Alkaline Earths

No, Group 7A elements are the halogens - a highly reactive group of nonmetals. Alkaline earth metals are found in Group 2A of the periodic table and are characterized by being shiny, silvery-white metals that react readily with water.

The group name for beryllium is the alkaline earth metals.

Alkaline earth metals typically have a charge of +2 in their ionic forms, as they lose two electrons to achieve a stable electron configuration. This charge is a result of their tendency to form ionic bonds by losing two valence electrons.

I believe that the answer you are looking for is Transition Metals.

Yes, beryllium is a non-ferrous metal. Non-ferrous metals are those that do not contain significant amounts of iron, and beryllium falls into this category.

Beryllium is a metal. It is a lightweight, strong metal that is commonly used in aerospace and defense applications due to its high melting point and stiffness.

I'm tempted to say; Gramma Tassium...Grampa Tassium...however; http://updatecenter.britannica.com/art?assemblyId=91&type=A shows the Family of 'Alkaline Earth Metals'; Francium, Cesium, Rubidium, Sodium and Lithium NOT, however, Hydrogen, despite it being in the same column!!!

An example of a compound containing an alkaline earth metal is calcium carbonate (CaCO3), which is commonly found in minerals like limestone and marble. Another example is magnesium hydroxide (Mg(OH)2), which is used in antacid medications.

The cost of beryllium has fluctuated over time due to factors such as supply and demand, technological advancements, and geopolitical events. However, it tends to be a relatively expensive metal compared to others due to its rarity and unique properties.

Beryllium belongs to the alkaline earth metals family on the periodic table.

The boiling points of alkaline earth metals generally increase down the group. For example, the boiling point of beryllium is around 2469°C and the boiling point of barium is around 1860°C. The melting points also generally decrease down the group.

The heaviest alkaline earth metal is radium, with a molar mass of 226. If you're referring to the largest quantity in nature, it's usually calcium, due to its abundance and the fact that radium is radioactive and occurs in much smaller amounts.

The heaviest alkaline-earth metal is radium. Radium is a highly radioactive element and is the heaviest and most unstable of the alkaline-earth metals.

They don't, they actually have a greater tendency to lose electrons.

This is for a number of reasons.

First of all, the alkali metals form a stable cation by losing one electron, while the alkaline-earth metals need to lose two to form a stable ion. It takes more energy to remove one electron from an atom than it does to remove two.

Additionally an alkaline earth metal has a greater positive charge on its nucleus and a smaller atomic radius than an alkali metal in the same row of the periodic table. This make it even harder to remove valence electrons.

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?? WRONG: Alkali metals have a valence electron configuration of ns1 so they can accept another electron in the ns orbital. On the other hand, alkaline earth metals have a valence electron configuration of ns2. Alkaline earth metals have little tendency to accept another electron, as it woudl have to go into a higher energy p orbital.

The charge on any ion formed by an alkaline earth metal is typically +2. Alkaline earth metals have two valence electrons that they can lose to achieve a stable electron configuration, resulting in a 2+ charge.

One characteristic property of alkaline earth metals is their tendency to form ionic compounds with a +2 oxidation state. This makes them readily react with nonmetals to form stable compounds. Additionally, alkaline earth metals have relatively low electron affinities, making them less reactive than alkali metals.

All alkali metals, alkaline earth metals, and halogens have a common valence electron configuration: alkali metals have 1 valence electron, alkaline earth metals have 2 valence electrons, and halogens have 7 valence electrons. This shared electron configuration influences their chemical properties, such as reactivity and bonding tendencies.

Alkaline earth metals have 2 valence electrons.

1. Alkaline earth metals are the second group of the periodic table.
2. They are shiny, silvery-white, and relatively reactive.
3. Alkaline earth metals have two valence electrons in their outer shell and tend to form 2+ cations in chemical reactions.

Transition metals such as copper, silver, and gold are less reactive than alkali metals and alkaline-earth metals. These metals are less likely to react vigorously with water or air compared to alkali and alkaline-earth metals.

The charge on any ion formed by an alkaline earth metal is typically +2. This is because alkaline earth metals readily lose two electrons to achieve a full outer electron shell and acquire a stable electron configuration.

b. valence electrons

d. electrons needed to fill their octet

Alkaline earth metals have a moderate reactivity level compared to other metals. They are less reactive than alkali metals, but more reactive than transition metals. Alkaline earth metals readily form ionic compounds with nonmetals due to their tendency to lose two electrons.

Alkaline earth metals are less reactive than alkali metals, but more reactive than transition metals. They readily form 2+ cations in chemical reactions due to their tendency to lose two electrons. Their reactivity increases down the group as the atomic radius increases.

Alkali metals are found in Group 1 of the periodic table and are highly reactive metals with one electron in their outer shell. On the other hand, alkaline earth metals are found in Group 2 and are also reactive but less so than alkali metals, with two electrons in their outer shell. Alkaline earth metals also have higher melting and boiling points compared to alkali metals.