Ready to test your knowledge with our biology chapter 2 self quiz? Whether you're reviewing ap biology chapter 2 topics or prepping for exams, this chapter 2 biology quiz explores the ins and outs of molecules and reactions. Our biology atomic structure quiz section helps you master electron configuration and bonding, while the basic biological elements quiz segment tests your grasp of life's building blocks. From understanding atomic numbers to identifying essential elements, you'll build a solid chemistry foundation tailored to biology. Perfect for high school and college students, this self quiz offers dynamic questions, instant feedback, and clear explanations. Jump in now - challenge yourself with our biology chapter 2 self quiz life's chemical basis or expand your review with a biology part 2 quiz !
What subatomic particle has a positive charge and is found in the nucleus of an atom?
Photon
Proton
Neutron
Electron
Protons carry a positive electrical charge and reside in the atomic nucleus alongside neutrons. Their number defines the element's atomic number and identity. Electrons are negative and orbit the nucleus, while neutrons are neutral. Learn more about atomic structure.
Which element is the most abundant by mass in the human body?
Carbon
Oxygen
Hydrogen
Nitrogen
Oxygen makes up about 65% of the human body's mass, largely due to water (H?O) being the most abundant compound. It is essential for cellular respiration and energy production. Carbon and hydrogen are also abundant but not to the extent of oxygen. Human body composition.
What is the atomic number of an element?
Total number of neutrons
Sum of protons and neutrons
Sum of protons and electrons
Total number of protons
An element's atomic number equals the number of protons in its nucleus, which also determines its chemical identity. Neutrons can vary in isotopes, but protons are fixed. The sum of protons and neutrons gives the mass number. Atomic number explained.
Which bond involves the sharing of electron pairs between atoms?
Hydrogen bond
Covalent bond
Van der Waals interaction
Ionic bond
Covalent bonds form when two atoms share one or more pairs of electrons, leading to a more stable electron configuration. They can be polar or nonpolar depending on electronegativity differences. Ionic bonds result from electrostatic attraction, not sharing. Covalent bonds overview.
What is the most electronegative element?
Fluorine
Oxygen
Nitrogen
Chlorine
Fluorine is the most electronegative element, with an electronegativity of 3.98 on the Pauling scale. It strongly attracts electrons in a chemical bond, making compounds highly polar. Oxygen and nitrogen are also very electronegative but less so. Electronegativity trends.
Which element is essential for the structure of amino acids and proteins?
Calcium
Sulfur
Phosphorus
Nitrogen
Nitrogen is a key component of amino acids, the building blocks of proteins, as it is found in the amino group (-NH?). Without nitrogen, peptide bonds and protein structure cannot form. Sulfur appears in a few amino acids but is not universal. Amino acids overview.
What does pH measure?
Solute concentration
Concentration of OH- ions
Molecular weight
Concentration of H+ ions
pH is the negative logarithm of hydrogen ion concentration, indicating acidity or basicity. Lower pH (<7) is acidic (higher H+), and higher pH (>7) is basic (lower H+). It is crucial for enzyme activity and biochemical reactions. Understanding pH.
Which ion concentration is higher in a basic solution compared to a neutral solution?
H+ ions
Cl- ions
Na+ ions
OH- ions
Basic solutions have lower hydrogen ion concentration and correspondingly higher hydroxide ion concentrations. The pH scale inversely relates H+ and OH- levels. Neutral solutions at pH 7 have equal H+ and OH- concentrations. Acids and bases explained.
An atom with 6 protons, 6 electrons, and 6 neutrons is:
Carbon-12
Carbon-14
Oxygen-16
Nitrogen-14
Carbon-12 has 6 protons and 6 neutrons, giving it a mass number of 12. Carbon-14 has 8 neutrons, and other choices have different proton numbers. The element identity is defined by proton count. Isotopes and mass numbers.
Which essential element is a major component of phospholipids and nucleic acids?
Iron
Sulfur
Magnesium
Phosphorus
Phosphorus is central to the backbone of nucleic acids (DNA/RNA) and forms the head group in phospholipid membranes. It exists in cells as phosphate (PO?³?). Sulfur is in some amino acids but not in nucleic acids. Role of phosphorus in cells.
What type of bond stabilizes the alpha-helix and beta-sheet structures of proteins?
