Chapter 4 Reactions in Aqueous Solutions
... The oxidation number of Al increases; it is oxidized; it is the reducing agent. The oxidation number of H decreases; it is reduced; H2SO4 is the oxidizing agent. ...
... The oxidation number of Al increases; it is oxidized; it is the reducing agent. The oxidation number of H decreases; it is reduced; H2SO4 is the oxidizing agent. ...
The Chemical Context of Life by Dr. Ty C.M. Hoffman
... measure of an atom's degree to which it attracts electrons is called its electronegativity. If a covalent bond is formed between two atoms that have drastically different electronegativities, the shared elect ...
... measure of an atom's degree to which it attracts electrons is called its electronegativity. If a covalent bond is formed between two atoms that have drastically different electronegativities, the shared elect ...
Chapter 16 Redox chemistry and corrosion
... Would elements from the following groups be more likely to be oxidised or reduced when they take part in chemical reactions with the other group? Give reasons for your answers. Group A: sodium, calcium and magnesium. Group B: sulfur, oxygen and chlorine. A24. Group A will be oxidised because metals ...
... Would elements from the following groups be more likely to be oxidised or reduced when they take part in chemical reactions with the other group? Give reasons for your answers. Group A: sodium, calcium and magnesium. Group B: sulfur, oxygen and chlorine. A24. Group A will be oxidised because metals ...
THE p -BLOCK ELEMENTS
... N≡N) and to other second row elements (e.g., C=O, C=N, C≡N, N=O). This type of π - bonding is not particularly strong for the heavier p-block elements. The heavier elements do form π bonds but this involves d orbitals (dπ – pπ or dπ –dπ ). As the d orbitals are of higher energy than the p orbitals, ...
... N≡N) and to other second row elements (e.g., C=O, C=N, C≡N, N=O). This type of π - bonding is not particularly strong for the heavier p-block elements. The heavier elements do form π bonds but this involves d orbitals (dπ – pπ or dπ –dπ ). As the d orbitals are of higher energy than the p orbitals, ...
Lecture 9
... The sizes of the atoms and ions do not decrease much as the block is crossed. Although the atoms of each successive element have one more proton in the nucleus, increasing the attraction on the outer 4s electrons, there is increased repulsion on these outer electrons caused by the new electron in th ...
... The sizes of the atoms and ions do not decrease much as the block is crossed. Although the atoms of each successive element have one more proton in the nucleus, increasing the attraction on the outer 4s electrons, there is increased repulsion on these outer electrons caused by the new electron in th ...
Transition Metals
... transition elements but, because of the close proximity of the 3d orbitals, the third ionisation energy is low, resulting in the easy removal of a third electron : Mn2+ (4S0 3d5) ...
... transition elements but, because of the close proximity of the 3d orbitals, the third ionisation energy is low, resulting in the easy removal of a third electron : Mn2+ (4S0 3d5) ...
Valence, Oxidation Number, and Formal Charge: Three Related but
... be determined from an empirical formula alone. The valences of atoms in some simple compounds are illustrated in Table 2. Employing Sidgwick’s preferred definition of valence, it is clear that it is a very important quantity for establishing the properties of a molecule since it indicates how many e ...
... be determined from an empirical formula alone. The valences of atoms in some simple compounds are illustrated in Table 2. Employing Sidgwick’s preferred definition of valence, it is clear that it is a very important quantity for establishing the properties of a molecule since it indicates how many e ...
Problem Set 5_Chem165_Spring14
... (c) For the other three d orbitals, their overlap with the ligand σ orbitals shown in Figure 18.6 is zero (by symmetry). Which ones are these? Explain this. The dxy, dxz, and dyz orbitals have no net overlap with the ligands shown in Figure 18.6. In each case, this because the two lobes of the d orb ...
... (c) For the other three d orbitals, their overlap with the ligand σ orbitals shown in Figure 18.6 is zero (by symmetry). Which ones are these? Explain this. The dxy, dxz, and dyz orbitals have no net overlap with the ligands shown in Figure 18.6. In each case, this because the two lobes of the d orb ...