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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times to make a polymer and is used to link subunits in lipid molecules. In condensation reactions a water molecule is released‚ a covalent bond is formed and a larger molecule is formed by the bonding together of smaller molecules. When a larger molecule splits this is called a hydrolysis reaction. In hydrolysis reactions a water molecule is used‚ a covalent bond is broken‚ smaller molecules are formed from splitting larger ones. * State the structural difference between α and β glucose
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secondary structure refers to segments of polypeptide chains which are folded or coiled‚ as a result of hydrogen bonding on the polypeptide backbones. (Reece‚ 2011). The electrognetaive oxygen and nitrogen atoms both have a partial negative charge and attach to the weakly positive hydrogen atom. (Reece‚ 2011). There are two secondary structures that can form: an ɑ helix‚ with hydrogen bonding every fourth amino acid‚ and a β pleated sheet when the polypeptided backbones bond to form parallel or anti-parallel
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find Sodium Chloride on the periodic table because Sodium Chloride is a molecule made up of two atoms: Sodium and Chloride. 3. Sodium Chloride represents two atoms that together form a molecule: NaCl. Na: Sodium and Cl: Chloride 4. An ionic bond occurs when two or more ions (an atom whose number of elections differs from its number of protons) bond together because of their opposite charge. They are drawn to each other like magnets because of their opposite charge. 5. Sodium Chloride
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Chem 201 /HW#10 Chapter 9 Electronegativity Table: use this table to answer Q [pic] 1. Bromine tends to form a monatomic ion which has the electronic configuration of a noble gas. What is the electron configuration of that noble gas? a. 1s2 2s2 2p6 3s2 3p6 3d10 4p6 b. 1s2 2s2 2p6 3s2 3p6 4p6 4d10 c. 1s2 2s2 2p6 3s2 3p6 4s2 4p6 d. 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 e. 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 2. Which ion of
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gain enthalpy and ionization energy of an atom are –a and +b eV respectively. The electronegativity of that atom on Mulliken scale is given by (A) a – b (B) (b – a )/2 (C) a + b (D) (a + b)/2 (3) The atomic radii of Li is 1.23 A0 and ionic radius of Li+ is 0.76 A0. The fraction of the volume occupied by 2s electron in Li is (A) 0.764 (B) 0.184 (C) 0.595 (D) 0.236 (4) Photons of monochromatic light having just sufficient energy to ionize Ar-atom are incidened over the
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They’re sub units/monomers and.. Peptide bond: Where is it? Is it covalent or ionic? Amino acids are linked together by peptide bonds to form polypeptide chains and it’s covalent. Primary‚ secondary‚ tertiary‚ and quaternary structure and examples. Primary: One long‚ squiggly line made up of amino acids Secondary: Occurs when the sequence of amino acids are linked by
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chart and state how many bonds each of the CHNOPS elements can form. Carbon | Hydrogen | Nitrogen | Oxygen | Phosphorous | Sulfur | 4 | 1 | 3 | 2 | 3 or 5 | 2 | 3. Create a Venn Diagram to compare and contrast polar covalent bonds‚ 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
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Which of the following types of molecules are the major structural components of the cell membrane? A) phospholipids and cellulose B) nucleic acids and proteins C) phospholipids and proteins D) proteins and cellulose E) glycoproteins and cholesterol For the following questions‚ match the labeled component of the cell membrane (Figure 7.1) with its description. [pic] Figure 7.1 5) peripheral protein 6) cholesterol 9) glycolipid 11) The presence of cholesterol in
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gained electrons‚ cation lost electrons) Electron shells‚ orbitals‚ valency‚ rule of 8 Bonds = ionic‚ covalent (polar‚ nonpolar)‚ hydrogen‚ Van der walls Electronegativity Relationship of molecular shape and function of molecules (morphine and endorphins) Making and breaking chemical bonds (photosynthesis – co2 + h20 = glucose and 02) Balancing chemical equations CH3 Water – hydrogen bonding very important Cohesion (like molecules)‚ Adhesion(differing) Moderate temperature (aborb heat by
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