Comparison of Physical Properties of Metal Compounds with Non-Metallic Compounds
Examples of metal bonds:
Non-Metallic Metal
1. Metal solids are good conductors of electricity 1. Non-metallic solids are usually not conductors of electricity
2. Having metal luster 2. Not shiny
3. Strong and hard (when used as an alloy metal) 3. Most non-metals are not strong and soft
4. Can be bent and stretched 4. Usually fragile and broken when bent or stretched
5. Good heat conductor 5. Difficult to deliver heat
6. Most metals have a large density 6. Most non metals have a low density
7. Most metals have a high boiling point and melting point 7. Most non-metals have a low boiling point and melting point
METAL COMPOUND REACTIONS:
Alkali metals have several physical properties including soft, shiny white and easily cut. If the metals are left open, the surface will become dull because they react easily with water or oxygen, and are usually stored in kerosene.
As the atomic number increases, the softness level also increases. The level of softness of the alkali metals increases with the increasing atomic number of the metals. The chemical properties of alkaline earth metals can be observed among other things from their reaction to water. The reaction with water produces hydrogen and hydroxide gas and is quite hot. Reactivity to cold water gets bigger with increasing metal numbers.
Alkaline earth metals, except for beryllium, are all white, easily cut and appear to be more shiny when cut, and quickly become dull in the air. Its reactivity to water varies. Beryllium can react with water in an incandescent state and the water is in the form of steam. Magnesium reacts with cold water slowly and faster when it gets hotter, other alkaline earth metals react very quickly with cold water to produce hydrogen and hydroxide gas and produce a lot of heat.
Chloride compounds from alkali metals and alkaline earth dissolve in water to form simple hydrate ions. many covalent or somewhat covalent chlorides undergo hydrolysis and produce chlorides and oxides or hydroxides. For example aluminum chloride solution reacts with water to form aluminum hydroxide.
Based on known octet rules, the hydrogen atom lacks 1 electron and the chlorine atom needs 1 electron to form a stable configuration of the noble gas group. When viewed in terms of electronegativity, chlorine has an electronegativity value that is not small. A stable configuration can be achieved by using shared electrons. The hydrogen atom and the chlorine atom each contribute one electron to form a shared pair of electrons.
In the Lewis structure for NaCl and HCl, the Cl atom obtains an electron configuration of noble gas atoms. The tendency of Cl atoms to accept an electron under any circumstances is always the same, but when compared between Na or H atoms, the atoms will not simply release their electrons. To release valence electrons from Na, energy (I1) of -5.14 eV / atom is required which is smaller than the energy needed to release valence electrons from H, which is 13.6 eV / atom. Sodium is more metallic than hydrogen. In fact, hydrogen is not a metal under normal conditions; hydrogen does not give its electrons to other non-metal atoms. The formation of a bond between an H atom and a Cl atom involves the sharing of electrons which results in a covalent bond.