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This is the complete lecture note for CHM 302 Inorganic Chemistry II. You can read it online below, open it in the full viewer, or download the PDF for offline study. It pairs with the course's video lectures, so you can read and watch together.
LA-NET | ONLINE LEARNING VIDEO PLATFORM FOR POST-SECONDARY & HIGHER INSTITUTION STUDENTS
LA-NET | ONLINE LEARNING VIDEO PLATFORM FOR POST-SECONDARY & HIGHER INSTITUTION STUDENTS Course code: CHM 302 Course title: Inorganic Chemistry II Course uint: (2 Units C: LH 30) List of series: Series 1: Comparative Chemistry of Main Group Elements Series 2: Chemistry of Non-Metals and Their Compounds Series 3: Transition Metal Chemistry and Complexes Series 4: Radioactivity and Radiochemistry Series 5: Biological Roles of Metals in Living Systems Suggested Outline 1 General Characteristics of Group IA (Alkali Metals) • 1.1 Position in the periodic table • 1.2 Electronic structure and oxidation states • 1.3 Physical and chemical properties 2 General Characteristics of Group IIA (Alkaline Earth Metals) • 2.1 Position in the periodic table • 2.2 Electronic structure and oxidation states • 2.3 Physical and chemical properties 3 Comparative Chemistry of Group IA and Group IIA • 3.1 Trends in atomic and ionic radii • 3.2 Ionisation energies and reactivity • 3.3 Similarities and differences in compounds 5.4 Periodic Properties and Applications of Group IA and IIA Compounds • 4.1 Solubility and stability of salts • 4.2 Industrial and laboratory applications • 4.3 Environmental and biological relevance
LA-NET | ONLINE LEARNING VIDEO PLATFORM FOR POST-SECONDARY & HIGHER INSTITUTION STUDENTS Introduction Many of the materials and processes you encounter daily — from the salts used in industry to the metals in household products — trace their behaviour to the chemistry of the main group elements. This Series focuses on the comparative chemistry of Group IA (alkali metals) and Group IIA (alkaline earth metals), showing how their positions in the periodic table and electronic structures determine their properties and uses. Understanding these relationships will help you apply core inorganic concepts across the rest of CHM 302. The aim of this Series is to develop your ability to describe and compare the electronic structure, physical and chemical properties, and practical applications of Group IA and Group IIA elements, and to use periodic trends to predict and rationalise their chemistry. We shall commence this Series by examining the general characteristics of Group IA, including their position in the periodic table, electronic configuration and typical properties. Next, we will consider the general characteristics of Group IIA in the same way, so you can see parallels and contrasts. Following that, we will compare Groups IA and IIA directly, analysing trends such as ionic radii, ionisation energies and reactivity. Finally, we will conclude by exploring periodic properties, common compounds, and the industrial, environmental and biological relevance of these elements. Series Learning Outcomes Upon completing this Series, you should be able to: • SLO 1.1 define the position of Group IA elements in the periodic table and describe their electronic structures, • SLO 1.2 explain the general physical and chemical properties of Group IA elements, • SLO 1.3 define the position of Group IIA elements in the periodic table and describe their electronic structures, • SLO 1.4 explain the general physical and chemical properties of Group IIA elements, • SLO 1.5 analyse similarities and differences between Group IA and Group IIA elements in terms of periodic trends such as atomic radii, ionisation energies, and reactivity, • SLO 1.6 evaluate the solubility, stability, and applications of common compounds of Group IA and Group IIA elements, and • SLO 1.7 apply knowledge of periodic properties to discuss the industrial, environmental, and biological relevance of Group IA and Group IIA compounds. 1 General Characteristics Of Group IA (Alkali Metals) 1.1 Position in the periodic table Alkali metals are the elements in Group IA of the periodic table, which include lithium, sodium, potassium, rubidium, caesium, and francium. They are located at the far left of the table and are characterised by having a single electron in their outermost s orbital. This configuration makes them highly reactive and strongly inclined to lose that electron, forming +1 cations. Fill in the blank: Alkali metals are located in Group __________________ of the periodic table.
