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210 Cards in this Set
- Front
- Back
Electrons within the same orbital are represented as having parallel spins. This goes against what? |
Pauli exclusion principle
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What are the four quantum numbers and what do they refer to?
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n principal quantum #
l azimuthal quantum # angular momentum quantum # m_l magnetic quantum # m_s spin quantum # |
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No two electrons in a given atom can posess the same quantum numbers is stated by:
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Pauli exclusion principle
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principal quantum number (n) is defined by
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energy level
(0, 1, 2, 3...n) |
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azimuthal quantum number (l) is defined by
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shape of orbitals. subshells
(0, 1, 2, 3, up to n-1) (s, p, d, f) |
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The maximum number of electrons in energy level n is
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2n^2
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The maximum number of electrons that can exist within a subshell is given by
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4l+2
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For any given principal quantum number (n), the value of the azimuthal quantum number (l) ranges from
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0 to n-1
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The greater value of ___, the greater energy of the subshell.
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l
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The ____ value of l, the greater energy of the subshell.
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greater
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The greater value of l, the greater ________.
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energy of the subshell
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The greater value of l, the ______ energy of the subshell
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greater
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magnetic quantum number (m_l) is defined by
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orientation of the orbital in space
all integers (-l to l) including 0 |
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The possible values of m_l are
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all integers (-l to l) including 0
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spin quantum number (m_s) is defined by
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the direction of spin
(-1/2, +1/2) |
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How many electrons can be in the same orbital?
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2
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The Pauli exclusion principle states that whenever two electrons are in the same orbital, they must have ____ spins
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opposite
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Subshells are ranked by increasing energy by finding
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n+l
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The lower the value of ___, the lower the energy of the subshell.
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n+1
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The ____ the value of n+l, the lower the energy of the subshell.
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lower
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The lower the value of n+l, the ____ of the subshell.
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lower the energy
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Hund's rule states that
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in subshells that contain more than one orbital, the orbitals are filled so that there are a maximum number of half-filled orbitals with parallel spins
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In Bohr's model of the hydrogen atom the energy of an electron is directly dependent on
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principal quantum number (n)
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What describes the excitation exhibited when an electron jumps from its ground state to a higher energy level?
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atomic absorption spectrum
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The Heisenberg uncertainty principle states that
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it is impossible to determine the momentum and the position of an electron simultaneously
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This says it is impossible to determine the momentum and the position of an electron simultaneously
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Heisenberg uncertainty principle
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What is planck's constant
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6.62E-34J*s
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What is the speed of light
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3E8 m/s
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What is the final orbital of Ca
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4s^2
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How many electrons in Ca
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20
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What is the final orbial and # of electrons if an atom has 20 electrons
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4s^2
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If an atom's final orbital is 4s^2, how many total electrons does it have
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20
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An energy (x) corresponds to the energy of an electron in which principal energy level?
What formula? |
E = -R_H/n^2
x = E solve for n R_H is given |
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In going from 1s2-2s2-2p6-3s2-3p6-4s1 to
1s2-2s2-2p6-3s2-3p5-4s2 an electron would |
absorb energy
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In going from 1s2-2s2-2p6-3s2-3p5-4s2 to
1s2-2s2-2p6-3s2-3p6-4s1 an electron would |
emit energy
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How do you find the amount of energy it takes to move an electron from one energy level to another?
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E = -R_H ((1/n_i)^2 - (1/n_f)^2)
R_H = 2.18E-18J/electron |
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How to determine the energy of a photon given the photon frequency?
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E=hv
h=planck's constant 6.62E-34J*s |
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How to determine the wavelength given a photon that carries an x amount of energy?
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E = hc/wavelength
h=planck's constant 6.62E-34J*s |
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On the periodic table electronegativity increases this direction
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up and to the right
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On the periodic table ionization energy increases this direction
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up and to the right
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On the periodic table atomic radius increases this direction
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down and to the left
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dipole-dipole interactions and dispersion forces are known as
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van der Waals forces
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van der Waals forces are
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dipole-dipole interactions and dispersion forces
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dipole-dipole interactions are formed by
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polar molecules arranging so that positive sides of molecules get close to negative sides of other molecules
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polar molecules arranging so that positive sides of molecules get close to negative sides of other molecules is called
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dipole-dipole interactions
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dipole-dipole interactions are negligible in this state phase
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gaseous
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_____ species tend to have higher boiling points than _____ species of comparable molecular weight
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Polar
nonpolar |
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Polar species tend to have ____ boiling points than nonpolar species of comparable molecular weight
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higher
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Substances with hydrogen bonding tend to have ______ boiling points compared with compounds of similar molecular formula without H bonding
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unusually high
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Substances with ____ tend to have unusually high boiling points compared with compounds of similar molecular formula without _____.
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hydrogen bonding
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the short lived formation of dipoles caused by the rapid polarization and counterpolarization of the bonding electron cloud
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dispersion forces
london forces |
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These kind of molecules possess greater dispersion forces
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large
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Large molecules possess more of this intermolecular force
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london dispersion forces
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How many moles in (x)grams of XY_2
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mol = weight of sample (g)
_________________________ total molar weight (g/mol) |
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For the general reaction
aA + bB --> cC + dD rate= ? |
rate = k[A]^x[B]^y
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The concentration of radioactive substance A at time t is found by
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[A_t] = [A_o]e^-(kt)
*** ln(A_t) = ln(A_o)-k*e*t |
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How is the first order halflife of a reaction found
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t_(1/2) = ln (2/k) = .693k
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___ enthalpy change indicates an endothermic reaction
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negative
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___ enthalpy change indicates an exothermic reaction
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positive
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Negative enthalpy change indicates an _____ reaction
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endothermic
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Positive enthalpy change indicates an _____ reaction
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exothermic
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If K_eq is ____ compared to 1 an equilibrium mixture of reactants and products will contain very little of the reactants compared to the products
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very large
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If K_eq is very large compared to 1 an equilibrium mixture of reactants and products will contain
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very little of the reactants compared to the products
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If K_eq is ____ compared to 1 an equilibrium mixture of reactants and products will contain very little of the products compared to the reactants
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very small
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If K_eq is very large compared to 1 an equilibrium mixture of reactants and products will contain
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very little of the products compared to the reactants
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If K_eq is ____ compared to 1 an equilibrium mixture of reactants and products will contain approximately equal amount of reactants and products
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close to 1
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If K_eq is close to 1 compared to 1 an equilibrium mixture of reactants and products will contain
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approximately equal amount of reactants and products
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In an exothermic reaction adding heat will cause the reaction to
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shift to the left
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In an endothermic reaction adding heat will cause the reaction to
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continue forward faster
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An adiabatic process occurs when
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no heat exchange occurs in a system
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An isothermal process occurs when
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temperature of the system remains constant
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Isobaric process occurs when
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pressure of the system remains constant
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An isolated system occurs when
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it cannot exchange energy or matter with its surroundings
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A closed system occurs when
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it can exchange energy but not matter with its surroundings
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An open system occurs when
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it can exchange energy and matter with its surroundings
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To find the heat moved in a given process
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q = m*c*dT
m=mass c=specific heat dT=change in temp |
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Given:
Several reactions and their changes in enthalpy. Calculate change in enthalpy for another reaction based on this. |
Comine given reactions, multiply/factor to cancel needed compounds on either side after adding is complete so that the final reaction is the same as the one that must be calculated for. Add the reactions' dH's to find the dH for the answer.
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Change in entropy is given by
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dS=Sfinal-Sinitial
dS=q_rev/T |
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Change in Gibbs free energy is found by
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dG = dH - TdS
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If dG is negative the reaction is _______
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spontaneous
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If dG is positive the reaction is _______
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not spontaneous
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If dG is zero the reaction is ______
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in a state of equilibrium
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If dH = TdS the reaction is ____
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in a state of equilibrium
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If dH > TdS the reaction is ____
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not spontaneous
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If dH < TdS the reaction is ____
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spontaneous
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If dG is ____ the reaction is spontaneous
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negative
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If dG is ____ the reaction is not spontaneous
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positive
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If dG is _____ the reaction is in equilibrium
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zero
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The heat of formation of any element in its elemental state is
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0
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P1V1=?
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P2V2
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V1/T1=?
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V2/T2
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n1/V1=?
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n2/V2
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PV=?
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nRT
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P1V1
____ = ? T1 |
P2V2
____ T2 |
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density = ?
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m/v
P(MM) _____ RT |
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KE=(1/2)mv^2=
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(3/2)kT
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KE=
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(1/2)mv^2
(3/2)kT |
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r1/r2 = ?
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sqrt(MM2/MM1)
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Natural processes want to decrease ____ and increase ____
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enthalpy
entropy |
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Natural processes want to ____ enthalpy and _____ entropy
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decrease
increase |
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Any process that increases entropy and decreases enthalpy will be
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spontaneous at any temperature
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Any process that does this will be spontaneous at any temperature
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increase entropy
decrease enthalpy |
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The higher the molecular mass, the ___ the gas will diffuse
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slower
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The ____ the molecular mass, the slower the gas will diffuse.
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higher
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To find bond order from a MO diagram:
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subtract antibonding(*) electrons from bonding electrons and divide by two
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What type of amine is found as an organic salt?
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quaternary
NH4 |
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What are the colligative properties?
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lowering vapor pressure
boiling point elevation freezing point depression osmotic pressure |
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What functional group cannot be formed from carboxylic acids?
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ethers
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In proton NMR, a peak with a shift between 6.0 and 9.5PPM denotes which functional group
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aromatic
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In proton NMR, a peak with a shift between 9.5 and 10.5PPM denotes which functional group
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aldehyde
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In proton NMR, a peak with a shift between 2.1 and 2.6PPM denotes which functional group
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ketone
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In proton NMR, a peak with a shift between 3.3 and 3.9PPM denotes which functional group
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ether
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The smaller the K_sp the lower the ___
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solubility
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The smaller the _____ the lower the solubility
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K_sp
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The ____ the K_sp the lower the solubility
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smaller
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Whatever is being oxidized is the ____
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reducing agent
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Whatever is being reduced is the ____
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oxidizing agent
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A gain in charge is ____
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oxidation
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A loss in charge is ____
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reduction
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A gain in electrons is ____
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reduction
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A loss in electrons is ____
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oxidation
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this hybridization is linear
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sp
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this hybridization is trigonal planar
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sp2
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this hybridization is tetrahedral
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sp3
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this hybridization is trigonal bipyrimidal
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sp3d
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this hybridization is tetrahedral
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sp3d2
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the shape of sp3d2 is
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octahedral
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the shape of sp3d is
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trigonal bipyramidal
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the shape of sp3 is
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tetrahedral
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the shape of sp2 is
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trigonal planar
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the shape of sp is
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linear
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How would you determine which part of an organic compound caused a peak on a mass spectrograph at X amu
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Find which molecular mass adds up to the given amu
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Which thermodynamics property tends to increase in a spontaneous process
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entropy
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What is the most advanced theory of molecular bonding
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MO theory
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A broad peak at 3200-3550cm^-1 in an IR spectrograph is
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-OH group
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A peak at 1630-1780cm^-1 in an IR spectrograph is
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carbonyl
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A peak at 2220-2260cm^-1 in an IR spectrograph is
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nitrile
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A peak at 2853-2962cm^-1 in an IR spectrograph is
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C-H stretch
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When asked to find the coordination number of the coordination complex, do this
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count the number of coordinate covalent bonds on the central atom
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K_sp = ?
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[A]^x * [B]^y ...
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LeChatelier's principle states that
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when a stress (change in concentration, temperature, volume, or total pressure) is applied to a system, the equilibrium will shift to relieve that stress
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Which is the anode and which is the cathode. What do the double lines represent
Cu|Cu2+ || Ag+|Ag |
Cu side is anode
Ag side is cathode the salt bridge |
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Cu|Cu2+ || Ag+|Ag
Where does oxidation occur |
at the anode on the left
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Cu|Cu2+ || Ag+|Ag
Where does reduction occur |
at the cathode on the right
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Meta directors do this
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help stabilize a positive charge on the meta position
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What is the order of oxidation for functional groups from lowest to highest
|
alkyne
alkene alkane alcohol ketone/aldehyde COOH CO2 |
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The dehydration of -COOH with an -OH yields what functional group
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ester
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What is the order of stability for a Carbon free radical from lowest to highest
|
methyl
primary secondary tertiary |
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Which of the following functional groups will have the greatest partial positive charge in carbon on the beta position to the functional group? Why?
amine aldehyde alcohol alkene |
aldehyde
O has a large electronegativity so it has an inducive effect on adjacent carbons |
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What results in a free radical
|
homolytic cleavage
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homolytic cleavage results in
|
a free radical
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The solution of a salt with a cation of a strong base and an anion of a weak acid will form what type of solution
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basic
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The solution of a salt with a cation of a weak base and an anion of a strong acid will form what type of solution
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acidic
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The solution of a salt with a cation of a ___ base and an anion of a ___ acid will form a basic solution
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strong, weak
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The solution of a salt with a cation of a ___ base and an anion of a ___ acid will form an acidic solution
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weak, strong
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As temperature increases reaction rates increase was an idea from
|
Arrhennius
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If a gas is only on the product side of the equation it means
|
entropy has increased
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If a gas is only on the reactant side of the equation it means
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entropy has decreased
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A solute in a liquid will cause vapor pressure ____
|
depression
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To find heat capacity do this
|
mass x specific heat
|
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to find rate of effusion
|
rate 1
______ = sqrt(MW2/MW1) rate 2 |
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wavelength x frequency =
|
c (speed of light)
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On the periodic table atomic radii tend to increase
|
down and to the left
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To determine which solutes in water will raise the boiling temperature the most:
|
determine which solute produces the most moles when dissolved
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Given the initial concentration of a reactant in a first-order reaction, a rate constant, find the molarity after t seconds
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ln([A0]/A]) = kt
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When _______, equilibrium shifts in the direction to produce a smaller gas volume.
