Colorado State University-Fort Collins
CHEM 103 chapter 2 and 3 Exams (Final exam review)
Mastery Guide Octet Rule Ionic Covalent Bonding
Electronegativity Periodic Trends Valence Electrons
VSEPR Molecular Geometry Bond Angles Polarity
Electron Groups Linear Trigonal Planar Tetrahedral
Trigonal Bipyramidal Octahedral Square Pyramidal
Square Planar Lone Pairs Halogens Cations Anions
Electron Sharing Exam Questions Verified and Provided
with Complete A+ Graded Answers Latest Updated 2026
1. According to the octet rule, a magnesium atom has a tendency to
A. lose one electron.
B. lose two electrons.
C. gain one electron.
B. lose two electrons.
2. Which of the following pairs of elements can be joined by a covalent bond?
A. N and C
B. Na and C
C. Mg and C
A. N and C
,3. Which of the following is an ionic compound?
A. CO B. HCl C. Na2O
C. Na2O
4. According to periodic trends, which element is the most electronegative?
A. Ne B. O C. F
C. F
5. According to the octet rule, which of elements will have a tendency to loss 2 electrons?
A. strontium B. oxygen C. cesium
A. strontium
6. How do the molecular shapes of the molecules IF5 and PF5 differ?
A. In IF5 there is a lone pair of electrons on iodine where as in PF5 there are no lone pairs on
phosphorus. As a result, the molecular shape of IF5 is square pyramidal and PF5 is trigonal
bipyramidal.
B. In PF5 there is a lone pair of electrons on phosphorus where as in IF5 there are no lone
pairs on iodine. As a result, the molecular shape of PF5 is square pyramidal and IF5 is trigonal
bipyramidal.
C. In IF5 there is a lone pair of electrons on iodine where as in PF5 there are no lone pairs on
phosphorus. As a result, the molecular shape of IF5 is octahedral and PF5 is trigonal
bipyramidal.
A. In IF5 there is a lone pair of electrons on iodine where as in PF5 there are no lone pairs on
phosphorus. As a result, the molecular shape of IF5 is square pyramidal and PF5 is trigonal
bipyramidal.
, 7. In the molecule PF5 what are the bond angles of the fluorine's in the structure?
A. 90° B. 120° C. 109.5°
A. 90°
8. Using VSEPR theory, predict the molecule shape of a molecule that contains 2 electron
groups.
A. trigonal planar B. linear C. bent
B. linear
9. Using VSEPR theory, predict the electron group geometry, molecular shape, and the bond
angles in a molecule that contains 5 electron groups (2 bonds and 3 lone pair electrons).
A. trigonal bipyramidal, linear, 180°
B. trigonal bipyramidal, trigonal bipyramidal, 90° and 120°
C. trigonal bipyramidal, trigonal bipyramidal, 180°
A. trigonal bipyramidal, linear, 180°
10. Using VSEPR theory, predict the electron group geometry, molecular shape, and the bond
angles in a molecule that contains 6 electron groups (5 bonds and 1 lone pair electrons).
A. octahedral, octahedral, 90°
B. octahedral, square planar, 90°
C. octahedral, square pyramidal, 90°
C. octahedral, square pyramidal, 90°
CHEM 103 chapter 2 and 3 Exams (Final exam review)
Mastery Guide Octet Rule Ionic Covalent Bonding
Electronegativity Periodic Trends Valence Electrons
VSEPR Molecular Geometry Bond Angles Polarity
Electron Groups Linear Trigonal Planar Tetrahedral
Trigonal Bipyramidal Octahedral Square Pyramidal
Square Planar Lone Pairs Halogens Cations Anions
Electron Sharing Exam Questions Verified and Provided
with Complete A+ Graded Answers Latest Updated 2026
1. According to the octet rule, a magnesium atom has a tendency to
A. lose one electron.
B. lose two electrons.
C. gain one electron.
B. lose two electrons.
2. Which of the following pairs of elements can be joined by a covalent bond?
A. N and C
B. Na and C
C. Mg and C
A. N and C
,3. Which of the following is an ionic compound?
A. CO B. HCl C. Na2O
C. Na2O
4. According to periodic trends, which element is the most electronegative?
A. Ne B. O C. F
C. F
5. According to the octet rule, which of elements will have a tendency to loss 2 electrons?
A. strontium B. oxygen C. cesium
A. strontium
6. How do the molecular shapes of the molecules IF5 and PF5 differ?
A. In IF5 there is a lone pair of electrons on iodine where as in PF5 there are no lone pairs on
phosphorus. As a result, the molecular shape of IF5 is square pyramidal and PF5 is trigonal
bipyramidal.
B. In PF5 there is a lone pair of electrons on phosphorus where as in IF5 there are no lone
pairs on iodine. As a result, the molecular shape of PF5 is square pyramidal and IF5 is trigonal
bipyramidal.
C. In IF5 there is a lone pair of electrons on iodine where as in PF5 there are no lone pairs on
phosphorus. As a result, the molecular shape of IF5 is octahedral and PF5 is trigonal
bipyramidal.
A. In IF5 there is a lone pair of electrons on iodine where as in PF5 there are no lone pairs on
phosphorus. As a result, the molecular shape of IF5 is square pyramidal and PF5 is trigonal
bipyramidal.
, 7. In the molecule PF5 what are the bond angles of the fluorine's in the structure?
A. 90° B. 120° C. 109.5°
A. 90°
8. Using VSEPR theory, predict the molecule shape of a molecule that contains 2 electron
groups.
A. trigonal planar B. linear C. bent
B. linear
9. Using VSEPR theory, predict the electron group geometry, molecular shape, and the bond
angles in a molecule that contains 5 electron groups (2 bonds and 3 lone pair electrons).
A. trigonal bipyramidal, linear, 180°
B. trigonal bipyramidal, trigonal bipyramidal, 90° and 120°
C. trigonal bipyramidal, trigonal bipyramidal, 180°
A. trigonal bipyramidal, linear, 180°
10. Using VSEPR theory, predict the electron group geometry, molecular shape, and the bond
angles in a molecule that contains 6 electron groups (5 bonds and 1 lone pair electrons).
A. octahedral, octahedral, 90°
B. octahedral, square planar, 90°
C. octahedral, square pyramidal, 90°
C. octahedral, square pyramidal, 90°