LA-NET | ONLINE LEARNING VIDEO PLATFORM FOR POST-SECONDARY & HIGHER INSTITUTION STUDENTS Diagram of the periodic table highlighting Group IA elements. Figure 1.1 Position of alkali metals in the periodic table. “periodic table alkali metals group IA OER” 1.2 Electronic structure and oxidation states The electronic structure of alkali metals is characterised by a single valence electron in the outermost s orbital (ns¹). This makes them prone to losing that electron easily, resulting in the formation of stable +1 oxidation states. For example, sodium has the configuration [Ne]3s¹ and readily forms Na⁺ ions. Because they almost exclusively exhibit the +1 oxidation state, their chemistry is relatively straightforward compared to transition metals. This simplicity also explains their strong tendency to form ionic compounds. Fill in the blank: The most common oxidation state of alkali metals is __________________. Diagram showing electronic configurations of lithium, sodium, and potassium, highlighting the ns¹ valence electron. Figure 1.2 Electronic configurations of selected alkali metals. “alkali metals electronic configuration ns1 OER”
LA-NET | ONLINE LEARNING VIDEO PLATFORM FOR POST-SECONDARY & HIGHER INSTITUTION STUDENTS 1.3 Physical and chemical properties Alkali metals share several distinctive physical properties: they are soft, have low densities, and possess relatively low melting points compared to other metals. Chemically, they are highly reactive, especially with water, producing hydrogen gas and alkaline hydroxides. Their reactivity increases down the group, with lithium being the least reactive and caesium among the most reactive. For example, sodium reacts vigorously with water to form sodium hydroxide and hydrogen gas. This reaction demonstrates their strong tendency to form ionic compounds and their importance in everyday chemistry. Fill in the blank: When alkali metals react with water, they produce hydrogen gas and __________________ hydroxides. Box 1.3 General properties of alkali metals. Single-column table listing physical properties (soft, low density, low melting points) and chemical properties (reactive with water, form ionic compounds, reactivity increases down the group). “alkali metals physical chemical properties OER” 2 General Characteristics Of Group IIA (Alkaline Earth Metals) 2.1 Position in the periodic table Alkaline earth metals are the elements in Group IIA of the periodic table, which include beryllium, magnesium, calcium, strontium, barium, and radium. They are located immediately to the right of the alkali metals and are characterised by having two electrons in their outermost s orbital. This configuration makes them less reactive than alkali metals but still strongly inclined to lose both electrons, forming +2 cations.
LA-NET | ONLINE LEARNING VIDEO PLATFORM FOR POST-SECONDARY & HIGHER INSTITUTION STUDENTS Fill in the blank: Alkaline earth metals are located in Group __________________ of the periodic table. Diagram of the periodic table highlighting Group IIA elements. Figure 1.3 Position of alkaline earth metals in the periodic table. “periodic table alkaline earth metals group IIA OER” 2.2 Electronic structure and oxidation states The electronic structure of alkaline earth metals is characterised by two valence electrons in the outermost s orbital (ns²). This makes them prone to losing both electrons, resulting in the formation of stable +2 oxidation states. For example, magnesium has the configuration [Ne]3s² and readily forms Mg²⁺ ions. Because they almost exclusively exhibit the +2 oxidation state, their chemistry is predictable, and they form ionic compounds such as oxides, hydroxides, and halides. Fill in the blank: The most common oxidation state of alkaline earth metals is __________________.
LA-NET | ONLINE LEARNING VIDEO PLATFORM FOR POST-SECONDARY & HIGHER INSTITUTION STUDENTS Diagram showing electronic configurations of magnesium, calcium, and barium, highlighting the ns² valence electrons. Figure 1.4 Electronic configurations of selected alkaline earth metals. “alkaline earth metals electronic configuration ns2 OER” 2.3 Physical and chemical properties Alkaline earth metals share several distinctive physical properties: they are harder than alkali metals, have higher densities, and possess higher melting points. Chemically, they are reactive, though less so than alkali metals. They react with water (except beryllium) to form hydroxides and hydrogen gas, and they readily form oxides and salts. Their reactivity increases down the group, with beryllium being the least reactive and barium among the most reactive. For example, calcium reacts with water to form calcium hydroxide and hydrogen gas, a reaction that demonstrates their tendency to form alkaline solutions. Fill in the blank: When alkaline earth metals react with water, they produce hydrogen gas and __________________ hydroxides.
LA-NET | ONLINE LEARNING VIDEO PLATFORM FOR POST-SECONDARY & HIGHER INSTITUTION STUDENTS Box 1.5 General properties of alkaline earth metals. Single-column table listing physical properties (harder than alkali metals, higher density, higher melting points) and chemical properties (reactive with water, form oxides and salts, reactivity increases down the group). “alkaline earth metals physical chemical properties OER” 3 Comparative Chemistry Of Group IA And Group IIA 3.1 Trends in atomic and ionic radii Both Group IA (alkali metals) and Group IIA (alkaline earth metals) show predictable trends in atomic radius, which is the distance from the nucleus to the outermost electron shell. Atomic radii increase down each group as additional electron shells are added. However, Group IIA elements have smaller radii than Group IA elements in the same period because they have a
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