Disulfide bond
Peptide bond
Ionic bond
Hydrogen bond
Hydrogen bonds between backbone NH and CO groups stabilize secondary structures such as alpha-helices and beta-sheets. Disulfide bonds are covalent and stabilize tertiary structure. Peptide bonds link amino acids but do not alone determine folding. Protein structure levels.
Which molecule is the universal solvent in biological systems?
Methane
Acetone
Ethanol
Water
Water's polarity and ability to form hydrogen bonds make it an excellent solvent for ionic and polar substances. It is essential for transport, reactions, and temperature regulation. Other solvents lack water's universal capacity in organisms. Water properties.
What is the term for atoms of the same element that differ in neutron number?
Isotopes
Ions
Allotropes
Isomers
Isotopes are variants of an element with the same proton count but different neutrons, affecting mass number. Ions differ by electron count, allotropes by molecular form, and isomers are same formula different structure. Understanding isotopes.
Which property of water allows insects to walk on its surface?
Cohesion
High specific heat
Low density as a solid
Adhesion
Cohesion, due to hydrogen bonding between water molecules, creates surface tension that supports lightweight insects. Adhesion is water's attraction to other substances. High specific heat and density anomalies relate to heat capacity and freezing behavior. Surface tension of water.
Which of the following elements is NOT considered a bulk element in living organisms?
Nitrogen
Phosphorus
Zinc
Calcium
Bulk elements, like C, H, O, N, P, S, Ca, and K, are required in large amounts. Zinc is a trace element needed in small quantities as a cofactor. Bulk versus trace distinction depends on biological demand. Essential minerals.
What is the mass number of an atom with 8 protons and 10 neutrons?
10
18
16
8
Mass number equals the sum of protons and neutrons: 8 + 10 = 18. However, that answer indicates 18. Checking choices, 16 is incorrect. The correct sum is 18. Atomic mass explained.
Which type of bond is formed by the complete transfer of electrons from one atom to another?
Ionic bond
Covalent bond
Hydrogen bond
Peptide bond
Ionic bonds arise when one atom donates electrons to another, generating oppositely charged ions that attract each other. Covalent bonds share electrons, while hydrogen bonds are weaker attractions. Peptide bonds link amino acids. Ionic bond details.
Which region of the periodic table contains the metalloids?
Rightmost column only
Groups 1 and 2
Lanthanide series
Between metals and nonmetals along the stair-step line
Metalloids lie along the diagonal stair-step line between metals and nonmetals in the periodic table, exhibiting intermediate properties. Groups 1 and 2 are alkali and alkaline earth metals. Lanthanides are in the f-block. Periodic table regions.
What is the main reason water has a high specific heat capacity?
Nonpolar covalent structure
Strong ionic bonds
High molecular weight
Hydrogen bonding between molecules
Hydrogen bonds between water molecules absorb significant heat energy before breaking, leading to high specific heat. This moderates temperature fluctuations in organisms and environments. Ionic bonds and molecular weight have lesser impact on specific heat. Water's specific heat.
Which isotope is commonly used in radiometric dating of organic materials?
Uranium-238
Carbon-12
Potassium-40
Carbon-14
Carbon-14, a radioactive isotope with a half-life of about 5,730 years, decays in once-living matter and is used to date organic remains up to ~50,000 years old. Carbon-12 is stable. Uranium-238 and potassium-40 date geological samples. Radiocarbon dating.
What does the term 'mole' refer to in chemistry?
One liter of a substance
6.022 × 10^23 entities
Concentration unit
Atomic mass in grams
A mole is Avogadro's number (6.022 × 10^23) of atoms, molecules, or ions, providing a bridge between atomic-scale and macroscopic measurements. It allows quantification by mass. It is not a volume or concentration measure. The mole concept.
Which element plays a central role in the hemoglobin molecule?
Magnesium
Zinc
Iron
Calcium
Iron in the heme group binds oxygen in hemoglobin, allowing oxygen transport in blood. Each heme contains one Fe²? that can reversibly bind O?. Magnesium and calcium have roles in other proteins but not hemoglobin. Hemoglobin structure.
Which property best explains why sodium chloride dissolves in water?
Hydrophobic interactions
Van der Waals forces
Hydrogen bonding with chloride ions
Ion - dipole interactions
Ion - dipole interactions occur when water's polar molecules surround and stabilize Na? and Cl? ions, dissolving the salt. Hydrogen bonds do not form with Na?. Van der Waals forces are too weak. Solution chemistry.
What type of reaction joins monomers into polymers by releasing water?
