General Chemistry I Chem 110 Dr. Laila Mohammed Al-Harbi Assistant professor Contact Info: Lalhrbi@kau.edu.sa  Web Site: http://lalhrbi.kau.edu.sa

Technicalities Class hours: SMW 8:00 am to 8:50 am (AA) SMW 10:00 am to 10:50 am (AE) Locations: Science tower 07 room 173 first floor phone 6400000 ext. 23024 email Lalhrbi@kau.edu.sa web site: http://lalhrbi.kau.edu.sa Exam schedule: 1st exam : from lecture 1-11 ( Chapters 1-4) = 30 marks 2nd exam: from lecture 12-24 (Chapters 5,7-9) = 30 marks Final exam: from lecture 1-33 = 40 marks (Chapters 1,2,3,4,5,7,8,9,10,14,15,24,25) Home works = Bonus marks

Dr. Laila Mohammed Al-harbi Assistant professor in physical chemistry 1st term schedule (2010-2011) DAY 8-9 9-10 10-11 11-12 12-1 1-2 2-3 3-4 4-5 Saturday CHEM 110 (AA) Office hour (EA) Sunday Lab281 (BB) Monody Lab 281 (JD) (JC) Tuesday CHEM 491 Wednesday CHEM 110 (EA) >>> room 2167 at 1st floor CHEM 110(AA) >>> room 101 A at ground floor Email Lalhrbi@kau.edu.sa Web site: http://lalhrbi.kau.edu.sa

Chemistry, by Chang, 10th. ed., 2007, McGraw-Hill. Course No. Course Title No. of Units Pre-requisites Th. Pr. Credit   Chem 110 General Chemistry  I 3 - Course Objectives: The course aims to introduce students to basic knowledge and principle in chemistry.   Course Description : It provides an introduction to the general principles of chemistry for students planning a professional career in chemistry, a related science, the health professions, or engineering. By the end of this course the student will be able to understand the following: Significant figures, scientific notation and units, stoichiometry, atomic structure & periodic table, chemical bonding, gases, ionic equilibrium, basic principles of organic and basic principles of biochemistry .  Main text books:   Chemistry, by Chang, 10th. ed., 2007, McGraw-Hill. Chemistry, by Steven S. Zumdahl, 6th ed., Houghton Mifflin College Div. Subsidiary books :        Chemistry, by Mortimer, 6th ed., Wadsworth Inc.

Chemistry, by Chang, 10th. ed., 2007, McGraw-Hill.  Main text book :   Chemistry, by Chang, 10th. ed., 2007, McGraw-Hill.

Chapter 1 The study of change 1-7 Measurement SI units Mass and weight Volume Temperature scales Homework Page 33 1.17,1.19,1.22,1.23,1.25,1.26.

Introduction Chemistry is the study of matter and the changes it undergoes There are three states of matter solid liquid gas

1.7 Measurement and Units Macroscopic Which can be determined directly Ex: volume Microscopic Determined indirectly on atomic or molecular scale

Extensive and Intensive Properties An extensive property of a material depends upon how much matter is being considered. mass length volume An intensive property of a material does not depend upon how much matter is being considered. density temperature color

The International System of units (SI Units) used for commerce and science around the world Table 1.2 SI Base Units Base Quantity Name of Unit Symbol Length meter m Mass kilogram kg Time second s Temperature kelvin K Amount of substance mole mol

m

to measure some thing too small (atomic radius of nitrogen ) some thing too big (distance between earth and moon) 7×10-9 m = 7 nm 383403000 m = 384 Mm

Example 1 A) 6.0 km is how many micrometers? Solution 1 1 km = 103 m 6 km = x = 6 × 103 m 1µm = 1× 10-6 m x = 6 × 103 m x = 6 × 109µm Solution 2 1 km = 103 m → 1 m = 10-3 km 1µm = 1× 10-9 m → 1 m = 106µm 10-3 km = 106µm 6 km = x X = 6 × 106 µm/ 10-3 km = x = 6 × 109µm

Which of these quantities represents the largest mass? Examples 2 The diameter of an atom is approximately 1  10-7 mm. What is this diameter when expressed in nanometers?  A. 1  10-18 nm B. 1  10-15 nm C. 1  10-9 nm D. 1  10-1 nm = 1× 10-7 × 1 × 106 = 1 × 10-1 nm = 0.1 nm Examples 3 Which of these quantities represents the largest mass?  A. 2.0  102 mg B. 0.0010 kg C. 1.0  105 g D. 2.0  102 cg Put all of them in the same unit

