Bair Stuff Cheat Sheet by ChemIsForSheeit

STP=1a­tm,­0de­grees celsius

Standard Temper­ature and Pressure

1mol=6.02­x10­^23­par­ticles X=molar mass(g) X

particles {
atoms(­single elements),
molecu­les(two or more non metals),
formulas units(two or more non metals­)(f.u)
ions(m­ine­rals, electr­oly­tes­,ch­arged particles

}

1atm=k­Pa=­760­tor­r=1­0.3­mH2­O=1­4.7­psi­=76­0mmHg

Constants
h= 6.63x10^-34J*s
c=3x10⁸ m/s
h is Planck's Constant
c is speed of light

1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f
6s 6p 6d 6f
7s 7p 7d 7f

s=2 p=6 d=10 f=14

To determine the number of signif­icant figures in a number use the following 3 rules:

1.Non-zero digits are always signif­icant

2.Any zeros between two signif­icant digits are signif­icant

3.A final zero or trailing zeros in the decimal portion ONLY are signif­icant

Example: .500 or .632000 the zeros are signif­icant

.006 or .000968 the zeros are NOT signif­icant

For addition and subtra­ction use the following rules:

1.Count the number of signif­icant figures in the decimal portion ONLY of each number in the problem

2.Add or subtract in the normal fashion

3.Your final answer may have no more signif­icant figures to the right of the decimal than the LEAST number of signif­icant figures in any number in the problem.

For multip­lic­ation and division use the following rule:

1.The LEAST number of signif­icant figures in any number of the problem determines the number of signif­icant figures in the answer. (You are now looking at the entire number, not just the decimal portion)
This means you have to be able to recognize signif­icant figures in order to use this rule

Example: 5.26 has 3 signif­icant figures

6.1 has 2 signif­icant figures

#unit¹ x #unit(­con­verting to) / #unit¹

#=number

cancel like units

then multiple and divide then you get your answer with new units

Atmosp­her­e-atm
Bar-Bar
millimeter of mercur­y-mmHg
Pascal-pa
Pounds per square inch-psi
Torr-torr

K=°C+2­73.15

Hydrogen (H2)
Nitrogen (N2)
Oxygen (O2)
Fluorine (F2)
Chlorine (Cl2)
Iodine (I2)
Bromine (Br2)

1. Gas particles are much farther apart from each other than liquid and solid particles
2. Gases are fluids, fluids are any substance that can flow
3. Gases have low density
4. Gases are highly compre­ssible
5. Gases completely fill a container
6. Kinetic molecular theory
*model used to predict gas behavior
*constant random motion, increasing temp, increases motion
7. Interm­ole­cular forces­(at­tra­ctive forces) are very weak or nonexi­stent between gas particles

1-mono
2-di
3-tri
4-tetra
5-penta
6-hexa
7-hepta
8-octa
9-nona
10-deca

(6.02x10²³)(6.63x10^-34)(V)

Multiply this exactly how this is once you get your V and you will get your mole of a photon for the problem.

1m=1x10⁹nm
1kHz=1x10³Hz
1mHz=1x10⁶Hz

C=VA (A is lambda)
E=hV
E is energy
V is frequency
A is lambda

P¹V¹/T¹=P²V²/T²

The Combined Gas Law is useful when: Given two pressures, volumes, or temper­atures and asked for an unknown pressure, volume, or temp. Whenever it gives you conditions for one gas, and asks for conditions of another gas, you're most likely going to use this Law.

v¹/t¹ = v²/t²

Since pressure is kept constant, the only variable that is manipu­lated is temper­ature. This means that we can use Charles's law in order to compare volume and temper­ature. Since volume and temper­ature are on opposite sides of the ideal gas law, they are directly propor­tional to one another.

PV/nT=nRT/nT

P=atm
V=L
n=# of mols
T=Kelvin
R= 0.0821 atm x L / mol x K ---Always divide the numbers underneath

P¹V¹ = P²V²

Key Points:

~According to Boyle’s Law, an inverse relati­onship exists between pressure and volume.

~Boyle’s Law holds true only if the number of molecules (n) and the temper­ature (T) are both constant.

~Boyle’s Law is used to predict the result of introd­ucing a change in volume and pressure only, and only to the initial state of a fixed quantity of gas.

~The relati­onship for Boyle’s Law can be expressed as follows: P1V1 = P2V2, where P1 and V1 are the initial pressure and volume values, and P2 and V2 are the values of the pressure and volume of the gas after change.

PV/nT=nRT/nT

P=atm
V=L
n=# of mols
T=Kelvin
R= 0.0821 atm x L / mol x K ---Always divide the numbers underneath

p¹/t¹ = p²/t²

Gay-Lu­ssac's law is a form of the ideal gas law in which gas volume is kept constant.

When volume is held constant, pressure of a gas is directly propor­tional to its temper­ature.

The usual equations for Gay-Lu­ssac's law are P/T = constant or Pi/Ti = Pf/Tf.