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 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?
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.
Question 1: To determine which period has 4 electron shells on the periodic table, you should first locate the element with atomic number 36, which is Krypton (Kr). The period that Krypton belongs to is period 4, so you can draw a square box around this period.
Sodium: Sodium (Na) is located in group 1 and period 3. It has 1 valence electron.
Oxygen: Oxygen (O) is located in group 16 and period 2. It has 6 valence electrons.
Argon: Argon (Ar) is located in group 18 and period 3. It has 8 valence electrons.
Magnesium: Magnesium (Mg) is located in group 2 and period 3. It has 2 valence electrons.
Question 2: To draw the Lewis structure for H2CNH, follow these steps:
1. Determine the total number of valence electrons by adding up the valence electrons for each atom: 2 (H) + 4 (C) + 1 (N) + 1 (H) = 8 valence electrons.
2. Place the central atom, which is carbon (C), in the center of the structure.
3. Attach the other atoms to the central carbon atom with single bonds: C-H-N.
4. Distribute the remaining valence electrons around the atoms as lone pairs.
- Hydrogen (H) can only have 2 valence electrons, so it will have a lone pair of electrons.
- Nitrogen (N) has 5 valence electrons, so it will have 3 lone pairs of electrons.
- Carbon (C) has 4 valence electrons, so it will have 2 lone pairs of electrons.
The bonding in H2CNH is as follows:
- There is a single bond between each pair of atoms, so all the bonds (C-H, C-N, and N-H) are single bonds.
- Each atom makes the number and type of bonds it does to achieve a stable electron configuration.
- Hydrogen (H) has only one valence electron and needs 1 more to achieve a stable octet configuration, so it forms one single bond.
- Carbon (C) has 4 valence electrons and needs 4 more to achieve a stable octet configuration, so it forms two single bonds.
- Nitrogen (N) has 5 valence electrons and needs 3 more to achieve a stable octet configuration, so it forms three single bonds.
- Each atom follows the octet rule, which states that atoms tend to gain, lose, or share electrons to achieve a stable electron configuration with 8 valence electrons.
To answer the questions and complete the tasks, let's use the periodic table and the concept of valence electrons.
Question 1: Put a square box around the period that has 4 electron shells.
To identify the period with 4 electron shells, you can count the rows (or periods) on the periodic table. The period with 4 electron shells is the fourth row or period, so put a square box around that period.
Question 2: How many valence electrons do the following elements have?
To determine the number of valence electrons for each element, you can use the periodic table. The group number represents the number of valence electrons for most of the main group elements.
- Sodium (Na) is in Group 1, so it has 1 valence electron.
- Oxygen (O) is in Group 16, so it has 6 valence electrons.
- Argon (Ar) is in Group 18 (noble gases), so it has 8 valence electrons.
- Magnesium (Mg) is in Group 2, so it has 2 valence electrons.
For the next part, we need to draw the Lewis Structure for H2CNH and explain the bonding.
H2CNH Lewis Structure:
To draw the Lewis Structure, we represent the atoms by their symbols and show their valence electrons as dots or crosses around the atomic symbol.
H - C - N - H
Each hydrogen (H) atom has 1 valence electron. Carbon (C) has 4 valence electrons, Nitrogen (N) has 5, and Hydrogen (H) has 1.
To form bonds, atoms typically aim to achieve a full valence shell. In the Lewis Structure for H2CNH, we can see that Carbon (C) forms 4 single bonds. Nitrogen (N) also forms 3 single bonds.
The bonding in H2CNH:
- Each bond in the Lewis Structure of H2CNH is a single bond.
- Carbon (C) forms 4 single bonds because it needs 4 additional electrons to complete its octet (8 valence electrons).
- Nitrogen (N) forms 3 single bonds because it needs 3 additional electrons to complete its octet (8 valence electrons).
- Hydrogen (H) forms 1 single bond with Carbon (C) and Nitrogen (N) to complete its duet (2 valence electrons).
Overall, H2CNH has single bonds, and each atom makes the number and type of bonds it does to achieve a stable electron configuration by either completing its octet or duet.