Introduction to the Course General Chem II

Introduction to the Course General Chem II

Presenter

Dr. Luis Bello

[e-mail]

Northeast Campus

Office AB272G Phone Ext. 7451

About me

• More than 35 years of experience

• Taught Chemistry in different countries; (Cuba, Ethiopia, Angola, USA)

• At TCC since January 2020

• Mother language Spanish

• Like to travel (a lot)

• Like to ride bikes and going to the beach.

Now, your turn to introduce yourself...

Name

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Hobbies

Expectations about this class.

General info about the course

General info about the course

• Teaching methods

• Discussions, Quizzes, Mid-Term, Final Term

• Lab Activities and Reports (missing labs!!)

• Safety Rules (clothes, goggles, pants, close toes shoes)

• Late submissions

• Textbook

• Schedule

General Chemistry I Syllabus

Essential Ideas 

Atoms molecules and Ions 

Composition of Substances and solutions 

Stoichiometry of Chemical Reactions

Thermochemistry 

Electronic Structure and Periodic Properties of Elements 

Chemical Bonding and Molecular Geometry 

Gases Liquids, Solids, and Intermolecular Forces 

Topics to be covered on General Chemistry II

Unit 1: Liquids and Solutions: Liquids and Solutions covers the properties of liquids, the process of dissolving, solutions and their concentrations, colligative properties of solutions, and the kinetics of liquids including rates of evaporation and freezing.
Unit 2: Kinetics and Equilibrium: The Kinetics and Equilibrium chapter covers the concepts of reaction rates, rate laws, activation energy, catalysis, chemical equilibrium, Le Chatelier's principle, equilibrium constants, and factors that affect chemical equilibrium.
Unit 3: Acid-Base and Additional Equilibria: The Acid-Base and Additional Equilibria chapter covers the properties of acids and bases, pH and pOH, acid and base strength, acid-base equilibrium calculations, buffers, acid-base titrations, solubility equilibria, and complex ion equilibria
Unit 4: Thermodynamics and Electrochemistry: The Thermodynamics and Electrochemistry chapter covers the laws of thermodynamics, entropy and free energy, redox reactions, electrochemical cells, cell potential, and applications of electrochemistry including corrosion and electrolysis.

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Electronic Structure and Periodic Properties of Elements 

Multiple Choice

What are the building blocks of matter?

• Atoms

• Protons

• Cells

• Neutrons

Multiple Choice

In what section would Noble Gases be found?

• white

• yellow

• blue

• red

Multiple Choice

What is the number of protons that the element in this image contain?

• 14

• 7

• 15

• 18

Multiple Choice

The electronic configuration of Ca is?

• 2,8,8,2

• 2,8,8,8,8,6

• 2,8,8

Multiple Choice

The atomic number of this element is___________and it is located in group ____________

• 5 and group 2

• 7 and group 7

• 7 - group 5

• 7 and group 2

Multiple Choice

Which of the following best describes isotopes?

• Isotopes have different numbers of neutrons.

• Isotopes have different numbers of protons.

• Isotopes are atoms of the same element with the same mass.

• Isotopes have different numbers of electrons.

Multiple Choice

How does the average atomic mass of an element compare to the mass number?

• The average atomic mass is the average mass of a mixture of isotopes, whereas each isotope has its own mass number.

• The average atomic mass of an element is the same as its mass number.

• The average atomic mass is equal to the mass number of the most abundant isotope of an element.

• The average atomic mass includes the mass of the electrons, whereas the mass number depends only on the neutrons and the protons.

Multiple Choice

The image shows the periodic grid of potassium. How many electrons are found in the potassium atom?

• 19

• 20

• 39

• 40

Multiple Choice

What are the building blocks of matter?

• Atoms

• Protons

• Cells

• Neutrons

Composition of Substances and solutions

Multiple Choice

What is the purpose of Filtration?

• Separating and insoluble solid from a liquid

• Separation of a mixture of 2 solids

• Separates heavier substances from a suspension

Multiple Choice

Which process names a change you could predict would happen to water due to cooling?

• Boiling

• Evaporating

• Freezing

• Melting

Multiple Choice

The process of changing solid to gas directly is ______

• Evaporation

• Condensation

• Melting

• Sublimation

Multiple Choice

A mixture that has the same composition throughout because all the parts are mixed evenly is a(n)

• State of Matter

• Solution

• Evaporation

• Condensation

Multiple Choice

Dry ice is solid carbon dioxide, or CO2. Dry ice may be used as a cooling agent and contains two oxygen atoms bonded to a carbon atom. Dry ice is a ___________________ .

• pure substance

• mixture

Stoichiometry of Chemical Reactions

Multiple Choice

When does a chemical reaction stop?

• When the lab is finished

• When the excess reactant is used up

• When the limiting reactant is used up

• Chemical reactions never stop

Multiple Choice

What is the mole ratio of H₂O to H₃PO₄ in the following chemical equation?   P₄O₁₀ + 6 H₂O --> 4 H₃PO₄ 

• 6:4

• 4:6

• 1:3

• 3:1

Multiple Choice

If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the

• theoretical yield

• mole ratio

• actual yield

• percentage yield

Multiple Choice

2Al + 3H₂SO₄ -> Al₂(SO₄)₃ + 3H₂ How many grams of aluminum sulfate would be formed if 250g H₂SO₄ completely reacted with aluminum?

• 0.85 g

• 290 g

• 450 g

• 870 g

Thermochemistry 

Multiple Choice

During an exothermic reaction, heat content in the surroundings increases because

• heat energy is destroyed during reactions

• the reaction absorbs heat energy

• the energy contained in the reactants is lower then the products

• the energy contained in the products is lower than the reactants

Multiple Choice

The diagram represents two solids and the temperature of each. What occurs when the two solids are placed in contact with each other?

• Heat energy flows from solid A to solid B. Solid A decreases in temperature

• Heat energy flows from solid A to solid B. Solid A increases in temperature

• Heat energy flows from solid B to solid A. Solid B decreases in temperature.

• Heat energy flows from solid B to solid A. Solid B increases in temperature.

Multiple Choice

The potential energy diagram of a reaction is shown. Which statement below is correct relating to this reaction?

• #1 represents the enthalpy change for this exothermic reaction.

• #2 represents the enthalpy change for this endothermic reaction.

• #3 represents the enthalpy change for this endothermic reaction.

• #4 represents the enthalpy change for this exothermic reaction.

Multiple Choice

The amount of heat energy required to change the temperature of 12 g of gold from 45°C to 15°C is -47 J. What is the specific heat capacity of gold?

• 0.13 J/(g°C)

• 17,000 J/(g°C)

• 1600 J/(g°C)

• 0.065 J/(g°C)

Multiple Choice

Any substance that does not conduct electricity when in solution is called a(n) ―

• nonelectrolyte

• electrolyte

• conductor

• semiconductor