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NAME _____________________________________
DATE ________
PERIOD ______
Chemistry (Honors)
Atomic Structure (Unit 3)
____
1. An atom is
a. a tiny, indivisible particle
b. the smallest piece of matter
c. the smallest particle of an element that retains the chemical identity of that element
d. an artificially assembled unit that contains protons and electrons
____
2. Dalton’s atomic theory did NOT include the idea that
a. matter is made of small particles called atoms.
b. atoms contain electrons, protons, and neutrons.
c. atoms are neither created nor destroyed in chemical reactions.
d. compounds always contain the same relative numbers and kinds of atoms.
____
3. Rutherford’s scattering experiment indicated that
a. the nucleus of an atom occupies most of an atom’s volume.
b. positive charges are dispersed throughout the atom.
c. positive charges are concentrated in a very small core at the atom’s center surrounded by
empty space.
d. protons and neutrons are located in the nucleus.
____
4. Scientists have determined that electrons
a. move in the space around the nucleus.
b. have a mass equal to the mass of protons.
c. orbit the nucleus in a well-defined path.
d. are electrically neutral.
____
5. Atoms of each element contain a unique number of
a. neutrons in their nuclei
c. electrons in their nuclei
b. protons in their nuclei
d. all of the above.
____
6. Two isotopes of the same element may have different
a. mass numbers and atomic numbers.
b. numbers of protons and numbers of neutrons.
c. mass numbers and numbers of neutrons.
d. chemical properties.
____
7. An atom that consists of 2 protons, 2 neutrons and 2 electrons is
a. the valence shell of an atom
c. the kernel of an atom
b. the nucleus of an atom
d. a neutral atom
____
8. The atomic mass of an element is determined from an atom’s number of
a. electrons
c. protons
b. neutrons
d. protons and neutrons
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____
9. The line emission spectrum of an element (choose all that apply)
a. is a continuous spectrum.
c. can be used to identify elements.
b. is produced when electrons emit light.
d. can distinguish mixtures of elements.
____ 10. Elements produce a unique line spectra because
a. electrons remain in fixed orbits.
b. elements are most stable in their excited
states.
c. electrons release energy at specific
wavelengths.
d. energy is reflected by electrons.
____ 11. Which of the following of Dalton’s Atomic Theory is incorrect?
a. All atoms of a given element are different in their physical and chemical properties.
b. Atoms of different elements have different physical and chemical properties.
c. Atoms combine in whole-number ratios.
d. Chemical reactions are the combination, separation, or rearrangement of atoms.
____ 12. The electrical charges of an atom are located
a. only in the nucleus
b. on protons and neutrons
c. on protons and electrons
d. on protons, neutrons, and electrons
____ 13. Electrons must first be added the lowest energy orbitals available according to
a. Hund’s rule
c. the Pauli Exclusion Principle
b. the Heisenberg Principle
d. the Aufbau Principle
____ 14. An orbital is a region in space where an electron with a particular energy is likely to be found.
a. true
b. false
____ 15. An atom in the ground state
a. is giving off electromagnetic radiation.
c. has all the lowest energy levels occupied.
b. has all the highest energy levels occupied. d. is excited.
____ 16. What did Rutherford’s gold foil experiment discover about atoms?
a. Atoms have multiple energy levels.
b. The nucleus is a solid core that contains protons.
c. Atoms have very little empty space.
d. Electrons and protons are equally mixed in the nucleus.
____ 17. Carbon 14 has more ____________ than Carbon 12.
a. positrons
b. electrons
c. protons
d. neutrons
____ 18. The maximum number of electrons in the valence shell of an atom with 3 principle energy levels is
a. 2
b. 8
c. 18
d. 32
____ 19. The number of orbitals that are found in the 3rd principle energy level is
a. 1
b. 2
c. 4
d. 9
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____ 20. The maximum number of electrons that can occupy an orbital at one time is
a. 1
b. 2
c. 3
d. 4
____ 21. An atom of potassium has 19 protons and 20 neutrons. Its mass number is
a. 19
b. 20
c. 39
d. 10
____ 22.
[Ar]4s23d5 is the Noble gas notation for
a. argon (Ar)
b. manganese (Mn)
c. chromium (Cr)
d. chlorine (Cl)
____ 23. The atomic mass of an atom of carbon is 12, and the atomic mass of an atom of oxygen is 16. To produce
CO, 16g of oxygen can be combined with 12g of carbon. According to the Law of Multiple Proportions, the
ratio of oxygen to carbon when 32g of oxygen combine with 12g of carbon is
a. 1:1
b. 2:1
c. 1:2
d. 8:3
____ 24. According to the Law of Definite Composition, any two samples of KCl will have
a. the same mass.
c. the same melting point.
b. slightly different molecular structures.
d. the same ratio of elements.
____ 25. According to the Law of Definite Proportion
a. the ratio of the masses of the elements in a compound is always the same.
b. the total mass after a chemical change is the same as before.
c. if the same two elements form two different compounds, they do so in the same ratio.
d. it is not possible for the same two elements to form more than one compound.
____ 26. According to the Law of Conservation of Mass, when sodium, hydrogen, and oxygen react to form a
compound, the mass of the compound will be _________ the masses of the individual elements.
a. equal to
c. less than
b. greater than
d. either greater than or less than
Short Answer
27. Write the electron configuration for zinc, 30Zn -2 (WRITE BIG. You’ll be marking up your configuration.)
65
Reference your electron configuration for zinc in #27.
28. Underline the highest principle energy level.
29. Circle the valence electrons.
30. Did Zinc gain electrons or lose electrons? Justify.
________________________________________________________________________________________
31. Draw the orbital notation for Iron 56
26
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Fe +2
#32 Compare the following elements in terms of mass, charge, atomic number, and one
other way of your choice. Justify your comparisons. How do you know?
31 P
15
-2
33 P
15
Alike
Different
3p
2p
3s
1s
2s
33. Which isotope in #32 is represented by the orbital notation? _________________
34. Justify the way in which the orbital diagram supports or breaks Hund’s Rule.
__________________________________________________________________________
__________________________________________________________________________
35. Justify the way in which the orbital diagram above supports or breaks the Pauli Exclusion Principle. Next,
fix the diagram if the rule is broken.
__________________________________________________________________________
__________________________________________________________________________
36. Re-draw the 1s orbital so that it breaks the Aufbau Principle. Write your new orbital over the old one in
the diagram.
37. Phosphorus 31 has an abundance of 92% and Phosphorus 33 has an abundance of 8%. Calculate the average
atomic mass . _______________
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