Reference no: EM131108727

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 C₁₀H_1IN₅SO
b. C₅HN₂S₃O
c. C_1OH_I2N₅SO
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 BaC1_2(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) + CO_2(g) → CaCO_3(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) + _____O_{2 (g)} →  ________Na₂O (s)

(b) ______ K₂O (s) + _____H₂O(l) → ______ KOH (aq)

(c) _______ H₂O₂ (l)  → _______ H₂O (l) + ______O₂ (g)

(d) _______ C₅H₆O(l) + ______O₂ → ______CO₂ +   H₂O

(e) _______ I₂O_7(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