CHEM 219 MODULE 1 PROFESSIONAL
EXAM REVIEW WITH TESTED QUESTIONS
AND EXPERT SOLUTIONS
◉ Explain how bonds are formed between atoms from the
perspective of atomic orbital theory.
Answer: Atoms form bonds by overlapping individual atomic
orbitals from each atom to produce molecular (bonding) orbitals.
◉ Explain the two types of atomic orbital overlap that contribute
to bond formation in organic molecules.
Answer: End-on overlap of atomic orbitals leads to the formation
of sigma (single) covalent bonds. Sideways overlap of P orbitals
leads to the formation of pi (multiple) covalent bonds.
◉ Using the VSEPR method, predict the molecular geometry
(shape and bond angle) around the indicated atoms for the
following structure:
a) C(I)
b) C(II)
c) N
d) S
Answer: a) C(I) = 4 bond pairs = TETRAHEDRAL, 109.5°
b) C(II) = 3 bond pairs = TRIGONAL PLANAR, 120°
, c) N = 3 bond pairs/1 lone pair = TRIGONAL PYRAMIDAL, 107°
d) S = 2 bond pairs/2 lone pairs = ANGULAR/BENT, 105°
◉ Catenation
Answer: The process or preference of an element to link/bond
with another atom of the same element.
◉ Ionic bond
Answer: ***the complete transfer of one or more valence
electrons from one atom to another
- electronegativity diff > 1.8 (large)
◉ (Pure) Covalent bonds
Answer: ***formed by the sharing of electrons
- electronegativity diff: < 0.4 (zero difference)
◉ Diatomic element
Answer: When an atom is more stable when bonded to another
atom
◉ Pure covalent bond
Answer: ***A bond that forms between atoms of identical
electronegativity values. (aka shared electrons)
- electronegativity diff < 0.4 (zero)
EXAM REVIEW WITH TESTED QUESTIONS
AND EXPERT SOLUTIONS
◉ Explain how bonds are formed between atoms from the
perspective of atomic orbital theory.
Answer: Atoms form bonds by overlapping individual atomic
orbitals from each atom to produce molecular (bonding) orbitals.
◉ Explain the two types of atomic orbital overlap that contribute
to bond formation in organic molecules.
Answer: End-on overlap of atomic orbitals leads to the formation
of sigma (single) covalent bonds. Sideways overlap of P orbitals
leads to the formation of pi (multiple) covalent bonds.
◉ Using the VSEPR method, predict the molecular geometry
(shape and bond angle) around the indicated atoms for the
following structure:
a) C(I)
b) C(II)
c) N
d) S
Answer: a) C(I) = 4 bond pairs = TETRAHEDRAL, 109.5°
b) C(II) = 3 bond pairs = TRIGONAL PLANAR, 120°
, c) N = 3 bond pairs/1 lone pair = TRIGONAL PYRAMIDAL, 107°
d) S = 2 bond pairs/2 lone pairs = ANGULAR/BENT, 105°
◉ Catenation
Answer: The process or preference of an element to link/bond
with another atom of the same element.
◉ Ionic bond
Answer: ***the complete transfer of one or more valence
electrons from one atom to another
- electronegativity diff > 1.8 (large)
◉ (Pure) Covalent bonds
Answer: ***formed by the sharing of electrons
- electronegativity diff: < 0.4 (zero difference)
◉ Diatomic element
Answer: When an atom is more stable when bonded to another
atom
◉ Pure covalent bond
Answer: ***A bond that forms between atoms of identical
electronegativity values. (aka shared electrons)
- electronegativity diff < 0.4 (zero)
