When you carefully added ammonia to your solutions containing copper‚ a light-blue precipitate formed initially that eventually disappeared as more ammonia was added. What do you think this precipitate was? Write an equation. The ammonia molecules attach slowly‚ and in between each attachment‚ there is a chemical equilibrium. The more ammonia is added‚ the more complex is formed‚ as the equilibrium is pushed to the product side. The
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Waals’ forces • Hydrogen bonding • Surface tension and viscosity of liquids Topic 6 Microscopic World II Unit 23 Shapes of molecules Unit 23 23.1 23.2 23.3 23.4 23.5 23.6 23.7 Shapes of molecules Covalent molecules with non-octet structures Shapes of molecules of methane‚ ammonia and water Shapes of some other molecules Influence of the nature of electron pairs on bond angles in molecules of methane‚ ammonia and water Shapes of
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Final Exam Review Chapter 2 Study Questions 1. Define the following a) element b) compound c) pure substance 2. Classify each of the following as a pure substance or a mixture. For each pure substance‚ indicate whether it is an element or a compound. Which of the mixtures are solutions a) air b) titanium c) oak d) baking soda e) oxygen f) 7-Up g) wine h) carbon monoxide 3. Label each of the following drawings as element‚ compound‚ or mixture (Assume each type of circle
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Name:____________________________ CHM 1045: Exam 4 – Chapters 9 & 10 Chapter 9: Chemical Bonding I – Lewis Theory 1. Which of the following statements is TRUE? a) A covalent bond is formed through the transfer of electrons from one atom to another. b) A pair of electrons involved in a covalent bond are sometimes referred to as "lone pairs." c) It is not possible for two atoms to share more than two electrons. e) A covalent bond has a lower potential energy than the two separate atoms. d) Single
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nuclei‚ or as the result of a dipole attraction. The strength of chemical bonds varies considerably; there are "strong bonds" such as covalent or ionic bonds and "weak bonds" such as dipole-dipole interactions‚ the London dispersion force and hydrogen bonding. Since opposite charges attract via a simple electromagnetic force‚ the negatively charged electrons orbiting the nucleus and the positively charged protons in the nucleus attract each other. Also‚ an electron positioned between two nuclei will be
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Organic Chemistry Basic Ideas: Carbon chains: Straight chains and branched chains‚ Numbering of chains and branches. Carbon Rings: Cyclic Molecules‚ Aromatic Compounds Types of Organic reactions: Combustion Addition Substitution Condensation Oxidation What is organic chemistry? Carbon compounds. Methane CH4 Hexane C6 H14 Ethane C2H 6 Heptane C7 H16 Propane C3H 8 Octane C8 H18 Butane C4H10 Nonane C9H20 Pentane C 5 H12 Decane C1 0 H22 Alkanes: Saturated Hydrocarbons
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Transition Metal/Ions The d-block element is called transition metal if it has partly filled d-orbitals in the ground state as well as in its oxidised state. The general electronic configuration of transition metal is (n–1) d1–10ns1–2. Exceptions in electronic configuration are due to (a) very little engery difference between (n–1) d and ns orbitals and (b) extra stability of half filled and completely filled orbitals in case of Cr and Cu in 3d series. Cr : Is 2 2s2 2p6‚ 3s2 3p6 4s1 3d5 Cu : Is2 2s2 2p6
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1) Chemistry Review Key Terms: empirical knowledge theoretical knowledge law of conservation of mass coefficient chemical amount mole Key Concepts: Write chemical equations when given reactants and products (1.5‚ 1.6) Write balanced chemical equations (2.2‚ 2.3) Interpret balanced chemical equations in terms of chemical amount (in moles) (2.3) Convert between chemical amount and mass (2.4) Classify chemical reactions (2.5‚ 2.6) Predict the solubility of elements and ionic and
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the nature of the bonding that occurs in the semiconductor solid. Type of bonding is directly related to conductivity of solid. Bonding in Elemental Solids Electronegativity – the ability of an atom to attract electrons to itself. Atoms with low e.n. (metals) don’t hold valence electrons tightly valence electron orbitals are diffuse (large distances away from nucleus) Atoms with high e.n. (nonmetals) hold valence electrons tightly valence electron orbitals are less diffuse
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