SCI118 - Chemistry · SCI118 - Chemistry Tue –6:00pm to 9 ... Chemistry liquid nitrogen gold ingots silicon crystals. Scientific Method •Being able to answer the who, what, why,

SCI118 - ChemistryTue – 6:00pm to 9:20pmThu – 1:30pm to 4:50pm Fri – 10:00pm to 1:20pm

Instructor: Paul Desi

Contact InformationINSTRUCTOR: Paul Desi

E-MAIL: [email protected]

INSTRUCTORS OFFICE HOURS: By appointment

TELEPHONE:(602)254-3099 (leave message at frontdesk)

(480)779-9469 (Personal Google number)

mailto:[email protected]

Course Information

CLASSROOM LOCATION: 202

COURSE LENGTH: 6 weeks START DATE: 7/5/2016

COMPLETION DATE: 8/12/2016

DAY AND TIME:Tue – 6:00pm to 9:20pmThu – 1:30pm to 4:50pm Fri – 10:00pm to 1:20pm

COURSE CREDIT HOURS: 4.0

PREREQUISITES: None

Classroom Material• Textbook:

• Title: Essentials of General, Organic, and Biochemistry:

An integrated Approach. 2nd Edition 2014 Author:

Guinn, D. Publisher: W. H. Freeman and Company: New

York, New York. ISBN: 978-1-1-4292-3124-4

• Lab Manual

• Solutions Guide

• Additional Resources:• http://www.adichemistry.com/index.html

• http://www.chemguide.co.uk/index.html#top

• http://www.iupac.org/

• http://www.asu.edu/courses/chm332/studyaids.html

• http://scienceworld.wolfram.com/chemistry/

• http://ocw.mit.edu/courses/find-by-topic/

• http://environmentalchemistry.com/yogi/chemistry/MolarityMolality

Normality.html

• http://www.msdssearch.com/

http://www.adichemistry.com/index.html

http://www.chemguide.co.uk/index.html#top

http://www.iupac.org/

http://www.asu.edu/courses/chm332/studyaids.html

http://scienceworld.wolfram.com/chemistry/

http://ocw.mit.edu/courses/find-by-topic/

http://environmentalchemistry.com/yogi/chemistry/MolarityMolalityNormality.html

http://www.msdssearch.com/

Course Description

• This course provides instruction in the Introduction to atomic structure, chemical bonding, states of matter, organic and inorganic chemical reactions, and acids and bases. Virtual laboratory experiences are included in the course.

Course ObjectivesAt the completion of the course, students will be able to:

• Compare and contrast the properties of the states

of matter, classify matter and explain its alteration

through chemical and physical changes.

• Explain key concepts, models and experiments

leading to the development of atomic theory and

apply the concepts of atomic theory in writing the

electron configurations of select elements.

• Explain the factors that affect the formation of

solutions and perform calculations of concentration.

• Understand the concept of pH and be able to

perform pH calculations.

• Explain the concept of equilibrium and be able to

apply this concept to strong and weak electrolytes,

acids and bases.

• Describe the properties of acids and bases.

• Implement good study habits for successful

completion of the class.

• Use the language of and vocabulary of general chemistry to describe the scientific method.

• Use the periodic table to identify elements,

atomic numbers, and atomic masses and explain

periodic trends in the properties of the elements.

• Use scientific notation to express very large and

very small numbers and represent measured

quantities to the correct number of significant

figures.

• Use English, metric and SI units to express

measurements and perform appropriate unit

conversions using dimensional analysis.

• Classify chemical reactions and write balanced

chemical equations.

• Use the mole concept in performing mole and

stoichiometric calculations.

• Develop laboratory skills needed to assay some

of the important biochemical compounds found in

samples from living systems.

• Participate in class discussion.

• Appreciate the applications of Chemistry to everyday life and the health profession.

Methods of Evaluation and GradeScale

A minimum passing grade of C+ or 78% is required for successful completion of thiscourse.

