Quantum Numbers

Quantum Numbers

In solving quantum numbers we always should always use specific representations for determining the quantum numbers of an electron. These specific representations are n, l, ml, ms.

Principal quantum numbers

•  Represented by “n”.
• You can identify it by looking at the energy level or shell where the last electron of a specific element is located.

For example: 2p⁶, the principal quantum number is 2 because 2p⁶ is located at the 2^nd shell.

Azimuthal Quantum number

• represented by “l”.
• You can identify it by looking at the subshell. Subshells are the s, p, d and f from the electron configuration.

The subshells have different kinds of shapes.

S is a sphere shaped area, 

P is a dumbbell shaped area, 

D is a clover shaped area, and 

F is a fundamental shaped area. 

• We also have representations for subshells s, p, d and f when looking for the azimuthal quantum number.

s= 0

p= 1

d= 2

f= 3

For example: 2p⁶, its subshell is p and therefore its azimuthal quantum number is 1.

The magnetic quantum number

• Represented by “ml”.
• It is somehow connected with the azimuthal quantum number.
• You can identify it by looking at the compartment of the element. Every subshell has different numbers of compartments.

                      S= 1 compartment,

                      P= 3 compartments  

                      D= 5 compartments

                     F=  7 compartments

• The center of the compartment is always zero, so if you’re going to look at the left side it means that it is negative and if you are going to look at the right side it means that it is positive.

For example: 2p⁶, its magnetic quantum number is 1 because the 6^th electron of 2p⁶ is located at the 3^rd compartment.

Magnetic Spin

•  The representation for magnetic spin is “ms”.
• Inside of every compartment, there are 2 arrows but their direction is opposite:

               

1.  Upwards which means that arrow is going to a clockwise direction and it denotes +1/2 or having a positive spin.
2. Downwards which means that arrow is going to a counter clockwise direction and it denotes -1/2 or having a negative spin.

• These 2 spins are called magnetic spins

Example for this quantum number: 2p⁶, the magnetic spin of it is -1/2 because the last arrow is going to a counter clockwise direction. 

Scientific Measurements

Measurement

-Process of comparing an object’s physical quantities using a standard measuring device.

-It involves numbers accompanied by the appropriate unit of measurement.

Units of Measurement

-Identifies the physical quantity being measured by the measuring device.

All systems of weights measure, metric and non-metric, are linked through a network of International System is called the SI, using the first two initials of its French name Systeme Intenational d'Unites. 

S.I Base Units

Physical Quantity

• Length (m)
• Mass (kg)
• Time (s)
• Amount of Substance (mol)
• Thermodynamic Temperature (K)
• Electric Current (A)
• Luminous Intensity (cd)

Non - S.I. Base Units

• Time(min, hr, d)
• Volume (L, ml)
• Density (g, ml)
• Thermodynamic Temperature
• Pressure (C)
• Energy

Calibrations

-Lines and number found on a measuring device that represents place values.

-Each segment ID divided into 10 equal parts and was patterned after the metric system of measurement.

Accuracy 

-Place value usually represented by the smallest lines on the measuring device and is the smallest value represented by the measuring device's calibration.

Sensitivity

-The estimates, approximated place value after accuracy.

Place Values

-In our decimal number system, the value of a digit depends on its place, or position, in the number. Each has a value of 10 times the place to its right.

Number in standard form is separated into groups of three digits using commas. Each of these groups is called period.

Numbers, such as 84, have two digits. Each digit is a different place value.

The left digit is the tens' place. It tells you that there are 8 tens.

The last or right is the ones' place which is 4 in this example. Therefore, there are 8 sets of 10, plus 4 ones in the number 84.

            8  4

            |  |_____ ones' place

            | __________ tens' place

http://www.aaaknow.com/plc12ax2.htm
http://www.math.com/school/subject1/lessons/S1U1L1GL.html#sm1 

 



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CHEMISTRY: Aspects of Matter

                Chemistry or also known as “The Central Science” is the study of Matter and the changes it undergoes.

