CHEM 120: Introduction to Inorganic Chemistry

Instructor: Upali Siriwardane (Ph.D., Ohio State University)

CTH 311, Tele: 257-4941, e-mail: upali@chem.latech.edu

Office hours: 10:00 to 12:00 Tu & Th ; 8:00-9:00 and 11:00-12:00 M,W,& F

Chapters Covered and Test dates

Tests will be given in regular class periods from 9:30-10:45 a.m. on the following days:

September 21,     2004 (Test 1): Chapters 1 & 2

October 6,           2004(Test 2): Chapters 3, & 4

October 20,         2004 (Test 3): Chapter 5 & 6

November 3,        2004 (Test 4): Chapter 7 & 8

November 15,      2004 (Test 5): Chapter 9 & 10

November 17,      2004 MAKE-UP: Comprehensive test (Covers all chapters

Grading:

[( Test 1 + Test 2 + Test3 + Test4 + Test5)] x.70 + [ Homework + quiz average] x 0.30 = Final Average

                                            5

"Chemistry"

Chemistry

Study of the composition, structure and properties of matter and the changes (including energy) that matter undergoes.

Major Areas of Chemistry

Analytical

Biological (Biochemistry)

Inorganic

Organic

Physical.

Chemistry: the ‘central’ science

"Discovery of Penicillin"

Discovery of Penicillin

Alexander Fleming

1. Observation.

2. Formulation of a question

3. Pattern recognition

4. Developing theories. (hypothesis and eventfully theory)

5. Experimentation

6. Summarizing information.( scientific laws)

Matter and properties

Properties are characteristics of matter and are classified as physical or chemical properties.

Matter can exist in 3 physical states.

The three states of matter

_____: atoms or molecules are close together in orderly array; fixed volume and shape.

______: atoms or molecules are close together but relatively free to move about; has a definite volume but takes on shape of container

___: atoms or molecules are widely separate and free to move about; have no definite volume or shape--expand to fill entire container

Slide 7

Physical Properties

_________________ (and change): measured and observed without changing composition of substance; e.g: color, mass, density, volume, melting and boiling points , odor taste

water boils (physical change)

Chemical identity of substance unchanged.

Chemical Properties

__________________: must carry out chemical change to observe; e.g., burning gasoline, smelling perfume, digesting sugar. Atoms rearrange to form new substances

Chemical identities of substances change.

Classify as chemical or physical change

Water boiling to become steam

Butter becoming rancid

Combustion of wood

Melting of ice in spring

Decay of leaves in winter

Intensive and extensive properties

__tensive property: depends on amount of substance; e.g., mass, volume, energy

__tensive properties are additive

__tensive property: does not depend on amount of substance; e.g., temperature, density, pressure.

__tensive properties are not additive

Classification of matter

All matter is either a pure substance or a mixture.

Pure Substances

A. Substance (pure):

    1. has only one component

    2. definite unvarying composition (as         carbon dioxide: 27.3 % carbon, 72.7% oxygen)

    3. uniform properties throughout

    4. cannot be separated into other components or further purified by physical means.

Substances can be

1. _________: substances that cannot be separated into simpler substances by chemical means.

2.__________: substances composed of 2 or more elements chemically united in fixed proportions (as CO₂). Compounds can be separated into the elements that make it up by chemical (not physical) means

Mixtures

B. Mixtures: 2 or more substances that can be:

1. combined in any proportion

2. separated into the substances that make it up by physical means

"Mixtures can be:"

Mixtures can be:

1. _____ogeneous : composition is not uniform (granite, orange juice)

2. ____ogeneous: composition is uniform throughout. Solutions are mixtures (salt water, brewed tea and coffee)

Identify as pure substance, homogeneous of heterogeneous mixture

Air

Paint

Perfume

Carbon monoxide

Data, Results and Units

Chemistry is a quantitative science based on experimentation. Take measurements (data).

Each piece of data is the outcome of a measurement.

Results are the outcome of experiments (generally several pieces of data).

"Chemistry is a quantitative science..."

Chemistry is a quantitative science based on experimentation. Take measurements.

A measurement is a number and a unit that describes what the measurement is measuring.

In chemistry we use the metric system for taking measurements. We also use scientific notation to make life easier.

Scientific notation

Based on powers of 10

1000 = 1 x 10 x 10 x 10 = 1 x 10³

56,000,000 = 5.6 x 10,000,000 or 5.6 x 10⁷

0.000068 = 6.8 x 1/100,000 or 6.8 x 10^-5

"Express in scientific notation:"

Express in scientific notation:

     0.000570

      248,000,000

Express in decimal notation:

      3.44 x 10^-4

       1.45 x 10⁵

Move decimal one place to right, , exponent

Move decimal one place to left,      exponent

Brief review

Addition or subtraction: both numbers must be expressed as the same power of 10: 145.756 + 5.3 x 10^-2

Multiplication : N₁ x N₂, add exponents of the nos.

Division: N₁/N₂ , subtract the exponents of N₂ from N₁

Exponents on your calculator

6.56 x 10⁸ (7.054 x 10^-6)(4.9 x 10¹²)

To put exponents in your calculator, use the EE or EXP key!!!!!

Metric system

Base unit as meter (m),(for length), gram (g) (for mass), liter (L) (for volume), etc

In order to express our measuremenmts as #s that are close to whole #s, we use the following prefixes. Prefixes that tell us how far the measurement is from the base unit.

"Learn this table!!!!"

Learn this table!!!!

Prefix          symbol              meaning

   Mega-              M                      10⁶(1,000,000)

Kilo-                k                      10³(1,000)

Deka-              da                     10¹(10)

        base unit                          10⁰(1)

Deci-               d                       10^-1 (0.1)

Centi-              c                       10^-2(0.01)

Milli-              m                      10^-3(0.001)

Micro-            m                       10^-6 (0.000001)

Nano-              n                      10^-9 (0.000000001)

"1 ns (nanosecond)"

1 ns (nanosecond) = ?

           1 ns (nanosecond) =

1mm (millimeter) =   ?

          1mm (millimeter) =

1kg (kilogram) =        ?

          1kg (kilogram) =

1 cL (centiliter) =       ?

          1 cL (centiliter) =

Significant figures

How many nos. can I write down, legitimately, when I make a measurement?

You are allowed to write down all nos. that are measured with certainty plus one that is estimated, The no. of the recorded figures (including the estimated no.) are the no. of sig. fig. in the measurement.

How to figure the no. of sig fig in a recorded no.

1.All nonzero digits are significant 965 12,456 3.41567

Zeroes may be troublesome.

2. Zeroes btn 2 nonzero digits are sig. 10.143 20006 230807 3.00001

3. Zeroes that come before the first nonzero digit (after the decimal pt) are not sig. 0.000000045 (4.5 x 10^-8)

"4."

4. Zeroes at the end of a no. and after a decimal are significant (trailing zeros). 0.076800 10.076800

5. Zeroes at the end of a no. without a decimal are ambiguous. 4500

Rounding off of data

1. If the first "extra" digit is LESS than 5-drop it. Now the last digit of the number remains the same.

Ex. 4.321 becomes 4.32

2. If the first "extra" digit is 5 or MORE than 5, drop the number and increase the last significant digit by 1.

Ex. 4.336 becomes 4.34

What is this "even/odd rule" I keep hearing about?

When digit is exactly 5: option will give an even number as the answer (last digit is 0, 2, 4, 6, or 8). Refer to the examples above.

Addition and subtraction rules

Rule for addition and subtraction: the answer can’t have more nos. after the decimal pt than the original no with the fewest nos after the decimal.

What is the result of adding 8.355, 4.687 x 10^-3 and 99.1568?

"Rule for multiplication and division..."

Rule for multiplication and division:the answer can’t have more sig. fig. Than the no. with the least no. of sig. fig.

4.56 x 10⁶ (7.954 x 10^-8)(4.5 x 10¹¹)

What is the answer to the correct no. of significant figures of...

