CHEM1305 Introductory Chemistry
Chapter 1 Discussion
Chemistry in Our Everyday Lives
In this discussion, you will give an example of an item used in our everyday world that was made with chemistry (hint: everything man-made was made using chemistry!). List the item first and then give a brief description of the chemistry behind the item.
You can come up with your own idea, but I highly recommend using an item from the following website: https://pubs.acs.org/cen/whatstuff/stuffABCText.html (Links to an external site.)
There, you can click an item, and use the corresponding article to come up with a description of the chemistry behind that item.
Your post must be at least 3-4 sentences in length.
Click "Reply " below this box to post to the discussion.
To help, here is an example discussion post:
Dryer sheets
Dryer sheets are pieces of material covered with a special softening agent. The softening agent will melt off when heated and next stick to the fabrics as they are being dried. The softening agent not only makes fabric feel softer, it also helps to dissipate static charge. A heat-resistant fragrance is often added to dryer sheets, which will transfer to fabrics as well.
CHEM1305 Introductory Chemistry
Chapter 2 Discussion
Metric or English System?
In this discussion, you will give your opinion about which system of measurements you prefer. In the United States, the English system is used (units of length are inches, feet, yards, miles; units of mass are ounces and pounds; units of volume are quarts, pints, gallons; units of temperature are degrees Fahrenheit). In the rest of the world, the Metric system is used (units of length are centimeters, meters, kilometers; units of mass are grams and kilograms; units of volume are milliliters and liters; units of temperature are degrees Celsius).You should first state either "English" or "Metric" to say which you prefer. And next add 1-2 sentences to explain why.
CHEM1305 Introductory Chemistry
Chapter 3 Discussion
Classification of Matter
Think of a substance that you may see everyday. State whether it is an element, a compound, a homogeneous mixture, or a heterogeneous mixture and use 1-2 sentences to describe why. I recommend a web search to help you (example search: "is salad dressing an element, compound, homogeneous mixture, or heterogeneous mixture").
CHEM1305 Introductory Chemistry
Chapter 4 Discussion
Building Isotopes
This discussion is more of an activity. Please click on the following link (Links to an external site.) to visit the Isotopes and Atomic Mass simulator.
Click on the simulator, and choose the 'Isotopes' option
Once there, choose one of the elements seen in the top right corner (only the first 10 elements are available)
Expand the 'Abundance in Nature' box on the right
Determine which isotopes of the element are stable by adding or taking away neutrons from the nucleus (a bucket of neutrons is to the left)
Report which isotopes are stable (using the correct isotope name) and what percent abundance of each isotope is found in nature
I have used hydrogen as an example to show how you should report your findings:
Hydrogen-1 has 99.9885% natural abundance
Hydrogen-2 has 0.0115% natural abundance
All other isotopes are NOT stable
I have included screenshots of the hydrogen example below. You DO NOT need to upload any screenshots, I have only put them here to help guide you.
H-1
H-2
H-3
If the images do not appear, see them in the .pdf file here
CHEM1305 Introductory Chemistry
Chapter 5 Discussion
What is Your Favorite Element?
In this discussion, you will tell us about the element that you find the most interesting.
You should visit the photographic periodic table (http://periodictable.com/ (Links to an external site.)), which has photographs of all the stable elements as well as facts and stories about each element. Choose the one that looks the most interesting to you and click on it to read about it. To contribute to this discussion, first name the element you chose and next copy one (or more!) of the facts or stories and post it here.
Here is an example:
Element: Radium
Radium was once widely used in self-luminous clock and watch hands, until too many watch factory workers had died. It had not been understood yet that exposure to radium leads to radiation poisoning and eventually death. Those antique watches are still quite radioactive, and will stay that way for thousands of years.
CHEM1305 Introductory Chemistry
Chapter 6 Discussion
Uses of Inorganic Compounds
1616 unread replies.3535 replies.
In this discussion, you will choose one of the inorganic compounds from the table below. First, state whether it is a binary ionic compound, ternary ionic compound, binary molecular compound, binary acid, or ternary oxyacid.
Next, do a web search to see what uses the compound has. Use the term "what are the uses of [compound]" and list at least two of the uses you find.
For example aluminum hydroxide is a ternary ionic compound. And a search of the term "what are the uses of aluminum hydroxide" shows that it is used both as an antacid and to reduce phosphate levels in people with certain kidney conditions.
