Principles of Chemistry Pre-Test Questions - 2174 Verified Questions

Principles of Chemistry

Pre-Test Questions

Course Introduction

Principles of Chemistry provides a comprehensive introduction to the fundamental concepts of chemical science. The course covers atomic and molecular structure, chemical bonding, stoichiometry, states of matter, thermochemistry, and the properties of solutions. Students will explore the relationships between chemical reactions and energy, learn to balance equations, and understand the behavior of gases, liquids, and solids. Emphasis is placed on developing problem-solving skills and applying theoretical knowledge to practical experiments, forming a solid foundation for further study in chemistry and related scientific fields.

Recommended Textbook

Fundamentals of General Organic and Biological Chemistry 7th Edition by John E. McMurry

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Chapter 1: Matter and Measurements

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Sample Questions

Q1) How many pounds are contained in 84.0 kg?

A)0.038 lb

B)0.084 lb

C)38.0 lb

D)185 lb

E)380 lb

Answer: D

Q2) Which of the following is a physical change?

A)the rusting of iron

B)the condensation of water vapor

C)the baking of a potato

D)the explosion of nitroglycerin

Answer: B

Q3) An object weighs 37.4 kg.What does the object weigh in the English system?

1 lb = 453.6 g

A)82.5 lb

B)16,965 lb

C)0.0824 lb

D)169.65 lb

Answer: A

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Chapter 2: Atoms and the Periodic Table

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Q1) In terms of atomic structure,the common characteristic of elements in the same group is

A)number of electrons.

B)number of electrons in the outermost shell.

C)number of neutrons.

D)number of protons.

E)none of the above

Answer: B

Q2) The element with the electron configuration 1s²2s²2p⁴ is ________.

A)Be

B)C

C)O

D)Si

E)S

Answer: C

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Chapter 3: Ionic Compounds

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Sample Questions

Q1) Which of the following formulas represents a compound that is an acid?

A)CaSO₄

B)NH₄Cl

C)Mg(OH)₂

D)H₂O

E)H₃PO₄

Answer: E

Q2) The property that describes the ease with which an atom gives up an electron to form a positive ion is

A)atomic number.

B)electron affinity.

C)electronegativity.

D)ionization energy.

E)none of the above

Answer: D

Q3) How are noble gases related to the octet rule?

Answer: Noble gases,except helium,illustrate the stability of elements with a full outer shell (an octet).These elements are unreactive because their valence shell is filled.Helium is also grouped with these elements because it is unreactive due to its filled 1s shell.

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Chapter 4: Molecular Compounds

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Sample Questions

Q1) When two atoms share one or more pairs of electrons,a covalent bond is formed.

A)True

B)False

Q2) The formula for carbon disulfide is ________.

A)CS₂

B)C₂S

C)CSi₂

D)CaS₂

E)(CS)₂

Q3) A chemical bond formed between two identical atoms is a(an)________ bond.

A)atomic

B)covalent

C)hydrogen

D)ionic

E)molecular

Q4) Which point identifies the bond length between the two atoms of the diatomic molecule whose potential energy is shown on the graph?

Q5) Explain how it is possible for CCl₄ to have polar bonds but be a non-polar molecule.A diagram may be helpful in your answer,but it must be explained.

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Chapter 5: Classification and Balancing of Chemical Reactions

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Sample Questions

Q1) The balanced equation for the reaction occurring when iron(III)oxide,a solid,is reduced with pure carbon to produce carbon dioxide and molten iron is

A)2 Fe₃O + C (s) 6 Fe (l)+ CO₂ (g).

B)2 FeO₃ + 3 C (s) 2 Fe (l)+ 3 CO₂ (g).

C)4 Fe₂O₃ + 6 C (s) 8 Fe (l)+ 6 CO₂ (g).

D)2 FeO + C (s) 2 Fe (l)+ CO₂ (g).

E)2 Fe₂O₃ + 3 C (s) 4 Fe (l)+ 3 CO₂ (g).

Q2) In the correctly balanced reaction the coefficient for the H₂O is: ____ Al(OH)₃ + ____ H₂SO₄ ____ Al₂ (SO₄)₃ + ____ H₂O

A)1

B)2

C)3

D)6

E)8

Q3) LX (aq)+ MY (aq) LY (s)+ MX (aq)

A)redox

B)acid-base

C)precipitation

Page 7

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Chapter 6: Chemical Reactions: Mole and Mass

Relationships

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Sample Questions

Q1) A solution containing 145.0 g AgNO₃ is mixed with a CaCl₂ solution and 98.4 of AgCl is recovered.Calculate the % yield of the reaction.

