which of the following indicates whether the solid substance represented by the particulate diagram shown above conducts electricity and explains why or why not?
a it conducts electricity because it is made of positive and negative particles.
b it conducts electricity because electrons are free to move through the substance.
c it does not conduct electricity because electrons are strongly attracted to specific positive particles.
d it does not conduct electricity because the positive particles are not free to move through the substance.

Question

which of the following indicates whether the solid substance represented by the particulate diagram shown above conducts electricity and explains why or why not?
a  it conducts electricity because it is made of positive and negative particles.
b  it conducts electricity because electrons are free to move through the substance.
c  it does not conduct electricity because electrons are strongly attracted to specific positive particles.
d  it does not conduct electricity because the positive particles are not free to move through the substance.

Accepted Answer

# Brief Explanations:
To determine if the solid conducts electricity, we analyze the particulate diagram (likely an ionic solid or a metal? Wait, the diagram has positive ions and electrons. Wait, no—wait, in ionic solids, ions are fixed, but in metals, electrons are delocalized. Wait, the diagram shows positive ions (maybe metal cations) and electrons. But wait, the options: Let's recall electrical conductivity in solids. For a solid to conduct electricity, charge carriers (electrons or ions) must be free to move.

- Option A: Just having positive and negative particles isn't enough (e.g., ionic solids have ions but they're fixed in solid state, so A is wrong).
- Option B: If electrons are free to move, it conducts. But wait, in the diagram, are electrons free? Wait, maybe the solid is an ionic solid? Wait, no—wait, the diagram: positive ions and electrons? Wait, maybe it's a metal? Wait, no, the options: Let's check each option.

Wait, the diagram: positive ions (maybe cations) and electrons. But in a solid ionic compound, ions are fixed, and electrons are associated with ions (not free). Wait, maybe the solid is a metal? No, the options: Let's re-examine.

Wait, the key is: in a solid, for conductivity, charge carriers must be mobile.

- Option C: Says it does not conduct because electrons are strongly attracted to specific positive particles (like in an ionic solid, where electrons are in bonds, not free; or in a covalent network, but here positive ions and electrons—maybe it's an ionic solid? Wait, ionic solids have ions (positive and negative), but in solid state, ions are fixed. Wait, the diagram has positive ions and electrons (maybe the negative particles are electrons? Wait, no—negative particles in ionic solids are anions. Wait, maybe the diagram is of a metal? No, metals have positive ions and delocalized electrons (free to move). But option B says electrons are free to move, so it conducts. But wait, the correct answer? Wait, maybe the solid is an ionic solid, but in solid state, ions are fixed. Wait, no—let's check the options again.

Wait, the question is about the solid. Let's analyze each option:

A: "It conducts electricity because it is made of positive and negative particles." — Having positive and negative particles isn't sufficient. For example, solid NaCl has Na⁺ and Cl⁻ but doesn't conduct because ions are fixed. So A is wrong.

B: "It conducts electricity because electrons are free to move through the substance." — If electrons are free (like in metals), then it conducts. But does the diagram show free electrons? Wait, maybe the diagram is of a metal? But the options: Wait, maybe the solid is an ionic solid, but in solid state, electrons are not free. Wait, no—maybe the diagram is of a metallic solid. But let's check option C and D.

C: "It does not conduct electricity because electrons are strongly attracted to specific positive particles." — If electrons are bound (like in ionic bonds, where electrons are in the anion, or in covalent bonds), then they can't move. So in a solid ionic compound, electrons are in the anions (bound to specific cations), so electrons aren't free. So the solid (ionic) doesn't conduct because electrons are stuck to specific positive ions (cations), and ions are fixed. Wait, but option D says "positive particles are not free to move". Wait, in ionic solids, both ions are fixed. But the diagram has positive ions and electrons (maybe the negative particles are electrons? No, negative particles in ionic are anions. Wait, maybe the diagram is of a metal? No, metals have delocalized electrons. Wait, maybe the diagram is of an ionic solid, where electrons are in the anions (so electrons are attracted to specific positive ions, making them not free). So option C: electrons are strongly attracted to specific positive particles (so not free to move), so the solid doesn't conduct. Wait, but let's check the options again.

