This 12-minute video lesson discusses the properties of alkali, alkaline earth and transition metals. It also looks at Halogens and noble gases. [Chemistry playlist: Lesson 8 of 106].
Chlorine monoxide (ClO) in the atmosphere as measured by the Microwave Limb Sounder (MLS) instrument on NASAs Aura satellite. MLS can simultaneously measure several trace gases and ozone-destroying chemicals in the upper troposphere and photosphere. In this series of animations we present chlorine monoxide (ClO), hydrogen chloride (HCl), nitric acid (HNO3), ozone (O3), water vapor (H2O) and temperature measurements. These are first light data taken when the MLS was operated for the first time. ClO is a temporary byproduct of the chemical reaction sequence by which chlorine from chlorofluorocarbons (CFCs) destroys ozone.
Hydrogen chloride (HCl) in the atmosphere as measured by the Microwave Limb Sounder (MLS) instrument on NASAs Aura satellite. MLS can simultaneously measure several trace gases and ozone-destroying chemicals in the upper troposphere and photosphere. In this series of animations we present chlorine monoxide (ClO), hydrogen chloride (HCl), nitric acid (HNO3), ozone (O3), water vapor (H2O) and temperature measurements. These are "first light" data taken when the MLS was operated for the first time. Ozone-destroying chlorine (Cl) atoms are neutralized when they bond with hydrogen (H) to form HCl.
Inorganic chemistry is a division of chemistry that studies metals, their compounds, and their reactivity. Metal atoms can be bound to other metal atoms in alloys or metal clusters, to nonmetal elements in crystalline rocks, or to small organic molecules, such as a cyclopentadienyl anion in ferrocene. These metal atoms can also be part of large biological molecules, as in the case of iron in hemoglobin (oxygen-carrier protein in the blood). Upon successful completion of this course, students will be able to: Describe nuclear charge and calculate effective nuclear charge in terms of Slater's rules; Demonstrate an understanding of trends in the periodic table; Describe the bonding between atoms in terms of valence bond theory; Describe inorganic structures by using valence shell electron pair repulsion theory; Identify the nomenclature rules of coordination compounds; Demonstrate an understanding of crystal structures, lattice energies, and different types of unit cells; Explain the electronic structure of solids, the concept of band gap energy, and how this band gap determines the electronic properties (insulator, conductor, and semiconductor) of solid materials; Describe general trends in the reactivity of elements within Groups I through VII. (Chemistry 107)
