CHEMISTRY Chemical Bonds

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Natalie
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13203
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CHEMISTRY Chemical Bonds
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2010-04-05 21:44:30
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Chemical Bonds
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  1. What is the Octet Rule?
    • Atoms with 8 valence elecrons are stable (unreactive)
    • *Atoms without this stable octet react so they end up with 8 valence electrons
  2. What are chemical reactions?
    • Rearrangements of atoms as they form stable octets and go toward lower energy states
    • *Old bonds break, new bonds form
  3. When do bond formations occur?
    • When atoms or molecules collide
    • *Involves valence electrons (D sublevel electrons in transition metals may also be involved
    • *Is exothermic
  4. What kind of reaction is breaking bonds?
    • Endothermic
    • *Must replace energy given off when bond was formed
  5. When is a reaction exothermic?
    If the energy given off by forming new bonds is greater than the energy needed to break old bonds
  6. When is a reaction endothermic?
    If the energy needed to break old bonds is greater than the energy given off by forming new bonds
  7. What is activation energy?
    • The energy needed to get a reaction started
    • *Used to break old bonds
    • *Continuous for endothermic reactions, not continuous for exothermic
  8. What is a chemical bond?
    • A force of attraction between atoms due to opposite charges
    • *Electrons may be transferred or shared
  9. What is an ion?
    An atom with the wrong number of electrons
  10. What is a cation?
    An atom losing electrons that is positively charged
  11. What is an anion?
    An atom gaining electrons that is negatively charged
  12. What is an ionic bond?
    • A force of attraction due to the transfer of one or more valence electrons from one atom to another
    • *Atoms attract due to opposite charges
  13. What is the resulting compound of ionic bonds?
    An ionic compound
  14. An ionic compound is _______ (charge)
    Arranged in regular repeating patterns called ______ which are not molecules
    Have _____ bonds, causing them to be _____ at room temperature and to have high _____ point
    Separate into _____ (dissociate) when dissolved in water
    Aqueous solutions conduct ______
    They are _____
    • neutral
    • crystals
    • strong, brittle, melting
    • ions
    • electricity
    • electrolytes
  15. What is a covalent bond?
    • A force of attraction due to sharing one or more pairs of valence electrons, with each atom contributing one electron in a pair
    • *The electron pair jumps back and forth between atoms
    • *Causes temporary charges that result in attraction
    • *Makes covalent compounds
    • *Can havedouble and triple bonds that are stronger than single bonds
  16. Covalent compounds are also called _____ compounds
    Has a _______ charge
    Form _____
    Do not ______
    Not _____
    Have weak intermolecular forces, causing them to be _____ at room temperature
    Have ___ melting points
    • molecular
    • neutral
    • molecules
    • dissociate
    • electrolytes
    • gases or liquids
    • low
  17. What is the rearrangement of orbitals in a valence shell into equal energy orbitals?
    • Hybridization
    • *Allows a larger number of equal energy covalent bonds
    • *Carbon is an example
  18. What are large covalently bonded structures?
    • Network solids
    • *The number of bonds gives these a great strenght and very high melting point
    • *Example: diamond
  19. What is a molecule?
    Two or more atoms Covalently bonded
  20. What is a compound?
    Two or more different atomschemically bonded
  21. Molecule or Compound?
    H-Cl
    NaCl
    N=N
    • Molecule and compound
    • Not a molecule, but a compound
    • A molecule, not a compound
  22. What are two atoms of the same element covalently bonded?
    Diatomic molecules
  23. What are the seven diatomic elements?
    • H, N, O, F, Cl, Br, I
    • *Written H2, N2 etc.
  24. What are metallic bonds?
    • A force of attraction caused by sharing loosely held valence electrons among many metal ions
    • *This results in the special properties of luster, conductivity, malleability and ductility
    • *Usually between like atoms in a piece of the element
    • *Form alloys, not compounds
    • *Mixtures show individual metallic properties
  25. What is a bond formed between a metal and a nonmetal?
    Ionic
  26. What is a bond formed between two nonmetals?
    Covalent
  27. What is a bond formed between two metals?
    Metallic
  28. What are the:
    Phases at room temperature
    Melting point
    Conductivity when melted
    Water solubility
    Conductivity of water solution
    of ionic versus covalent compounds?
    • Crystalline solid ....... Solid, liquid or gas
    • High ....................... Low
    • Yes .........................No
    • High.........................Low
    • Yes..........................No
  29. What is the measure of an atom's attraction for electrons in a covalent bond?
    • Electronegativity
    • *EN
    • *Scale from 0 to 4
  30. What is the most electronegative element?
    Flourine, because it only needs to gain one electron and it is the smallest. Not Hydrogen because it only has one proton pulling on it.
  31. What is the least electronegative element?
    Francium
  32. Electronegativity ______ from left to right on the periodic table
    • increases
    • *This is due to the increase in the number of protons and smaller atomic size
  33. Electronegativity __ as you move down a group on the periodic table
    • decreases
    • *This is due to teh increase in atomic size and shielding effect of electrons between the nucleus and valence shell
  34. If the difference in electronegativity is greater than 2.0, the bond is _____
    If it is less that 2.0, it is ______
    • Ionic
    • Covalent
  35. What is a bond that has perfect sharing?
    • Pure covalent bond
    • *Occurs when difference in electronegativity equals 0
    • *Diatomic elements have pure covalent bonds
  36. What is a covalent bond in which the difference in electronegativity is greater than 0.4
    • A polar covalent bond
    • *Has a positive and negative end
    • *Negative end has the higher electronegativity
    • *The greater the difference in electronegativity, the stronger the polarity
  37. When is there a nonpolar covalent bond?
    • When the difference in electronegativity is less than or equal to 0.4
    • *Unequal sharing so little that polaritiy is not significant
  38. What are molecules with polar bonds and a geometry that allows poles to occur?
    • Polar molecules
    • *Also called dipoles
    • *Polarity affects physical properties
  39. What are some properites affected by polarity?
    • Phase at room temperature
    • Melting point/Boiling point (Polar have high BP/MP)
    • Viscosity (Polar are more viscous)
    • Density (Polar are more dense)
    • Solubility (Polar solvents dissolve polar solutes)
  40. What kind of bond has shared electrons that come from one atom
    • Coordinate covalent bonds
    • *Occurs in some polyatomic ions
  41. What are models showing bonding and nonbonding electrons in molecules?
    • Lewis structures
    • *Primarily for covalent molecules
    • *Doesn't show molecular geometry
  42. What are the bonding rules for the families?
    • H and Halogens - 1
    • O Family - 2
    • N Family - 3
    • C Family - 4
    • B - 3
  43. What is resonance?
    • When molecules have more than one correct lewis structure
    • *Electrons shift between these arrangements
  44. What is the difference between the number of electrons each atom has in the lewis structure and its valence electrons?
    • Formal Charges
    • *Always occurs in ions
    • *Atoms with more electrons are negative, with more protons are positive
  45. What are the bonding rules for ions?
    • H and Halogens - 1
    • O family - 1, 2, or 3
    • N family - 2, 3, or 4
    • C family - 4
    • B - 4
  46. What is VSEPR?
    • Valence shell electron -pair repulsion
    • *Method of predictiong molecular shape
  47. What does A, X and E stand for?
    • A - central atom
    • X - atom bonded to a
    • E - lone pairs
  48. What is the VSEPR notation for, predicted shape, and bond angles for:
    2 atoms bonded to a
    3 atoms bonded to a
    4 atoms bonded to a
    3 atoms bonded to a and 1 lone pair
    2 atoms bonded to a and 2 lone pairs
    • AX2, linear, 180
    • AX3, trigonal planar, 120
    • AX4, tetrahedral, 109.5
    • AX3E, trigonal pyramidal, 107
    • AX2E2, bent, 104.5
  49. Lone pairs ______ more than bonded electrons
    • repel
    • *This affects tetrahedral shapes AX3E and AX2E2
    • *Actual angles known only by experiment
  50. Polarity:
    Polar bonds ______ polar molecule
    Strongly affected by _____
    After determing shape, look for _____
    ____ reduces polarity
    Lone pairs are _____ sites
    • do not equal
    • shape
    • positive and negative sites
    • symmetry
    • negative

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