able to appear because an excited electron was unstable and had to fall back to a more stable energy level‚ creating energy in the form of light. However‚ to understand this‚ one must understand what causes an electron to be excited. So from the very beginning‚ a person named Max Plank proposed a theory that energy is emitted and absorbed in quantities called “quanta.” Einstein then came along and said that light contained quanta energy called “photons.” Electrons that are present in atoms are on
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Electrical Current An electric current is a flow of electrical charge. When a metal conducts electricity‚ the charge is carried by electrons moving through the metal. Electrons are subatomic particles with a negative electrical charge. When a solution conducts electricity‚ the charge is carried by ions moving through the solution. Ions are atoms or small groups of atoms that have an electrical charge. Some ions have a negative charge and some have a positive charge. Citric Acid Citric acid is
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upon the structure of the atom. Before Rutherford‚ there was a man named Joseph John Thomson who proposed the structure of the atom. He stated that the electrons of the atoms are actually inside the atom‚ and the atom itself is positively charged‚ like a “raisin pudding”. The electrons are scattered all around the atom. He stated that the electrons and the positively charged material cancel each other‚ making it stable. The structure of the atom‚ proposed by Thomson. (J.J Thomson Plum Pudding Model
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Shapes‚ Valance Bond Theory‚ and Molecular Orbital Theory 1) Determine the electron geometry (eg) and molecular geometry(mg) of BCl3. A) eg=trigonal planar‚ mg=trigonal planar B) eg=tetrahedral‚ mg=trigonal planar C) eg=tetrahedral‚ mg=trigonal pyramidal D) eg=trigonal planar‚ mg=bent E) eg=trigonal bipyramidal‚ mg= trigonal bipyramidal Answer: A 2) Determine the electron geometry (eg)‚ molecular geometry (mg)‚ and polarity of SO2. A) eg=tetrahedral
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SLG Practice Final Exam Chem. 113 True and False 1. The Bohr Theory explains that an emission spectral line is due to an electron losing energy and changing orbitals. 2. 4s orbitals have higher energy than 3d orbitals. 3. An atom with an even number of electrons is always diamagnetic. 4. Covalent bonds are formed by atoms sharing electrons. Multiple Choice 5. Choose the INCORRECT statement about NH2-: a) There is one lone pair on N. b) There are two σ bonds. c) There are no π
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CHAPTER-23 HW. Rahaf AlBathi 121114 Question 1 The electron configuration of a Ni2+ ion is: | A) [Ar]4s23d8 | | B) [Ar]4s23d6 | | C) [Ar]3d8 | | D) [Ar]3d6 | Question 2 The Fe3+ ion has _____ electrons in 3d orbitals. | A) 6 | | B) 5 | | C) 4 | | D) 3 | | E) 2 | Question 3 A ligand is: | A) a molecule or ion that has at least one lone pair of electrons | | B) a nucleophile | | C) a Lewis base | | D) part of a coordination compound |
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CH 202 Breakdown UV/Vis: Molecules containing π-electrons or non-bonding electrons (n-electrons) can absorb the energy in the form of ultraviolet or visible light to excite these electrons to higher anti-bonding molecular orbitals. The more easily excited the electrons (i.e. lower energy gap between the HOMO and the LUMO)‚ the longer the wavelength of light it can absorb. Conjugation raises the energy of the bonding orbitals and lowers the energy of the antibonding molecular orbital. This
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Atoms release light photons when their electrons become excited. If you’ve read How Atoms Work‚ then you know that electrons are the negatively charged particles that move around an atom’s nucleus (which has a net positive charge). An atom’s electrons have different levels of energy‚ depending on several factors‚ including their speed and distance from the nucleus. Electrons of different energy levels occupy different orbitals. Generally speaking‚ electrons with greater energy move in orbitals farther
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The Photoelectric Effect Definition: It is the emission of electrons from a metal surface under the illumination of a suitable radiation. The photoelectric effect is the phenomenon whereby electrons are emitted from a surface (usually metallic) upon the exposure to and absorption of electromagnetic radiation‚ such as visible light‚ that is above the threshold frequency. This is because electrons cannot get enough energy to overcome their atomic bonding. The photoelectric effect furthered wave
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15.2 Born-Haber Cycle Our calculations of enthalpies so far have involved covalent substances. Now we need to look at the enthalpy changes involved in the formation of giant ionic lattices. Lattice enthalpy is defined as either the: ’the enthalpy change that occurs when one mole of a solid ionic crystal is broken into its ions in the gaseous state‚ at standard temperature and pressure. Because all the bonds in the ionic lattice are broken‚ it is an endothermic process‚ ∆H is positive. ’ The
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