Thursday, February 24

Today we began the class by looking at Wednesday's blog. From there we proceeded to review ionic compounds, which was discussed on Wednesdays. We recapped on the difference between ionic, Polar, and Non-Polar bonds. We were also given the answers from the previous days homework, Pg. 3 of the packet.

1.a.- 1 b.-2

c.-6 d.-7 f.-3

2.a- [Ne] 3s1 & it loses 1 electron

b.-[Ne] 3s2 3p4 & it gains 2 electrons

c.-[Ar]4s2 & it loses 2 electrons

d.-[Ar] 4s2 3d10 4p5 & it gains 1 electron

We then began to discuss covalent bonds and the Lewis dot structure. From last nights homework we all know that every element wants to gain or lose electrons so that it has 8 valence electrons (2 in the case of H and He). That is why noble gases are so stable. In an ionic bond, one atom will gain electron wh

ile another atom loses an electron. (ex: in NaCl, sodium gives up 1 electron to chlorine, so that both elements have 8 valence electrons). However sometimes, 2 atoms will form covalent bonds and each element will share atom. To begin diagramming a covalent bond, you have to be able to Lewis Dot structure any given

element given the number of electrons.

For example, if you have Cl, you know it has 7 valence electrons.

Step 1: write Cl

Step 2: place 1 dot around Cl for every electron

-it should look like

Now if you wish to write a covalent, you:

1. begin by drawing the Lewis Dot Structure for each element

2. remove 1 electron and draw an electron to represent a pair

3. it should look like this

Each pair of dots can be represented by a dash. As you can see, the H and Cl are each sharing a dot so that H has 2 valence electrons and Cl has 8. They are both stable.

HW:

Webassign