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

Consider the collection of nonmetallic elements: B, As, O,
and I. (a) Which two would form the most polar single
bond?

Dipole arrow is representative of bond polarity between 2 elements and points towards a more EN element.

There is another choice in which the difference in electronegativity of the bonded elements is greater.

 The greater the difference in electronegativity, the greater the bond polarity. 

Which of the following is the most polar bond?

Electronegativity increases moving from left to right and going up a group.

Arrange the bonds in each of the following sets in order 
of increasing polarity: (c) C¬S, B¬F, N¬O.

You may have only calculated the bond dipole if the electron were completely transferred.  Compare this to the actual bond dipole.

The percent ionic character should be less than 100%.  Check your calculation you may have inverted a term.

Be sure that you converted the ratio of dipoles to a percentage.

Be sure that you are using a ratio of the actual dipole to the dipole if the electron were completely transferred.

 Determine the dipole of the bond if the electron were completely transferred, then calculate the percent ionic character using the formula for percent ionic character. 

What is the percent ionic character of a 125 pm bond which has a bond dipole of 4.5 D?

Bond Polarity, Electronegativity and Dipole Moment - Chemistry Practice Problems

(b) If you were to put HBr under very 
high pressure, so its bond length decreased significantly, 
would its dipole moment increase, decrease, or stay the 
same, if you assume that the effective charges on the atoms 
do not change?

Which of the following bonds would be the most polar without being considered ionic?

Polar Bonds, Polarity and Intermolecular Forces

Two dichloroethylene molecules with the same chemical formula
1C2H2Cl22, but different arrangements of atoms are shown.

(b) Which form of dichloroethylene has a dipole moment of 2.39 D, and which has a dipole moment of 0.00 D?

(b) It turns out that ozone, O3, has a small dipole moment. How is
this possible, given that all the atoms are the same?

A polar covalent bond would form in which of the following pairs of atoms

Dipole Moment Example 2

Match the following descriptions with the type of bond (ionic, nonpolar covalent, covalent). 
(a) One or more electrons are transferred from a metal to a nonmetal atom.

1.5 Polarity

Which of the substances CdBr2, P4, BrF3, MgO, NF3, BaCl2, POCl3, and LiBr contain bonds that are:
(b) nonpolar covalent?

(b) What would you expect for the magnitude and direction of the bond
dipoles in this series?

Dipole Moment

Electronegativity: bond character/bond type: electronegativity difference and predicting bond type

(c) The measured dipole moment of BrCl is 0.57 D. If you assume the 
bond length in BrCl is the sum of the atomic radii, what are 
the partial charges on the atoms in BrCl using the experimental 
dipole moment?

(a) From the data in Table 8.2, calculate the effective charges
on the Br atom of the HBr molecule in units of the
electronic charge, e.

Differences in EN between bonds help us classify the different types of bonds possible.

Which of the substances S8, CaCl2, SOCl2, NaF, CBr4, BrCl, LiF, and AsH3 contain bonds that are:
(a) largely ionic? 
(b) nonpolar covalent? 
(c) polar covalent?

The Chemical Bond: Covalent vs. Ionic and Polar vs. Nonpolar

Determine whether a bond between each pair of atoms would be pure covalent, polar covalent, or ionic.

The substance chlorine monoxide, ClO(g), is important in
atmospheric processes that lead to depletion of the ozone
layer. The ClO molecule has an experimental dipole moment
of 1.24 D, and the Cl¬O bond length is 160 pm. (b) Based on the
electronegativities of the elements, which atom would you
expect to have a partial negative charge in the ClO molecule?

Chemical Bonds: Ionic and Covalent

(b) Using these partial charges and the atomic radii given in Figure 
7.8, estimate the dipole moment of the molecule.

Which bond would you expect to be the most polar?

Order the following compounds according to the increasing ionic character of their bonds: CCl4, BaCl2, TiCl3, ClO2.

(c) Does the molecule BF2Cl have a dipole moment?

The iodine monobromide molecule, IBr, has a bond length
of 249 pm and a dipole moment of 1.21 D. (a) Which atom of
the molecule is expected to have a negative charge?

Which of the following correctly identifies the chemical bond between a carbon and oxygen atom?a) Polar Covalentb) Pure Covalentc) Nonpolar&nbsp;d) Ionic

Arrange the bonds in each of the following sets in order 
of increasing polarity: (b) O¬Cl, S¬Br, C¬P

Draw the Lewis structure for BrF with an arrow representing the 
dipole moment.

Molecular polarity | AP Chemistry | Khan Academy

A polar covalent bond would form in which one of the following pairs of atoms?

Ionic Bonds, Polar Covalent Bonds, and Nonpolar Covalent Bonds

Dipole Moment Example 1

The O¬H bond lengths in the water molecule 1H2O2 are
96 pm, and the H¬O¬H angle is 104.5°. The dipole moment
of the water molecule is 1.85 D. (b) Calculate the magnitude of the bond dipole of the O¬H bonds. (Note: You will need to use vector addition
to do this.)

Polar Covalent Bonds and Nonpolar Covalent bonds, Ionic Bonding - Types of Chemical Bonds

Determine if a bond between each pair of atoms would be pure
covalent, polar covalent, or ionic.
a. Br and Br 
b. C and Cl 
c. C and S 
d. Sr and O

For each bond, show the direction of polarity by selecting the correct partial charges.

(a) Does CS2 have a dipole moment? If so, in which direction 
does the net dipole point?

Which of the following bonds are polar? (a) C¬O, 
(b) Sl¬F, (c) N¬Cl, (d) C¬Cl. Which is the more electronegative 
atom in each polar bond?

Show the direction of polarity for each of the bonds in Problem 7.51 using the  notation. 
(b) Si-Li or Si-Cl

Which of the following substances contain bonds that are largely ionic?
(a) HF
(b) HI 
(c) PdCl2 
(d) BBr3 
(e) NaOH
(f) CH3Li

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Lewis Dot Structures: Neutral Compounds

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