                 Matter is anything made of atoms and molecules and is anything that has Mass, a property that reflects the quantity of Matter in a sample.

States of Matter

SOLID

                The molecules are closely bound to one another by molecular forces. The particles are packed closely together. It has a stable, definite shape, and a definite volume. It can only change their shape by force, as when broken or cut.

LIQUID

                The molecular forces are weaker than in a Solid. It will take the shape of its container with a free surface in a gravitational field. It has a fixed volume. It also occupies a shape or volume nut assumes the shape of the occupied portion of its container.

GAS

                                          The molecular forces are very weak and it has no definite shape or volume, but occupies the entire container in which it is confined. It expands to fill completely whatever container it occupies. 

 Examples:

Heterogeneous

Homogeneous

History of Chemistry

I. Discovery
        2500 years ago, were perhaps the first to formulate rational theories of chemistry-explanations of the behavior of the matter     they generally did not test their theories by experimentation.
        The experimental roots of chemistry are planted in alchemy, a mystical mixture of chemistry and magic that flourished in Europe during the Middle Ages from about 500 to 1500 CE
 Modern day chemists inherited from the alchemists an abiding interest in human health and quality of life.  

II. The Four Elements
            The Greek philosopher Empedocles, a native of Sicily, introduces a theory which will be accepted in Europe until the 17th century. He states that all matter is made up, in differing proportions, of four elemental substances - earth, air, fire and water. Not until the arrival of a 'skeptical chemist' (the title of a book by Robert Boyle in 1661) is there a serious threat to this Greek theory of the elements.

ASPECTS OF MATTER

§        Structure

-  arrangement of atoms in a molecule

§        Composition

-  what a molecule is made of

§        Properties

          -  unique characteristics of an object

              ex: H₂O - clear

           -  boils at 100 degrees Celsius

           -  freezes at 0 degree Celsius

§        Changes

-  to alter

§        Principles and laws

-   logical explanation of events that occur in nature supported by results

    of repeated experiments

      ex: Law of conservation of mass

§        Application

          -    process of testing the data

          -    identification of use

                ex: Penialin: fighting bacteria

BRANCHES OF CHEMISTRY

   Organic Chemistry

           -   carbon containing compounds

           -   H, N, O, P, S

                ex: Ethyl Alcohol  CH₃ - CH₂ - O - H

           -   study of compounds produced by living organism

                

    Inorganic Chemistry

           -   deals with elements or compounds other than carbon

                ex: NaCl - table salt

                    H₂O - water

                    NH₃ - anomia

    Physical Chemistry

    -   math / physics

    -   theories / behavior

    -   why? / how?

       ex: How fast will the reaction occur?

    Analytical Chemistry

    -   identifies what substance is present

    -   how much is there

   a.) Qualitative                                                   b.) Quantitative

      - what?                                                              - how much?

      - descriptive                                                      - numerical

       

  Biochemistry

  -   chemistry of living organisms

  -   processes in the body

       ex: Digestion, Excretion , Metabolism , Amino Acids(glycine)


TRY THIS!
1.)Give at least 5 examples of matter.
2.)Differentiate element from a compound.
3.)Give 5 examples of heterogeneous and homogeneous mixtures.
4.)What branch of chemistry deals with elements or compounds other than carbon?
5.)What branch of chemistry identifies what substance is present?
6.)Is Air an example of homogeneous mixture?
7.)What do you call the change in the phase of gas to liquid?
8.)What do you call the change in the phase of liquid to solid?
9.)What are the two types of Pure Substance?
10.)What is the state of matter wherein particles are closely together?
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ANSWERS!
4.)Inorganic Chemistry
5.)Analytical Chemistry
6.)Air is a homogenous mixture because you can't distinguish between the substances.
7.)Condensation
8.)Sodification
9.)Element and Compound
10.)Solid

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