Hydrogen, it is one of the most difficult elements to classify: it can form +1 ions like the alkali metals, it can form -1 ions like the halogens, it is a nonmetal.
Well, let's think...what is the only non-metal that has one electron (considering most nonmetals are on the right side of the PToE)? Hydrogen, of course!
Hydrogen!
hydrogen
Hydrogen.
There is no metal like you describe in your question. Hydrogen is in Group 1, but is not an alkali metal. It is a gas at standard temperature. It does rarely behave like an alkali metal, and it does have only one electron. Hydrogen is in Group 1 primarily because of its electron configuration, which is 1s1. All of the alkali metals also have one electron in their outermost s orbital.
If you could see an alkali metal atom, it would have a nucleus containing protons and neutrons, and an electron cloud containing electrons. In the electron cloud, the highest energy level would contain only one electron.
Hydrogen has a single valence electron, just like the alkali metals. Unlike them, however, hydrogen prefers to covalently bond instead of forming an ionic bond.
Alkali metals can be substituted for hydrogen. Any of them. They include lithim (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs) and francium (Fr). The alkali metals are in group one of the periodic table of the elements, and are all stacked up in the column below hydrogen. All the alkali metals are all organized with a lone electron in their outer most shell, or valence shell (in the neutral atom) and all of the alkali metals would like to loan out that electron to anything that would like to borrow it. It turns out that the reactivity of alkali metals are least to greatest from the top of the column to the bottom. This is because of electron screening. A link to our friends at Wikipedia is provided.
Hydrogen
You think probable to hydrogen.
Hydrogen.
There is no metal like you describe in your question. Hydrogen is in Group 1, but is not an alkali metal. It is a gas at standard temperature. It does rarely behave like an alkali metal, and it does have only one electron. Hydrogen is in Group 1 primarily because of its electron configuration, which is 1s1. All of the alkali metals also have one electron in their outermost s orbital.
Hydrogen
Hydrogen, of course. On some periodic tables you still see it in the alkali position and heading the halogen column to.
If you could see an alkali metal atom, it would have a nucleus containing protons and neutrons, and an electron cloud containing electrons. In the electron cloud, the highest energy level would contain only one electron.
Yes, chemical similarities exist between hydrogen and alkali metals; also the electron configuration has a parallel.
Hydrogen has a single valence electron, just like the alkali metals. Unlike them, however, hydrogen prefers to covalently bond instead of forming an ionic bond.
The element Hydrogen (H) has only 1 electron. When it loses it, it becomes the Ion H+.
Alkali metals can be substituted for hydrogen. Any of them. They include lithim (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs) and francium (Fr). The alkali metals are in group one of the periodic table of the elements, and are all stacked up in the column below hydrogen. All the alkali metals are all organized with a lone electron in their outer most shell, or valence shell (in the neutral atom) and all of the alkali metals would like to loan out that electron to anything that would like to borrow it. It turns out that the reactivity of alkali metals are least to greatest from the top of the column to the bottom. This is because of electron screening. A link to our friends at Wikipedia is provided.
Na 1s2 2s2 2p6 3sLooks like the one valance electron. This is a Group one metal, an alkali metal.