alkaline earth metal forms a +2 cation and halogen forms a -1 anion
alkaline earth metal is a metal and halogens are non metals therefore the bond between them is ionic
Alkali metals are metals in Group I (far left column) such as Lithium, Sodium, Potassium, etc. They have a valence of -1.Alkali Earth Metals are in Group II (second column from the left) such as Berylium, Magnesium, Calcium, etc. and have a valence of -2.One Hydroxide (OH-) ion will form an ionic bond with group 1 elements {Like NaOH }, and two Hydroxide ions will form an ionic bond with group 2 elements {like Ca(OH)2 }
Alkaline Earth Metal found in second group of periodic table. The components are beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra). Below some characteristics of Alkaline Earth metals, 1. These metals have an oxidation number of +2 that makes them very reactive. 2. These elements are not freely in nature. 3. These elements are found on earth crust but not in their basic form. 4. they have couple of electrons in their outer most shell. 5. They are distributed in rock structures. 6. They have a high boiling and melting point. 7. they have low density, electron affinity and electromagnetic. 8. they are silver in color. 9. ductile and malleable. 10. Easily reactive with halogens and water.
metallic bond
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If the starting point are elements then the inner shell electrons (non valence) these orbit the nuclei of the atoms and the formation of a chemical bond does not affect these materially. What happens to the valence electrons depends on the bond formed. In an ionic bond electrons are transferred from say the metal atom to the nonmetal- these electrons essentially "orbit" the nuclei of the cations and anions. They are "localised". When a covalent bond is formed the valence electrons involved are shared between the atoms, they "orbit" both nuclei. When the bond is polar covalent they spend a little more time nearer the more electronegative element. When a "delocalised"covalent bond is formed as in bezene or graphite the electrons orbit a number of atomic nuclei. In a metallic bond the valence electrons are also delocalised (the sea of electrons model) across the metal lattice, but in transition metals there is additional bonding between electrons in d orbitals (the tight bound electrons) and these electrons are essentially localised.
the alkali metals have one valence electron, or one electron available to bond with another particle. this lets them bond easily with, lets say, a halogen, which has one 'slot' for an electron. two atoms of an alkali metal would be able to bond with a chalcogen, and so on. it's really all in the number of electrons. the alkaline earth metals have two valence electrons, so they would bond less easily with other elements.
Potassium iodide is an ionic compound.
Ionic. The metal will donate electron(s) to the halogen that will accept electrons. NaCl, for example.
A metal and halogen react to form an ionic bond in which the metal gives an eletron to the halogen Most basic example would be table salt NaCl NaOH + HCl = NaCl + H20
We know that the alkaline earth metal beryllium (Be) and the halogen chlorine (Cl) form the ionic compound beryllium chloride (BeCl2). The equation might look like this:Be + Cl2 => BeCl2
CaF2, Calcium Fluoride. It is useful in iron smelting
No. This is an ionic bond. Look at the electronegativity Cl (3.0) - Sr (1.0) = 2.0; 0.0 to 0.4 is covalent, 0.4+ to 1.7 is polar-covalent and above 1.7 is ionic. You can also assume that a metal and non-metal will form an ionic bonds.
easier to gain electron from alkali metal than sharing with non-metal for covalent bond
ionic bond
any alkaline earth metals
A transition metal is one of the metals that can use the inner shell before using the outer shell to bond. A alkaline earth metal is one of the elements of Group 2 of the periodic table.
It is ionic as are all strontium compounds.