CHM1100C All Quizzes Latest 2023

CHM1100C Section 06 General Chemistry Module 02 Quiz

Question 1

Why is it necessary for the spins of two electrons that occupy one orbital, to be in the opposite directions? What is that law called?

Question 2

You have been tasked to give a report about the differences in the Bohr Model v. Quantum Mechanical Model of the atom. Describe the 5 main differences between the Bohr Atom Model and the Quantum Mechanical model.

Question 3

Describe the difference between the principal quantum number and the angular momentum quantum number.

Question 4

How does an orbit differ from an orbital?

Question 5

An element has 2 neutrons, 2 electrons and 2 protons. Which element does this describe? Is it a neutral atom, isotope, or an ion? What is the mass number? What is the net charge?

Question 6

An element has 4 neutrons, 3 electrons and 4 protons. Which element does this describe? Is it a neutral atom, isotope, or an ion? What is the mass number? What is the net charge?

Question 7

How many protons do you need to add to the orbit to make a stable fluorine atom?

Question 8

How many electrons do you need to add to the orbit to make a stable Beryllium atom?

Question 9

Which ion has +3 charge, 28 electrons, and an atomic mass of 70 amu?

Question 10

Identify the element that fits into each of these categories on the periodic table: Halogens

Question 11

Identify the element that fits into each of these categories on the periodic table: Nonmetal

Question 12

Identify the element that fits into each of these categories on the periodic table: Noble gases

Question 13

Calculate the average atomic mass for the following isotopes: Hydrogen: hydrogen-1 (1.0078 amu) at 99.989%, hydrogen-2 (2.0141 amu) at 0.0115%

Question 14

Calculate the average atomic mass for the following isotopes: Lithium: lithium-6 (6.0151 amu) at 7.59%, lithium-7 (7.0160 amu) at 92.41%

Question 15

Liv is trying to decide which molecules to use for her chemistry reaction. The first thing she has to do is find the molar mass of each of the molecules she can potentially use. Calculate the molar mass of the molecules: NaHCO3

Question 16

Question 17

The National Institute of Health (NIH) provides dietary recommendations for adults over various supplements. Convert the following recommendations for supplements over to mass or moles. You have 1.45 moles of Vitamin C (C6H8O6). Convert moles to mg to determine if it matches the NIH's daily recommendation of 75mg.

Question 18

The National Institute of Health (NIH) provides dietary recommendations for adults over various supplements. Convert the following recommendations for supplements over to mass or moles. You have 0.834 moles of Potassium. The NIH recommends 2,600mg of potassium as a daily intake recommendation. Convert the moles to mg.

Question 19

As a medical professional, it is very important to understand the types of radiation and wavelengths in the electromagnetic spectrum. What types of radiation are safe for the human body, and what types of radiation are unsafe for the human body?

Question 20

As a medical professional, it is very important to understand the types of radiation and wavelengths in the electromagnetic spectrum. At 400nm, would the wavelength be short or long? Would the frequency be high or low?

Question 21

Identify the shape of the sub shell and how many electrons it holds: "D" sub shell

Question 22

Identify which of these orbitals has the lowest energy.

Question 23

Which of the following orbitals do not exist?

Question 24

Identify which of these orbitals has the lowest energy.

Question 25

State the number of TOTAL electrons and VALENCE electrons in each of the following atoms: Fr

Question 26

State the number of TOTAL electrons and VALENCE electrons in each of the following atoms: Ar

Question 27

Identify the element associated with the following electron configurations. 1s2 2s2 2p6 3s2 3p2

Question 28

Identify the element associated with the following electron configurations. 1s2 2s2 2p6 3s2 3p6 4s2 3d5

Question 29

Write the electron configurations for the following ions Mg2+

Question 30

Write the electron configurations for the following ions Li+ CHM1100C Section 06 General Chemistry Module 03 Quiz

Assignment Content

Question 1

Choose one molecule that is vital to the human body. Provide the following information: Name of molecule

Question 2

Now, provide the following information: Molecular formula

Question 3

Now, provide the following information about your chosen molecule: Molecular mass

Question 4

Now, provide the following information about your chosen molecule: The type of molecule (covalent or ionic)

Question 5

Now, provide the following information about your chosen molecule: Percent composition of each element

Question 6

Now, provide the following information about your chosen molecule: Intermolecular forces within the molecular

Question 7

Now, provide the following information about your chosen molecule: Describe why the molecule is important and its function within the human body.

