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ELECTRON ARRANGEMENT AND PERIODIC TABLE


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

1. 
The idea of arranging the elements in the periodic table according to their chemical and physical properties is attributed to
a.
Mendeleev.
c.
Bohr.
b.
Moseley.
d.
Ramsay.
 

2. 
Mendeleev noticed that properties of elements usually repeated at regular intervals when the elements were arranged in order of increasing
a.
atomic number.
c.
reactivity.
b.
density.
d.
atomic mass.
 

3. 
Moseley's work led to the realization that elements with similar properties occurred at regular intervals when the elements were arranged in order of increasing
a.
atomic mass.
c.
radioactivity.
b.
density.
d.
atomic number.
 

4. 
Argon, krypton, and xenon are
a.
alkaline earth metals.
c.
actinides.
b.
noble gases.
d.
lanthanides.
 

5. 
The periodic law states that the physical and chemical properties of elements are periodic functions of their atomic
a.
masses.
c.
radii.
b.
numbers.
d.
structures.
 

6. 
In Period 3 there are 8 elements. What sublevel(s) is (are) being filled?
a.
s
c.
s and p
b.
s and d
d.
d and f
 

7. 
Within the p-block elements, the elements at the top of the table, compared with those at the bottom,
a.
have larger radii.
c.
have lower ionization energies.
b.
are more metallic.
d.
are less metallic.
 

8. 
Which orbitals are characteristic of the lanthanide elements?
a.
d orbitals
c.
f orbitals
b.
s orbitals
d.
p orbitals
 

9. 
The most reactive group of the nonmetals are the
a.
lanthanides.
c.
halogens.
b.
transition elements.
d.
rare-earth elements.
 

10. 
Which represents a neutral atom acquiring an electron in an exothermic process?
a.
A + e– + energy ® A–
c.
A + e– ® A– + energy
b.
A + e– ® A– – energy
d.
A– + energy ® A + e–
 

11. 
A measure of the ability of an atom in a chemical compound to attract electrons is called
a.
electron affinity.
c.
electronegativity.
b.
electron configuration.
d.
ionization potential.
 

12. 
Ionization energy is the energy required to remove ____ from an atom of an element.
a.
the electron cloud
c.
an electron
b.
the nucleus
d.
an ion
 

13. 
The force of attraction by Group 1 metals for their valence electrons is
a.
weak.
b.
zero.
c.
strong.
d.
greater than that for inner shell electrons.
 

14. 
Which response includes all the following that are properties of most metals, and no other properties?
I.   They tend to form cations.
II.  They are good heat insulators.
III. They have outer electronic shells that contain more than four
     electrons.
IV.  They tend to form ionic compounds when they combine with the
     elements of Group VIIA.
a.
I, II, and III
c.
III and IV 
b.
II, III, and IV
d.
I and IV
 

15. 
Which of the following statements is false?
a.
The effective nuclear charge experienced by an electron in an outer shell is less than the actual nuclear charge
c.
Electrons in inner shells screen, or shield, electrons in outer shells from the full effect of the nuclear charge.
b.
Within a family (vertical group in the periodic table) of representative elements atomic radii increase from top to bottom.
d.
Transition elements have larger atomic radii than the preceding IA and IIA elements in the same period because transition elements have electrons in their d orbitals.
 

16. 
Arrange the following elements in order of increasing atomic radii.
                      K, Na, Mg, Cs, Cl
a.
Na < Mg < Cl < K < Cs
c.
Cs < K < Cl < Mg < Na
b.
Cl < Mg < Na < K < Cs
d.
Cl < Mg < Cs < K < Na
 

17. 
Arrange the following elements in order of increasing first ionization energy.
                     Mg, Al, Si, P, S
a.
Al < Mg < Si < S < P
c.
Al < Mg < Si < P < S
b.
Mg < Al < Si < P < S
d.
Mg < Al < Si < S < P
 

18. 
Consider the group of ions that are isoelectronic with krypton. Which response contains all the true statements and no others?
I.   The ion with the highest positive charge is the largest ion.
II.  The ion with the highest atomic number bears the highest positive
     charge.
III. The ion with the lowest atomic number bears the least negative
     charge.
IV.  The ion with a 1+ charge is obtained by adding one electron to a
     Group VIIA element.
V.   All the ions have a noble gas electronic configuration.
a.
II and III
c.
II, IV, and V
b.
I, II, and V
d.
I and IV
 

19. 
Which of the following statements is true regarding sodium and potassium?
a.
Sodium has a larger first ionization energy and a larger atomic radius
c.
Sodium has a smaller first ionization energy and a larger atomic radius
b.
Sodium has a larger first ionization energy and a smaller atomic radius
d.
Sodium has a smaller first ionization energy and a smaller atomic radius.
 

