Solids And Unit Cells

Based on electronic configurations, which of the following species would you predict to be most magnetic?

• Sc

• Ti

• V

• Cr

Which factors contribute to the increase in atomic radius?

• Removal of electron shells and decrease in effective nuclear charge

• Removal of electron shells and increase in effective nuclear charge

• Addition of electron shells and decrease in effective nuclear charge

• Addition of electron shells and increase in effective nuclear charge

What is the electron configuration for the zinc ion?

• 1s2 2s2 2p6 3s2 3p6 3d10

• 1s2 2s2 2p6 3s2 3p6 4s2 3d8

• 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2

• 1s2 2s2 2p6 3s2 3p6 4d10

What is the electron configuration for the zinc atom in the ground state?

• 1s2 2s2 2p6 3s2 3p6 4s2 3d10

• 1s2 2s2 2p6 3s2 3p6 4s2 4d10

• 1s2 2s2 2p6 3s2 3p6 4d10

• 1s2 2s2 2p6 3s2 3p6 3d10

Going down a group in the periodic table.

• electronegativity decreases.

• the metallic properties increase.

• ease of cation formation increases.

Sulfur has a lower ionization energy than chlorine because 

• the effective nuclear charge of sulfur is less than that of chlorine. 
• the effective nuclear charge of sulfur is greater than that of chlorine. 
• False; sulfur has a greater ionization en- ergy than chlorine. 
• sulfur elevates one of its p electrons to a d orbital, thus making it easier to remove the electron. 

From the data  which element is likely to be a metal? 

• 2
• 3
• 4
• 5

Let X be a hypothetical element.  Which of the following would be largest?

• X^2-
• X^1-
• X
• X¹⁺

Which of the following statements about periodic trends is/are true?
I. Atomic radius decreases from left to right across a period because Z_eff increases.
II. Ionization energy increases from top to bottom in a group because the distance of the valence electrons from the nucleus increases.
III. Electronegativity increases from left to right across a period because Z_eff decreases.

• I only
• I and II only
• II and III only
• II only

In the neutral Al atom, what are the effective nuclear charges for a 1s electron and a valence electron, respectively? 

• +13; +3 
• +10; +13
  
• +12; +3 
• +3; +3