Wait, the diagram: positive ions (maybe cations) and electrons (or anions?). Wait, the label is "Electron" and "Positive Ion". So the negative particles are electrons. So it's a metal? No, metals have positive ions and delocalized electrons (free to move). But option B says electrons are free, so it conducts. But maybe the diagram is of an ionic solid, but with electrons? No, ionic solids have anions (negative ions), not free electrons. Wait, maybe the diagram is of a metallic solid, but the answer is B? But that contradicts. Wait, no—maybe the solid is an ionic solid, but in solid state, ions are fixed, and electrons are in the anions (so electrons are attracted to specific positive ions, so not free). So option C: it does not conduct because electrons are strongly attracted to specific positive particles (so can't move). Let's check the options:

Option C: "It does not conduct electricity because electrons are strongly attracted to specific positive particles." — If electrons are bound (like in ionic bonds, where each anion is near a cation), then electrons can't move freely, so no conductivity.

Option D: "It does not conduct electricity because the positive particles are not free to move through the substance." — In ionic solids, both positive and negative ions are fixed, but the reason for no conductivity is that charge carriers (ions or electrons) aren't free. But if the negative particles are electrons (as per the diagram), then the charge carriers would be electrons. So if electrons are bound (attracted to specific positive ions), then they can't move. So option C is better. Wait, but let's think again.

Wait, the diagram shows positive ions and electrons (negative particles labeled as electrons). So it's a metal? No, metals have delocalized electrons (free to move), so they conduct. But option B says that. But maybe the diagram is of an ionic solid, but with electrons? No, ionic solids have anions. Wait, maybe the question is about a metallic solid, but the answer is B. But I'm confused. Wait, let's recall:

- Metallic solids: positive ions (cations) in a sea of delocalized electrons (free to move) → conduct electricity.

- Ionic solids: positive and negative ions (anions) fixed in a lattice → do not conduct in solid state (ions can't move), but conduct when molten or dissolved (ions free).

- Molecular solids: no ions, just molecules → no conductivity.

- Covalent network solids: no free charge carriers → no conductivity.

Now, the diagram has positive ions and electrons (labeled as electrons). So it's a metallic solid? Then electrons are free to move, so it conducts (option B). But wait, maybe the diagram is of an ionic solid, but the negative particles are electrons (which is incorrect, ionic has anions). So maybe the diagram is a metal, so option B is correct. But wait, let's check the options again.

Wait, the options:

A: Wrong, because having positive and negative particles isn't enough (e.g., solid NaCl has them but doesn't conduct).

B: If electrons are free to move, then it conducts. Metals have free electrons, so this is correct.

C: Says electrons are strongly attracted to specific positive particles (so not free), so no conductivity. But in metals, electrons are delocalized (not attracted to specific cations), so C is wrong.

D: Says positive particles are not free. But in metals, positive ions are fixed, but electrons are free. So the reason for conductivity is free electrons, not moving positive ions. So D's explanation is wrong (the reason for no conductivity would be if charge carriers aren't free, but in metals, electrons are free). Wait, maybe the diagram is of an ionic solid, but with electrons (which is a mistake). But according to the diagram labels, negative particles are electrons, positive are ions. So it's a metal. So option B is correct? But I'm confused. Wait, maybe the correct answer is C. Wait, no—let's think again.

Wait, maybe the solid is an ionic solid, and the negative particles are anions (not electrons), but the diagram labels them as electrons (maybe a mistake). Then, in solid ionic, ions are fixed, so no conductivity. But the options:

Option C: electrons are strongly attracted to specific positive particles (so anions are near cations, electrons in the anion are attracted to cation, so not free). So the solid doesn't conduct because electrons (in anions) are stuck to specific positive ions. So option C.

