symbol for an ion with a charge of -2, 18 electrons, and 18 neutrons. ______________a. How many protons are in this ion? ______________b. Is it an anion or cation? _______________15. Write the nuclear symbol for an ion with a charge of +3, 13 protons, and 15 neutrons. ______________a. How many electrons are in this ion? ______________b. Is it an anion or cation?     !CPjlxD P . 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