Final answer:
The alkali metals and the alkaline earth metals are two groups of elements found on the periodic table. They have both similarities and differences in their physical and chemical properties, magnetic properties, and electron configurations. The alkali metals are more reactive than the alkaline earth metals, and their electron configurations follow the pattern of ns1. The alkaline earth metals have a completed s subshell in their outermost shell, and their electron configurations follow the pattern of ns2.
Step-by-step explanation:
The alkali metals and the alkaline earth metals are two groups of elements found on the periodic table. The alkali metals are located in Group 1A and include elements such as lithium, sodium, and potassium. The alkaline earth metals are located in Group 2A and include elements such as beryllium, magnesium, and calcium. These two groups of metals have some similarities, but also some differences in their physical and chemical properties, magnetic properties, and electron configurations.
Physical and Chemical Properties:
The alkali metals and the alkaline earth metals have different physical and chemical properties. The alkali metals are soft, shiny, and highly reactive. They have low melting and boiling points and are good conductors of heat and electricity. They react vigorously with water and oxygen and form strong bases when reacting with acids. In contrast, the alkaline earth metals are harder, denser, and less reactive than the alkali metals. They have higher melting and boiling points and are also good conductors of heat and electricity. They react slowly with water and oxygen and form weaker bases when reacting with acids.
Magnetic Properties:
Both the alkali metals and the alkaline earth metals are diamagnetic, which means they are not attracted to magnets. This is because their electron configurations do not allow for unpaired electrons, which are necessary for paramagnetic behavior (attraction to magnets). Therefore, neither group of metals exhibits magnetic properties.
Electron Configurations:
The alkali metals have a single valence electron in their outermost (valence) shell, which gives them similar chemical properties. Their electron configurations follow the pattern of ns1, where n represents the principal quantum number. For example, lithium has an electron configuration of 1s2 2s1, sodium has an electron configuration of 1s2 2s2 2p6 3s1, and potassium has an electron configuration of 1s2 2s2 2p6 3s2 3p6 4s1. On the other hand, the alkaline earth metals have a completed s subshell in their outermost (valence) shell, which also gives them similar chemical properties. Their electron configurations follow the pattern of ns2. For example, beryllium has an electron configuration of 1s2 2s2, magnesium has an electron configuration of 1s2 2s2 2p6 3s2, and calcium has an electron configuration of 1s2 2s2 2p6 3s2 3p6 4s2.