Full SAT Chemistry Practice Test 1: Part A

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Question 23 questions

Time 16 minutes

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1. May be used in combination with a calorimeter to compare the specific heats of two substances

A. Thermometer
B. Conductivity tester
C. Salt bridge
D. Buret
E. Graduated cylinder

2. Is used to measure the volume of a solid by water displacement

A. Thermometer
B. Conductivity tester
C. Salt bridge
D. Buret
E. Graduated cylinder

3. Useful for adding small quantities of acid into a base

A. Thermometer
B. Conductivity tester
C. Salt bridge
D. Buret
E. Graduated cylinder

4. Completes the circuit of an electrochemical cell

A. Thermometer
B. Conductivity tester
C. Salt bridge
D. Buret
E. Graduated cylinder

5. Always amphoteric in nature

A. Nucleic acids
B. Proteins
C. Carbohydrates
D. Lipids
E. Electrolytes

6. Found as both straight-chained and branched polymers

A. Nucleic acids
B. Proteins
C. Carbohydrates
D. Lipids
E. Electrolytes

7. Deoxyribose in DNA nucleotides belongs to this family of biologically important molecules

A. Nucleic acids
B. Proteins
C. Carbohydrates
D. Lipids
E. Electrolytes

8. Always ionic in nature

A. Nucleic acids
B. Proteins
C. Carbohydrates
D. Lipids
E. Electrolytes

9. Tend not to be water soluble, and aggregate into droplets or molecular bilayers

A. Nucleic acids
B. Proteins
C. Carbohydrates
D. Lipids
E. Electrolytes

10. Represents the decomposition of a compound into its constituent elements

A. Ag+ + Br → AgBr
B.
C.
D. +
E. 2HgO → 2Hg + O2

11. Represents alpha decay

A. Ag+ + Br → AgBr
B.
C.
D. +
E. 2HgO → 2Hg + O2

12. Represents an oxidation-reduction reaction

A. Ag+ + Br → AgBr
B.
C.
D. +
E. 2HgO → 2Hg + O2

13. Causes the neutron-to-proton ratio in a nucleus to be lowered

A. Ag+ + Br → AgBr
B.
C.
D. +
E. 2HgO → 2Hg + O2

14. Is the activation energy of the reverse reaction

A.
B.
C.
D.
E.

15. Is the enthalpy change of the forward reaction

A.
B.
C.
D.
E.

16. Represents energy of the activated complex

A.
B.
C.
D.
E.

17. Holds a sample of barium iodide, BaI2, together

A. Hydrogen bonding
B. Ionic bonding
C. Metallic bonding
D. Nonpolar covalent bonding
E. Polar covalent bonding

18. Allows solids to conduct electricity

A. Hydrogen bonding
B. Ionic bonding
C. Metallic bonding
D. Nonpolar covalent bonding
E. Polar covalent bonding

19. Attracts atoms of hydrogen to each other in an H2 molecule

A. Hydrogen bonding
B. Ionic bonding
C. Metallic bonding
D. Nonpolar covalent bonding
E. Polar covalent bonding

20. Responsible for relatively low vapor pressure of water

A. Hydrogen bonding
B. Ionic bonding
C. Metallic bonding
D. Nonpolar covalent bonding
E. Polar covalent bonding

21. Gives off a purplish vapor as it sublimes

A. Iron(III) chloride, FeCl3(s)
B. Iodine, I2(s)
C. Sodium hydroxide, NaOH(s)
D. Sucrose, C12H22O11(s)
E. Graphite, C(s)

22. Can conduct electricity in the solid state

A. Iron(III) chloride, FeCl3(s)
B. Iodine, I2(s)
C. Sodium hydroxide, NaOH(s)
D. Sucrose, C12H22O11(s)
E. Graphite, C(s)

23. Its dissolution in water is highly exothermic

A. Iron(III) chloride, FeCl3(s)
B. Iodine, I2(s)
C. Sodium hydroxide, NaOH(s)
D. Sucrose, C12H22O11(s)
E. Graphite, C(s)