![]() ![]() Refer to table below for the Electrical properties ofCalcium Electrical ConductivityĬalcium Heat and Conduction Properties Thermal ConductivityĬalcium Magnetic Properties Magnetic Type Hardness of Calcium - Tests to Measure of Hardness of Element Mohs HardnessĬalcium is Conductor of electricity. Sharing electrons, as is done in covalent bonding, creates a strong bond, but not nearly as strong as bonds created by the coming together of negatively and positively charged ions as we see in ionic bonding.Refer to below table for Calcium Physical Properties Densityġ.55 g/cm3(when liquid at m.p density is $1.378 g/cm3) It's important to understand the distinction between ionic and covalent bonds. It will take 4 hydrogens to form a bond with carbon. So, we have Carbon, wanting 4 electrons, and we have hydrogen only wanting one. Hydrogen wants to gain 1 electron to be like helium.Įach dot in this image represents an electron needed to form a covalent bond. It wants to gain 4 electrons to be like Neon. ![]() Let's see how Carbon and hydrogen get together to form methane (CH4), commonly called natural gas.įirst, we find Carbon in group 4a. Remember, our non-metals are located here.ĭon't forget hydrogen it's also a non-metal. Non-metals combine to form covalent bonds to make molecules. Let's do the same thing for two non-metals. Therefore, when Calcium and Fluorine combine to make calcium fluoride, it takes one Ca and two F?s. It will take two fluorides to even out that charge. Right now, the calcium ion has a positive charge of two plus. When bonds form, they always come together to create a neutral charge. Once it does that, it becomes Ca two plus.Īnd what about Fluorine? It?s in group 7A, so to be like it?s nearest noble gas, Neon, it only needs to gain one electron, thus it becomes F one minus or simply F minus, we know it as Fluoride. So, Calcium being no different, and wanting to be like it?s nearest noble gas, Argon, needs to lose 2 electrons. This is called having an electro valence of plus two. It?s located in group 2A.Īll of the elements in group 2A form ions with a positive two charge. Let's start by seeing how calcium fluoride (CaF2) is formed.įirst, we need to find calcium. ![]() So let?s go back to our original question, how does a metal and a non-metal combine to form an ionic bond? Since opposites attract, these dipolar opposites create the strongest bond possible, the ionic bond. When an element loses or gains electrons, allowing it to become iso-electronic with its nearest noble gas, it becomes an ion with a positive or negative charge. So what does that have to do with forming ionic bonds? Everything, really. When it does that, Beryllium will have a positive charge of two, and it will be stated as B-e two plus. Thus, Beryllium wants to lose two electrons. It's nearest noble gas is Helium, which is 2 elements behind Beryllium. The number of electrons an element will gain or lose depends upon its group number in the periodic table. In order to be similar to a noble gas, an element must either take on or give up electrons. The noble gases are the elements located in the last column (8A) of the table.Īll elements want to be like their nearest noble gas because a noble gas is the most stable of all the elements. To understand this process, you must first understand the noble gas rule. In this presentation, we are going to explore how representative, or A column, metals combine with non-metals to form ionic compounds. We have metals, located in the highlighted portion of the table. The periodic table can really be divided into two categories. Let's go back to our old friend, the Periodic Table. ![]()
0 Comments
Leave a Reply. |
AuthorWrite something about yourself. No need to be fancy, just an overview. ArchivesCategories |