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Chemical Bonds and Mixtures in Anatomy & Physiology

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이 집합의 용어 (20)

  • What are the three basic types of mixtures?

    Solutions, colloids, and suspensions.

  • Define a solution in terms of mixtures.

    A homogeneous mixture with particles evenly distributed; solvent is the substance in greatest amount, solute is dissolved in solvent.

  • What characterizes a colloid mixture?

    A heterogeneous mixture with larger particles than solutions; particles scatter light but do not settle out; can undergo sol-gel transformations.

  • What is a suspension in mixture terms?

    A heterogeneous mixture with very large particles that settle out over time; example is blood where cells settle out if left undisturbed.

  • List three main differences between mixtures and compounds.

    Mixtures do not involve chemical bonding, can be separated physically, and can be heterogeneous or homogeneous; compounds involve chemical bonds, separated chemically, and are homogeneous.

  • What is the role of electrons in chemical bonding?

    Electrons in the outermost shell (valence shell) determine chemical reactions and bond formation by gaining, losing, or sharing electrons to achieve stability.

  • What is the octet rule in chemical bonding?

    Atoms tend to have 8 electrons in their valence shell to achieve stability, except hydrogen and helium which are stable with 2 electrons.

  • What makes an element chemically inert?

    Having a complete valence shell (full outermost energy level), making it nonreactive, like noble gases.

  • Define ionic bonds.

    Bonds formed by the transfer of valence electrons from one atom to another, creating oppositely charged ions that attract each other.

  • What happens to sodium and chlorine atoms during ionic bond formation?

    Sodium transfers its lone valence electron to chlorine, forming Na+ and Cl- ions that attract to form sodium chloride.

  • Describe covalent bonds.

    Bonds formed by sharing two or more valence electrons between atoms; can be single, double, or triple bonds depending on electron pairs shared.

  • What is the difference between polar and nonpolar covalent bonds?

    Nonpolar bonds share electrons equally; polar bonds share electrons unequally, creating partial charges on atoms.

  • Give examples of molecules with nonpolar covalent bonds.

    Nitrogen (N2), methane (CH4), oxygen (O2), and carbon dioxide (CO2).

  • Why is water a polar molecule?

    Oxygen is more electronegative than hydrogen, pulling shared electrons closer and creating a partial negative charge on oxygen and partial positive charges on hydrogens.

  • What is a hydrogen bond?

    A weak attraction between a hydrogen atom with a partial positive charge and an electronegative atom of another molecule or within the same molecule.

  • How do hydrogen bonds affect water's properties?

    They create high surface tension and allow water molecules to stick together, enabling phenomena like water striders walking on water.

  • Compare the relative strengths of covalent, ionic, and hydrogen bonds.

    Covalent bonds are strongest, ionic bonds are intermediate, and hydrogen bonds are weakest.

  • What are van der Waals interactions?

    Weak attractions due to asymmetrical electron distribution creating temporary regions of positive and negative charge, allowing atoms and molecules to stick when very close.

  • What is the valence shell and why is it important?

    The outermost electron shell of an atom; electrons here have the most potential energy and participate in chemical bonding.

  • How many electrons can the first three electron shells hold?

    Shell 1: 2 electrons, Shell 2: 8 electrons, Shell 3: 18 electrons.