Al(OH)3, aluminum hydroxide
BaSO4, barium sulfate
CaCO3 calcium carbonate
CCl4, carbon tetrachloride
CF4, carbon tetrafluoride
CO2, carbon dioxide
ClO2, chloride dioxide
HCl(aq), hydrochloric acid
HClO4(aq), perchloric acid
HF(aq), hydrofluoric acid
H2O, dihydrogen oxide
H2SO4(aq), sulfuric acid
KI, potassium iodide
K3PO4, potassium phosphate
Mg(OH)2, magnesium hydroxide
MgSO4, magnesium sulfate
Na2CO3, sodium carbonate
NaCl, sodium chloride
NaF, sodium fluoride
NaHCO3, sodium bicarbonate
Na2HPO4, sodium hydrogen phosphate
NaOCl, sodium hypochlorite
NaOH, sodium hydroxide
Na2SO3, sodium sulfite
NH3, nitrogen trihydride
(NH4)2CO3, ammonium carbonate
NH4NO3, ammonium nitrate
NO, nitrogen monoxide
NO2, nitrogen dioxide
P4S2, tetraphosphorus disulfide
SF6, sulfur hexafluoride
SO2, sulfur dioxide
SiH4, silicon tetrahydride
TiO2, titanium(II) oxide
ZnO, zinc oxide
CHEM1305 Introductory Chemistry
Chapter 7 Discussion
Chemical Reactions in Daily Life
In this discussion, you will do a web search to find an example of a chemical reaction which may be encountered in daily life. Describe a little about the chemical changes that occur. If possible, classify the chemical reaction and write out the chemical equation.
See each of these websites for some ideas:
https://sciencestruck.com/chemical-reactions-in-everyday-life (Links to an external site.)
https://www.thoughtco.com/chemical-change-examples-608334 (Links to an external site.)
For example, baking soda (sodium hydrogen carbonate) is used in baking. When the baking soda heats up, carbon dioxide and water vapor gases are released, leading to the cookie dough or cake batter rising. This is a decomposition reaction, and the chemical equation is: 2 NaHCO3(s) heatrxn Na2CO3(s) + H2O(g) + CO2(g)
CHEM1305 Introductory Chemistry
Chapter 8 Discussion
How Big is Avogadro's Number?
In this discussion, you will do a calculation using Avogadro's number, 6.02 × 1023, or 1 mole. Think of an everyday item and either do a google search to see what it's mass is or else measure it's mass yourself. Next, multiply that mass by Avogadro's number to determine how much 1 mole of that item would weigh. Report your result in both scientific notation and as an ordinary number.
For example, 1 m&m candy weighs about 0.88 g
0.88 g × 6.02 × 1023 = 5.3 × 1023 g = 530,000,000,000,000,000,000,000 g
1 m&m = 0.88 g
1 mole m&m = 5.3 × 1023 g or 530,000,000,000,000,000,000,000 g
CHEM1305 Introductory Chemistry
Chapter 9 Discussion
Limiting Reactants
This discussion is an activity. Please click on the following link (Links to an external site.) to visit the Reactants, Products and Leftovers simulator.
Click on the simulator, and take some time to practice the limiting reactant concept first with the 'Sandwiches' option and next the 'Molecules' option
When you feel you have had enough practice, choose the 'Game' option
Practice with the 'Level 1' game (you will see in each game, you have a few attempts to get the right answer)
Next, choose the 'Level 2' game
Once there, you will choose one of the 5 challenges within the game to report on
For the challenge you pick, you must report:
the balanced chemical equation
number of molecules of the reactants for your example
number of molecules of the products for your example
number of molecules of the leftovers for your example
Here is an example to show how you should report your findings:
1 H2 + 1 F2 → 2 HF
5 H2 and 4 F2
8 HF
1 H2 and 0 F2
I have included screenshots of the example below. You DO NOT need to upload any screenshots, I have only put them here to help guide you.
10_1.png
10_2.png
10_3.png
10_5.png
CHEM1305 Introductory Chemistry
Chapter 10 Discussion
Scuba Diving
A scuba diver is at an underwater depth where the surrounding pressure is 3 atm. The diver must be very careful when coming up to sea level, where surrounding pressure becomes 1 atm. The reason has to do with the volume of gas in the diver's lungs and gas bubbles that exist in the blood vessels and other tissues.
Using Boyle's Law, discuss why this is.
CHEM1305 Introductory Chemistry
Chapter 11 Discussion
Properties of Liquids and Solids
For this discussion, you will choose one liquid AND one solid from the table below. For the liquid, you must state what type(s) of intermolecular forces exist between molecules of that liquid. For the solid, you must state what type of solid it is (either ionic, metallic, covalent network, or molecular).
Liquids Solids
water, H2O sodium chloride, NaCl
ethanol, C2H5OH diamond, C
bromine, Br2 copper, Cu
ether, C2H5OC2H5 sulfur, S8
chloroform, CHCl3 aluminum, Al
acetone, CH3COCH3 calcium carbonate, CaCO3
pentane, C5H12 iron, Fe
butanol, C4H9OH zinc oxide, ZnO
CHEM1305 Introductory Chemistry
Chapter 12 Discussion
Molecule Shapes
Visit the following website: https://phet.colorado.edu/en/simulation/molecule-shapes (Links to an external site.)
