CHEMISTRY 101 Dr. Mohammad Nahid Siddiqui Sections 04, 05, 06  Textbook : Zumdahl, 7 th Edition  Office Location: Building 4, Room 114  Office Hours: SMW 09:00-11:00 am or by appointment  Office Telephone: 2529   Website: faculty.kfupm.edu.sa/Chem/mnahid

Students’ Responsibilities 1.Read and Study every detail in textbook. 2.Use Online Study Center of Zumdahl website: Search for other sources of information: other textbooks and references, internet, etc. 4.Solve and submit homeworks on time in webCT. 5.Homeworks are NOT enough to get a good grade, students should solve all the problems they can and also old exams.

Homework Students are advised to do the homework problems in webCT. Solutions to the homework problems will be posted on CHEM 101 bulletin board located outside Room # after the completion of each chapter. The exam results will be posted on CHEM 101 bulletin board and in my personal website also. Quizzes and Exams Quizzes will be given at the beginning of recitation classes and exams will be common. The problems in quizzes and exams can be related to any material mentioned in the syllabus. General Policy on attendance and make-ups Attendance in the classes will be taken within 5 minutes of the beginning of the class. DN grade will be given to any student exceeding: 9 unexcused or 15 excused/unexcused absences in the lecture classes. OR 3 unexcused or 5 excused/unexcused absences in the lab classes. Officially authorized excuse of absences must be presented to the instructor no later than one week following his resumption of classes. (c) No make-ups will be given for any missed majors, quizzes & labs.

Final Grade Distribution ComponentPointsPercent (%) First major Second major Laboratory work 100* 25 Classwork: (a) Quizzes + WebCT 90** 22.5 (b) Attendance 10*** 2.5 Final Exam Total (*) Normalized to an average of 75 (**) Normalized to an average of 58.5 (***) One point will be deducted for each absence.

CHEM 101-LLF (062) - Attendance Write your FIRST or LAST Name Only, No Signature, Dated: Sept SNSN Sec-04NameWRITESec-05 NameWRITE Sec-06 NameWRITE AL-QATEEFI, AHMAD JASIM M AL- OTAIBI, HAITHEM SHAREA AL- GHUFAILI, MANEA MUHAMM AL- SHAMMARI, SULTAN AL- AS ZAINI, HASSAN REDHA HASSA AL- GAHTANI, NADER SAEED A AL-ANAZI, AHMAD MUSAAD ME AL-EID, ALI SAAD ALI AL- MUHAIMID, ABDUL- KARIM AL- HAMDAN, MOHAMMAD ABDUL AL- SHUHAIL, IBRAHIM SALEH AL-HARBI, NAYEF OWAIDH AY

Instructor’s Role To summarize important points of each chapter. Give directions on how and where to find information. Solve typical problems and give quizzes during recitation. Answer your questions during office hours. In summary, I am a facilitator and a teacher that will provide information.

Chapter 1 Chemical Foundations

Steps in the Scientific Method 1.Observations  quantitative  qualitative 2.Formulating hypotheses  possible explanation for the observation 3.Performing experiments  gathering new information to decide whether the hypothesis is valid whether the hypothesis is valid

Outcomes Over the Long-Term Theory (Model)  A set of tested hypotheses that give an overall explanation of some natural phenomenon. overall explanation of some natural phenomenon. Natural Law  The same observation applies to many different systems different systems  Example - Law of Conservation of Mass

Law and Theory A law summarizes what happens; A theory (model) is an attempt to explain why it happens. Theory is a human invention and attempts to explain human experience. It may change with time e.g. solar system.

Nature of Measurement Measurement - quantitative observation consisting of two parts: Part 1 - number Part 2 - scale (unit) Part 2 - scale (unit)Examples: 20 grams 6.63    Joule seconds

International System (le Système International) Based on metric system and units derived from metric system.

Physical QuantityNameAbbreviation Masskilogramkg Lengthmeterm Timeseconds TemperatureKelvinK Electric CurrentAmpereA Amount of Substance molemol Luminous Intensitycandelacd The Fundamental SI Units

Common types of laboratory equipment used to measure liquid volume.

An electronic analytical balance.

Uncertainty in Measurement A digit that must be estimated is called uncertain. A measurement always has some degree of uncertainty.

Measurement of volume using a buret. The volume is read at the bottom of the liquid curve (called the meniscus) ml 20.17ml 20.15ml 20.18ml ±0.01ml

Precision and Accuracy Accuracy refers to the agreement of a particular value with the true value. Precision refers to the degree of agreement among several elements of the same quantity. Example: Accuracy and PrecisionAccuracy and Precision

Figure 1.10: The results of several dart throws show the difference between precise and accurate.

Types of Error Random Error (Indeterminate Error) - measurement has an equal probability of being high or low. Systematic Error (Determinate Error) - Occurs in the same direction each time (high or low), often resulting from poor technique.

