(a)
Interpretation:
Given Lewis structure is to be drawn using line structure.
Concept introduction:
Line structures are compact like condensed structures. When drawing line structures, carbon atoms and hydrogen atoms attached to them are not drawn explicitly. A carbon atom is implied at the intersection of two bonds and at the end of each bond. All the other atoms except carbon and hydrogen are shown explicitly. Non-bonding electrons are usually not shown unless they are important to emphasize an aspect of the atom.
(b)
Interpretation:
Given Lewis structure is to be drawn using line structure.
Concept introduction:
Line structures are compact like condensed structures. When drawing line structures, carbon atoms and the hydrogen atoms attached to them are not drawn explicitly. A carbon atom is implied at the intersection of two bonds and at the end of each bond. All the other atoms except carbon and hydrogen are shown explicitly. Non-bonding electrons are usually not shown unless they are important to emphasize an aspect of the atom.
(c)
Interpretation:
Given Lewis structure is to be drawn using line structure.
Concept introduction:
Line structures are compact like condensed structures. When drawing line structures, carbon atoms and the hydrogen atoms attached to them are not drawn explicitly. A carbon atom is implied at the intersection of two bonds and at the end of each bond. All the other atoms except carbon and hydrogen are shown explicitly. Non-bonding electrons are usually not shown unless they are important to emphasize an aspect of the atom.
(d)
Interpretation:
Given Lewis structure is to be drawn using line structure.
Concept introduction:
Line structures are compact like condensed structures. When drawing line structures, carbon atoms and the hydrogen atoms attached to them are not drawn explicitly. A carbon atom is implied at the intersection of two bonds and at the end of each bond. All the other atoms except carbon and hydrogen are shown explicitly. Non-bonding electrons are usually not shown unless they are important to emphasize an aspect of the atom.
(e)
Interpretation:
Given Lewis structure is to be drawn using line structure.
Concept introduction:
Line structures are compact like condensed structures. When drawing line structures, carbon atoms and the hydrogen atoms attached to them are not drawn explicitly. A carbon atom is implied at the intersection of two bonds and at the end of each bond. All the other atoms except carbon and hydrogen are shown explicitly. Non-bonding electrons are usually not shown unless they are important to emphasize an aspect of the atom.
(f)
Interpretation:
Given Lewis structure is to be drawn using line structure.
Concept introduction:
Line structures are compact like condensed structures. When drawing line structures, carbon atoms and the hydrogen atoms attached to them are not drawn explicitly. A carbon atom is implied at the intersection of two bonds and at the end of each bond. All the other atoms except carbon and hydrogen are shown explicitly. Non-bonding electrons are usually not shown unless they are important to emphasize an aspect of the atom.
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Chapter 1 Solutions
Organic Chemistry: Principles And Mechanisms: Study Guide/solutions Manual (second)
- 1. For the polyatomic ion NO3-, answer the following: (a) Number of valence electrons in the ion (b) Identity of the central atom (c) Number of electron groups on the central atom (d) Number of bonding groups on the central atom (e) Number of double bonds in the ion (f) Number of single bonds in the ion (g) Number of unpaired electrons on the central atom (h) Shape of the polyatomic ion (i) Name of the polyatomic ionarrow_forwardQuestion: Consider a hypothetical molecule, X₄Y₃, composed of four atoms of element X and three atoms of element Y. The molecule is in a gaseous state. a) According to the octet rule, which elements are likely to form multiple bonds in this molecule? Explain your reasoning. b) Calculate the total number of valence electrons in X₄Y₃. c) Based on the total number of valence electrons, determine the formal charge on each atom in X₄Y₃.arrow_forward(1) Determine if the molecule is ionic or covalent (2) Provide the IUPAC name of each of the following: Molecule IUPAC Name Na 2 (SO4) NH4 (NO3 ) K CI to Mg (CrO4) Li 2 (HPO4)arrow_forward
- Draw the VSEPR sketch for each of the following showing the polarity of each bond. Describe each molecule as either polar or nonpolar. (b) GaH3 (d) CH2FCl (e) C2H2arrow_forwardDetermine the if IONIC or COVALENT. In capital letters only. (d) CoBr2(e) K2S(f)COarrow_forward(B). Compare between ionic compounds with covalent compoundsarrow_forward
- 5. b) c) Lewis dot diagram. a) What is a double covalent bond? Illustrate double covalent bonding using a Lewis dot diagram of an oxygen molecule. What is a triple covalent bond?arrow_forwardDraw the molecules in Problem 1.61 using line structuresarrow_forwardFor the polyatomic ion NO3-, answer the following: (a) total number of valence electrons in the ion (enter a number only) (b) identity of the central atom (element symbol) Now draw the Lewis Structure and answer the following questions: (c) number of electron groups on the central atom (enter a number only) (d) number of bonding groups on the central atom (enter a number only) (e) number of double bonds in the ion (enter a number only) (f) number of single bonds in the ionarrow_forward
- Considering only ions with charges of 1+,2+,1, and 2 or neutral atoms, give the symbols for four species that are isolectronic with the chloride ion, Cl.arrow_forwardC4H10O is the formula of diethyl ether. The same group of atoms is attached on either side of the oxygen atom. Draw the Lewis diagram. Diethyl ether was among the first anesthetics used in surgery, but it has been largely replaced by safer anesthetics today.arrow_forwardWhich elements on the periodic table (other than H) are likely to form a+1 cation?arrow_forward
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