QuestionWhich of these figures would have the lowest melting point?
A
B
C
Studdy Solution
STEP 1
1. Figure A represents a covalent network solid.
2. Figure B represents an ionic solid.
3. Figure C represents a molecular solid.
4. The melting point of a substance is influenced by the type of bonding and structure.
STEP 2
1. Identify the type of solid each figure represents.
2. Compare the melting points of different types of solids.
3. Determine which figure corresponds to the solid with the lowest melting point.
STEP 3
Identify the type of solid for each figure: - Figure A is a covalent network solid, characterized by strong covalent bonds in a continuous network. - Figure B is an ionic solid, characterized by strong electrostatic forces between positive and negative ions. - Figure C is a molecular solid, characterized by discrete molecules held together by weaker intermolecular forces.
STEP 4
Compare the melting points of the different types of solids: - Covalent network solids (Figure A) typically have very high melting points due to strong covalent bonds throughout the structure. - Ionic solids (Figure B) also have high melting points due to strong ionic bonds. - Molecular solids (Figure C) generally have lower melting points because they are held together by weaker intermolecular forces such as van der Waals forces or hydrogen bonds.
STEP 5
Determine which figure corresponds to the solid with the lowest melting point:
- Based on the comparison, molecular solids (Figure C) have the lowest melting points among the three types of solids.
The figure with the lowest melting point is:
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