A scientist isolates a gaseous compound. Is the compound ionic or covalent? Why?
Probably covalent. Most gaseous compounds are diatomic molecules (O2, H2, F2, Cl2 etc) or compounds between elements on the same side of the periodic table (SO2, CO2, SO3, etc) or the middle and side of the periodic table (CH4, C2H2, etc).
To determine whether a gaseous compound is ionic or covalent, we need to consider the types of elements present in the compound and their chemical properties.
Ionic compounds are formed when there is a transfer of electrons between a metal and a non-metal. In an ionic compound, the metal donates electrons to the non-metal, resulting in the formation of ions that have opposite charges. These charged ions are attracted to each other, forming ionic bonds. Examples of ionic compounds include sodium chloride (NaCl) and calcium carbonate (CaCO3).
Covalent compounds, on the other hand, are formed when electrons are shared between non-metal atoms. Unlike ionic compounds, covalent compounds do not involve the transfer of electrons but rather the sharing of electrons in order to achieve a stable electron configuration. Examples of covalent compounds include water (H2O) and methane (CH4).
In the case of a gaseous compound that a scientist has isolated, we can determine whether it is ionic or covalent by examining the elements involved. If the compound consists of a metal and a non-metal, it is more likely to be ionic. However, if the compound is composed of non-metals only, it is likely to be covalent.
To definitively determine the nature of the compound, the scientist may employ various experimental techniques, such as analyzing the compound's melting and boiling points, conducting conductivity tests, or using spectroscopic methods to identify the types of chemical bonding present.
So, to answer the question more specifically, a scientist isolating a gaseous compound would need to analyze its chemical composition and employ appropriate techniques to determine whether it is ionic or covalent.