11. Bonding & Molecular Structure

Lewis Dot Structures: Neutral Compounds

11. Bonding & Molecular Structure

Lewis Dot Structures: Neutral Compounds

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Lewis Dot Structures: Neutral Compounds

Lewis Dot Structures: Neutral Compounds Example 1

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How to draw Lewis structures for covalent compounds - Dr K

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How to draw Lewis structures for covalent compounds - Dr K

Bonding Models and Lewis Structures: Crash Course Chemistry #24

Lewis Dot Structures for Covalent Compounds - Part 1 CLEAR & SIMPLE

Lewis Structures for Covalent Molecules: Step-by-Step

Steps To Draw Lewis Structures

Lewis Diagrams Made Easy: How to Draw Lewis Dot Structures

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Multiple Choice

Determine the Lewis Dot Structure for the disulfur dichloride molecule, S₂Cl₂.

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Multiple Choice

How many lone pairs are on the central element for the following compound:AsH₃.

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Multiple Choice

How many total bonding electrons are on the central element for the following compound:CO₂.

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Multiple Choice

How many lone pairs are on the central element for the following compound:NOCl

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Multiple Choice

Determine the Lewis Dot Structure for the silicon tetrabromide molecule, SiBr₄.

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Open Question

Determine the Lewis Dot Structure for the diazene molecule, N₂H₂.

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Textbook Question

The partial Lewis structure that follows is for a hydrocarbon molecule. In the full Lewis structure, each carbon atom satisfies the octet rule, and there are no unshared electron pairs in the molecule. The carbon—carbon bonds are labeled 1, 2, and 3. (a) How many hydrogen atoms are in the molecule?

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Textbook Question

(b) How many nonbonding electrons surround the Xe in XeF2?

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Textbook Question

How many nonbonding electron pairs are there in each of the following molecules: (b) CO

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Textbook Question

How many nonbonding electron pairs are there in each of the following molecules: (a) N1CH323

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Textbook Question

Using Lewis symbols and Lewis structures, make a sketch of the formation of NCl3 from N and Cl atoms, showing valence-shell electrons. (e) How many lone pairs of electrons are in the NCl3 molecule?

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Textbook Question

Using Lewis symbols and Lewis structures, diagram the formation of BF3 from B and F atoms, showing valence-shell electrons. (c) How many valence electrons surround the B in the BF3 molecule?

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Textbook Question

(b) How many bonding electrons are in the structure?

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Textbook Question

The following ball-and-stick molecular model is a representation of thalidomide, a drug that causes birth defects when taken by expectant mothers but is valuable for its use against leprosy. The lines indicate only the connections between atoms, not whether the bonds are single, double, or triple. (Red = O, gray = C, blue = N, ivory = H). Give the formula of thalidomide, and indicate the positions of multiple bonds and lone pairs.

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Textbook Question

Draw Lewis structures for the following: (d) CH2O (C the central atom)

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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

Write the Lewis structure for each molecule. a. PH3

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Textbook Question

(b) Draw the Lewis structures of two example THMs.

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Textbook Question

Write the Lewis structure for each molecule. a. SF2

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Textbook Question

Write the Lewis structure for each molecule. b. SiH4

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Textbook Question

Write the Lewis structure for each molecule. d. CH3SH (C and S central)

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Textbook Question

Write the Lewis structure for each molecule. a. CH2O b. C2Cl4 c. CH3NH2 d. CFCl3 (C central)

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Textbook Question

Vinyl chloride, C2H3Cl, is a gas that is used to form the important polymer called polyvinyl chloride (PVC). Its Lewis structure is (a) What is the total number of valence electrons in the vinyl chloride molecule?

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Textbook Question

Benzaldehyde, C7H6O, is a fragrant substance responsible for the aroma of almonds. Its Lewis structure is

(e) How many valence electrons remain in nonbonding pairs in the molecule?

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Textbook Question

Benzaldehyde, C7H6O, is a fragrant substance responsible for the aroma of almonds. Its Lewis structure is

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Textbook Question

Write the Lewis structure for each molecule or ion. d. C2H4

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Textbook Question

Write the Lewis structure for each molecule or ion. a. H3COCH3

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Textbook Question

In the vapor phase, BeCl2 exists as a discrete molecule. (a) Draw the Lewis structure of this molecule, using only single bonds. Does this Lewis structure satisfy the octet rule?

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Textbook Question

Identify the third-row elements, X, that form the following ions. (a)

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Textbook Question

Identify the fourth-row elements, X, that form the following compounds. (a)

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Textbook Question

Write the Lewis structure for each molecule (octet rule not followed). b. NO2

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Textbook Question

Ibuprofen 1C13H18O22, marketed under such brand names as Advil and Motrin, is a drug sold over the counter for treatment of pain and inflammation. Complete the structure of ibuprofen by adding hydrogen atoms and lone pairs where needed.