Click on the "Molecule Shapes" simulation, and next choose the "Real Molecules" option.
Choose a molecule from the top right corner. Please choose either CO2, SO2, BF3, NH3, or CH4, as the other options involve geometries that will not be discussed in this course. Try clicking on the molecule and dragging it around to get a feeling for the 3-dimensional structure.
Once you have made your final selection, click the boxes at the bottom to name the 'Molecule Geometry' and 'Electron Geometry' and report your findings. The molecule H2O is used below as an example.
Molecule: H2O
Molecule Geometry: Bent
Electron Geometry: Tetrahedral
(a screenshot of the simulation is given below, you do not need to include the screenshot in your answer)
CHEM1305 Introductory Chemistry
Chapter 1 Homework Assignment
Question 1Which of the following items was made using chemistry?
a computer
a firework
a loaf of bread
all of the above
Question 2What is the definition of chemistry?
the study of living organisms
the scientific study of the human mind
the study of the composition, properties, and interactions of matter
the study of earth's physical structure and substance
Question 3Chemistry is sometimes referred to as “the central science”.
True
False
Question 4Which field of science can be connected to chemistry?
biology
physics
medicine
all of the above
Question 5Which branch of chemistry deals with the study of chemicals that contain carbon?
inorganic chemistry
organic chemistry
physical chemistry
analytical chemistry
Question 6Attempts to understand the behavior of matter extend back for more than 2500 years.
True
False
Question 7Which of the following is NOT a step in the scientific method?
make up some fake data
formulate a hypothesis
design and perform experiments
accept or modify the hypothesis
Question 8Is the following statement an example of a scientific theory or law?
If the temperature of a gas in a closed system is increased, the pressure will increase.
theory
law
Question 9Is the following statement an example of a scientific theory or law?
An element is composed of tiny particles called atoms.
theory
law
Question 10One of the best ways to succeed in a chemistry course is to do ALL of the given practice problems.
True
False
CHEM1305 Introductory Chemistry
Chapter 2 Homework Assignment
Question 1Which of the following is a proper measurement?
12
yard stick
50 meters
dozen
Question 2Give the number of significant figures in each:
a) 6000 mL
1
b) 0.02508 cm
4
c) 94.2 g
3
d) 1,001 in
Question 3What is the number 0.000583 in scientific notation format?
5.83 × 10-4
5.83 × 104
5.83 × 10-3
5.83
Question 4What is the number 7.9 × 108 written as an ordinary number?
790,000
0.000000079
790,000,000
7,900,000,000
Question 5Complete the calculation and choose the answer using the correct number of significant figures:
5.007 m × 6 m
30.042 m2
30.04 m2
30 m2
30 m
Question 6Complete the calculation and choose the answer using the correct number of significant figures:
17.75 g + 21 g
39 g
38.8 g
38.75 g
38.75 g2
Question 7Choose the correct abbreviation for the unit "milliliter" and define in terms of the base unit.
mil; 100 mil = 1 l
ML; 1 ML = 1,000,000 L
mL; 1000 mL = 1 L
μL; 1,000,000 μL = 1 L
Question 8Convert 651,000 m to km, given 1000 m = 1 km
65.1 km
6.51 km
651,000,000 km
651 km
Question 9Convert 135 lb to kg, given 1 lb = 454 g; 1000 g = 1 kg
3.36 kg
61.3 kg
0.000297 kg
297 kg
Question 10What is the density of oxygen, given that a 2.00 L sample of oxygen has a mass of 2.86 g?
5.72 g/L
1.43 g/mL
0.699 g/L
1.43 g/L
CHEM1305 Introductory Chemistry
Chapter 3 Homework Assignment
Question 1Which of the following is NOT an example of matter?
a cup of water
a helium balloon
light
a pillow
Question 2How many carbon atoms are there in the chemical formula for iron(III) carbonate, Fe2(CO3)3?
1
2
3
4
Question 3Which phase of matter has a definite volume but an indefinite (variable) shape?
solid
liquid
gas
plasma
Question 4Classify each type of matter as either an element, a compound, a homogeneous mixture, or a heterogeneous mixture.
a) a bowl of cereal with milk heterogeneous mixture
b) sodium element
c) carbon dioxide compound
d) apple juice homogeneous mixture
Question 5Classify each property as physical or chemical.
a) silver is a silver-colored metal physical property
b) propane gas readily burns in air chemical property
c) pure sodium will explode if dropped in water chemical property
d) copper conducts electricity physical property
Question 6Classify each change as physical or chemical.
a) a match is ignited physical change
b) a drop of alcohol evaporates
c) two colorless solutions are combined and form a yellow color
d) a tablet of aspirin is ground to a powder physical change
Question 7In a reaction, 1.000 g copper metal is heated with yellow sulfur to form copper sulfide as a product. 1.252 g of copper sulfide is made. What is the mass of sulfur that had reacted with the copper metal?
