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Chemistry 12 - Unit 2 Quiz



True/False
Indicate whether the sentence or statement is true or false.
 

1. 

The term “orbital” refers to the path or trajectory an electron follows as it orbits a nucleus.
 

2. 

The configuration [Ne] 2s2 2p1 represents an aluminum atom in its lowest energy state.
 

3. 

Rutherford knew that alpha particles were small and massive, and when moving fast should act much as bullets do when striking a target. He expected them to punch through his foil target and be slowed enough to let him determine the density of the atoms in the foil.
 

4. 

Light passed through a flame may have certain frequencies absorbed, because ions in the gas have electrons jump from lower energy levels to higher energy levels.
 

5. 

The ground state electron configuration for all alkali metals shows that the highest energy electrons are in a p sublevel.
 

6. 

There are thought to be seven d energy sublevels.
 

7. 

Spectra from atoms larger than hydrogen do not follow simple “rules” because when an atom has multiple electrons they repel each other and interfere with each other’s orbital.
 

8. 

Schrödinger became famous by predicting that the particles called electrons might behave like waves under certain conditions, and then demonstrating this experimentally.
 

9. 

The aufbau principle states that when electron configurations are written, the lower energy levels must be filled before the higher levels.
 

10. 

VSEPR theory predicts that a sulfate ion, SO42–, should be tetrahedral in shape.
 

11. 

VSEPR theory predicts that a central atom with three bonded atoms and one lone pair of electrons should have a trigonal planar shape.
 

12. 

A hydrogen bond is a particularly strong intermolecular bond existing between a hydrogen on one molecule and a lone pair of electrons on another molecule.
 

13. 

VSEPR and Lewis theories are not complete enough to explain the structure and shape of the molecules in gaseous uranium hexafluoride, UF6(g), which is used in uranium nuclear fuel-enriching processes.
 

14. 

VSEPR and Lewis theories are not complete enough to explain the structure and shape of the molecules in gaseous silane, SiH4(g), which is used as a doping agent in the manufacture of semiconductors for solid-state devices.
 

15. 

A molecule with tetrahedral shape and all bonds equally polar will be nonpolar, overall.
 

16. 

A three-atom molecule with linear shape and two identical atoms attached to the central atom will always be nonpolar.
 

17. 

Metallic bonding involves 3-D structures with vacant valence orbitals and mobile valence electrons.
 

18. 

Ionic bonding involves 3-D structures with vacant valence orbitals and mobile valence electrons.
 

19. 

Silver normally forms a 1+ ion, indicating that normally only one electron occupies its highest energy level.
 

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

20. 

The atomic structure that did not follow directly from Rutherford’s experiments is the idea of the
a.
electron.
b.
proton.
c.
neutron.
d.
nucleus.
e.
“empty” electron.
 

21. 

Observing a frequency of light emitted by a hot gas will also allow prediction of a frequency that this same gas will absorb, when cool, according to theory advanced by
a.
Rutherford.
b.
Bohr.
c.
Planck.
d.
Heisenberg.
e.
Chadwick.
 

22. 

The concept of atomic structure contributed by Niels Bohr is that
a.
atoms can absorb and release only specific frequencies of electromagnetic radiation.
b.
protons are extremely close together in a tiny part of the atomic volume.
c.
electrons can have only certain specific different levels of energy.
d.
electrons orbit a nucleus like tiny planets orbiting a star.
e.
uncharged particles exist in the nucleus.
 

23. 

The biggest flaw in Bohr’s theory was that it
a.
did not be applied to atoms larger than hydrogen.
b.
predicted electrons would slow and spiral into the nucleus.
c.
did not explain blackbody radiation.
d.
predicted that protons in nuclei would repel and fly apart.
e.
ignored the structure of the nucleus.
 

24. 

An energy-level diagram for fluorine would show the highest level of energy for
a.
7 electrons.
b.
9 electrons.
c.
10 electrons.
d.
18 electrons.
e.
19 electrons.
 

25. 

The major differences in electron energy levels are described by the
a.
principal quantum number, n .
b.
secondary quantum number, l .
c.
magnetic quantum number, ml .
d.
spin quantum number, ms .
e.
exclusion principle.
 

26. 

