1. Which of the following statements about protons is FALSE?  A. Protons have an elementary positive charge of 1. B. Protons have one Dalton of mass. C. Protons are always found in the nucleus of the atom. D. Any atom found in nature always has the same number of protons as electrons. 2. Which of the following statements about electron orbitals is FALSE?  A. They correlate with the number of protons in the nucleus. B. They do not contain more than two electrons. C. Each orbital contains electrons of the same energy. D. They are paths around the nucleus in which the electrons orbit.

Periodic Table of the Elements 2 2

Draw electron configurations and write out electron configurations of the following elements: Oxygen (O) Magnesium (Mg) Carbon (C) Nitrogen (N) Chlorine (Cl) Neon (Ne) Marcey’s example: e.g. Phosphorus (P)

A. Compare and contrast covalent and ionic bonds B. Why do salts (NaCl, say) easily dissolve in water? C. Discuss: identify as many properties of water (H2O) as possible D. Why does pure water have a pH = 7? E. Explain how buffers can stabilize the pH of a solution?

Hydrogen Bonding of water (liquid, solid) hydrogen bonds hydrogen bonds

Why does water have a high boiling point?

Why does water have a high boiling point?

Why does water have high surface tension / cohesion?

Why does water have high surface tension / cohesion?

3) What is the difference between covalent bonds and ionic bonds? A) Covalent bonds are formed between atoms to form molecules; ionic bonds are formed between atoms to form compounds. B) Covalent bonds involve the sharing of pairs of electrons between atoms; ionic bonds involve the sharing of single electrons between atoms. C) Covalent bonds involve the sharing of electrons between atoms; ionic bonds involve the electrical attraction between atoms. D) Covalent bonds involve the sharing of electrons between atoms; ionic bonds involve the sharing of protons between atoms. E) Covalent bonds involve the transfer of electrons between atoms; ionic bonds involve the sharing of electrons between atoms.   4) Which bond or interaction between atoms would be most difficult to disrupt when the interacting atoms are put into water and heated slightly? A) covalent bond B) hydrogen bond C) van der Waals interaction D) ionic bond E) either hydrogen bonds or ionic bonds

  5) Consider two solutions: solution X has a pH of 4; solution Y has a pH of 7. From this information, we can reasonably conclude that A) solution Y has no free hydrogen ions (H+). B) the concentration of hydrogen ions in solution X is 30 times as great as the concentration of hydrogen ions in solution Y. C) the concentration of hydrogen ions in solution Y is 1,000 times as great as the concentration of hydrogen ions in solution X. D) the concentration of hydrogen ions in solution X is 3 times as great as the concentration of hydrogen ions in solution Y. E) the concentration of hydrogen ions in solution X is 1,000 times as great as the concentration of hydrogen ions in solution Y.

6) Which of the structures illustrated above is an impossible covalently bonded molecule? A) A B) B C) C D) D E) E   7) In which of the structures illustrated above are the atoms bonded by ionic bonds? D) C, D, and E only E) none of the structures 8) Which of the structures illustrated above cannot form hydrogen bonds with water molecules? 9) Relatively small organic molecules with a central carbon atom which is bonded to a carboxyl group, an amino group, a carbon containing group, and a hydrogen atom are called  A. amino acids. B. fatty acids. C. enzymes. D. peptides. E. nucleotides.