Download CHEMISTRY Midterm Practice

Survey
yes no Was this document useful for you?
   Thank you for your participation!

* Your assessment is very important for improving the work of artificial intelligence, which forms the content of this project

Document related concepts
no text concepts found
Transcript
CHEMISTRY Midterm Practice '05
Name:________________
1. Matter can be divided into three categories:
2. This is a good example of a heterogeneous mixture:
3. Are the following extensive or intensive properties?
A.At 20oC, lead is a solid:
B.The density of lead is 11.35 g/cm3:
C.The mass of a lead sample is 8.00 grams:
4. When cooled, the volume of a sample of gas decreases. Does its density increase or decrease?
5. How many valence electrons does Nitrogen have?:
6. The following are elements (X,Y & Z) as they are found the periodic table:
X
Y
Z
Element Y has a ground state electron configuration that ends with 3p3.
Identify these three elements (symbols only):
X=
Y=
Z=
7. Write the electron configuration for Sulfur:
8. Write the electron configuration for Rubidium:
9. Write the electron configuration for Xenon:
10. Which of the following are ionic compounds? Circle your answers.
A) Calcium Chloride
B) S-2
C) PCl3
D) SrO
E) CO
11. Fill in the table below:
Cl-1
K+1
Mg+2
12. What are the ionic charges on the following?:
N-3
ClO3-1
A) Ba:
B) Al
C) Li
D) O
E) F
F) P
13. Name the following ionic compounds:
A) MgBr2:
B) Li2S:
14. Which of the following are ionic compounds? Circle your answers.
A) Strontium Chloride B) Be+2 C) NF3
D) BaI2
E) NO
15. Fill in the table below:
F-1
P-3
HCO3-1
Rb+1
Al+3
16. What are the ionic charges on the following?:
A) K
B) S
C) Cl
D) N
E) Sr
F) Br
17. What is the frequency (Hz) of a wave with a wavelength of 3.50 x 10-10 m? (c=3.00 x 108 m/s)
18. WRITE FORMULAS FOR THE FOLLOWING:
a. Ferric acetate:
e. Copper (I) oxide:
b. Calcium hydroxide:
f. Lead (IV) iodide:
c. Lithium cyanide:
g. Strontium nitrite:
d. Magnesium fluoride:
h. Magnesium chlorate:
19. Write the names of the following formulas:
a. Al(ClO2)3 :
e. BeI2:
b. Sn(HCO3)4:
f. Al2O3:
c. KI:
g. AgNO3:
d. Cs2S:
h. Ca3P2:
20. Write the formulas of the following compounds:
a. Iron (II) sulfate:
e. Tin (IV) acetate:
b. Nitrogen trifluoride:
f. Carbon tetrabromide:
c. Potassium chlorate:
g. Lithium dichromate:
d. Ammonium chloride:
h. Barium phosphate:
21. Write the names of the following formulas:
a. Al2(CrO4)3 :
e. BeI2:
b. K2CO3:
f. P3O6:
c. PI3:
g. Zn(ClO2)2:
d. Rb2S:
h. Mg3P2:
22. Write the formulas of the following compounds:
a. Copper (I) sulfate:
e. Lead (II) acetate:
b. Nitrogen triiodide:
f. Phosphorus trifluoride:
c. Potassium chlorite:
g. Zinc dichromate:
d. Ammonium phosphate:
h. Barium hydroxide:
23. Write the names of the following formulas:
a. Ca(CrO4)2 :
e. MgI2:
b. Al2(CO3)2:
f. N3O6:
c. CI4:
g. Zn(HCO3)2:
d. Rb2O:
h. Mg3N2:
24. A mole is equal to:
representative particles.
USE MUST SHOW ALL WORK AND USE DIMENSIONAL ANALYSIS.
25. What is the mass of 1 mole of the following:
a) Cobalt:
c) Ba3(PO4)2:
b) NaNO3:
d) Potassium chloride:
26. What is the mass of 0.45 moles of sodium hydroxide?
27. How many moles of carbon are in 1 mole of Al2(CO3)3 ?
28. What is the mass of 0.356 moles of sodium sulfide?
29. How many atoms of vanadium (V) are in 60.0 grams?
30. What is the mass of 20.0 liters of oxygen gas at STP?
