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Matter, Energy, Measurement and Atoms

Emannuel Ramli, PhD, CPIM

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1-2Emannuel Ramli, PhD, CPIM

Textbook

Frederick A. Bettelheim

William H. Brown

Mary K. Campbell

Shawn O. Farrell

www.cengage.com/chemistry/bettelheim

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Matter

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Measurement

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Mass and WeightWeight is affected by gravity.

Weight is measured in Newton.Earth gravity = 9.81 m/s2

Moon gravity = 1.63 m/s2

Weight = mass x acceleration

(Force = mass x acceleration)

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Mass and Density

Example:Example: If 73.2 mL of a liquid has a mass of 61.5 g, whatis its density in g/mL?

d=m d= densitym = mass

V = volumeV

d= mV

= 61.5 g

73.2 mL= 0.840 g/mL

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Density and Specific Gravity

Example:Example: The density of copper at 20C is 8.92 g/mL. Thedensity of water at this temperature is 1.00 g/mL. What is

the specific gravity of copper?

= 8.928.92 g/mL

1.00 g/mLSpecific gravity =

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Specific Gravity

Urinometer its a Hydrometer

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Energy

Kinetic Energy is the energy of motion

Potential Energy is stored energy

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Temperature

oC = 5/9 (oF - 32)

oC = K 273

0 K is absolute zero(its the lowest possible temperature)

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Temperature and Heat

Heat is a form of energy

Heat accompanies chemical reactions

Heat is usually measured in calorie (cal) or joule (J)

1 cal = 4.184 J

It takes 1 cal to raise temperature of 1 g of water by 1 oC

Temperature is not a form of energy

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Temperature and Heat

50 kJ of

Heat

50 kJ of

Heat

T = 50 oC

Warm

T = 95 oC

Hot

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Heat and Specific Heat

Specific Heat is the amount of heat needed to raise the

temperature of 1 g of any substance by 1 oC

Each substance has its own unique Specific Heat

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Specific Heat

Example:Example: How many calories are required to heat 352 gof water from 23C to 95C?

Amoun t of h t. l

Cx 35 x ( 5 - 3)C

.5 x4

l 5 k l

Amount of h t s f h t x mass x hange n temperature

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1. Nonzero digits are always significantE.g. 233.1 has four significant figures; 2.3 g has two.

2. Zeros at the beginning of a number are never significant

E.g. 0.0055 L has two significant figures.

3. Zeros at the end of a number that contains a decimal point arealways significant

E.g. 3.00 L has three significant figures; 0.0450 mm has three.

4. Zeros at the end of number that contains no decimal point may or

may not be significantE.g. How many significant figures does 2500 g have?

2.5 x 103 g has two significant figures

2.500 x 103 g has four significant figures.

Significant Figures

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Conversion factorConversion factor::A ratio of two different units, used as amultiplier to change from one system or unit to another.

Example:Example: Convert 381 grams to pounds.

ExampleExample:: Convert 1.844 gallons to milliliters.

3 g x lb453.6 g = . 4 lb

. 44 gal x 3.7 5gal

x . = 6 .

Factor-Label Method

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Atoms

1 amu = 1.6605 x 10-24 g

Subatom c

partic

Mass

g)Charg

Locationin

anatom

Proton

Electron

Neutron

1.6726 x 10 -24

9.1094 x 10 -28

1.6749 x 10 -24

1

0.0005

1

+1

-1

0

Insidethenucleus

Outsidethenucleus

Insidethenucleus

1.0073

1.0087

5.4859 x 10 -4

Mass (amu)Mass (amu)

(1 sig. fig.)

Mass number:Mass number: The number of protons and neutrons in the nucleus of an atom.

(The mass of the electrons in an atom is so small compared to that of its protons

and neutrons that electrons are not counted in determining mass number.)

Atomic number:Atomic number: The number of protons in the nucleus of an atom.

Massnumber (numberofprotons & neutrons)

Atomic number (numberofprotons) 6

12 C

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Atoms

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Isotopes

Isotopes:Isotopes:Atoms with the same number of protons but adifferent number of neutrons.

Carbon-12 has 6 protons and 6 neutrons



Most elements found on Earth are mixtures of isotopes.

Chlorine is 75.77% chlorine-35 (18 neutrons) and 24.23%chlorine-37 (20 neutrons).

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Atomic Weights

Atomic weight:Atomic weight: The weighted average of the masses(in amu) of the naturally occurring isotopes of an element.

Example: Chlorine is 75.77% chlorine-35 and 24.23%

chlorine-37

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The Periodic Table

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Electron Configurations

Electron configuration:Electron configuration: The arrangement of electrons inthe extra-nuclear space.

T

he energy of electrons in an atom is quantizedquantized, whichmeans that an electron in an atom can have only certainallowed energies.

GroundGround--state electron configuration:state electron configuration:T

he electronconfiguration of the lowest energy state of an atom.

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1s, 2s, and 2p Orbitals

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Electron Spins

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Distribution of Electrons

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Ground State Electron Configurations

Carbon

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Oxygen

Ground State Electron Configurations

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The Periodic Table and Orbitals

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Valence Electrons & Lewis Structures

Valence shell:Valence shell: The outermost incomplete shell.

Valence electron:Valence electron:An electron in the valence shell.

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Valence Electrons & Lewis Structures

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End of Module

er bio103 201008 week 1

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