*An extra credit assignment will be announced at the beginning of the5th week of class. For those students whose grade is within onepercentage point of the next letter grade, this provides an opportunityto secure a letter grade before the final exam. This may or may not beof importance, depending on how the student performs on the finalexam and throughout the duration of the class.

Assignment Points PercentGrade

LetterPercentage

Qualit

y

Points

Attendance (x18) 90 (5 ea.) 9% (0.5% ea.) A 95 to 100 4.0

Quizzes (x5) 100 (20 ea.) 10% (2% ea.) A- 90 to 94 3.7

Labs (x5) 150 (30 ea.) 15% (3% ea.) B+ 87 to 89 3.3

Homework (x8) 160 (20 ea.) 16% (2% ea.) B 83 to 86 3.0

Test (x3) 300 (100 ea.) 30% (10% ea.) B- 80 to 82 2.7

Final Exam 200 20% C+ 78 to 79 2.3

Dental Chemistry Ex. Cr.

Project50 5% C 73 to 77 2.0

Extra Credit Assignment* 10 1% C- 70 to 72 1.7

TOTAL 1060/1000 106 % D+ 67 to 69 1.3

D 60 to 66 1.0

F 59 or below 0.0

Course Calendar, Objectives, and Assignment

Weekly Schedule SCI 118 – Chemistry

LEC TOPICS:

Important Due Dates

Week 1 – 7/5/16 – 7/8/16

Measuring Matter and Energy

LEC

Chapters 1

Study Guide - Chapter 1 Quizzes – 7/8/16

Quiz 1 – Chapter 1 – 7/8/16

Lab – Chapter 1 (TBD)

Week 2 – 7/12/16 – 7/15/16

Atomic Structure and Nuclear

Radiation

Compounds and Molecules

LEC

Chapters 2, 3

Study Guide - Chapter 2 & 3 Quizzes – 7/15/16

Quiz 2 – Chapter 2 & 3 – 7/15/16

Lab – Chapter 2 & 3 (TBD)

Week 3 – 7/19/16 – 7/22/16

Chemical Quantities and Chemical

Equations

Changes of State and the Gas Laws

LEC

Chapters 4, 5

Test 1 – 7/19/16 Chapters (1-3)

Study Guide – Chapter 4 & 5 Quiz – 7/22/16

Quiz 3 – Chapter 4 & 5 – 7/22/16


Week 4 – 7/26/16 – 7/29/16

Mixtures, Solution Concentrations,

and Diffusion

Acids and Bases

LEC

Chapters 8, 9

Test 2 – 7/26/16 Chapters (4 & 5)

Study Guide - Chapter 8 & 9 Quiz – 7/29/16

Quiz 4 – Chapter 8 & 9 – 7/29/16


Week 5 – 8/2/16 – 8/5/16

Organic Chemistry: Hydrocarbons

LEC

Chapters 6

Study Guide - Chapter 6 Quizzes – 8/5/16

Quiz 5 – Chapter 6 – 8/5/16

Lab – Chapter 6 (TBD)

Week 6 – 8/9/16 – 8/12/16

Review for final

LEC

Review and Final Exam

Test 3 – 8/9/16 Chapters (8,9, & 6)

Dental Chemistry Extra Credit Project – 8/9/16

Review – 8/11/16

Extra Credit Assignment Due 8/12/16

Final Exam – 8/12/16 (Comprehensive)

• Chemistry is the study of matter and the

changes it undergoes

• Matter is anything that occupies space and has

mass.

Chemistry

liquid nitrogen gold ingots silicon crystals

Scientific Method

• Being able to answer the who, what, why, how, and when type questions.

• Helps to develop your critical thinking skills and metacognition.

• Scientists use a planned, organized approach to solving problems.

• A key element of this approach is gathering information through detailed observations.

• Scientists extend their ability to observe by using scientific tools and techniques.