Isomerization
Redox reaction
Hydrolysis
Dehydration synthesis
Dehydration synthesis (condensation) links monomers by forming covalent bonds and releasing water. Hydrolysis is the reverse, adding water to break bonds. Redox involves electron transfer, isomerization rearranges bonds. Macromolecule formation.
Which term describes the attraction between water and cellulose in plant cell walls?
Hydrophobic exclusion
Surface tension
Adhesion
Cohesion
Adhesion refers to water's attraction to other polar surfaces like cellulose fibers in cell walls, aiding water transport. Cohesion is water-to-water attraction. Surface tension is a result of cohesion at surfaces. Adhesion basics.
Which atomic interaction is most important for stabilizing tertiary protein structure?
Hydrophobic interactions, hydrogen bonds, ionic bonds, and disulfide bridges
Van der Waals forces only
Hydrogen bonds only
Peptide bonds
Tertiary structure is stabilized by multiple interactions: hydrophobic effects bury nonpolar side chains, hydrogen and ionic bonds, van der Waals forces, and covalent disulfide bridges. Peptide bonds stabilize primary structure only. Protein folding.
What is the typical charge on a sodium ion in biological systems?
0
+2
-1
+1
Sodium loses one electron to attain a noble gas configuration, yielding a +1 charge as Na?. This ion is critical for nerve impulses and osmoregulation. A -1 charge would indicate a gained electron, which sodium does not do. Sodium ions.
Which essential element is a key component of chlorophyll in plants?
Iron
Potassium
Calcium
Magnesium
Magnesium sits at the center of the chlorophyll porphyrin ring and is vital for capturing light energy during photosynthesis. Iron is central in heme, not chlorophyll. Calcium and potassium have other roles. Chlorophyll structure.
Which type of chemical bond is strongest in aqueous solution?
Covalent bond
Van der Waals forces
Ionic bond
Hydrogen bond
Covalent bonds involve shared electron pairs and are strong even in water. Ionic bonds can be weakened or shielded by water's polarity. Hydrogen bonds and van der Waals forces are weaker. Bond strength comparison.
Which property of water allows it to moderate Earth's climate?
High density as a solid
Nonpolarity
Low heat of vaporization
High specific heat
Water's high specific heat capacity enables it to absorb or release large amounts of heat with small temperature changes, stabilizing climate. Its density anomaly helps ice formation but less influences climate moderation. Water and climate.
Which phrase best describes an amphipathic molecule?
Entirely polar
Contains both hydrophilic and hydrophobic regions
Ionic at physiological pH
Entirely nonpolar
Amphipathic molecules have both polar (hydrophilic) and nonpolar (hydrophobic) regions, enabling them to form micelles or bilayers. Phospholipids are classic examples. Entirely polar or nonpolar molecules lack this dual character. Amphipathic molecules.
Which process in cells relies directly on proton gradients across membranes?
Photosynthesis light reactions
Glycolysis
ATP synthesis via chemiosmosis
DNA replication
ATP synthase uses a proton gradient across the inner mitochondrial or thylakoid membrane to drive ATP production by chemiosmosis. Glycolysis and DNA replication do not directly use proton gradients. Light reactions create the gradient. Chemiosmosis explained.
Which phenomenon explains water climbing up a narrow tube against gravity?
Surface tension
Osmosis
Capillary action
Diffusion
Capillary action arises from adhesive forces between water and tube walls and cohesive forces among water molecules, pulling water upward. Osmosis is solvent movement across membranes. Surface tension is a result of cohesion at an interface. Capillary action.
What is the effective nuclear charge (Zeff) experienced by the valence electron in sodium (Z=11) approximated if inner electrons screen charge by about 10?
11
10
1
0
Effective nuclear charge Zeff ? Z ? S, where S is screening constant (~10 for Na). So Zeff ? 11 ? 10 = 1 for valence electron, explaining its ease of removal. Slater's rules and Zeff.
Which is the pKa value closest to the carboxyl group of an amino acid?
~12.0
~2.0
~7.4
~9.5
Most amino acids have a carboxyl group pKa around 2.0, meaning it donates a proton at low pH. The amino group pKa is ~9.5. Side chains vary, but carboxyl groups are acidic. Amino acid pKa values.
In a peptide bond, which two atoms share electrons?
