CHEM1110 TERM TEST 1 - SECTION 1 CLARIFICATION Flashcards
Isotopes
Atoms with the same number of protons but different numbers of neutrons (a p Z)
a: atomic pass
p: proton
z: atomic number
Conversion from m to nm
m x (10^-9nm/1m)
ER spectrum order
Big wavelength (low energy)–> small wavelengths (high energy)
Radio, microwave, infrared, visible light, UV, Xray, gamma ray
Visible light spectrum
Big wavelength (low energy) –> small wavelength (high energy)
Red, orange, yellow, green, blue, violet
Equation for speed of light, frequency, wavelength λ (3)
c = λv
λ = c/v
v = c/λ
Energy of photon equation (2)
E = hc/λ
E = hv
V = E/h
Conversion from nm to m
nm x 1m/10^9nm
Absorption
Gaining more energy to go higher orbit
Emission
Releasing energy to go to lower orbit
Energy of electron in orbit equation
-2.179 x 10^-18 J (z^2/n^2f - z^2/n^2i)
De Broglie relation equation
λ = h/mass(e-) v
Uncertainty principle fixed equation
h/(pi)(mass)(v)
Nodes
- Location of no electrons (n-1)
- Radial & spherical nodes
Principle quantum number (n)
- Indicates orbital size and energy
- Non zero integer
- As n increases, so does distance from nucleus
- Bigger n = larger orbital
Angular momentum quantum number (l)
- Indicates the shape of the orbital
- Integer
- Every number from from 0 to n-1
Magnetic quantum number (ml)
- Indicates the orientation of the orbital
- Integer from -l to 0 to +1
- Number of ml = number of orbitals
Size of orbital
l = 0 (s)
l = 1 (p)
l = 2 (d)
I = 3 (f)
Kinetic energy equation
KE = hv - binding energy
Ground state configuration
Just write configuration normally
Excited state configuration
In transition metals and we take out the s electron and put it in the d orbital
SI Units
- Mega 10^6
- Kilo 10^3
- Deci 10^-1
- Centi 10^-2
- Milli 10^ -3
- Micro 10^-6
- Nano 10^-9
- Pico 10^-12
Draw the orbitals