0.252 g
1.000 g
1.252 g
2.252 g
Question 8Energy cannot be created or destroyed, it can only be changed from one form to another.
True
False
Question 9Substances at higher temperatures have a higher kinetic energy (atoms are moving faster) than substances at lower temperatures (atoms are moving slower).
True
False
Question 10What is the boiling point of water according to the Kelvin scale?
100 K
212 K
273 K
373 K
CHEM1305 Introductory Chemistry
Chapter 4 Homework Assignment
Question 1Which of the following scientists proposed the first Atomic Theory?
J. J. Thomson
Ernest Rutherford
John Dalton
James Chadwick
Question 2Match the following information about the subatomic particles:
relative mass is 0.00055
electron
relative charge is +1
proton
location is inside nucleus
neutrons and protons
Other Incorrect Match Options:
neutrons and electrons
Question 3Refer to the periodic table (https://ptable.com/ (Links to an external site.)) and type in the number of protons each of the following elements have in their nucleus:
silver, Ag 47
xenon, Xe 54
potassium, K 19
copper, Cu 29
nitrogen, N 7
Question 4Choose the correct atomic notation for an atom of cobalt with 32 neutrons in its nucleus.
co3.png
co2.png
co1.png
co4.png
Question 5What is the term for atoms of the same element that have different numbers of neutrons.
nucleotides
atomic notation
protons
isotopes
Question 6Type in the number of neutrons in each of the following isotopes of tungsten, W:
W-182
108
W-186
112
Question 7Fill in the following table (assume the atoms are neutral):
Isotope Number of Protons Number of Neutrons Number of Electrons
Os-192
76
116
76
Al-27
13 14
13
Question 8Chlorine has two naturally occurring isotopes: Cl-35 with mass 34.969 amu and a natural abundance of 75.78%, and Cl-37 with mass 36.966 amu and a natural abundance of 24.22%. What is the calculated atomic mass of chlorine?
36 amu
3545 amu
35.45
35.45 amu
Question 9Type in how many electrons can each of the following sublevels hold:
s
2
p
6
d
10
f
14
Question 10Electrons will occupy sublevels in order of increasing…
energy
mass
time
sound
CHEM1305 Introductory Chemistry
Chapter 5 Homework Assignment
Question 1Using the periodic table, classify each of the following elements as a metal or a nonmetal, and then further classify each as a representative element, transition metal, or inner transition metal:
a. Se nonmetal ["", "", ""]
b. Yb ["", ""] ["", "", ""]
c. Mo ["", ""] ["", "", ""]
d. K ["", ""] representative element
metal
Question 2Give the group name for the following elements:
a. F halogen
b. Xe noble gas
c. Mg alkaline earth metal
d. Rb alkali metal
Question 3Identify each of the following elements (type in the chemical symbol for the element, not the name):
a. the halogen in the same period as potassium
b. the Group 10 element in the same period as Ba
c. the alkali metal in the same period as the element with 14 protons
d. the noble gas in the same period as an isotope with 80 protons and 120 neutrons
e. the alkaline earth metal in the fifth period
Question 4Find the element that corresponds to the following electron configurations (type in the chemical symbol for the element, not the name):
a. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d3
b. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3
c. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2
d. (Kr) 5s2 4d1
e. (Ar) 4s2 3d10 4p1
Question 5State how many valence electrons each of the following elements has:
a. Cl
b. Al
c. P
d. K
e. O
f. Si
g. Mg
h. Ar
Question 6Predict the ionic charge for each of the following ions based on the group number of the element in the periodic table:
a. P ion 3-
b. Rb ion 1+
c. F ion 1-
d. Ba ion 2+
e. Al ion 3+
Question 7Give the noble gas that each of the following ions are isoelectronic with (type in the chemical symbol for the element, not the name):
a. Br -
b. N3-
c. Ca2+
d. Li+
e. Ba2+
Question 8a. From the following list of elements, which one has the smallest atomic radius?
Fe, K, Br, Ca, Ge Br
b.From the following list of elements, which one has the largest atomic radius?
Ca, Be, Sr, Ba, Mg Ba
Question 9a. From the following list of elements, which one has the most metallic character?
Ag, Sn, Zr, I, Rb Rb
b.From the following list of elements, which one has the least metallic character?
As, Bi, P, N, Sb N
Question 10
a. From the following list of elements, which one has the highest ionization energy?
O, Ne, C, Li, F Ne
b.From the following list of elements, which one has the lowest ionization energy?
K, Rb, Li, Cs, Na Cs
CHEM1305 Introductory Chemistry
Chapter 6 Homework Assignment
Question 1Classify each of the following as a binary ionic compound, ternary ionic compound, binary molecular compound, binary acid, or ternary oxyacid:
a. bleach, NaClO ternary ionic compound
b. carbon monoxide, CO binary molecular compound
c. phosphoric acid, H3PO4(aq) ternary oxyacid
d. iodized salt, KI binary ionic compound
e. hydrofluoric acid, HF(aq) binary acid
Question 2Give the name for each of the following ions:
a. NO2- nitrite ion
b. NH4+ ammonium ion
c. S2- sulfide ion
d. Ag+ silver ion
e. Sn2+ tin ion
Question 3Give the formula for each of the following ions: (the superscript and subscript functions will not appear in the dropdown choices, but the correct answer should still be clear to you)
a. zinc ion Zn2+
b. hydronium ion H3O+
c. nitride ion N3-
d. lead(II) ion Pb2+
e. cyanide ion CN-
Question 4Give the formula for the each of the following ionic compounds given their constituent ions: (the subscript function will not appear in the dropdown choices, all numbers seen should be thought of as subscripts)
a. sodium sulfide, Na+ and S2- Na2S
b. lead(IV) sulfate, Pb4+ and SO42- Pb(SO4)2
Question 5Give the name for each of the following ionic compounds:
a. SrI2 strontium iodide
b. Fe2(CrO4)3 iron(III) chromate
c. Na2O sodium oxide
d. CrP chromium(III) phosphide
e. BaCO3 barium carbonate
Question 6Give the formula for each of the following ionic compounds: (the subscript function will not appear in the dropdown choices, all numbers seen should be thought of as subscripts)
a. lead(II) sulfite PbSO3
b. zinc bromide ZnBr2
c. copper(II) phosphide Cu3P2
d. magnesium nitrate Mg(NO3)2
e. aluminum oxide Al2O3
Question 7Give the name for each of the following binary molecular compounds:
a. Cl2O5 dichlorine pentaoxide
b. BrF bromine monofluoride
c. I2O4 diiodine tetraoxide
d. SF4 sulfur tetrafluoride
e. CO carbon monoxide
Question 8Give the formula for each of the following binary molecular compounds: (the subscript function will not appear in the dropdown choices, all numbers seen should be thought of as subscripts)
a. nitrogen monoxide NO
b. carbon tetrachloride CCl4
c. dihydrogen monoxide H2O
d. dichlorine heptaoxide Cl2O7
e. dinitrogen trioxide N2O3
Question 9Give the name for each of the following acids:
a. HCl(aq) hydrochloric acid
b. H2SO3(aq) sulfurous acid
c. HClO3(aq) chloric acid
d. HI(aq) hydroiodic acid
e. H2CO3(aq) carbonic acid
Question 10Give the formula for each of the following acids: (the subscript function will not appear in the dropdown choices, all numbers seen should be thought of as subscripts)
a. hypochlorous acid HClO(aq)
b. hydrofluoric acid HF
c. nitrous acid HNO2(aq)
d. phosphoric acid H3PO4(aq)
e. hydrobromic acid HBr(aq)
CHEM1305 Introductory Chemistry
Chapter 7 Homework Assignment
Question 1Choose the correct evidence of a chemical reaction for each of the following observations:
a) adding a piece of zinc metal to acid causes bubbles to form
a gas is produced
b) mixing two colorless solutions gives a pink solution
a gas is produced
c) adding potassium metal to water causes flames
an energy change is observed
d) adding sodium chloride to a silver nitrate solution causes a white powder to form in the solution
an insoluble solid is produced in a solution
Question 2Choose the most correct chemical equation (with all the appropriate symbols) for the following reaction:
nitric acid reacts with aqueous ammonium hydroxide to give aqueous ammonium nitrate plus water
HNO3 + NH4OH → NH4NO3 + H2O
HNO3 + NH4OH + NH4NO3 + H2O
