Module Four III: Part B1 Dot Structures via Formal Charge 7 points

Using a periodic chart draw the electron dot/stick structures of the following molecules. Use the method of formal charges to show the best structure: (Steric Numbers 2-6)

H₂SO₄ Also look at: H₂SO₃

Formal Charge

=

Valence Electrons

-

Nonbonding Val Electrons

-

Bonding e^1- 2

=

Total

H₃PO₄ Also look at: H₃PO₃

Formal Charge

=

Valence Electrons

-

Nonbonding Val Electrons

-

Bonding e^1- 2

=

Total

HClO₄ Also Look at: HClO₃ HClO₂ HClO

Formal Charge

=

Valence Electrons

-

Nonbonding Val Electrons

-

Bonding e^1- 2

=

Total

SO₂

Formal Charge

=

Valence Electrons

-

Nonbonding Val Electrons

-

Bonding e^1- 2

=

Total

SO₃

Formal Charge

=

Valence Electrons

-

Nonbonding Val Electrons

-

Bonding e^1- 2

=

Total

SF₆

Formal Charge

=

Valence Electrons

-

Nonbonding Val Electrons

-

Bonding e^1- 2

=

Total

SF₄

Formal Charge

=

Valence Electrons

-

Nonbonding Val Electrons

-

Bonding e^1- 2

=

Total

SbCl₅

Formal Charge

=

Valence Electrons

-

Nonbonding Val Electrons

-

Bonding e^1- 2

=

Total

PCl₅ Also look at PCl₃

Formal Charge

=

Valence Electrons

-

Nonbonding Val Electrons

-

Bonding e^1- 2

=

Total

AsF₅

Formal Charge

=

Valence Electrons

-

Nonbonding Val Electrons

-

Bonding e^1- 2

=

Total

SeF₆

Formal Charge

=

Valence Electrons

-

Nonbonding Val Electrons

-

Bonding e^1- 2

=

Total

HArF (first Nobel Gas Molecule)

Formal Charge

=

Valence Electrons

-

Nonbonding Val Electrons

-

Bonding e^1- 2

=

Total

Br₂^1-

Formal Charge

=

Valence Electrons

-

Nonbonding Val Electrons

-

Bonding e^1- 2

=

Total

XeF₄

Formal Charge

=

Valence Electrons

-

Nonbonding Val Electrons

-

Bonding e^1- 2

=

Total

XeO₄

Formal Charge

=

Valence Electrons

-

Nonbonding Val Electrons

-

Bonding e^1- 2

=

Total

BrCl₃

Formal Charge

=

Valence Electrons

-

Nonbonding Val Electrons

-

Bonding e^1- 2

=

Total

PCl₆^1-

Formal Charge

=

Valence Electrons

-

Nonbonding Val Electrons

-

Bonding e^1- 2

=

Total

BrF₄¹⁺

Formal Charge

=

Valence Electrons

-

Nonbonding Val Electrons

-

Bonding e^1- 2

=

Total

SO₂Cl₂

Formal Charge

=

Valence Electrons

-

Nonbonding Val Electrons

-

Bonding e^1- 2

=

Total

KrF₂

Formal Charge

=

Valence Electrons

-

Nonbonding Val Electrons

-

Bonding e^1- 2

=

Total

Other Ions/Compounds to consider which may be the exam question:

ClF₅ AsF₆^1- SeF₄ PF₃Cl₂ I₃^1- BrF₅

Reading Reference: Sections 8.5 Octet Rule and 8.7 Formal Charge (page 374)

Reference Octet Rule: B. Dot Structures of Covalent Compounds Section 2.10, 6.6, 7.1, 7.5, 7.6

Octet Rule Answers: http://www.fccj.us/chm2045/SampleTest/45M4bAnswers.htm