1.446 x 10^-3 - 2.91 x 10^-5

(12.675)(10.03) (9.44 + 6.885)

Experimental quantities that we measure

Mass (amt of matter in an object--location independent) in kilograms(kg) (SI units) but grams (g) more convenient

Weight: force that gravity exerts on an object--location dependent

weight = mass x acceleration due to gravity,

When gravity is constant, mass and weight are directly proportional. (Gravity depends on distance from center of the earth)

Units of mass

1 pound = 16 ounces; 1 ton = 2000. lbs

1 pound = 454 g; 2.2 lbs = 1 kg = 10³ g

1 amu (atomic mass unit) = 1.661 x 10^-24 g

"Length:"

Length: distance btn 2 points

Length in meters ( SI units); frequently cm: 1 cm = 10^-2m

1 ft = 12 inches; 1 yd = 3 ft; 1 mile = 5280ft

1 inch = 2.54 cm; 1 yd = 0.91 m (1 m = 39. 56 in)

"Volume (amt of space..."

Volume (amt of space occupied by matter) in m³(SI units) ;

more conveniently liters (1 L = 1 dm³)

or milliliters (1 mL = 1 cm³)

1 gallon = 4 qts; 1 qt = 2 pts = 32 fluid oz (4 cups = 1 qt)

1 qt = 0.946 L (1L = 1.06 qt); 1 gal = 3.78 L

Conversion from one unit to another: factor label method

1. Identify the problem.

2. Write down all conversion factors that let you go from the given units to the units that you want your answer to be in. (Or write down the relevant equation.)

3. Set up conversion factors so units cancel and you’re left with the units you want your answer in. (Or substitute in the eqn and solve.)

"Convert 32.0 oz to..."

Convert 32.0 oz to lbs, tons, grams, milligrams 1 lb = 454 g

How many miles in 1.0 km? 1 in = 2.54 cm

Convert 3.0 km to inches, yds, millimeters.

Convert 10.0 pts to qts, gals, and microliters 1 qt = 0.946 L

Convert 68.3 cm³ to cubic kilometers.

"1.64:"

1.64: A newborn is 21 inches in length and weighs 6 lb 9 oz. Convert to metric units. 1 lb = 454 g 1 in = 2.54 cm

Other things we measure

Concentration: amt of a substance in a given unit volume; as the no of red blood cells/L; the number of rose petals in a given volume in a vase of a given size, etc.

Molarity: Moles of a compound in a liter of solution

"In chemistry a useful concentration..."

In chemistry a useful concentration unit is density.

Density = mass volume

d = m V

Units g/mL(for solids and liquids) or g/L (for gases)

Specific gravity

Specific gravity = density of object(g/mL) density of water (g/mL)

Specific gravity is unitless. Normally use 1.00 g/mL for density of water.

Density problems

A lead sphere has a mass of 1.20 x 10⁴ g and a volume of 1.05 x 10³ cm³. Calc the density of lead.

1.76: What volume, in liters, will 8.00 x 10² g of air occupy if the density of air is 1.29 g/L?

"1.78."

1.78. What is the mass, in grams, of a femur (leg bone) having a volume of 118 cm³? The density of bone is 1.8 g/cm³ ?

We also measure

Time: in seconds (s)

60 s = 1 minute; 60 minutes = 1 hour, etc

And temperature ( degree of hotness)

Temperature usually in degrees Celsius (°C)

Related to familiar degrees Fahrenheit (°F) by °C = (°F -32) 1.8

And ^oF = 1.8^oC + 32

"As a check"

As a check water freezes at 0°C (32^oF), boils at 100°C (212^oF)

Kelvin scale used in many chemistry calculations

Kelvin is “absolute temperature,” related by K = °C + 273.15

Water boils at 373 K, freezes at 273 K.

Slide 50

Temperature conversions

Convert 85^oC to ^oF and K.

Convert -15^oF to ^oC and K.

Comvert 251K to ^oC.

Energy

Energy: ability to do work

Kinetic energy: energy of motion

Potential energy: energy of position.

