1. Intro to General Chemistry

2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Lone pairs do not participate in bonding but contribute to the octet rule.

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.

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

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

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.

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.

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

Lewis Dot Structures: Neutral Compounds

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

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

Identify the fourth-row elements, X, that form the following compounds.
(a) <img src="https://lightcat-files.s3.amazonaws.com/problem_images/dd82270c5bd5e897-1670351232407.jpg" alt="" />

Write the Lewis structure for each molecule.
b. SiH4

How to draw Lewis structures for covalent compounds - Dr K

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

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?

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? <img src="https://lightcat-files.s3.amazonaws.com/problem_images/d5f3974190862824-1661181591962.jpg" alt="" />

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

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.

Lewis Dot Structure of CH2O where H follows the duet rule.

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?

Benzaldehyde, C7H6O, is a fragrant substance responsible for 
the aroma of almonds. Its Lewis structure is 
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/c4ae1e59f8456d60-1661186341623.jpg" alt="" /> 
(e) How many valence electrons remain in nonbonding pairs in the molecule?

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

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

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

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.
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/e3f0ce1581dc71ce-1670431554622.jpg" alt="" />

Lewis Structures for Covalent Molecules: Step-by-Step

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.)

Identify the third-row elements, X, that form the following ions.
(a) <img src="https://lightcat-files.s3.amazonaws.com/problem_images/e0dba4429077e2a2-1670351205437.jpg" alt="" />

Benzaldehyde, C7H6O, is a fragrant substance responsible for
the aroma of almonds. Its Lewis structure is
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/ef931ff33fceafea-1661186288973.jpg" alt="" />
(c) How many of the valence electrons are used to make s bonds in the molecule?

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.

Bonding Models and Lewis Structures: Crash Course Chemistry #24

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

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

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

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

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

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?

Write the Lewis structure for each molecule.
a. PH3

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

Lewis Dot Structures: Neutral Compounds Example 1

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

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.

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

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

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?

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

Write the Lewis structure for each molecule. 
a. SF2

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

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

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. 
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/7189a0c89f420e49-1670424785658.jpg" alt="" />

Lewis Structures

Lewis Diagrams Made Easy: How to Draw Lewis Dot Structures

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

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?

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.

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

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

Steps To Draw Lewis Structures

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?

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

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Lewis Dot Structures or Electron Dot Structures&nbsp;are diagrams that show how elements in a molecule use their valence electrons to form bonds.&nbsp;

Average Bond Order

Average Bond Order represents the average number of chemical bonds between a pair of bond elements.

Lewis Dot Structures: Ions

Lewis Dot Structures of Ions involves losing or gaining valence electrons to draw the most likely structure.&nbsp;

Octet Rule

The&nbsp;Octet Rule states that main-group elements will generally form enough bonds to obtain 8 electrons in their valence shell.&nbsp;

Lewis Dot Symbols

Lewis Dot Symbols represent the outer shell electrons of an element.&nbsp;

Lewis Dot Structures: Sigma & Pi Bonds

Sigma Bonds directly connect element together, while Pi Bonds provide insulation and protection for those bonds.&nbsp;

Lewis Dot Structures: Exceptions

Lewis Dot Structure Exceptions&nbsp;happen when the central element violates the Octet Rule.

Born Haber Cycle

In the Born-Haber Cycle, ionic solids are created through the ionization and eventual combination of elements.&nbsp;

Coulomb's Law

Coulomb's Law is used to determine the forces experienced by charged particles.&nbsp;

Chemical Bonds

A chemical bond is the connection&nbsp;of different elements through the sharing, transferring or pooling of electrons.&nbsp;

Resonance Structures

Resonance Structures are used to represent the different possible bonding arrangements of a molecule.

Lewis Dot Structures: Acids

Drawing the Lewis Dot Structure of Acids&nbsp;involves first drawing the polyatomic anion and then attaching the H+ ion.&nbsp;

Formal Charge

Formal Charge is the charge given to an element within a molecule when assuming equal sharing of electrons between bonded elements.&nbsp;

Bond Energy

Bond Energy is the amount of energy stored within a chemical bond.

Lattice Energy

Lattice Energy&nbsp;is the estimate for the strength of ionic bonds.&nbsp;

Dipole Moment

Dipole arrows are used anytime a molecule possesses a dipole moment, which happens when a molecule is polar.&nbsp;