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Quizzes > Science > Chemistry

Master AP Biology Unit 2: Chemistry of Life Quiz - Test Yourself!

Ready for a ch.2 self-quiz biology challenge? Dive into this unit 2 AP Bio practice test now!

Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper cut style molecules and beakers above textbook on teal background, AP Bio Unit 2 chemistry practice quiz

Ready to level up your study routine? Challenge yourself with our free ap bio unit 2 practice test, focused on Chapter 2 chemistry essentials! This ch.2 self-quiz biology tool helps you review pH, macromolecules, and bonding in minutes, boosting your confidence before exam day. Dive into the interactive ap bio unit 2 practice test. Whether you want quick feedback and clear explanations or to reinforce water properties and macromolecules, this quiz covers key reactions to solidify your understanding. Want more? Tackle our ap bio chapter 2 quiz to master every concept. Ready to crush your exam prep? Take the quiz now!

What subatomic particle defines the atomic number of an element?
Proton
Electron
Photon
Neutron
The atomic number is equal to the number of protons in an atom's nucleus. Neutrons and electrons do not affect the atomic number, and photons are particles of light. The identity of an element is determined by its proton count. More on atomic number
Which statement correctly describes an isotope?
Atoms with the same number of protons but different numbers of neutrons
Atoms with the same number of neutrons but different numbers of electrons
Atoms with the same mass number but different atomic numbers
Atoms with different numbers of protons and neutrons
Isotopes of an element share the same proton count (atomic number) but differ in neutron number, which changes their mass. Different atomic numbers would change the element itself. Electron count variations create ions, not isotopes. Learn about isotopes
What type of bond involves the equal sharing of electrons between two atoms?
Nonpolar covalent bond
Polar covalent bond
Hydrogen bond
Ionic bond
Nonpolar covalent bonds occur when two atoms share electrons equally due to similar electronegativities. Polar covalent bonds share electrons unequally, ionic bonds transfer electrons, and hydrogen bonds are weak attractions between molecules. Details on covalent bonds
Which property of water allows insects to walk on its surface?
Cohesion
Adhesion
High specific heat
Density
Cohesion is the attraction between water molecules via hydrogen bonding, creating surface tension that can support small insects. Adhesion is water's attraction to other surfaces, and high specific heat and density relate to temperature regulation and phase behavior. Water properties explained
What term describes water molecules sticking to other polar surfaces?
Capillarity
Solvent properties
Adhesion
Cohesion
Adhesion is the attraction between water molecules and other polar or charged surfaces, helping water climb up plant vessels. Cohesion refers specifically to water-to-water attraction. Capillarity involves both cohesion and adhesion. More on adhesion
What is the pH of pure water at 25°C?
14
7
0
1
Pure water at 25°C has equal concentrations of H+ and OH? ions, each at 10?? M, giving a pH of ?log(10??) = 7. Solutions with pH 7 are neutral. pH scale overview
Which functional group consists of a carbon double-bonded to oxygen and also bonded to a hydroxyl group?
Amino group
Carboxyl group
Hydroxyl group
Phosphate group
A carboxyl group has the structure - COOH, with a carbon double-bonded to oxygen and single-bonded to a hydroxyl. This group acts as an acid by donating H+. Details about carboxyl groups
Which biomolecule includes monomers called amino acids?
Proteins
Lipids
Carbohydrates
Nucleic acids
Proteins are made from amino acid monomers linked by peptide bonds. Carbohydrates are built from sugars, lipids from fatty acids/glycerol, and nucleic acids from nucleotides. Protein basics
What process joins monomers by removing water?
Dehydration synthesis
Hydrolysis
Ionic bonding
Denaturation
Dehydration synthesis (condensation) links monomers by removing water, forming covalent bonds. Hydrolysis is the reverse, adding water to break bonds. Macromolecule formation
Which term describes a solution that resists changes in pH?
Buffer
Acid
Salt
Base
