Concept explainers
(a)
Interpretation:
Resonance structures of
Concept Introduction:
Resonance structures refers to different forms of a same molecule which has same
(b)
Interpretation:
Resonance structures of
Concept Introduction:
Resonance structures refers to different forms of a same molecule which has same chemical bonding between the atoms but different electron distribution among the atoms in the molecule.
(c)
Interpretation:
Resonance structures of
Concept Introduction:
Resonance structures refers to different forms of a same molecule which has same chemical bonding between the atoms but different electron distribution among the atoms in the molecule.
(d)
Interpretation:
Electron dot structure of
Concept Introduction:
Electron dot structure also known as Lewis dot structure is a diagram representing a compound revealing the valence electrons of the constituent atoms.
Want to see the full answer?
Check out a sample textbook solutionChapter 4 Solutions
General Chemistry: Atoms First
- Write the Lewis structure for each molecule. These molecules do not follow the octet rule.(a) BCl3(b) NO2(c) BH3arrow_forwardDraw all possible resonance structures for each of these compounds. Determine the formal charge on each atom in each of the resonance structures:(a) O3(b) SO2(c) NO2 −(d) NO3−arrow_forwardThese species do not obey the octet rule. Draw a Lewis structure for each, and state the type of octet-rule exception:(a) PF₆(b) ClO₃(c) H₃PO₃(one P−H bond)arrow_forward
- Iodine forms a series of fluorides (listed here). Write Lewis structures for each of the four compounds and determine the formal charge of the iodine atom in each molecule:(a) IF(b) IF3(c) IF5(d) IF7arrow_forwardCalculate the enthalpy change for the following reactions using the bond enthalpy given below. (Bond enthalpy/kJ : H−H = 436, C−H = 413, C=O = 799, O=O = 495, O−H = 463) (a) H2(g) + 1⁄2O2(g) → H2O(g) (b) CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)arrow_forward3) The molecule diphosphorus tetraoxide (P,O,) has two central atoms and four different resonance structures that do not violate the octet rule. Draw two of these resonance structures below. 4) The compound acetone is a common solvent. It has a chemical formula of CH,COCH, Acetone has three central atoms. (a) Draw the Lewis Dot structure for acetone. (b) Give the Ideal Bond Angle for all three central atoms. 5) Four covalent molecules are drawn below. :o: H. H-CH H H (1) (2) (3) (4) a) Define each of these molecules as polar or non-polar. (1) (2) (3) b) Describe the type of intermolecular force that each molecule would use: (1) (2) (3) (4)arrow_forward
- Write Lewis structures for the following molecules or ions. (Assign lone pairs, radical electrons, and atomic charges where appropriate.) (a) BrF3 (b) AsF5 (c) BI3 (d) AsF6−arrow_forwardDraw Lewis structures for each of the following compounds. In each case, specify the number of valence electrons surrounding the central atom. (Assign lone pairs and radical electrons where appropriate.) (Assume the central atom does not contain an expanded octet.) (a) bromine dioxide (BrO2) (b) beryllium bromide (BeBr2) (c) phosphorus pentafluoride (PF5)arrow_forwardDraw Lewis structures for HFO4, HFO3, HC0O4, HC0O3, HCO2. (These molecules have the halogen atom as the central atom. All O atoms are attached to the halogen. The hydrogen atom is bonded to one of the O atoms.) Use formal charges to determine which molecule is least likely to occur in nature. (A) HFO4 (B) HC(O2 (C) HC!O3 (D) HFO3 (E) HC\O4 DO000arrow_forward
- Cyanogen (CN)2 is known as pseodohalogen because it has some properties like halogens. It is composed of two CN’s joined together.(i) Draw the Lewis structure for all the possible combination for (CN)2.(ii) Calculate the formal charge and determine which one of the structures that you have drawn is most stable.(iii) For the stable structure, determine the geometry around the two central atoms.(iv) For the stable structure, draw the dipole arrows for the bonds.(v) Base on the stable structure, determine the polarity of molecule and state your reason.arrow_forwardWhich two species have the same number of lone electron pairs in their Lewis structures?(a) H2O and H3O+(b) NH3 and H3O+(c) NH3 and CH4(d) NH3 and NH4+arrow_forwardThese species do not obey the octet rule. Draw a Lewis structure for each, and state the type of octet-rule exception: (a) PF6- (b) ClO3 (c) H3PO3 (one P-H bond)arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning