Bond Type Practice
Describe the following bond types and tell what type of element(s) are involved:
Non-polar Covalent
Ionic
Metallic
Polar Covalent
Electronegativities
Carbon = 2.5
Cesium = 0.7
Chromium = 1.6
Fluorine = 4.0
Hydrogen = 2.1
Iodine = 2.5
Iron = 1.8
Magnesium = 1.2
Molybdenum = 1.8
Oxygen = 3.5
Phosphorus = 2.1
Silicon = 1.8
Sodium = 0.9
Sulfur = 2.5
Barium = 0.9
Bromine = 2.8
Chlorine = 3.0
Lead = 1.8
Iodine = 2.5
Determine the type of bond (ionic, polar/nonpolar covalent, metallic). If it is polar covalent, determine where
the dipoles would be. If it is ionic, denote which would be the positive and negative ions.
BaF2
CuPb
HBr
PH3
SiH4
HCl
CH4
SiO2
Au
CCl4
SiCl4
PbI
Bond Type Practice (Key)
Describe the following bond types and tell what type of element(s) are involved:
Non-polar Covalent
Electrons are shared between the two atoms evenly
Ionic
Electrons are transferred from one atom to another, creating positive and negative ions that attract each
other
Metallic
A sea of electrons, electrons are shared between all atoms in the piece of metal
Polar Covalent
Electrons are shared, but not shared evenly, so one atom becomes partially negative (negative dipole) and
the other partially positive (positive dipole)
Electronegativities
Carbon = 2.5
Cesium = 0.7
Chromium = 1.6
Fluorine = 4.0
Hydrogen = 2.1
Iodine = 2.5
Iron = 1.8
Magnesium = 1.2
Molybdenum = 1.8
Oxygen = 3.5
Phosphorus = 2.1
Silicon = 1.8
Sodium = 0.9
Sulfur = 2.5
Barium = 0.9
Bromine = 2.8
Chlorine = 3.0
Lead = 1.8
Iodine = 2.5
Determine the type of bond (ionic, polar/nonpolar covalent, metallic). If it is polar covalent, determine where
the dipoles would be. If it is ionic, denote which would be the positive and negative ions.
BaF2
Ionic
Ba+2, FSiH4
Non-polar
Au
Metallic
CuPb
Metallic
HCl
Polar
+----
CCl4
Polar
+--
HBr
Polar
+---
CH4
Polar
---+
SiCl4
Polar
+--
PH3
Non-polar
SiO2
Ionic
Si+4, O-2
PbI
Polar
+--