A)40.16%

B)61.11%

C)61.99%

D)80.44%

E)161.3%

Q2) Consider the reaction N₂ (g)+ O₂ (g) 2 NO (g).

a.How many g NO can be produced when 25.0 g of nitrogen reacts?

b.How many g NO can be produced when 25.0 g of oxygen reacts?

c.Based on your answers in a and b,predict the amount of NO that can be produced when 25.0 g nitrogen is reacted with 25.0 g of oxygen.

d.Explain the reasoning used in part c.

Q3) How much Ca(NO₃)₂ should be weighed out to have 0.650 mol?

A)66.4 g

B)97.6 g

C)107 g

D)133 g

E)165 g

Page 8

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Chapter 7: Chemical Reactions: Energy, rates, and Equilibrium

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Sample Questions

Q1) For the reaction given below,what quantity of heat will be produced if 90.0 g of C₃H₈ are consumed in the reaction?

C₃H₈ + 5 O₂ 3 CO₂ + 4

H₂O + 488 kcal

A)996 kcal

B)488 kcal

C)332 kcal

D)239 kcal

E)976 kcal

Q2) For a chemical reaction to occur,all of the following must happen except

A)chemical bonds in the reactants must break.

B)reactant particles must collide with enough energy for change to occur.

C)reactant particles must collide with the correct orientation.

D)a large enough number of collisions must occur.

E)chemical bonds in the products must form.

Q3) Which of the following will affect all reaction rates?

A)the temperature of the reactants

B)the concentrations of the reactants

C)the presence of a catalyst

D)All are correct.

Page 9

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Chapter 8: Gases, liquids, and Solids

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Sample Questions

Q1) Which process is exothermic?

A)gas liquid

B)liquid gas

C)solid liquid

D)solid gas

E)none of the above

Q2) According to Avogadro's Law,the volume of a gas will ________ as the ________ is increased while the ________ are held constant.

A)increase; number of moles; pressure and temperature

B)decrease; number of moles; pressure and temperature

C)increase; temperature; pressure and number of moles

D)decrease; pressure; temperature and number of moles

E)increase; pressure; temperature and number of moles

Q3) Which description best fits a liquid?

A)definite shape and volume; strong intermolecular attractions

B)definite volume; shape of container; moderate intermolecular attractions

C)definite volume; shape of container; no intermolecular attractions

D)volume and shape of container; no intermolecular attractions

E)volume and shape of container; strong intermolecular attractions

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Page 10

Chapter 9: Solutions

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Sample Questions

Q1) What is the molarity of a solution prepared by dissolving 0.750 mol CaCl₂ in enough water to make 0.500 L of solution?

A)0.375 M

B)0.667 M

C)1.50 M

D)83.2 M

E)166.5 M

Q2) The passage of a solvent across a semipermeable membrane because of concentration differences is called

A)dialysis.

B)hemolysis.

C)hydration.

D)osmosis.

E)solvation.

Q3) The term "miscible" is used to describe which type of solution?

A)liquid/liquid

B)liquid/solid

C)gas/liquid

D)gas/gas

E)all of the above

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Chapter 10: Acids and Bases

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Sample Questions

Q1) Which of the following cannot act as a Brønsted base?

A)HCO₃^-

B)CO₃^2-

C)NH₃

D)NH₂^-

E)NH₄⁺

Q2) Which example is not acidic?

A)orange juice

B)soil for azaleas with pH of 4.8

C)a solution of NH₄NO₃ with pH < 7.00

D)lake water that turns blue litmus to red

E)a solution in which [H₃O⁺] = 1.00 × 10^-7

Q3) Which of the following is a weak acid?

A)HNO₃

B)H₃PO₄

C)NH₃

D)HCl

E)OH^-

Q4) Explain the term "amphoteric." Use the hydrogen carbonate ion,HCO₃^- to illustrate amphoteric behavior.

Page 12

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Chapter 11: Nuclear Chemistry

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Sample Questions

Q1) A REM is a biological radiation measurement which is independent of the type of radiation

A)True

B)False

Q2) A sievert is

A)the amount of radiation that produces 2.1 × 10⁹ units of charge in one cubic centimeter of air.

B)a unit used to measure the amount of radiation absorbed per gram of tissue.

C)a unit that measures both the energy and the penetrating power of different types of radiation.

D)the SI unit for radiation absorbed.

E)the amount of radioactive substance that undergoes 3.7 × 10¹⁰ disintegrations per second.

Q3) Three applications of nuclear chemistry are medical imaging,energy production,and archaeological dating.Describe each of these applications and explain what properties of radioactive elements are used in each one.

Q4) List and discuss two criteria used to choose appropriate radioisotopes for use as tracers in medical imaging procedures.

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Chapter 12: Introduction to Organic Chemistry: Alkanes

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Sample Questions

Q1) Which is not a property of most alkanes?

A)soluble in water

B)light odor

C)colorless

D)burn readily in an open flame

E)They are all properties of alkanes.

Q2) The alcohol functional group has

A)a carbon-carbon triple bond.

B)a carbon-oxygen-hydrogen group.

C)a six-membered ring with three double bonds.

D)a double bond between carbon and oxygen.

E)one or more bonds between carbon and nitrogen.

Q3) All of the families below include functional groups which contain oxygen except A)carboxylic acids.

B)alkyl halides.

C)esters.

D)ethers.

E)ketones.

Q4) Describe the unique characteristics of carbon that make it the basis of such a large number of organic compounds.

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Chapter 13: Alkenes, alkynes, and Aromatic Compounds

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Sample Questions

Q1) The bond angle about a carbon atom involved in a triple bond is

A)90°.

B)105°.

C)109.5°.

D)120°.

E)180°.

Q2) This question has three parts:

a.Sketch the carbon skeleton of 3-ethyl-2,5-hexadiene.

b.Explain why this name is not correct.

c.Give the correct name and molecular formula of the compound with the carbon skeleton you drew.

Q3) The term used to describe the geometry of a carbon atom involved in a double bond is

A)distorted tetrahedral.

B)linear.

C)perpendicular.

D)tetrahedral.

E)trigonal planar.

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Chapter 14: Some Compounds With Oxygen, sulfur, or a Halogen

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Sample Questions

Q1) All of the following are properties of ethers except A)the molecules are polar,but do not form hydrogen bonds with other ether molecules. B)low molecular weight ethers are flammable and evaporate easily.

C)ethers dissolve readily in water in all proportions.

D)ethers are relatively unreactive except for flammability.

E)ethers dissolve many organic compounds readily.

Q2) Compounds with the -OH group attached to an aromatic ring are known as A)alcohols.

B)alkyl halides.

C)ethers.

D)hydroxyls.

E)phenols.

Q3) Which alcohol is most soluble in water?

A)ethanol

B)1-propanol

C)1-butanol

D)1-pentanol

E)1-hexanol

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Chapter 15: Amines

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Sample Questions

Q1) Amines can be considered organic derivatives of the inorganic compound

A)ammonia.

B)carbon dioxide.

C)sodium hydroxide.

D)water.

E)none of these

Q2) Which type of amine will react with mineral acids to form soluble ammonium salts?

A)1°

B)2°

C)3°

D)A and B

E)A,B and C

Q3) An amine that is insoluble in water can be made to dissolve by adding it to an aqueous solution of A)HCl.

B)NaOH.

C)a different amine.

D)an amide.

E)none of the above; it can't be made water soluble.

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Chapter 16: Aldehydes and Ketones

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Sample Questions

Q1) What is the product of reduction of 2-butanone?

A)butanal

B)2-butanol

C)butanoic acid

D)1-butanol

E)no reaction

Q2) The substance that precipitates in a positive Benedict test is ________.

A)Ag

B)CuO

C)Cu₂O

D)none of these

Q3) Which of the following names does not fit a real compound?

A)3-methyl-1-pentanone

B)2-methyl-3-pentanone

C)2-butanone

D)3-octanone

E)All are correct.

Q4) Arrange the following compounds in order of increasing boiling point: acetone,n-butane,propanal,1-propanol,2-propanol.

Explain the reasons for your arrangement.

18

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Chapter 17: Carboxylic Acids and Their Derivatives

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Sample Questions

Q1) Which acid would be expected to have the lowest boiling point?

A)acetic

B)benzoic

C)formic

D)oxalic

E)stearic

Q2) When an alcohol reacts with phosphoric acid,the product is referred to as a

A)phosphate salt.

B)phosphate ester.

C)phosphate anion.

D)pyrophosphate.

E)none of the above

Q3) Which of the following has the highest boiling point?

A)ethane,CH₃CH₃

B)dimethyl ketone,CH₃COCH₃

C)ethyl alcohol,CH₃CH₂OH

D)acetic acid,CH₃COOH

E)formaldehyde,HCHO

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Chapter 18: Amino Acids and Proteins

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Sample Questions

Q1) Which protein is considered to be a globular protein?

A)albumin

B)keratin

C)collagen

D)myosin

Q2) The tripeptide represented as ala-leu-gly is named

A)Alanine-glycine-leucine.

