Adv CHEM Fall Mid-Term Unit 4

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. 

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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 

Rank the following in terms of decreasing ionic radii.

• Na⁺, Mg²⁺, O²⁻, N³⁻, F⁻
  
• Na⁺, Mg²⁺, N³⁻, O²⁻, F⁻
  
• F⁻, O²⁻, N³⁻, Na⁺, Mg²⁺
  
• N³⁻, O²⁻, F⁻, Na⁺, Mg²⁺  

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The electronegativity of an atom generally ______ going up columns and _____ going right  to left across rows. An element like calcium  would most likely form a(n) _____ bond with  an element like nitrogen. 

• decreases; increases; covalent
  
• increases; decreases; covalent
  
• increases; decreases; ionic 
• decreases; increases; ionic
  

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

• 2
• 3
• 4
• 5

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F⁻ is bigger than F because 

• F⁻ has one more electron which causes greater electron repulsions in the outer orbitals, thus expanding the electron cloud. 
• F⁻ has one more electron so there is less effective shielding of the nuclear charge. 
• F⁻ has one less electron so there is less effective shielding of the nuclear charge. 
• F⁻ has one more electron which causes less electron repulsions in the outer orbitals, thus expanding the electron cloud. 

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What is the primary reason that atomic radius decreases as you move from left to right across the periodic table even though the number of electrons is increasing?

• All atoms in a given period of the table are the same size because the same main energy level is being filled.
• As electrons are added, they go into orbitals in new primary energy levels which are further from the nucleus so the atoms get larger.
• Increasing effective nuclear charge more strongly attracts the outermost electrons so the atoms get smaller.
• There is no clear trend, the atoms all have different radii.

Why is it harder to remove an electron from fluorine than from carbon, or, to put it another way, why are the valence electrons of fluorine more strongly bound than those of carbon?

• Carbon has a lower atomic mass than does fluorine.
• Fluorine has a greater effective core charge, Z_eff, than carbon.
• This statement is false; it takes very nearly the same ionization energy to remove an electron from both elements.
• Fluorine is more closer to having a completey filled octet than carbon.

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

• X^2-
• X^1-
• X
• X¹⁺

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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

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