Sample A:

Solid appearance:crystals, solids, white
Solid Conductivity:no
Solubility: soluble
Solution appearance:substance disappears slowly
Solution Conductivity: yes
Relative melting point:2nd

Sample B:
Solid appearance:brown, tiny solids, dirt appearance
Solid Conductivity: no
Solubility: not soluble
Solution appearance: looks like mud
Solution Conductivity: no
Relative melting point: 4th

Sample C:
Solid appearance: clearish, white, small solid, powder like
Solid Conductivity: no
Solubility: soluble
Solution appearance: white tiny pieces still at the bottom
Solution Conductivity: yes
Relative melting point: 3rd

Sample D:
Solid appearance: Silver, shiny, metallic
Solid Conductivity: yes
Solubility: not soluble
Solution appearance:substance still looks the same as it was before
Solution Conductivity: yes
Relative melting point: 5th

Sample E:
Solid appearance: white, chunks, crystal-like
Solid Conductivity: no
Solubility: not soluble
Solution appearance: chunks are sitting on top of the water
Solution Conductivity: no
Relative melting point: 1st

Classify each solid as non-polar covalent, polar covalent, ionic, network covalent, or metallic and give reasons for your classification based on observations.

Based on the given observations, we can classify each solid as follows:

Sample A:
- Solid Appearance: Crystals, solids, white
- Solubility: Soluble
- Solution Appearance: Substance disappears slowly
- Solution Conductivity: Yes
- Relative Melting Point: 2nd

Classification: Ionic
Reasoning: The solid appears as crystals, indicating a regular repeating pattern. It is soluble and forms a conductive solution, suggesting the presence of ions. The relative melting point is the 2nd, indicating that it requires a relatively high temperature to melt, which is consistent with ionic compounds.

Sample B:
- Solid Appearance: Brown, tiny solids, dirt appearance
- Solubility: Not soluble
- Solution Appearance: Looks like mud
- Solution Conductivity: No
- Relative Melting Point: 4th

Classification: Non-polar covalent
Reasoning: The solid's appearance suggests impurities and does not have a regular crystal structure. It is not soluble and does not form a conductive solution. The high relative melting point (4th) indicates strong covalent bonds, consistent with non-polar covalent compounds.

Sample C:
- Solid Appearance: Clearish, white, small solid, powder-like
- Solubility: Soluble
- Solution Appearance: White tiny pieces still at the bottom
- Solution Conductivity: Yes
- Relative Melting Point: 3rd

Classification: Polar covalent
Reasoning: The solid appears as a powder-like substance and is soluble in water. The solution retains some solid particles at the bottom, indicating incomplete dissolution. It forms a conductive solution, suggesting the presence of ions. The relative melting point (3rd) suggests relatively weaker bonds, characteristic of polar covalent compounds.

Sample D:
- Solid Appearance: Silver, shiny, metallic
- Solid Conductivity: Yes
- Solubility: Not soluble
- Solution Appearance: Substance still looks the same as it was before
- Solution Conductivity: Yes
- Relative Melting Point: 5th

Classification: Metallic
Reasoning: The solid's appearance indicates a metallic luster. It conducts electricity both in the solid state and when dissolved in a solution. It is not soluble, and the solution appearance remains unchanged. The high relative melting point (5th) suggests strong metallic bonding.

Sample E:
- Solid Appearance: White, chunks, crystal-like
- Solid Conductivity: No
- Solubility: Not soluble
- Solution Appearance: Chunks are sitting on top of the water
- Solution Conductivity: No
- Relative Melting Point: 1st

Classification: Network covalent
Reasoning: The solid appears as chunks with a crystal-like structure. It does not conduct electricity in the solid state or when dissolved in a solution. It is not soluble, and the solid chunks float on top of the water. The low relative melting point (1st) indicates weaker bonding, consistent with network covalent compounds.

Based on the given observations, we can classify the solids as follows:

Sample A:
Solid appearance: Crystals, solids, white
Solubility: Soluble
Solution appearance: Substance disappears slowly
Solution Conductivity: Yes
Relative melting point: 2nd

Sample A can be classified as an ionic solid. Ionic solids are characterized by their crystal-like appearance, solubility in water, and the ability to conduct electricity in solution. The fact that the substance disappears slowly in solution and the solution conductivity is positive indicates the presence of ions dissolved in water, which are characteristic of ionic compounds.

Sample B:
Solid appearance: Brown, tiny solids, dirt appearance
Solubility: Not soluble
Solution appearance: Looks like mud
Solution Conductivity: No
Relative melting point: 4th

Sample B can be classified as a non-polar covalent solid. Non-polar covalent solids are usually insoluble in water and do not conduct electricity in any form. The brown color and dirt-like appearance suggest a non-polar covalent compound, such as organic matter or a non-polar molecule, which is typically insoluble and does not dissociate into ions.

Sample C:
Solid appearance: Clearish, white, small solid, powder-like
Solubility: Soluble
Solution appearance: White tiny pieces still at the bottom
Solution Conductivity: Yes
Relative melting point: 3rd

Sample C can be classified as a polar covalent solid. Polar covalent solids have characteristics such as being soluble in water and the ability to conduct electricity in solution. The clearish and white appearance, along with the solubility and positive solution conductivity, suggests the presence of polar molecules that can dissolve in water and form ions, giving it a polar covalent nature.

Sample D:
Solid appearance: Silver, shiny, metallic
Solid Conductivity: Yes
Solubility: Not soluble
Solution appearance: Substance still looks the same as it was before
Solution Conductivity: Yes
Relative melting point: 5th

Sample D can be classified as a metallic solid. Metallic solids exhibit characteristics such as high luster, conductivity of heat and electricity, and high melting points. The silver, shiny appearance, the ability to conduct electricity both in the solid and solution state, and the fact that the substance remains unchanged in solution all point to a metallic solid.

Sample E:
Solid appearance: White, chunks, crystal-like
Solid Conductivity: No
Solubility: Not soluble
Solution appearance: Chunks are sitting on top of the water
Solution Conductivity: No
Relative melting point: 1st

Sample E can be classified as a network covalent solid. Network covalent solids have characteristics such as high melting points, insolubility in water, and lack of conductivity. The white, crystal-like appearance and the fact that the substance does not dissolve or conduct electricity suggest a network covalent solid, which is typically composed of a network of covalent bonds extending throughout the entire structure.