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IB Topic 3 Practice

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

 1. 
What is the maximum number of electrons in the second principal energy level?
a.
2
c.
18
b.
8
d.
32
 

 2. 
What types of atomic orbitals are in the third principal energy level?
a.
s and p only
c.
s, p, and d only
b.
p and d only
d.
s, p, d, and f
 

 3. 
What is the electron configuration of potassium?
a.
1smc003-1.jpg2smc003-2.jpg2pmc003-3.jpg3smc003-4.jpg3pmc003-5.jpg4smc003-6.jpg
c.
1smc003-12.jpg2smc003-13.jpg3smc003-14.jpg3pmc003-15.jpg3dmc003-16.jpg
b.
1smc003-7.jpg2smc003-8.jpg2pmc003-9.jpg3smc003-10.jpg3pmc003-11.jpg
d.
1smc003-17.jpg2smc003-18.jpg2pmc003-19.jpg3smc003-20.jpg3pmc003-21.jpg4smc003-22.jpg
 

 4. 
How does the speed of visible light compare with the speed of gamma rays, when both speeds are measured in a vacuum?
a.
The speed of visible light is greater.
b.
The speed of gamma rays is greater.
c.
The speeds are the same.
d.
No answer can be determined from the information given.
 

 5. 
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
 

 6. 
Each period in the periodic table corresponds to ____.
a.
a principal energy level
c.
an orbital
b.
an energy sublevel
d.
a suborbital
 

 7. 
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.
 

 8. 
Which subatomic particle plays the greatest part in determining the properties of an element?
a.
proton
c.
neutron
b.
electron
d.
none of the above
 

 9. 
How does atomic radius change from top to bottom in a group in the periodic table?
a.
It tends to decrease.
c.
It first increases, then decreases.
b.
It tends to increase.
d.
It first decreases, then increases.
 

 10. 
What causes the shielding effect to remain constant across a period?
a.
Electrons are added to the same principal energy level.
b.
Electrons are added to different principal energy levels.
c.
The charge on the nucleus is constant.
d.
The atomic radius increases.
 

 11. 
What is the element with the lowest electronegativity value?
a.
cesium
c.
calcium
b.
helium
d.
fluorine
 

 12. 
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
 

 13. 
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.
more shielding of the electrons by the highest occupied energy level
b.
an increase in size of the nucleus
c.
an increase in number of protons
d.
fewer electrons in the highest occupied energy level
 

 14. 
Which of the following statements is NOT true about ions?
a.
Cations are positively charged ions.
b.
Anions are common among nonmetals.
c.
Charges for ions are written as numbers followed by a plus or minus sign.
d.
When a cation forms, more electrons are transferred to it.
 

 15. 
Which of the following elements has the smallest ionic radius?
a.
Li
c.
O
b.
K
d.
S
 

 16. 
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.
 

 17. 
Which of the following elements has the smallest first ionization energy?
a.
sodium
c.
potassium
b.
calcium
d.
magnesium
 

 18. 
Compared with the electronegativities of the elements on the left side of a period, the electronegativities of the elements on the right side of the same period tend to be ____.
a.
lower
c.
the same
b.
higher
d.
unpredictable
 

 19. 
As you move from left to right across the second period of the periodic table ____.
a.
ionization energy increases
c.
electronegativity decreases
b.
atomic radii increase
d.
atomic mass decreases
 

Short Answer
 

 20. 
Which group of elements in the periodic table is known as the alkali metals?
 

 21. 
An element has an atomic number of 80. How many protons and electrons are in an atom of the element?
 

 22. 
From which orbital in a lithium atom is an electron transferred to form Lisa022-1.jpg?
 

Numeric Response
 

 23. 
How many electrons are there in the highest occupied energy level of atoms in Group 5A elements?

 

Essay
 

 24. 
Explain how ions form. Provide examples.
 

 25. 
Describe the trends in electronegativity within groups and across periods in the periodic table. Provide examples.
 



 
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