Chapter 7 Flashcards
(24 cards)
Wavelength
(Upside down y) – distance between two peaks or troughs in a wave. In meters
Frequency
(V) – number of waves (cycles) per second that pass a given point in space
In 1/s
Speed
(c) – speed of light
wave
a continuously repeating change or oscillation in matter or in a physical field.
Light
an electromagnetic wave, consisting of oscillations in electric and magnetic fields traveling through space.
Wave formula
c = yv_
Max plank energy formula
E = hν_
h = 6.626 × 10-34 J *s (Planck’s constant)
Albert Einstein plank formula variation
Ephoton = hν_=hc /y
Albert Einstein energy formulation
E=mc2
So m=h/yc
m=h/yv
Dualityof light
Light has wavelength it is a wave
Light has mass it is matter
Continuous spectrum
Acontinuousspectrumcontainsall wavelengths of light.
Line spectrum
line spectrum shows only certain colors or specific wavelengths of light.
Energy level orbitate formula
𝐸𝑛 = −𝐵 z2/𝑛2
n = principal quantum number
Z= atomic number
* B = Bohr orbit’s constant = 2.178 x 10-18 J
Quantum numbers
n: principale quantum number (shell, energy and size)
l: angular quantum number (shape of subshells)
ml:magnetic quantum number (orientation of subshells and orbitals)
ms: spin quantum number (spin of electron)
No 2 electron in one same atom have the same set of quantum number
value of l with letters
0=s (spehrical)
1=p (two lobes, butterfly noeud)
2=d
3=f
4=g
determining quantum numbers
l= 0…n-1
ml=-l…l
ms=1/2 or -1/2
except electron configuration
cr (4s1 3d5) and cu (4s1 3d10)
light wavelength spectrum
10-12/10-11 gamma rays
10-11/10-8 x rays
10-8/3.5 10-7 ultra violet
3.5 10-7/8 10-7 visible
8 10-7/10-3 infrared
10-3/10-2 microwaves
10-2/101 radar
101/104 radio waves
Period vs column/group
period horizontal
column vertical
atomic radius
within each column, atomis radius increases as we go down (larger shells)
within each period, atomic radius decreases as we go right
(effective nuclear charge more powerful, electrons more attracted towards center)
first ionization energy meaning
minimum amount of energy required to remove an electron from a neutral atom in the gaseous state (forming positive ion)
ionization energy
within a column, the first ionizatiion energy decreses from top to bottom because electrons are farther from the nucleaus at the bottom
within each period, the first ionization energy increases from left to right because electrons are closer to nucleus at the right and require more energy to be rejected
ionization energy increases a lot when atom is at a noble gas configuration (outermost layer full) removing core electrons hard
electron affinity meaning
the energy change produced by adding an electron to a neutral atom in the gaseous state (forming negative ion)
negative change (adding electron) indicate a stable anion is formed. the bigger negative the more stable. positive indicate anion is unstable
electron affinity
IN FIRST COLUM ONLY electron affinity becomes less negative from top to bottom because the electron enter the oribital further from the nucleus, matters less (less exothermic)
in a same period, from left to right the electron affinity becomes more negative because atom gets smaller and electron is closer to nucleus (more exothermic)
