Question

In: Chemistry

Draw a Lewis structure for each of the following compounds:

Draw a Lewis structure for each of the following compounds:

(a) C_2H_6 \hspace{.2cm} (b) C_2H_4 \hspace{.2cm} (c) C_2H_2 \hspace{.2cm} (d) C_3H_8 \hspace{.2cm} (e) C_3H_6 \hspace{.2cm} (f) CH_3OH

Solutions

Expert Solution

Solution

The task is to draw Lewis dot structures for the following compounds:

(a) C_2H_6 \hspace{.2cm} (b) C_2H_4 \hspace{.2cm} (c) C_2H_2 \hspace{.2cm} (d) C_3H_8 \hspace{.2cm} (e) C_3H_6 \hspace{.2cm} (f) CH_3OH

 

When drawing Lewis structures, first determine the number of valence electrons for each atom. The number of valence electrons is indicated by the group number.

Therefore, carbon has 4 (one on each side) and hydrogen 1.

'slader'

Then, connect atoms that can form more than one bond and place them in the centrum.

In the end, arrange hydrogens at terminals. Keep in mind the octet rule. The rule states that each atom tends to have 8 electrons in its valence shell (except hydrogen which tends to have a duet) in order to have a noble gas configuration and hence maximum stability.

 

(a) Since carbon can form more than one bond, connect the two carbons first and place them in the centrum. Three hydrogens go on each carbon and so the octet rule is satisfied.

'slader'


(b) In this case, by the distribution of hydrogens, the octet is not satisfied. Therefore, the two remaining unpaired electrons are shared between two carbons to form a double bond.

'slader'

 

(c) After the addition of hydrogens, each carbon is left with two unpaired electrons. So, four unpaired electrons are shared to form a triple bond so that each carbon would have an octet.

'slader'


(d) First, connect the three carbon atoms since carbon can form multiple bonds. By the distribution of hydrogens, each carbon achieves an octet.

'slader'

 

(e) A similar situation as in (b). There are not enough hydrogens for each carbon to have an octet, so two unpaired electrons are shared to form a double bond.

'slader'


(f) Oxygen has 6 valence electrons. Four of them make up for two lone electron pairs (not shared), whereas two unpaired electrons are shared with other atoms. Place carbon and oxygen in the centrum and add hydrogens at terminals. Do not forget to place two lone pairs on oxygen.

'slader'


Related Solutions

Draw a Lewis structure for each of the following compounds:
Draw a Lewis structure for each of the following compounds:(a) C_22​H_66​ \hspace{.2cm} (b) C_22​H_44​ \hspace{.2cm} (c) C_22​H_22​ \hspace{.2cm} (d) C_33​H_88​ \hspace{.2cm} (e) C_33​H_66​ \hspace{.2cm} (f) CH_33​OH
Draw the best Lewis structure for the following three compounds: ______, ______ and _______. The instructors...
Draw the best Lewis structure for the following three compounds: ______, ______ and _______. The instructors will choose three molecules from the following list for the exam. All structures must be perfect to get credit for this question. Possible compounds: CO2, CH2O, BH3, H2O, CH4, SF6, SF4, PCl5, ICl4 - , NH4 + , SF5, SF5
Draw the Lewis Dot Structure for the following compounds and then determine a) the hybridization of...
Draw the Lewis Dot Structure for the following compounds and then determine a) the hybridization of the central atom b) the electron group arrangement c) the bond angle around the central atom d) the molecular geometry. a) H3O+           b) NO3-                 c) O3      `                 d) HCN           e) CH3CH3
Draw Lewis structures for the following compounds.
Draw Lewis structures for the following compounds. a)  HCN b)  CS2 C)  HCCH   
Draw Lewis structures for each of the following compounds. In each case, specify the number of...
Draw Lewis structures for each of the following compounds. In each case, specify the number of valence electrons surrounding the central atom. a) bromine dioxide (BrO2) (Assume the central atom does not contain an expanded octet.) There are ___ valence electrons surrounding the central atom. b) beryllium fluoride (BeF2) There are___ valence electrons surrounding the central atom. c) phosphorus pentabromide (PBr5) There are ___ valence electrons surrounding the central atom.
For each of the following compounds draw an acceptable Lewis dot structure (CH3CH2)2CHCO2CH(CH3)2 HSO4 - sulfur...
For each of the following compounds draw an acceptable Lewis dot structure (CH3CH2)2CHCO2CH(CH3)2 HSO4 - sulfur tetrafluoride bromine trichloride dinitrogen pentoxide (CH3)2SO CH2Cl2
lewis structure for the compounds
lewis structure for the compounds XeO2 LiHCO3 CLO2
Draw a Lewis structure for each of the following molecules and ions. In each case the...
Draw a Lewis structure for each of the following molecules and ions. In each case the ions can only be corrected in one way. (a) Br2 (b) H2S (c) N2H4
Draw the Lewis structure for each of the following. IDENTIFY each first as being a simple...
Draw the Lewis structure for each of the following. IDENTIFY each first as being a simple ion, polyatomic ion, ionic compound (with or without a polyatomic ion), or covalent compound. Don’t forget to balance out the charge on the ionic compounds. REMEMBER: include brackets with a charge for ions! A. Nitrite Ion B. Nitrogen gas (hint: it's diatomic" C. Cyanide Ion D. Bromide Ion E. Sulfur Dioxide F. Ammonium Phosphate G. Sulfur Hexafluoride H. Bromine Pentachloride I. Chlorate Ion J....
For each of the following molecules, draw the most preferred Lewis structure and label each of...
For each of the following molecules, draw the most preferred Lewis structure and label each of the atoms with its formal charge. Question to consider: What is/are the main criteria for drawing a preferred Lewis structure? (a) TeF5 – (b) NO2 +
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT