Metallic Bonding and Types of Solids: Quiz
Seven questions on metallic bonding, alloys and the four types of solid, with explanations.
Metallic Bonding and Types of Solids: Quiz
7 questions
In metallic bonding the outer electrons are delocalized and free to move, so they carry the current. The positive ions stay in the lattice.
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Answer: Delocalized electrons
In metallic bonding the outer electrons are delocalized and free to move, so they carry the current. The positive ions stay in the lattice.
Melting a molecular solid only overcomes the weak forces between molecules, so molecular solids usually melt at low temperatures.
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Answer: Molecular
Melting a molecular solid only overcomes the weak forces between molecules, so molecular solids usually melt at low temperatures.
In the solid the ions are fixed in the lattice; when molten they can move and carry charge. NaCl has no delocalized electrons.
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Answer: Its ions are free to move
In the solid the ions are fixed in the lattice; when molten they can move and carry charge. NaCl has no delocalized electrons.
A very high melting point means strong bonds throughout; no conduction even when molten rules out ionic and metallic solids. Silicon dioxide fits.
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Answer: Covalent network
A very high melting point means strong bonds throughout; no conduction even when molten rules out ionic and metallic solids. Silicon dioxide fits.
Within each layer the covalent bonds are very strong, but the forces between layers are weak, so the layers slide over each other.
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Answer: Its layers are held together only weakly and can slide
Within each layer the covalent bonds are very strong, but the forces between layers are weak, so the layers slide over each other.
Atoms of a different size distort the regular layers of iron ions, making it harder for layers to slide: the alloy is harder and stronger.
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Answer: Carbon atoms disrupt the layers so they slide less easily
Atoms of a different size distort the regular layers of iron ions, making it harder for layers to slide: the alloy is harder and stronger.
Ice is a molecular solid. Melting overcomes the intermolecular forces, mainly hydrogen bonds; the O–H bonds inside each molecule are not broken.
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Answer: Forces between water molecules (including hydrogen bonds)
Ice is a molecular solid. Melting overcomes the intermolecular forces, mainly hydrogen bonds; the O–H bonds inside each molecule are not broken.