Chapter 2 Practice Exam
Bio 112
Instructor: Carter
 
Mode:   
     

  1. Anything that occupies space and has mass is considered:
a. Cells
b. Gas
c. Matter
d. Energy
e. Solid
 


  1. Negatively charged particles that move in orbits around the atomic nucleus are:
a. Anions
b. Cations
c. Protons
d. Neutrons
e. Electrons
 


  1. The sum of the protons and neutrons in an atom is known as:
a. Atomic number
b. Atomic mass
c. Chemical formula
d. Isotope
e. Oxidation number
 


  1. Which of the following has the smallest mass?
a. Atom
b. Ion
c. Molecule
d. Electron
e. Proton
 


  1. Neutral (uncharged) atoms contain the same number of electrons as:
a. Protons
b. Neutrons
c. Cations
d. Anions
 


  1. Helium (atomic number 2) is stable because it has 2 electrons, which satisfies the octet rule.
a. True
b. False
 


  1. Because the third shell will hold 18 electrons, chlorine (Cl), atomic number 17, which has seven electrons in the third shell, forms bonds by:
a. Gaining an additional 11 electrons (and the ion becoming Cl-11) to fill the third shell
b. Losing seven electrons (and becoming the ion Cl+7) to make the already full second shell its valence shell
c. Sharing 11 pairs of electrons in covalent bonds to fill the third shell
d. What are you talking about, the third shell doesn’t have to be full, the octet rules says full or eight, Cl only needs to pick up one more electron to be stable
 


  1. The bond formed by sharing electron pairs is:
a. Covalent
b. Ionic
c. Hydrogen
d. Organic
e. Inorganic
 


  1. A chemical bond formed by transferring electrons is:
a. Covalent
b. Ionic
c. Peptide
d. Hydrogen
e. Phosphate
 


  1. Ionic bonds are formed because:
a. The atoms that form ionic bonds are both polar
b. The atoms that form ionic bonds are both nonpolar
c. The ions formed when atoms ionize have the same charge
d. Opposite charges attract
 


  1. When electrons are shared unequally between atoms in a molecule the bond between the atoms is:
a. Polar covalent
b. Ionic
c. Hydrogen
d. Non-polar covalent
e. Water
 


  1. What type of bond forms between the H atoms on one water molecule and the O atoms of other water molecules?
a. Covalent bonds
b. Ionic bonds
c. Hydrogen bonds
d. Phosphate bonds
e. Peptide bonds
 


  1. Positively charged atoms are:
a. Cations
b. Anions
c. Electrons
d. Protons
e. Optimistic
 


  1. The element iodine has the atomic number 53 and an atomic mass of 127. Which of the following is correct for I?
a. 74 electrons, 74 protons, and 53 neutrons
b. 127 electrons, 53 protons, and 74 neutrons
c. 53 electrons, 53 protons, and 53 neutrons
d. 53 electrons, 53 protons, and 74 neutrons
e. 53 electrons, 74 protons, and 74 neutrons
 


  1. When salts are dissolved in water they dissociate into particles called:
a. Acids
b. Electrolytes
c. Bases
d. Electrons
e. Buffers
 


  1. Which of the following bonds is stronger?
a. Covalent
b. Ionic
c. Hydrogen
 


  1. Water is a/an
a. Polar molecule
b. Non-polar molecule
c. Organic compound
d. Element
e. Solute
 


  1. The properties of water are primarily due to:
a. The ability of water to dissolve non-polar compounds
b. The ionic bonds within a water molecule
c. The absence of carbon
d. Hydrogen bonding between water molecules
 


  1. All of the following will increase the rate of a chemical reaction except:
a. An enzyme
b. Decreasing temperature
c. Smaller size molecules
d. Increasing the concentration of the reactants
 


  1. The molecular formula H20 means:
a. An atom of water contains 2 hydrogen molecules and 1 oxygen molecule.
b. A molecule of water contains 2 hydrogen atoms and 1 oxygen atom.
c. An atom of water contains 1 hydrogen molecule and 2 oxygen molecules.
d. A molecule of water contains 1 hydrogen atom and 2 oxygen atoms.
 


