Classify each of the following as a pure substance (A) or a mixture (B)
(1) copper
(2) water
(3) nitrogen
Classify each of the following as a compound (A), element (B), or mixture (C):
(4) gasoline
(5) carbon dioxide
(6) sulfur
The following are properties of the element cesium; classify them as physical (A) or chemical(B) properties
(7) metals bum in fluorine
(8) When cesium is add to water, hydrogen is given off and the metal dissolved
(9) boiling point 678.4 °C
(10) Cesium has a hardness on the Mobs scale of 0.2
(11) yellow gas
Classify the following changes as physical (A) or chemical (B)
(12) melting of gold
(13) mixing sugar with water
(14) rusting of nail
(15) separating components of oil by distillation
(16) coal burning
(17) exploding of nitroglycerin
Using the Periodic Table, determine to which group (family), e.g. alkali (A), alkaline earth (B), chalcogen (C), halogen (D), noble gas (E) each of the following elements belongs.
(18) calcium
(19) iodine
(20) sulfur
Using the Periodic Table, classify the following elements as metals (A), nonmetals (B), or metalloids (C).
(21) boron
(22) nitrogen
(23) barium
Using the Period Table, indicate the number of valence electrons for each of the following elements:
(24) oxygen A. two B. six C. five D. seven E. none of A to D.
(25) bismuth A. two B. three C. five D. seven E. none of A to D.
(26) aluminum A. two B. three C. five D. seven E. none of A to D.
Predict whether each of the following compounds is molecular (A) or ionic (B):
(27) Ag2aSO4,
(28) CH3OH
(29) PF5
(30) NOCI
(31) LaP
(32) CsBr
33. Naturally occurring magnesium has the following isotopic abundances. What is the average atomic mass of Mg?
|
Isotope
|
Abundance
|
Atomic mass (amu)
|
|
24Mg
|
78.99%
|
23.98504
|
|
25mg
|
10.00%
|
24.98584
|
|
26ma
|
11.01%
|
25.98259
|
34. Fill in the gap in the following table, assuming each column represents a neutral atom.
|
Symbol
|
65Zn
|
|
|
|
|
|
Protons
|
|
38
|
|
|
92
|
|
Neutrons
|
|
58
|
49
|
|
|
|
Electrons
|
|
|
38
|
36
|
|
|
Mass no
|
|
|
|
81
|
235
|
35. Fill in the gap in the following table.
|
Symbol
|
31P3-
|
|
|
|
|
Protons
|
|
34
|
50
|
|
|
Neutrons
|
|
45
|
69
|
118
|
|
Electrons
|
|
|
46
|
76
|
|
Net charges
|
|
2- |
|
3+
|
36. Complete the table by filling in the formula for the ionic compound formed by each pair of cations and anions, as shown for the first pair.
|
Ion
|
K+ |
NH4+
|
Mg2+
|
Fe3+
|
|
Cl-
|
KCl
|
|
|
|
|
OH-
|
|
|
|
|
|
O2-
|
|
|
|
|
|
N3-
|
|
|
|
|
|
CO32-
|
|
|
|
|
|
PO43-
|
|
|
|
|
37. Using the periodic table to guide you, predict the chemical formula and name of compound formed by the following elements:
(a) Ga and F (b) Li and H (c) Al and S (d) Ba and N (e) K and 0.
38. Calculate the number of carbon dioxide molecules in 0.235 moles of carbon dioxide.
a. 0.235
b. 6.02x1023
c. 2.56 x 1024
d. 1.42 x 1023
e. none of a to d
39. Calculate the number of grams of cupper (II) sulfide in 0.584 moles of cupper (II) sulfide.
a. 93.2 g
b. 58.4 g
c. 55.8 g
d. 164 g
e. none of a to d
40. Calculate the number of moles of potassium carbonate in 955 mg potassium carbonate.
a. 6.91 mol
b. 132 mol
c. 1000 mol
d. 0.00691 mol
e. none of a to d
41. Calculate the number of grams of sulfur dioxide in 1.86 x 1022 molecules of sulfur dioxide.
a 1.98 g
b. 1.86 g
c 0.309 g
d. 119 g
e. none of a to d
42. Calculate the number of moles of carbon atoms in 46.7 grams of calcium acetate.
a. 0.295 mol
b. 1.18 mol
c. 1.89 mol
d. 0.471 mol
e. none of a to d
43. What are the numbers of SO2 molecules in 20.0 grams of SO2?
a. 0312
b. 1.88 x1023
c. 2.56 x 1026
d. 1.42 x 1023
e. none of a to d
44. Calculate the percent composition of Zn3(PO4)2.
a. 16.0 % Zn, 50.8% P, 33.2% O
b. 50.8 % Zn, 16.0% P, 33.2% O
c. 33.2 % Zn, 16.0% P, 50.8 % O
d. 50.8 % Zn, 33.2% P,16.0% O
45. A 0.279 g sample of iron was heated to the resulting product with a mass of 0.400 g. Determine the empirical formula for iron oxide.