Question 8

Dr. Laila Malik has been tasked to help her graduate student with making a ground-breaking molecule, but she has to start with helping the student understand how different elements bond to each other and the characteristics they have. Help Dr. Malik identify whether the following compounds are ionic or covalent: COF2

Question 9

Question 10

Question 11

Question 12

Question 13

Question 14

Understanding resonance is a key concept to understanding the different ways a molecule can exist, simultaneously. How many resonance structures does the following molecule have: O3

Question 15

Understanding resonance is a key concept to understanding the different ways a molecule can exist, simultaneously. How many resonance structures does the following molecule have: HPO42-

Question 16

Zahara Noor wants to create a presentation of different molecules that helped change the world, but she needs help in naming them, so that anyone is able to understand the molecules that she is talking about. Provide the name of the molecule described here:H2O2: an important compound that comes in a liquid form at room temperature, and used in wound cleaning, and disinfecting.

Question 17

Zahara Noor wants to create a presentation of different molecules that helped change the world, but she needs help in naming them, so that anyone is able to understand the molecules that she is talking about. Provide the name of the molecule described here:SiO2: Used to make glass and anything related to glass such as quartz, lab glassware, mirrors, camera lenses, etc. There are both crystalline and amorphous version.

Question 18

During her presentation, Zahara was asked several questions from the audience and to provide the molecular formula for molecules that the audience had questions about. Help Zahara show the molecular formula for the following compounds: Sodium carbonate

Question 19

Question 20

During her presentation, Zahara was asked several questions from the audience and to provide the molecular formula for molecules that the audience had questions about. Help Zahara classify whether the following items are an element, a compound, a homogenous mixture, or a heterogenous mixture: Iron

Question 21

During her presentation, Zahara was asked several questions from the audience and to provide the molecular formula for molecules that the audience had questions about. Help Zahara classify whether the following items are an element, a compound, a homogenous mixture, or a heterogenous mixture: Neon

Question 22

During her presentation, Zahara was asked several questions from the audience and to provide the molecular formula for molecules that the audience had questions about. Show Zahara how to name Type 2 ionic compounds. AuCl3

Question 23

Question 24

For the following compound, calculate the molar mass: OF2Example: CHCl3 = 119.38 amu

Question 25

For the following compound, calculate the molar mass: CO2Example: CHCl3 = 119.38 amu

Question 26

For the following compound, determine the number of electron domains: HNO3

Question 27

For the following compound, determine the number of electron domains: OF2

Question 28

Identify the molecular geometry for the compound: CH3OH

Question 29

Identify the molecular geometry for the compound: SO3

Question 30

Identify the bond angles for the compound: CH4

Question 31

Identify the bond angles for the compound: CH3OH

Question 32

Identify all of the intermolecular forces within the molecule: HNO3

1.Van der Waals

2.Dipole-dipole

3.Hydrogen bonding

Question 33

Identify all of the intermolecular forces within the molecule: CHCl3

1.Dipole-dipole

2.Hydrogen bonding

3.Van der Waals

Question 34

There is 45% oxygen, 33% sodium and 22% sulfur. What is the empirical formula?

Question 35

What is the percent composition of each element in K2Cr2O7? CHM1100C Section 06 General Chemistry Module 04 Quiz

Question 1

You have plenty of salts that are in front of you and you are trying to figure out which salts are soluble in water, and which ones of their products are soluble in water. For the following equation, provide the net ionic equation. KI+ Pb(NO3)2 equation

Question 2

If you wanted to dilute the 3M NaOH solution to 500mL of 1M NaOH solution, how much L of the 3M NaOH solution would you need?

Question 3

Consider this reaction: 6 CO2 + 6 H2O + light equation C6H12O6 + 6 O2 If there were 2.38 x 102 g of H2O, 18.6 moles of CO2, and plenty of light, what would be the theoretical yield of the reaction?

