midterm review. 1. what is the mass of the solution when 50.0 g of salt is dissolved in 150.0 grams...
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Midterm Review
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1. What is the mass of the solution when 50.0 g of salt is dissolved in 150.0 grams of water?
a. 190.0 grams
b. 150.0 grams
c. between 50.0 and 150.0 grams
d. 200.0 grams
e. more than 200.0 grams
200.00 g
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2. How many significant digits are in the following measurement?
345000000000 nm
3
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3. Read the graduated cylinder below to the appropriate number of significant digits.
67.9 mL
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4. Read the ruler below to the appropriate number of significant digits.
30.0 mm
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6.50 mL
5. Read the graduated cylinder below to the appropriate number of significant digits.
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19 in = ? km1 in= 2.54 cm
0.00048 km
6. Convert the following measurement to the indicated unit using dimensional analysis.
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a. 7. Predict which element would be most likely to form an anion and what charge:
a. Pb
b. Cl
c. He
d. Ca
e. Zn
b. Cl 1-
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8. A distinct pattern of lines emitted by an excited atom and viewed through a spectroscope is a _______________ spectrum.
Emission
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9. Which of the following correctly represents the first ionization energy of Calcium?
Ca(g) Ca+(g) + e-
a. Ca(s) Ca+(s) + e-
b. Ca(g) + e- Ca+(g)
c. Ca(s) + e- Ca+(s)
d. Ca(g) Ca+(g) + e-
e. Ca(g) Ca2+(g) + e-
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10. An area of 90% probability for finding an electron is a(n) ______________?
Orbital
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11. Which of the following bonds is probably the most polar?
– N–H– O–H– P–H– Se–H– C–H
O–H
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12. Light has a wavelength of 470 nm. What is the energy of this light?
E= h [c/ wavelength]
4.2x10x10-19 J
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13. A sample of zinc-72 has an initial activity of 2310 counts per minute on a device that measures the level of radioactivity. After 120 hours the activity declined to 457 counts per min. What is the half-life for decay of zinc-72?
457 = 2310 ( .5)n
n= 2.33
120/2.33 = 52 hrs
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14. A student in the laboratory determined the density of a substance to be 14.2 g/mL. The accepted value for the density of this substance is 13.87 g/mL. What is the percent error of the student’s measurement to the correct number of sig figs?
2%
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15. List the following in order of increasing radius: K+, Se2–, Cl–, Na+, S2–
Na+ < K+ < Cl- < S2- < Se2-
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16. Which +3 ion has the electron configuration [Ar]3d5?
a. Fe
b. Nb
c. Cr
d. Mo
e. Sc
a. Fe3+
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17. Which ion has the smallest radius?
a. Ca2+
b. K+
c. As3-
d. Br -
e. I-
a. Ca2+
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18. What is the correct systematic (IUPAC) name for the molecule?
H3C-CH2
H2C-CH-CH2 -CH3
CH2CH2CH3
4-ethyl-heptane
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19. What particle is emitted when lead–214, undergoes natural radioactive decay to bismuth–214, Bi?
• beta decay
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20. Complete and balance the following transmutation reactions
a.
b.
a. = , b. =
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21. Calculate the average atomic mass of lithium, which occurs as two isotopes that have the following atomic masses and abundances in nature: 7.30%, 6.017 amu and 92.7%, 7.018 amu. Consider sig figs when expressing your answer.
6.95 amu
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22. Write the electron configuration and orbital diagram for Ag.
[Kr]5s14d10
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23.
a. How many -bonds are there in this molecule?
b. How many -bonds are there?
c. Identify the hybridization of carbon atom 1 and oxygen atom 3.
A
B C
1
3
2
a. 11b. 1c. C = sp3, O = sp3
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A. B
C
24. A shows examples of __________________ isomers.
25. B and C are examples of ______________ isomers.
geometric
structural
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26. A piece of copper (Cp= 0.38J/goC) was heated to 380.3oC and then placed in 150.g of water at 23.5oC. After the copper was sitting in the water for a little while, the water’s temperature was 35.0oC, what was the mass of the copper?
m = 55.0 g
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27. When aqueous potassium hydroxide and aqueous copper (II) chloride react, potassium chloride and copper (II) hydroxide are formed. ____. Which of the following represents the correct balanced equation?
a.KH(aq) + CuCl2(aq) KCl(aq) + CuH (s)
b.2KOH(aq) + CuCl2(aq) 2KCl (aq) + Cu(OH)2((s)
c.KOH(aq) + CuCl(aq) KCl (s) + CuOH (s)
d.KOH(aq) + CuCl(aq) KCl (s) + Cu(OH)2(s)
e.b
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28. What is the balanced chemical equation for the reaction that takes place between bromine and sodium iodide?
a.Br (l) + NaI (aq) NaBr(aq) + I (s)
b.Br2 (l) + 2NaI (aq) 2NaBr (aq) + I2(s)
c.Br (l) + NaI(aq) NaBrI (s)
d.Br2 (l) + NaI(aq) Br2I2 (aq) + Na (s)
e.This reaction does not take place.
B.
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29. Complete and balance the chemical equation for the following single replacement reaction. What are the products of the reaction?
Solid silver reacts with aqueous potassium nitrate