Use the periodic table to determine the element corresponding to each electron configuration. d. [Kr] 5s²

Use the periodic table to determine each quantity. a. the number of 2s electrons in Li

Use the periodic table to determine each quantity. b. the number of 3d electrons in Cu d. the number of 4d electrons in Zr

Use the periodic table to determine each quantity. c. the number of 4p electrons in Br

Use the periodic table to determine each quantity.

b. the number of 3d electrons in Cr

Name an element in the fourth period (row) of the periodic table with the following: a. five valence electrons

Name an element in the fourth period (row) of the periodic table with the following: b. four 4p electrons

Name an element in the fourth period (row) of the periodic table with the following: c. three 3d electrons

Name an element in the fourth period (row) of the periodic table with the following: d. full s and p sublevels

Name an element in the third period (row) of the periodic table with the following: a. three valence electrons

Name an element in the third period (row) of the periodic table with the following: b. four 3p electrons

Name an element in the third period (row) of the periodic table with the following: c. six 3p electrons

Name an element in the third period (row) of the periodic table with the following: d. two 3s electrons and no 3p electrons

Determine the number of valence electrons in an atom of each element. a. Ba c. Ni d. S

Determine the number of valence electrons in an atom of each element. b. Cs

Determine the number of valence electrons in each element. Which elements do you expect to lose electrons in chemical reactions? Which do you expect to gain electrons? a. Al b. Sn c. Br d. Se

Which outer electron configuration would you expect to belong to a reactive metal? a. ns² b. ns²np⁶ c. ns²np⁵ d. ns²np²

Which outer electron configuration would you expect to belong to a reactive nonmetal? a. ns² b. ns²np⁶ c. ns²np⁵ d. ns²np²

Which outer electron configurations would you expect to belong to a noble gas? a. ns² b. ns²np⁶ c. ns²np⁵ d. ns²np²

Which outer electron configurations would you expect to belong to a metalloid? ns² b. ns²np⁶ c. ns²np⁵ d. ns²np²

According to Coulomb's law, which pair of charged particles has the lowest potential energy? a. a particle with a 1- charge separated by 150 pm from a particle with a 2+ charge b. a particle with a 1- charge separated by 150 pm from a particle with a 1+ charge c. a particle with a 1- charge separated by 100 pm from a particle with a 3+ charge

According to Coulomb's law, rank the interactions between charged particles from lowest potential energy to highest potential energy. a. a 1+ charge and a 1- charge separated by 100 pm b. a 2+ charge and a 1- charge separated by 100 pm c. a 1+ charge and a 1+ charge separated by 100 pm d. a 1+ charge and a 1- charge separated by 200 pm

Which experience a greater effective nuclear charge: the valence electrons in beryllium or the valence electrons in nitrogen? Why?

Arrange the atoms according to decreasing effective nuclear charge experienced by their valence electrons: S, Mg, Al, Si.

If core electrons completely shielded valence electrons from nuclear charge (i.e., if each core electron reduced nuclear charge by 1 unit) and if valence electrons did not shield one another from nuclear charge at all, what would be the effective nuclear charge experienced by the valence electrons of each atom? a. K

If core electrons completely shielded valence electrons from nuclear charge (i.e., if each core electron reduced nuclear charge by 1 unit) and if valence electrons did not shield one another from nuclear charge at all, what would be the effective nuclear charge experienced by the valence electrons of each atom? b. Ca

If core electrons completely shielded valence electrons from nuclear charge (i.e., if each core electron reduced nuclear charge by 1 unit) and if valence electrons did not shield one another from nuclear charge at all, what would be the effective nuclear charge experienced by the valence electrons of each atom? c. O d. C

In Section 3.6, we estimated the effective nuclear charge on beryllium's valence electrons to be slightly greater than 2+. What would a similar treatment predict for the effective nuclear charge on boron's valence electrons? Would you expect the effective nuclear charge to be different for boron's 2s electrons compared to its 2p electron? In what way? (Hint: Consider the shape of the 2p orbital compared to that of the 2s orbital.)

Choose the larger atom in each pair. a. Al or In b. Si or N c. P or Pb d. Si or Cl