Question 4

Consider this reaction: 6 CO2 + 6 H2O + light equation C6H12O6 + 6 O2 If there were 2.38 x 102 g of H2O, 18.6 moles of CO2, and plenty of light, which reactant would be the limiting reactant?

Question 5

How many mols of a 3M NaOH solution are in 1L of the solution?

Question 6

If a solution contained a substance of 4.67kg (molar mass of 34.6 g/mol) in 350mL, what is the molarity of the solution?

Question 7

Describe the differences between Bronsted acids and bases v. Lewis acids and bases.

Question 8

For the following reactions, calculate the ionization constant of each reaction. CH3COOH (aq) + H2O (l) equation H3O+ (aq) + CH3COO-(aq); [CH3COOH] = 0.8M, [H3O+] = 7.6M, [CH3COO-] = 16.4MKa =

Question 9

You have 13.2 mols of CO2 . Calculate the mass of CO2.

Question 10

Plants undergo photosynthesis in order to provide oxygen into the air, which is vital for the human body to stay alive: 6 CO2 + 6 H2O + light equation C6H12O6 + 6 O2 If there were 2.38 x 102 g of H2O and 18.6 moles of CO2, how much C6H12O6 can be produced?

Question 11

Consider this reaction: 6 CO2 + 6 H2O + light

C6H12O6 + 6 O2

If you actually produced 30g of C6H12O6 what would be the percent yield? Calculate the theoretical yield from having 2.38 x 102 g of H2O, 18.6 moles of CO2. equation

Question 12

For the following reactions, calculate the ionization constant of each reaction. HCl (aq) + H2O (l) equation H3O+ (aq) + Cl- (aq); [HCl] = 16.9M, [H3O+] = 13.3M, [Cl-] = 7.4MKa =

Question 13

Help Asha identify whether the reaction is a synthesis or decomposition reaction: 2 C + O2equationCO

Question 14

Help Asha identify whether the reaction is a synthesis or decomposition reaction: H2 + F2equation2 HF

Question 15

Identify if the following reaction is balanced or not balanced: NaCl + F2equationNaF + Cl2

Question 16

Identify if the following reaction is balanced or not balanced: BF3 + Li2SO3equationB2(SO3)3 + LiF

Question 17

You have plenty of salts that are in front of you and you are trying to figure out which salts are soluble in water, and which ones of their products are soluble in water. For the following equation, identify the potential products. PbSO4 + KF equation

Question 18

You have plenty of salts that are in front of you and you are trying to figure out which salts are soluble in water, and which ones of their products are soluble in water. For the following equation, identify the potential products. CsClO3+ RbNO3 equation

Question 19

Question 20

Question 21

You have plenty of salts that are in front of you and you are trying to figure out which salts are soluble in water, and which ones of their products are soluble in water. For the following equation, identify which reactants and products are soluble/insoluble in water. NH4Cl + NaClO3equation

Question 22

You have plenty of salts that are in front of you and you are trying to figure out which salts are soluble in water, and which ones of their products are soluble in water. For the following equation, identify which reactants and products are soluble/insoluble in water. H2SO4+ Ba(OH)2equation

Question 23

Identify if the following molecule is a strong acid, strong base, weak acid or a weak base. Sulfuric acid

Question 24

Identify if the following molecule is a strong acid, strong base, weak acid or a weak base. Hydrofluoric acid

Question 25

Identify if the following molecule is a strong acid, strong base, weak acid or a weak base. Hydrogen sulfide

Question 26

Identify if the following substance has high, low, or neutral pH: Coffee

Question 27

Identify if the following substance has high, low, or neutral pH: Drain cleaner

Question 28

Calculate the pH for the following concentration: [H3O+] = 2.19 x 10-5 M

Question 29

Calculate the pH for the following concentration: [H3O+] = 10.33 x 10-9 M

Question 30

Calculate the concentration for the following pH: pH = 9.45

Question 31

Calculate the concentration for the following pH: pH = 7.00

Question 32

Unbuffered yellow solution, PH=8.0 Buffer and Unbuffered red solution, PH= 8.0 Buffer A strong acid has been poured into both beakers in the image on the left. Why did the color of the unbuffered solution change, but the buffered solution remained the same?

Question 33

What happens when a strong base is added to a weak acid solution?