  1. A substance that releases hydrogen ions in solution is a/an:
a. Salt
b. Base
c. Acid
d. Lipid
e. pH
 


  1. More hydrogen ions would be in a solution with a pH of:
a. 2.5
b. 4.4
c. 7.35
d. 8.2
e. 12
 


  1. Which solution is acidic?
a. H20
b. H20 + Na+ + Cl-
c. H20 + H+ + Cl-
d. Na+ + OH- + H20
 


  1. The difference in hydrogen ion concentration between a solution with a pH of 9 and a solution with a pH of 5 is:
a. 4 times
b. 40 times
c. 0 – they neutralize each other
d. 10,000 times
e. Can’t compare – the pH 9 solution has OH- ions and the pH 5 solution has H+ ions
 


  1. A substance which minimizes fluctuations in the pH of body fluids is a:
a. Salt
b. Base
c. Acid
d. Buffer
e. Ion
 


  1. Which of the following would be in a good blood buffer?
a. A strong acid
b. A strong base
c. Carbonic acid and sodium bicarbonate
d. Sodium chloride and hydrochloric acid
 


  1. The atomic mass of Na is 23 and the atomic mass of Cl is 35. A 1 M solution of NaCl would contain _____ grams of NaCl in 1 liter of water.
a. 58
b. 28
c. 116
d. 98
e. 48
 


  1. A chemical reaction that builds up or makes bonds is:
a. Catabolic
b. Anabolic
c. Decomposition
d. Exchange
e. Oxidation
 


  1. The sum of all the chemical reactions occurring in the body is/are:
a. Anabolism
b. Catabolism
c. Homeostasis
d. Metabolism
e. Exchange reactions
 


  1. Life is said to be carbon based because carbon atoms make up:
a. Carbohydrates
b. Lipids
c. Proteins
d. Nucleic acids
e. All of the above
 


  1. Nitrogen is always found in which molecule?
a. Inorganic
b. Carbohydrate
c. Lipid
d. Protein
e. Cholesterol
 


  1. Which of the following is most likely a carbohydrate?
a. C6H12O6
b. C22H44COOH
c. CO2
d. C2H4NH2
 


  1. The building blocks or subunits joined to form a carbohydrate are:
a. Monosaccharides
b. Nucleotides
c. Amino acids
d. Phosphate groups
e. Fatty acids
 


  1. Which of the following is a disaccharide?
a. Sucrose
b. Fructose
c. Glucose
d. Glycogen
e. Deoxyribose
 


  1. The amino acid sequence of a protein is known as the:
a. Primary structure
b. Secondary structure
c. Tertiary structure
d. Quarternary structure
 


  1. The building blocks or subunits joined to form a protein are:
a. Monosaccharides
b. Nucleotides
c. Amino acids
d. Phosphate groups
e. Fatty acids
 


  1. The bonds that join the subunits to form a protein are:
a. Ionic bonds
b. Phosphate bonds
c. Hydrogen bonds
d. Peptide bonds
e. Primary bonds
f. Tertiary bonds
 


  1. Hydrogen bonding helps determine the structure of proteins at all levels except:
a. Primary
b. Secondary
c. Tertiary
d. Quaternary
 


  1. The secondary structure of a protein would not contain or be characterized by:
a. Beta pleated sheets
b. Alpha helix
c. Hydrogen bonds
d. Several peptide subunits joined together
 


  1. A triglyceride has:
a. 1 glycerol and 3 fatty acids
b. 3 glycerols and 1 fatty acid
c. 3 glycerols and 3 fatty acids
d. 1 glycerol and 1 fatty acid
 


  1. A polyunsaturated fat has:
a. No double bonds between carbon atoms
b. More than one double bond between carbon atoms
c. Many hydrogens
d. More than one double bond between hydrogen atoms
e. Many carbons
 


  1. An enzyme/substrate complex yields a product and:
a. Hydrogen
b. An unchanged enzyme
c. A denatured enzyme
d. A substrate
 


  1. DNA is in an orderly sequence of:
a. Nucleotides
b. Fatty acids
c. Nucleic acids
d. Amino acids
e. Monosaccharides
 


  1. Which of the nitrogenous bases will bond with guanine?
a. Adenine
b. Cytosine
c. Uracil
d. Thymine
e. Guanine
 


  1. The sugar in RNA is:
a. Ribose
b. Deoxyribose
c. Phosphate
d. Uracil
e. Glucose
 


  1. Which of the following is NOT correct concerning DNA and RNA?
a. They are nucleic acids.
b. They both have a pentose sugar.
c. They contain phosphate groups.
d. They are inorganic molecules.
e. They both contain nitrogenous bases.
 


  1. DNA does not have:
a. Adenine
b. Uracil
c. Thymine
d. Guanine
e. Cytosine
 


  1. The most readily available form of stored energy inside the cell is found in:
a. A peptide bond
b. ATP
c. DNA
d. Kinetic energy
e. Activation energy
 




End of Test