Rules for Counting Significant Figures - Overview 1.Significant Figures = Certain + Uncertain Digits 2.Nonzero integers (1-9) 3.Zeros  leading zeros, before (1-9)  captive zeros, between (1-9)  trailing zeros, after (1-9) 4.Exact numbers = NO Uncertain Digits

Rules for Counting Significant Figures - Details Nonzero integers always count as significant figures has 4 sig figs.

Rules for Counting Significant Figures - DetailsZeros  Leading zeros do NOT count as significant figures has 3 sig figs.

Rules for Counting Significant Figures - DetailsZeros  Captive zeros always count as  Captive zeros always count as significant figures has 4 sig figs.

Rules for Counting Significant Figures - DetailsZeros  Trailing zeros are significant only  Trailing zeros are significant only if the number contains a decimal point has 4 sig figs.

100. has 3 significant figures = 1.00 x has 1 significant figures = 1 x ??

Rules for Counting Significant Figures - Details Exact numbers have an infinite number of Sig Figs. Significant Figures = Certain + Uncertain Digits Significant Figures = Certain + Uncertain Digits Exact numbers = Certain Digits Only + No Uncertain Exact numbers = Certain Digits Only + No Uncertain Independent of measuring device: 1 apple, 10 students, 5 cars…. 2πr The 2 is exact and 4/3 π r 2 the 4 and 3 are exact From Definition: 1 inch = 2.54 cm exactly The 1 and 2.54 do not limit the significant figures

Scientific Notation The number of atoms in 12 g of carbon: 602,200,000,000,000,000,000, x The mass of a single carbon atom in grams: x N x 10 n N is a number between 1 and 10 n is a positive or negative integer

Scientific Notation n > = x 10 2 move decimal left n < = 7.72 x move decimal right Addition or Subtraction 1.Write each quantity with the same exponent n 2.Combine N 1 and N 2 3.The exponent, n, remains the same 4.31 x x 10 3 = 4.31 x x 10 4 = 4.70 x 10 4

Rules For Rounding 1.In a series of calculations, carry the extra digits through to the final result, then round. 2.If the digit to be removed: A.Is less than 5, then no change e.g rounded to 2 sig. fig = 1.3 B.Is equal or greater than 5, the preceding digit increase by 1 e.g rounded to 2 sig. fig = 1.4

Rules for Significant Figures in Mathematical Operations Multiplication and Division: Number of sig figs in the result MUST equals the Lowest number in the precise measurement used in the calculation  2.0 =  13 (2 sig figs)

Rules for Significant Figures in Mathematical Operations Addition and Subtraction: Number of decimal places in the result MUST equals the Lowest number of decimal places in the precise measurement used in the calculation =  18.7 (3 sig figs)

Rules for Counting Significant Figures. For more information: go to Appendix A1 at the end of the book

Dimensional Analysis Proper use of “unit factors” leads to proper units in your answer: 2.54 cm = 1 inch 1 inch/2.54 cm = 1 Unit factor What is the length in inch of 2.85 cm pencil 2.85 (cm) x 1 (inch)/2.54(cm) = 2.85/2.54 = 1.12 in

Dimensional Analysis 1.Determine which unit conversion factor(s) are needed 2.Carry units through calculation 3.If all units cancel except for the desired unit(s), then the problem was solved correctly. 1 L = 1000 mL How many mL are in 1.63 L? 1L 1000 mL 1.63 L x = 1630 mL 1L 1000 mL 1.63 L x = L2L2 mL

For more information go to Appendix A26 at the end of the book

Temperature Celsius scale =  C Kelvin scale = K Fahrenheit scale =  F

Temperature SIGNIFICANT FIGURES DEPEND ON THE VALUE OF T C or T F ONLY – MEASURED VALUE

Figure 1.11: The three major temperature scales. 180/100= 9/5

TFTF Tc

Figure 1.12: Normal body temperature on the Fahrenheit, Celsius, and Kelvin scales.

Density Density is the mass of substance per unit volume of the substance:

Matter: Anything occupying space and having mass.

Classification of Matter Three States of Matter: Solid: rigid - fixed volume and shape Liquid: definite volume but assumes the shape of its container Gas: no fixed volume or shape - assumes the shape of its container

Types of Mixtures Mixtures have variable composition. A homogeneous mixture is a uniform solution- visibly indistinguishable (for example, vinegar, gasoline, gold) A heterogeneous mixture is, to the naked eye, clearly not uniform-distinguishable (for example, soil, atmosphere, carbonated drinks- pepsi)

Pure Substances Can be isolated by separation methods:  Chromatography  Filtration  Distillation

Figure 1.15a: Paper chromatography of ink. (a) A line of the mixture to be separated is placed at one end of a sheet of porous paper.

Figure 1.15b: Paper chromatography of ink. (b) The paper acts as a wick to draw up the liquid.

Figure 1.15c: Paper chromatography of ink. (c) The component with the weakest attraction for the paper travels faster than the components that cling to the paper.

Figure 1.14: Simple laboratory distillation apparatus.

Element: A substance that cannot be decomposed into simpler substances by chemical means. Compound: A substance with a constant composition that can be broken down into elements by chemical processes.

Figure 1.16: The organization of matter.