Chapter 3, Problem 3.6E

A fundamental idea of Daltons atomic theory is that atoms of an element can be neither created nor destroyed. We now know that this is not always true. Specifically, it is not true for uranium and lead atoms as they appear in nature. Are the numbers of these atoms increasing or decreasing? Explain.

Certain elements have special affinities for other elements. This causes them to bind together in special ways to form .

Boron (BB)  has two naturally occurring isotopes: BB-10, which has a percent abundance of 19.88 %% and a mass of 10.013 amuamu , and BB-11, which has a 80.12 %% abundance and a mass of 11.009 amuamu . Calculate the atomic mass for boron using the weighted-average mass method.

Nitrogen (N), has two naturally occurring isotopes: N-14 that has a percent abundance of 99.63 % and a mass of 14.00 amu, and NN-15 that has a percent abundance of 0.37 % and a mass of 15.00 amu Calculate the atomic mass for nitrogen using the weighted average mass method.

how would you describe the elements from group 1 to group 12 in the periodic table

List and explain Dalton's atomic theory (postulates). Explain which postulates were rejected and state why

Consider the following information about three atoms: (a) How are they similar to one another? (b) How do they differ from one another? (c) What are the members of such a group of atoms called? (d) Using the planetary model, draw the atomic configuration of 126C showing the relative position and numbers of its subatomic particles.