The weight of man on earth is 50 pounds. Mass and Weight Mass is the measure of the amount of matter in an object. SI unit of mass is the kilogram (kg) 1 kg = 1000 g = 1 x 103 g Weight is the measurement of the pull of gravity on an object. The Mass of an object doesn't change when an object's location changes. Weight, on the other hand does change with location. Chemist are interested primarily in mass weight = c x mass The weight of man on earth is 50 pounds. is 8.25 pounds on moon

Volume – SI derived unit for volume is cubic meter (m3) 1 cm3 = (1 x 10-2 m)3 = 1 x 10-6 m3 1 dm3 = (1 x 10-1 m)3 = 1 x 10-3 m3 1 L = 1000 mL = 1000 cm3 = 1 dm3 1 mL = 1 cm3 Common unit of volume is liter

Density mass density = volume The density of copper is 8.94 g/cm3. Density is defined as the amount of matter in a given amount of space. d = m/V SI derived unit for density is kg/m3 1 g/cm3 = 1 g/mL = 1000 kg/m3 Density is intensive property Density decrease with temperature Unit of density is Kg/l g/ml )g/cm3 for liquid and solids g/l = 0.001g/ml for gases Because density of gases are very low density = mass volume The density of copper is 8.94 g/cm3.

Example 1.1 A piece of Gold metal has a volume of 15.6 cm3, with a mass of 301 g What is its density? A piece of platinum metal with a density of 21.5 g/cm3 has a volume of 4.49 cm3. What is its mass? d = m V d = m V m = d x V 301 g/ 15.6 cm3 = 19.3 g/ cm3 = 21.5 g/cm3 x 4.49 cm3 = 96.5 g

Example 1.2 The density of mercury is 13.6 g/mL has a volume of 5.50 mL. What is its mass? The density of sulfuric acid is 1.41 g/mL has a volume of 242 mL. What is its mass? d = m V d = m V m = d x V = 13.6 g/mL x 5.50 mL = 74.8 g m = d x V = 1.41 g/mL x 242 mL = 341.22 g

Fahrenheit °F →°F = [ (9/5) × °C] + 32 Temperature Scales Fahrenheit °F →°F = [ (9/5) × °C] + 32 Celsius °C → °C = (5/9) (°F - 32) Kelvin ° K → ° K = °C + 273.15

Example 1.3 Convert -452 0F to degrees Celsius. Convert 224 0C to degrees Fahrenheit? °F = (9 0F /5 0C) × °C + 32 [°F = (9 0F /5 0C) × 224 °C] + 32 0C = 435 0F Convert -452 0F to degrees Celsius. °C = (5 0C /9 0F) (°F - 32 0F) °C = (5 0C /9 0F) (-452 °F - 32 0F) = -269 0C Convert -38.9 0C to degrees Kelvin.. ° K = [-38.9 °C + 273.15 °C ] × 1 K/ 1 0C = 234.3 K

Test bank 1. The SI unit of time is the A. hour B. second C. minute D. ampere 2. The diameter of an atom is approximately 1  10-7 mm. What is this diameter when expressed in nanometers?  A. 1  10-18 nm B. 1  10-15 nm C. 1  10-9 nm D. 1  10-1 nm

3. 6.0 km is how many micrometers?  A. 6.0  106 µm B. 1.7  10-7 µm C. 6.0  109 µm D. 1.7  10-4 µm 4. The SI prefixes giga and micro represent, respectively:  A. 10-9 and 10-6. B. 106 and 10-3. C. 103 and 10-3. D. 109 and 10-6.

6. How many cubic centimeters are there in exactly one cubic meter?  A. 1  10-6 cm3 B. 1  10-3 cm3 C. 1  10-2 cm3 D. 1  106 cm3 Solution (1m )3 = (1  10-2 cm )3 1m3 = 1  10-6 cm 3 5. Which of these quantities represents the largest mass?  A. 2.0  102 mg B. 0.0010 kg C. 1.0  105 g D. 2.0  102 cg Solution A) 0.2 g B)1 g C) 0.1 g D) 2 g

7. Ammonia boils at -33.4C. What temperature is this in F?  A. -60.1F B. -92.1F C. -28.1F D. +13.5F F = (9 0F /5 0C) × °C + 32 [°F = (9 0F /5 0C) × -33.4 °C] + 32 0C = 435 0F