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File A File A Presentation Transcript

  • 2 Chemical Principles
    • Chemistry is the study of interactions between atoms and molecules.
    • The atom is the smallest unit of matter that enters into chemical reactions.
    • Atoms interact to form molecules.
    Chemistry
  • The Study of Atoms
    • Atoms are composed of
    • Electrons: Negatively charged particles
    • Protons: Positively charged particles
    • Neutrons: Uncharged particles
  • The Study of Atoms
    • Protons and neutrons are in the nucleus.
    • Electrons move around the nucleus.
    Figure 2.1
  • Chemical Elements
    • Each chemical element has a different number of protons.
    • Isotopes of an element are atoms with different numbers of neutrons. Isotopes of oxygen are:
    16 8 O 17 8 O 18 8 O
  • Table 2.1
  • Electronic Configurations
    • Electrons are arranged in electron shells corresponding to different energy levels.
  • Electronic Configurations Table 2.2 (1 of 2)
  • Electronic Configurations Table 2.2 (2 of 2)
  • How Atoms Form Molecules: Chemical Bonds
    • Atoms combine to complete the outermost shell.
    • The number of missing or extra electrons in this shell is known as the valence.
  • How Atoms Form Molecules: Chemical Bonds
    • A compound contains different kinds of atoms. H 2 O
    • The forces holding atoms in a compound are chemical bonds.
  • How Atoms Form Molecules: Chemical Bonds
    • The number of protons and electrons is equal in an atom.
    • Ions are charged atoms that have gained or lost electrons.
    Figure 2.2a
  • Ionic Bonds
    • Ionic bonds are attractions between ions of opposite charge. One atom loses electrons and another gains electrons.
    Figure 2.2b
  • Covalent Bonds
    • Covalent bonds form when two atoms share one or more pairs of electrons.
    Figure 2.3a
  • Hydrogen Bonds
    • Hydrogen bonds form when a hydrogen atom covalently bonded to an O or N atom in another molecule.
    Figure 2.4
  • Molecular Weight and Moles
    • The sum of the atomic weights in a molecule is the molecular weight.
    • One mole of a substance is its molecular weight in grams.
    H 2 O 2H = 2  1 = 2 O = 16 MW = 18 1 mole weighs 18g
  • Chemical Reactions
    • Chemical reactions involve the making or breaking of bonds between atoms.
    • A change in chemical energy occurs during a chemical reaction.
    • Endergonic reactions absorb energy.
    • Exergonic reactions release energy.
    • Occur when atoms, ions, or molecules combine to form new, larger molecules.
    • Anabolism is the synthesis of molecules in a cell.
    Synthesis Reactions A + B AB Atom, ion, or molecule A  Atom, ion, or molecule B New molecule AB Combines to form
    • Occur when a molecule is split into smaller molecules, ions, or atoms.
    • Catabolism is the decomposition reactions in a cell.
    Decomposition Reactions A + B AB Atom, ion, or molecule A  Atom, ion, or molecule B New molecule AB Breaks down into
  • Exchange Reactions
    • Are part synthesis and part decomposition.
    NaCl + H 2 O NaOH + HCl 
    • Can readily go in either direction.
    • Each direction may need special conditions.
    Reversible Reactions A + B Water   AB Heat