Rank the following in order of increasing atomic radius: Ba, F,Cr ,Si

Write the electron configurations far each of the following elements: (a) Sc. (b) Ti. (c) Cr. (d) Fe. (e) Ru

Name and give the symbol of the element that has the characteristic given below. (a) Its electron configuration in the excited state can be 1s22s22p63s1 3p3. (b) It is the least electronegative element in period 3. (c) Its +3 ion has the configuration [36Kr]. (d) It is the halogen with the largest atomic radius. (e) It has the largest ionization energy in Group 16.

Write the ground state electron configuration for (a) Mg, Mg2+(b) N, N3- (c) Ti, Ti4+ (d) Sn2+ Sn4+

6.82 A particular element has the following values for its first four ionization energies: 900, 1760, 14, 850, and 21,000 kJ/mol. Without consulting a list of ionization energy values, determine what group in the periodic table this element belongs in.

The following numbers are the ratios of second ionization energy to first ionization energy: Na: 9.2 Mg: 2.0 Al: 3.1 Si: 2.0 P: 1.8 S: 2.3 Cl: 1.8 Ar: 1.8 Explain these relative numbers.

Which of the following statements is(are) true? a. F has a larger first ionization energy than does Li. b. Cations are larger than their parent atoms. c. The removal of the first electron from a lithium atom (electron configuration is ls2 2s1 ) is exothermic-that is, removing this electorn gives off energy. d. The He atom is larger than the H+ ion. e. The Al atorn is smaller than the Li atom.

Arrange the following groups of atoms in order of increasing size. a. Rb, Na, Be b. Sr, Se, Ne c. Fe, P, O

Based on their positions in the periodic table, predict which has the smallest atomic radius: Mg, Sr, Si, Cl, I.

What is the electron configuration of the Ba3+ ion? Suggest a reason why this ion is not normally found in nature.