a. FeO
b. FeO3
c. Fe2eO3
d. Fe3sO4
e. none of a to d
46. A compound has the following composition: 48.0% carbon, 4.0% hydrogen, 22.4% nitrogen, 12.8% sulfur and 12.8% oxygen. The molecular mass is found to be 250. amu. Determine the molecular formula for the compound.
a C10H1IN5SO
b. C5HN2S3O
c. C1OHI2N5SO
d. C10H10N4SO2
47. Calculate the number of grams of barium phosphate that could be produced by reaction of 50.8 g of barium chloride with excess sodium phosphate.
3 BaC12(aq) + 2 Na3PO4 (aq) → 6 NaCl (aq) + Ba3(PO4)2 (s)
a 48.9 g.
b. 25.4 g
c. 100. g
d. 147 g
e. none of a to d
48. Calcium carbonate is formed when calcium oxide combines with COz.
CaO(s) + CO2(g) → CaCO3(s)
Calculate the grams of calcium carbonate that could be formed from the reaction of 14.5 g of calcium oxide with 12.0 grams of carbon dioxide. If 15.3 g of calcium carbonate are actually formed, what is the percent yield?
a. 15.3 g, 25.0%
b. 25.9 g, 59.1 %
c. 25.9 g, 169%
d. 153 g, 59.1%
Problem 49-51: A commercial method of manufacturing hydrogen involves the reaction of iron and steam. A
3 Fe(s) + 4 H2O → Fe3O4 (s) + 4 H2 (g)
49. How many moles of H2 can be produced from 42.7 g Fe and an excess of H2O (g) ?
a. 0.765 mol
b. 3.06 mol
c. 1.02 mol
d. 0.471 mol
e. none of a to d
50. How many grams of H2O are consumed in the conversions of 63.5 g Fe to Fe3O4?
a. 1.14 g
b. 4.55 g
c. 1.52 g
d. 27.3 g
e. none of a to d
51. If 7.36 mol H2(g) is produced, how many grams of Fe3O4 must also be produced?
a. 426 g
b. 232 g
c. 1.84 g
d. 342 g
e. none of a to d
52. Balance the following reaction equations.
Eg. ___1___ MgO (s) + ___1___ H2O (g) → ___1___ Mg(OH)2 (s)
(a) ______ Na(s) + _____O2 (g) → ________Na2O (s)
(b) ______ K2O (s) + _____H2O(l) → ______ KOH (aq)
(c) _______ H2O2 (l) → _______ H2O (l) + ______O2 (g)
(d) _______ C5H6O(l) + ______O2 → ______CO2 + H2O
(e) _______ I2O7(s) + H2O(l) → _______HIO4 (aq)
(f) _______ H3PO4(aq) + ________Ca3(PO4)2 (aq) → Ca(H2PO4)2
(g) ______ NaHCO3 (s) → _______Na2CO3 (s) + ________CO2(g) + H2O(g)
(h) ______ KClO3(s) → ______O2 (g) + _____ KCl(s)
(i) ______ C2H4 (g) + _______ O2 (g) → ______CO2 (g) + _________H2O (g)
53. Using the periodic table to guide you, predict the chemical formula and name of compound formed by the following elements: (a) Ga and F (b) Li and H (c) Al and S (d) Ba and N (e) K and 0.
54. Name the following compounds:
(a) Li2O (b) NO (c) P2O5 (d) Fe (NO3)2 (e) NaClO (f) KClO4 (g) CaSO3 (h) NaBrO2 (i) NaH2PO4, (j) Ag2Cr2O7 (k) H2CO3 (i) HNO2 (m) S2Cl2 (n) Ca3N2 (o) HClO3 (p) HCl (aq) (q) Cu(OH)2 (r) Hg2(OH)2 (s) CuCl
55. Give the chemical formula for the following Compounds:
(a) hydroiodic acid (b) chromium(III) acetate (c) ammonium dichromate
(d) sulfurous acid (e) mercury (I) chloride (f) potassium permanganate
(g) sodium cyanide (h) dinitrogen tetroxide (i) diloric acid (j) hydrocyanic acid (k) potassium monohydrogen phosphate (l) calcium hydroxide (m) iron(III) oxide