Three peculiar properties of sodium:

It has low boiling point and melting point.
It is a very soft metal where one can cut it with knife.
It does not produce resonant sound when it is dropped to the earth (non-sonorous).

Explanation:

Sodium is a silver colored metal whose atomic number is 11 with Na as chemical formula. Sodium has stable electronic configuration. It reacts with oxygen to form its oxide. It is widely used in many chemical industries.

Properties of Sodium that Differ from Most Metals:

Sodium is a highly reactive alkali metal that exhibits several unique properties, which set it apart from the general physical properties of most metals. These properties include:

1. Low Density:
Sodium has a relatively low density compared to other metals. Its density is approximately 0.97 grams per cubic centimeter (g/cm³), which is significantly lower than the average density of metals (around 7-9 g/cm³). This low density is due to the relatively large atomic radius and the presence of a single valence electron in the outermost energy level of sodium atoms. As a result, sodium is less dense and lighter than most other metals, allowing it to float on water.

2. Low Melting and Boiling Points:
Another characteristic feature of sodium is its relatively low melting and boiling points. The melting point of sodium is 97.8 degrees Celsius (°C), while its boiling point is 883 °C. These temperatures are considerably lower compared to the melting and boiling points of typical metals, which often exceed 1000 °C. The low melting and boiling points of sodium can be attributed to the weak metallic bonding between its atoms, which arises due to the presence of a single valence electron. The low energy required to separate sodium atoms from each other results in these relatively low phase transition temperatures.

3. High Reactivity:
Sodium is highly reactive, especially in the presence of moisture or oxygen. It readily reacts with water, releasing hydrogen gas and forming sodium hydroxide. This reaction is exothermic and can be highly vigorous, often resulting in the ignition of the hydrogen gas produced. Additionally, sodium reacts with oxygen in the air, forming sodium oxide. This reactivity is due to the low ionization energy and the tendency of sodium to lose its single valence electron in order to achieve a stable electron configuration. The high reactivity of sodium distinguishes it from many other metals, which often exhibit lower reactivity or are relatively inert.

In conclusion, sodium possesses several distinct properties that differentiate it from the general physical properties of most metals. Its low density, low melting and boiling points, and high reactivity contribute to its unique characteristics and applications in various fields.