Textbook Question
Draw Lewis structures for the following: (f) NH2OH
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Ch.8 - Basic Concepts of Chemical Bonding
Chapter 8, Problem 51
Write Lewis structures that obey the octet rule for each of the following, and assign oxidation numbers and formal charges to each atom: (a) OCS (b) SOCl2 (S is the central atom) (c) BrO3- (d) HClO2 (H is bonded to O)
Verified step by step guidance1
Step 1: Identify the total number of valence electrons for each molecule or ion. For each atom, use the periodic table to determine the number of valence electrons and sum them up, adjusting for any charges in ions.
Step 2: Draw a skeletal structure for each molecule or ion. Typically, the least electronegative atom is placed in the center (except for hydrogen, which is always terminal). Connect the atoms with single bonds initially.
Step 3: Distribute the remaining valence electrons as lone pairs to satisfy the octet rule for each atom, starting with the outer atoms and moving towards the central atom. Remember that hydrogen only needs 2 electrons.
Step 4: If any atoms do not have a complete octet, consider forming double or triple bonds by converting lone pairs from adjacent atoms into bonding pairs.
Step 5: Assign oxidation numbers and formal charges. For oxidation numbers, use the rules based on electronegativity and known oxidation states. For formal charges, use the formula: Formal Charge = (Valence Electrons) - (Non-bonding Electrons) - 0.5*(Bonding Electrons).
Related Practice
Textbook Question
Write Lewis structures for the following: (a) H2CO (both
H atoms are bonded to C), (b) H2O2, (c) C2F6 (contains
a C¬C bond), (d) AsO33 - , (e) H2SO3 (H is bonded to O), (f) NH2Cl.
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Textbook Question
Which one of these statements about formal charge is true? (a) Formal charge is the same as oxidation number. (b) To draw the best Lewis structure, you should minimize formal charge. (c) Formal charge takes into account the different electronegativities of the atoms in a molecule. (d) Formal charge is most useful for ionic compounds. (e) Formal charge is used in calculating the dipole moment of a diatomic molecule.
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Textbook Question
For each of the following molecules or ions of sulfur and oxygen, write a single Lewis structure that obeys the octet rule, and calculate the oxidation numbers and formal charges on all the atoms: (c) SO32- Write a single Lewis structure that obeys the octet rule for SO32- and assign the formal charges on all the atoms.
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Textbook Question
(b) With what allotrope of oxygen is it isoelectronic?
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Textbook Question
Consider the formate ion, HCO2-, which is the anion formed when formic acid loses an H+ ion. The H and the two O atoms are bonded to the central C atom. (b) Are resonance structures needed to describe the structure?
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