__________ paired and __________ unpaired electrons. A) 4‚ 2 B) 0‚ 5 C) 2‚ 5 D) 6‚ 1 E) 4‚1 2. Which of the following would have to gain two electrons in order to achieve a noble gas electron configuration? O Sr Na Se Br A) Sr B) Br C) Sr‚ O‚ Se D) Na E) O‚ Se 3. The electron configuration of the S2- ion is __________. A) [Ne]3s23p2 B) [Ne]3s23p6 C) [Kr]3s22p-6 D) [Ar]3s23p2 E) [Ar]3s23p6 4. The ion NO- has __________ valence electrons. A) 10 B) 16 C) 12 D) 14 E) 15 5
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TextBooks Sr No T-1 T-2 Title Engineering Chemistry Chemistry Reference Books Sr No R-1 Other Reading Sr No OR-1 OR-2 OR-3 OR-4 OR-5 OR-6 OR-7 Journals articles as Compulsary reading (specific articles‚ complete reference) http://onlinelibrary.wiley.com/journal/10.1002/(ISSN)1097-4601 ‚ http://www.springer.com/chemistry/electrochemistry/journal/10800 ‚ http://www.sciencedirect.com/science/journal/13882481 ‚ http://www.springerlink.com/content/100224/ ‚ http://www.sciencedirect.com/science/journal/00108545
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move one element to the right on the periodic table which ONE of the following is always TRUE? A. an extra electron is added to a previously empty orbital B. the charge on the atom increases by 1 C. the number of neutrons increases by 1 D. the number of protons increases by 1 E. all of the above 2. Which ONE of the following best describes what happens when an electron moves to a lower energy shell? A. the nucleus decays B. a quantum of energy is emitted C. a quantum of
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Objectives of the course • Wave mechanics / Atomic orbitals (AOs) – The basis for rejecting classical mechanics (the Bohr Model) in the treatment of electrons – Wave mechanics and the Schrödinger equation – Representation of atomic orbitals as wave functions – Electron densities and radial distribution functions – Understanding the effects of shielding and penetration on AO energies • Bonding – Review VSEPR and Hybridisation – Linear combination of molecular orbitals (LCAO)‚ bonding
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chemical properties Nonmetals are on the right side of the periodic table (with the exception of H). Metalloids border the stair-step line (with the exception of Al‚ Po‚ and At). Metals are on the left side of the chart. When atoms lose or gain electrons‚ they become ions. Cations are positive and are formed by elements on the left side of the periodic chart. Anions are negative and are formed by elements on the right side of the periodic chart. Ionic compounds (such as NaCl) are generally formed
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Lensey Ford Mrs.Beckwith Pre-Ap Physical Science 23 November 2015 Revolving with Electrons Have you ever wondered exactly how the elements on the periodic table are organized‚ what the groups on the periodic table mean‚ and how electrons work in an atom‚ compound‚ and chemical bond? The way elements are organized on a periodic table has to do with the characteristics that they hold. There are groups‚ periods‚ compound formation and color coordination in a periodic table. The periodic
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σ-bonding‚ and a degree of π-back bonding‚ which is well observed in carbonyl containing species. π-back bonding occurs when empty π* (anti bonding) orbitals accepts electrons from the metal center’s d-orbitals. Back bonding allows metals like Mo to exist in a wide range of oxidation states‚ as it allows the metal to distribute electron density to the ligand. When back bonding occurs‚ it causes the M-C bond to shorten‚ and the C-O bond lengthens6. In this lab‚ molybdenum hexacarbonyl (Mo(CO)6) was
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97.8°C) melts at a considerably higher temperature than the element (neon) which precedes it in the Periodic Table.Sodium has the electronic structure 1s22s22p63s1. When sodium atoms come together‚ the electron in the 3s atomic orbital of one sodium atom shares space with the corresponding electron on a neighbouring atom to form a molecular orbital - in much the same sort of way that a covalent bond is formed.The difference‚ however‚ is that each sodium atom is being touched by eight other sodium
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individual atoms forming the bonds. 1. The new orbitals are called molecular orbitals. ii. Electrons shared by atoms in a molecule reside in the molecular orbitals. iii. Molecular orbitals are like atomic orbitals in that they have specific shapes and specific energies and they can each accommodate a maximum of two electrons. iv. Two electrons residing in the same molecular orbital must have opposite spins. v. The number of molecular orbitals
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The atom is a basic unit of matter that consists of a dense central nucleus surrounded by a cloud of negatively charged electrons. Atoms lack a well-defined outer boundary‚ so their dimensions are usually described in terms of an atomic radius. This is a measure of the distance out to which the electron cloud extends from the nucleus. However‚ this assumes the atom to exhibit a spherical shape‚ which is only obeyed for atoms in vacuum or free space. Atomic radii may be derived from the distances
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