Exam 2 Flashcards by Max Colby

Molarity =?

Moles/ liters

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Energy

Capacity to do work

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Heat (q)

Energy transferred from different temperatures.

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Work (w)

Work = force * distance (a force applied over a distance)

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Internal energy (E)

Sum of all kinetic energy and potential energy (energy in particles)

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Electrostatic potential energy equation

Eel = (kQ1*Q2)/distance

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Positive vs negative electrostatic potential energy

Positive = atoms want to leave negative = atoms like eachother and are close

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Joules to calories

1 cal = 4.184 joules

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Joule equations

1 J = (kg*m^2)/ sec^2

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First law of thermodynamics

Energy cannot be created nor destroyed

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System vs surroundings

The solute we use vs the water (everything else that isn’t the chemical equation)

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Open system

Can exchange heat and mass with surrounding (pot)

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Closed system

Heat can leave, chemicals cannot

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Isolated system

Neither heat nor mass can leave

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Delta E what does + and - mean for the system

+ taking energy from surroundings
- giving energy to surroundings

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Exothermic

energy based on the system

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Endothermic

+ based on the system

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Solubility of NO3

Always soluble

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Solubility of CH3COO

Always soluble

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Enthalpy

H= P times V times heat (q)

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What is the goal of heat of formation

form ONE mole of the product (can have 1/2s)

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elemental molecules heat of formation

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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