University:
Glendale Community College
Course:
CHM130 | Fundamental Chemistry
Academic year:

2020
Views:

486

Pages:

3
Author:

Prexl20

Name: _______________________ Section: _____________ Chapter 4 Practice Worksheet: Periodic Trends 1) Write electron configurations of the following ions: a) K+ (long hand notation): b) F- (long hand): c) Ni2+ (short hand): d) Zn2+ (short hand): e) Br- (short hand): f) Cu2+ (short hand): g) Ag+ (short hand): 2) Draw orbital diagrams (for valence electrons only) for the following ions: a) K+ b) Brc) Ni2+ d) Zn2+ 3) Define the following terms: atomic radius. Describe the periodic trend for atomic radius. 4) Define Zeff (effective nuclear charge). How does this property affect radii of atoms as you move from left to right in a period? Does it affect atomic radius as you move down a group? page 1 of 3 Name: _______________________ Section: _____________ 5) Arrange the following atoms in order of increasing radius: N, Sb, P, Bi, As. Explain your answer in terms of the atomic number of the elements and/or their valence electron configuration. 6) Define the phrase isoelectronic series. Describe how sizes of ions change as you move from the most positively charged ion to the most negatively charged ion in an isoelectronic series. 7) Arrange the following ions in order of increasing radius: F-, Na+, O2-, Mg2+, N3-. Is this an isoelectronic series? 8) Define ionization energy. 9) Write the chemical equation that corresponds to the ionization energy of iodine. 10) On the periodic table below, use arrows to show the general trends in ionization energy and atomic radius among the elements. Indicate which elements have the highest and lowest ionization energy. Also indicate the largest and smallest elements. page 2 of 3 Name: _______________________ Section: _____________ 11) Which has higher ionization energy, Li or Na? Explain your reasoning in terms of the electronic configurations of each. Check the values to make sure you are correct. 12) Which has higher ionization energy, Al or Cl? Explain your reasoning in terms of the electronic configurations of each. Check the values to make sure you are correct. 13) Which has higher first ionization energy, N or O? Explain your reasoning in terms of the electronic configurations of each. Check the values to make sure you are correct. 14) Which has higher first ionization energy, Be or B? Explain your reasoning in terms of the electronic configurations of each. Check the values to make sure you are correct. 15) A new element is discovered which has the following ionization energies: IE1 IE2 IE3 IE4 IE5 127 kJ/mol 287 kJ/mol 625 kJ/mol 2651 kJ/mol 3540 kJ/mol Which group do you suppose this new element belongs in? page 3 of 3