Question 34

Help Asha balance the following equation by completing the equation with the correct numbers:__H2 + __F2equation __HF

Question 35

Help Asha balance the following equation by completing the equation with the correct numbers:__P4 + __F2 equation __PF3 CHM1100C Section 06 General Chemistry Module 05 Quiz

Question 1

Describe the 4 standards that gases need to have in order to fit the kinetic molecular theory of gases.

Question 2

Describe how surface area, temperature, and intermolecular forces are related to the rate of evaporation of a liquid and vapor pressure.

Question 3

What are the 3 interactions that happens in a solution between the solute and the solvents? Describe the interactions in terms of salt dissolved in water.

Question 4

Why can’t the kinetic molecular theory be applied to liquids and solids?

Question 5

Identify which of these gases exhibit non-ideal gas behavior:

Gas A, Gas B, Gas C, Gas D, Gas E, Gas F

Question 6

A box contains 100 particles of gas at room temperature. What is the correlation between the volume and pressure in a box containing a certain amount of gas particles and why?

Question 7

You are a nurse and you have several patients that need treatment. Thank goodness you were taught how to manipulate gas laws in order to help the patients. Help each patient solve the issue they are encountering. Patient A has a collapsed lung and needs to be airlifted to a different hospital for treatment. You know from your schoolwork that pressure has an effect on volume, and the pressure changes as altitude changes. If the volume of the collapsed lung is at 1435mL on the ground (1 atm), what would the volume of the lung be at 632mmHg?

Question 8

You are a nurse and you have several patients that need treatment. Thank goodness you were taught how to manipulate gas laws in order to help the patients. Help each patient solve the issue they are encountering. You are checking the purity of the air in a unit of the hospital and find the following readings: CO2 (17.8 Pa), O2 (20.2 bar), CO (56.6 psi), N2 (71.7 mmHg), SO2 (22.4 torr), and Ar (42.3 atm). What is the total pressure of the unit?

Question 9

You are a nurse and you have several patients that need treatment. Thank goodness you were taught how to manipulate gas laws in order to help the patients. Help each patient solve the issue they are encountering. It is the middle of the summer and a room in the ICU is a lot warmer than it should be. A patient has been wheeled into the room and needs to be put on oxygen. When the room was at room temperature, the pressure in the gas was at 250 psi for 13L of gas. What is the pressure in the gas cylinder since the room warmed up and if the volume of the gas increased to 20L?

Question 10

You are a nurse and you have several patients that need treatment. Thank goodness you were taught how to manipulate gas laws in order to help the patients. Help each patient solve the issue they are encountering. Patient B needs nitrous oxide (N2O) before surgery, and you have to figure out if there is enough nitrous oxide in the cylinder. How many moles of nitrous oxide is in a cylinder of 9.0kg (6kg when empty) at standard temperature and pressure?

Question 11

Liquids have more tightly packed molecules than solids. True False

Question 12

In a solid state, molecules can move past each other. True False

Question 13

Which of these examples are liquids of high viscosity?

Question 14

Which of these examples are liquids of low viscosity?

Question 15

Using the phase diagram, identify the phase that water is in for the following conditions: 300kPa and -20?C DiagramDescription automatically generated

Question 16

Using the phase diagram, identify the phase that water is in for the following conditions: 10000kPa and 50?C DiagramDescription automatically generated

Question 17

Identify which of these molecules has the highest boiling point and give the reasoning why in terms of intermolecular force. CHCl3, CH3COOH, CO2

Question 18

Identify which of these molecules has the highest boiling point and give the reasoning why in terms of intermolecular force. H2O, KCl, CO2

Question 19

Identify the following phase change as endothermic or exothermic processes: Liquid to gas

Question 20

Identify the following phase change as endothermic or exothermic processes: Gas to liquid

Question 21

Reference this image and identify whether the following solution is saturated, supersaturated or undersaturated: KCl at a solubility of 140 at 0?C

Question 22

Reference this image and identify whether the following solution is saturated, supersaturated or undersaturated: NaNO3 at a solubility of 140 at 40?C Supersaturated Saturated Undersaturated

Question 23

Calculate the molality of the following solution: 30g of NaCl in 350g of water

Question 24

Calculate the molality of the following solution: 4.2g of LiBr in 52.6g of water

Question 25

Calculate the molality of the following solution: 37g of glucose (C6H12O6 ) in 64g of water

