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PreAP Chemistry Spring 2016 Final Exam Review
Name ionic compounds containing main group or transition metals, covalent compounds,
acids, and bases, using International Union of Pure and Applied Chemistry (IUPAC)
nomenclature rules
Write the chemical formulas of common polyatomic ions, ionic compounds containing main
group or transition metals, covalent compounds, acids, and bases
1. Name and write formulas for ionic compounds
a. Na2O
b. FeCl3
c. Cu(NO3)2
d. BaCO3
e. Lithium nitride
f. lead (II) chloride
g. mercury (II) chlorate
2. When are roman numerals used in the names of ionic compounds?
3. Which compounds have names that end in “ate” or “ite”?
4. What type of ions have names ending in “ide”?
5. Name and write formulas for covalent compounds
a. N2O5
b. SF6
c. Diarsenic trioxide
d. Carbon tetrachloride
6. Name and write formulas for acids
a. HBr
b. H2SO3
c. HClO4
d. Nitrous acid
e. Hydroiodic acid
f. Acetic acid
Construct electron dot formulas to illustrate ionic and covalent bonds
Predict molecular structure for molecules with linear, trigonal planar, or tetrahedral electron pair
geometries using Valence Shell Electron Pair Repulsion (VSEPR) theory.
7. Be able to write Lewis dot structures for molecules showing covalent bonds and unshared electron pairs
(FOLLOW THE STEPS)
a. CO2
b. NH3
c. H2O
d. BF3
e. SO2
f. BeF2
g. CH4
8. Predict the molecular geometry for each of the molecules listed in #7.
9. Which atoms are exceptions to the octet rule with fewer than 8 electrons?
10. Which atoms can have multiple covalent bonds?
11. Define diatomic molecule.
12. List the seven elements that exist in nature as diatomic molecules.
PreAP Chemistry Spring 2016 Final Exam Review
Describe the nature of metallic bonding and apply the theory to explain metallic properties
such as thermal and electrical conductivity, malleability, and ductility
13. List the properties of metals
14. Define metallic bond.
Define and use the concept of a mole.
Use the mole concept to calculate the number of atoms, ions, or molecules in a sample of material.
Calculate percent composition and empirical and molecular formulas.
15.
16.
17.
18.
19.
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21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
31.
What is the formula mass of tin (II) perchlorate?
How many hydrogen atoms would there be in 6 formula units of ammonium acetate?
Which of the following is correct?
(a) mass equals moles divided by molecular mass
(b) moles times mass equals molecular weight
(c) moles equals molecular mass times mass (d) mass equals molecular weight times moles
(e) molecular weight equals moles divided by mass
Which of the following one gram sample of crystals would contain the MOST formula units?
(a) sodium chloride (b) sodium bromide (c) sodium fluoride (d) sodium iodide (e) sodium sulfide
Which would contain more molecules, 1/3 mole of water or 1/3 mole of sulfur dioxide gas?
How many moles are there in 3.67 x 1024 atoms of helium gas? Helium (He) is #2.
I am holding 0.0452 moles of a pure element and it weighs 542 mg. What element is it?
How much would 7.12  109 formula units of silver sulfate weigh in grams? The formula mass of
silver sulfate is 312 g/mole
If 499.5 grams of monatomic pure element are known to contain 2.6858  1024 atoms of that
element, what element is it?
How many molecules of water weigh the same as 100 billion carbon dioxide molecules?
How many grams of pure copper can be obtained from decomposing 4.78 grams of copper (II)
phosphate?
Which of the following is NOT an empirical formula?
(a) C91H168O84Br7N6 (b) C24H42O12Cl9 (c) C9H6O (d) C24H44O21 (e) all are empirical
A chemist has a 100-gram sample of a compound that contains 17.073 grams of carbon, 2.168
grams of hydrogen, 10.840 grams of oxygen, 8.5366 grams of nitrogen, 28.8618 grams of
chlorine and the rest is bromine. What is the empirical formula of the compound?
Refer to Question # 27 to answer this question. If the molecular mass of the compound in
Question #27 is between 8000 and 9000 g/mole, what is the factor by which you would multiply
all the subscripts in the empirical formula by to find the molecular formula?