Option D: positive particles are not free. But in ionic solids, both ions are fixed, but the reason for no conductivity is that charge carriers (ions) aren't free. But if the negative particles are electrons (as per diagram), then charge carriers would be electrons. So if electrons are bound (attracted to specific positive ions), then they can't move, so no conductivity (option C).

Wait, the key is: for a solid to conduct electricity, there must be mobile charge carriers (electrons or ions).

- If the solid has free electrons (like metals), it conducts (option B).

- If the solid has ions but they're fixed (like solid ionic), it doesn't conduct (options C or D).

But the diagram has positive ions and electrons (labeled as electrons). So if electrons are free (option B), it conducts. But maybe the diagram is of an ionic solid, and the negative particles are anions (mislabeled as electrons). Then, in solid ionic, ions are fixed, so no conductivity. But the options:

Option C: electrons (anions) are strongly attracted to specific positive particles (cations), so not free → no conductivity.

Option D: positive particles are not free → but the reason for no conductivity in ionic solids is that ions (both positive and negative) are fixed, but the charge carriers are ions. So if the question is about ionic solid, then the reason would be that ions are fixed. But option D says "positive particles are not free", which is true, but is that the reason? Wait, in ionic solids, both ions are fixed, so neither can move. So the conductivity requires mobile charge carriers. If the charge carriers are ions, then both positive and negative ions need to move. But in solid state, they can't. So option D's explanation is about positive particles not moving, but the reason for no conductivity is that charge carriers (ions) are not free. But if the negative particles are electrons (as per diagram), then charge carriers are electrons. So if electrons are bound (option C), then no conductivity.

This is confusing. Let's look for the correct answer. Typically, in such questions, the diagram is of an ionic solid (positive ions and negative ions, but labeled as electrons—maybe a mistake). In solid ionic compounds, the ions are fixed in a lattice, so they can't move, and the electrons are in the anions (bound to specific cations), so electrons can't move freely. Therefore, the solid does not conduct electricity because electrons (in anions) are strongly attracted to specific positive particles (cations), so they can't move. So option C. Wait, but option D says positive particles are not free. But in ionic solids, both ions are fixed. However, the charge carriers in ionic compounds are ions (not electrons), so the reason for no conductivity is that ions are not free to move. But the diagram labels negative particles as electrons, which is confusing. Maybe the diagram is of a metallic solid, but then option B would be correct. But I think the intended answer is C or D. Wait, let's check standard questions.

In a typical question, if the diagram shows positive ions and negative ions (anions) in a lattice (solid ionic), then the solid does not conduct because ions are fixed. But the options here:

Option C: electrons are strongly attracted to specific positive particles → if the negative particles are anions (with electrons), then electrons in anions are attracted to cations, so not free.

Option D: positive particles are not free → if the charge carriers are ions, then positive ions not moving would be a reason, but in ionic solids, both ions are fixed.

But the diagram labels negative particles as "Electron", so maybe it's a metal with delocalized electrons. Then option B: electrons are free to move, so it conducts. But that contradicts the usual ionic solid questions. Wait, maybe the diagram is of a metal, so option B is correct. But I'm not sure. Wait, let's think of the options again.

Option A: Wrong, because having positive and negative particles isn't enough (solid NaCl has them but doesn't conduct).

Option B: If electrons are free, it conducts. Metals have free electrons, so this is correct.

Option C: If electrons are attracted to specific positive particles (not free), then no conductivity. But in metals, electrons are delocalized (not attracted to specific cations), so C is wrong.

Option D: If positive particles are not free, but in metals, positive ions are fixed, but electrons are free, so the conductivity is due to electrons, not positive ions. So D's explanation is wrong (the reason for no conductivity would be if charge carriers aren't free, but in metals, electrons are free). So D is wrong.

Therefore, the correct answer should be B. Wait, but I'm confused because the diagram labels negative particles as electrons, which in a metal are free. So the solid conducts because electrons are free to move (option B).
# Answer:
B. It conducts electricity because electrons are free to move through the substance.

Sovi.AI - AI Math Tutor

QUESTION IMAGE

Question

Explanation:

Answer: