![]() ![]() To draw an electron dot symbol, start with the abbreviation for the element of interest as the center, signifying the nucleus of the atom. The graphical notation used for valence electrons is called an Electron-Dot Symbol. Main group, transition and inner transition elements are indicated.Īlthough it is entirely possible to define the number of valence electrons in an atom through numbers, sometimes it is helpful to have a graphical representation. For all of the transition elements and the inner transition elements, they have a total of 2 electrons in their valence shell.įigure 4.1 Periodic Table of the Elements. For example all of the elements in the halogen family belong to group VIIA and correspondingly have 7 electrons in their valence shell. The main group elements are numbered IA to VIIIA, and their number of valance shell electrons correspond to their group number (Fig 4.1). When looking at the periodic table, it it divided into main group elements and transition elements. Electron-Dot Symbolsįor each element on the periodic table, it is possible to predict the number of valence shell electrons that they will contain. Covalent bonding and covalent compounds will be discussed in Chapter 4 “Covalent Bonding and Simple Molecular Compounds”. The bond made by electron sharing is called a covalent bond. These shared electrons simultaneously occupy the outermost shell of both atoms. The second way for an atom to obtain an octet of electrons is by sharing electrons with another atom. The resulting compounds are called ionic compounds. Because opposite charges attract (while like charges repel), these oppositely charged ions attract each other, forming ionic bonds. If an atom has lost one or more electrons, it is positively charged and is called a cation. If an atom has gained one or more electrons, it is negatively charged and is called an anion. Recall that atoms carrying positive or negative charges are called ions. Those that lose electrons become positively charged, and those that gain electrons become negatively charged. Because some atoms will lose electrons and some atoms will gain electrons, there is no overall change in the number of electrons, but with the transfer of electrons the individual atoms acquire a nonzero electric charge. One way is the transfer of electrons between two atoms until both atoms have octets. There are two ways for an atom that does not have an octet of valence electrons to obtain an octet in its outer shell. The tendency of an atom toward a configuration in which it possesses eight valence electrons is referred to as the “ Octet Rule.” In these lower energy states, the outermost energy level has eight electrons (an “octet”). This instability drives them toward the lower energy states represented by the noble gases that are nearby in the periodic table. The elements in the other groups have valence electron configurations that are not full, so they are unstable when compared to the noble gases. They are already at a low energy state, so they tend to stay as they are. These elements have electron configurations characterized by full valence electron configurations. For atoms, these lower energy states are represented by the noble gas elements. ![]() Lower energy configurations are more stable, so things are naturally drawn toward them. Throughout nature, things that are high in energy tend to move toward lower energy states. Deviations from this ratio result in charged particles called ions. This one-to-one ratio of charges is not, however, the most common state for many elements. The overall charge on the atom is zero, because the magnitude of the negative charge is the same as the magnitude of the positive charge. This is because the number of electrons (negative in charge) is equal to the number of protons (positive in charge). Up until now we have been discussing only the elemental forms of atoms which are neutrally charged. \): In an ionic solution, the A + ions migrate toward the negative electrode, while the B − ions migrate toward the positive electrode.4.1 Introduction to the Octet Rule 4.2 Ions and the Periodic Table Common Cations Common Anions Ions of Transition Metals 4.3 Ionic Bonding 4.4 Practice Writing Correct Ionic Formulas 4.5 Naming Ions and Ionic Compounds 4.6 Polyatomic Ions 4.7 Naming Polyatomic Ions 4.8 Properties and Types of Ionic Compounds 4.9 Arrhenius Acids and Bases 4.10 Ions, Neurons, and Action Potentials ![]()
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