Question

1. choose the best answer.

which of these represents an atoms tendency to bond in order to fill its valence shell?
electron dot notation
molecular geometry
vsepr theory
octet rule

1. choose the best answer.

which structure has 2 double bonds?
si₂o₂
si₃o₂
sio₂
sio

Explanation:

Question 8

• Electron dot notation: Represents valence electrons of an atom, not about bonding to fill valence shell.
• Molecular geometry: Deals with the 3D arrangement of atoms in a molecule, not about bonding tendency to fill valence shell.
• VSEPR Theory: Predicts molecular geometry based on electron pairs, not about filling valence shell through bonding.
• Octet rule: States that atoms tend to bond to achieve a stable electron configuration (usually 8 valence electrons), which matches the description of an atom’s tendency to bond to fill its valence shell.

Step1: Analyze the valence electrons and bonding for each compound.

• For \( \text{Si}_2\text{O}_2 \): Let's consider the valence electrons. Si has 4 valence electrons, O has 6. The structure of \( \text{Si}_2\text{O}_2 \) (disilicon dioxide) can be thought of as having a structure where each Si is bonded to O. But let's check the other options.
• For \( \text{Si}_3\text{O}_2 \): Unlikely to have a stable structure with this formula as the valence electron distribution would be odd.
• For \( \text{SiO}_2 \): In silicon dioxide, each Si is bonded to 4 O atoms (single bonds in a network, no double bonds).
• For \( \text{SiO} \): Let's look at \( \text{Si}_2\text{O}_2 \) (which is equivalent to \( 2\text{SiO} \) but as a dimer). Wait, actually, the correct approach is to calculate the number of bonds. Let's consider the Lewis structure. For \( \text{Si}_2\text{O}_2 \), the Lewis structure can be drawn as \( \text{O}=\text{Si}-\text{Si}=\text{O} \), which has 2 double bonds (between O and Si on each end).

Step2: Confirm the double bonds.

In \( \text{Si}_2\text{O}_2 \), the structure has two \( \text{Si}=\text{O} \) double bonds.

Answer:

D. octet rule

Question 9