Exam 2 Flashcards
Molarity =?
Moles/ liters
Energy
Capacity to do work
Heat (q)
Energy transferred from different temperatures.
Work (w)
Work = force * distance (a force applied over a distance)
Internal energy (E)
Sum of all kinetic energy and potential energy (energy in particles)
Electrostatic potential energy equation
Eel = (kQ1*Q2)/distance
Positive vs negative electrostatic potential energy
Positive = atoms want to leave negative = atoms like eachother and are close
Joules to calories
1 cal = 4.184 joules
Joule equations
1 J = (kg*m^2)/ sec^2
First law of thermodynamics
Energy cannot be created nor destroyed
System vs surroundings
The solute we use vs the water (everything else that isn’t the chemical equation)
Open system
Can exchange heat and mass with surrounding (pot)
Closed system
Heat can leave, chemicals cannot
Isolated system
Neither heat nor mass can leave
Delta E what does + and - mean for the system
+ taking energy from surroundings
- giving energy to surroundings
Exothermic
- energy based on the system
Endothermic
+ based on the system
Solubility of NO3
Always soluble
Solubility of CH3COO
Always soluble
Enthalpy
H= P times V times heat (q)
What is the goal of heat of formation
form ONE mole of the product (can have 1/2s)
elemental molecules heat of formation
0
Making a bond enthalpy value
generally negative
negative = relaxed
positive = charged
delta H of the rxn =
Bonds broken - bonds produced
wavelength
difference between two peaks (horz)
Frequency
how frequently a wave sequence occurs (like a full sine wave)
c in wavelength calc?
c= 3 x 10^8 m/s
wavelength formula
v = c/ h (weird h)
weird h in wavelength calc?
wavelength
v in wavelength calc?
hz or hertz
Nano-
10^-9
seven flavors of light in order from smallest wavelength to largest
Violet to red (ROYGBIV backwards)
blackbody radiation
if it gets hot enough, light comes off and vice versa to 0
Plancks constant
6.626x10^-34 j times s
quantized
countable
photoelectric effect
shining light on a surface of metal will eject electrons
work function
amount of energy required to eject an electron
amplitude/intensity
height of the wave or more of the same sized packets of light
Energy of photon =?
planck’s constant times wavelength
Bohr model
electron is a particle, and can only occupy certain spaces called allowed orbits
With light, every element has a unique amount of ____
bands
photon aborbed:
Photon released:
up in energy level
down in energy level
Rydberg constant
E =(-hcRH) (1/n^2) = (-2.18 x 10^-18 J) (1/n^2)
excitation with electrons
electrons go up
Relaxation with electrons
electrons go down
1 J =?
1kg (m^2S^2)
electron orbits are considered
standing waves
de Broglie wavelength equation
wavelength = h/mv mass has to be in kg
Heisenberg’s uncertainty principle
yeahhhhh we kinda dont know where the electron is, just where it is probable to be.
Heisenberg’s uncertainty equation
(delta X)(delta mv) is greater than or equal to h/4pi
delta X = change in position
bohrs model vs schrodinger model
bohrs we know where the electron is, schrodingers we dont
principal quantum number
n, the shell
angular momentum number
L, the shape of the shell
s= 0 p=1 d=2 f=3 basically 0 -> n-1
Magnetic quantum number
ML (L is subscript) differentiates the orbit the electron is in
