Ionic Bonds
When does a covalent bond form?
A covalent bond forms when atoms share electrons.
What is meant by the term "polarity" in the context of chemical bonding?
In the context of chemical bonding, "polarity" refers to the unequal sharing of electrons in a covalent bond, resulting in a partial positive or partial negative charge on the atoms involved. This unequal distribution of electrons occurs when there is a difference in electronegativity between the bonded atoms. As a result, one atom has a slightly negative charge (δ-) and the other has a slightly positive charge (δ+), leading to a polar covalent bond. Additionally, the overall polarity of a molecule is determined by the spatial arrangement of polar bonds within the molecule.
What are intermolecular forces, and how do they differ from intramolecular forces?
Intermolecular forces are forces between molecules. Intramolecular forces are forces within molecules (ionic, molecular, metallic bonding)
What classifies as the difference in electronegativity values for a polar bond?
Anything between 0.5 and 1.6
What are the three major types of intermolecular forces? Rank them in terms of strength.
London dispersion, Dipole-Dipole interaction, and Hydrogen bonding. They are listed from weakest to strongest.
What is another name for a covalent bond?
molecular bond
Is CH4 a polar molecule? Explain
No because it is symmetrical
Explain the origin and characteristics of London dispersion forces.
The origin of London dispersion forces can be attributed to momentary dipoles As electrons move around a molecule, they may become momentarily concentrated on one side, creating a temporary dipole. This temporary dipole induces a corresponding dipole in a neighboring molecule, resulting in an attractive force between the two molecules.
London dispersion is the weakest type of intermolecular force.
Draw the Lewis Dot structure and write the name for Fe2O3
Iron (III) Chloride
What is the difference between a single, double, and triple covalent bond?
In a single covalent bond, two atoms share one pair of electrons. In a double covalent bond, two atoms share two pairs of electrons. In a triple covalent bond, two atoms share three pairs of electrons. As the number of shared electron pairs increases, the bond becomes stronger and shorter. Triple bonds are stronger and shorter than double bonds, and double bonds are stronger and shorter than single bonds.
Is H2O a polar molecule? Explain
Yes, because it is asymmetrical
Define dipole-dipole interactions.
Dipole-dipole interactions are intermolecular forces that occur between polar molecules. These interactions result from the attraction between the partial positive (+) end of one polar molecule and the partial negative (-) end of another polar molecule, due to the unequal distribution of electrons within the molecules.
Why are metals so malleable?
"sea of mobile electrons"
How does the polarity of a molecule affect its physical properties, such as boiling point and solubility?
Polar molecules tend to have higher boiling points than non-polar molecules. This is because polar molecules exhibit stronger intermolecular forces, such as dipole-dipole interactions and hydrogen bonding, which require more energy to overcome, resulting in a higher boiling point.
Explain the conditions under which hydrogen bonding occurs and provide examples of molecules that exhibit hydrogen bonding.
Hydrogen bonding occurs when a hydrogen atom is covalently bonded to a highly electronegative atom (such as nitrogen, oxygen, or fluorine) and is also attracted to an unshared pair of electrons on another electronegative atom. The conditions for hydrogen bonding include the presence of hydrogen atoms bonded to strongly electronegative elements and the availability of unshared electron pairs on neighboring atoms.