1. Honors Chapter 6
Assessment answers

2. Section 1

3. What is the smallest unit of matter?
Atom
2. How are atoms and elements related?
The same type of atoms make up an element

4. 3. List the similarities and differences among protons, electrons, and neutrons. All of these are similar because they make up an atom. Protons, neutrons in nucleus Electrons in outer shell Protons positive Electrons negative Neutrons neutral

5. 4. How does the location of the electrons in an atom allow them to be involved in bonding? Electrons in the outer shell will be nearer to the outer shells of other atoms and allow them to bond covalently.

6. Look in the textbook on p. 149 Figure 6. 3
Look in the textbook on p. 149 Figure What is the most abundant element that exists in living things?
Hydrogen
6. How does the atom of an isotope differ from the atom of the same element? How are they the same?
Differ in the number of neutrons
Similar because they have the same number of electrons & protons

7. 7. What type of medical test makes use of radioisotopes. P
7. What type of medical test makes use of radioisotopes? P. 150 in textbook Radiation therapy, x-rays 8. Why is CO, carbon monoxide not an element? It is a compound of carbon and oxygen; 2 different elements

8. 9. Are all compounds molecules. No Why or why not
9. Are all compounds molecules? No Why or why not? Only compounds formed by covalent bonding are molecules

9. 10. Compare van der Waals forces, ionic bonds, and covalent bonds.
Van der Waals hold molecules together
Ionic and covalent bonds hold atoms together
Covalent bonds – electrons are shared between atoms
Ionic bonds – electrical attractions between two oppositely charged atoms

10. 11. How does the atom of an isotope differ from the atom of the same element? Number of neutrons
12. What factor determines that an oxygen atom can form two covalent bonds while a carbon atom can form four?
The number of electrons in the outer shell
Carbon has 4
Oxygen has 6

11. Honors 6.2 assessment
What is the relationship between a chemical bond and a chemical reaction?
Chemical bonds are create or broken by chemical reactions

12. 2. Why must chemical equations be balanced
2. Why must chemical equations be balanced? Because the law of conservation of mass states that matter cannot be created or destroyed; matter can only change forms

13. 3. Practice balancing equations
3. Practice balancing equations. 6K + B2O3 -> 3K2O + 2B HCl + NaOH -> NaCl + H20 4. What are enzymes? Special proteins that act as a catalyst to speed up the rate of a biological reaction.

14. 5. What effect does an enzyme have on a chemical reaction?
It lowers the activation energy of the reaction so the rate of the reaction speeds up
6. Identify the parts of this chemical reaction:
A + B  AB
Reactants Products

15. Because of conservation of mass
7. Why do the number of atoms of reactants have to equal the number of atoms of products formed?
Because of conservation of mass

16. 8. Compare and contrast the substrate and active site.
Both are part of enzyme substrate complex
active site – specific place where a substrate binds on an enzyme
substrate – reactant of an enzyme-catalyzed reaction

17. 9. Identify and describe factors that can influence enzyme activity.
Temperature, pH, and other substances

18. 6.3 assessment
Distinguish between solutions and suspensions. Give an example of each.
Solutions are mixtures that has substances evenly mixed throughout (homogeneous). Example: salt water.
Suspensions are heterogenous mixtures that separate over time. Example: sand and water.

19. 2. Relate the structure of water to its ability to act as a solvent
2. Relate the structure of water to its ability to act as a solvent. Water is a polar molecule meaning it has unequal charges. Positive charges are attracted to negative charges on other water molecules and other solutes.

20. 3. Baking soda is a basic substance
3. Baking soda is a basic substance. Describe the effect of baking soda on the H+ ion concentration of stomach contents with pH 4. The baking soda will buffer the H+ ions because it has more OH- ions. Therefore, the substance will be less acidic and the pH will rise.

