Question
Elements are organized on the periodic table based on their properties. Which statement correctly predicts and explains the chemical reactivity of two metals?
Rubidium (Rb) is more reactive than strontium (Sr) because strontium atoms must lose more electrons.
Sodium (Na) is more reactive than magnesium (Mg) because sodium atoms must gain more electrons.
Calcium (Ca) is less reactive than potassium (K) because potassium atoms must lose more electrons.
Beryllium (Be) is less reactive than lithium (Li) because beryllium atoms must gain more electrons.
Rubidium (Rb) is more reactive than strontium (Sr) because strontium atoms must lose more electrons.
Sodium (Na) is more reactive than magnesium (Mg) because sodium atoms must gain more electrons.
Calcium (Ca) is less reactive than potassium (K) because potassium atoms must lose more electrons.
Beryllium (Be) is less reactive than lithium (Li) because beryllium atoms must gain more electrons.
Answers
GPT-4o mini
The correct statement that accurately predicts and explains the chemical reactivity of two metals is:
**Rubidium (Rb) is more reactive than strontium (Sr) because strontium atoms must lose more electrons.**
Here’s why this statement is accurate and the others are not:
1. **Rubidium (Rb) vs. Strontium (Sr)**: Both are metals, and in the periodic table, reactivity increases down a group for alkali metals (group 1, where rubidium is) and decreases down a group for alkaline earth metals (group 2, where strontium is). Rubidium is indeed more reactive than strontium because as you move down a group, elements tend to lose electrons more easily, making them more reactive.
2. **Sodium (Na) vs. Magnesium (Mg)**: This statement is incorrect. Sodium is an alkali metal (group 1) and is more reactive than magnesium (an alkaline earth metal from group 2) because sodium needs to lose one electron, while magnesium needs to lose two. However, the reactivity trends show that sodium is generally more reactive than magnesium, not because sodium must gain electrons, which it does not; it loses electrons.
3. **Calcium (Ca) vs. Potassium (K)**: This statement is incorrect. Potassium is more reactive than calcium. Both are metals, but potassium, being in group 1, is more reactive because it has a single outer electron that it can easily lose, while calcium, being in group 2, loses two electrons but is less reactive than potassium.
4. **Beryllium (Be) vs. Lithium (Li)**: This statement is incorrect. Lithium is more reactive than beryllium. Lithium is an alkali metal (group 1) and loses one electron, while beryllium, an alkaline earth metal (group 2), loses two electrons but is less reactive overall than lithium.
Thus, the first statement about rubidium and strontium is the only one that correctly explains the reactivity of the metals based on their electron configurations and their positions in the periodic table.
**Rubidium (Rb) is more reactive than strontium (Sr) because strontium atoms must lose more electrons.**
Here’s why this statement is accurate and the others are not:
1. **Rubidium (Rb) vs. Strontium (Sr)**: Both are metals, and in the periodic table, reactivity increases down a group for alkali metals (group 1, where rubidium is) and decreases down a group for alkaline earth metals (group 2, where strontium is). Rubidium is indeed more reactive than strontium because as you move down a group, elements tend to lose electrons more easily, making them more reactive.
2. **Sodium (Na) vs. Magnesium (Mg)**: This statement is incorrect. Sodium is an alkali metal (group 1) and is more reactive than magnesium (an alkaline earth metal from group 2) because sodium needs to lose one electron, while magnesium needs to lose two. However, the reactivity trends show that sodium is generally more reactive than magnesium, not because sodium must gain electrons, which it does not; it loses electrons.
3. **Calcium (Ca) vs. Potassium (K)**: This statement is incorrect. Potassium is more reactive than calcium. Both are metals, but potassium, being in group 1, is more reactive because it has a single outer electron that it can easily lose, while calcium, being in group 2, loses two electrons but is less reactive than potassium.
4. **Beryllium (Be) vs. Lithium (Li)**: This statement is incorrect. Lithium is more reactive than beryllium. Lithium is an alkali metal (group 1) and loses one electron, while beryllium, an alkaline earth metal (group 2), loses two electrons but is less reactive overall than lithium.
Thus, the first statement about rubidium and strontium is the only one that correctly explains the reactivity of the metals based on their electron configurations and their positions in the periodic table.