Chemical, electrical, nuclear, wind, etc energy

Law of conservation of energy

Energy cannot be created or destroyed, only changed in form. The total energy in the universe is a constant.

Energy measured in calories(cal) and joules (J).

1 cal = 4.184 J and is the amt of heat energy needed to raise the temperature of 1 gram of water by 1 degree C.

Food calorie = 1000 cal or Kcal (kilocalories)


	Instructor: Upali Siriwardane (Ph.D., Ohio State University)
	CTH 311, Tele: 257-4941, e-mail: upali@chem.latech.edu
	Office hours: 10:00 to 12:00 Tu & Th ; 8:00-9:00 and 11:00-12:00 M,W,& F


	Tests will be given in regular class periods from 9:30-10:45 a.m. on the following days:
	September 21, 2004 (Test 1): Chapters 1 & 2
	October 6, 2004(Test 2): Chapters 3, & 4
	October 20, 2004 (Test 3): Chapter 5 & 6
	November 3, 2004 (Test 4): Chapter 7 & 8
	November 15, 2004 (Test 5): Chapter 9 & 10
	November 17, 2004 MAKE-UP: Comprehensive test (Covers all chapters
	Grading:
	[( Test 1 + Test 2 + Test3 + Test4 + Test5)] x.70 + [ Homework + quiz average] x 0.30 = Final Average
	5


	Chemistry
		Study of the composition, structure and properties of matter and the changes (including energy) that matter undergoes.
	Major Areas of Chemistry
		Analytical
		Biological (Biochemistry)
		Inorganic
		Organic
		Physical.
	Chemistry: the ‘central’ science


	Discovery of Penicillin
	Alexander Fleming
	1. Observation.
	2. Formulation of a question
	3. Pattern recognition
	4. Developing theories. (hypothesis and eventfully theory)
	5. Experimentation
	6. Summarizing information.( scientific laws)


	Properties are characteristics of matter and are classified as physical or chemical properties.

	Matter can exist in 3 physical states.


	_____: atoms or molecules are close together in orderly array; fixed volume and shape.
	______: atoms or molecules are close together but relatively free to move about; has a definite volume but takes on shape of container
	___: atoms or molecules are widely separate and free to move about; have no definite volume or shape--expand to fill entire container


	_________________ (and change): measured and observed without changing composition of substance; e.g: color, mass, density, volume, melting and boiling points , odor taste
	water boils (physical change)
	Chemical identity of substance unchanged.


	__________________: must carry out chemical change to observe; e.g., burning gasoline, smelling perfume, digesting sugar. Atoms rearrange to form new substances
	Chemical identities of substances change.



	Water boiling to become steam
	Butter becoming rancid
	Combustion of wood
	Melting of ice in spring
	Decay of leaves in winter


	__tensive property: depends on amount of substance; e.g., mass, volume, energy
	__tensive properties are additive
	__tensive property: does not depend on amount of substance; e.g., temperature, density, pressure.
	__tensive properties are not additive


	A. Substance (pure):
	1. has only one component
	2. definite unvarying composition (as carbon dioxide: 27.3 % carbon, 72.7% oxygen)
	3. uniform properties throughout
	4. cannot be separated into other components or further purified by physical means.


	1. _________: substances that cannot be separated into simpler substances by chemical means.
	2.__________: substances composed of 2 or more elements chemically united in fixed proportions (as CO₂). Compounds can be separated into the elements that make it up by chemical (not physical) means


	B. Mixtures: 2 or more substances that can be:
	1. combined in any proportion
	2. separated into the substances that make it up by physical means


	Mixtures can be:
	1. _____ogeneous : composition is not uniform (granite, orange juice)
	2. ____ogeneous: composition is uniform throughout. Solutions are mixtures (salt water, brewed tea and coffee)


	Chemistry is a quantitative science based on experimentation. Take measurements (data).
	Each piece of data is the outcome of a measurement.
	Results are the outcome of experiments (generally several pieces of data).