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pressure increases
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When _______, equilibrium shifts in the direction to produce a larger gas volume.
|
pressure decreases
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This can react with either an acid or a base and is formed by an amphoteric element, which is an element that can react as a metal or a nonmetal
|
An amphoteric oxide
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The larger the value of the equilibrium constant, K_A,
|
the stronger the acid/base
|
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The smaller the value of the equilibrium constant, K_A,
|
the weaker the acid/base
|
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What are the solubility rules
|
-All salts formed with alkali metals
-All ammonium salts(NH4+) and nitrate salts (NO3-) -Many chlorides bromides and iodides -Many sulfates (SO4 2-) |
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When _______, equilibrium shifts in the direction to produce a smaller gas volume.
|
pressure increases
|
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When _______, equilibrium shifts in the direction to produce a larger gas volume.
|
pressure decreases
|
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This can react with either an acid or a base and is formed by an amphoteric element, which is an element that can react as a metal or a nonmetal
|
An amphoteric oxide
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The larger the value of the equilibrium constant, K_A,
|
the stronger the acid/base
|
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The smaller the value of the equilibrium constant, K_A,
|
the weaker the acid/base
|
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What are the solubility rules
|
-All salts formed with alkali metals
-All ammonium salts(NH4+) and nitrate salts (NO3-) -Many chlorides bromides and iodides -Many sulfates (SO4 2-) |
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These are the three steps to forming a polymer
|
initiation - formation of free radical
propagation - chain lengthening step termination - when something bonds to the free radical and discontinues the chain growth |
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What kind of reactant is most likely to react with an aromatic compound
|
eletrophile
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What type of alcohol will most rapidly undergo a dehydration reaction? Why
|
tertiary
it will have the most stable carbocation intermediate, tertiary |
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To find functional groups this spectroscopy is best
|
IR
|
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To find molecular fragments this spectroscopy is best
|
MS
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To find bonding structure this spectroscopy is best
|
NMR
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1 mole of electrons is symbolized as
|
1 faraday
|
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This is the only kind of nuclear decay that can increase atomic number
|
beta decay
|
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When an aldehyde is oxidized it becomes
|
carboxylic acid
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How is singlet/doublet/triplet/etc determined?
|
count the number of H on the desired C and any adjacent C
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What represents the energy gained by giving an electron to an element
|
electron affinity
|
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Ag+ + I- <--> AgI
what can be added to remove more silver from the solution |
KI
|
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In oxyacids, the _____, the stronger the acid
|
more oxygen present
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In oxyacids, the more oxygen present the ______
|
stronger the acid
|
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In polyprotic acids, the more hydrogen bonds of oxygen lost hydronium ions, the ____
|
stronger the acid
|
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In polyprotic acids, ____, the stronger the acid
|
the more hydrogen bonds of oxygen lost hydronium ions
|
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In equilibrium equations, ____ is not included because its will remain almost constant
|
H2O
|
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H2O is not included in _______ because its concentration will remain almost constant
|
equilibrium equations
|
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H2O is not included in equilibrium equations because
|
its concentration will remain almost constant
|
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This is the formation of a solid from a gas
|
deposition
|
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Causing a reaction to occur by increasing the temperature increases the influence of this
|
entropy
dG = dH - TdS |
|
What kind of isomer will rotate plane polarized light
|
enantiomer
|
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This has chiral carbons that cancel the rotation of light out on each other
|
diastereomer
|
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What type of amine is most alkaline in water
|
tertiary
|
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A Claisen rearrangement yields what type of compound
|
phenol derivative
o-substituted phenol |
|
Ether oxidizes to this
|
CO2
|
|
Alpha decay does this
|
reduces atomic number by 2
|
|
Beta decay does this
|
increases the atomic number
|
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When naming a benzene ring, constituents on adjacent carbons go in this order (carbon 1, 2, 3)
|
ortho, meta, para
|
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A Claisen condensation will produce what
|
beta keto ester
|
|
This is the reaction of esters in the presence of sodium ethoxide
|
Claisen condensation
|
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These are created by a dehydration reaction with a carboxylic acid and an alcohol
|
esters
|
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These are created by a dehydration reaction with a carboxylic acid and an amine
|
amides
|