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Chapter 7
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Chapter 10
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100
What is the Speed of Light?
3.000 x10^8
100
What is Z? (Factor Affecting Atomic Orbital Energy)
Nuclear charge
100
Draw the Lewis structure for Nitrogen.
** *N* *
100
Draw the Lewis structure of NF3
Slide 5 of Ch 10 ppt.
100
What is Hess's Law?
Enthaply change overall = H1+H2+...Hn
200
What is the conversion factor from A to meters?
1 A=10^-10 meters
200
Put the energy levels in order. f,s,p,d
sd>p>s
200
What is Lattice energy?
The energy required to separate 1 mol of an ionic solid into gaseous ions. (Lattice energy is a measure of the strength of the ionic bond)
200
Draw the Lewis Structure of Ethylene.(C2H4)
Slide 10 of Ch. 10 ppt.
200
Two gaseous pollutants that form in auto exhausts are CO and NO. An environmental chemist is studying ways to convert them to less harmful gases through the following reaction: CO (g) + NO (g) → CO2 (g) + ½N2 (g) DH = ? Given the following information, calculate the unknown DH: Equation A: CO (g) + ½O2 (g) → CO2 (g) DHA = –283.0 kJ Equation B: N2 (g) + O2 (g) → 2NO (g) DHB = 180.6 kJ
-373.3 kJ Work on slide 45 of Ch. 6 ppt.
300
What is the Heisenberg Uncertainty Priciple? (Equation or definition)
It is not possible to know both the position and moment of a moving particle at the same time. (delta)x*m*(delta)u>= h/4pi
300
What is Hund's rule?
When orbitals of equal energy are available, the lowest energy electron configuration has the maximum number of unpaired electrons with parallel spins.
300
Describe the difference between ionic bonds, covalent bonds, and metallic bonds.
Ionic= one atom loses an electron (metal and non metal) Covalent= share electrons (2 non metals) Metallic= electron pool(2 metals)
300
Find the shape, Polarity, and bond angle of CO2.
Linear NonPolar 180 degrees
300
Calculate the energy of an X-Ray that has a wavelength of 1.15e-10 m.
1.73e-15 Mock Exam question 3
400
When describing an atomic orbital what do the "n", "l", and "ml" show?
n= the principle quantum number. l= the angular moment quantum number. ml= the magnetic quantum number (-l to +l)
400
Write out the partial ground-state electron configuration for lead.
[Xe] 6s^2 6p^2
400
At what electronegativities are bonds mostly ionic, non polar covalent, mostly covalent, and polar covalent? (Hint: these are not in order)
Non Polar Covalent- >0 Mostly Covalent- between 0 and 0.4 Polar Covalent- between 0.4 and 1.7 Mostly Ionic- between 1.7 and 3.3
400
Draw out a Trigonal Bipyramidal bond structure.
Slide 43 of Ch. 10 ppt.
400
Use the Rydberg equation to find the wavelength (in nm) of a photon emitted when an electron in an H atom undergoes a transition from n=5 to n=2.
434.17 nm Mock Exam question 16
500
What is blackbody radiation and what is it's equation?
It is when a solid emits visible light when it is heated to about 1000K. E=nhv E=energy n is a positive integer h is Planck's constant
500
Draw out all of the periodic trends.
Atomic size= lower left Electron Affinity= upper right Ionization energy= upper right Metallic Behavior= lower left Lattice Energy= lower left*
500
Calculate the Enthalpy change of the reaction for the chlorination of methane to form chloroform. H H | | H-C-H + 3 Cl-Cl -> Cl-C-Cl + 3 H-Cl | | H H C-H = 413 kJ/mol Cl-Cl= 243 kJ/mol C-Cl= -339 kJ/mol C-H= -413 kJ/mol H-Cl= -427 kJ/mol
-330kJ Work on Slide 47 of Ch. 9 ppt.
500
Name the angles for all of the different bond structures.
Linear- 180 Trigonal Planar- 120 Bent with 3 electron groups- <120 Tetrahedral- 109.5 Trigonal Pyramidal- <109.5 Bent with 4 electron groups- <109.5 Trigonal Bipyramidal- Axial -90 Equtorial- 120 Seesaw- Axial- <90 Equtorial- <120 T Shaped - Axial- <90 Linear with 5 electron groups- 180 Octahedral- 90 Square pyramidal- <90 Square Planar- 90
500
Describe the VSPER method.
Draw a dot structure to show the valence electrons Count the number of electron groups surrounding the central atom Predict geometry of the electron groups around the central atom Ignor any lone pairs and predict the geometry of the molecule/ion