A compound contains twice as many oxygen atoms as it has nitrogen atoms, 4 times as many
hydrogen atoms as it has oxygen atoms and one-half as many carbon atoms as it has hydrogen
atoms. Its molecular weight is 510 g/mole. What is the whole-number multiplier which you
would use to multiply the subscripts of the empirical formula by?
What is the percentage by mass of carbon in dimethylsulfoxide, C 2H6SO?
What is the percentage by mass of H in CH 4?
PreAP Chemistry Spring 2016 Final Exam Review
Use the law of conservation of mass to write and balance chemical equations
32.
Pure bismuth reacts with nitrogen dioxide to produce bismuth (III) oxide and nitrogen monoxide
as the only products. What is the sum of the coefficients of the products in this reaction?
(a) 3 (b) 4 (c) 5 (d) 6 (e) none of these
33.
Iron (II) selenide reacts with oxygen gas to produce iron (III) oxide plus selenium dioxide. What is
the sum of the coefficients of the reactants? (a) 17 (b) 6 (c) 11 (d) 9 (e) none of these
34.
What is the sum of ALL of the coefficients when isopropyl alcohol (C3H7OH) reacts with oxygen
gas to produce carbon dioxide and water? (a) 25 (b) 21 (c) 18 (d) 12 (e) none of these
35.
What is the sum of the coefficients of the PRODUCTS when tin (IV) nitrate reacts with iron (III)
sulfate? The products of the reaction are tin (IV) sulfate and iron (III) nitrate. (a) 12 (b) 7 (d) 5 (d) 14
(e) reaction will not take place
Perform Stoichiometric calculations, including determination of mass relationships between reactants
and products, calculations of limiting reagents, and percent yield.
36.
If 1.00 g of liquid ethanol (C2H5OH) is completely burned in oxygen gas, how many molecules of
carbon dioxide are formed? Water vapor is a second product of the reaction. (a) 1.31  1022 molecules
(b) 2.62  1022 molecules
(c) 1.02  1023 molecules
(d) 4.33  1025 molecules
(e) 2.04 
25
10 molecules
37.
If 4.0 moles of carbon disulfide had been reacted with excess oxygen, _(?)_ moles of sulfur
dioxide and _(?)_ moles of carbon dioxide would be formed? (a) 4.0, 8.0 (b) 3.0, 6.0(c) 8.0, 4.0 (d)
4.0, 2.0 (e) 8.0, 16
38.
If 88.0 liters of hydrogen gas at STP react with 3.4 moles of iodine vapor in a synthesis reaction,
how many liters of HI gas will be formed at STP? (a) 44 liters (b) 152 liters (c) 176 liters (d) 88
liters (e) 76.2 liters
39.
Equal masses of liquid hexane and liquid octane are burned in oxygen gas. Which would produce
the greater volume of carbon dioxide at STP? Water vapor is a second product of the reaction. (a)
hexane (b) octane (c) they would be the same since the masses are the same (d) you must be given
the density of each liquid to work this problem (e) liquids will not burn
40.
Which of the following is NOT a true statement concerning limiting and excess reactants?(a) the
amount of product obtained is determined by the limiting reactant (b) a balanced equation is necessary
to determine which reactant is the limiting reactant (c) some of the excess reactant is left over after the
reaction is complete (d) the reactant that has the smallest given mass is the limiting reactant (e)
adding more of the limiting reactant to the reaction flask will cause more product to be produced
41.
Identify the limiting reactant when 150 grams of carbon disulfide (MW = 76 g/mole) reacts with
167 grams of oxygen (MW = 32 g/mole). The products of the reaction are sulfur dioxide and carbon
dioxide. (a) carbon disulfide (b) oxygen(c) carbon dioxide (d) sulfur dioxide (e) there is no limiting
reactant here
42.
_(?)_ grams of _(?)_ will be left over in the above reaction. (a) 132 g carbon disulfide(b) 17.8 g
oxygen (c) 53.3.0 g oxygen (d) 17.8 g carbon disulfide (e) 95.0 g oxygen
PreAP Chemistry Spring 2016 Final Exam Review
43.
When a balanced equation is used to calculate the amount of product that will form during a
reaction, the value obtained by the calculation is known as the (a) theoretical yield (b) actual yield (c)
percent yield (d) percent error (e) limiting reactant
44.
When 50.0 grams of ethane are completely combusted with oxygen gas, 72.3 grams of water are
produced (carbon dioxide is also a product). What is % yield of the reaction? (a) 80.3% (b) 64.34% (c)
35.7% (d) 19.7% (e) none of these
45.
