Chemistry Chapter 4 and 5

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1. Proportional or Inversely Proprtional

Frequency/Wave Length
Inversely proportional
2. Proportional or Inversely Proprtional

Wavelength/ Energy
Inversely Proportional
3. Proportional or Inversely Proprtional

Frequency / energy
Proportional
4. Frequency  =  (symbol and Unit)
u (1/sec;  Hz )
5. Wavelength =  (symbol and unit)
(m) the upside down y
6. C =  (2answers)
• speed of light is wavelength times frequency
• c = 3.00 x 108 m/s
7. High frequency is _____ energy
High
8. Long wavelength is ___ energy
Low
9. Plancks Constant
Energy of Light=
h u(frequency)
10. In Planck's constant:
Energy of Light= h u(frequency)
h=
h = 6.626 x10-34 J s
11. What is Planck’s constant
E = h u
12. What model is this?
The Bohr Model
13. When electrons move between energy levels they_____ or ____ light.
absorb or give off
14. atomic spectra.
• when Electrons can move between
•     energy levels absorbing or
•     giving off light
15. Emission spectra “atomic  finger prints”
16. A problem with Bohr’s atom
Electrons traveling in an orbit should give off light continuously  …  they don’t.
17. What did De Broglie say about electrons
They were waves containing specific amounts of energy
18. Wave particle duality
both sets of properties present – wave and particle properties
19. Heisenberg Uncertainty Principle
We can only observe electrons by interaction with photons. Interactions with photons cause electrons to move.
20. What did Heisenberg say about how we can know where and atom is.
• Heisenberg says: we
• can’t know where an electron
• is AND where it is going at the
• same time.
21. Orbital: Definition
A three dimensional space around the nucleus where an electron is likely to be found. 90% probablility.
22. Orbitals
23. Quantum Numbers:
-Tells us.....
-The 4 numbers are...
• Tell us where electrons are LIKELY TO BE based on energy states of electrons
• 1) energy level, 2) the sub level, 3) the orbital and 4) the spin.
24. Energy Level or ______ _____ _______.
What NUmbers
• “principle quantum number”
• n= 1,2,3,4,5,6,7
25. As n increases,  the energy and distance from nucleus _____.
Increases
26. 2) The Sub Level:
-Describe the ____
- What are they
• Describes the SHAPE
• There are 4 shapes:  s, p, d, f
27. 3) The Orbital
Each orbital holds _ electrons.
What is it?
• 2
• The orbital is the specific region of the sublevel the electron is in.
•   s has 1, p has 3, d has 5, f has 7
28. s orbitals are
are spherical 29. p orbitals are dumbell shaped
30. d orbitals are complex
31. f orbitals are really complex
32. 4) The Spin
For each orbital there are two spins: up and down.
33. n^2=
total number of obitals in the Energy Level
34. 2n^2=
Number of Electrons in an Energy Level
35. As ____ _____ goes up, orbitals get _____.
Energy Levels, Bigger
36. Electron Configuration:
Arrangement of electrons in an atom.
37. Aufbau principle:
an electron occupies the lowest-energy orbital that it can.
38. Hund’s Rule:
orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron.
39. Pauli exclusion principle:
no two electrons in the same atom can have the same four quantum numbers
40. Orbital Notation
41. IRREGULARS
24         Cr     [Ar] 4s1 3d5 Crunium
29         Cu     [Ar] 4s1 3d10 Copper
• IRREGULARS
• 24         Cr     [Ar] 4s1 3d5 crunium
• 29         Cu     [Ar] 4s1 3d10 copper
42. If an electron moves from a lower energy level to a higher energy level light is________.
Absorbed
43. If an electron moves from a higher energy level to a lower  energy level light is _______
Emitted
44. Lyman series:
UV light, goes to n=1 level
45. Balmer series:
visible light, goes to n=2 level
46. Paschen series:
Infrared light, goes to n=3 level
47. Atomic #= # of ______and # of ______.
protons and electrons
48. atomic mass=
(mass #* %)+ (mass #* %)/ 100
49. isotope
same element but different nuetrons and different mass number
50. mass # =
num of protons + Nuetrons
51. Forms of radiation for low to high energy
• Radio - High wavelength  low frequency and energy
• Microwaves
• Infared
• Visible- red (low energy) Orange Yellow Green Blue
• Ultraviolet
• Xrays
• Gamma rays- High energy and frequency low wave length
52. Stable electron configurations are likely to contain orbitals that are completely _______ or _________.
full or empty
 Author: hwillson834538 ID: 179212 Card Set: Chemistry Chapter 4 and 5 Updated: 2012-10-23 02:20:01 Tags: chemistry chapter4 chapter5 Folders: Description: Chemisty Show Answers: