What is chlorines charge

This process is illustrated below. In table salt, this electron comes from the sodium atom. With two oppositely charged ions, there is an electrostatic attraction between them because opposite charges attract. The resulting combination is the compound sodium chloride. Notice that there are no leftover electrons. The number of electrons lost by the sodium atom one equals the number of electrons gained by the chlorine atom one , so the compound is electrically neutral.

In macroscopic samples of sodium chloride, there are billions and billions of sodium and chloride ions, although there is always the same number of cations and anions. Write the formula of the resulting ion and its electron configuration. The electron configuration of Al atom is 1 s 2 2 s 2 2 p 6 3 s 2 3 p 1. The second shell has octet 2 s 2 2 p 6 while the valence shell has 3 electrons 3 s 2 3 p 1.

Mg can achieve octet by losing the 3 valence electrons. The electron configuration of O atom is 1 s 2 2 s 2 2 p 4. The second shell has six electrons 2 s 2 2 p 4 and needs two electrons to achieve octet. Oxygen will gain 2 electrons. In many cases, elements that belong to the same group vertical column on the periodic table form ions with the same charge because they have the same number of valence electrons.

Thus, the periodic table becomes a tool for remembering the charges on many ions. Note the convention of first writing the number and then the sign on a multiply charged ion. These diagrams have two advantages over the electron shell diagrams.

First, they show only valence electrons. Second, instead of having a circle around the chemical symbol to represent the electron shell, they have up to eight dots around the symbol; each dot represents a valence electron.

These dots are arranged to the right and left and above and below the symbol, with no more than two dots on a side. For example, the representation for sodium is as follows:. For the above diagrams, it does not matter what sides the dots are placed on in Lewis diagrams as long as each side has a maximum of two dots. These diagrams are called Lewis electron dot diagrams , or simply Lewis diagrams, after Gilbert N.

Lewis, the American chemist who introduced them. Up to four dots are placed above, below, to the left, and to the right of the symbol in any order, as long as elements with four or fewer valence electrons have no more than one dot in each position. The next dots, for elements with more than four valence electrons, are again distributed one at a time, each paired with one of the first four.

In other words, place the dots singly on each side before pairing them. The Lewis electron dot diagram of fluorine, for example, with seven valence electrons, is constructed as follows:. For the main group elements, the number of valence electrons is the same as the group number listed at the top of the periodic table. Oxford: Oxford University Press, Understanding the Properties of Matter, 2nd edition. Dronskowski, Richard. Computational Chemistry of Solid State Materials.

KGaA, Ebbing, Darrell D. General Chemistry, 8th edition. Emsley, John. The Elements, 3rd edition. Firestone, Richard B. Table of Isotopes, 8th edition, volume 2. Edited by Virginia S. Shirley, with assistant editors Coral M. Baglin, S. Frank Chu, and Jean Zipkin.

Galasso, Francis S. Structure and Properties of Inorganic Solids. Oxford: Pergamon Press, Ghosh, Dulal C. Greenwood, N. Chemistry of the Elements, 2nd edition. Oxford: Butterworth-Heinemann, Gwyn Williams. Electron Binding Energies. Accessed on April 30, Ho, C. Powell, and P. I—1 to I— Huheey, James E. Keiter, and Richard L Keiter. Inorganic Chemistry: Principles of Structure and Reactivity, 4th edition. Hurly, J. Ihde, Aaron J. The Development of Modern Chemistry. New York: Dover Publications, Inc.

International Chemical Safety Card for Chlorine. Accessed on May 5, Accessed on May 4, Kittel, Charles. Introduction to Solid State Physics, 8th edition. Krause, M. Liboff, Richard L. Introductory Quantum Mechanics, 3rd edition. Lide, David R. Mann, Joseph B.

Meek, and Leland C. Manuel, O. New York: Kluwer Academic Publishers, Marshall, James L. Martin, W. McDonough, W. Edited by Richard W. Oxford: Elsevier Ltd. Mechtly, Eugene A. Since chlorine gained an electron it has 17 protons and 18 electrons. The positive sodium ion and negative chloride ion attract one another. They make an ionic bond and form the ionic compound NaCl. Show students a model of a sodium chloride crystal and have them identify the ions. Ask students: What ion is the larger ball with the negative charge?

The chlorine ion. What made it negative? It gained an electron. What is the ion with the positive charge? The sodium ion. What made it positive? It lost an electron. Explore Have students observe actual sodium chloride crystals and relate their shape to the molecular model. Teacher preparation The day before the lesson, dissolve about 10 grams of salt in 50 mL of water. Materials for each group Black paper Salt Cup with salt from evaporated saltwater Magnifier Permanent marker Materials for each student 2 small Styrofoam balls 2 large Styrofoam balls 2 toothpicks Procedure, Part 1 Observe sodium chloride crystals.

Place a few grains of salt on a piece of black paper. Use your magnifier to look closely at the salt. Use your magnifier to look at the salt crystals in the cup. Ask students: What do the photograph, molecular model, and your observations of real salt crystals tell you about the structure of salt?

In each case, the salt seems to be shaped like a cube. Have students build a 3-dimensional model of sodium chloride. Procedure, Part 2 Make NaCl units. Break two toothpicks in half. Use one of the half-toothpicks to connect the centers of the small and large ions together to make a unit of sodium chloride NaCl. Do the same thing with the other small and large ball. Use another half-toothpick to connect the two NaCl units in a straight line as shown. Put NaCl ions together to make one layer of ions.

Build a class sodium chloride crystal. Ask students Based on the way sodium and chloride ions bond together, why are salt crystals shaped like cubes?

The size and arrangement of the ions forms a cube on the molecular level. Since the pattern repeats over and over again in the same way, the shape stays the same even when the crystal becomes the normal size that we can see. Extend Show students how calcium and chlorine atoms bond to form the ionic compound calcium chloride. Ask students: What ions do you think CaCl 2 is made of? One calcium ion and two chloride ions. One calcium and two chlorine are near each other.

The protons of the calcium atom attract the electrons from the chlorine atom. The protons of the two chlorine atoms attract the electrons from the calcium atom more strongly as shown by the thicker arrows. During the interactions between the atoms, the two electrons in calcium's outer energy level are transferred to the outer energy level of each of the chlorine atoms.

Since calcium lost two electrons, it has 20 protons, but only 18 electrons. Since each chlorine atom gained an electron, they each have 17 protons and 18 electrons. Oppositely charged ions attract each other, forming an ionic bond.

The bonded ions are more stable than the individual atoms were. Downloads Lesson 4. Student Reading Use this related reading to extend student comprehension after completing the lesson.