Q2. (8 marks total) Types of atomic bonding. Describe both which type(s) of bond
ID: 716067 • Letter: Q
Question
Q2. (8 marks total) Types of atomic bonding. Describe both which type(s) of bonding are present in the following materials and how that type of bonding affects the propcrtics of that material. Consider the electronegativity differences between elements where applicable to justify your comments (a) H20 in ts liquid form. Why does water expand when it freezes? (2 marks) (b) Mercury. Comment on the strength of interatomic bonding in mercury (Hint: why is it a liquid at room tempcrature)? (2 marks) (c) Polystyrene (2 marks) (d) Copper oxide (CuoO) (2 marks)Explanation / Answer
(a) H2O shows co-valent bonding.The electronegetivity difference between O and H is not so much that complete transfer of electron will take place. The co-valent bonding is the reason it is liquid at room temperature.
Water due the slight difference in electronegetivity of H and O forms partial (+)ve and (-)ve charge on H and O respectively. This leads to H-bonding. While freezing the crystall structure of water is imposed over the H bonds making them significantly longer in turn making the atoms even further apart as a result reducing the density.
(b) Mercury has metallic bonding between its atoms. Though, normally metallic bonding is really strong and results in hard crystal structures. But, the case of mercury is different. The metallic bonds in mercury are very weak because it has completely filled 5d-orbital. This makes it difficult to form metallic bonds. Also, the other elements in the group show weak metallic bonding.
(c) Polystyrene molecule is made up of styrene monomers with co-valent bonds between each moonomer. Even in the styrene molecule which is an aromatic hydrocarbon has co-valent bonds between its atoms.
(d) CuO shows co-valent bonding. More precisely polar co-valent bonding. The electronegetivity difference is 1.54 which is in the co-valent range only.
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