CHEMICAL COMPOUNDS AND THEIR CHARACTERISTIC PROPERTIES

Size: px

Start display at page:

Download "CHEMICAL COMPOUNDS AND THEIR CHARACTERISTIC PROPERTIES"

Victoria West
5 years ago
Views:

Seminar_2 1. Chemical compounds and their characteristic properties. 2. Types of chemical bonds (theses). 3. Basic types of complex compounds (theses). 4. Stability of complex compounds.

1 Seminar_2 1. Chemical compounds and their characteristic properties. 2. Types of chemical bonds (theses). 3. Basic types of complex compounds (theses). 4. Stability of complex compounds. TEST 2_ Chemical compounds. Complex compounds. Be prepared to answer! How to calculate the molar mass of chemical substances The classification of chemical compounds: acids, bases, salts, oxide The characteristic reactions of the acid basic interaction Naming of complex compounds CHEMICAL COMPOUNDS AND THEIR CHARACTERISTIC PROPERTIES Now we will illustrate the periodicity of chemical properties by considering some reactions of hydrogen, oxygen, and their compounds. We choose to discuss hydrogen and oxygen because, of all the elements, they form the most kinds of compounds with other elements. Additionally, compounds of hydrogen and oxygen are very important in such diverse phenomena as all life processes and most corrosion processes. Atomic hydrogen has the 1s 1 electron configuration. It reacts with metals and with other nonmetals to form binary compounds called hydrides. These can be (a) ionic hydrides, which contain hydride ions, H2, formed when hydrogen gains one electron per atom from an active metal; or (2) molecular hydrides, in which hydrogen shares electrons with an atom of another nonmetal. The ionic or molecular character of the binary compounds of hydrogen depends on the position of the other element in the periodic table. Common hydrides of the representative elements. The ionic hydrides are shaded blue, molecular hydrides are shaded red, and those of intermediate character are shaded purple. The Group 7A hydrogen halides are acids and do not include hydride in their names. The reactions of H 2 with the alkali (1A) and the heavier (more active) alkaline earth (2A) metals result in solid ionic hydrides. The reaction with the molten (liquid) 1A metals may be represented in general terms as Thus, hydrogen combines with lithium to form lithium hydride and with sodium to form sodium hydride.

In general terms, the reactions of the heavier (more active) 2A metals may be represented as Thus, calcium combines with hydrogen to form calcium hydride: These ionic hydrides are all basic because

2 In general terms, the reactions of the heavier (more active) 2A metals may be represented as Thus, calcium combines with hydrogen to form calcium hydride: These ionic hydrides are all basic because they react with water to form hydroxide ions. When water is added by drops to lithium hydride, for example, lithium hydroxide and hydrogen are produced. The reaction of calcium hydride is similar. Hydrogen reacts with nonmetals to form binary molecular hydrides. The nonmetals have higher (or equal) electronegativity relative to hydrogen, so the nonmetal takes on a negative oxidation state while hydrogen goes into the +1 oxidation state. For example, H 2 combines with the halogens to form colorless, gaseous hydrogen halides: Specifically, hydrogen reacts with fluorine to form hydrogen fluoride and with chlorine to form hydrogen chloride: Hydrogen combines with oxygen to form molecular compounds with a 2:1 stoichiometry: The heavier members of the Group 6A family also combine with hydrogen to form binary compounds that are gases at room temperature. Their formulas resemble that of water. These compounds are named: H 2 O, hydrogen oxide (water), H 2 S, hydrogen sulfide, H 2 Se, hydrogen selenide, H 2 Te, hydrogen telluride. All except H 2 O are very toxic. The primary industrial use of H 2 is in the synthesis of ammonia, NH 3, by the Haber process. Most of the NH 3 is used in liquid form as a fertilizer or to make other fertilizers, such as ammonium nitrate, NH 4 NO 3, and ammonium sulfate, (NH 4 ) 2 SO 4 : Many of the molecular (nonmetal) hydrides are acidic; their aqueous solutions contain hydrogen cations (H + ). These include HF, HCl, HBr, HI, H 2 S, H 2 Se, and H 2 Te. Example. PREDICTING PRODUCTS OF REACTIONS

and noble (unreactive) metals (Au, Pd, Pt). Oxides are binary compounds that contain oxygen.

After these reactions are initiated, most release more than enough energy to be self-sustaining, and some become red hot.

3 Example. IONIC AND MOLECULAR PROPERTIES Predict the ionic or molecular character of the product in the previous example Oxygen forms oxides by direct combination with all other elements except the noble gases and noble (unreactive) metals (Au, Pd, Pt). Oxides are binary compounds that contain oxygen. Although such reactions are generally very exothermic, many proceed quite slowly and require heating to supply the energy necessary to break the strong bonds in O 2 molecules. After these reactions are initiated, most release more than enough energy to be self-sustaining, and some become red hot. Reactions of O 2 with Metals In general, metallic oxides (including peroxides and superoxides) are ionic solids. The Group 1A metals combine with oxygen to form three kinds of solid ionic products called oxides, peroxides, and superoxides. Lithium combines with oxygen to form lithium oxide. By contrast, sodium reacts with an excess of oxygen to form sodium peroxide, Na 2 O 2, as the major product, rather than sodium oxide, Na 2 O. Peroxides contain the O-O 2- ion (O 2-2), in which the oxidation number of each oxygen is -1, whereas normal oxides such as lithium oxide, Li 2 O, contain oxide ions, O 2-. The heavier members of the family (K, Rb, Cs) react with excess oxygen to form superoxides.

