Test 1 Key - WEB . WHRSD . ORG

Name: ________________________ Class: ___________________ Date: __________
MCC Bio Principles Test 1 Fall 2014
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. The three particles that make up atoms are
a. protons, neutrons, and isotopes.
b. neutrons, isotopes, and electrons.
c.
d.
positives, negatives, and electrons.
protons, neutrons, and electrons.
____
2. Isotopes are atoms of the same element with the same number of protons and
a. a different number of electrons.
c. a different number of neutrons.
b. a different number of molecules.
d. the same number of neutrons.
____
3. Which of the following makes up a molecule of water?
a. one atom of hydrogen and one atom of oxygen
b. one atom of sodium and one atom of chlorine
c. one atom of hydrogen and two atoms of oxygen
d. two atoms of hydrogen and one atom of oxygen
____
4. A covalent bond is formed as the result of
a. transferring electrons.
b. sharing an electron pair.
c.
d.
transferring protons.
sharing a proton pair.
____
5. What type of ion forms when an atom loses electrons?
a. neutral
c. negative
b. positive
d. possibly positive or negative
____
6. Water molecules are polar, with the
a. oxygen side being slightly positive and the hydrogen side being slightly negative.
b. oxygen and hydrogen sides being slightly positive.
c. oxygen and hydrogen sides being slightly negative.
d. oxygen side being slightly negative and the hydrogen side being slightly positive.
____
7. A monosaccharide is a
a. carbohydrate.
b. lipid.
____
c.
d.
nucleic acid.
protein.
8. Over 96% of all living matter is made of six elements—oxygen, carbon, sulfur,
a. iron, nitrogen, and platinum.
b. hydrogen, nitrogen, and phosphorus.
c. nitrogen, iron, and potassium.
d. sodium, nitrogen, and hydrogen.
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ID: A
Name: ________________________
ID: A
Figure 01.01
____
9. The black dots in the Figure 01.01 diagram represent
a. atoms.
c. electrons.
b. molecules.
d. chemical bonds.
____ 10. If there were eight neutrons in the nucleus of the Figure 01.01 diagram, how would it be related to
the original?
a. It would be a molecule.
b. Its charge would increase.
c.
d.
It would be an isotopic form.
Its charge would decrease.
____ 11. If one of the black dots in the Figure 01.01 diagram was lost during a reaction, the charge of the atom
would
a. remain the same.
b. be positive.
c.
d.
be negative.
be neutral.
____ 12. An ionic bond is formed as the result of
a. the actual sharing of electrons.
b. a release of energy.
c.
d.
the transfer of electrons.
a combination of fats and proteins.
____ 13. The building blocks for carbohydrates are
a. simple sugars.
b. glycerol and fatty acids.
c.
d.
metabolism.
nucleotides.
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Name: ________________________
ID: A
____ 14. Which of the diagrams below is the Bohr model for magnesium (Mg), atomic number of 12?
a.
b.
c.
d.
e.
A
B
C
D
E
____ 15. The slight negative charge at one end of one water molecule is attracted to the slight positive charge of
another water molecule. What is this attraction called?
a. a covalent bond
b. a hydrogen bond
c. an ionic bond
d. a hydrophilic bond
e. a hydrophobic bond
____ 16. What do cohesion, surface tension, and adhesion have in common with reference to water?
a. All increase when temperature increases.
b. All are produced by ionic bonding.
c. All are properties related to hydrogen bonding.
d. All have to do with nonpolar covalent bonds.
e. C and D only
____ 17. At what temperature is water at its densest?
a. 0°C
b. 4°C
c. 32°C
d. 100°C
e. 212°C
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Name: ________________________
ID: A
The picture below illustrates a solute molecule surrounded by a hydration shell of water. Use it to answer the
following question.
____ 18. Based on your knowledge of the polarity of water molecules, the solute molecule is most likely
a. positively charged.
b. negatively charged.
c. without charge.
d. hydrophobic.
e. nonpolar.
____ 19. Hydrophobic substances such as vegetable oil are
a. nonpolar substances that repel water molecules.
b. nonpolar substances that have an attraction for water molecules.
c. polar substances that repel water molecules.
d. polar substances that have an affinity for water.
e. charged molecules that hydrogen-bond with water molecules.
____ 20. Which two functional groups are always found in amino acids?
a. ketone and aldehyde
b. carbonyl and carboxyl
c. carboxyl and amino
d. phosphate and sulfhydryl
e. hydroxyl and aldehyde
____ 21. Amino acids are acids because they always possess which functional group?
a. amino
b. carbonyl
c. carboxyl
d. sulfhydryl
e. aldehyde
____ 22. The electrons of an atom
a. are found in the nucleus along with the protons.
b. occupy the space surrounding the nucleus.
c. have a positive charge.
d. are attached to the positive charge of neutrons.
