1.      How many electrons are in a triple bond? 2.      All elements want to reach octet, which means they want valence electrons to be stable except for hydrogen, helium, phosphorous, sulfur, boron and beryllium.

3.      Draw the electron configuration and write the ion that has 7 electrons.

4.      Answer the following questions using the compound CN-.

a.      Calculate the total number of valence electrons.

b.      Draw the Lewis structure.

c.      Determine the bond angle.

d.      Determine the molecular geometry (shape).

5.      Why does an element gain or lose electrons?

6.      What is a cation and an anion? State the charges that the cation and anion would have.

7.      If an ion has a -3 charge this means that the atom 3 electrons.

8.      Explain why a Cl- atom is bigger in size than a Cl atom?

9.      What type of bond does a dipole moment occur in and why? Then draw the dipole moment in HF (include the partial charges and arrow).

10.  What type of bond is in KBr based on the type of elements. Explain your answer. Then explain if the electrons are shared or transferred.

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the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.