Chem Test 1

1. What is kinetic energy?

A. Stored energy

B. Energy of an object in motion

C. Energy caused by temperature

D. Chemical energy

2. What is potential energy?

A. Energy of motion

B. Stored energy based on an object's position, composition, or state

C. Heat energy only

D. Energy released during boiling

3. What is the SI unit of energy?

A. Calorie

B. Gram

C. Joule

D. Liter

4. One calorie (cal) is approximately equal to:

A. 100 J

B. 1,000 J

C. 4.184 J

D. 41.84 J

5. One food Calorie (Cal) is equal to:

A. 1 cal

B. 10 cal

C. 100 cal

D. 1,000 cal

6. Which state of matter has a definite shape and definite volume?

A. Gas

B. Liquid

C. Solid

D. Plasma

7. Which state has a definite volume but takes the shape of its container?

A. Solid

B. Liquid

C. Gas

D. None

8. Which state has an indefinite shape AND indefinite volume?

A. Solid

B. Liquid

C. Gas

D. Ice

9. In a solid, particles are:

A. Very far apart and moving rapidly

B. Closely packed and vibrating in fixed positions

C. Able to slide freely past one another

D. Completely motionless

10. Melting is the change from:

A. Liquid → solid

B. Gas → liquid

C. Solid → liquid

D. Solid → gas

11. Melting is:

A. Exothermic

B. Endothermic

C. Neither

D. A chemical reaction

12. Freezing is the change from:

A. Solid → liquid

B. Liquid → solid

C. Gas → liquid

D. Gas → solid

13. Which phase change is gas → liquid?

A. Melting

B. Vaporization

C. Condensation

D. Sublimation

14. Which phase change is solid → gas?

A. Deposition

B. Sublimation

C. Condensation

D. Freezing

15. Which phase change is gas → solid?

A. Deposition

B. Sublimation

C. Vaporization

D. Melting

16. Vaporization is:

A. Solid → liquid

B. Liquid → gas

C. Gas → liquid

D. Gas → solid

17. Evaporation occurs:

A. Only at the boiling point

B. At the surface of a liquid, below its boiling point

C. Only when a liquid freezes

D. Throughout the entire liquid

18. Which statement describes an exothermic process?

A. It absorbs heat from the surroundings

B. It releases heat into the surroundings

C. It destroys energy

D. It always causes melting

19. An endothermic process makes the surroundings feel:

A. Hotter

B. Colder

C. The same

D. Heavier

20. Which is a physical property?

A. How a substance reacts with oxygen

B. Flammability

C. Density

D. Ability to form a new substance

21. A chemical property describes:

A. The color of a substance

B. The mass of a substance

C. How a substance reacts or changes into a new substance

D. The volume of a substance

22. Why does ice float in liquid water?

A. Ice is hotter

B. Ice is less dense than liquid water

C. Ice has more mass

D. Ice has no particles

23. Water is considered a universal solvent mainly because of its:

A. Density

B. Polarity

C. Low temperature

D. High mass

24. Cohesion is when water:

A. Sticks to other surfaces

B. Sticks to itself

C. Freezes

D. Evaporates

25. Adhesion is when water:

A. Sticks to other surfaces

B. Sticks only to itself

C. Changes into gas

D. Becomes less dense

26. Which law states that matter cannot be created or destroyed in a chemical reaction?

A. Law of Definite Proportions

B. Law of Conservation of Mass

C. Law of Gravity

D. Law of Energy

27. According to the Law of Conservation of Mass:

A. Reactants always have more mass than products

B. Products always have more mass than reactants

C. Mass of reactants = mass of products

D. Mass disappears during reactions

28. What is the chemical formula for carbon dioxide?

A. CO

B. CO₂

C. C₂O

D. C₂O₂

29. What is the formula for sodium chloride?

A. NaCl

B. SoCl

C. Na₂Cl

D. SCl

30. What is the formula for glucose?

A. C₆H₆

B. C₆H₁₂O₆

C. CH₄

D. C₁₂H₆O₆

31. What is the formula for methane?

A. CH₄

B. CO₂

C. C₆H₁₂O₆

D. HCl

32. What is the formula for hydrochloric acid?

A. H₂O

B. NaCl

C. HCl

D. CO₂

33. The Law of Definite Proportions says that a chemical compound:

