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Bond Type Practice
The concept of electronegativity was introduced by Linus Pauling in 1932, and
this became very useful in explaining the nature of bonds between atoms in
molecules. For this work, Pauling was awarded the Nobel Prize in Chemistry in
1954. He also received the Nobel Peace Prize in 1962 for his campaign against
above-ground nuclear testing.
The greater the electronegativity of an atom of an element, the stronger its
attractive pull on electrons. For example, in a molecule of hydrogen bromide
(
), the electronegativity of bromine (2.8) is higher than that of hydrogen (2.1),
and so the shared electrons will spend more of their time closer to the bromine
atom. Bromine will have a slightly negative charge, and hydrogen will have a
slightly positive charge. In a molecule like hydrogen ( ) where the
electronegativities of the atoms in the molecule are the same, both atoms have
a neutral charge.
Part A Directions: Determine the type of bond that will form between each pair of atoms in the
table below. Use the Electronegativity Chart and Bond Type Chart to help you.
Bond Type
Atom 1
Atom 2
Arsenic
Sulfur
Cobalt
Bromine
Electronegativity
Difference (∆EN)
(Nonpolar Covalent (NPC), Moderately
Polar Covalent (MPC), Very Polar Covalent
(VPC), or Ionic (I))
Germanium Selenium
Silicon
Fluorine
Potassium
Nitrogen
Nickel
Oxygen
Barium
Tin
Hydrogen
Oxygen
Calcium
Sulfur
Iron
Carbon
Part B Directions: Draw the Lewis Dot Structure for each compound below. Then, label each bond
as either nonpolar covalent (NPC), moderately polar covalent (MPC), very polar covalent (VPC), or
ionic (I).
11. H2O
13. CO2
12. NaCl
14. PF3
Part C Directions: Determine what elements would form each of the 4 bond types with the elements
given.
Element
15. Boron
I
VPC
MPC
NPC
Fluorine
Oxygen
Sulfur
Phosphorus
16. Calcium
17. Sulfur