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BSC2010 Exam 1 Study Guide:
Steven Marks | Chapters 2-5
Review
Prepare for BSC2010 Exam 1 with Steven Marks using
this focused study guide covering Chapters 2-5. Topics
include chemical context of life, water properties, carbon
diversity, and biological macromolecules. Covers atoms,
bonds, pH, functional groups, proteins, carbohydrates,
lipids, and nucleic acids. Based on lecture materials and
Mastering Biology resources. Includes key concepts,
terminology, and review questions for exam preparation.
Question 1
Which subatomic particle determines an atom's bonding behavior?
A) Protons
B) Neutrons
C) Electrons
D) Isotopes
Rationale: Valence electrons in the outermost shell determine how an atom bonds with
other atoms.
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Question 2
A sodium atom forms a cation because it:
A) Gains one electron
B) Loses one electron
C) Gains one proton
D) Loses one neutron
Rationale: Sodium loses one electron to achieve a stable electron configuration,
forming a positive ion.
Question 3
Isotopes of the same element differ in the number of:
A) Protons
B) Neutrons
C) Electrons
D) Bonds
Rationale: Isotopes have different neutron numbers, affecting mass but not chemical
behavior.
Question 4
Which of the following is a trace element essential for biological function?
A) Carbon
B) Iron
C) Oxygen
D) Hydrogen
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Rationale: Iron is a trace element required in small amounts, while C, H, O, and N are
major elements.
Question 5
A covalent bond is likely to be polar under which condition?
A) The two atoms are identical
B) One atom is more electronegative than the other
C) Both atoms have equal electronegativity
D) The bond involves a metal and nonmetal
Rationale: Unequal electron sharing due to electronegativity differences creates
polarity.
Question 6
What type of bond forms when electrons are transferred from one atom to another?
A) Covalent bond
B) Ionic bond
C) Hydrogen bond
D) Van der Waals interaction
Rationale: Ionic bonds result from electron transfer, creating oppositely charged ions.
Question 7
Which of the following is the weakest type of bond or interaction?
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A) Covalent bond
B) Ionic bond
C) Hydrogen bond
D) Peptide bond
Rationale: Hydrogen bonds are individually weak but collectively important in
biological systems.
Question 8
The valence of an atom is determined by:
A) The number of protons
B) The number of unpaired electrons in the valence shell
C) The atomic mass
D) The number of neutrons
Rationale: Valence is the bonding capacity determined by unpaired electrons in the
outermost shell.
Question 9
What does it mean when a chemical reaction is at equilibrium?
A) The reaction has stopped completely
B) The forward and reverse reactions occur at the same rate
C) All reactants have been converted to products
D) The reaction is irreversible
Rationale: At equilibrium, forward and reverse reactions proceed at equal rates, so
concentrations remain constant.
BSC2010 Exam 1 Study Guide:
Steven Marks | Chapters 2-5
Review
Prepare for BSC2010 Exam 1 with Steven Marks using
this focused study guide covering Chapters 2-5. Topics
include chemical context of life, water properties, carbon
diversity, and biological macromolecules. Covers atoms,
bonds, pH, functional groups, proteins, carbohydrates,
lipids, and nucleic acids. Based on lecture materials and
Mastering Biology resources. Includes key concepts,
terminology, and review questions for exam preparation.
Question 1
Which subatomic particle determines an atom's bonding behavior?
A) Protons
B) Neutrons
C) Electrons
D) Isotopes
Rationale: Valence electrons in the outermost shell determine how an atom bonds with
other atoms.
,2|Page
Question 2
A sodium atom forms a cation because it:
A) Gains one electron
B) Loses one electron
C) Gains one proton
D) Loses one neutron
Rationale: Sodium loses one electron to achieve a stable electron configuration,
forming a positive ion.
Question 3
Isotopes of the same element differ in the number of:
A) Protons
B) Neutrons
C) Electrons
D) Bonds
Rationale: Isotopes have different neutron numbers, affecting mass but not chemical
behavior.
Question 4
Which of the following is a trace element essential for biological function?
A) Carbon
B) Iron
C) Oxygen
D) Hydrogen
,3|Page
Rationale: Iron is a trace element required in small amounts, while C, H, O, and N are
major elements.
Question 5
A covalent bond is likely to be polar under which condition?
A) The two atoms are identical
B) One atom is more electronegative than the other
C) Both atoms have equal electronegativity
D) The bond involves a metal and nonmetal
Rationale: Unequal electron sharing due to electronegativity differences creates
polarity.
Question 6
What type of bond forms when electrons are transferred from one atom to another?
A) Covalent bond
B) Ionic bond
C) Hydrogen bond
D) Van der Waals interaction
Rationale: Ionic bonds result from electron transfer, creating oppositely charged ions.
Question 7
Which of the following is the weakest type of bond or interaction?
, 4|Page
A) Covalent bond
B) Ionic bond
C) Hydrogen bond
D) Peptide bond
Rationale: Hydrogen bonds are individually weak but collectively important in
biological systems.
Question 8
The valence of an atom is determined by:
A) The number of protons
B) The number of unpaired electrons in the valence shell
C) The atomic mass
D) The number of neutrons
Rationale: Valence is the bonding capacity determined by unpaired electrons in the
outermost shell.
Question 9
What does it mean when a chemical reaction is at equilibrium?
A) The reaction has stopped completely
B) The forward and reverse reactions occur at the same rate
C) All reactants have been converted to products
D) The reaction is irreversible
Rationale: At equilibrium, forward and reverse reactions proceed at equal rates, so
concentrations remain constant.