Given the following decomposition: lead (II) nitrate decomposes to yield lead (II) oxide plus
nitrogen dioxide plus oxygen gas
What is the percent yield of this reaction if 9.90 grams of lead (II) nitrate (FW = 331 g/mole) is heated and
yields 5.50 grams of lead (II) oxide (FW = 223 g/mole) (a) 18% (b) 44% (c) 56% (d) 67% (e) 82%
Describe the unique role of water in chemical and biological systems
46.
How does the boiling point of water compare with the boiling point of other molecules of similar
size? (a) It is higher (b) It is lower (c) It is about the same
47.
What is the shape of the water molecule? (a) pyramidal (b) bent (c) trigonal planar
tetrahedral (e) linear
48.
The attraction between the negative end of one water molecule and the positive end of another
water molecule is called a ___. (a) dispersion force (b) hydrogen bond (c) polar covalent bond (d)
ionic bond
49.
50.
(d)
Water is NOT a good solvent for substances that are ____. (a) ionic (b) polar (c) nonpolar
The fact that ice is less dense than water is related to the fact that ___. (a) the molecular
structure of ice is much less orderly than that of water (b) ice has a molecular structure that is an open
framework held together by hydrogen-bonding (c) ice has a molecular structure in which water
molecules are arranged randomly (d) the molecules of ice are held to each other by covalent bonding
Develop and use general rules regarding solubility. Investigate factors that influence solubilities and
rates of dissolution such as temperature, agitation and surface area.
51.
Which of the following would dissolve in water? (a) lead (IV) sulfate (b) mercury (II) carbonate
(c) strontium chloride (d) silver iodide (e) more than one of these would dissolve
52.
Which of the following compounds could be added to a solution of silver nitrate to cause a
precipitate to form? (a) hydrochloric acid (b) acetic acid (c) nitric acid (d) lead (II) chlorate (e)
uranium (VI) perchlorate
53.
Which of the following is NOT soluble in water? (a) strontium sulfate (b) Pb(SO4)2
HgI2 (d) Hg2(ClO4)2 (e) more than one of these is not soluble
54.
Which of the following compounds would dissolve in water? (a) iodine pentafluoride (b)
butane (c) bromine (d) carbon tetrachloride (e) none of these
55.
As temperature increases, the solubility of solids ______ and the solubility of gases ______.
(a) decreases, decreases
(c) decreases, increases
(b) increases, decreases
(c)
PreAP Chemistry Spring 2016 Final Exam Review
56.
Under which conditions of temperature and pressure is a gas most soluble in water? (a) high
temperature and low pressure (b) high temperature and high pressure (c) low temperature and low
pressure (d) low temperature and high pressure
Calculate the concentration of solutions in units of molarity. Use molarity to calculate the dilutions of
solutions.
57.
The molarity of an aqueous solution of NaCl is defined as the ___. (a) grams of NaCl per liter of
water (b) grams of NaCl per liter of solution (c) moles of NaCl per liter of water (d) moles of NaCl per
liter of solution
58.
What is the molarity of 1.5 liters of an aqueous solution that contains 52 grams of lithium
fluoride? (a) 35 M (b) 1.3 M (c) 3.0 M (d) 0.33 M
59.
How many milliliters of 15.0 M acetic acid must be used to prepare 4.50 liters of a 3.33 M acid
solution? (a) 999 ml (b) 0.999 ml (c) 20.3 ml (d) 66.8 ml (e) must be given a constant for acetic acid
in order to work the problem
60.
50.0 g of sodium bromide are dissolved in enough water to make 500 ml of solution. After the
solution is made, 75 ml of it are withdrawn and diluted with 200 ml of water. What is the molarity of the
final diluted solution? (a) 0.36 M (b) 1.76 M (c) 2.45 M (d) 0.26 M (e) none of these
61.
If 50.0 ml of stock nitric acid solution whose molarity is 16.0 M is diluted until the molarity of the
diluted solution is 5.0 M, how many ml of water did you add? (a) 160 ml water (b) 210 ml water (c)
110 ml (d) 15.6 ml (e) none of these
Distinguish between types of solutions such as electrolytes and nonelectrolytes and unsaturated,
saturated, and supersaturated solutions.
62.
Which of the following would you expect to conduct an electric current? (a) Pr (s) (#59) (b)
liquid NH3 (c) KF(s) (d) LiCl(aq) (e) more than one of these would conduct an electric current.
63.
How many grams of potassium
nitrate would dissolve in 250 grams of
water at 40oC?
(a) 13 g
(b) 60 g
(c) 120 g
(d) 150 g
(e) 180 g
64.
How many grams of ammonium
chloride would dissolve in 735 grams of
water at 90oC?
(a) 515 g
(b) 70 g
(c) 237 g
(d) 490 g
(e) 334 g
PreAP Chemistry Spring 2016 Final Exam Review
65.
How many more grams of potassium nitrate would dissolve in 200 grams of water when the
temperature is increased from 10oC to 70oC?
(a) 100 g (b) 75 g (c) 150 g (d) 200 g (e) 250 g
66.
300 grams of ammonium chloride are added to 465 grams of water at 50 oC. By how many
degrees must the temperature BE RAISED before all of the ammonium chloride will dissolve? (a) 80 oC (b)
-30oC (c) -80oC (d) 30oC (e) not possible to raise the temperature high enough to get it all to dissolve
67.
A student is working with a solution in chemistry lab. The student places a seed crystal into the
solution and many crystals quickly form. The student is working with a solution that is -- (a) saturated
(b) immiscible (c) unsaturated (d) supersaturated
Define acids and bases and distinguish between Arrhenius and Bronsted-Lowry definitions and predict
products in acid base reactions that form water.
68.
]
In an alkaline solution, ____.
(a) [H3O+] = [OH-]
+
(d) [H3O ] = 0 M
(e) [OH ] > 7.00
69.
I. sour
(a) I only
Alkaline solutions are generally
II. Bitter III. Slippery
(b) I & II (c) II only (d) II, III
(b) [H3O+] > [OH-]
(c) [H3O+] < [OH-
(e) I, II, & III
70.
Name H3As. (a) hydroastatic acid (b) hypoarsenous acid (c) hydroarsenic acid (d) arsenous
acid (e) none of these.
71.
Acids with the ending (-ous) come from (a) Polyatomic ions ending in –ide.
(b)
Polyatomic ions ending in –ite.
(c) Polyatomic ions ending in –ate.
(d) Polyatomic ion
beginning with per- and ending in –ate.
72.
Which solution below has the highest concentration of hydroxide ions?
pH = 3.21 (b) pH = 12.59 (c) pH = 7.93 (d) pH = 9.82 (e) pH = 7.00
73.
(a)
A solution with a hydroxide ion concentration of 1  10-7 M.
(a) acidic (b) basic (c) neutral
74.
A Brønsted base is defined as a substance that ___. (a) Increases [H +] when placed in H2O (b)
Decreases [H+] when placed in H2O (c) Increases [OH-] when placed in H2O
(d) Acts as a [H+]
+
acceptor in any system (e) Acts as a [H ] donor in any system
75.
In the reaction:
NH3 + HCl  NH4+ + ClThe NH3 acts as (a) a Bronsted acid (b) a Bronsted base (c) both a Bronsted acid and a Bronsted base (d)
neither a Bronsted acid nor a Bronsted base
Define pH and use the hydrogen or hydroxide ion concentration to calculate the pH of a solution
76.
77.
If [H+] = 1.3 X 10-6 M, is this solution acidic or basic?
If [OH-] = 1.29 X 10-8 M, what is the [H+]? (a) 7.89
8.32 X 10-8 M (e) none of these
(a) acidic
(b) basic
(b) 7.75 X 10-7 M
(c) 1.29 X 10-8 M (d)
PreAP Chemistry Spring 2016 Final Exam Review
78.
If the pH of a strong monoprotic acid solution is known to be 1.24, what is the molar
concentration of acid? (a) 1.24 M (b) 1.11 M (c) 0.116 M (d) 0.058 M (e) none of these
79.
What is the pH when the hydrogen ion concentration is 7.0 x 10-3 M? (a) 3.00 (b) 2.2 (c) 2.15
(d) 11.85 (e) 12
80.
What is the pH of a solution with a [OH-] = 4.5 x 10-9 M? (a) 8.35 (b) 8.3 (c) 9.00 (d) 5.65 (e)
5.7
Distinguish between degrees of dissociation for strong and weak acids and bases
81.
