Chemistry Tri A Review

1
Chemistry Tri A Review
Cat. 1 Review Cat. 2 Radiant energy Cat. 3 Quantum Theory Cat. 4 The Atom Cat. 5 A New Look Cat. 6 Electron Config.
200 200 200 200 200 200
400 400 400 400 400 400
600 600 600 600 600 600
800 800 800 800 800 800
1000 1000 1000 1000 1000 1000
2
Review200

• How many significant figures are in the
  measurement 0.0032? 40500? Convert these numbers
  to scientific notation
• 2, 3
• 3.2 x 10-3, 4.05 x 104

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3
Review 400

• A tentative answer to a scientific question is
  called? What is the variable? The experimental
  control
• The hypothesis
• The one factor being tested
• Keeps all conditions constant

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4
Review 600

• Hydrogen has three isotopes H-1, H-2 and H-3.
  Given the average atomic mass is 1.01, what is
  the most common isotope of hydrogen? What is
  Mass Defect?
• H-1
• Mass lost during a nuclear reaction

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5
Review 800

• All atoms of the same elements have the same
  number of? Isotopes of the same element vary in
  their numbers of. What are the relative AMU of
  protons, neutrons and electrons?
• Protons
• Neutrons and atomic mass
• 1, 1, 0

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6
Review 1000

• Absolute zero is what number in Kelvin? In
  Celsius? At what temperature does water boil in
  Celsius? In Kelvin?
• 0, -273C
• 100C, 373K

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7
Radiant Energy200

• A hertz is the same as? How is wavelength
  measured?
• Cycle/second s-1
• Distance between corresponding points on
  consecutive waves

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8
Radiant Energy 400

• Light has properties of? What is the speed of
  light?
• Particles and waves
• 3.00 x 108 m/s

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9
Radiant Energy 600

• How are s-1 and 1/s use in measuring frequency?
• Frequency Hertz Joule seconds (Js) or
  Joules/s-1

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10
Radiant Energy 800

• What are the colors of the visible spectrum? What
  color has the shortest wavelength? What color has
  the lowest energy? Which of the following is not
  a form of electromagnetic radiation (xrays\gamma
  rays\soundwaves\visable light?
• R O Y G B I V
• Violet
• Red
• soundwaves

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11
Radiant Energy 1000

• What does the equation ?c/v mean? If a wave has
  a length of 800nm what is its frequency? What is
  that in KHz?
• Wavelength (speed of light) / frequency
• 3.75x1014 Hz
• 3.75x1011 KHz

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12
Quantum Theory200

• What is Planks constant? How can you use this to
  find the Energy of a particle. What did Plank
  mean by energy quantization?
• h 6.6262x10-34Js
• Ehv
• Electrons can only jump in a quanta of energy not
  a partial quanta.

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13
Quantum Theory 400

• Explain why x-rays can harm humans and radio
  waves can not.
• Name all parts of the diagram
• Ehv, so the energy associated with a X-ray is
  much higher then the energy associated with a
  radio wave. The energy of a radio wave is too low
  to harm humans.
• Awave height, b wavelength, c , d
  amplitude . Trough,

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14
Quantum Theory 600

• Why does violet light release electrons from
  metal and red does not. What is this process
  called the Einstein figured out?
• Violet light has such a high quanta of energy
  that it releases the excited electrons escape
  from the metal. Red light is a lower energy and
  doesnt move the electrons enough to displace
  them from the metal.
• Photoelectric effect.

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15
Quantum Theory 800

• Which group has two different numbers of valance
  electrons? Give the valence electrons in each
  group of the Main Group elements.
• Noble gases
• 1, 2, 3 4, 5 6 , 7

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16
Quantum Theory 1000

• What is a particle of light called? How fast can
  this particle travel, (name and number).
• photon
• Speed of light 3.00 e 8 m/s

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17
The Atom200

• What is a continuous spectrum? What is an
  electron doing in a emission spectrum and a
  absorption spectrum?
• One show the blending of the colors of ROY G Biv.
• Absorption electrons are moving from ground
  state to excited state.
• Emission electron is moving from excited to
  ground state

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18
The Atom 400

• Describe how neon lights work.
• Electricity causes electrons to move from ground
  to excited and back releasing energy and giving
  off colored light depending upon the gas in the
  tube.