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Textbook Question

Write an appropriate Lewis structure for each compound. Make certain to distinguish between ionic and molecular compounds. b. ClF5

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Textbook Question

Amino acids are the building blocks of proteins. The simplest amino acid is glycine (H2NCH2COOH). Draw a Lewis structure for glycine. (Hint: The central atoms in the skeletal structure are nitrogen and the two carbon atoms. Each oxygen atom is bonded directly to the right-most carbon atom.)

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Textbook Question

Formic acid is responsible for the sting of ant bites. By mass, formic acid is 26.10% C, 4.38% H, and 69.52% O. The molar mass of formic acid is 46.02 g/mol. Determine the molecular formula of formic acid and draw its Lewis structure.

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Textbook Question

1,2-dihydroxybenzene is obtained when two of the adjacent hydrogen atoms in benzene are replaced with an OH group. A skeleton of the molecule is shown here. (a) Complete a Lewis structure for the molecule using bonds and electron pairs as needed.

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Textbook Question

Draw the Lewis structure for each organic compound from its condensed structural formula. e. CH3CHO

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Textbook Question

Draw the Lewis structure for each organic compound from its condensed structural formula. c. CH3COCH3

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Textbook Question

Draw the Lewis structure for each organic compound from its condensed structural formula. b. CH3OCH3

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Textbook Question

Draw the Lewis structure for urea, H2NCONH2, one of the compounds responsible for the smell of urine. (The central carbon atom is bonded to both nitrogen atoms and to the oxygen atom.) Does urea contain polar bonds? Which bond in urea is most polar?

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Textbook Question

Ammonia reacts with boron trifluoride to form a stable compound, as we saw in Section 8.7. (a) Draw the Lewis structure of the ammonia–boron trifluoride reaction product.

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Textbook Question

A compound composed of only carbon and hydrogen is 7.743% hydrogen by mass. Propose a Lewis structure for the compound.

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Textbook Question

A compound composed of only carbon and chlorine is 85.5% chlorine by mass. Propose a Lewis structure for the compound.

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Textbook Question

The mechanism for the oxidation of HBr by O2 to form 2 H2O and Br2 is shown in Exercise 14.74. (c) Draw a plausible Lewis structure for the intermediate HOOBr. To what familiar compound of hydrogen and oxygen does it appear similar?

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Textbook Question

Methyl isocyanate, CH3NCO, was made infamous in 1984 when an accidental leakage of this compound from a storage tank in Bhopal, India, resulted in the deaths of about 3800 people and severe and lasting injury to many thousands more. (a) Draw a Lewis structure for methyl isocyanate.

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Textbook Question

Gaseous iodine pentafluoride, IF5, can be prepared by the reaction of solid iodine and gaseous fluorine: I21s2 + 5 F21g2¡2 IF51g2 A 5.00-L flask containing 10.0 g of I2 is charged with 10.0 g of F2, and the reaction proceeds until one of the reagents is completely consumed. After the reaction is complete, the temperature in the flask is 125 °C. (c) Draw the Lewis structure of IF5.

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Textbook Question

When 0.500 mol of N2O4 is placed in a 4.00-L reaction vessel and heated at 400 K, 79.3% of the N2O4 decom- poses to NO2. (b) Draw an electron-dot structure for NO2, and rational- ize the structure of N2O4.

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Open Question

Complete these structures by adding electrons, in the form of dots, as needed.

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Open Question

Choose a likely identity for x, y, and z in these structures.

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Open Question

Which molecule has only one lone (non-bonding) pair in its lewis model?

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Open Question

In a Lewis structure, _______. (select all that apply.)

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Open Question

What is the maximum number of covalent bonds a carbon atom can form with other atoms?

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Open Question

How many double bonds are in the lewis structure for carbon dioxide, CO₂?

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Open Question

How does adding a lone pair affect the position of existing atoms and lone pairs?

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Open Question

Draw a Lewis structure for Cl₂O₂ based on the arrangement of atoms shown above.

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Open Question

Which model best represents the Lewis dot structure for phosphorus trichloride (PCl₃)?

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Open Question

Determine the number of valence electrons in hcn and then draw the corresponding lewis structure.

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Open Question

Which model best represents the Lewis dot structure for phosphorus trichloride (PCl₃)?

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Open Question

Draw a Lewis structure for Cl₂O₂ based on the arrangement of atoms shown above.

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Open Question

Determine the number of valence electrons in BrF₅ and then draw the corresponding lewis structure.

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Open Question

What is the total number of outer (valence) electrons in sulfur dioxide, SO₂?

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Open Question

How many valence electrons must be accounted for in the Lewis structure of chloroethane (C₂H₅Cl)?

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Open Question

The Lewis structure of N₂H₂ shows ________.

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11. Bonding & Molecular Structure

Lewis Dot Structures: Neutral Compounds

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