Connor Shortall AP Biology Vocabulary List for Chapters 1-5 Chapter 1 Properties of life a. Order: Molecules in living things are arranged in specific structures. b. Reproduction: Organisms will reproduce their own kind; life comes from life c. Growth & Development - DNA directs the pattern of growth and development‚ producing an organism that is characteristic of its species d. Energy Processing- Organisms take in energy though various methods and make it usable e. Response to the Environment -
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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 bonds are shorter than double bonds. 2. Which of the following represent the Lewis structure for Cl
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each? 3. Distinguish between anions and cations. 4. What are the four major chemical elements of the body? 5. Distinguish between an ionic and a covalent chemical bond. 6. Define electronegativity. 7. Describe how polar covalent bonds are formed and how electrical charges are distributed in them. 8. Describe how nonpolar covalent bonds are formed and how electrical charges are shared in them. 9.
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Task 1: Assessment criterion 2.1 Determine the enthalpy change for the reaction (ΔHfθ) between zinc and copper sulphate solution‚ giving full practical details. Aim To determine the enthalpy change for the reaction between zinc and copper sulphate. Zn (s) + CuSO4 (aq) ZnSO4 (aq) + Cu (s) Introduction In the study of energy (thermodynamics) the system refers to the reacting chemicals (zinc and copper sulphate solution) and the surroundings is everything else (atmosphere
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------------------------------------------------- 1.Top of Form Arrange the following elements in order of increasing electronegativity: germanium‚ bromine‚ selenium‚ arsenic Please answer this question according to the general rules you have learned regarding periodic trends. DO NOT base your answer on tabulated values since exceptions may occur. | germanium smallest arsenic selenium bromine largest Feedback: Electronegativity is the ability of an atom in a molecule to attract
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within types of covalent and non-covalent bonding. Covalent bonding involves the pairing of electrons that are shared between atoms‚ whereas non-covalent bonding involves the attraction of electromagnetic forces between atoms. Covalent bonds are strong and non-covalent bonds are weak. Both covalent and non-covalent bonds relate in a sense of stability as covalent bonds are most stable when its outmost electron shell filled‚ typically octet (or eight electrons)‚ and non-covalent bonds are stable when
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Lewis structure The Lewis structure is used to represent the covalent bonding of a molecule or ion. Covalent bonds are a type of chemical bonding formed by the sharing of electrons in the valence shells of the atoms. Covalent bonds are stronger than the electrostatic interactions of ionic bonds‚ but keep in mind that we are not considering ionic compounds as we go through this chapter. Most bonding is not purely covalent‚ but is polar covalent (unequal sharing) based on electronegativity differences
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1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. 17. 2015SP-BIOL-1408-43440 Biology for Non-Science Majors I_Pebble Barbero EXAM ONE Cheating Question – I acknowledge I won’t cheat. You expose the bacteria Staphylococcus aureus to low levels of antibiotic methicillin. The surviving bacteria are then exposed to higher concentrations of methicillin and the process repeated until a strain of methicillin-resistant S. aureus (MRSA) was generated. To test your hypothesis‚ you perform an experiment
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reactions involve the making and breaking of bonds. It is essential that we know what bonds are before we can understand any chemical reaction. To understand bonds‚ we will first describe several of their properties. The bond strength tells us how hard it is to break a bond. Bond lengths give us valuable structural information about the positions of the atomic nuclei. Bond dipoles inform us about the electron distribution around the two bonded atoms. From bond dipoles we may derive electronegativity data
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Chemical bonds are what make up the world. In bonds‚ elements are held together and form compounds that may have new physical and chemical properties. There are two main kinds of bonds‚ they ionic and covalent. In bonding the goal of the atoms involved is to reach a level of stability with less energy. In order to reach the epitome of stability‚ as in the case of noble gases‚ an atom strives to complete its outer shell. Either losing or gaining electrons may do this‚ which concludes in an ionic bond
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