bonding
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Considering the followng question.
An element (melting point above 3000°C) forms an oxide which is a gas at room temperature.
Which type of bonding is likely to be present in the element?
A Metallic B Polar covalent C Non-polar covalent D Ionic
I think the oxide is CO2 therefore giant-covalent bonding must be one of the choice. Am i right??
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given the structure of Ice which I cant reproduce here. Which of the following statements is not true about ice?
A Ice has a lower density than water at 0oC due to its open structure
B The bond angle about oxygen in ice is 109.5o
C Ice has a giant covalent structure.
D Ice does not conduct electricity.
A and B are correct. I think C is wrong but what about D. D is equally wrong. Given the covalent bonding in Ice as know in tetrahedral fashion D should be wrong. Please explain.
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Yes, carbon has a giant covalent lattice structure. Since the option "giant covalent" is not present in the options, the best option would be "non-polar covalent". The covalent bonds are non-polar, since afterall there's only one element present, carbon.
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A, B and D are essentially correct.
(B is not entirely correct, because the water-water hydrogen bond angle in ice is 109.5 deg, at least for this particular structural form of ice; but the H-O-H bond angle is 104.5 deg rather than 109.5 deg, due to lone pair - lone pair repulsion greater than lone pair - bond pair repulsion greater than bond pair - bond pair repulsion.)
Hence, the best answer is C, which is an incorrect statement, since ice is a giant hydrogen bonded lattice, not giant covalent bonded lattice.
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Thank you Sir.
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Totally welcome as always, Kahynickel :)