Chemical Bonding Basics Practice Worksheet | Practices worksheets ... - Free Printable

To solve this problem, we need to look at each chemical formula and figure out two things:
1. How many atoms of each element are in one molecule (or formula unit).
2. How those atoms connect (bond) to each other.

Here is the step-by-step breakdown for each compound listed in your table.

Step 1: Analyze Silicon Dioxide ($SiO_2$)

* Count the atoms: The formula is $SiO_2$. There is no number after Si, so there is 1 Silicon atom. There is a small '2' after O, so there are 2 Oxygen atoms.
* Bonding: Silicon is in the middle. It needs to share electrons with the two Oxygen atoms to stay together. In a simple diagram, you draw the Si in the center and an O on each side.
* *Diagram idea:* $O - Si - O$

Step 2: Analyze Carbon Dioxide ($CO_2$)

* Count the atoms: The formula is $CO_2$. There is 1 Carbon atom and 2 Oxygen atoms.
* Bonding: Carbon is in the middle. Like silicon dioxide, it connects to the two oxygens.
* *Diagram idea:* $O = C = O$ (Carbon often forms double bonds, but for basic diagrams, just showing them connected in a line $O-C-O$ is often accepted depending on your grade level).

Step 3: Analyze Sodium Bromide ($NaBr$)

* Count the atoms: The formula is $NaBr$. There are no little numbers, so there is 1 Sodium atom and 1 Bromine atom.
* Bonding: This is an ionic bond (metal + non-metal). They stick together in a pair.
* *Diagram idea:* $Na - Br$

Step 4: Analyze Cesium Chloride ($CsCl$)

* Count the atoms: The formula is $CsCl$. There is 1 Cesium atom and 1 Chlorine atom.
* Bonding: Similar to Sodium Bromide, these two stick together.
* *Diagram idea:* $Cs - Cl$

Step 5: Analyze Barium Iodide ($BaI_2$)

* Count the atoms: The formula is $BaI_2$. There is 1 Barium atom. The '2' after the I means there are 2 Iodine atoms.
* Bonding: The Barium is in the middle, holding onto the two Iodines.
* *Diagram idea:* $I - Ba - I$

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Final Answer

Here is the information to fill into your table rows:

1. Silicon dioxide ($SiO_2$)
* Electron-dot diagrams for each atom:
* Si: Symbol Si with 4 dots around it.
* O: Symbol O with 6 dots around it (you will need two of these).
* Rearranged dot diagrams to show bonding:
* Draw Si in the middle. Draw one O on the left and one O on the right. Share pairs of electrons between them so that every atom has 8 dots total around it.

2. Carbon dioxide ($CO_2$)
* Electron-dot diagrams for each atom:
* C: Symbol C with 4 dots around it.
* O: Symbol O with 6 dots around it (you will need two of these).
* Rearranged dot diagrams to show bonding:
* Draw C in the middle. Draw an O on the left and an O on the right. Share two pairs of electrons between C and each O (double bonds) so everyone has 8 dots.

3. Sodium bromide ($NaBr$)
* Electron-dot diagrams for each atom:
* Na: Symbol Na with 1 dot.
* Br: Symbol Br with 7 dots.
* Rearranged dot diagrams to show bonding:
* Move the 1 dot from Na over to Br. Now Na has 0 dots (and usually gets brackets with a + sign) and Br has 8 dots (and usually gets brackets with a - sign). They sit next to each other.

4. Cesium chloride ($CsCl$)
* Electron-dot diagrams for each atom:
* Cs: Symbol Cs with 1 dot.
* Cl: Symbol Cl with 7 dots.
* Rearranged dot diagrams to show bonding:
* Move the 1 dot from Cs over to Cl. Now Cs has 0 dots (brackets with +) and Cl has 8 dots (brackets with -). They sit next to each other.

5. Barium iodide ($BaI_2$)
* Electron-dot diagrams for each atom:
* Ba: Symbol Ba with 2 dots.
* I: Symbol I with 7 dots (you will need two of these).
* Rearranged dot diagrams to show bonding:
* Take 1 dot from Ba and give it to the first Iodine. Take the second dot from Ba and give it to the second Iodine. Now Ba has 0 dots (brackets with 2+), and both Iodines have 8 dots (brackets with -). Arrange them like $[I]^- [Ba]^{2+} [I]^-$.