First Semester Exam Review

Pre-AP Chemistry, Chapters 1-10

Charles Page High School, Stephen L. Cotton

 

 

Name__________________________________Class______

 

From Chapter 1:

1.       A characteristic of a scientific theory is that it can never ____.

2.       When can a hypothesis become a theory?

3.       What area of chemistry focuses on the composition of matter, such as measuring the level of lead in drinking water?

4.       What area of chemistry studies chemicals that generally do NOT contain carbon?

5.       Which step in the scientific method requires you to use your senses to obtain information?

 

From Chapter 2:

1.      A substance that forms a vapor is generally in what physical state at room temperature?

2.      Which state of matter has a definite volume and takes the shape of its container?

3.      What must occur for a change to be called a chemical reaction?

4.      Which state of matter takes both the shape and volume of its container?

5.      An example of an extensive property of matter is _____.

 

From Chapter 3:

1.      Be able to calculate the density of an object, when you are given the mass and volume.

2.      Be able to express numbers in scientific notation.

3.      What is the boiling point of water, in Kelvin?

4.      Be able to round off numbers to the proper number of significant figures.

5.      Be able to perform calculations (such as multiply, divide, add, subtract), and express the answer to the proper number of significant figures.

 

From Chapter 4:

  1. Know the parts of Dalton’s atomic theory.
  2. An element has an atomic number of 76.  The number of protons and electrons in a neutral atom of the element are _____.
  3. Isotopes of the same element have different _____.
  4. Using the periodic table, determine the number of neutrons in 16O.
  5. The mass number of an element is equal to _____.

 

From Chapter 5:

1.          In Bohr’s model of the atom, where are the electrons and protons located?

2.          What is the basis for exceptions to the aufbau diagram?

3.          How many unpaired electrons are in a sulfur atom (atomic number 16)?

4.          Be able to do the electron configuration for a given atom.

5.          According to the aufbau principle, an orbital may be occupied by how many electrons?

 

From Chapter 6:

  1. Be able to identify representative elements and transition elements.
  2. How do the metals in Groups 1A, 2A, and 3A form ions?
  3. The modern periodic table is arranged in order of increasing atomic _____.
  4. What is the charge of a cation?
  5. Who arranged the elements according to atomic mass, and used the arrangement to predict the properties of missing elements?

 

From Chapter 7:

1.        How many electrons does nitrogen gain in order to achieve a noble-gas electron configuration?

2.        Ionic compounds are normally in which physical state at room temperature?

3.        What particles are free to drift in metals?

4.        What is the name given to the electrons in the highest occupied energy level of an atom?

5.        Under what conditions can potassium bromide (KBr) conduct electricity?

 

From Chapter 8:

  1. When one atom contributes both bonding electrons in a single covalent bond, the bond is called a(n) _____.
  2. Once formed, how are coordinate covelent bonds different from other covelent bonds?
  3. How do atoms achieve noble-gas electron configurations in single covalent bonds?
  4. A bond formed between a silicon atom and an oxygen atom is likely to be _____.
  5. What causes water to have a “bent” shape, according to VSEPR theory?

 

From Chapter 9:

  1. Binary molecular compounds are made of two _____.
  2. What is the correct name for Sn3(PO4)2?  Be able to name other ionic compounds.
  3. What is the name of H2SO3?  Be able to name other acids.
  4. What is the name of N2O5?  Be able to name other molecular compounds.
  5. What is the correct formula for barium chlorate?  Be able to write formulas for other compounds, both ionic and molecular.

 

From Chapter 10:

  1. Be able to calculate the empirical formula, when given the percentage of each element by weight.
  2. The molar volume of a gas at STP occupies _____.
  3. What is the molar mass of AuCl3?  Be able to calculate the molar mass of other compounds.
  4. Be able to do conversion problems between moles and liters of a gas at STP.  Example: What is the number of moles in 500 L of He gas at STP?
  5. Be able to do conversion problems between atoms and moles.  Example:  How many moles of tungsten atoms are in 4.8 x 1025 atoms of tungsten?