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60 Cards in this Set
- Front
- Back
which atoms are found within the nucleus of an atom
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protons and neutrons
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charge of a proton/electron?
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1.6e-19Coulombs
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atomic number(Z)
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Protons
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Mass number(A)
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Protons + Neutrons
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structure of Element from the periodic table? X^(?)_?
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X^A_Z
where A is the superscript Z is the subscript |
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isotope
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same proton#, different Neutron number
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electron <<< proton in mass
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know this
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lower electric potential of electron =
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closer to nucleus
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higher electric potential of electron =
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further from the nucleus
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trend: further from nucleus = higher energy level
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know this
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outer shell electrons that feel the least electrostatic pull towards the nucleus are _____
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valence electrons
-more likely to become involved in bonds with other atoms |
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valence electrons determine the _____ of an atom
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reactivity
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neutral state of an atom =
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equal number of electrons and protons
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gain of electrons is _____
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negative charge; anion
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loss of electrons is ______
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positive charge; cation
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electrons are found ____ the nucleus in separate but defined ______
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outside; shells or orbitals
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determine the number of protons, electrons and neutrons in Ni
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P: 28
N: 30 E: 28 |
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atomic mass
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aka the mass number (P + N)
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atomic weight
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g/mol
-look off the periodic table |
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avogadro's number
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6.02e23
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isotopes of Hydrogen
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hydrogen/protium = 1P, 1E, 0N
deuterium = 1P, 1E, 1N tritium = 1P, 1E, 2N |
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energy equation
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E =hf
E = joules f = frequency h = 6.6e-34J*s |
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Bohr model of hydrogen
angular momentum = energy of the electron = |
L = nh/2(pi)
n = quantum number h = 6.6e-34 E = -Rh/n^2 Rh = 2.2e-18 n = quantum number |
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trend within angular momentum equation?
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yes;
L ~ n since (h/2(pi)) is a constant |
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trend with energy of the electron equation?
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yes
E ~ 1/n^2 so as one goes up in quantum numbers(n) the energy is drastically increased since the E value approaches "0" which is getting larger |
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orbit with the smallest radius around the nucleus is the ______ state which corresponds to n = ?
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ground state
n = 1 |
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excited state
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n > 1
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electrons can obtain an excited state through ______
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use of heat
use of radiation |
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excited --> ground = ____
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emission of light/energy
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ground --> excited = _____
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absorption of light/energy
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emission of light occurs in _____ amounts of energy in the form of ______
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discrete/pre-determined
photons |
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electromagnetic energy equation
E = |
E = hc/lambda
h = 6.6e-34 c = 3e8 lambda = wavelength (e-9) |
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trend within the electromagnetic equation?
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yes;
E ~ 1/lambda; as lambda becomes larger(800nm) the Energy level decreases as lambda becomes smaller(closer to 0) the energy value increases this is in relation to frequency; higher frequencies produce smaller wavelengths thus higher energy outputs! |
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emitted wavelength ~ to energy transition experienced
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know this
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Bohr + Planck theory EQ
E = hc/lambda = -Rh(Ni^-2 - Nf^-2) |
know this
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trend with bohr/planck theory?
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yes; energy is proportional to frequency (inversely to lambda)
this means that the larger the difference between Ni^-2 - Nf^-2 is, the larger the energy will be ex) 1 --> 2 vs 1 --> 4 1-->2 will be smaller in energy than 1-->4 |
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electrons move within ____ around the nucleus
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orbitals
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heisenberg uncertainty principle
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can not determine position and momentum at the same time
momentum = p = mv can determine momentum and velocity though! |
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quantum numbers(4)
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n, l, M(l), M(s)
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principal quantum number
-max number of electrons? |
= n
associated with valence shell energy level and radius size max number = 2n^2 |
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difference in energy between energy levels(n)....
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decreases with increased n value
ex) 1-->2 vs 3-->4 using 1/Ni^2 - 1/Nf^2 =1 - .25 = .75 = .111 - .0625 = .04861 |
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azimuthal number
max number? |
= l
the number of subshells within an energy level max number is 4l + 2 |
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range of (l) values?
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0 to n-1
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magnetic number
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= M(l)
orbital within the subshell |
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values for M(l)
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-l to l
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M(l) values of:
s --> p --> d ---> f ---> |
s = 0
p = -1,0,1 d = -2,-1,0,1,2 f = -3,-2,-1,0,1,2,3 |
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s shell =
p shell = |
spherical
dumbbell p orbitals broken into Px,Py,Pz |
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spin number
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= M(s)
+ 1/2 - 1/2 |
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if two electrons are in the same orbital, they must have ____ spins
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opposite
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electrons in different orbitals but same M(s) values are in _____
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parallel
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orbitals are filled
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low to high energy
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show the pattern of filling for the element Carbon
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1s2 /2s2/ 2p2
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what orbital in n = 3 has the largest energy?
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3d...dont forget that this is part of n = 3!!!
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to gain/lose a charge, what is manipulated?
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electrons
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hunds rule
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orbitals are filled until all are filled
(either not full, half full or completely full) |
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what is the exception to metal cations within the d shell?
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they will lose their s electrons before they lose their d electrons
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what are two elements within the d shell that fill weirdly?
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Mn and Te
Mn+ = [Ar]4s1,3d5 Te+ = [Kr]5s1, 4d5 |
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paramagnetic
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unpaired electrons; weakly attracted to magnetic field
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diamagnetic
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all paired electrons; repelled by magnetic field
ex) Be = 1s2, 2s2 elements on the right side of the table |
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valence electrons
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outermost electrons
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