Lecture Outline- Chapter 1. · Lecture Outline- Chapter 1. • Great ideas of chemistry • Where...

Lecture Outline- Chapter 1.

• Great ideas of chemistry

• Where did the elements come from?

• Structure of The Periodic Table

• Properties of Matter

• Measurement and Units

• Accuracy, Precision and Significant Figures

Chapter one: Matter and Measurement

The Six Great Ideas of Chemistry

Chapter one: Matter and Measurement

The Six Great Ideas of Chemistry

-structure of matter

-electrostatic forces

-biomolecules & functions-zeolites, solid surfaces-synthetic polymers-VSEPR

1. Atoms Molecules and ions

2. The Chemical Bond

3. Molecular Shape and Geometry

4. Kinetic Theory-PV = 1/3nmc2 = nRT-relates to T, motion, vibration, rotating, librating

5. The Chemical Reaction-formation of new molecules-acids and bases-periodic table

6. Energy and Entropy

-1st and 2nd Law of Thermodynamics-heat transfer-increase in disorder in universe-energy cannot be created or destroyed

Where did the elements come from?

Large Magellanic Cloud179,000 light-years away

http://www.seds.org/messier/xtra/ngc/lmc.html

http://www.seds.org/messier/xtra/ngc/lmc.html

6 weeks later.

• What is the proof for the big bang?

Proof of the Big BangProof of the Big Bang

• G.– Galaxies, stars and clusters of galaxies

Proof of the big bangProof of the big bang

• G.– Galaxies, stars and clusters of galaxies

• B- Background radiation

Proof of the big bangProof of the big bangG.– Galaxies, stars and clusters of

galaxies!• B- Background radiation!• U- Universe is expanding!

Proof of the Big BangProof of the Big Bang• G.– Galaxies, stars and clusters of

galaxies!• B- Background radiation!• U- Universe is expanding!• S- Sky at night is dark!

Proof of the Big BangProof of the Big Bang

• G.– Galaxies, stars and Clusters of galaxies!• B- Background radiation!• U- Universe is Expanding!• S- Sky at night is dark!• H-Hydrogen/Helium abundance!

G.

B

U

S

H

Properties of Matter 01Properties of Matter 01

• Matter: anything that has both mass & volume.

• Properties: describe or identify matter.

• Intensive Properties do not depend on amount.

• Extensive Properties do depend on amount.

Chemistry and the ElementsChemistry and the Elements

Names of Some Common Elements and Their SymbolsAluminum Al Chlorine Cl Manganese Mn Copper (cuprium ) Cu

Argon Ar Fluorine F Nitrogen N Iron (ferrum ) Fe

Barium Ba Helium He Oxygen O Lead (plumbum ) Pb

Boron B Hydrogen H Phosphorus P Mercury (hydrargyrum ) Hg

Bromine Br Iodine I Silicon Si Potassium (kalium ) K

Calcium Ca Lithium Li Sulfur S Silver (argentum ) Ag

Carbon C Magnesium Mg Zinc Zn Sodium (natrium ) Na

Elements and the Periodic Table 01Elements and the Periodic Table 01

• Periods: The seven horizontal rows that group

elements based on their principal quantum number.

• Groups: The 18 vertical columns that group

elements based on their angular momentum

quantum number.

• Main Groups:• s-block elements:

• p-block elements:

• Transition Metal Groups:

• d-block elements:

• f-block elements:

•Two groups on the left (1 & 2)Six groups on the right (13–18)

Ten groups in the middle (3–12)

Fourteen groups between 3 & 4 are called inner transition metals.

Aabtpxr0.mov

• Physical Properties of Halogens

• Physical Properties can be determined without changing the chemical makeup of the sample.

• Some typical physical properties are:

• Some typical physical changes are:

Melting Point, Boiling Point, Density, Mass, Touch, Taste, Temperature, Size, Color, Hardness, Conductivity.

Melting, Freezing, Boiling, Condensation, Evaporation, Dissolving, Stretching, Bending, Breaking.



• Chemical Properties are those that do change the chemical makeup of the sample.

• Some typical chemical properties are:Burning, Cooking, Rusting, Color change, Souring of milk,

Ripening of fruit, Browning of apples, Taking a photograph,

Digesting food.

•Note: Chemical properties are actually chemical changes.

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• Periodic Properties


List of chemical changes possible.

Description by senses –shape, color, odor, etc.Measurable properties –density, boiling point, etc.

PROPERTIES

Old substance destroyed.New substance formed.

New form of old substance.No new substances formed.

CHANGE

CHEMICALPHYSICAL


• Homogeneous matter

• Heterogeneous matter

has the same appearance, composition,

and properties throughout.

has visibly different phases which can be seen,

or properties that vary through the substance.


• Pure substances

• A mixture

have a distinct set of physical and chemical properties and cannot be separated by physical changes.

is two or more pure substances that can be separated by physical changes.

MixturesandCompounds.MOV

• Mixtures and Compounds.


• An element is a pure substance with its own set of

physical and chemical properties that cannot be

decomposed into simpler substances.

• A compound is a pure substance that can be

decomposed by a chemical change into two or

more pure substances.


• Matter Classification: Matter can be subdivided into mixtures and pure substances.


• Metals: Found on left side of periodic table.

• Nonmetals: Found on the right side of periodic table.