• The scientific process or scientific method is a systematic approach to research or solving a problem

Observation

Gather Data

Create Hypothesis

Test Hypothesis

Form Conclusion

Theories

Laws

Observations

• A way of solving problems

• Observation- what is seen or measured

• Types of Observations:

• Qualitative observations: observed using your. Think of a property such as sight, smell, touch, taste and hear.

• Quantitative observations: observed using an instrument such as rulers, balances, graduated cylinders, beakers, and thermometers. These results are measurable.

Observations

Gather Data

• Data includes both qualitative and quantitative observations

Observation

Gather Data

Hypothesis

• Educated guess of why things behave the way they do (possible explanation)

• Based on the qualitative and quantitative data

Observation

Gather Data

Create Hypothesis

Test the Hypothesis

• We design/use experiments to test hypothesis

• Leads to new observations and data

Observation

Gather Data

Create Hypothesis

Test Hypothesis

Draw Conclusions

• We form a conclusion based on the results (observations and new data) of our tests/experiments

Observation

Gather Data

Create Hypothesis

Test Hypothesis

Form Conclusion

• Our conclusions may lead to new questions (New Hypothesis Created)

• Others’ data may agree with our conclusions (Theory)

• Our conclusion may be a relation that always holds true (Law)

Observation

Gather Data

Create Hypothesis

Test Hypothesis

Form Conclusion

TheoriesLaws

Theories and Laws

• Can form after many tested hypotheses• Theory - why

• Multiple tests that show the same results in different systems • Used to predict what will happen in a similar situation• May change over time

• Law - how• Equations of how things change• Shows a relationship that is always true such as a mathematical

formula.

Hypotheses, Theories, and Laws

• Hypotheses attempt to explain several observations and are often modified after testing.

• Theories are based upon facts as an explanation or based on several laws and can change with time.

• Laws describe relationships (such as equations) that are the same overtime under the same conditions.

Observations

Hypothesis Theories Laws

Facts and Laws Equations/Same

CHAPTER 1: MEASURING MATTER AND ENERGY

• 1.1 Matter and Energy

• 1.2 Measurement in Science and Medicine

• 1.3 Significant Figures and Measurement

• 1.4 Using Dimensional Analysis

Chapter 1: Measuring Matter and Energy

CHAPTER OUTLINE

• Matter is anything that has mass and occupies volume.

• Matter is found in three states, or phases.

• Solid

• Liquid

• Gas

1.1 Matter and Energy

Chapter 1: Measurement, Atoms, and Molecules


• Energy is the capacity to do work.

• There are two forms of energy:

• kinetic energy

•potential energy

KE = ½mv2



• Heat involves the motion of particles.

• Heat always flows from hotter to colder.

• Temperature is not the same as heat: it is a measure of kinetic energy.

• Potential energy is stored energy.

• A rock balanced on a precipice, a gallon of gasoline, and food all contain potential energy.



• A physical change does not affect composition.• Water melting is a physical change. It is reversible.

• A chemical change involves a change in composition. • Cooking food is a chemical change―it is not easily reversible.



• Matter can be macroscopic, microscopic, or atomic in scale.


1.2 Measurement in Science and Medicine

• A measurement is a number and a unit.• The two most common systems of

measurement are the English system and the metric system.

• The metric system has base units:the meter (m) for measuring lengththe gram (g) for measuring massthe second (s) for measuring timethe calorie (cal) for measuring energy





• Prefixes are used when a measurement is much larger or smaller than the base unit.



• Length• The meter is the base unit of length.

•Mass• Mass is a measure of the amount of matter.

• Volume• Volume is a measure of how much space a substance occupies.

• Energy• A calorie is the energy required to raise the temperature of 1

gram of water by 1°C.



• Precision indicates how close measurements are to one

another.

• Accuracy indicates how close measurements are to a

“true” value.


1.3 Significant Figures and Measurement

• The greater the precision of the measuring device, the

more significant figures you can report.

• The last digit is uncertain.





