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Chapter 11 - Prep Test

Matching
 
 
Match each item with the correct statement below.
a.
electronegativity
f.
periodic law
b.
ionization energy
g.
cation
c.
atomic radius
h.
period
d.
metal
i.
group
e.
transition metal
j.
electrons
 

 1. 

 horizontal row in the periodic table
 

 2. 

 vertical column in the periodic table
 

 3. 

 A repetition of properties occurs when elements are arranged in order of increasing atomic number.
 

 4. 

 type of element that is a good conductor of heat and electric current
 

 5. 

 type of element characterized by the presence of electrons in the d orbital
 

 6. 

 one-half the distance between the nuclei of two atoms when the atoms are joined
 

 7. 

 type of ion formed by Group 2A elements
 

 8. 

 subatomic particles that are transferred to form positive and negative ions
 

 9. 

 ability of an atom to attract electrons when the atom is in a compound
 

 10. 

 energy required to remove an electron from an atom
 

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

 11. 
Which of the following electron box diagrams correctly represents an atom of carbon?
a.
mc011-1.jpg
c.
mc011-3.jpg
b.
mc011-2.jpg     
d.
mc011-4.jpg
 

 12. 
Which of the following groups of atoms have the same outermost electron configurations but with different n values?
a.
N, O, F, Ne
c.
Ca, Ge, Sr, In
b.
S, Cl, Ar, K
d.
O, S, Se, Te
 

 13. 
Which of the following is NOT a valid electron configuration?
a.
1s22s22p63s23p64s1     
c.
 1s22s22p62d103s23p64s2     
b.
1s22s22p63s23p64s23d5     
d.
 1s22s22p63s23p6
 

 14. 
A student drew the following electron box diagram for an atom of sodium in the ground state.
            mc014-1.jpg
Which of the following statements is true?
a.
The student’s diagram is correct.
b.
The student’s diagram is incorrect because it shows an incorrect number of electron.
c.
The student’s diagram is incorrect because the arrows that represent the electrons should have opposite spins.
d.
The student’s diagram violates the law of conservation of mass.
 

 15. 
For an electron in an atom to change from the ground state to an excited state,
a.
energy must be released.
b.
energy must be absorbed.
c.
radiation must be emitted.
d.
the electron must make a transition from a higher to a lower energy level.
 

 16. 
Bohr's theory helped explain why
a.
electrons have negative charge.
b.
most of the mass of the atom is in the nucleus.
c.
excited hydrogen gas gives off certain colors of light.
d.
atoms combine to form molecules.
 
 
nar001-1.jpg
 

 17. 
According to Bohr, electrons cannot reside at ____ in the figure above.
a.
point A
c.
point C
b.
point B
d.
point D
 

 18. 
A spherical electron cloud surrounding an atomic nucleus would best represent
a.
an s orbital.
c.
a combination of px and py orbitals.
b.
a px orbital.
d.
a combination of an s and a px orbital.
 

 19. 
An orbital that could never exist according to the quantum or wave-mechanical description of the atom is
a.
3d.
c.
6d.
b.
8s.
d.
1p.
 

 20. 
The letter designations for the first four sublevels with the number of electrons that can be accommodated in each sublevel are
a.
s:1, p:3, d:10, and f:14.
c.
s:2, p:6, d:10, and f:14.
b.
s:1, p:3, d:5, and f:7.
d.
s:1, p:2, d:3, and f:4.
 

 21. 
The number of orbitals for the d sublevel is
a.
1.
c.
5.
b.
3.
d.
7.
 

 22. 
The atomic sublevel with the next highest energy after 4p is
a.
4d.
c.
5p.
b.
4f.
d.
5s.
 

 23. 
In the ground state, the 3d and 4s sublevels of the chromium atom (atomic number 24) may be represented as
a.
3d6 4s1.
c.
3d5 4s1.
b.
3d4 4s2.
d.
4s2 3d4.
 

 24. 
If the s and p orbitals of the highest main energy level of an atom are filled with electrons, the atom has a(n)
a.
electron pair.
c.
ellipsoid.
b.
octet.
d.
circle.
 

 25. 
The number of electrons in the highest energy level of the argon atom (atomic number 18) is
a.
10.
c.
6.
b.
2.
d.
8.
 

 26. 
In the Bohr model of the atom, an electron in an orbit has a fixed ____.
a.
position
c.
energy
b.
color
d.
size
 

 27. 
How does the energy of an electron change when the electron moves closer to the nucleus?
a.
It decreases.
c.
It stays the same.
b.
It increases.
d.
It doubles.
 