Which of the following is not a strong acid or strong base?
HNO2 (d) HI (e) KOH (f) NaOH
82.
A solution of an acid that ionizes completely in water would be termed (a) concentrated (b)
strong (c) dilute (d) weak
83.
(a) HClO 4
(b) Ba(OH)2
(c)
Which of the following dissociates incompletely? (a) HF (b) HClO4 (c) HCl (d) H2SO4
Describe and calculate the relations between volume, pressure, number of moles and temperature for
an ideal gas as described by Boyle’s law, Charles’ law, Avogadro’s law, Dalton’s law of partial pressure
and the ideal gas law
84.
If 3.21 mol of a gas occupies 56.2 L at 44ºC and 793 torr, 5.29 mol of this gas occupies _____
under these conditions. (a) 14.7 L (b) 61.7 L (c) 30.9 L (d) 92.6 L (e) 478 L
85.
A 24.2 g sample of gas initially at 4.00 atm was compressed from 8.00 L to 2.00 L at constant
temperature. What would be the new pressure after the compression?
(a) 4.00 atm
(b) 2.00 atm (c) 1.00 atm (d) 8.00 atm (e) 16.0 atm
86.
What happens to a volume of gas if the pressure is doubled and the temperature Kelvin is
tripled? (a) the volume decreases to 2/3 of its original (b) the volume increases to 3/2 its original (c)
the volume remains unchanged (d) the volume increases to 4/3 its original (e) the volume decreases to
3/4 its original
87.
To what temperature Celsius must a sample of helium be heated in order to increase its volume
from 8.00 liters to 13.2 liters if the original temperature is –20oC and the pressure remains constant? (a)
123ºC (b) 213ºC (c) 144ºC (d) 25.4ºC (e) 30.5ºC
88.
The volume of a gas is 158 liters when the pressure is 763 torr and the temperature is 21ºC. The
volume expands to 192 liters when the pressure is changed to 548 torr. How much has the temperature
CHANGED Celsius? (a) 37.4ºC (b) 16.4oC (c) - 4.6oC (d) -16.4oC (e) -37.4oC
Perform Stoichiometric calculations, including determination of mass and volume relationships
between reactants and products for reactions involving gases
89.
The molar volume of a gas at STP is _____.
(e) 14.7 L
(a) 0.08206 L
(b) 62.36 L
(c) 1.00 L
(d) 22.4 L
PreAP Chemistry Spring 2016 Final Exam Review
What is the volume occupied by 0.333 mol of neon gas at STP? (a) 22.4 L (b) 0.00 L (c) 7.46 L
90.
(d) 149 L
91.
According to the following equation, what volume of hydrogen gas at STP is needed to
completely react with 32.00 g of oxygen to form water? 2H2(g) + O2(g)  2H2O(l)
(a) 4.04 L (b) 11.2 L (c) 22.4 L (d) 44.8 L
Describe the postulates of kinetics molecular theory
92.
Which of the following has the greatest kinetic energy? (a) 10 grams of hydrogen at 25ºC and
700 torr (b) 10 grams of nitrogen at 100ºC and 700 torr (c) 10 grams of helium at 10ºC and 700 torr
(d) 10 grams of carbon dioxide at 30ºC and 700 torr (e) they all have the same kinetic energy.
93.
Which statement best describes the particles of an ideal gas based on the kinetic molecular
theory? (a) the particles are relatively far apart and have negligible volume (b) the particles are in
constant nonlinear motion (c) the particles have attractive forces between them (c) the gas particles
have collisions that lose energy
Perform calculations using heat, mass, temperature change, and specific heat
Use calorimetry to calculate the heat of a chemical process
94.
An unknown metal with a mass of 10.0 grams is heated to a temperature of 74 oC and is dropped
into 100. grams of water with an initial temperature of 30oC. The final temperature of the system is 32oC.
What is the specific heat of the unknown metal in J/g∙ oC? (Use cp = 4.186 J/g∙oC for water)
(a) 2.0 (b) 0.20 (c) 1.9 (d) 0.19
95.
What is the heat capacity (in J/g∙oC) of gold if it takes 15.48 J of energy to raise the temperature
of 24.0 g by 5.00oC?
(a)
0.909 (b) 0.385 (c) 2.03 (d) 0.129 (e) 0.00108