Identify the atom that has each ground-state electron ...

[krzymel]

Identify the atom that has each ground-state electron configuration.
   
  (a) 1s²2s²2p⁶3s²3p⁴
  (b) 1s²2s²2p⁴

Question 2

Write ground-state electron configuration for each atom. After each atom is its atomic number in parentheses.
   
 

 
• Sodium (11)

 
• Magnesium (12)

 
• Oxygen (8)

 
• Nitrogen (7)

 

Question 3

Draw three contributing structures of the following compound (called guanidine) and state the hybridization of the four highlighted atoms. In which orbitals do the three lone pairs drawn reside
 

Question 4

Estimate the relative contribution of the members in each set of contributing structures.
 

Question 5

Which sets are valid pairs of contributing structures?
 

Question 6

Draw the contributing structure indicated by the curved arrows. Show all valence electrons and all formal charges.

Question 7

Describe the bonding in these molecules in terms of hybridization of C and N, and the types of bonds between carbon and nitrogen, and if there are any lone pairs, describe what type of orbital contains these electrons.
  (a) CH₃-CH=CH₂
  ^(b) CH₃-NH₂

Question 8

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Question 9

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<sub>Question 10

Which molecules are polar? For each molecule that is polar, specify the direction of its dipole moment.

Question 11

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(c) H2O2
The H2 O2 molecule can rotate around the O-O single bond

Question 12

Predict all bond angles for these molecules.
  (a) CH3OH
  (b) PF3
  (c) H2CO3 (Carbonic Acid)

Question 13

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(c) H₂CO₃ (Carbonic Acid)

Question 14

Draw structural formulas for the four esters with molecular formula C₄H₈O₂.

Question 15

Draw condensed structural formulas for the two carboxylic acids with molecular formula C₄H₈O₂.

Question 16

Draw condensed structural formulas for the three ketones with molecular formula C₅H_{1 0}O.

Question 17

Draw structural formulas for the three secondary amines with molecular formula C₄H_{1 1}N.

Question 18

  Draw Lewis structures and condensed structural formulas for the four alcohols with molecular formula C₄H_{1 0}O.
 

   
  Classify each alcohol as primary, secondary, or tertiary.

Question 19

Draw Lewis structures, showing all valence electrons, for these molecules.
  (a) C₂H₆
  (b) CS₂
  (c) HCN

Question 20

Judging from their relative positions in the Periodic Table, which element in each set is more electronegative?
   
  (a) Lithium or potassium
  (b) Nitrogen or phosphorus
  (c) Carbon or silicon

[reelove4eva]

Answer to Question 1

(a) 1s²2s²2p⁶3s²3p⁴
Sulfur (16) has this ground-state electron configuration
(b) 1s²2s²2p⁴
Oxygen ( has this ground-state electron configuration

Answer to Question 2

• Sodium (11) Na (11 electrons) 1s² 2s² 2p⁶ 3s¹


• Magnesium (12) Mg (12 electrons) 1s² 2s² 2p⁶ 3s²


• Oxygen ( O (8 electrons) 1s² 2s² 2p⁴


• Nitrogen (7) N (7 electrons) 1s² 2s² 2p³

Answer to Question 3


Remember that if any significant contributing structure contains a  bond, then the hybridization of that atom must be able to accommodate the  bond. Consideration of the three significant contributing structures indicates that all of
the nitrogen atoms are sp2 hybridized because of the  bonding. To be consistent with the contributing structures,

two of the lone pairs on the original structure are in 2p orbitals, while the third resides in an sp2 orbital. Guanidine is one of many examples you will encounter in which the lone pair on nitrogen is delocalized into an adjacent  bond. Such delocalization of electron density in  orbitals is stabilizing and therefore favorable, a phenomenon that is best explained using quantum mechanical arguments (beyond the scope of this text) .


Answer to Question 4

The first structure makes the greater contribution in (a) and (b). In both cases, the second contributing structure involves the disfavored creation and separation of unlike charges.

Answer to Question 5

The set in (a) is a pair of contributing structures, while the set in (b) is not. The structure on the right in set (b) is not a viable contributing structure because there are five bonds to the carbon atom, implying 10 electrons in the valence shell, which can only hold a maximum of 8 electrons.

Answer to Question 6





Answer to Question 7

(a) CH₃-CH=CH₂

[krzymel]

Excellent

[isabelt_18]

Gracias!