21. 4. If you add hydrochloric acid to water, what effect would this have on the H+ ion concentration? On the pH? Increase the H+ ions but decrease the pH number

22. 5. What is the relationship between a
5. What is the relationship between a. solution----mixture A solution is a type of mixture b. pH-----buffer Buffer is a substance that is added to a solution to adjust H+ so that pH is changed be more acidic or basic

23. c. acid---base Acids and bases can both be measured by concentration of H+ through pH scale. The more H+ there are, the more acidic the solution. The less H+, the more basic the solution.

24. d. solvent---solute
A solute is dissolved by a solvent.
e. polar molecule---hydrogen bond
A polar molecule is able to form hydrogen bonds because of the unequal charges around the molecule.

25. 6. Hydrochloric acid (HCl) is a strong acid
6. Hydrochloric acid (HCl) is a strong acid. What ions are formed when HCl dissolves in water? H+ and Cl- What effect of HCl on the pH of water? It would decrease the pH, because of the increase in H+ ion concentration

26. 7. Compare and contrast adhesion and cohesion.
Water is cohesive and adhesive
Cohesive means the water molecules stick to each other
Adhesive means the water molecules stick to other substances

27. 8. Why is water considered the universal solvent
8. Why is water considered the universal solvent? Because it will mix with more substances than any other solvent

28. 9. Give an example of a homogenous and heterogenous mixture
9. Give an example of a homogenous and heterogenous mixture. Homogenous – food coloring and water Heterogenous – fruit salad

29. 6.4
What is the name of the element that is found in all living things?
carbon
How many bonds can this element’s atom form with other atoms?
four

30. What kind of bond does it form?
covalent
4. What is the name of the type of chemistry that studies only this element?
organic
What is a macromolecule?
A giant molecule made of hundreds or thousands of smaller molecules

31. 6. What are some other names that are used in place of macromolecules?
Polymers, organic molecules
What is a monomer?
small molecules that can join with other small molecules to make larger molecules ( macromolecules)

32. What is polymerization?
process of making macromolecules/polymers by joining smaller compounds together
9. What are the four major categories of macromolecules?
carbohydrates, lipids, proteins, and nucleic acids.

33. What monomer makes up the macromolecule carbohydrate?
monosaccharide
What elements make up a carbohydrate?
Carbon, hydrogen, oxygen

34. 12. What is it called when you have 2 monosaccharides together
12. What is it called when you have 2 monosaccharides together? dissacharide What about 100? Polysaccharide

35. 13. One of the functions of a carbohydrate is to store energy
13. One of the functions of a carbohydrate is to store energy. What are the two types of polysaccharides discussed that store energy?
Starches and glycogen
Which types of polysaccharides provide structural support to organisms?
Cellulose and chitin

36. 15. What is the formula for a carbohydrate?
—(CH2O)n
16. Give some examples of lipids.
Fats, oil, & waxes
What is the monomer for a lipid.
Fatty acid and glycerol

37. Lipids are nonpolar. What does that mean?
That this molecule has equal charges around it therefore; lipids do not mix well with other substances
What is a phospholipid and where can it be found?
A lipid joined to a lipid molecule; found in the cell membrane; doesn’t mix well with water so it makes a good barrier for the cell

38. What are the elements found in lipids?
Carbon and hydrogen
21. What is a saturated fat?
lipids that have tail chains made up of only single bonds between the carbon atoms.

39. What is an unsaturated fat?
Lipids that have tail chains with at least one double bond between the carbon atoms.
23. What is a polyunsaturated fat?
A lipid with more than one double bond between the carbon bonds

40. What are the monomers for the macromolecule protein?
Amino acids
25. What are the elements found in proteins?
Carbon, hydrogen, oxygen, sulfur and nitrogen

41. 26. What are the components of an amino acid? There are 5.
Central carbon, hydrogen, carboxyl group COOH, variable group, and an amino group NH3
How many different amino acids are there? 20

42. Why do proteins have so many more functions than any of the other macromolecules?
Diversity of amino acids
4 levels of organization