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Chapter 6 Study Guide


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

 1. 
What is another name for the representative elements?
a.
Group A elements
b.
Group B elements
c.
Group C elements
d.
transition elements
 

 2. 
What is another name for the transition metals?
a.
noble gases
b.
Group A elements
c.
Group B elements
d.
Group C elements
 

 3. 
Which of the following elements is in the same period as phosphorus?
a.
carbon
b.
magnesium
c.
nitrogen
d.
oxygen
 

 4. 
Who arranged the elements according to atomic mass and used the arrangement to predict the properties of missing elements?
a.
Henry Moseley
b.
Antoine Lavoisier
c.
John Dalton
d.
Dmitri Mendeleev
 

 5. 
Which of the following categories includes the majority of the elements?
a.
metalloids
b.
liquids
c.
metals
d.
nonmetals
 

 6. 
Of the elements Pt, V, Li, and Kr, which is a nonmetal?
a.
Pt
b.
V
c.
Li
d.
Kr
 

 7. 
In which of the following sets is the symbol of the element, the number of protons, and the number of electrons given correctly?
a.
In, 49 protons, 49 electrons
b.
Zn, 30 protons, 60 electrons
c.
Cs, 55 protons, 132.9 electrons
d.
F, 19 protons, 19 electrons
 

 8. 
The atomic number of an element is the total number of which particles in the nucleus?
a.
neutrons
b.
protons
c.
electrons
d.
protons and electrons
 

 9. 
What element has the electron configuration 1smc009-1.jpg2smc009-2.jpg2pmc009-3.jpg3smc009-4.jpg3pmc009-5.jpg?
a.
nitrogen
b.
selenium
c.
silicon
d.
silver
 

 10. 
Which of the following is true about the electron configurations of the noble gases?
a.
The highest occupied s and p sublevels are completely filled.
b.
The highest occupied s and p sublevels are partially filled.
c.
The electrons with the highest energy are in a d sublevel.
d.
The electrons with the highest energy are in an f sublevel.
 

 11. 
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
 

 12. 
Which of the following elements is a transition metal?
a.
cesium
b.
copper
c.
tellurium
d.
tin
 

 13. 
Which of the following groupings contains only representative elements?
a.
Cu, Co, Cd
b.
Ni, Fe, Zn
c.
Al, Mg, Li
d.
Hg, Cr, Ag
 

 14. 
Which of the following is true about the electron configurations of the representative elements?
a.
The highest occupied s and p sublevels are completely filled.
b.
The highest occupied s and p sublevels are partially filled.
c.
The electrons with the highest energy are in a d sublevel.
d.
The electrons with the highest energy are in an f sublevel.
 

 15. 
What are the Group 1A and Group 7A elements examples of?
a.
representative elements
b.
transition elements
c.
noble gases
d.
nonmetallic elements
 

 16. 
Of the elements Fe, Hg, U, and Te, which is a representative element?
a.
Fe
b.
Hg
c.
U
d.
Te
 

 17. 
How does atomic radius change from top to bottom in a group in the periodic table?
a.
It tends to decrease.
b.
It tends to increase.
c.
It first increases, then decreases.
d.
It first decreases, then increases.
 

 18. 
How does atomic radius change from left to right across a period in the periodic table?
a.
It tends to decrease.
b.
It tends to increase.
c.
It first increases, then decreases.
d.
It first decreases, then increases.
 

 19. 
Atomic size generally ____.
a.
increases as you move from left to right across a period
b.
decreases as you move from top to bottom within a group
c.
remains constant within a period
d.
decreases as you move from left to right across a period
 

 20. 
What element in the second period has the largest atomic radius?
a.
carbon
b.
lithium
c.
potassium
d.
neon
 

 21. 
Which of the following factors contributes to the increase in atomic size within a group in the periodic table as the atomic number increases?
a.
an increase in number of occupied energy levels
b.
an increase in size of the nucleus
c.
an increase in number of protons
d.
fewer electrons in the highest occupied energy level
 

 22. 
Which of the following elements has the smallest atomic radius?
a.
chlorine
b.
bromine
c.
sulfur
d.
selenium
 

 23. 
What is the charge of a cation?
a.
a positive charge
b.
no charge
c.
a negative charge
d.
The charge depends on the size of the nucleus.
 

 24. 
Which of the following statements is true about ions?
a.
Cations form when an atom gains electrons.
b.
Cations form when an atom loses electrons.
c.
Anions form when an atom gains protons.
d.
Anions form when an atom loses protons.
 

 25. 
The metals in Groups 1A, 2A, and 3A ____.
a.
gain electrons when they form ions
b.
all form ions with a negative charge
c.
all have ions with a 1mc025-1.jpg charge
d.
lose electrons when they form ions
 

 26. 
Why is the second ionization energy greater than the first ionization energy?
a.
It is more difficult to remove a second electron from an atom.
b.
The size of atoms increases down a group.
c.
The size of anions decreases across a period.
d.
The nuclear attraction from protons in the nucleus decreases.
 

 27. 
In which of the following sets are the charges given correctly for all the ions?
a.
Namc027-1.jpg, Mgmc027-2.jpg, Almc027-3.jpg
b.
Kmc027-4.jpg, Srmc027-5.jpg, Omc027-6.jpg
c.
Rbmc027-7.jpg, Bamc027-8.jpg, Pmc027-9.jpg
d.
Nmc027-10.jpg, Omc027-11.jpg, Fmc027-12.jpg
 

 28. 
In which of the following groups of ions are the charges all shown correctly?
a.
Limc028-1.jpg, Omc028-2.jpg, Smc028-3.jpg
b.
Camc028-4.jpg, Almc028-5.jpg, Brmc028-6.jpg
c.
Kmc028-7.jpg, Fmc028-8.jpg, Mgmc028-9.jpg
d.
Namc028-10.jpg, Imc028-11.jpg, Rbmc028-12.jpg
 

 29. 
What is the element with the lowest electronegativity value?
a.
cesium
b.
helium
c.
calcium
d.
fluorine
 

 30. 
What is the element with the highest electronegativity value?
a.
cesium
b.
helium
c.
calcium
d.
fluorine
 

 31. 
Which of the following elements has the smallest ionic radius?
a.
Li
b.
K
c.
O
d.
S
 

 32. 
For Group 2A metals, which electron is the most difficult to remove?
a.
the first
b.
the second
c.
the third
d.
All the electrons are equally difficult to remove.
 

 33. 
Which of the following factors contributes to the decrease in ionization energy within a group in the periodic table as the atomic number increases?
a.
increase in atomic size
b.
increase in size of the nucleus
c.
increase in number of protons
d.
fewer electrons in the highest occupied energy level
 

 34. 
Which of the following elements has the smallest first ionization energy?
a.
sodium
b.
calcium
c.
potassium
d.
magnesium
 

 35. 
Which of the following elements has the lowest electronegativity?
a.
lithium
b.
carbon
c.
bromine
d.
fluorine
 

 36. 
Which statement is true about electronegativity?
a.
Electronegativity is the ability of an anion to attract another anion.
b.
Electronegativity generally increases as you move from top to bottom within a group.
c.
Electronegativity generally is higher for metals than for nonmetals.
d.
Electronegativity generally increases from left to right across a period.
 

 37. 
Which of the following statements correctly compares the relative size of an ion to its neutral atom?
a.
The radius of an anion is greater than the radius of its neutral atom.
b.
The radius of an anion is identical to the radius of its neutral atom.
c.
The radius of a cation is greater than the radius of its neutral atom.
d.
The radius of a cation is identical to the radius of its neutral atom.
 

 38. 
Which of the following factors contributes to the increase in ionization energy from left to right across a period?
a.
an increase in the shielding effect
b.
an increase in the size of the nucleus
c.
an increase in the number of protons
d.
fewer electrons in the highest occupied energy level
 

 39. 
As you move from left to right across the second period of the periodic table ____.
a.
ionization energy increases
b.
atomic radii increase
c.
electronegativity decreases
d.
atomic mass decreases
 

 40. 
Of the following elements, which one has the smallest first ionization energy?
a.
boron
b.
carbon
c.
aluminum
d.
silicon
 



 
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