Buffers are solutions that minimize pH changes by absorbing or releasing H+ when acids or bases are added. Acids lower pH, bases raise pH, and salts have no buffering action. Buffer solutions
Which element is the backbone of organic molecules?
Nitrogen
Carbon
Oxygen
Phosphorus
Carbon's four valence electrons allow it to form four covalent bonds, creating diverse organic structures. Oxygen, nitrogen, and phosphorus are important but do not form the backbone. Organic chemistry overview
An electronegativity difference greater than which value typically indicates an ionic bond?
0.5
1.7
0.1
2.1
Electronegativity differences above ~1.7 usually lead to ionic bond character, where electrons transfer rather than share. Smaller differences yield polar or nonpolar covalent bonds. Ionic bond details
Which interaction is a weak attraction between molecules due to fluctuating dipoles?
Ionic bond
Hydrogen bond
Van der Waals forces
Covalent bond
Van der Waals forces arise from transient dipoles induced in atoms and molecules. They are weaker than hydrogen bonds and covalent or ionic interactions. Van der Waals forces
Which feature of water contributes to moderating Earth's climate by absorbing heat?
High density as a solid
High specific heat
Nonpolar nature
Low heat of vaporization
Water's high specific heat allows it to absorb large amounts of heat with minimal temperature change, buffering climate fluctuations. Its solid form is less dense, but that affects ice formation. Water's thermal properties
Which pH indicates a basic solution?
7
6
12
2
Solutions with pH values above 7 are basic (alkaline). A pH of 12 is strongly basic, while pH 7 is neutral and pH below 7 is acidic. Understanding pH
What is the monomer of carbohydrates?
Monosaccharide
Amino acid
Fatty acid
Nucleotide
Monosaccharides, or simple sugars like glucose, are the building blocks of carbohydrates. Disaccharides and polysaccharides form via glycosidic linkages between monosaccharides. Monosaccharides explained
Which functional group contains nitrogen and acts as a base by accepting H+?
Amino
Carbonyl
Sulfhydryl
Phosphate
Amino groups ( - NH2) can accept a proton to become - NH3+, acting as bases. Sulfhydryl groups are - SH, carbonyls are C=O, and phosphates are acidic. Amino group details
Which macromolecule class is insoluble in water and makes up cellular membranes?
Carbohydrates
Lipids
Nucleic acids
Proteins
Lipids, including phospholipids, are hydrophobic and form the bilayer of cell membranes. Carbohydrates and proteins are more water-soluble. Lipid overview
Which type of isomer has the same molecular formula but differs in spatial arrangement around a double bond?
Enantiomer
Structural isomer
Cis-trans isomer
Functional isomer
Cis-trans (geometric) isomers differ around a double bond, with substituents on the same side (cis) or opposite sides (trans). Structural isomers differ in connectivity, and enantiomers are mirror images. Geometric isomerism
Which buffer system is important in maintaining blood pH around 7.4?
Carbonic acid-bicarbonate buffer
Hemoglobin buffer
Ammonia buffer
Phosphate buffer
The carbonic acid (H2CO3) - bicarbonate (HCO3?) system is the primary buffer in blood, keeping pH near 7.4. Phosphate buffers work in cells, and ammonia/hemoglobin have secondary roles. Bicarbonate buffer
At chemical equilibrium, what is true about the rates of the forward and reverse reactions?
The forward reaction stops
The reverse reaction stops
They occur at the same rate
Both rates are zero
At equilibrium, the forward and reverse reaction rates are equal, so concentrations of reactants and products remain constant. Neither reaction stops, and rates are not zero. Chemical equilibrium
What is the definition of molarity?
Grams of solute per liter of solution
Moles of solute per liter of solution
Moles of solute per kilogram of solvent
Grams of solute per kilogram of solvent
Molarity (M) is defined as the number of moles of solute dissolved per liter of solution. It is a common concentration unit in chemistry. Molar concentration
Calculate the pH of a solution with [H+] = 1 × 10?? M.
pH 5
5 × 10?
pH 9
1 × 10??
pH is calculated as ?log[H+]. For [H+] = 1×10?? M, pH = ?log(10??) = 5. pH calculations
Using the Henderson-Hasselbalch equation, pH = pKa + log([A?]/[HA]), what ratio [A?]/[HA] is required for pH = pKa?
1 : 1
1 : 10
0 : 1
10 : 1
When pH equals pKa, log([A?]/[HA]) = 0, so [A?]/[HA] = 1. That means equal concentrations of conjugate base and acid. Henderson - Hasselbalch