Question 26

Calculate the mass percent of the following solution: 13g of KBr in 93g of water

Question 27

Calculate the mass percent of the following solution: 30g of NaCl in 350g of water

Question 28

Calculate the mass percent of the following solution: 4.2g of LiBr in 52.6g of water

Question 29

Osmotic drug delivery is a technique used in the pharmaceutical industry to help an active drug dissolve when swallowed. There are holes that are drilled onto the outside of the tablet allowing for the phenomenon to occur. With your knowledge of how osmotic pressure works, hypothesize what you think happens when a drug is ingested into the body.

Question 30

Describe how temperature and pressure affects the solubility of a solute in a solution. CHM1100C Section 06 General Chemistry Module 06 Quiz

Question 1

What is the difference between the heat capacity and specific heat of a substance?

Question 2

Describe the difference between an exothermic and endothermic process in terms of a chemical compound or reaction.

Question 3

How does Gibbs energy, enthalpy, and entropy determine whether a process will be a spontaneous or nonspontaneous reaction?”

Question 4

Explain the difference between the 3 energy systems and provide a real-world example of a system of energy.

Question 5

Describe the differences between the first, second and third law of thermodynamics.

Question 6

If the energy of the system is the sum of the energy and work, identify the following: What would be the sign of energy (Q) if the system was releasing heat?

Question 7

If the energy of the system is the sum of the energy and work, identify the following: What would be the sign of energy (Q) if the system was absorbing heat?

Question 8

Solve the following thermochemical reactions:

2 HCl + Pb PbCl2+ H2 H = -1861 J/mole What is the enthalpy if there was 4.5 x 10-3g of HCl?

Question 9

Solve the following thermochemical reactions:

2 HCl + Pb PbCl2 + H2 H = -1861 J/mole What is the enthalpy if there was 3.86g of PbCl2?

Question 10

Calculate the amount of heat absorbed or released by the following substances: 65.3g of nitrogen,

T = 334K

Question 11

Calculate the amount of heat absorbed or released by the following substances: 34.6g of water, final temperature = 60°C, initial temperature = 44°C

Question 12

Describe if the following reaction is spontaneous or non-spontaneous based on enthalpy, entropy and Gibbs energy: H = -7458J/mol, S = -3756J/K*mol, and G = -436J at low temperature

Question 13

Describe if the following reaction is spontaneous or non-spontaneous based on enthalpy, entropy and Gibbs energy: H = 8457J/mol, S = 546J/K*mol, and G = 432J at room temperature

Question 14

Predict the trend of entropy in the following scenario: Freezing of water

Question 15

Predict the trend of entropy in the following scenario: Salt dissolving in water

Question 16

Predict the trend of entropy in the following scenario: Entropy of helium v. entropy of Argon Hide answer choices

1.Entropy is higher

2.Entropy is lower

3.No change in entropy

Question 17

Predict the trend of entropy in the following scenario: Water as steam compared to liquid

Question 18

Calculate the reaction entropy ( S°rxn) for the following reaction: 2 LiOH + CO2 Li2CO3 + H2O

Question 19

Calculate the reaction entropy ( S°rxn) for the following reaction: HCl + NaOH NaCl + H2O

Question 20

Calculate the Gibbs energy for the following condition K = 8.2 x 10-11, T = 35?C

Question 21

What is the heat required for a substance that has a mass of 633g, specific heat of 2.454J/g C to change from room temperature to 45C?

Question 22

Write out the equilibrium constant expressions for the following reaction: 2 KClO3 (s) → 2 KCl (s) + 3 O2 (g)

Question 23

Write out the equilibrium constant expressions for the following reaction: H2O (l) → H+ (aq) + OH- (aq)

Question 24

Consider an exothermic reaction. How does the following action affect an equilibrium reaction by driving the reaction? Increasing the temperature of the system

1.Forward reaction

2.Reverse reaction

Question 25

Consider the endothermic reaction N2(g) + 3H2(g) ? 2NH3(g). How does the following action affect an equilibrium reaction by driving the reaction? Decreasing volume of the system, while increasing the pressure