Chemistry Chapters 3 & 4: Matter
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- 1.What did Dalton's atomic theory of matter state?
- 2.Is neither created nor destroyed, only changed. What is it and what states this?
- A.
Matter; Law of Matter
- B.
Mass; Law of Conservation of Mass
- C.
Matter; Law of Conservation of Matter
- D.
Mass; Law of Constitution of Mass
- 3.We measure elements and compounds by their...
- A.
Ratios of mass
- B.
Ratios of matter
- C.
Average Atomic Mass
- D.
EM Waves
- 4.What states: The elements that compose the compounds are always in a certain proportion by mass.
- A.
Law of conservation of elements
- B.
Law of conservation of compounds
- C.
Law of definite proportions
- D.
Law of indefinite proportions
- 5.Who proposed his atomic theory of matter in 1803?
- 6.Atoms of the element that are chemically alike but differ in mass. (Same element, different number of neutrons.)
- 7.The sum of the protons and the neutrons=
- 8.EM Waves include:
- A.
Energy
- B.
Sound
- C.
Light
- D.
TV
- E.
Microwave
- F.
Speed
- 9.Order of electrons in the main four energy levels:
- A.
1st=2; 2nd=4; 3rd=8; 4th=10
- B.
1st-1; 2nd-5; 3rd-15; 4th-31
- C.
1st-2; 2nd-8; 3rd-16; 4th-30
- D.
1st-2; 2nd-8; 3rd-18; 4th-32
- 10.Electrons in the outermost energy level.
- 11.The magic number in chemistry is....
- 12.Uses dots to represent valence electrons: A ______ ____ Diagram
- 13.Choose the correct way to calculate atomic mass:
- A.
Mass contribution*mass of isotope=abundance
- B.
Mass contribution=mass of isotope*abundance
- C.
Mass contribution*abundance=mass of isotope
- 14.The average atomic mass is the sum of the...
- A.
Mass contributions of each isotope.
- B.
Mass of each isotope.
- C.
Abundance of each isotope.
- D.
Mass contributions and abundance of each isotope.
- 15.Chemical or physical: You CANNOT reverse it.
- 16.The Law of Definite proportions is measured by:
- A.
Ratio of Mass
- B.
Proportions of Mass
- C.
Percent by Mass
- D.
Proportions of Matter
- 17.mass of element ______________ x 100 = ? mass of compound
- 18.States the different masses of one element combine with the same relative masses of another element to form a different compound.
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