• Semimetals: Form a zigzag line at the boundary between metals and nonmetals.


• Which of the following represents a mixture?


• If the red spheres are oxygen and the white are hydrogen, which of the following represents (a) hydrogen peroxide, (b) hydroxide ions, and (c) a mixture of hydrogen and oxygen gas?

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• Sodium and potassium in water

Measurement and Units 01Measurement and Units 01

• Seven Fundamental SI Units of Measurement.

Physical Quantity Name of Unit Abbreviation Mass kilogram kg

Length meter m Temperature kelvin K

Amount of substance mole mol Time second s

Electric current ampere A Luminous intensity candela cd


• Some Prefixes for Multiples of SI Units.Factor Prefix Symbol

1,000,000,000 = 109 giga G1,000,000 = 106 mega M

1,000 = 103 kilo k100 = 102 hecto h10 = 101 deka da0.1 = 10-1 deci d

0.01 = 10-2 centi c0.001 = 10-3 milli m

0.000,001 = 10-6 micro µ0.000,000,001 = 10-9 nano n

0.000,000,000,001 = 10-12 pico p


• Some Derived Quantities.

Quantity Definition Derived Unit (Name)Area Length times length m2

Volume Area times length m3

Density Mass per unit volume kg/m3

Speed Distance per unit time m/sAcceleration Change in speed per unit time m/s2

Force Mass times acceleration (kg·m)/s2 (newton, N)Pressure Force per unit area kg/(m·s2) (pascal, Pa)Energy Force times distance (kg·m2)/s2 (joule, J)


• Density relates the mass of an object to its volume.

• Density decreases as a substance is heated because the substance’s volume increases.

• Knowing the density of a substance allows measurements in volume to be recorded in mass.


• Densities of Some Common Materials.

Substance Density (g/cm3) Substance Density (g/cm3)Ice (0.0°C) 0.917 Human Fat 0.94

Water (4.0°C) 1.0000 Cork 0.22–0.26Gold 19.31 Table Sugar 1.59

Helium (25.0°C) 0.000164 Balsa Wood 0.12Air (25.0°C) 0.001185 Earth 5.54


• What is the density of glass (in grams per cubic centimeter) if a sample weighing 26.43 g has a volume of 12.40 cm3?

• Chloroform, a substance once used as an anesthetic, has a density of 1.483 g/mL at 20°C. How many mL would you use if you needed 9.37 g?


• Temperature Conversions:• The Kelvin and Celsius

degree are essentially

the same because both

are one hundredth of the

interval between freezing

and boiling points of water.


• Temperature Conversions:• Celsius (°C) — Kelvin temperature conversion:

Kelvin (K) = °C + 273.15

• Fahrenheit (°F) — Celsius temperature conversions:

°C =

59

(°F − 32) °F =95

°C

+ 32


• Carry out the indicated temperature conversions:

(a) –78°C = ? K

(b) 158°C = ? °F

(c) 375 K = ? °C

(d) 98.6°F = ? °C

(e) 98.6°F = ? K


• Dimensional-Analysis method uses a conversion factor to express the relationship between units.

Original Quantity × ConversionFactor = Equivalent Quantity

Example: Express 2.50 kg in lb.ConversionFactor: 1.00 kg = 2.205 lb arranged as 2.205 lb

1.00 kg∴ 2.50 kg × 2.205 lb

1.00 kg = 6.00 lb (correct to 3 significant figures)


• The volcanic explosion that destroyed Krakatau on

August 17, 1883, released an estimated 4.3 cubic

miles (mi3) of debris into the atmosphere. In SI

units, how many cubic meters (m3) were released?


• How many meters are there in a marathon race

(26 miles and 385 yd)?

• How large, in cubic centimeters, is the volume of a

red blood cell if the cell has a circular shape with a

diameter of 6.0 x 10–6 m and a height of 2.0 x 10–6 m?

Accuracy, Precision, and Significant Figures in Measurement 01Accuracy, Precision, and Significant Figures in Measurement 01

• Accuracy is how close to the true value a given measurement is.

• Precision is how well a number of independent measurements agree with one another.


• Significant Figures are the total number of digits in the measurement.

• The results of calculations are only as reliable as the least precise measurement.

• Rules exist to govern the use of significant figures after the measurements have been made.


• Rules for Significant Figures:• Zeros in the middle of a number are significant

• Zeros at the beginning of a number are not significant

• Zeros at the end of a number and following a period are

significant

• Zeros at the end of a number and before a period may or

may not be significant.


• Rules for Calculating Numbers:• During multiplication or division, the answer can’t

have more sig figs than any of the original numbers.

• During addition or subtraction, the answer can’t have

more digits to the right of the decimal point than any

of the original numbers.


• Rules for Rounding Numbers:• If the first digit removed is less than 5 - round down

• If the first digit removed is greater than 5 - round up

• If the first digit removed is 5 and following numbers

are nonzero - round up

• If the first digit removed is 5 and following numbers

are zero - round down


• How many significant figures does each of the

following measurements have?

(a) 0.036653 m (b) 7.2100 x 10–3 g

(c) 72,100 km (d) $25.03


• Round off each of the following measurements.

(a) 3.774499 L to four significant figures

(b) 255.0974 K to three significant figures

(c) 55.265 kg to four significant figures

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