HNO3(aq) + NH4OH(aq) → NH4NO3(aq) + H2O(l)
HNO3(s) + NH4OH(l) → NH4NO3(aq) + H2O(g)
Question 3Balance the following chemical reactions (choose "1" if no coefficient is needed):
a) 1 Al2(CO3)3(s) → 1 Al2O3(s) + 3 CO2(g)
b) 1 Hg2(NO3)2(aq) + 2 NaBr(aq) → 1 Hg2Br2(s) + 2 NaNO3(aq)
c) 2 (NH4)3PO4(aq) + 3 Pb(NO3)2(aq) → 1 Pb3(PO4)2(s) + 6 NH4NO3(aq)
Question 4Classify each of the following chemical reactions:
a) 3 Sn(s) + 2 P(s) → Sn3P2(s)
combination
b) 2 HClO4(aq) + Ba(OH)2(s) → Ba(ClO4)2(s) + 2 H2O(l)
neutralization
c) Cu(s) + 2 AgC2H3O2(aq) → Cu(C2H3O2)2(aq) + 2 Ag(s)
single-replacement
d) 2 LiClO3(s) → 2 LiCl(s) + 3 O2(g)
decomposition
e) Pb(NO3)2(aq) + 2 LiCl(aq) → PbCl2(s) + 2 LiNO3(aq)
double-replacement
Question 5Choose the correct, balanced chemical equation for the following combination reaction:
aluminum metal is heated with sulfur powder to form solid aluminum sulfide
Al(s) + S(s) heatrxn AlS(s)
Al(s) + S(s) heatrxn Al2S3(s)
2 Al(s) + 3 S(s) heatrxn Al2S3(s)
Question 6Choose the correct, balanced chemical equation for the following decomposition reaction:
solid lithium carbonate decomposes with heat to form solid lithium oxide and carbon dioxide gas
Li2CO3(s) heatrxn Li2O(s) + CO2(g)
LiCO3(s) heatrxn 2 LiO(s) + CO2(g)
LiCO2(s) heatrxn Li(s) + CO2(g)
Question 7Using the activity series, predict whether a reaction occurs or no reaction occurs for each of the following single-replacement reactions:
a) Cu(NO3)2(aq) + Ni(s) →Reaction Occurs
b) Au(s) + H2SO4(aq) →No Reaction
c) FeSO4(aq) + Ag(s) →Reaction Occurs
Question 8Using the solubility table, determine whether each of the following compounds are soluble or insoluble in water:
a) calcium sulfide, CaSsoluble
b) lead(II) sulfate, PbSO4insoluble
c) barium chromate, BaCrO4insoluble
Question 9Using the solubility table, predict whether a reaction occurs or no reaction occurs for each of the following double-replacement reactions:
a) AgC2H3O2(aq) + SrI2(aq) →No Reaction
b) FeSO4(aq) + CuCl2(aq) →No Reaction
c) NaOH(aq) + Co(NO3)2(aq) →No Reaction
Question 10Choose the correct, balanced chemical equation for the following neutralization reaction:
nitric acid reacts with aqueous barium hydroxide to form aqueous barium nitrate and water
HNO3 + BaOH → BaNO3 + H2O
2 HNO3(aq) + Ba(OH)2(aq) → Ba(NO3)2(aq) + 2 H2O(l)
HNO3(aq) + Ba(OH)2(aq) → Ba(NO3)2(aq) + H2O(l)
CHEM1305 Introductory Chemistry
Chapter 8 Homework Assignment
Question 1One half of a mole of atoms would contain how many atoms?
6.02 × 1023 atoms
6 atoms
3.01 × 1023 atoms
144 atoms
Question 2Calculate the number of particles in 0.200 mol of chlorine molecules, Cl2.
6.02 × 1023 molecules
7.09 molecules
35.45 molecules
1.2 × 1023 molecules
Question 3Calculate the number of moles in 3.00 × 1024 formula units of manganese(II) sulfate, MnSO4.
151.00 moles
4.98 moles
6.02 × 1023 moles
2.00 × 1023 moles
Question 4Determine the molar mass for each of the following:
a) silicon, Si28.09 g/mol
b) ozone, O348.0 g/mol
c) iron(II) acetate, Fe(C2H3O2)2173.93 g/mol
d) nitroglycerin, C3H5O3(NO2)3227.09 g/mol
Question 5How many moles of dinitrogen oxide, N2O are in a 19.3 g sample of N2O?
6.43 moles
2.28 moles
0.439 moles
19.3 moles
Question 6What is the mass of 61.5 moles of zinc, Zn?
0.941 g
1.06 g
4021 g
61.5 g
Question 7Calculate the number of molecules in 5.68 g propane, C3H8.
7.75 × 1022 molecules
0.129 molecules
2.33 × 1024 molecules
5.68 molecules
Question 8What is the mass percent of C in oxalic acid, H2C2O4?
12.01 %
26.7 %
13.3 %
33.3 %
Question 9An iron phosphide compound contains 335 grams of iron and 124 grams of phosphorus. What is the empirical formula of this compound?
Fe6P4
FeP
Fe3P2
Question 10Hexamethylene diamine has a molar mass of 115 g/mol and an empirical formula of C3H8N. What is the molecular formula of the compound?
