11.8.10

Announcements- 6 QUIZZES this chapter, Chemthink & Webassign MUST be done before class. We picked up the calender and pages 1-8 in class today.

Homework- Pages 1-8, except 3(most finished in class)

Today in class we learned about covalent bonds. We observed the “potential energy curve” with covalent bonds.




Using a graph like this, we explain that when two atoms are moved far apart to close together the potential energy of the two atoms decrease, making the stability (how stable the atoms are) increase. This would make the electrostatic force a proton-electron attraction meaning that one proton from one atom attracts an electron from the other atom.

When the two atoms move from close together to far apart the potential energy of the two atoms would increase, making the stability (how stable the atoms are) decrease. This would cause a proton-proton repulsion meaning that the protons repel as they get too close to each other.

Next in class we talked about naming covalent bonds. Covalent bonds are ONLY nonmetals. You don’t need to worry about figuring out the charges. When naming the first element NEVER has a mono, but the second one will.

We use these prefixes:
1-mono 2-di 3-tri 4-tetra 5-penta 6-hexa


If the element starts in a vowel and the prefix ends in a vowel take out the prefix vowel, for example Carbon Monoxide.

• Here are a few examples of naming covalent bonds:
CO- Carbon Monoxide
CF3- Carbon Tetrafluoride
N2O3- Dinitrogen Trioxide
AsCl3- Arsenic Trichloride

*Remember to still use –ide at the end of second element





When figuring out if it is an Ionic or Covalent bond look for these:

• Polyatomic Ions (SO4-, NO3-, NH4+, etc.)
• Transition Elements (Cu, Fe, Pb, etc.)
• Metals (Ca, Al, Na, etc.)

Here are some examples on figuring out ionic (I) or covalent (C) bonds and writing the formulas:

• Nitrogen Dioxide C NO3
• Copper(II) Phosphide I Cu3P2
• Sulfur Trioxide C SO3
• Chromium(III) Bromide I CrBr3








Next Scriber- Gennah L