The elements of group 13 are more electronegative than those of groups 1 and 2.True/False

Answer

To determine whether the statement "The elements of group 13 are more electronegative than those of groups 1 and 2" is true or false, we can analyze the properties of the elements in these groups step by step.

### Step 1: Identify the Groups
- **Group 1**: Contains alkali metals (e.g., Lithium, Sodium, Potassium).
- **Group 2**: Contains alkaline earth metals (e.g., Beryllium, Magnesium, Calcium).
- **Group 13**: Contains elements like Boron, Aluminum, Gallium, Indium, and Thallium.

### Step 2: Understand Electronegativity
- Electronegativity is the tendency of an atom to attract electrons towards itself when it is part of a compound.
- Generally, electronegativity increases across a period (from left to right) and decreases down a group.

### Step 3: Compare Electronegativity of Groups
- **Group 1 Elements**: These are highly electropositive, meaning they tend to lose electrons easily rather than attract them. Their electronegativity values are low.
- **Group 2 Elements**: These elements are also electropositive but slightly more electronegative than Group 1 elements.
- **Group 13 Elements**: These elements, particularly Boron, have higher electronegativity compared to both Group 1 and Group 2 elements. For example, Boron has an electronegativity of about 2.04 on the Pauling scale, while Sodium (Group 1) has about 0.93 and Magnesium (Group 2) has about 1.31.

### Step 4: Conclusion
- Since the electronegativity of Group 13 elements is indeed higher than that of both Group 1 and Group 2 elements, the statement "The elements of group 13 are more electronegative than those of groups 1 and 2" is **True**.

### Final Answer
**True**

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