GENERAL DIRECTIONS: CHOOSE THE BEST ANSWER FROM THE SUGGESTED OPTIONS AND WRITE THE LETTER OF YOUR CHOICE ON THE ANSWER SHEET.
1. Which of the following is different from others?
Covalent bonding C. Metallic bonding
B. Ionic bonding D. Hydrogen bonding
2. Which one of the following pair of molecules or species is not isoelectronic pair?
A. CO and N2 B. NH3 and H3O+ C. N2 and CN- D. CO2 and SO2
3. Which covalent molecule contains more number of total valance electrons than the others?
A. SO4 -2 B. NH4+ C. N2O4 D. CO2
4. Which of the following is the correct Lewis Structure for oxygen atom?
A. The three lone-pairs of valance electrons.
B. One lone-pair of valance electrons and one bonding site.
C. Two lone-pair of valance electrons and one bonding site.
D. Two lone-pair of valance electrons and two bonding site.
5. Which of the statement below best explains why atoms react chemically with each other?
A. When atoms react, they gain protons and are more stable
B. When atoms react, they lose all their electrons and become more stable
C. When atoms react, they lose, gain, or share electrons and are then less stable
D. When atoms react, they lose, gain, or share electrons to attain a full outer energy level and
are then more stable.
6. The force that holds different atoms or ions together are called?
A. Electrical force B. Physical bonding C. Chemical bonding D. Atomic force
7. Which of the following substances contains an atom that obey the octet rule?
A. PCl3 B. AlF3 C. SF4 D. NO2
8. How many unpaired electrons are there in the Lewis structure of an N 3- ion?
A.0 B. 1 C. 2 D.3
9. "Two atoms each provide two electrons that are shared by the two atoms" This is a description of a
A. Triple covalent bond C. Double covalent bond
B. Coordinate covalent bond D. Single covalent bond
10. Which of the following compounds contain both ionic and covalent bonds?
A. CO2 B. Na2O C. NH4Cl D. BaCl2
11. Inert gases do not react with any other element because
A. The temperature is not high enough
B. Their outermost electron level is filled with 8 electrons
C. Their nucleus is very small
D. The systems pressure is not enough
12. Which of the following has a dipole moment?
A. CCl4 B. NH3 C. CS2 D. BF3
13. If you provided with four covalent compounds namely naphthalene, graphite, iodine and ethanol to investigate their electrical conductivity, which one would you expect to conduct electricity either in the solid or in the liquid state?
A. Graphite B. Ethanol C. Naphthalene D. Iodine
14. Which of the following ionic compounds has the greatest lattice energy?
A. CsI B. LiI C. NaI D. KI
15. How many π bonds are present in HCN?
A. One B. Two C. Three D. Four
16. The amount of sigma and pi bonds present in benzene (C6H6) molecule is
A. 12 sigma and 3 pi bond C.18 sigma and 6 pi bond
B. 3 sigma and 12 pi bond D.6 pi and 18 sigma bond
17. Which of the following solid substance contains positive ions immersed in a sea of mobile
electrons?
A.O2 B. Cu C. CuO D.SiO2
18. Which one of the following molecules has not T-shape molecular geometry?
A. H2O B, BrCl3 C. ICl3 D. ClF3
19. Which one of the following usually produces the weakest interaction between particles of
similar molar mass?
A. Van der Waals forces C. Covalent bonds
B. Dipole-dipole forces D. Hydrogen-bonding
20. All of the following have the same molecular shape except one. Identify it.
A. CHCl3 B. NH3 C. PH4+ D. CH4
21. Which of the following statements concerning the length of carbon –carbon single, double
& Triple bond is true?
A. Carbon - carbon single bond is shorter than either double or triple bond
B. The carbon – carbon double bond is shorter than either single or triple bond
C. The carbon –carbon triple bond is shorter that either carbon – carbon single or double bond
D. The carbon – carbon single, double and triple bond all have the same length
22. Which of the following best describes the formation of pi (π) bonds?
A. They are formed by the sideways overlap of parallel orbitals.
B. They are formed by the axial overlap of orbitals.
C. They are formed by the sideways overlap of an s and p orbitals.
D. They are formed by the axial overlap of either s or p orbitals.
23. The type of orbital overlap for the formation of SF6 compounds?
A. sp3d-p overlap B. sp3d2- p overlap C. sp3-p overlap D. sp2-p overlap
24. The bond order and magnetic nature of nitrogen molecule are:
A. 2, diamagnetic C. 2, paramagnetic
B. 3, diamagnetic D. 3.paramagnetic
25. For which molecules or molecule ion, the number of electron in bonding molecular orbital’s equals to the number of electrons in anti-bonding molecular orbitals?
A. O2 B. N2 C. C2 D.Be2
26. Which of the following is the basic chemical bonding theory?
A. Covalent Bond Theory B. Molecular Bond Theory
C. Valance Shell Electron Pair Repulsion (VSEPR) Theory D. Ionic Bonding Theory
27. Why are metals soft and malleable?
A. Because they are very shiny
B. Because of the presence of mobile electrons
C. B/c they experience electrostatic repulsion
D. Because the metal cations can slip over each other fairly easily
1. D. Hydrogen bonding
2. A. CO and N2
3. A. SO4 -2
4. D. Two lone-pair of valance electrons and two bonding site
5. D. When atoms react, they lose, gain, or share electrons to attain a full outer energy level and are then more stable
6. C. Chemical bonding
7. B. AlF3
8. A.0
9. A. Triple covalent bond
10. C. NH4Cl
11. B. Their outermost electron level is filled with 8 electrons
12. B. NH3
13. A. Graphite
14. A. CsI
15. B. Two
16. C.18 sigma and 6 pi bond
17. B. Cu
18. A. H2O
19. A. Van der Waals forces
20. C. PH4+
21. C. The carbon –carbon triple bond is shorter that either carbon – carbon single or double bond
22. A. They are formed by the sideways overlap of parallel orbitals.
23. B. sp3d2- p overlap
24. D. 3. paramagnetic
25. B. N2
26. A. Covalent Bond Theory
27. B. Because of the presence of mobile electrons