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Some General Properties of Group 1 Elements- The s-Block Elements Video Lecture - JEE
FAQs on Some General Properties of Group 1 Elements- The s-Block Elements Video Lecture - JEE
| 1. What are the general properties of Group 1 elements? |  |
Ans. Group 1 elements, also known as alkali metals, exhibit some common properties. They have a single valence electron, which makes them highly reactive. They are soft and have low melting and boiling points. They readily form ionic compounds with non-metals and have a strong tendency to lose their valence electron to form a positive ion.
| 2. What are the elements present in Group 1 of the periodic table? | |
Ans. Group 1 elements include lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr). These elements are located in the first column of the periodic table and are commonly referred to as alkali metals.
| 3. Why are Group 1 elements called alkali metals? | |
Ans. Group 1 elements are called alkali metals because they readily react with water to form alkaline solutions. When alkali metals react with water, they produce hydroxide ions, resulting in the formation of alkaline solutions. This property gives them the name "alkali" metals.
| 4. What is the significance of the s-block in relation to Group 1 elements? | |
Ans. The s-block in the periodic table consists of two groups: Group 1 (alkali metals) and Group 2 (alkaline earth metals). The s-orbital in the outermost electron shell of these elements is partially filled, making them highly reactive. The s-block elements exhibit similar properties due to their similar electronic configurations and valence electron behavior.
| 5. How do Group 1 elements react with non-metals? | |
Ans. Group 1 elements have a strong tendency to lose their valence electron and form a positive ion. When they react with non-metals, such as oxygen or halogens, they readily donate their valence electron to form ionic compounds. For example, sodium reacts with chlorine to form sodium chloride (common salt) by transferring its valence electron to chlorine. This reaction results in the formation of a stable ionic compound.
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