Question

Consider the hypothetical elements A and X.

Element A has 4 valence electrons.
Element X has 6 valence electrons.
Use the Lewis Symbols of A and X to draw the Lewis Diagram of imaginary compound AX2
What is the molecular geometry of this compound? I need the drawn Lewis diagram
O Tetrahedral
Trigonal Planar
Trigonal Pyramidal
Bent 109
Bent 120
Linear

Answer 1

The molecular geometry of this compound is Trigonal planar. Hence, option B is correct.

Sure, here is the Lewis diagram of AX2:

A:

.

.

X--A--X

.

.

The molecular geometry of AX2 is trigonal planar. This is because the central atom A has 3 bonding electron pairs and 0 lone pairs around it. The three bonding electron pairs repel each other and try to get as far apart as possible, resulting in a trigonal planar geometry.

Here are the possible molecular geometries with 3 bonding electron pairs and 0, 1, or 2 lone pairs:

* **0 lone pairs:** Trigonal planar

* **1 lone pair:** Bent

* **2 lone pairs:** Trigonal pyramidal

In the case of AX2, there are no lone pairs on the central atom A, so the molecular geometry is trigonal planar.

Here are the answer choices with the corresponding molecular geometry:

| Answer Choice | Molecular Geometry |

| a. Tetrahedral | Not applicable |

| b. Trigonal Planar | Yes |

| c. Trigonal Pyramidal | No |

| d. Bent 109° | No |

| e. Bent 120° | No |

| f. Linear | No |

Therefore, the correct answer is b. Trigonal Planar.