Explain the following statement: The smallest particles unique to a compound cannot be atoms.

What would you get if you could break an element into its smallest particle?

What class of elements lies along the "staircase" line in the periodic table? How do their properties compare with those of metals and nonmetals?

How can you use probability to make decisions$?$

Chlorine has two naturally occurring isotopes, 35C1 and 37C1. What is the mass number of each isotope? How many protons, neutrons, and electrons are present in each?

Explain the difference between a molecular element and a molecular compound.

Scene A-I depicts various types of matter on the atomic scale. Choose the correct scene(s) for each of the following:
(d) A homogeneous mixture

Scene A-I depicts various types of matter on the atomic scale. Choose the correct scene(s) for each of the following:
(b) A substance that cannot be broken down into simpler ones

The tap water found in many areas of the United States leaves white deposits when it evaporates. Is this tap water a mixture or a compound? Explain.

Evaluate the limit of the following sequences or state that the limit does not exist.

$$a _ { n } = \cos \left( 0.99 ^ { n } \right) + \frac { 7 ^ { n } + 9 ^ { n } } { 63 ^ { n } }$$

Molecular scenes A and B depict changes in matter at the atomic scale:

Which result(s) in different chemical properties?

Can the relative amounts of the components of a mixture vary? Can the relative amounts of the components of a compound vary? Explain.

Describe why it is important to take measurements that are both accurate and precise:

Choose the correct answer. The difference between the mass number of an isotope and its atomic number is (a) directly related to the identity of the element: (b) the number of electrons: (c) the number of neutrons; (d) the number of isotopes.