• Exact numbers are obtained by counting. They

have no uncertainty and an infinite number of

significant figures.



• Significant Figures in Calculations

• When multiplying or dividing, the final calculated answer cannot have more significant figures than the measurement with the fewest number of significant figures.

• When adding or subtracting, the final calculated answer should not have more places past the decimal than the measurement with the fewest places past the decimal.



• Energy• To convert between Calories and joules, convert

from Calories to calories, then from calories to joules.

• Dosage• Dosage is a conversion factor between the mass or

volume of the medicine and the weight of the patient.

• Density• Density is mass per unit volume.


1.4 Using Dimensional Analysis

• Converting between English and Metric Units



• Energy conversions• To convert between nutritional Calories and joules, two

conversion factors are needed.

• Convert from Calories to calories, then from calories to joules.

• Adjust significant figures.



15 Cal x 1000 calCal

x4.184Jcal

62,760 J = 63,000 J or 63 kJ

• Temperature • Celsius and Fahrenheit are relative temperature scales, based

on the freezing and boiling points of water.

• A Celsius degree is larger than the size of a Fahrenheit degree. The two scales are offset by 32.

• A Celsius degree is the same size as a kelvin. The two scales are offset by 273 degrees.



• Specific heat is the amount of heat required to raise the temperature of 1 g of a particular substance by 1°C.



Specific heat

• is different for different substances

• is the amount of heat that raises the temperature of 1 g of a

substance by 1 C

• in the SI system has units of J/g C

• in the metric system has units of cal/g C

• SH = J/(g x ΔT) or cal/(g x ΔT)



48

Rearranging the specific heat expression givesthe heat equation.

q = J (or cal) = SH x g x ΔT

The amount of heat energy (q) lost or gained by a substance is calculated from the

• mass of substance (g)

• temperature change (T)

• specific heat of the substance (J/g °C)

Heat Equation

Basic Chemistry Copyright © 2011 Pearson Education, Inc.



49

Transferring Heat EnergyHeat energy

• flows from a warmer object to a colder object

• provides kinetic energy for the colder object

• lost by the warmer object is equal to the heat energy gained by the colder object




Study Check

1. When ocean water cools, the surrounding air

A. cools B. warms C. stays the same

2. Sand in the desert is hot in the day and cool at night. Sand must have a

A. high specific heat B. low specific heat

Solution

1. When ocean water cools, the surrounding air

B. warms

2. Sand in the desert is hot in the day and cool at night. Sand must have a

B. low specific heat

Calculations Using Specific Heat

When we know the specific heat of a substance, we can

• calculate the heat lost or gained by measuring its mass and

temperature change

• write a heat equation

Core Chemistry Skill Using the Heat Equation

Guide to Solving Specific Heat Problems

Study Check

What is the specific heat if 24.8 g of a metal absorbs 275 J of energy and the temperature rises from 20.2 °C to 24.5 °C?

Solution


STEP 1 State given and needed quantities.

STEP 2 Calculate the temperature change.

ΔT = 24.5 °C – 20.2 °C = 4.3 °C

ANALYZE GIVEN NEED

THE PROBLEM 24.8 g metal specific heat

275 J energy

Tinitial = 20.2 °CTfinal = 24.5 °C

Solution


STEP 3 Write the heat equation.

Heat = m × ΔT × SH

STEP 4 Substitute in the given values and calculate the heat, making sure units cancel.

