Covalent bonding assignment and quiz

On a sheet of paper, draw the Lewis structure for the following compound. A link to the periodic table has been provided for you. PCl5

Check all features below that you included in your Lewis structure. correct number of P and Cl atoms P as the central atom line (single bond) between P and each of the five Cl atoms six dots (electrons) associated with each Cl atom no other lines or dots

On a sheet of paper, draw the Lewis structure for the following compound. A link to the periodic table has been provided for you. SCl2

Check all features below that you included in your Lewis structure. correct number of S and Cl atoms S as the central atom line (single bond) between S and each of the two Cl atoms six dots (electrons) associated with each Cl atom four dots (electrons) associated with the S atom no other lines or dots

On a sheet of paper, draw the Lewis structure for the following compound. A link to the periodic table has been provided for you. SO3

Check all features below that you included in your Lewis structure. correct number of S and O atoms S as the central atom two lines (double bond) between S and one and only one of the three O atoms line (single bond) between S and the other two O atoms not doubled bonded to O four dots (electrons) associated with the O atom double bonded to S six dots (electrons) associated with the O atoms not double bonded to S no other lines or dots

Which element has the greatest number of valence electrons available for bonding? selenium boron calcium chlorine

Chlorine

Which compound is an exception to the octet rule? H2O HCl CCl4 ClF3

ClF3

Acetone and sodium chloride both have similiar mass. Explain why their other properties differ. Acetone: C3H6O, melting point = −94°C, liquid at room temperature, low electrical conductivity Sodium chloride: NaCl, melting point = 801°C, solid at room temperature, high electrical conductivity

Does your explanation contain the following? Acetone is a covalent compound, whereas sodium chloride is an ionic compound. Covalent compounds have strong bonds that do not break apart like ionic compounds do, and they do not conduct electric charge in solution. Covalent compounds do not have strong attractions between molecules and so have very low melting points, unlike ionic compounds.

Explain what is wrong with the following structure. es002-1.jpg

Does your explanation include the following? Hydrogen cannot have more than two electrons. Hydrogen bonds to only one other atom at a time. There are too many electrons in the final structure.

Which compound contains only nonpolar covalent bonds? O2 CO2 H2O NO3

O2

What is the best reason for the difference in properties of LiCl and C6H14O? LiCl and C6H14O have different atomic masses. Cl and O belong to different groups of the periodic table. One compound is ionic, and the other is metallic. One compound is covalent, and the other is ionic.

One compound is covalent, and the other is ionic.

Some atoms are exceptions to the octet rule by having an expanded octet. Which characteristic is needed for an atom to have an expanded octet? The atom has empty d-orbitals. The atom has more than eight valence electrons before bonding. The atom has empty p-orbitals. The atom has fewer than eight valence electrons after bonding.

The atom has empty d-orbitals.

Which statement about covalent compounds is true? They are able to melt at high temperatures. They are poor conductors of heat. They have strong intermolecular attractions. They have atomic bonds that are easy to break.

They are poor conductors of heat.

Which statement describes a property of covalent compounds? They have a high boiling point because of strong intermolecular forces. They have a low boiling point because of weak intermolecular forces. They have a low melting point because of strong intermolecular forces. They have a high melting point because of weak intermolecular forces.

They have a low boiling point because of weak intermolecular forces.

Identify arrows pointing to structures containing pi bonds

a

A solid compound in a sealed container was kept at a very low temperature in a freezer. When placed at room temperature, the substance quickly turned into a liquid. This compound is most likely which of the following? an ionic compound because it has a low boiling point a covalent compound because it has a low boiling point an ionic compound because it has a low melting point a covalent compound because it has a low melting point

a covalent compound because it has a low melting point

Which type of bond will form between two chlorine atoms? an ionic bond a metallic bond a polar covalent bond a nonpolar covalent bond

a non polar covalent bond

Which type of bond will most likely be found in HBr? an ionic bond a metallic bond a polar covalent bond a nonpolar covalent bond

a polar covalent bond

Identify arrows pointing to bonding electrons.

a,b,d

Identify arrows pointing to structures containing sigma bonds

a,b,d

Which element has the fewest valence electrons available for bonding? iodine aluminum carbon nitrogen

aluminum

Identify arrows pointing to nonbonding electrons.

c

Which structure shows the correct electron arrangement in CCl4?

d (C in the center connected to 4 chlorines by single bonds. Each Cl has 6 electrons)

How many valence electrons are available for bonding in silicon? four five eight fourteen

four

Which pair of elements will form a covalent bond? hydrogen and chlorine sodium and chlorine copper and bromine zinc and bromine

hydrogen and chlorine

How many valence electrons are available for bonding in bromine (Br)? one two five seven

seven