The tendency of the Group 1A metals to form oxygen-rich compounds increases going down the group. This is because cation radii increase going down the group.

They react with an excess of oxygen to give oxides with higher oxidation states (such as Fe 2 O 3 and CuO). The normal oxides of the representative elements in their maximum oxidation states.

4 The tendency of the Group 1A metals to form oxygen-rich compounds increases going down the group. This is because cation radii increase going down the group. You can recognize these classes of compounds as Metals that exhibit variable oxidation states react with a limited amount of oxygen to give oxides with lower oxidation states (such as FeO and Cu 2 O). They react with an excess of oxygen to give oxides with higher oxidation states (such as Fe 2 O 3 and CuO). The normal oxides of the representative elements in their maximum oxidation states. Acidic oxides (acid anhydrides) are shaded red, amphoteric oxides are shaded purple, and basic oxides (basic anhydrides) are shaded blue. An amphoteric oxide is one that shows some acidic and some basic properties. Reactions of Metal Oxides with Water Oxides of metals are called basic anhydrides (or basic oxides) because many of them combine with water to form bases with no change in oxidation state of the metal. Anhydride means without water, and in a sense, the metal oxide is a hydroxide base with the water removed. Metal oxides that are soluble in water react to produce the corresponding hydroxides. The oxides of the Group 1A metals and the heavier Group 2A metals dissolve in water to give solutions of strong bases. Most other metal oxides are relatively insoluble in water. Reactions of O 2 with Nonmetals Oxygen combines with many nonmetals to form molecular oxides. For example, carbon burns in oxygen to form carbon monoxide or carbon dioxide, depending on the relative amounts of carbon and oxygen.

Reactions of Nonmetal Oxides with Water Nonmetal oxides are called acid anhydrides (or acidic oxides) because many of them dissolve in water to form acids with no change in oxidation state of the

5 Reactions of Nonmetal Oxides with Water Nonmetal oxides are called acid anhydrides (or acidic oxides) because many of them dissolve in water to form acids with no change in oxidation state of the nonmetal. Several ternary acids can be prepared by reaction of the appropriate nonmetal oxides with water. Ternary acids contain three elements, usually H, O, and another nonmetal. Nearly all oxides of nonmetals react with water to give solutions of ternary acids. The oxides of boron and silicon, which are insoluble, are two exceptions. Reactions of Metal Oxides with Nonmetal Oxides Another common kind of reaction of oxides is the combination of metal oxides (basic anhydrides) with nonmetal oxides (acid anhydrides), with no change in oxidation states, to form salts. Example. ACIDIC CHARACTER OF OXIDES

6 Example. BASIC CHARACTER OF OXIDES Example. BASIC CHARACTER OF OXIDES Example. BASIC CHARACTER OF OXIDES

7 TYPES OF CHEMICAL BONDS Covalent Bonding Coordinate Covalent Bond (Dative Bond) Ionic Bonding Dipole-Dipole Bonding

8 Ion-Dipole Bonding (Solvation) Hydrogen-Dipole Bonding Van der Waals Bonding

9 BASIC TYPES OF COMPLEX COMPOUNDS Complexes When ammonia is added to an aqueous solution of a copper(ii) salt, a deep, almost opaque, blue color develops. This color is due to the formation of the Cu(NH 3 ) 4 + ion, in which four NH 3 molecules are bonded to a central Cu 2+ ion. The formation of this species can be represented by the equation The nitrogen atom of each NH 3 molecule contributes a pair of unshared electrons to form a covalent bond with the Cu H ion. This bond and others like it, where both electrons are contributed by the same atom, are referred to as coordinate covalent bonds. The Cu(NH 3 ) + 4 ion is commonly referred to as a complex ion, a charged species in which a central metal cation is bonded to molecules and/or anions referred to collectively as ligands. The number of atoms bonded to the + central metal cation is referred to as its coordination number. In the Cu(NH 3 ) 4 complex ion- the central metal cation is Cu 2 + the ligands are NH 3 molecules the coordination number is 4 Unidentate Ligands EXAMPLES Bidentate Ligands

10 Tridentate Ligands Quadridentate Ligands Pentadentate Ligands Hexadentate Ligands

11 STABILITY OF COMPLEX COMPOUNDS The equilibrium constant for the formation of a complex ion is called a formation constant (or stability constant) and given the symbol K f. A typical example is Table lists formation constants of complex ions. In each case, K f applies to the formation of the complex by a reaction of the type just cited. Notice that for most complex ions listed, K f is a large number, 10 5 or greater. This means that equilibrium considerations strongly favor complex formation. Consider, for example, the system The large K f value means that the forward reaction goes virtually to completion. Addition of ammonia to a solution of AgNO 3 will convert nearly all the Ag + ions to Ag(NH 3 ) 2 + Formation Constant of Complex Ions

12 Example. CALCULATION OF EQUILIBRIUM CONSTANTS From Example we see that the reaction for the conversion of Ag(NH 3 ) 2 + to Ag(S ) 2 3- has a large equilibrium constant. Looking at it in a slightly different way, we can say that of these two complexes of Ag +, the Ag(S ) 2 3- ion is the more stable.

F321: Atoms, Bonds and Groups Structure & Bonding

F321: Atoms, Bonds and Groups Structure & Bonding 1. This question is about different models of bonding and molecular shapes. Magnesium sulfide shows ionic bonding. What is meant by the term ionic bonding?