Answer:
Use the following answers for questions 1 - 2. (1984 - #8 & 9)
(A) A network solid with covalent bonding
(B) A molecular solid with zero dipole moment
(C) A molecular solid with hydrogen bonding
(D) An ionic solid
(E) A metallic solid
1. Solid ethyl alcohol, C2H5OH (C)
2. Silicon dioxide, SiO2 (A)
Use these answers for questions 3-6 (1989 #11 – 14)
(A) hydrogen bonding (B) hybridization (C) ionic bonding
(D) resonance (E) van der Waals forces (London dispersion forces)
3. Is used to explain why iodine molecules are held together in the solid state (E)
4. Is used to explain why the boiling point of HF is greater than the boiling point of HBr (A)
5. Is used to explain the fact that the four bonds in methane are equivalent (B)
6. Is used to explain the fact that the carbon-to-carbon bonds in benzene, C6H6, are identical (D)
Use the following diagram for questions 7-8
(1989 - #49&51)
7. The normal boiling point of the substance
represented by the phase diagram above is
(A) -15 °C (B) -10 °C
(C) 140 °C (D) greater than 140 °C
(E) not determinable from the diagram
8. For the substance represented in the diagram,
which of the phases is most dense and which is
least dense at - 15 °C.
Most Dense Least Dense
(A) Solid Gas
(B) Solid Liquid
(C) Liquid Solid
(D) Liquid Gas
(E) The diagram gives no information
A crystalline solid has a high melting point and is known to be held together with covalent bonds. This solid is an example of a network solid with covalent bonding.
A covalent bond is the strongest type of bond.
Covalent bond join the atom and molecules together.
Covalent bond is formed by sharing of electrons from both the atoms.
These bonds are formed when there is negligible amount of electronegativity between the atoms.
Thus, the correct option is (A) A network solid with covalent bonding
Learn more about covalent bond
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