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60 Cards in this Set
- Front
- Back
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electromagnetic radiation
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light energy spetrum, how energy travels through space
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wavelength
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distance between peaks/troughs of a wave.
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frequency
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number of waves(cycles) per second that pass a given point in space
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Planck's constant (h)
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6.626x10^-34 J.s
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quantized
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energies occur at specific values, not continuous
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photons
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particles of light
each one deals with one electron individually |
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photoelectric effect
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electrons emitted from metal surface when light strikes it
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continuous spectrum
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when white light passes through a prism
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atomic line spectrum
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each energy level is the position in PE relative to the nucleus
specific set, lines, not continuous each level jump gives off photon with specific wavelength and frequency |
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E = ?
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hv
h=6.626x10^-34 v=frequency |
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v=
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c/π
c=speed of light=3.00* |
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relationship between energy, frequency, and wavelength
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energy+frequency=direct
frequencey+wavelength=inverse wavelength+energy=inverse |
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If there is insufficent energy to remove the elctron the wavelength should be __________?
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decreased
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photoelectric effect occurs at ______________?
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high frequency and energy
low wavelength |
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Bohr model
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electrons travel in ciruclar orbits at differend energy levels
only works for hydrogen |
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quantum model
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wave-like characteristics
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ground state
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lowest possible energy state
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orbital
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par of electrons
four types (spdf) |
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quantum numbers
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characterization of orbitals based by series of numbers
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principle quantum number
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size and energy of the orbital
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angular momentum quantum number
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relative to the shape
(sphere, bumbshell, cloverleaf) |
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magnetic quantum number
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identifies the orbitals
orientation |
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shell
subshell |
energy levels of electrons, similar PE
same exact PE |
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electron spin quantum number
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identifies the specific electron
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polyelectronic atom
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atom with more than one atom
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Aufbau principle
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protons are added one by one to the nucleus to build up elements.
electrons are similarly added to the hydrogen orbitals, lowest energy level first |
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Hundt Rule
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lowest energy configuration for an atom is the one having the max number of unpaired elecrons
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valence electrons
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electrons in the outermost principal quantum level of an atom
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core electrons
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inner electrons
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first ionization energy
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energy required to remove the highest energy electron of an atom
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electron affinity
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energy chance associated iwth the addition of an electron
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isoelectronic
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ions containing the same number of electrons
more protons is smaller radius |
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lattice energy
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change in energy that takes place when separated gaseous ions are packed together to form an ionic solid
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which is bigger? cation or anion, compared to the non ionic atom
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cation is smaller, closer to nucleus
anion is larger, farther from nucleus |
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how strong is electrostatic attraction?
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depends on charge and distance between the charges
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bond energy
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energy required to break/form the bond
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bond length
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distance where energy is minimal
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covalent bonding
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electrons are shared by nuclei
2 nonmetals |
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single, double, triple bond
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# of pairs of electrons
never single electrons |
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lone pairs
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just 2 electrons, not bonded
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bonding pairs
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bond contains 2 electrons shared between to atoms
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Lewis structure
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shows the vlanence electron arrangment among atoms in the molecule
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octet rule
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each atoms is surrounded by eight electrons
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resonance
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when more than one valid Lewis structure can be written for a particular molecule
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formal charge
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difference bewteen the number of valence electrons on the free atom and the number of valence electrons assigned to the atom in the molecule
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covalent bond
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shared electrons
overlapping orbitals electrostatic attraction(attraction of a negative to a positive) |
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the formation of a bond is always ___________?
breaking a bond is always _______________? |
exothermic
endothermic |
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how to draw Lewis structures...
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sum valence electrons
assume single bonds between atoms complete octet of terminal atoms place remaining electrons on central atom |
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evaluating formal charge
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the most likely to be naturally found is the one with the formal charge closest to ZERO
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molecular structure
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three dimensional arrangement of atoms in a molecule
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VSEPR model
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valence shell electron pair repulsion
best arrangement of for a given number of electron pairs is the one that minimizes the repulsions among them |
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number of electron pairs=electron pair structure
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2-linear
3-trigonal planar 4-tetrahedral 5-trigonal bipyramidal 6-octahedral |
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nonbonding pairs require more room than bonded pairs.
equitoral have more space |
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electronegativity
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ability of an atom to attract the shared electrons together
teh most electronegative element is F |
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dipole
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separation of charge
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polar
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unequal distribution of charge
greater difference=greater polarity |
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hybridization
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mizing of atomic orbitals to form special orbitals for bonding
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sigma bond
pi bond |
hybridized, covalent bond, regions overlap between two nuclei
non-hybridized, regions overlap when not between two nuclei |
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hybrid orbital
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bonding orbital obtained when 2 or more atomic orbitals of the same atom combine to prepare for covalent bond info
form sigma bonds |
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how to hybridize
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draw lewis structure
determine electron-pair geometry specify hybrid orbitals needed single bond-1sigma double bond- 1sigma, 1pi triple bond- 1 sigma, 2pi |
