Circle the following elements on the table - Tungsten, Iron, Copper, Antimony, Potassium Put a square box around the group that has 5 valence electrons

Question

Question 1: Put a square box around the period that has 4 electron shells
How many valence electrons do the following elements have?
Sodium: __________ Oxygen: __________ Argon: __________ Magnesium: __________

Question 2: Draw the Lewis Structure and then describe the bonding in H2CNH
Be sure to answer - Are the bonds single, double, tripple? Why does each atom make the number and type of bonds that it does?

Answer 1

Circle the following elements on the table: Tungsten, Iron, Copper, Antimony, Potassium
Square box around the group that has 5 valence electrons: Antimony

Question 1: Square box around the period that has 4 electron shells: Tungsten

Valence electrons:
Sodium: 1
Oxygen: 6
Argon: 8
Magnesium: 2

Question 2:
Lewis Structure of H2CNH:
H - C - N - H

Bonding in H2CNH:
The H2CNH molecule has covalent bonding. Each bond in the molecule is a single bond, including the bonds between H and C, C and N, and N and H.

Each atom in H2CNH makes a specific number and type of bonds due to the following reasons:

- Hydrogen (H): Hydrogen only has one electron and requires one more electron to achieve a stable electron configuration, so it forms one bond with another atom to fulfill this requirement.

- Carbon (C): Carbon has four valence electrons and needs four more electrons to achieve a stable electron configuration. It forms four bonds, one with each hydrogen atom, to fulfill this requirement.

- Nitrogen (N): Nitrogen has five valence electrons and needs three more electrons to achieve a stable electron configuration. It forms one bond with the carbon atom and two bonds with the hydrogen atoms, totaling three bonds.

- Hydrogen (H): The second hydrogen atom behaves the same as the first hydrogen atom, forming one bond with the nitrogen atom to satisfy its requirement for an additional electron to achieve stability.