20. 
For the following atoms the order of increasing electron affinity is:
a.
Br < Rb < Cl < I
c.
Rb < I < Br < Cl
b.
I < Rb < Cl < Br
d.
Cl < Br < Rb < I
 

21. 
With the quantum model of the atom, scientists have come to believe that determining an electron's exact location around the nucleus
a.
is impossible.
b.
can be done before 2005.
c.
can be done easily.
d.
can be done only with specialized equipment.
 

22. 
All of the following describe the Heisenberg uncertainly principle EXCEPT
a.
it states that it is impossible to determine simultaneously both the position and velocity of an electron or any other particle.
b.
it is one of the fundamental principles of our present understanding of light and matter.
c.
it helped lay the foundation for the modern quantum theory.
d.
it helps to locate an electron in an atom.
 

23. 
All of the following describe the Schrödinger wave equation EXCEPT
a.
it is an equation that treats electrons in atoms as waves.
b.
only waves of specific energies and frequencies provide solutions to the equation.
c.
it helped lay the foundation for the modern quantum theory.
d.
it is similar to Bohr's theory.
 

24. 
The solutions to the Schrödinger wave equation are
a.
quantum numbers.
c.
energy levels.
b.
wave functions.
d.
orbitals.
 

25. 
A three-dimensional region around a nucleus where an electron may be found is called a(n)
a.
spectral line.
c.
orbital.
b.
electron path.
d.
orbit.
 

26. 
Unlike in an orbit, in an orbital
a.
an electron's position cannot be known precisely.
b.
an electron has no energy.
c.
electrons cannot be found.
d.
protons cannot be found.
 

27. 
An electron for which n = 4 has more ____ than an electron for which n = 2.
a.
spin
c.
energy
b.
stability
d.
wave nature
 

28. 
The set of orbitals that are dumbbell-shaped and directed along the x, y, and z axes are called
a.
d orbitals.
c.
f orbitals.
b.
p orbitals.
d.
s orbitals.
 

29. 
An orbital that could never exist according to the quantum description of the atom is
a.
3d.
c.
6d.
b.
8s.
d.
3f.
 

30. 
For n = 4, the number of possible orbital shapes is
a.
1.
c.
16.
b.
4.
d.
32.
 

31. 
A single orbital in the 3d level can hold ____ electrons.
a.
10
c.
3
b.
2
d.
6
 

32. 
The statement that an electron occupies the lowest available energy orbital is
a.
Hund's rule.
c.
Bohr's law.
b.
the Aufbau principle.
d.
the Pauli exclusion principle.
 

33. 
"Orbitals of equal energy are each occupied by one electron before any is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin" is a statement of
a.
the Pauli exclusion principle.
c.
the quantum effect.
b.
the Aufbau principle.
d.
Hund's rule.
 

34. 
In the electron configuration for scandium (atomic number 21), what is the notation for the three highest-energy electrons?
a.
3d1 4s2
c.
3d3
b.
4s3
d.
4s2 4p1
 

35. 
The element with electron configuration 1s2 2s2 2p6 3s2 3p2 is
a.
Mg (Z = 12).
c.
S (Z = 16).
b.
C (Z = 6).
d.
Si (Z = 14).
 

36. 
The electron notation for aluminum (atomic number 13) is
a.
1s2 2s2 2p3 3s2 3p3 3d1.
c.
1s2 2s2 2p6 3s2 3p1.
b.
1s2 2s2 2p6 3s2 2d1.
d.
1s2 2s2 2p9.
 

Problem
 
 
electron_arrangemen_files/i0390000.jpg
 

37. 
Use the figure above. Which element has the following electron configuration: [Ar] 4s2 3d10 4p5?
 

38. 
Use the figure above. Which element has the following electron configuration: [Kr] 5s2 4d10 5p3?
 

39. 
Use the figure above and the symbols for the noble gases to write the electron configuration for silicon.
 
 
electron_arrangemen_files/i0430000.jpg
 

40. 
What element's orbital diagram is shown in the figure above?
 



 
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