Honors Chemistry MIDTERM STUDY GUIDE
1.
Convert 2.045 km to mm
2.
What is the correct reading of the volume of liquid in the graduated cylinder on the right?
3.
What is the mass of 7.5 cm3 of Silver (Density of Silver = 10.5 g/cm3). Answer to the correct
number of significant figures.
Use the three tables below to answer question 4
Table One (Substance
One)
Mass
1.
Volume
Table Two (Substance
Two)
3. Mass
3
2.
Volume
Density of
Substances
Substance Density
3
5g
10 cm
4. 5 g
5 cm
Sodium
1 g/ cm3
10 g
20 cm3
5. 10 g
10 cm3
Calcium
1.55 g/ cm3
15 g
30 cm3
6. 15 g
15 cm3
Carbon
2.26 g/ cm3
20 g
40 cm3
7. 20 g
20 cm3
Lithium
0.50 g/cm3
25 g
50 cm3
8. 25 g
25 cm3
4.
From the data in tables one and three, sample one is most likely_______________.
5.
Four students each measured the mass of one 7.25 g sample four times. The results in the table below indicate that the data
collected by ____________ reflect the greatest accuracy and precision
Mass Data of Sample
Student A
Student B
Student C
Student D
6.
Trial 1
7.30 g
6.95 g
7.54 g
7.24 g
Trial 2
7.21 g
7.40 g
7.58 g
7.24 g
Trial 3
7.27 g
7.36 g
7.50 g
7.25 g
Trial 4
7.35 g
7.44 g
7.56 g
7.26 g
The following illustrations depicts
(A)
(B)
(C)
(D)
(E)
An element
A compound
A mixture of elements
A mixture of compounds
A mixture of elements and compounds
7.
Which of the following rationales explains why iron rusting is classified as a chemical change?
a. Changes shape
b. Changes size
c. Produces new substances
8.
What did Rutherford discover?
9.
How many protons and electrons are in an atom of Iron?
10. Cl-35 (atomic number 17) has how many neutrons?
11. Isotopes are atoms of the same element with different _____________?
12. Find the average atomic mass of this element given the abundance of the isotopes?
Isotopes of an element
Abundance
Mass
(%)
(amu)
65.10
23.41
14.20
22.19
20.70
22.75
13. What is the longhand electron configuration for Manganese?
14. What is the shorthand electron configuration for Titanium?
15. In each of the following pairs, circle the larger particle
a. Na or Al
b. Ba or Be
c. Cl or Cld. K or K+
16. What type of compound is soluble in water, has a high melting point, conducts electricity when dissolved in water, and forms
between a metal and a nonmetal?
17. What type of compound is usually insoluble in water, has a low melting point, does not conduct electricity, and forms
between two nonmetals.
18. Use the data table below to determine which compounds should be grouped as ionic, covalent, and polar covalent:
Substance
Sodium carbonate
Boron trifluoride
Acetylene
Camphor
Selenium dichloride
Melted
No
Yes
Yes
Yes
Yes
Solubility
Soluble
Soluble
Insoluble
Insoluble
Slightly soluble
Conductivity
High
Low
None
None
Low
19. Classify the C--- Br bond in CBr4 as ionic, polar covalent, or nonpolar covalent.
20. How many unshared pairs of electrons surround the central atom in each of the following molecules?
a. CO2
b. H2S
c. PH3
d. CCl4
21. What is the VSEPR shape for each of the molecules in question 20?
22. What is the polarity of each of the molecules in question 20?
23. What is the Lewis structure for N2H2?
24. Potassium reacts with a certain element to form a compound, KX. If Calcium reacts with element X, what will the formula of
the resulting compound be?
25. What is the cation in NH4NO3?
26. What is the chemical name for SBr5?
27. What is the formula for Calcium iodide?
28. Name the following substance: NiPO4 ∙ 7 H2O
29. Write the name for the following acid: H2CO3
30. What is the volume for one mole of gas at STP?
31. What is the molar mass of C6H6?
32. Convert 250.0 g of MgO to moles.
33. How many bromine atoms are present in 3.00 mol of AlBr 3?
34. What is the mass, in grams, of one iron atom?
35. How many liters is 2.55 x 1024 molecules of Cl2 gas at STP?
Think back to the mole unit experiment done in class…use the data table below to answer the following questions:
Trial
#
1
Initial Mass of Nail
(Fe + Zn)
6.55
Final Mass of Nail
(Fe)
6.13
2
6.34
5.80
36. What is the average mass of Zinc?
37. If the nail was removed from the acid too soon, how would that affect the results?
38. What is the molarity (M) of a solution that has 9.0 moles of solute dissolved in 2.5 liters of solvent?
39. What mass of MgCl2 is needed to prepare 300.0 mL of 0.500 M Magnesium Chloride solution?
40. What is the difference between an empirical and a molecular formula?
41. A compound contains 259.2 g of F and 40.8 g of C. What is the empirical formula of this compound?
42. If the molecular mass of the compound in question #41 is 176.0 g/mol, what is the molecular formula of the compound?
43. What is the percent by mass of water in the hydrate, CuSO4 · 5H2O?
44. A 5.36 g sample of the hydrate, Na2SO4 · n H2O, on heating produces 2.52 g of water. What is the empirical formula of this
compound?
45. What are the coefficients that balance the chemical reaction below:
___H3PO4 + ___MgF2 → ___Mg3(PO4)2 + ___ HF
46. Flourine gas is passed over solid potassium. Write the balanced equation for the reaction that would occur.
47. Write the balanced equation for the decomposition of hydrochloric acid?
48. Predict the products of the following reaction: Mg(s) + HNO3 (aq) →
49. Write the balanced equation for the reaction between solutions of silver nitrate and potassium bromide
50. Write the correct balanced equation for the combustion of sucrose, C12H22O11
51. Write the TOTAL IONIC equation for a reaction between aqueous lead (II) nitrate and aqueous potassium chloride solutions.
52. Write the NET IONIC equation for the reaction given in question #52.
53. Think back to the Electrolysis of Water Lab done in class.
a. Which gas did you collect more of?
b. Which gas was collected at the red (positive) electrode?
c. Which gas was collected at the black (negative) electrode?
54. How is a mole ratio used in stoichiometric calculations?
55. Given the following reaction, what is the mole ratio of iron to chlorine? 2 Fe (s) + 3 Cl2 (g) → 2FeCl3 (s)
56. Using the equation given in question #55, how many moles of iron (III) chloride can be obtained from 9 moles of chlorine
gas?
57. For the reaction, 2NO(g) + O2(g) → 2NO2(g), how many moles of NO2 can be produced from 150.0 grams of NO?
58. For the reaction, 2KClO3 (s) → 2KCl (s) + 3O2 (g), how many grams of KCl can be produced from 200.0 g of KClO3?