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CHEMICAL BONDING

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

1. 
Which element has a full outermost energy level containing only two electrons?
a.
oxygen (O)
c.
fluorine (F)
b.
hydrogen (H)
d.
helium (He)
 

2. 
Which of the following describes what happens when an atom becomes an ion with a 2– charge?
a.
The atom gains 2 protons.
c.
The atom gains 2 electrons.
b.
The atom loses 2 protons.
d.
The atom loses 2 electrons.
 

3. 
The properties of ductility and malleability are associated with which type of bonds?
a.
ionic
c.
metallic
b.
covalent
d.
none of the above
 

4. 
In which area of the periodic table do you find elements whose atoms easily gain electrons?
a.
across the top two rows
c.
on the right side
b.
across the bottom row
d.
on the left side
 

5. 
Which pair of atoms can form an ionic bond?
a.
sodium (Na) and potassium (K)
c.
fluorine (F) and chlorine (Cl)
b.
potassium (K) and fluorine (F)
d.
sodium (Na) and neon (Ne)
 

6. 
The number of ____ is most important in determining how an atom will bond.
a.
protons
c.
electrons in the innermost energy level
b.
neutrons
d.
electrons in the outermost energy level
 

7. 
Why do atoms have no charge?
a.
The number of protons is equal to the number of neutrons.
b.
The number of electrons is equal to the number of neutrons.
c.
The number of protons is equal to the number of electrons.
d.
There is an equal number of neutrons, protons, and electrons.
 

8. 
____ are formed by atoms losing electrons.
a.
Negative ions
c.
Elements
b.
Positive ions
d.
Compounds
 

9. 
The number of electrons in an atom can be determined from the ____ of the element.
a.
atomic mass
c.
atomic number
b.
mass number
d.
bonding number
 

10. 
Electrons in an atom are organized
a.
in energy levels.
c.
in chains.
b.
in nuclei.
d.
None of the above
 

11. 
The first energy level is closest to the nucleus and can hold up to ____ electrons.
a.
2
c.
6
b.
4
d.
8
 

12. 
Electrons will enter the second energy level after the ____ electron enters the first energy level.
a.
first
c.
third
b.
second
d.
fourth
 

13. 
The second energy level can hold up to ____ electrons.
a.
2
c.
6
b.
4
d.
8
 

14. 
Most atoms form bonds using only the electrons in their ____ energy level.
a.
innermost
c.
outermost
b.
fullest
d.
first
 

15. 
Atoms of elements in Groups 1 and 2 have ____ their group number.
a.
the same number of valence electrons as
b.
no general rule relating their valence electrons to
c.
10 fewer valence electrons than
d.
None of the above
 

16. 
Atoms of elements in Groups 13–18 have ____their group number.
a.
the same number of valence electrons as
b.
no general rule relating their valence electrons to
c.
10 fewer valence electrons than
d.
None of the above
 

17. 
Oxygen is in Group 16. How many valence electrons does oxygen have?
a.
2
c.
8
b.
6
d.
16
 

18. 
Sodium is in Group 1. How many valence electrons does sodium have?
a.
1
c.
8
b.
2
d.
11
 

19. 
Atoms ____ to have a filled outermost energy level.
a.
split
c.
are attracted to protons in order
b.
bond
d.
None of the above
 

20. 
Atoms bond by ____ electrons.
a.
gaining
c.
sharing
b.
losing
d.
All of the above
 

21. 
The force of attraction between oppositely charged ions is a(n) ____ bond.
a.
atomic
c.
covalent
b.
ionic
d.
metallic
 

22. 
The force of attraction between the nuclei of atoms and the electrons shared by the atoms is a(n) ____ bond.
a.
metallic
c.
covalent
b.
ionic
d.
atomic
 

23. 
The joining of atoms to form new substances is
a.
chemical bonding.
c.
electron bonding.
b.
valence electrons.
d.
None of the above
 

24. 
A molecule is a neutral group of atoms held together by ____ bonds.
a.
atomic
c.
covalent
b.
ionic
d.
metallic
 

25. 
A transfer of electrons between atoms changes the number of electrons in each atom, while the number of protons
a.
decreases.
c.
increases.
b.
stays the same.
d.
None of the above
 



 
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