 28. 
What is the shape of the 3p atomic orbital?
a.
sphere
c.
bar
b.
dumbbell
d.
two perpendicular dumbbells
 

 29. 
The shape (not the size) of an electron cloud is determined by the electron's ____.
a.
energy sublevel (s, p, d, & f)
c.
speed
b.
diet
d.
principal quantum number
 

 30. 
How are the frequency and wavelength of light related?
a.
They are inversely proportional to each other.
b.
Frequency equals wavelength divided by the speed of light.
c.
Wavelength is determined by dividing frequency by the speed of light.
d.
They are directly proportional to each other.
 

 31. 
The atomic emission spectra of a sodium atom on Earth and of a sodium atom in the sun would be ____.
a.
the same
b.
different from each other
c.
the same as those of several other elements
d.
the same as each other only in the ultraviolet range
 

 32. 
Which of the following electron configurations is most likely to result in an element that is relatively inactive?
a.
a half-filled energy sublevel
b.
a filled energy sublevel
c.
one empty and one filled energy sublevel
d.
a filled highest occupied principal energy level
 

 33. 
Write the ground-state electron conguration of a lead atom.
a.
[Xe] 4f14 5d5 6s1 6p6 7s2
c.
[Xe] 4f14 5d10 6s1 6p3
b.
[Xe] 4f14 5d10 6s2 6p2
d.
[Xe] 4f14 5d10 6p4
 

 34. 
Which of the following subshells CANNOT exist in an atom?
a.
2p
c.
4f
b.
4d
d.
3f
 

 35. 
In a given atom, how many electrons can occupy the 3d set of orbitals?
a.
2
c.
10
b.
6
d.
14
 

 36. 
Which of the following is the correct orbital notation for the element oxygen (O, atomic #8)?
a.
mc036-1.jpg
c.
mc036-3.jpg
b.
mc036-2.jpg
d.
mc036-4.jpg
 

 37. 
The energy required to remove an electron from an atom is the atom's
a.
electron affinity.
c.
electronegativity.
b.
electron energy.
d.
ionization energy.
 

 38. 
The element that has the greatest electronegativity is
a.
oxygen.
c.
chlorine.
b.
sodium.
d.
fluorine.
 

 39. 
In a row/period in the periodic table, as you move across and as the atomic number increases, the atomic radius generally
a.
decreases.
c.
increases.
b.
remains constant.
d.
becomes unmeasurable.
 

 40. 
In the alkaline-earth group, atoms with the smallest radii
a.
are the most reactive.
c.
are all gases.
b.
have the largest volume.
d.
have the highest ionization energies.
 

 41. 
As you move down the periodic table from carbon through lead, atomic radii
a.
generally increase.
c.
do not change.
b.
generally decrease.
d.
vary unpredictably.
 

 42. 
Electrons are elevated from the ground state to the excited state by: 
a.
the absorption of energy
c.
the release of energy
b.
the loss of mass
d.
 the destruction of energy
 

 43. 
When a salt such as sodium chloride is exposed to a flame, the visible light given off is the result of:   
a.
ground state electrons moving to higher energy levels
c.
excited electrons returning to the ground state
b.
nuclear decay
d.
gamma radiation
 
 
nar002-1.jpg
 

 44. 
Given the representation of a chlorine atom, which circle might a chloride ion, Cl-? 
a.
Circle D
c.
Circle B
b.
Circle C
d.
None of these
 

 45. 
Cations have a ______________ charge and are ______________ than the atoms from which they formed.
a.
positive/larger
c.
negative/larger
b.
 negative/smaller
d.
positive/smaller
 

 46. 
What element has the noble-gas notation [Ne]3s23p5?
a.
Chlorine
c.
Sulfur
b.
Neon
d.
Oxygen
 

 47. 
mc047-1.jpg
The "up" and "down" arrows in electron orbital notation, such as is shown here, depict:
a.
electrons and protons attracting each other
c.
 protons and neutrons in orbitals
b.
oppositely charged electrons
d.
electrons with opposite spins
 

 48. 
The elements on the modern periodic table are organized by increasing:
a.
atomic number
c.
ionization energy
b.
 atomic mass
d.
 size
 

 49. 
The elements of the Noble Gas family, except for Helium, have an outer shell of:
a.
6 electrons
c.
2 electrons
b.
8 electrons
d.
18 electrons
 

 

 50. 
Which element is predicted to have the ground-state electron conguration [He] 2s2?
 a.
beryllium
 c.
 boron
 b.
lithium
 d.
carbon
 



 
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