	Chemistry is a quantitative science based on experimentation. Take measurements.
	A measurement is a number and a unit that describes what the measurement is measuring.

	In chemistry we use the metric system for taking measurements. We also use scientific notation to make life easier.


	Based on powers of 10

	1000 = 1 x 10 x 10 x 10 = 1 x 10³
	56,000,000 = 5.6 x 10,000,000 or 5.6 x 10⁷
	0.000068 = 6.8 x 1/100,000 or 6.8 x 10^-5


	Express in scientific notation:
	0.000570
	248,000,000
	Express in decimal notation:
	3.44 x 10^-4
	1.45 x 10⁵
	Move decimal one place to right, , exponent
	Move decimal one place to left, exponent


	Addition or subtraction: both numbers must be expressed as the same power of 10: 145.756 + 5.3 x 10^-2

	Multiplication : N₁ x N₂, add exponents of the nos.
	Division: N₁/N₂ , subtract the exponents of N₂ from N₁


	6.56 x 10⁸ (7.054 x 10^-6)(4.9 x 10¹²)
	To put exponents in your calculator, use the EE or EXP key!!!!!


	Base unit as meter (m),(for length), gram (g) (for mass), liter (L) (for volume), etc
	In order to express our measuremenmts as #s that are close to whole #s, we use the following prefixes. Prefixes that tell us how far the measurement is from the base unit.


	Learn this table!!!!
	Prefix symbol meaning
	Mega- M 10⁶(1,000,000)
	Kilo- k 10³(1,000)
	Deka- da 10¹(10)
	base unit 10⁰(1)
	Deci- d 10^-1 (0.1)
	Centi- c 10^-2(0.01)
	Milli- m 10^-3(0.001)
	Micro- m 10^-6 (0.000001)
	Nano- n 10^-9 (0.000000001)


	1 ns (nanosecond) = ?
	1 ns (nanosecond) =
	1mm (millimeter) = ?
	1mm (millimeter) =
	1kg (kilogram) = ?
	1kg (kilogram) =
	1 cL (centiliter) = ?
	1 cL (centiliter) =


	How many nos. can I write down, legitimately, when I make a measurement?
	You are allowed to write down all nos. that are measured with certainty plus one that is estimated, The no. of the recorded figures (including the estimated no.) are the no. of sig. fig. in the measurement.


	1.All nonzero digits are significant 965 12,456 3.41567
	Zeroes may be troublesome.
	2. Zeroes btn 2 nonzero digits are sig. 10.143 20006 230807 3.00001
	3. Zeroes that come before the first nonzero digit (after the decimal pt) are not sig. 0.000000045 (4.5 x 10^-8)


	4. Zeroes at the end of a no. and after a decimal are significant (trailing zeros). 0.076800 10.076800
	5. Zeroes at the end of a no. without a decimal are ambiguous. 4500


	1. If the first "extra" digit is LESS than 5-drop it. Now the last digit of the number remains the same.
	Ex. 4.321 becomes 4.32
	2. If the first "extra" digit is 5 or MORE than 5, drop the number and increase the last significant digit by 1.
	Ex. 4.336 becomes 4.34
	What is this "even/odd rule" I keep hearing about?
	When digit is exactly 5: option will give an even number as the answer (last digit is 0, 2, 4, 6, or 8). Refer to the examples above.


	Rule for addition and subtraction: the answer can’t have more nos. after the decimal pt than the original no with the fewest nos after the decimal.

	What is the result of adding 8.355, 4.687 x 10^-3 and 99.1568?


	Rule for multiplication and division:the answer can’t have more sig. fig. Than the no. with the least no. of sig. fig.
	4.56 x 10⁶ (7.954 x 10^-8)(4.5 x 10¹¹)


	Mass (amt of matter in an object--location independent) in kilograms(kg) (SI units) but grams (g) more convenient
	Weight: force that gravity exerts on an object--location dependent
	weight = mass x acceleration due to gravity,
	When gravity is constant, mass and weight are directly proportional. (Gravity depends on distance from center of the earth)