Given acetic acid with pKa 4.76, what is the pH of a buffer with [acetate] = 0.1 M and [acetic acid] = 0.1 M?
6.76
4.76
5.76
3.76
With equal concentrations of conjugate base and acid, pH = pKa = 4.76 by Henderson-Hasselbalch. Buffer calculations
Which type of bond is found between water molecules due to attraction between partial charges?
Ionic
Nonpolar covalent
Polar covalent
Hydrogen bond
Hydrogen bonds form between the partial positive hydrogen of one water molecule and the partial negative oxygen of another. Covalent bonds hold atoms in a single water molecule together. Hydrogen bonding
Linking five glucose monomers into a polysaccharide produces how many water molecules?
5
6
4
1
Dehydration synthesis removes one water molecule per glycosidic linkage. Five monomers link by four bonds, releasing four water molecules. Polysaccharide formation
Which functional group characterizes an amino acid side chain that can accept a proton?
Hydroxyl
Carbonyl
Carboxyl
Amino
Amino side chains contain - NH2 which can accept a proton to form - NH3+, acting as a base. Carboxyl groups donate protons, and hydroxyl/carbonyl are neutral or polar but not basic. Amino acid groups
Which statement distinguishes ketoses from aldoses?
Ketoses have the carbonyl within the chain while aldoses have it at the end
Aldoses have the carbonyl within the chain
Aldoses lack carbonyl groups entirely
Ketoses have the carbonyl at the end of the chain
Aldoses have a carbonyl group at the end of the carbon chain (aldehyde), whereas ketoses have it internally (ketone). This difference affects reactivity and sugar classification. Ketose vs aldose
What is the hybridization of the carbon atoms in ethylene (H?C=CH?)?
sp²
sp³d
sp
sp³
In ethylene, each carbon forms three sigma bonds and has one unhybridized p orbital for the pi bond, giving sp² hybridization. sp² hybridization
At physiological pH (~7.2), what is the net charge on glycine in its zwitterionic form?
+2
+1
-1
0
At physiological pH, glycine exists as a zwitterion with a positively charged amino group and negatively charged carboxyl group, resulting in a net neutral (0) charge. Amino acid zwitterions
Which type of bond allows for the tertiary structure of proteins via disulfide bridges?
Hydrogen bond
Van der Waals
Covalent bond
Ionic bond
Disulfide bridges are covalent bonds between sulfhydryl groups of cysteine residues, stabilizing tertiary protein structure. Hydrogen bonds and ionic interactions also contribute but are not disulfide bridges. Disulfide bond info
Which of the following is a structural isomer of glucose?
Fructose
Maltose
Cellulose
Sucrose
Fructose has the same molecular formula (C?H??O?) as glucose but a different structure (ketose vs aldose), making it a structural isomer. Sucrose and maltose are disaccharides, and cellulose is a polymer. Fructose structure
What property of water explains why ice floats on liquid water?
Lower specific heat
Increased polarity
Higher heat of vaporization
Lower density
In its solid form, water molecules are arranged in a lattice stabilized by hydrogen bonds, making ice less dense than liquid water, so it floats. This is unusual compared to most substances. Ice density
For a buffer of acetic acid (pKa = 4.76), what ratio of acetate to acetic acid is needed to achieve a pH of 5.76?
1 : 5
10 : 1
1 : 10
5 : 1
Using Henderson - Hasselbalch, pH ? pKa = log([A?]/[HA]), so 5.76 ? 4.76 = 1 = log ratio, ratio = 10:1. Buffer equation
How many liters of 0.5 M NaOH are required to fully neutralize 0.2 moles of HCl?
0.2 L
0.4 L
0.5 L
0.1 L
Neutralization requires equal moles of HCl and NaOH. 0.2 mol HCl needs 0.2 mol NaOH. Volume = moles / molarity = 0.2 mol / 0.5 M = 0.4 L. Neutralization reactions
Calculate the acid dissociation constant (Ka) for an acid with pKa of 3.5.
3.16 × 10??
1.0 × 10?³
3.5 × 10??
5.0 × 10??
Ka = 10^(?pKa). For pKa = 3.5, Ka = 10^(?3.5) ? 3.16 × 10??. Acid dissociation constant
The dielectric constant of water contributes to its ability to dissolve ionic compounds by:
Increasing hydrophobic interactions
Strengthening ionic bonds
Making water nonpolar
Weakening ionic bonds between ions
Water's high dielectric constant reduces the electrostatic attraction between oppositely charged ions, making it easier to separate and solvate them. This underlies its effectiveness as a solvent for salts. Dielectric constant
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Study Outcomes