57

Calorimeters and Heat Transfer

A calorimeter

• is used to measure heat transfer

• can be made with a coffee cup, water, and a thermometer

• indicates the heat lost by a sample and gained by water

Heat lost (-q) = Heat (q) gained


58

Change of Phase:Melting and FreezingA substance

• is melting while it changes from a solid to a liquid

• is freezing while it changes from a liquid to a solid

• such as water has a freezing (melting) point of 0 °C

59

Calculations Using Heat of Fusion

The heat of fusion

• is the amount of heat released when 1 g of liquid freezes (at its freezing point)

• is the amount of heat needed to melt 1 g of solid (at its melting point)

• for water (at 0 °C) is

334 J or 80. cal

1 g H2O 1 g H2O

heat released during

freezing = heat needed

during melting

Heat of Fusion

Heat of Fusion for Water

• To melt water,

H2O(s) + 80. cal/g (or 334 J/g) H2O(l)

• To freeze water,

H2O(l) H2O(s) + 80. cal/g (or 334 J/g)

Guide to Calculations Using a Heat Conversion Factor

Study Check

How many kilojoules are needed to melt 32.0 g of ice at 0 °C?

Solution

How many joules are needed to melt 32.0 g of ice at 0 °C?


STEP 2 Write a plan to convert the given quantity tothe needed quantity.

grams of H2O(s) joules (to melt)

ANALYZE GIVEN NEED

THE PROBLEM 32.0 g ice joules to melt ice

0 °C

Heat of

Fusion

Solution


STEP 3 Write the heat conversion factor and any metric factor.

1 g of H2O (s l) = 334 J

Solution


STEP 4 Set up the problem and calculate the needed quantity.

66

Change of Phase:Boiling of Water

At boiling,• all the water molecules

acquire the energy to form a gas (vaporize)

• bubbles of water vapor appear throughout the liquid

67

Heat of Vaporization

The heat of vaporization is the amount of heat

• absorbed to change 1 g of liquid to gas at the boiling point

• released when 1 g of gas changes to liquid at the boiling point

• boiling point of H2O = 100 °C• heat of vaporization (water) =

2260 J or 540 cal1 g H2O 1 g H2O

Heat of Vaporization

Heat of Vaporization for Water (Boiling Point 100 °C )

• Absorbed when 1 g of water changes to steam

H2O(l) + 540 cal/g (or 2260 J/g) H2O(g)

• Released when 1 g of steam changes to water

H2O(g) H2O(l) + 540 cal/g (or 2260 J/g)

Study Check

How many kilojoules (kJ) are released when 50.0 g of steam from a volcano condenses at 100 °C?

Solution



STEP 2 Write a plan to convert the given quantity to the needed quantity.

grams joules kilojoulesof H2O(g)

ANALYZE GIVEN NEED

THE PROBLEM 50.0 g steam kilojoules released

100 °C

Heat of

Condensation

Metric

Factor

Solution


STEP 3 Write the heat conversion factor and any metric factor.

STEP 4 Set up the problem and calculate the needed quantity.

1 g of H2O (g l) = 2260 J

72

Summary of Changes of State

73

Heating Curve

A heating curve

• illustrates the changes of state as a solid is heated

• uses sloped lines to show an increase in temperature

• uses plateaus (horizontal lines) to indicate a change of state

• We will be creating one in part A of the lab.

74

A. A plateau (horizontal line) on a heating curve represents

1) a temperature change

2) a constant temperature

3) a change of state

B. A sloped line on a heating curve represents




Learning Check

75

A. A plateau (horizontal line) on a heating curve represents



B. A sloped line on a heating curve represents


Solution

76

To reduce a fever, an infant is packed in 250. g of ice H2O(s). If the ice (at 0 °C) melts and warms to body temperature (37.0 °C), how many calories are removed?

Note: 2 things are happening here!!1. Change of phase (ice melting)2. Sample (now water) warming to body temperature.3. Must account for BOTH things happening to get the

correct answer!

Example of Combining Heat Calculations

77

STEP 1 List the grams of substance and change of state.

Given 250. g of ice H2O(s); H2O(l) water at 37.0 °C

Need calories to melt H2O(s) at 0 °C and warm to 37.0 °C

Example of Combining Heat Calculations (continued)

78

STEP 2 Write the plan to convert grams to heat.Total heat = kcals to melt ice at 0 °C and to warm liquid

water from 0 °C to 37 °C. For several changes, we can draw a heating diagram.

