Chemistry Exam Practice Quiz

73 Questions | Total Attempts: 38

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Chemistry Practice Quizzes & Trivia

This is a pratice quiz for my exam. This is for chemistry exam.


Questions and Answers
  • 1. 
    Main block elements form bonds by rearranging electrons so that each atom has a stable octet in its outermost energy level.
    • A. 

      Ionic bond

    • B. 

      Octet energy level

    • C. 

      Empirical formula

    • D. 

      Octet rule

  • 2. 
    A charged particle formed when an atoms loses or gains one or more electrons to form a stable outer shell.
    • A. 

      Ion

    • B. 

      Cation

    • C. 

      Ation

    • D. 

      Ionic bond

  • 3. 
    The particle formed when an acid has donated a H+ ion
    • A. 

      Base

    • B. 

      Conjugate base

    • C. 

      Acid

    • D. 

      Conjugate acid

  • 4. 
    A reaction between a acid and base in which H+ and OH- react to form H20 acid + base à salt + water
    • A. 

      Titration

    • B. 

      Conjugate acid

    • C. 

      Equivalence point

    • D. 

      Neutralization reaction

  • 5. 
    (equivalence point) a point in a titration indicated by the color change of an indicator
    • A. 

      Endpoint

    • B. 

      Midpoint

    • C. 

      Equivalence

    • D. 

      Titration point

  • 6. 
    The bond formed by the attraction of oppositely charged ions (cations- metals and anions – nonmetals) is called _________.
    • A. 

      Cation bond

    • B. 

      Ionic bond

    • C. 

      Covalent bond

    • D. 

      Ionic

  • 7. 
    Simplest whole number ratio of atoms that matches the relative ratio of atoms found in a chemical compound.
    • A. 

      Empirical formula

    • B. 

      Single bond

    • C. 

      VSPER theory

    • D. 

      Chemical reaction

  • 8. 
    Bond formed when atoms share pairs of electrons to achieve stability, often filling their outmost energy levels so that they will have a stable octet.
    • A. 

      Sharedpair

    • B. 

      Ionic bond

    • C. 

      Covalent bond

    • D. 

      Octet

  • 9. 
    Theory of Ionization. In an aqueous solution both molecular and ionic compounds can break apart and form ions Acids and release H+ into water bases release OH- into water
    • A. 

      Bronsted-lowry theory

    • B. 

      Conjugate acids

    • C. 

      Svante arrehenius discovery

    • D. 

      Base

  • 10. 
    the particle formed when a base that accepted a H+ ion
    • A. 

      Acid

    • B. 

      Base

    • C. 

      Conjuage base

    • D. 

      Ph scale

  • 11. 
    PH scale
    • A. 

      Conjuage acid

    • B. 

      Base scale

    • C. 

      Logarithmic scale

    • D. 

      None

  • 12. 
    Derived from the ideal gas law P1 V1/ T1 = P2 V2 / T2
    • A. 

      Ideal gas law

    • B. 

      Boyle's law

    • C. 

      Partial pressure

    • D. 

      Combined gas law

  • 13. 
    Units for Pressure
    • A. 

      Ph, atm, torr

    • B. 

      Ml,torr,atm,m3

    • C. 

      Kpa,mmhg,stm,torr

    • D. 

      Kpa,mmhg,atm,torr

  • 14. 
    The two proportionality constant for ideal gas law equation is…
    • A. 

      0.827 atm/ 74.6 l

    • B. 

      0.0821 Latm/ 62.4 Ltorrmol k

    • C. 

      1.3456 Latm/ 76.5 mol

    • D. 

      0.0812 L atm/ 64.2 Ltorrmol k

  • 15. 
    Material dissolved in a solution
    • A. 

      Solute

    • B. 

      Solution

    • C. 

      Souble

    • D. 

      Slovent

  • 16. 
    Material dissolving the solute to make the solution present in a larger amount. WATER!
    • A. 

      Sloute

    • B. 

      Solute

    • C. 

      Solvent

    • D. 

      Soublibilty

  • 17. 
    Any ion with a positive charge.
    • A. 

      Anion

    • B. 

      Proton

    • C. 

      Cation

    • D. 

      Neutron

  • 18. 
    Four properties of salts
    • A. 

      Melt easily, hard, low boling points, brittle

    • B. 

      Brittle, high boiling points, hard, doesnt melt easily

    • C. 

      Rough, hard, high boiling point, doesnt melt easily

    • D. 

      Salty, sour, bitter, rough

  • 19. 
    If the amount of solute is less than the solubility limited at a given temperature
    • A. 

      Saturated

    • B. 

      Insouble

    • C. 

      Solute

    • D. 

      Unsaturated

  • 20. 
    Concentrated unit, expressed as moles of solute per liter of solution M = mole solute/ liters of solution
    • A. 

      Molarity formula

    • B. 

      Partial pressure

    • C. 

      Moles formula

    • D. 

      Liters solution

  • 21. 
    A dissolved amount of solute that exceeds the normal solubility limit
    • A. 

      Saturated

    • B. 

      Super saturated

    • C. 

      Solube

    • D. 

      Unsaturated

    • E. 

      Constant

  • 22. 
    Any base that dissociates completely
    • A. 

      Weak base

    • B. 

      Base

    • C. 

      Strong base

    • D. 

      Strong acid

  • 23. 
    Bronsted acids are H+ donors and Bronsted bases are H+ acceptors. Example NH3 + H2O
    • A. 

      Bronsted law

    • B. 

      Bronsted base law

    • C. 

      Lowry law

    • D. 

      Bronsted-lowry

  • 24. 
    What principle explains why indicators change colors?
    • A. 

      Ph scale

    • B. 

      Indicator

    • C. 

      Le chatelius principle

    • D. 

      Le cruz principle

  • 25. 
    Reached when PH is 7. The point in a titration process where the moles of standard are stoichometrically equivalent to the moles of substance titrated. 
    • A. 

      Titration

    • B. 

      Stoichometrical

    • C. 

      Equivalence point

    • D. 

      Mid point

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