Topic 6 Microscopic World II Unit 23 Shapes of molecules Unit 24 Bond polarity and intermolecular forces Key C o ncepts Microscopic World II Shapes of molecules • Covalent molecules with non-octet structures • Shapes of molecules • The VSEPR theory • Molecular crystals of buckminsterfullerene (C60) • Carbon nanotubes Bond polarity and intermolecular forces • Electronegativity and bond polarity • Van der Waals’ forces • Factors affecting the strength
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CH3CH2N(CH3)2 (d) (CH3)3CNH2 5. Which of the following elements has the highest electronegativity? (a) C (b) P (c) Si (d) Cl 6. Which of the following is an ionic bond? (a) F-F (b) C-H (c) Li-O (d) C-N 7. Which of the following molecules has a molecular dipole? (a) 1 (b) 2 (c) 3 (d) 4 PAGE 2 8. Which of the following represents an sp3 hybridized atomic orbital containing the
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Ion Exchange Chromatography Discussion: The first exercise preformed in this lab was ion exchange chromatography. The purpose of this experiment is to separate molecules based on their differences in charge. Since it is based on charge the amino acids in the cation exchange column‚ if negatively charged‚ flow through the column first because they don’t want to bind to the sodium ions. The positively charged ions will elute last at the highest ph because they bind to the negatively charged beads
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factors. If the oil processing machinery have heat on oil‚ then the change of oil viscosity and oil binding. Steam heating effect of the process of speculation‚ make the billet in high temperature‚ and weaken the enhanced oil thermal motion of molecules and molecular cohesion‚ resulting in green oil viscosity and surface tension reduction‚ weakening the binding of grease and part of the green gel and enhance the mobility of the oil‚ oil get rid of protein hydrophobic adsorption force and to create
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nonpolar covalent bonds‚ and ionic bonds. 4. Why is water a polar molecule? Draw a water molecule and show the δ+ and δ- poles. Water is a polar molecule because electrons in a water molecule are not shared equally‚ and electrons are more strongly attracted to and spend more time orbiting
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or process. We consider two colliding diatomic molecules system. For simplicity we assume that the molecules do not interact chemically and that each molecule is homonuclear (molecules composed of only one type of element). The molecules are in a low-density gas‚ so that we need not consider interactions with other molecules in’ the neighborhood. In Fig. 0.3-1 we show the collision between the two homonuclear diatomic molecules‚ A and B‚ and in Fig. 0.3-2 we show the notation
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negative. a place where Ψ is positive. a place where Ψ = 0. a place where Ψ2 is large. a place where Ψ2 is negative. Ans: C Topic: Atomic Orbitals‚ Molecular Orbitals 2. When the 1s orbitals of two hydrogen atoms combine to form a hydrogen molecule‚ how many molecular orbitals are formed? A) 1 B) 2 C) 3 D) 4 E) 5 Ans: B Topic: Atomic Orbitals 3. Which principle(s) or rule must be used to determine the correct electronic configuration for carbon in its ground state? A) Aufbau Principle
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hydrogen molecules and one negatively charged oxygen molecule. Water molecules have uneven charge distribution as one end of the molecule is slightly positive and the other slightly negative‚ this is called polar. Ionic substances such as sodium chloride dissolve easily in water because the positively and negatively charged ions are separated due to the dipole nature of water. As water is dipolar‚ the positively charged atoms of one water molecule attracted the negatively charged molecule of another
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chemical equations. * To interpret chemical reactions. * To understand equilibrium reactions and the factors that can affect them. * Molecular Mass / Formula Mass * Is the sum of the atomic masses of all the atoms present in one molecule of that compound. Example: the molecular mass of sodium bromide‚ NaBr‚ is 103‚ which represents the sum of the atomic mass of sodium (23) plus that of bromide (80). * Calculating the Molecular Mass (Formula Mass) of a Compound * To find
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temperature outside affect how fast molecules move inside objects? Charles Law helps us understand how molecules move in different temperatures. It states that increasing the temperature of a constant pressure volume of gas causes individual gas molecules to move faster (Andrew Staroscik Staroscik 9/19/16)‚ and the volume is proportional to the absolute temperature of a gas at (Todd Helmenstine 10/16/16). Therefore‚ as the temperature increases‚ so does the speed of the molecules‚ and when the temperature
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