Carbon and sulfur
Oxygen and hydrogen
Nitrogen and sulfur
Nitrogen and carbonyl carbon
The peptide bond forms between the amino nitrogen ( - NH) and the carbonyl carbon (C=O) of adjacent amino acids, releasing water. This amide linkage is planar and partial-double bond in character. Peptide bond chemistry.
Which thermodynamic parameter determines spontaneity of a reaction?
?T
?S only
?H only
?G (Gibbs free energy)
Gibbs free energy change ?G = ?H ? T?S determines spontaneity: negative ?G is spontaneous. Enthalpy and entropy contribute but ?G integrates both. Temperature T influences spontaneity via the entropy term. Gibbs free energy.
Which crystalline form of ice is less dense than liquid water?
Ice V
Ice I_h
Ice II
Ice III
Ice I_h is the hexagonal form of ordinary ice and is less dense than liquid water due to its open hydrogen-bonded lattice. Other high-pressure ices are denser than water. Ice polymorphism.
Which element's isotope ratio is used in heavy water for NMR spectroscopy?
¹H to ³H
¹?O to ¹?O
¹H to ²H
¹²C to ¹³C
Deuterium (²H) replaces protium (¹H) in heavy water (D?O) for NMR to avoid proton signals. The ¹H/²H ratio must be low. Tritium (³H) is radioactive. Deuterated solvents.
Which concept explains why ionic radii decrease across a period?
Decreasing number of electrons
Increase in electron - electron repulsion
Increasing effective nuclear charge
Increasing shielding effect
Across a period, nuclear charge increases without significant added shielding, pulling electrons closer and decreasing ionic radii. Electron - electron repulsion doesn't increase enough to counteract this. Periodic trends.
What is the Henderson - Hasselbalch equation used to calculate?
Reaction rate
Solubility product
pH of a buffer solution
Enzyme activity
The Henderson - Hasselbalch equation relates pH, pKa, and the ratio of conjugate base to acid in a buffer: pH = pKa + log([A?]/[HA]). It's fundamental in biochemistry for buffer calculations. Buffer equation.
Which atomic orbital shape corresponds to an s orbital?
Double dumbbell
Spherical
Cloverleaf
Dumbbell-shaped
s orbitals are spherical around the nucleus, with no angular node. p orbitals are dumbbell-shaped, d orbitals often cloverleaf. The shape reflects angular momentum quantum number. Orbital shapes.
Which isotope is used in PET scans to trace metabolic activity?
¹?C
¹³C
³²P
¹?F
Fluorine-18 is a positron-emitting isotope commonly used in PET to image glucose uptake in tissues. It has a short half-life (~110 minutes). Carbon-14 is used in dating, not imaging. Fluorine-18 in PET.
Which term describes the energy required to remove an electron from a gaseous atom?
Reduction potential
Electronegativity
Ionization energy
Electron affinity
First ionization energy is the energy needed to remove the outermost electron from a gaseous atom, creating a cation. Electron affinity is energy change when an electron is added. Electronegativity is a relative measure. Ionization energy details.
Which of these liquids has the highest polarity index?
Hexane
Toluene
Water
Benzene
Water is highly polar (polarity index ~10.2) due to its strong dipole and hydrogen bonding. Hexane and toluene are nonpolar solvents. Benzene is moderately nonpolar. Solvent polarity.
What is the role of van der Waals interactions in biomolecules?
Primary covalent linkages
Weak attractions that stabilize tertiary structure
Electrostatic attractions between ions
Hydrogen bonding networks
Van der Waals forces are weak, transient attractions between nonpolar regions, important for fine-tuning tertiary and quaternary protein structures. They complement stronger bonds. They are not covalent or ionic. Noncovalent interactions.
Which acid-base pair acts as the phosphate buffer in human blood?
H?CO? / HCO??
H?PO?? / HPO?²?
NH? / NH??
HOAc / AcO?
The H?PO??/HPO?²? system helps buffer intracellular fluids and urine, maintaining pH around 6.8. Bicarbonate is the primary blood buffer extracellularly. Phosphate buffer operates in specific compartments. Buffer systems.
Which quantum number set is valid for a 4p electron?
n=4, l=0, m_l=0, m_s=+½
n=4, l=2, m_l=0, m_s= - ½
n=3, l=1, m_l=0, m_s=+½
n=4, l=1, m_l=0, m_s=+½
For a 4p electron, principal quantum number n=4 and azimuthal quantum number l=1. Magnetic quantum number m_l can be - 1, 0, or +1. Spin m_s may be +½ or - ½. Quantum numbers guide.
