Question

1)         Define the following: matter, element, atom, trace element, proton, electron, neutron, atomic number, mass number, isotopes, radioisotope, molecule, compound, salt, ion.

2)         List the 6 elements that make up about 99% of the weight of an organism.

3)         What are the functions of the trace elements iron, fluorine (fluoride), and iodine?

4)         An iodine deficiency can result in goiter. True/False

5)         Where are protons, neutrons and electrons located?

6)         Can you determine the atomic number and mass number from the number of protons, neutrons and electrons in an atom?

7)         Protons and neutrons are about the same mass. True/False

8)         Can you determine the number of protons, neutrons and electrons from the atomic number and the mass number of an atom?

9)         Can you sketch an atom (indicating the number of shells and the electrons on each shell) from the atomic number of that atom?

10)       What are the differences/similarities between ¹²C, ¹³C, and ¹⁴C?

11) Discuss the advantages of radioisotopes?

12) Discuss the disadvantages of radioisotopes?

13)       Discuss the arrangement of electrons on shells. (Make sure you include the number of electrons that each shell can hold, as well as the energy levels of electrons).

14)       If the atomic number of an atom were given, can you determine the number of electrons that atom will require in order for it to be stable?

15)       What is an orbital? An orbital can hold no more than ______ electrons.

16)      What is the valence shell? The innermost shell can hold no more than _____ electrons while the second and third shells can hold up to _____ electrons.

17)       Discuss the difference between covalent bonds, ionic bonds, and hydrogen bonds.

18)       What is the difference between a single covalent bond and a double covalent bond?

19)       What is electronegativity?

20)       Discuss the difference between polar and nonpolar covalent bonds and give some examples.

21)       Give some examples of molecules with polar and non-polar bonds.

22)       In a water molecule, which atom has a higher electronegativity and which atom has a lower electronegativity?   Which atom has a partial positive charge and which one has a partial positive charge?

23)       Covalent bonds are very strong bonds. True/False

24)       In an ionic bond in which Na⁺ and Cl^- are involved, can you determine which atom has lost or gained electrons and how many electrons have been lost or gained?

25)       Individual hydrogen bonds are weaker than covalent bonds. True/False

26)       In chemical reactions atoms are rearranged to form products. True/False

27)       Chemical reactions always destroy matter. True/False

28)       What are reactants and products?

29)       What type of bond holds the atoms of each water molecule? What type of bond holds separate water molecules together?

30)      Make sure you understand all the special properties of water discussed in class (include examples).

31)       Define the following: cohesion, surface tension, adhesion, thermal energy, evaporative cooling, solution, solute, solvent, aqueous solution, hydrophilic, hydrophobic.

32)       Hydrophilic substances are polar or ionic, while hydrophobic substances are non-polar or nonionic. True/False

33)       Water forms hydrogen bonds with hydrophobic substances but not hydrophilic substances. True/False

34)       How are acids, bases defined? Give some examples

35)       What is the pH of a solution?

36)       Why is the pH of water neutral?

37)       A solution with a pH of 9 is acidic. True/false

38)       What is a buffer? Discuss the importance of buffers.

39)       A solution of pH 5 is how many times more/less acidic than a solution of pH 3?

40)       The lower the pH, the _________ (lower/higher) the concentration of H⁺.

41)       Human blood has a pH of _________________.

42)       What is ocean acidification?

43)       How does ocean acidification affect shell-building organisms?

Answer 1