  1. Understand atomic structure -

    Identify the subatomic particles that compose atoms, distinguish isotopes, and describe how atomic number and mass number define each element.

  2. Differentiate chemical bonds -

    Analyze the characteristics of ionic, covalent, and hydrogen bonds and predict how bond type influences molecular stability and interactions.

  3. Explain water's unique properties -

    Describe how hydrogen bonding gives rise to cohesion, adhesion, high specific heat, and solvent capabilities critical for living systems.

  4. Apply pH and buffer concepts -

    Calculate pH values, evaluate buffer effectiveness, and assess how acid-base balance is maintained in biological contexts.

  5. Identify key functional groups -

    Recognize major organic functional groups in biological molecules and predict how they influence chemical reactivity and structure.

  6. Evaluate chemistry in biological systems -

    Integrate concepts of atoms, bonds, and water chemistry to explain their roles in macromolecule function and cellular processes.

Cheat Sheet

  1. Atomic Structure & Isotopes -

    Review how protons, neutrons, and electrons define an atom's identity and mass - atomic number = # protons, atomic mass ≈ protons + neutrons (per UC Berkeley). Mnemonic: "APE" (Atom's Protons Equal) helps recall that electrons balance proton charge. Understanding isotopes and their radioactivity is key for carbon dating in AP Biology Chapter 2.

  2. Covalent, Ionic & Hydrogen Bonds -

    Differentiate covalent (shared e - ), ionic (transferred e - ), and hydrogen bonds (partial charges) as outlined by Khan Academy. For example, O - H covalent bonds in H₂O create polar molecules that form H-bonds, driving cohesion and adhesion. Remember "CLIP" (Covalent, Ionic, Polar) to sort bond types when tackling your ap bio unit 2 practice test.

  3. Water's Unique Properties -

    Water's high specific heat, surface tension, and solvent capabilities stem from extensive hydrogen bonding (source: NOAA's Earth System Research Laboratory). These emergent properties are central to ch.2 self-quiz biology questions on thermoregulation and osmosis. Visualize sticky H₂O molecules "holding hands" to recall cohesion and adhesion effects in capillary action.

  4. Essential Functional Groups -

    Master the six major functional groups - hydroxyl, carbonyl, carboxyl, amino, phosphate, and methyl - as defined by NCBI. Use the memory phrase "Can Our Cat Always Purr Mellowly?" to picture C=O (carbonyl), - OH (hydroxyl), - COOH (carboxyl), - NH₂ (amino), - PO₄²❻ (phosphate), and - CH₃ (methyl). Recognizing these is crucial for forming macromolecules in AP Bio Chapter 2.

  5. pH, Acids, Bases & Buffers -

    Recall pH = - log₝₀[H❺] and how bicarbonate (H₂CO₃/HCO₃❻) stabilizes blood pH around 7.4 (per American Chemical Society). Practice calculating shifts in [H❺] for acid/base titration problems in your unit 2 AP Bio practice test. A quick tip: each pH unit change = tenfold difference in H❺ concentration!

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