37.0 °C

temperature increase

S L

melting 0 °C


79


STEP 3 Write heat conversion factors and metric factors if needed.

1 g of H2O(s l) = 80 cal (heat of fusion)

80 cal and 1 g H2O 1 g H2O 80 cal

SH of H2O = 1.00 cal/g °C

1.0 cal and g °C g °C 1.0 cal

80


STEP 4 Set up problem with factors.T = 37.0 °C – 0 °C = 37.0 °C

Heat to melt the water at 0 °C250. g H2O x 80 cal = 20000 cal

1 g H2O

Heat to warm the water from 0 °C to 37 °C250. g x 37.0 °C x 1 cal = 9250 cal

g °C Total: 20000 cal + 9250 cal = 29250 cal

• Matter and Energy

• Matter exists in three physical states: solid, liquid, and gas.

• Energy is defined as the capacity to do work.

• There are two forms of energy: kinetic energy and potential energy.

• Kinetic energy is the energy of motion.

• Potential energy is stored energy.

• Heat is a form of kinetic energy that is transferred from a hot to a cold object.

• The temperature of a substance reflects the average kinetic energy of the particles of that

substance.

• In the gas phase, the particles are far apart and moving rapidly and randomly. In the liquid

phase, they are close together and move randomly. In the solid phase, they are close together

and are arranged in a regular ordered pattern with only vibrational motion.

• A physical change, such as a change of state, does not affect the composition of a substance,

whereas a chemical change (a chemical reaction) alters the composition of a substance.


Chapter Summary

• Measurement in Science and Medicine

• Every measurement has a numerical value and a unit.

• The metric system uses prefixes that represent a multiple of 10 of the base unit:

giga, kilo, deci, centi, milli, micro, nano, pico.

• In the metric system, the base unit of length is the meter, for mass it is the gram,

and for volume it is the liter.

• Energy is a measurable quantity. The units used to describe energy are the joule and

the kilocalorie. The Calorie (with a capital C) is equal to a kilocalorie and used in

nutritional applications only.

• Density, m/V , is a physical property of a substance independent of its quantity.

• Temperature is a measure of kinetic energy and is measured using a thermometer.

• The three temperature scales are the Celsius, Fahrenheit, and Kelvin scales.


Chapter Summary

• Significant Figures and Measurement

• The degree of uncertainty in a measurement is indicated by the number of

significant figures reported in the measured value.

• Precision is an indicator of how close repeated measurements are to each other,

whereas accuracy is a measure of how close the measurements are to the true

value.

• Significant figures are all the nonzero digits and zeros in a measurement that are not

placeholders.

• Exact numbers have an infinite number of significant figures because they are

obtained by counting or represent definitions.

• Solutions to calculations that require multiplying and dividing measured numbers

must be rounded so that there are no more significant figures than in the measured

value with the least number of significant figures.

• Solutions to calculations that require addition and subtraction may not have more

places past the decimal than the measurement with the fewest decimal places.


Chapter Summary

• Using Dimensional Analysis

• Unit conversions are performed using dimensional analysis, a technique for solving

problems based on units. The supplied unit is multiplied by one or more conversion

factors that relate the supplied and requested units, allowing the supplied units to

cancel algebraically, leaving the requested unit.

• Dosage calculations typically involve an English metric conversion of the patient’s

weight multiplied by the dosage expressed as a conversion factor between the mass

of the medicine and the weight of the patient.

• Density is a physical property of a substance defined as its mass per volume: d =

m/V.

• Density can be used as a conversion factor to calculate mass or volume, if density

and either mass or volume is known.

• Temperature conversions between Celsius and Fahrenheit and Celsius and Kelvin

require the use of one of the temperature equations.


Chapter Summary

Documents

SCI118 - Chemistry · SCI118 - Chemistry Tue –6:00pm to 9 ... Chemistry liquid nitrogen gold ingots silicon crystals. Scientific Method •Being able to answer the who, what, why,