A. Can contain any amount of each element

B. Always contains the same elements in the same proportions by mass

C. Can change its elements depending on sample size

D. Is always a mixture

34. A homogeneous mixture is:

A. Completely uniform throughout

B. Made of visibly different parts

C. Always a solid

D. Always cloudy

35. A heterogeneous mixture is:

A. Completely uniform

B. Not uniform and has distinct phases

C. Always a solution

D. Made of only one substance

36. Which is an example of a mechanical mixture?

A. A mixture with large, easily visible pieces

B. A perfectly uniform solution

C. A pure compound

D. A single element

37. A suspension contains:

A. Tiny particles that never settle

B. Large particles that settle out over time

C. No particles

D. Only gases

38. A colloid contains:

A. Medium-sized particles that don't settle out over time

B. Large particles that quickly settle

C. No particles

D. Only solids

39. A solution consists of:

A. Solute + solvent

B. Solid + gas only

C. Two solids only

D. Reactant + product

40. In a salt-water solution, the salt is the:

A. Solvent

B. Solute

C. Colloid

D. Suspension

41. In a salt-water solution, the water is the:

A. Solute

B. Solvent

C. Suspension

D. Product

42. Which can increase the rate at which a substance dissolves?

A. Stirring

B. Crushing

C. Changing temperature

D. All of the above

43. A saturated solution contains:

A. No solute

B. The maximum amount of dissolved solute possible at that temperature

C. Less solute than possible

D. More solute than normally possible

44. An unsaturated solution contains:

A. Less than the maximum amount of solute

B. The maximum amount of solute

C. More solute than normally possible

D. No solvent

45. A supersaturated solution contains:

A. Less solute than normal

B. No solute

C. More dissolved solute than is normally stable at that temperature

D. Only solvent

46. Which method separates an insoluble solid from a liquid?

A. Filtration

B. Distillation

C. Chromatography

D. Electrolysis

47. Distillation separates liquids based mainly on differences in:

A. Color

B. Boiling points

C. Mass only

D. Density only

48. Chromatography separates substances based on:

A. How they travel across a surface

B. Their boiling points

C. Their melting points

D. Their mass

49. Evaporation can separate a solution by:

A. Freezing the solvent

B. Driving off the liquid and leaving the solid solute behind

C. Filtering the liquid

D. Turning the solute into a gas

50. To separate a compound into its elements, you may need to:

A. Filter it

B. Use electrolysis to break chemical bonds

C. Evaporate it

D. Use chromatography

🔢 Significant Figures

51. Scientific notation is generally written as:

A. M × 10ⁿ

B. M + 10ⁿ

C. M ÷ 10ⁿ

D. M − 10ⁿ

52. In scientific notation, M should generally be:

A. Less than 0

B. Between 1 and 10

C. Greater than 100

D. Exactly 10

53. How many significant figures are in 0.00520?

A. 1

B. 2

C. 3

D. 4

54. How many significant figures are in 5.20?

A. 1

B. 2

C. 3

D. 4

55. Zeros between nonzero numbers are:

A. Never significant

B. Always significant

C. Only significant in decimals

D. Only significant in whole numbers

56. Leading zeros are:

A. Significant

B. Not significant

C. Always counted

D. Only significant in scientific notation

57. Trailing zeros in a number with a decimal point are:

A. Always insignificant

B. Significant

C. Never counted

D. Negative

⭐ Challenge Questions

58. Which phase change is endothermic?

A. Freezing

B. Condensation

C. Deposition

D. Sublimation

59. Which pair contains two exothermic phase changes?

A. Melting and vaporization

B. Sublimation and melting

C. Freezing and condensation

D. Vaporization and sublimation

60. Which statement is TRUE?

A. Gases have definite volume

B. Liquids have definite shape

C. Solids have particles that vibrate in fixed positions

D. Solids expand to fill their containers