B)Alanylglycylleucine.

C)Alanine-leucine-glycine.

D)Alanylleucylglycine.

E)none of these

Q3) The side chains or R groups of amino acids can be classified into each of the following categories except

A)polar.

B)non-polar.

C)basic.

D)acidic.

E)isoelectric.

Q4) List three properties of enantiomers that are the same and three properties that are different.

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Chapter 19: Enzymes and Vitamins

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Q1) The genetic control strategy of enzyme control is most useful for production of enzymes that

A)act as hydrolases.

B)function for only one specific reaction.

C)are produced as zymogens.

D)require vitamins as cofactors.

E)are needed only at certain stages of development.

Q2) Another term for substances that bind irreversibly with the active site of an enzyme is

A)activators.

B)poisons.

C)coenzymes.

D)hormones.

E)zymogens.

Q3) What is the function of enzymes?

A)structure and support

B)energy reserves

C)biochemical catalysts

D)communication between cells

E)physical protection

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Chapter 20: The Generation of Biochemical Energy

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Sample Questions

Q1) Which of the following does not undergo oxidation-reduction reactions?

A)ATP

B)NADH

C)NADPH

D)FAD

Q2) The formation of acetyl coenzyme A is an example of a(an)________ reaction.

A)esterification

B)redox

C)addition

D)acid / base

E)elimination

Q3) The sum of all the biochemical reactions occurring in an organism is

A)anabolism.

B)catabolism.

C)digestion.

D)metabolism.

E)respiration.

Q4) List and discuss the reasons that ATP is so useful as a biochemical energy transport molecule.

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Chapter 21: Carbohydrates

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Q1) When a monosaccharide forms a ring by interaction of one of its hydroxyl groups with its aldehyde group,the bond is referred to as a(an)________ linkage.

A)ether

B)ester

C)acetal

D)hemiacetal

E)glycosidic

Q2) The molecular formula of the common disaccharides in human biochemistry is A)CH₂O.

B)C₂(H₂O)₂.

C)C₆H₁₂O₆.

D)C₁₂H₂₂O₁₁.

E)C₁₂H₂₄O₁₂.

Q3) A glycosidic bond is

A)a bond between any two carbohydrate molecules.

B)a bond formed between an anomeric carbon atom and any -OR group.

C)any bond that can be broken by reaction with water.

D)a bond between anomeric carbon atoms on two separate monosaccharides.

E)none of the above

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Chapter 22: Carbohydrate Metabolism

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Q1) When a person is deprived of food,in which order does the body use the following sources to produce glucose?

I.protein breakdown to amino acids used for gluconeogenesis

II.conversion of glycogen to glucose

III.catabolism of lipids

A)I,II,III

B)III,II,I

C)II,I,III

D)II,III,I

E)III,I,II

Q2) The pathway followed by glucose when energy is needed is A)gluconeogenesis.

B)glycogenesis.

C)glycolysis.

D)lipogenesis.

E)the pentose phosphate pathway.

Q3) Classify each pathway of carbohydrate metabolism as anabolic or catabolic.Justify your choice in each case.

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Chapter 23: Lipids

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Q1) Phosphoglycerides differ from glycerides in that one of the hydroxyl groups of the glycerol is esterified with

A)phosphoric acid.

B)phosphorous.

C)choline.

D)serine.

Q2) Which of the following is not a biochemical function of waxes?

A)prevention of water loss by leaves

B)waterproofing of feathers in shore birds

C)energy storage for animals

D)structural materials in beehives

E)physical protection of mammalian ears

Q3) The function of glycoproteins and glycolipids in cell membranes is to

A)vary the fluidity of the membrane as needed.

B)mediate interactions between the cell and outside agents.

C)provide channels for facilitated diffusion.

D)provide channels for active transport.

E)act as energy sources for active transport.

Q4) Describe the similarities and differences between soaps and emulsifying agents.

Q5) Sketch a lipid bilayer and identify its hydrophobic and hydrophilic portions.

Page 25

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Chapter 24: Lipid Metabolism

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Q1) The formation of malonyl CoA from acetyl CoA and CO₂ also requires the presence of

A)cyclic AMP.

B)ATP.

C)glucose.

D)FAD.

Q2) Each oxidation during fatty acid catabolism directly produces one molecule of ________ and a fatty acid molecule that has been shortened by ________ carbon atom(s).

A)ATP; two

B)acetyl-SCoA; two C)ATP; one

D)acetyl-SCoA; one E)CO₂; three

Q3) Digestion of lipids begins in the ________,in a process catalyzed by ________.