Correct!
C6H16N2
C9H24N3
C3H8N
C1.5H4N0.5
CHEM1305 Introductory Chemistry
Chapter 9 Homework Assignment
Question 1Consider the general chemical equation: A + 2 B → 3 C
How many moles of C are produced from 1 mol of A?
1
2
3
4
Question 2Given the decomposition of hydrogen peroxide, calculate the moles of oxygen gas produced from 5.00 mol of H2O2
2 H2O2(l) → 2 H2O(l) + O2(g)
1 mol
2.5 mol
5 mol
10 mol
Question 3How many moles of propane gas, C3H8, react with 1.29 mol of oxygen gas?
C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g)
6.45 mol
0.258 mol
1 mol
5 mol
Question 4Given the balanced equation, calculate the mass of H2 that can be prepared from 141 g Al.
2 Al(s) + 6 HNO3(aq) → 2 Al(NO3)3(aq) + 3 H2(g)
212 g
1.50 g
5.22 g
15.8 g
Question 5Given the balanced equation, calculate the mass of Cl2 required to produce 6.78 g of PCl3.
2 P(s) + 3 Cl2(g) → 2 PCl3(l)
5.25 g
137 g
10.2 g
70.9 g
Question 6What mass of CO2 will react with 1.00 g LiOH?
2 LiOH(s) + CO2(g) → Li2CO3(s) + H2O(l)
1.84 g
0.500 g
2.00 g
0.920 g
Question 7If 9.00 moles of hydrogen gas and 9.00 moles of oxygen gas are combined, what is the limiting reactant?
2 H2(g) + O2(g) → 2 H2O(l)
H2
O2
H2O
Question 8If 50.0 g of Co react with 30.0 g of S, which compound is the limiting reactant?
Co(s) + S(s) → CoS(s)
Co
S
CoS
Question 9A manufacturer performs a chemical reaction to produce sulfur hexafluoride, SF6. After the reaction is complete, 480.2 kg is isolated. If the theoretical yield of SF6 was 546.7 kg, what was the percent yield of the reaction?
113.8%
87.84%
26.25%
48.02%
Question 10A student dissolves 1.50 g of copper(II) nitrate in water. After adding aqueous sodium carbonate solution, the student obtains 0.875 g of CuCO3 First, calculate the theoretical yield of the CuCO3 and next use that to calculate the percent yield for this student’s experiment. What is the percent yield?
Cu(NO3)2(aq) + Na2CO3(aq) → CuCO3(s) + 2 NaNO3(aq)
58.3%
88.6%
113%
100%
CHEM1305 Introductory Chemistry
Chapter 10 Homework Assignment
Question 1Gases do not expand or compress.
True
False
Question 2A barometer reads 30.8 in. Hg. Express the pressure in each of the following units:
a) kPa104 kPa
b) torr782 torr
c) psi15.1 psi
d) atm1.03 atm
Question 3A container of gas at 7.00 atm and 212 K is cooled to 140 K. If volume is constant, what will the final pressure be?
70.0 atm
10.5 atm
4.69 atm
1.49 atm
Question 4A 3.2 L balloon of helium gas at 260 K increases in volume to 8.5 L. To keep the pressure constant, what should the final temperature of the balloon be?
690 K
0.10 K
130 K
27.2 K
Question 5A sample of air at 5.00 atm expands from 1.75 L to 2.50 L. If the temperature remains constant, what is the final pressure in atm?
0.286 atm
2.50 atm
1.25 atm
3.50 atm
Question 6A balloon with a volume of 1.0 L is filled with 0.10 moles of argon. If another 0.10 moles of argon is added (for a total of 0.20 moles) (and pressure and temperature remain constant), what will the final volume of the balloon be?
1.2 L
2.0 L
22 L
0.8 L
Question 7If 10.0 L of neon gas exerts a pressure of 8.5 atm at 373 K, what is the number of moles of gas?
2.78 moles
6.48 moles
0.781 mole
1.50 mole
Question 8At STP conditions, what is the volume of 2.30 moles of oxygen gas?
230 L
22.4 L
11.2 L
51.5 L
Question 9What is the density of neon gas at STP conditions?
20.18 g/L
0.90 g/L
1.00 g/L
22.4 g/L
Question 10A sample of O2 gas is collected over water at 21 °C. If the total pressure of the gas was 758 mm Hg, what is the partial pressure of the O2 gas? (the partial pressure of the water vapor at 21 °C is 18.7 mm Hg)
40.5 mm Hg
777 mm Hg
739 mm Hg
760 mm Hg
CHEM1305 Introductory Chemistry
Chapter 11 Homework Assignment
Question 1Liquids have a variable shape, but a fixed volume.
