When an electron falls to a lower energy level it:
Emits light
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5
How many carbons are there in 3-ethylpentane?
7
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10
Calculate the [H+] in a solution that has a pH of 9.48.
3.3 Ã 10â10 M
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10
If you have a negative entropy and a positive enthalpy, what can the Gibb's free energy be?
only positive
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If n=2, what is l and ml respectively?
l = 0, 1; ml= -1, 0, +1
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20
Calculate the [H+] in a solution that is 0.18 M in NaF and 0.25 M in HF. (Ka = 7.2 Ã 10â4)
1.0 Ã 10â3 M
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15
Using the following thermochemical data: 2Y(s) + 6HF(g) â 2YF3(s) + 3H2(g) ÎH° = â1811.0 kJ/mol 2Y(s) + 6HCl(g) â 2YCl3(s) + 3H2(g) ÎH° = â1446.2 kJ/mol calculate ÎH° for the following reaction: YF3(s) + 3HCl(g) â YCl3(s) + 3HF(g)
182.4 kJ/mol
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15
. Calculate E°cell for the following reaction: 2Fe2+ (aq) + Cd2+ (aq) à 2Fe3+ (aq) + Cd(s)
-1.17V
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25
What is the major product when 2-methylprop-1-ene is treated with HBr at room temperature?
2-bromo-2-methylpropane
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15
What is the VSEPR shape of AsH3
trigonal pyramidal (AX3E)
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15
State the condensed electron configuration of b. S^2- (sulfur anion)
[Ne]3s^2 3p^6
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10
Which of the following would you expect to have the highest boiling point? ethanol, ethyl ethanoate, ethanoic acid, ethane, ethene, ethyne, ethanal or chloroethane?
ethanoic acid - has the most hydrogen bonding therefore it takes more ENERGY to break those intermolecular bonds. Therefore it should have highest boiling point
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15
How many electrons in an atom can have the quantum numbers n = 3, l = 2?