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33 Cards in this Set
- Front
- Back
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electrons and photons travel in:
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waves
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the distance between the crest and the imaginary midpoint line is the:
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amplitude
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characteristics of a long wavelength:
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low frequency, low energies
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examples of a continuous spectrum:
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sunlight
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a packet of energy is called a:
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quantam
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synonym for discontinuous spectrum:
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bright line spectrum
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how are the wavelength and frequency of light related?
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Inverses
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what is ionization energy?
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the minimum amount of energy required to remove an electron from an atom
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Why are noble gases particularly stable and relatively unreactive?
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the last energy level is filled
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define isoelectronic:
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When two elements and/or ions have the same electronic configurations
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name the major groups on the periodic table:
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http://www.corrosionsource.com/handbook/periodic/periodic_table.gif
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characteristics of metals:
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chemically reactive, shiny, high density, ductile and malleable, high melting point, conducts electricity
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characteristics of non-metals:
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conducts heat and electricity poorly, forms acid oxides, dull and brittle, low density and melting point
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characteristics of semi-metals(metalloids):
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semiconductors, not malleable
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the 8 metalloids:
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Boron (B)
Silicon (Si) Germanium (Ge) Arsenic (As) Antimony (Sb) Tellurium (Te) Polonium (Po) |
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what is a group on the periodic table and how many are there?
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vertical columns, there are 18
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What is a period on the periodic table, how many are there?
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horizontal rows
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ionization energy
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the energy required to remove an electron from a gaseous atom
as you go across the periodic table, energy increases as you go down the periodic table ionization energy decreases |
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electronegativity
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the tendency for an atom to attract electrons to itself when it is chemically combined with another element
as you go across, increases as you go down, decreases |
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shielding
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across, constant
down, increase |
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nuclear charge
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the total charge of all the protons in the nucleus, it has the same value as the atomic number
across, increases down, increases |
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valence electrons
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amount of electrons in the last energy level. Valence electrons are important in determining how an element reacts chemically with other elements: The fewer valence electrons an atom holds, the less stable it becomes and the more likely it is to react
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moving Left --> right
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Atomic Radius Decreases
Ionization Energy Increases Electronegativity Increases |
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moving Top --> bottom
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Atomic Radius Increases
Ionization Energy Decreases Electronegativity Decreases |
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ionic compounds
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transfer electrons from one atom to another
high melting points dissolve in water conduct electricity |
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covalent compounds
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share electrons
low melting points dissolve in methanol do not conduct electricity |
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electronegativites...
less than or equal to .2 |
non-polar covalent
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.3-1.6
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polar covalent
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greater than or equal to 1.7
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ionic
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lewis dot structures
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-For molecules with only 2 elements, arrange the atoms symmetrically
-“COOH” is a carboxylic acid (both O’s bond to the C and the H goes on one of the O’s) Hydrogen and halogens cannot go in the middle Write the remaining atoms in the order they appear in the formula Write the hydrogen and halogen atoms around the element they are written next to in the formula |
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VSPER theory
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a theory that predicts molecular shapes based on the idea that pairs of valence electrons surrounding an atom repel each other
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H-bonding
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Nitrogen, Oxygen or Fluorine bonded with Hydrogen
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Dispersion
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Everthing has it
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