which type of oxides are formed when nonmetals combine with nonmetals

Hydrogen combines with non-metals, to give the respective hydrides. With oxygen Hydrogen burns in oxygen to form water. Instead of igniting the mixture, if a small quantity of well divided platinum is added to the mixture of the two gases, they instantly comb..

>Metals occupy the groups on the left of periodic table and are largely classified as alkali metals (group IA) alkaline earth metals (group IIA) and transition metals (elements between group IIA and IIIA) Metals and non-metals combine to form electrovalent or ionic com..

When dry chlorine is passed through molten sulphur it combines with sulphur to form vapors of sulphur monochloride S 2 Cl 2 . When these vapors are condensed, they form a red liquid (Fig.14.11)...

. Non-metal exhibit both electrovalency or covalency. Deposition during electrolysis They are always deposited at the cathode. They are always deposited at the anode. Redox reaction These lose electrons and hence get oxidized. These gain electrons and hence get reduced. Redox agents They ..

We are familiar with the fact that the atoms of all elements, except noble gases, have an incomplete outermost shell. Consequently, most elements are reactive and they try to achieve the stability of the noble or inert gases by electron transfer or by electron sharing. After this combinationh..

Question 1 - Question: Compare the properties of a typical metal and a non-metal on the basis of the following. Fill in Column A, B. Properties A Metal B Non- metal Electronic configuration ? ? Nature of oxides ? ? Oxidizing or reducing action ? ? Conduction of heat an..

With hydrogen - When hydrogen is passed through boiling sulphur, both hydrogen and sulphur combine to form hydrogen sulphide (Fig.13.28..

Oxides of metals and non-metals react with water to give the corresponding alkalis and acids. Oxides of metals give alkalis: The oxides of metals are basic in nature. These react with water to form the respective alkalis. For example, ..

The rules used for the calculation of oxidation number of an atom in a molecule are: The oxidation number of an element in the free or elementary state is always zero. For example, oxidation numbers of helium in He, hydrogen in H 2 , oxygen in O 2 , iron in Fe, brom..

When an element forms two monoatomic cations (representing different oxidation states), the two ions are distinguished by using the ending 'ous' and 'ic' at the end. The suffix 'ous' is used for the cation with lower oxidation state and the suffix 'ic' is used for the ..