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19
The Atom 600

• Describe what a principle quantum number n is.
  What did DeBroglie name ? Why
• the levels of electrons circling the nucleus
  from one to seven
• - matterwaves
• Light behaves like waves so matter behaves like
  waves hence matterwaves

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20
The Atom 800

• What is the Heisenberg Uncertainty Principal?
  Describe lights dual nature.
• Cant measure position and momentum of an
  electron simultaneously.
• Photons of lights act as waves and particles.

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21
The Atom 1000

• Were DeBroglies thoughts proven by him?
• Name a, b, c, d
• No, someone else did it.
• Amicrowaves, binfrared radiation ,
  cultraviolet d xrays

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22
A New Look 200

• Write the complete electron configuration for Cl.
  Write the abbreviated electron configuration for
  P
• How many dots would be in the dot diagrams of
  both Cl and P?
• 1s2 2s2 2p6 3s2 3p5
• (Ne) 3s2 3p3
• Cl 7 dots P 5 dots

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23
A New Look 400

• Why do electrons not have orbits but can be found
  in orbitals? What is the name of the model where
  the previous is described?
• Orbits are specific paths, orbitals are paths of
  high probability where electrons can be found.
• Quantum-Mechanical Model

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24
A New Look 600

• Name the 4 different kinds of orbitals. State
  the number of electron pairs that can be found in
  each orbital. Describe the orbital that has 6
  electrons in it with detailed addresses and
  filling order.
• s, p, d, f
• S1 pair, p3 pair, d 5 pair, f 7 pair
• Px1, py1, pz1, px2, py2, pz2
• 1

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25
A New Look 800

• Which orbital always fills first? What is its
  shape? What is the difference in its shape as
  energy grows?
• S
• Sphere
• Gets larger

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26
A New Look 1000

• What is the next highest energy level after 3d?
  According to Bohr, how do electrons circle the
  nucleus? How do electrons spin in an s orbital?
• 4p
• Specific allowed orbits
• Opposite directions /- 1/2

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27
Electron Config.200

• Which of these energy levels can never exist
  1p, 2d, 3f? What are the outermost electrons
  called? What are the used for?
• 1p, 2d, 3f
• Valence
• bonding

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28
Electron Config. 400

• Explain Aufbau Principle. Explain Pauli
  Exclusion Principle. Explain Hunds rule.
• Electrons fill orbitals one at a time to lowest
  energy orbitals first
• 1) only 2 electrons per orbital 2) electrons
  must have opposite spins
• Each orbital orientation of a sub level must
  contain 1 electron before being paired up.

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29
Electron Config. 600

• What makes the configuration for chromium and
  copper an exception to the Aufbau principle
• They fill like 4s1 then 3d5 rather than
• 4s2 then 3d4

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30
Electron Config. 800

• Draw the arrow diagram for neon. Give the
  electron configuration for P.
• 1s 2 (two arrows/1bed) 2s 2 (two arrows/1bed)
  2p 6 (6 arrows/3beds)
• 1s2 2s2 2p6 3s2 3p3orNe 3s2 3p3

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31
Electron Config. 1000

• What levels do the first s,p,d,f orbitals appear?
• s-1, p-2, d-3, f-4

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32
?200
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33
?400
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34
? 600
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35
?800
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36
?1000
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37
Final Jeopardy

• Calculate the frequency and energy of a wave of
  750nm?
• 4.0 x 1014 s-1 (frequency)
• How to calculate this answer
• 750nm 1x 108 m 7.5 x 10-7 m
• 1 1nm
• Vc/? v 3.0x 108 m/s 4 x 1014 s-1
  (frequency)
• 7.5x 10-7 m
• Then you must calculate Energy
• E hv
• E 6.6262 x 10-34 JS x 4 x 1014 s-1
• Rewrite to 6.6262 x 10-34 JS
  4 x 1014 s
• E 1.66x 10-48 J

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