Elements, Atoms And Bonding Rho Quiz

13 Questions | Total Attempts: 60

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Elements, Atoms And Bonding Rho Quiz

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Questions and Answers
  • 1. 
    What is the difference between a compound and a mixture?
    • A. 

      A compound is a pure substance made up of two or more elements that are combined chemically in a specific ratio. A mixture is two or more substances that are in the same place and are not chemically combined.

    • B. 

      A mixture is a pure substance made up of two or more elements that are combined chemically in a specific ratio. A compound is two or more substances that are in the same place and are not chemically combined.

    • C. 

      A compound is a mixture made up of two or more elements that are chemically combined. A mixture is a combination of two or more substances that occupy the same place.

    • D. 

      A compound is set of element that are blended but not chemically combined. A mixture is made up of emulsifiers.

  • 2. 
    A compound is different from an element because a compound is: 
    • A. 

      Made of two or more elements chemically combined.

    • B. 

      The building block of all matter.

    • C. 

      A mixture of elements.

    • D. 

      A pure substance.

  • 3. 
    Identify the scientist who theorized the atom to be made up of mostly empty space with electrons moving around a small positively charged nucleus in the center of the atom. This scientist named the positively charged particles in the nucleus protons.
    • A. 

      Rutherford

    • B. 

      Thomson

    • C. 

      Bohr

    • D. 

      Dalton

    • E. 

      Chadwick

  • 4. 
    Identify the scientist who contributed the basics of the atomic theory that is still accepted today. 
    • A. 

      Dalton

    • B. 

      Rutherford

    • C. 

      Thomson

    • D. 

      Chadwick

    • E. 

      Bohr

  • 5. 
    Identify the scientist who found that atoms contain negatively charged particles and reasoned that because atoms must be neutral, an atom needs to contain some positive charge. This scientist thought that the negatively charged particles would be scattered throughout a ball of positive charge. The negatively charged particles later became known as electrons. 
    • A. 

      Thomson

    • B. 

      Chadwick

    • C. 

      Dalton

    • D. 

      Rutherford

    • E. 

      Bohr

  • 6. 
    Identify the scientist who revised earlier models to show that electrons could only have a specific amount of energy and move in certain orbits. The electron orbits resemble planet orbits or layers of an onion.
    • A. 

      Bohr

    • B. 

      Dalton

    • C. 

      Chadwick

    • D. 

      Thomson

    • E. 

      Rutherford

  • 7. 
    This scientist discovered another particle in the nucleus of an atoms. The discovery completed the modern atomic model. This particle was hard to detect because it does not have an electrical charge even though it has nearly the same mass as a proton. Because the particle had no electrical charge it was called a neutron.
    • A. 

      Chadwick

    • B. 

      Bohr

    • C. 

      Thomson

    • D. 

      Rutherford

    • E. 

      Dalton

  • 8. 
    Elements are called building blocks of matter because:
    • A. 

      All matter is composed of one element or a combination of two of more elements.

    • B. 

      All elements are made of molecules.

    • C. 

      All matter is made of hydrogen.

    • D. 

      All matter is composed of two or more elements in a specific ratio.

  • 9. 
    In 430 b.c. ancient Greece, a philosopher named Democritus proposed the idea that matter is made up of very small pieces that are "uncuttable" into smaller parts and still be that element. It took 2000 years until Democritus' idea was accepted. These small "uncuttable" pieces are called:
    • A. 

      Atoms

    • B. 

      Molecules

    • C. 

      Ions

    • D. 

      Elements

  • 10. 
    What was important about Rutherford's gold foil experiment?
    • A. 

      Rutherford's team of scientists aimed a beam of positively charged particles at a thin sheet of gold foil. They predicted that the charged particles would pass right through the foil in a straight line. The gold atoms in the foil would not have enough positive charge in any given area to repel the charged particles. The scientists observed that MOST of the particles passed through the foil undisturbed, as expected. A few particles strongly deflected in another direction. Since charges that are alike repel each other, Rutherford inferred that an atom's positive charge must be clustered in a tiny area in its center. Because of this experiment, Rutherford test showed evidence that the beam particles were repelled by the gold atom's center or nucleus.

    • B. 

      Rutherford's team of scientists aimed a beam of negatively charged particles at a thin sheet of gold foil. They predicted that the charged particles would pass right through the foil in a straight line. The gold atoms in the foil would not have enough positive charge in any given area to repel the charged particles. The scientists observed that MOST of the particles passed through the foil undisturbed, as expected. A few particles strongly deflected in another direction. Since charges that are alike repel each other, Rutherford inferred that an atom's negative charge must be clustered in a tiny area in its center. Because of this experiment, Rutherford test showed evidence that the beam particles were repelled by the gold atom's center or nucleus.

    • C. 

      Rutherford's team of scientists aimed a beam of positively charged particles at a thin sheet of gold foil. They predicted that the charged particles would pass right through the foil in a straight line. The gold atoms in the foil would not have enough positive charge in any given area to repel the charged particles. The scientists observed that MOST of the particles passed through the foil undisturbed, as expected. A few particles strongly deflected in another direction. Since charges that are alike repel each other, Rutherford inferred that an atom's positive charge must be clustered in a tiny area in its center. Because of this experiment, Rutherford test showed evidence that the beam particles were repelled by the gold atom's center or valence.

    • D. 

      Rutherford's team of scientists aimed a beam of positively charged particles at a thin sheet of gold foil. They predicted that the negative charged particles would pass right through the foil in a straight line. The gold atoms in the foil would not have enough negative charge in any given area to repel the charged particles. The scientists observed that MOST of the particles passed through the foil undisturbed, as expected. A few particles strongly deflected in another direction. Since charges that are alike repel each other, Rutherford inferred that an atom's positive charge must be clustered in a tiny area in its center. Because of this experiment, Rutherford test showed evidence that the beam particles were repelled by the gold atom's center or nucleus.

  • 11. 
    All the atoms of a single element have the same number of protons. Different elements have different number of _______________
    • A. 

      Protons

    • B. 

      Neutrons

    • C. 

      Electrons

    • D. 

      Nucleus

  • 12. 
    Which of the following is not a mixture?
    • A. 

      Oxygen

    • B. 

      Air

    • C. 

      Soil

    • D. 

      Orange juice

  • 13. 
    Identify which statement is NOT part of John Dalton's atomic theory:
    • A. 

      Atoms have no overall electrical charge because each atom has the same number of electrons as protons.

    • B. 

      All atoms of the same element are exactly alike and have the same mass. Atoms of different elements are different and have different masses.

    • C. 

      An atom of one element cannot be changed into an atom of a different element. Atoms cannot be created or destroyed in any chemical change, only rearranged.

    • D. 

      Every compound is composed of atoms of different elements combined in a specific ratio. 

    • E. 

      All elements are composed of atoms that cannot be divided.

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