A)mouth; salivary amylase

B)stomach; hydrochloric acid

C)small intestine; pancreatic lipases

D)large intestines; bile acids

E)adipocytes; triacylglycerol lipase

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Chapter 25: Nucleic Acids and Protein Synthesis

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Q1) Replication of DNA produces two daughter DNA molecules in which

A)one daughter molecule contains both parent strands and one daughter molecule contains both newly synthesized strands.

B)each daughter molecule contains one parent strand and one newly synthesized strand.

C)each daughter molecule contains two newly synthesized strands.

D)each daughter molecule contains both parent strand.

E)None of the above happens during replication.

Q2) The bonding forces between the two DNA strands in a double helix are A)polar bonds.

B)peptide linkages.

C)phosphate bonds.

D)hydrogen bonds.

Q3) The chemical combination of ribose and one of the five nitrogen bases results in formation of a A)nucleotide.

B)nucleoside.

C)DNA molecule.

D)chromosome. E)gene.

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Chapter 26: Genomics

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Q1) The process of making multiple copies of DNA is accomplished by a process called

A)polymerase chain reaction.

B)recombinant DNA.

C)restriction endonuclease activity.

D)insertions.

Q2) The function of a restriction enzyme is to

A)build up DNA or RNA molecules one nucleotide at a time.

B)break down DNA or RNA into all their component nucleotides.

C)break a DNA molecule between two specific nucleotides.

D)prevent formation of a chemical bond between a specific pair of nucleotides.

E)prevent formation of the sugar-phosphate backbone of nucleic acids.

Q3) Discuss the importance of telomeres in cell death and in cancer.

Q4) A gene is a(an)

A)complex of DNA and histones formed in a cell nucleus before cell division.

B)segment of DNA that directs synthesis of a specific peptide or protein.

C)list of locations of markers that relate to inheritable traits.

D)set of identical copies of DNA segments from a single ancestor.

E)ordered list of the nucleotides in a segment of DNA.

Q5) Explain the difference between polymorphisms and mutations.

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Chapter 27: Protein and Amino Acid Metabolism

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Q1) nonessential amino acid

A)an amino acid whose carbon skeleton can be converted to a citric acid cycle intermediate,which ultimately becomes glucose

B)the transfer of an amine group from an amino acid to an -keto acid

C)an amino acid whose carbon skeleton can be converted to a citric acid cycle intermediate that later becomes a ketone body or a fatty acid

D)the collection of all the free amino acids in the body

E)an amino acid that must be obtained in the diet because humans do not have the appropriate anabolic pathways for its synthesis

F)the biochemical pathway that converts nitrogen and its derivatives to a less toxic form for excretion

G)an amino acid which can be synthesized by the human body as needed

Q2) The source of nitrogen for the synthesis of nonessential amino acids is A)glutamate. B)acetate.

C)pyruvate.

D)oxaloacetate. E)urea.

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Chapter 28: Chemical Messengers: Hormones, neurotransmitters, and Drugs

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Q1) Mineralocorticoids are a specific type of steroid whose function is to A)maintain pregnancy.

B)promote development of secondary male sex characteristics.

C)promote development of secondary female sex characteristics.

D)regulate the sodium/potassium balance in cellular fluids.

E)regulate glucose metabolism.

Q2) Chemical messengers deliver information by interacting with ________ in or at the target cell.

A)receptors

B)antibodies

C)antigens

D)hormones

E)neurotransmitters

Q3) All of the following types of molecules function as chemical messengers in the body except

A)polypeptide hormones such as insulin.

B)steroid hormones such as progesterone.

C)neurons,including axons and dendrons.

D)amino acid derivatives classified as catecholamines.

E)neurotransmitters such as acetylcholine.

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Chapter 29: Body Fluids

Available Study Resources on Quizplus for this Chatper

63 Verified Questions

63 Flashcards

Source URL: https://quizplus.com/quiz/65905

Sample Questions

Q1) Which of the following is considered to be a normal constituent of urine?

A)protein

B)ketone bodies

C)amino acids

D)hemoglobin

Q2) How would urinary output be affected if the antidiuretic hormone was overexcreted?

A)increased output

B)decreased output

C)greatly decrease output

D)no affect on output

Q3) In which part of the kidney is most of the water reabsorbed from the urine?

A)glomerulus

B)Henle's loop

C)kidney tubule

D)Bowman's capsule

E)nephrons

Q4) Distinguish between inflammatory and immune responses to antigens.

Q5) Comment on the tertiary structure of the defensive proteins immunoglobulins and fibrin.Explain how the structure of each protein contributes to its function.

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