Which effect explains the anomalously high boiling point of HF compared to HCl?
Stronger dispersion forces
Hydrogen bonding
Dipole-induced dipole interactions
Ionic character
HF forms strong hydrogen bonds between molecules, elevating its boiling point above HCl, which cannot hydrogen-bond to the same extent. Dispersion forces are weaker in HF. Intermolecular forces.
What principle explains why no two electrons in an atom can have the same set of four quantum numbers?
Aufbau principle
Hund's rule
Pauli exclusion principle
Heisenberg uncertainty principle
The Pauli exclusion principle states that each electron in an atom has a unique set of quantum numbers. This rule explains electron configuration and orbital filling. Hund's rule and Aufbau address energy and spin distribution. Quantum rules overview.
Which condition must be met for a reaction to be at equilibrium in terms of Gibbs free energy?
?G < 0
?H = 0
?G > 0
?G = 0
At equilibrium, ?G = 0, meaning there is no net change and forward and reverse reaction rates are equal. ?G < 0 indicates spontaneity, ?G > 0 indicates nonspontaneity. Enthalpy change alone doesn't define equilibrium. Chemical equilibrium.
Which advanced buffer system involves a weak base and its conjugate acid in the cytosol of cells?
Carbonic acid/bicarbonate
Hemoglobin buffer
Phosphate buffer
Ammonia/ammonium
The ammonia/ammonium (NH?/NH??) system buffers cytosolic pH, especially in renal cells. NH? diffuses and accepts protons, forming NH??. Carbonate and phosphate systems operate elsewhere. Cellular buffers.
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Study Outcomes
Identify Atomic Particles -
Pinpoint the roles and properties of protons, neutrons, and electrons in atomic structure using targeted quiz questions.
Describe Atomic Number and Mass -
Explain how atomic number, mass number, and isotopes determine element identity and behavior in biological contexts.
Differentiate Essential and Trace Elements -
Distinguish between elements required in bulk versus trace quantities and their significance in cellular functions.
Apply Atomic Principles to Biological Molecules -
Analyze how atomic interactions and bonding underpin the structure and function of macromolecules in living organisms.
Evaluate Knowledge and Pinpoint Gaps -
Use the biology chapter 2 self quiz to assess your understanding and identify areas for further review before exams.
Cheat Sheet
Atomic Structure Fundamentals -
Atomic structure is the cornerstone of your biology chapter 2 self quiz: protons define the atomic number (Z), neutrons add to the mass number (A), and electrons orbit the nucleus in shells. For example, carbon has Z=6 and A=12, meaning it usually carries 6 neutrons. Picture a tiny solar system to lock electron shells into memory.
Understanding Isotopes and Atomic Mass -
Isotopes are atoms of the same element with different neutron counts, and the atomic mass on your AP Biology Chapter 2 quiz is the weighted average of all isotopes. Carbon-12 (6 neutrons) and Carbon-14 (8 neutrons) illustrate how slight mass differences enable radiometric dating. Remember "mass matters" by thinking "mass# = protons + neutrons."
CHNOPS: Essential Elements for Life -
The six most abundant elements in living organisms - Carbon, Hydrogen, Nitrogen, Oxygen, Phosphorus, Sulfur - are summed up in the mnemonic CHNOPS ("Can Harry Never Offer Perfect Sushi?"). These elements form the backbone of macromolecules like proteins, nucleic acids, lipids, and carbohydrates. Spot them everywhere from the DNA helix to energy-carrying ATP.
Role of Trace Elements in Biological Processes -
Trace elements such as iron (Fe), iodine (I), and zinc (Zn) are vital in minute amounts: Fe is central to hemoglobin, I is in thyroid hormones, and Zn supports enzyme function. Iron deficiency leads to anemia, while low iodine can cause goiter - key points for any chapter 2 biology quiz. Think "Fe for red blood cells, I for Iodine in thyroid" to boost recall.
Types of Chemical Bonds and Their Significance -
Covalent bonds share electron pairs, ionic bonds transfer electrons, and hydrogen bonds form attractions between polar molecules like water - critical for cell structure and function. For instance, NaCl is ionic, while H₂O is a polar covalent molecule that engages in hydrogen bonding to create water's unique properties. Recall "shared vs. borrowed vs. eager" to distinguish covalent, ionic, and hydrogen bonds quickly.
