Chemistry Chapter 6B (Prentice)
 
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Chemistry Chapter 6B (Prentice)

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. 

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

 2. 

 type of ion formed by Group 2A elements
 

 3. 

 subatomic particles that are transferred to form positive and negative ions
 

 4. 

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

 5. 

 energy required to remove an electron from an atom
 

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

 6. 
What element in the second period has the largest atomic radius?
a.
carbon
c.
potassium
b.
lithium
d.
neon
 

 7. 
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
 

 8. 
Which of the following elements has the smallest atomic radius?
a.
sulfur
c.
selenium
b.
chlorine
d.
bromine
 

 9. 
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.
 

 10. 
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.
 

 11. 
The metals in Groups 1A, 2A, and 3A ____.
a.
gain electrons when they form ions
c.
all have ions with a 1mc011-1.jpg charge
b.
all form ions with a negative charge
d.
lose electrons when they form ions
 

 12. 
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.
 

 13. 
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.
 

 14. 
In which of the following sets are the charges given correctly for all the ions?
a.
Namc014-1.jpg, Mgmc014-2.jpg, Almc014-3.jpg
c.
Rbmc014-7.jpg, Bamc014-8.jpg, Pmc014-9.jpg
b.
Kmc014-4.jpg, Srmc014-5.jpg, Omc014-6.jpg
d.
Nmc014-10.jpg, Omc014-11.jpg, Fmc014-12.jpg
 

 15. 
In which of the following groups of ions are the charges all shown correctly?
a.
Limc015-1.jpg, Omc015-2.jpg, Smc015-3.jpg
c.
Kmc015-7.jpg, Fmc015-8.jpg, Mgmc015-9.jpg
b.
Camc015-4.jpg, Almc015-5.jpg, Brmc015-6.jpg
d.
Namc015-10.jpg, Imc015-11.jpg, Rbmc015-12.jpg
 

 16. 
What is the element with the lowest electronegativity value?
a.
cesium
c.
calcium
b.
helium
d.
fluorine
 

 17. 
What is the element with the highest electronegativity value?
a.
cesium
c.
calcium
b.
helium
d.
fluorine
 

 18. 
Which of the following elements has the smallest ionic radius?
a.
Li
c.
O
b.
K
d.
S
 

 19. 
What is the energy required to remove an electron from an atom in the gaseous state called?
a.
nuclear energy
c.
shielding energy
b.
ionization energy
d.
electronegative energy
 

 20. 
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.
 

 21. 
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
 

 22. 
Which of the following elements has the smallest first ionization energy?
a.
sodium
c.
potassium
b.
calcium
d.
magnesium
 

 23. 
Which of the following elements has the lowest electronegativity?
a.
lithium
c.
bromine
b.
carbon
d.
fluorine
 

 24. 
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.
 

 25. 
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
 

 26. 
Which of the following decreases with increasing atomic number in Group 2A?
a.
shielding effect
c.
ionization energy
b.
ionic size
d.
number of electrons
 

 27. 
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.
 

 28. 
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
 

 29. 
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
 

 30. 
Of the following elements, which one has the smallest first ionization energy?
a.
boron
c.
aluminum
b.
carbon
d.
silicon
 



 
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