PSAE Chemistry Review Part 2. Electrons Available for Bonding Are called __________ __________ The Electrons in the Outermost energy level Nucleus _______________.

PSAEPSAEChemistry Review Chemistry Review

Part 2Part 2

Electrons Available for BondingElectrons Available for BondingAre called __________ __________Are called __________ __________

The Electrons in the Outermost energy levelThe Electrons in the Outermost energy level

Nucleus

______________

________________

Slide 2

Electrons Available for Bonding

Table Type #1: ROMAN NUMERALS

Slide 3

Electrons Available for BondingHow Many Valence Electrons does each Element Have?

Use the ___________ ___________ at the top of each Column.

The Group Number tells you how Many Valence Electrons.

Group Numbers

Slide 4

Electrons Available for Bonding

Table Type #2: Groups Numbered 1 thru 18

1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18

Slide 5

Electrons Available for BondingHow Many Valence Electrons does each Element Have?

1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18

Slide 6

_________________: The Number tells you the # of ValenceElectrons.

Groups _______________: Subtract ________ from the Group Number.

The Remainder is the # of Valence Electrons.

How much does an Atom Weigh?

Electron Cloud

is_____________________________________

Almost______________________ of an Atom is in the Nucleus.

Even though the Nucleus is only a very small part of the Atom

Slide 7

How much does an Atom Weigh?

12

CCarbon

12.011

________ _________•Equals the # of Protons

&

•Equals the # of Electrons

___________________

•Average Mass of all known _______________

Slide 8

How much does an Atom Weigh?Isotopes: Atoms of an element that have

_____________ _____________.

WHY do they have Different Masses?

Because of a Different Number of ____________.

Particle Mass (amu)

Proton 1

Neutron 1

Electron 0

Slide 9

Note: Almost ALL of the Mass is in the Protons and Neutrons.

How much does an Atom Weigh?

Isotope Notation

C126

Mass Number

Includes: # of ____________&

# of _____________Atomic Number

# of _________________

# Neutrons = Mass Number Atomic Number

Slide 10

How much does an Atom Weigh?Examples of Isotopes

Carbon has three Isotopes:

They are all carbon atoms, but with different numbers of Neutrons

C__6C__

6 C__6

Carbon – 13

___Neutrons

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Carbon – 14

___NeutronsCarbon – 14

___Neutrons

TransUranium Elements

•________________________ not found in Nature

•Made by Smashing Different Atoms together with

• _____________ Accelerators

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States of Matter

__________________ ________

Slide 13

States of Matter• Retains a ____________________________

•rigid - particles locked into place • Not easily ____________________________

•little free space between particles • Does not _____________________________

•rigid - particles cannot move/slide past one another

SOLID

Slide 14

States of Matter

LIQUID

• Assumes _________________ of the part of the_________________ which it occupies•particles can move/slide past one another

• Not easily _____________________ •little free space between particles

• Flows ________________________•particles can move/slide past one another

Slide 15

States of Matter

•Assumes _____________ and volume of its container

•particles can move past one another • ___________________

•lots of free space between particles

•Flows ________________•particles can move past one another

GAS

Slide 16

States of Matter• The word "PLASMA" was first applied to _________________. • Plasma consists of a collection of _______________________ electrons and ions - atoms that have lost electrons.• Energy is needed to strip electrons from atoms to make plasma.

PLASMA

Slide 17

Phase Changesa.k.a. CHANGES OF STATE

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_______________

___________________ __________________

______________

__________________

____________________

Phase Change Diagrams

Time

Solid Changing to Liquid

_____________

Solid

Te

mp

era

ture

Liquid

Gas

_____________

Temperature Remains _____________ During Phase Changes

No Solid Remaining

Liquid Changing To Gas

No G

as Rem

aining

*Temp Increasing

Slide 19

Phase Change Diagrams

Time

Liquid Changing To Solid

______________

Solid

Te

mp

era

ture

Liquid

Gas

_____________

Temperature Remains _____________ During Phase Changes

Gas Changing To Liquid

*Temp Decreasing

Slide 20

Kinetic Molecular Theory _________________________________

________ Kinds of Motion

Translation – __________________ from point A to point B.

Rotation – _______________ or _______________

Vibration – ____________ and Forth Movement

Gases are in Constant Random Motion

G:\STUFF\visualizingmolecular.mov

G:\STUFF\visualizingmolecularmotion.mov

Visualizing Molecular Motion

1 Video

Visualizing Molecular Motion

(Many) Video

G:\STUFF\diffusionofagas.mov

Diffusion of Gases Video

Slide 21

Gas LawsPressure is defined as The Force per Unit Area on a Surface

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___ N/cm2 ___ N/cm2 ___ N/cm2

Gas LawsPressure is defined as The Force per Unit Area on a Surface

Gas Molecules exert pressure on any surface with which they collide.

The More Gas Molecules in a Container – the Higher the Pressure.

Ex. Double the # of Particles – ___________________

1.0 atm 2.0 atmSlide 23

Gas LawsThe More Gas Molecules in a Container – the

________________ This is a Direct Relationship. (Directly Proportional)

# of Particles (moles)

Pre

ssu

re (

atm

)

Volume Must be Held Constant

Slide 24

Gas LawsBoyle’s Law: _____________________

Slide 25

Gas LawsBoyle’s Law: P x V = Constant

When Pressure _______________ – Volume Decreases

When Volume Increases – Pressure ________________

This is an Inversely Proportional Relationship

Slide 26

Temperature Must be Held Constant

Gas LawsCharles’s Law: V T = Constant

When Temperature Increases – Volume Increases

This is a Direct Relationship. (Directly Proportional)

Vo

lum

e (L

ite

rs)

Temperature CSlide 27

Pressure Must be Held Constant

Gas LawsGay-Lussac’s Law: _________________

When Temperature Increases – Pressure _______________

This is a Direct Relationship. (Directly Proportional)

Pre

ssu

re (

atm

)

Temperature CSlide 28

Volume Must be Held Constant

Gas Laws STP

Standard _______________ & ____________

Standard Temperature: ____ Degrees Celsius ( 0 C )

Standard Pressure: _____________________ ( 1 atm)

Slide 29

Gas Laws Temperature

Temperature: a measure of the Average Kinetic Energies of All Molecules in a Sample

Converting From Celsius Scale To Kelvin Scale Degrees Celsius(C ) + 273 = Kelvins (K)

Ex: _____________________________ Converting From Kelvin Scale To Celsius Scale

Kelvins (K) – 273 = Degrees Celsius (C )

Ex: _____________________________

Note: The Kelvin Temperature is ALWAYS HIGHER !

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