Mastering Chemistry Assignment 6

Two hydrogen atoms interact to form a hydrogen molecule. Classify the following statements that describe the stages of bond formation in a hydrogen molecule according to the predominant force existing between the two hydrogen atoms.

Attractive force is predominant between the two atoms:

The two hydrogen atoms start to combine to form a hydrogen molecule.

The two hydrogen atoms approach each other to form a bond.

Repulsive force is predominant between the two atoms:

The internuclear distance between the two hydrogen atoms is less than the bond length.

The potential energy of the system is positive.

Attractive and repulsive forces balance each other:

The two hydrogen atoms form a stable hydrogen molecule.

The potential energy of the system is at minimum.

There is no interaction between the two atoms:

The two hydrogen atoms are very far apart.

Bond length is the distance between the centers of two bonded atoms. On the potential energy curve, the bond length is the internuclear distance between the two atoms when the potential energy of the system reaches its lowest value.

Given that the atomic radii of H and Br are 25.0 pm and 115 pm , respectively, predict the bond length of the HBr molecule.

25+115= 140pm

Sulfur tetrafluoride, SF4, reacts slowly with oxygen, O2, to form sulfur tetrafluoride monoxide, OSF4, according to the following unbalanced reaction: SF4(g)+O2(g)→OSF4(g)

When the equation is balanced, what are the coefficients?

2 SF4(g)+ O2(g)→ 2 OSF4(g)