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Name: ________________________
ID: A
____ 23. A substance that is composed of only one type of atom is called a(n)
a. nucleus.
c. element.
b. cell.
d. molecule.
____ 24. A molecule that has a partial positive charge on one side and a partial negative charge on the other side is
called a
a. nonpolar molecule.
c. charged molecule.
b. polar molecule.
d. bipolar molecule.
____ 25. A chemical formula shows the
a. kinds of bonds found in the molecule.
b. kinds of bonds found in the compound.
c. kinds of elements found in the compound.
d. arrangement of the elements found in the compound.
____ 26. Ionic bonds form between molecules that have
a. opposite charges.
c.
b. the same charge.
d.
no charges.
neutral charges.
____ 27. The bond formed when two atoms share a pair of electrons is called a(n)
a. hydrogen bond.
c. covalent bond.
b. ionic bond.
d. water bond.
____ 28. When placed in the same container, oil and water do not mix because
a. they are both polar.
c. they are both nonpolar.
b. water is polar and oil is nonpolar.
d. water is nonpolar and oil is polar.
____ 29. The atomic number refers to the
a. mass of an atom.
b. number of protons in an atom.
c. number of both protons and neutrons in an atom.
d. number of neutrons in an atom.
e. number of electrons in an atom.
____ 30. Radioactive isotopes
a. are electrically unbalanced.
b. behave the same chemically and physically but differ biologically from other isotopes.
c. are the same physically and biologically but differ from other isotopes chemically.
d. have an excess number of neutrons.
e. are produced when atoms lose electrons.
____ 31. All atoms of an element have the same number of
a. ions.
b. protons.
c. neutrons.
d. electrons.
e. protons and neutrons.
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Name: ________________________
ID: A
____ 32. Magnesium has 12 protons. How many electrons are in its third energy level?
a. 2
b. 4
c. 6
d. 8
e. 10
____ 33. Magnesium has 12 protons. How many electrons are in its first energy level?
a. 2
b. 4
c. 6
d. 8
e. 10
____ 34. Nitrogen has an atomic number of 7. How many hydrogen atoms are necessary to join with the nitrogen to
form a stable compound?
a. 1
b. 2
c. 3
d. 4
e. 5
____ 35. An atom that gains or loses electrons becomes
a. more stable.
b. an ion.
c. a molecule.
d. unable to form bonds.
e. radioactive.
____ 36. A single carbon atom may form as many as ____ covalent bonds with other atoms.
a. 2
b. 3
c. 4
d. 5
e. 6
____ 37. The atom present in all organic compounds is
a. carbon.
b. oxygen.
c. nitrogen.
d. sulfur.
e. hydrogen.
____ 38. An --OH group is a(n) ____ group.
a. carboxyl
b. hydroxyl
c. amino
d. methyl
e. carbonyl
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Name: ________________________
ID: A
____ 39. An --NH2 group is a(n) ____ group.
a. carboxyl
b. hydroxyl
c. amino
d. methyl
e. carbonyl
____ 40. A --COOH group is a(n) ____ group.
a. carboxyl
b. hydroxyl
c. amino
d. methyl
e. carbonyl
____ 41. Scientific hypotheses must be proposed in a way that
a. ensures that an experiment will be valid.
b. enables them to be proved valid.
c. enables them to be tested.
d. doesn’t contradict previous hypotheses.
____ 42. The basic unit of mass in the International System of Units, or SI, is the
a. meter.
c. liter.
b. ounce.
d. gram.
Short Answer
43. Why are atoms considered neutral?
44. What are the main types of chemical bonds?
45. What accounts for water’s properties of adhesion and cohesion?
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Name: ________________________
ID: A
Other
USING SCIENCE SKILLS
Element
Symbol
Protons
Neutrons
Hydrogen
H
1
Helium
He
2
Carbon
C
6
Oxygen
O
8
Neon
Ne
Aluminum
Al
Zinc
Zn
Electrons
Atomic
Number
1
Mass
Number
4
6
8
10
10
13
20
27
30
30
65
Figure 2–1
46. Calculating Based on Figure 2–1, what is the mass number of carbon?
47. Applying Concepts Based on Figure 2–1, what is the atomic number of oxygen?
48. Applying Concepts Using Figure 2–1, how many electrons does an atom of aluminum contain?
49. Applying Concepts According to Figure 2–1, an atom of which element contains two neutrons?
50. Applying Concepts Based on Figure 2–1, which element has a mass number of 16?
USING SCIENCE SKILLS
pH Values of Some Common Substances
Substance
pH
Hydrochloric acid
1.0
Sulfuric acid
1.2
Tomatoes
4.2
Rainwater
6.2
Pure water
7.0
Sea water
8.5
Ammonium chloride
11.1
Sodium hydroxide
13.0
Figure 2–2
51. Applying Concepts What is the strongest acid listed in Figure 2-2?
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