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Biochemistry Exam 2 Key Concepts

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Terms in this set (23)

  • Ionization energy

    Ionization energy is the energy required to remove a valence electron from a neutral atom.

  • Coulomb's Law in atomic structure

    Coulomb's Law explains that ionization energy increases with greater nuclear charge and decreases with increasing atomic radius.

  • Common ion charges for group 2 elements (Be, Mg, Ca, Sr)

    These elements typically form +2 cations by losing two valence electrons.

  • Naming ionic compounds with transition metals

    Use Roman numerals to indicate the metal's oxidation state, e.g., cobalt (III) oxide is Co2O3.

  • Polarity of S–Cl and S–O bonds

    S–Cl bond is slightly polar; S–O bond is polar due to higher electronegativity difference.

  • Polarity of molecule with S, Cl, and O bonds

    The molecule is polar because of the polar S–O bond and asymmetrical shape.

  • Lewis structure and shape of SO3 2−

    SO3 2− has resonance structures with trigonal pyramidal shape due to lone pairs on sulfur.

  • Hydrogen atoms bonded to carbons in tyrosine

    Carbon A: 2 H; Carbon B: 1 H; Carbon C: 0 H (due to bonding with other atoms).

  • 3D shapes around central atoms in glycine

    Atom A: tetrahedral; Atom B: trigonal planar; Atom C: tetrahedral.

  • Structural isomers of C2H6O

    Two isomers: ethanol (alcohol group) and dimethyl ether (ether group), each with distinct smells.

  • Condensed and molecular formula of 4-aminobutyrate

    Condensed: NH2(CH2)3COOH; Molecular formula: C4H9NO2.

  • Functional groups common to all amino acids

    Amino group (-NH2) and carboxyl group (-COOH) are present in all amino acids.

  • Most polar bond in amino acid

    The O–H bond is the most polar due to the large electronegativity difference.

  • Polarity of amino acid side chain

    Side chain polarity depends on functional groups; polar side chains contain electronegative atoms like O or N.

  • Dominant intermolecular forces (IMFs) in substances

    Carbon tetrafluoride: London dispersion; Ethylamine: hydrogen bonding; Acetaldehyde: dipole-dipole interactions.

  • Functional group common to all fatty acids

    Fatty acids contain a carboxyl (-COOH) functional group.

  • Classification of lauric acid and oleic acid

    Lauric acid: saturated fat; Oleic acid: monounsaturated fat.

  • Cis or trans configuration of oleic acid

    Oleic acid is a cis fat, indicated by the kink in its carbon chain at the double bond.

  • Intermolecular attractions in coconut oil vs olive oil

    Coconut oil (lauric acid) has stronger IMFs due to saturation and straight chains, making it solid at room temperature.

  • Nonpolar amino acid side chains

    Valine and isoleucine have nonpolar side chains composed mainly of hydrocarbons.

  • Strongest attractions between amino acid side chains

    Valine and isoleucine: London dispersion forces; Lysine and glutamic acid: ionic interactions.

  • Hydrogen bonding vs other IMFs in acetamide

    Hydrogen bonding occurs when H is bonded to N, O, or F; other attractions include dipole-dipole and London dispersion.

  • Relative boiling points of pentanol, ethoxypropane, and dimethylether

    Lowest to highest: dimethylether < ethoxypropane < pentanol, due to increasing hydrogen bonding and molecular mass.