The concept that electrons are oriented along different axes in 3-dimensional space is described by the
a.
principal quantum number, n .
b.
secondary quantum number, l .
c.
magnetic quantum number, ml .
d.
spin quantum number, ms .
e.
electron configuration.
 

27. 

The evidence that all substances are attracted or repelled by a magnetic field is described by the
a.
principal quantum number, n .
b.
secondary quantum number, l .
c.
magnetic quantum number, ml .
d.
spin quantum number, ms .
e.
electron configuration.
 

28. 

The electron configuration of a chlorine atom in its lowest energy state is
a.
1s2 2s2 2p6 3s2 3p6.
b.
1s2 2s2 2p6 3s2 3p5.
c.
1s2 2s2 2p6 3s1
d.
1s2 2s2 2p6.
e.
1s2 2s2 2p5.
 

29. 

The electron configuration of a calcium ion in its lowest energy state is
a.
1s2 2s2 2p6 3s2 3p6 4s2.
b.
1s2 2s2 2p6 3s2 3p6 4s1.
c.
1s2 2s2 2p6 3s2 3p4 4s2.
d.
1s2 2s2 2p6 3s2 3p6.
e.
1s2 2s2 2p6 3s1 3p5.
 

30. 

The electron configuration that could be a fluoride ion in an “excited”  energy state is
a.
1s2 2s2 2p5.
b.
1s2 2s2 2p4 3s14s1.
c.
1s2 2s2 2p6.
d.
1s2 2s2 2p5 3s14s1.
e.
1s2 2s2 2p6 3s13p1.
 

31. 

The idea of special stability due to the presence of a stable octet of electrons is central to
a.
Kekulé line diagrams.
b.
Bohr atomic structure.
c.
VSEPR molecular shape prediction.
d.
Pauling hybrid orbitals.
e.
Lewis dot diagrams.
 

32. 

The Lewis symbol of a calcium ion would show dots to represent
a.
0 electrons.
b.
2 electrons.
c.
10 electrons.
d.
18 electrons.
e.
20 electrons.
 

33. 

The Lewis symbol of a magnesium atom would show dots to represent
a.
0 electrons.
b.
2 electrons.
c.
8 electrons.
d.
10 electrons.
e.
12 electrons.
 

34. 

A Lewis symbol for an atom with a most stable electron configuration of 1s2 2s2 2p6 3s2 3p6 4s2 would show
a.
2 unpaired electrons and 2 electron pairs.
b.
1 unpaired electron and 3 electron pairs.
c.
2 unpaired electrons.
d.
1 electron pair.
e.
1 electron.
 

35. 

A Lewis symbol for a negative ion with a configuration of 1s2 2s2 2p6 would show
a.
3 unpaired electrons and 2 electron pairs.
b.
1 unpaired electron and 3 electron pairs.
c.
2 unpaired electrons and 3 electron pairs.
d.
no electrons, either single or paired.
e.
4 electron pairs.
 

36. 

A Lewis structure for the sulfur dichloride molecule, SCl2, would show
a.
3 electron pairs.
b.
4 electron pairs.
c.
10 electron pairs.
d.
12 electron pairs.
e.
18 electron pairs
 

37. 

A Lewis structure for the hydroxide ion, OH, would show
a.
3 electron pairs.
b.
4 electron pairs.
c.
7 electron pairs.
d.
10 electron pairs.
e.
12 electron pairs.
 

38. 

The molecule in the following list that has a linear shape, according to VSEPR theory, is
a.
H2O.
b.
OF2.
c.
CO2.
d.
H2O2.
e.
CH3COOH
 

39. 

The hydrogen bonding of large molecules is a very important area of study in biochemistry. A hydrogen bond can only form at a location on a large molecule where a hydrogen atom is bonded either to an oxygen atom, or to
a.
a nitrogen atom.
b.
a chlorine atom.
c.
a fluorine atom.
d.
a sulfur atom.
e.
another hydrogen atom.
 

40. 

The atoms of hard, brittle substances with high melting points have essentially all of their atoms joined in a network of
a.
ceramic bonds
b.
coordinate bonds
c.
metallic bonds
d.
covalent bonds
e.
hydrogen bonds.
 



 
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