Concept explainers
(a)
Interpretation:
The oxidation state of oxygen in each oxide and the oxidation state of the other element should be determined.
Concept introduction:
Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.
When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.
All the oxygen in oxides are in
(b)
Interpretation:
Each oxide should be identified as molecular or a solid with an infinity extended three-dimensional structure
Concept introduction:
Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.
When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.
(c)
Interpretation:
The oxides which are likely to be a gas or a liquid and which are likely to be a high-melting solid should be determined.
Concept introduction:
Most of ionic oxides form crystal lattice structures. Lattice energies are very high, so, the bonds between atoms are difficult to break. So, ionic oxides have higher melting points. Most first row and second row nonmetal oxides have lower melting points, so, most of them exists as gas or liquid at room temperature.
(d)
Interpretation:
The identity of the other element in (2) and (3) should be determined.
Concept introduction:
Oxygen has six valence electrons in its valence shell, therefore, oxygen can achieve an octet by accepting two electrons from an active metal or by sharing two additional electrons through covalent bonding.
When oxygen reacts with active metals, it gives ionic oxides. With nonmetals, oxygen forms covalent oxides.
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