True
False
Question 2What type of intermolecular forces exist between molecules of Cl2?
dipole-dipole attractions
dispersion forces
intramolecular bonding
hydrogen bonding
Question 3Which of the following liquids has the highest surface tension?
CHCl3
H2O
C5H12
CS2
Question 4Which of the following liquids has the highest viscosity?
C5H12
C6H14
C7H16
C8H18
Question 5What is the term for the change of physical state from liquid to solid?
melting
sublimation
freezing
condensation
Question 6Heat energy is NOT required to turn liquid water into gaseous water vapor.
True
False
Question 7Use the phase diagram below to answer what physical state H2O is at 99 °C and 500 kPa.
A graph is shown where the x-axis is labeled “Temperature in degrees Celsius” and the y-axis is labeled “Pressure ( k P a ).” A line extends from the origin of the graph which is labeled “A” sharply upward to a point in the bottom third of the diagram labeled “B” where it branches into a line that slants slightly backward until it hits the highest point on the y-axis labeled “D” and a second line that extends to the upper right corner of the graph labeled “C”. C is labeled “Critical point, with a dotted line extending downward to the x-axis labeled 374 degrees Celsius, and another dotted line extending to the y-axis labeled 22,089 k P a. The two lines bisect the graph area to create three sections, labeled “Ice (solid)” near the middle left, “Water (liquid)” in the top middle and “Water vapor (gas)” near the bottom middle. Point B is labeled “Triple point” and has a dotted line extending downward to the x-axis labeled 0.01, and another dotted line extending to the y-axis labeled 0.6. Halfway between points B and C a dotted line extends from the originally discussed line downward to the point 100 degrees Celsius on the x-axis, and another dotted line extends to the y-axis at 101 k P a. Another dotted line extends from this dotted line downward at 0 degrees Celsius.
solid
liquid
gas
Question 8Solids can readily compress and expand.
True
False
Question 9Identify the type of crystalline solid (metallic, network covalent, ionic, or molecular) formed by each of the following substances:
a. Timetallic
b. S8molecular
c. KBrionic
d. SiO2network covalent
Question 10Classify each substance as either a metallic, ionic, or molecular solid:
a) a hard, brittle substance that has a very high melting point metallic
b) a dull substance that is not soluble in water and has a low melting point molecular
c) a shiny substance that is a very good conductor of electricity ionic
CHEM1305 Introductory Chemistry
Chapter 12 Homework Assignment
Question 1Predict whether each of the following is held together by ionic or covalent bonds:
a. water, H2O covalent
b. calcium chloride, CaCl2 ionic
c. potassium oxide, K2O ionic
d. carbon disulfide, CS2 covalent
Question 2State whether the following is true or false about the following ionic compounds:
a. in a sodium bromide formula unit, NaBr, the sodium atom has lost electrons and the bromine atom has gained electrons
c. in a calcium oxide formula unit, CaO, the calcium and oxygen from a bond by sharing electrons
d. calcium and oxide ions form a bond by an attraction between the ions
Question 3State whether the following is true or false about the following molecular compounds:
a. in a molecule of sulfur dioixide, SO2, the valence electrons are transferred from oxygen to sulfur
b. the S-O bond length equals the sum of the two atomic radii
c. in a molecule of hydrogen bromide, HBr, the valence electrons are shared by the hydrogen and bromine atoms
d. the H-Br bond length is less than the sum of the two atomic radii
Question 4Predict which element in each of the following pairs is more electronegative according to the general electronegativity trends in the periodic table:
a. C or O O
b. Cl or Br Cl
c. F or N F
d. Si or P P
Question 5Calculate the electronegativity difference between each of the following:
a. the bond between P and S 0.4
b. the bond between H and Br 0.7
Question 6Classify each of the following as either a polar covalent bond or nonpolar covalent bond:
a. F-F nonpolar covalent bond
b. H-O polar covalent bond
c. H-P polar covalent bond
d. C-F polar covalent bond
Question 7Which of the following is the correct electron dot formula for a molecule of HOCl?
a. HOCl_1.png
b. HOCl_2.png
c. HOCl_3.png
d. HOCl_4.png
Question 8Which of the following is the correct structural formula for a molecule of CH2S?
a. CH2S_1.png
b. CH2S_2.png
c. CH2S_3.png
d. CH2S_4.png
Question 9Predict the electron geometry and molecular geometry for each of the following molecules:
a. NF3 electron geometry: tetrahedral
molecular geometry:
b. H2S electron geometry:
molecular geometry:
c. SiH4electron geometry:
molecular geometry:
d. HCN electron geometry:
molecular geometry: linear
Question 10CH3F has a polar bond (between the C-F), is it also a polar molecule?
yes
no
