Ionic compounds predicting formulas

Given the formula for an ionic compound, predict whether it is soluble in water or not. [Pg.146]

Given formulas for two ionic compounds, predict whether a precipitate will form when water solutions of the two are mixed, and write the complete equation that describes the reaction. (Section 4.2)... [Pg.368]

Describe energp relationships in ionic compounds Predict the formulas of ionic compounds... [Pg.270]

Using the solubility rules Given the formula of an ionic compound, predict its solnbihty in water. (EXAMPLE 4.1)... [Pg.164]

To predict the formula of an ionic compound, you need to know the charges of the two ions involved. Then you can apply the principle of electrical neutrality, which requires that the total positive charge of the cations in the formula must equal the total negative charge of the anions. Consider, for example, the ionic compound calcium chloride. The ions present are Ca2+ and Cl-. For the compound to be electrically neutral, there must be two Cl- ions for every Ca2+ ion. The formula of calcium chloride must be CaCl indicating that the simplest ratio of Cl- to Ca2+ ions is 2 1. [Pg.38]

Predict formulas of ionic compounds from charges of ions. [Pg.44]

Predict the formulas of binary ionic compounds (Example C.2). [Pg.53]

Diborane reacts with ammonia to form an ionic compound (there are no other products). The cation and anion each contain one boron atom, (a) Predict the identity and formula of each ion. (b) Give the hybridization of each boron atom, (c) Identify the type of reaction that has occurred (redox, Lewis acid-base, or Bronsted acid-base). [Pg.741]

Arts. We treat the oxidation states in part (b) just like the charges in part (a). In this manner, we can predict formulas for covalent and ionic compounds, (a) XY, and (b) WZ,. [Pg.221]

Cations and anions combine in very predictable ways within ionic compounds, always acting to neutralize overall charge. Therefore, the name of an ionic compound implies more than just the identity of the atoms that make it up. It also helps you determine the correct chemical formula, which tells you the ratio in which the elements combine. Consider these two examples, both of which involve lithium ... [Pg.82]

EXAMPLE C.2 Predicting the formula unit of a binary ionic compound... [Pg.65]

Write the chemical formulas for calcium chloride and ammonium sulfate. Predict what kind of reaction will occur between them. Write a balanced chemical equation to show the reaction. Ionic compounds containing the ammonium ion are soluble. Ammonium sulfate is soluble, but barium chloride is not. [Pg.185]

In Chapter 5, we learned to write formulas for ionic compounds from the charges on the ions and to recognize the ions from the formulas of the compounds. For example, we know that aluminum chloride is AICI3 and that VCI2 contains ions. We cannot make comparable deductions for covalent compounds because they have no ions there are no charges to balance. To make similar predictions for species with covalent bonds, we need to use the concept of oxidation number, also called oxidation state. A system with some arbitrary rules allows us to predict formulas for covalent compounds from the positions of the elements in the periodic table and also to balance equations for complicated oxidation-reduction reactions. [Pg.444]

To predict the formula of the ionic compound, we simply recognize that chemical compounds are always electrically neutral—they have the same quantities of positive and negative charges. In this case we must have equal numbers of Ca2+ and 02 ions, and the empirical formula of the compound is CaO. [Pg.595]

Predict the empirical formulas of the ionic compounds formed from the following pairs of elements. Name each compound. [Pg.642]

If the reactants in an equation are two elements, the only way in which they can react is to form a binary compound, which is composed of two elements. Often, when a metal reacts with a nonmetal, electrons are transferred and an ionic compound is formed. You can use the charges of the ions to predict the formula of the compound formed. Metals in Groups I and 2 lose one electron and two electrons, respectively. Nonmetals in Groups 16 and 17 gain two electrons and one electron, respectively. Using the charges on the ions, you can predict the formula of the product of a synthesis reaction, such as the one in Figure 10. [Pg.295]

Oxidation numbers are very useful in correlating and systematizing a lot of inorganic chemistry. A few simple rules allow the prediction of the formulas of covalent compounds, just as predictions were made for ionic compounds in Chapter 4 by using the charges on the ions. [Pg.87]

The following three examples show the formation of ionic compounds by the complete transfer of one or more electrons from the metal to the nonmetal. In each case, the total number of electrons lost equals the total number gained. Note that each ion has the electronic configuration of a noble gas. As you inspect each example, notice how the number of electrons lost by the metal and gained by the nonmetal determines the formula of the ionic product. The formula of the product can be predicted from the electronic configurations of the reactants. [Pg.262]

Predict the formula of the ionic compound formed from the reaction of sodium and oxygen atoms. [Pg.88]

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