31. What is the mass of 3.700 moles of potassium oxide?
32.Which of the following is expressed as an empirical formula?
a) C4H8
b) C9H18
c) CH4
d) C2H2
33. How many atoms of cadmium are in 80.0 grams?
34. What is the volume of 35.50 grams of nitrogen gas at STP?
35. a) Write out and balance the following reaction and answer the problem:
Sodium + Copper (II) nitrate --> sodium nitrate + copper
b) How many grams of copper will be produced if 42.0 grams of sodium is reacted ?
36.
a) Write out the following equation, balance it, and show phase labels:
Aqueous sodium iodide is combined with aqueous lead (II) nitrate to produce an aqueous solution of
sodium nitrate and a lead (II) iodide precipitate.
b) What type of reaction is this? How do you know?
37. Balance the following and give the type of reaction:
A)
____C2H6 + ____O2 ~~>____CO2 + ____H2O
Type____________
B)
____N2 + ____O2 ~~>
Type____________
____ N2O3
C)
____ Ca(HCO3)2 ~~> ____CaO + ____CO2 + ____H2O
Type____________
D)
____(NH4)3PO4 +____ ZnCrO4 ~~> ____Zn 3(PO4)2 (s) +____ (NH4)2CrO4
Type____________
38. Determine which of the following reactions will NOT occur. Write Yes or No.
a) Ba + HCl -->
____________________________
>___________________________
c) NaOH + AlCl3 --
b) Au + NaCl -->
____________________________
>____________________________
d) KCl + NH4Br --
39. Draw Lewis dot diagrams for the following and give the shape of the molecule:
a) F2
b) water
c) CCl4
d) PBr3
40. Describe the following as ionic, polar covalent or nonpolar covalent molecules (use electronegativity table)
a) CO2
b) NaCl
c) NH3
d) H2S
41. What is the % composition of acetic acid?
42. A sample of a compound of carbon and hydrogen is decomposed to produce 0.0134 g of solid carbon and
0.0500 L of hydrogen gas (at STP). What is the empirical formula of the compound?
ADDITIONAL PROBLEMS FOR HONORS STUDENTS ONLY:
43. If an honors chemistry student always drives 55 miles per hour on the highway, what is her speed in
meters/second? (1000 meters = 0.620 miles)
44. An How many Joules of energy is contained in an X-ray with a wavelength of 1.50 x 10-9 m? (c=3.00 x 108
m/s) (h= 6.6 x 10-34J/Hz)
45. Calculate the average atomic mass of element X from the data below:
Isotope
10
X
11
X
12
X
Relative Abundance
19.68%
80.22%
0.1000%
Atomic mass of the Isotope
10.013 u
11.009 u
12.005 u
46. Name the following formulas:
A) KH2PO4:____________________________
C) NH4MnO4 :_______________________________
B) KClO:______________________________
D) HClO4:___________________________________
47. List three ions that are isoelectronic with Krypton.
48. If an empirical formula for a compound is determined to be NO2 and its GFM is 92.02 g/mol, what is the
molecular formula for this compound?
49. Rewrite the following equations as net ionic equations:
a) 3Cu (s) + 2Al(ClO3)3 (aq) --> 3Cu(ClO3)2 (aq) + 2Al (s)
b) 2HCl (aq) + Ca(OH)2 (aq) --> CaCl2 (aq) + 2H2O (g)
50. Write out the full balanced equations for the following decomposition reactions:
a) Ca(OH)2-->
b) Li2CO3 -->
c) Mg(ClO3)2 -->
d) K2SO4 -->
51. 14.0 grams of magnesium undergoes an addition (synthesis) reaction when combined with 7.90 liters of
oxygen (at STP). Which is the limiting reactant and which is the excess reactant? How much of the excess
reactant remains (in liters)?
Related documents