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TKU 3023
Information and Communication
Technology In Chemistry
Simulation
Title : Atomic structure
Group A
Group member
Name Matrix No.
Nadiatul Azima Bt Ahmad Sabri D20081032358
Norhadisah Bt Mohd. Zaini D20081032367
Lecturers Name:Pn. Asmayati
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Contents
1. Introduction..2
2. Engage...4
3. Empower...5
4. Enhance11
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ATOMIC STRUCTURE
Matter
Matter is everything that has mass and occupied spaces. It is made ofatoms and
molecules.
Atoms are the basic building blocks of matter. They are the smallest units of an element:
An element is composed of only one kind of atom
In compounds the atoms of two or more elements combine in definite
arrangements
Mixtures do not involve the specific interactions between elements found incompounds, and the elements which comprise the mixture can be of varying ratios
Theory of Matter
The atom is considered the basic unit of any element, and atoms may combine
chemically to form molecules.The molecule being the smallest unit of any
substance that possesses the properties of that substance. An element in moderntheory is any substance that have the same atomic number, while a compound is
composed of different types of atoms together in molecules.
State of matter
There are three states of matter which is solids, liquids, and gases.
Matter in the solid state has both a definite volume and a definite shape. Matter inthe liquid state has a definite volume but no definite shape, assuming the shape of
whatever container it is placed in. Matter in the gaseous state has neither adefinite volume nor a definite shape and expands to fill any container
Atomic Structure
Atoms are made up of 3 types of particles electrons , protons and
neutrons . These particles have different properties. Electrons are tiny,
very light particles that have a negative electrical charge (-). Protons are much
larger and heavier than electrons and have the opposite charge, protons have a
positive charge. Neutrons are large and heavy like protons, however neutrons
have no electrical charge. Each atom is made up of a combination of theseparticles.
Atoms have electrical charges. Some atoms can either gain or lose electrons (the
number of protons never changes in an atom). If an atom gains electrons, the
atom becomes negatively charged. If the atom loses electrons, the atom becomes
positively charged (because the number of positively charged protons will exceedthe number of electrons). An atom that carries an electrical charge is called an
ion.
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http://www.chem4kids.com/files/atom_intro.htmlhttp://www.infoplease.com/ce6/sci/A0805227.htmlhttp://www.infoplease.com/ce6/sci/A0833627.htmlhttp://www.infoplease.com/ce6/sci/A0817024.htmlhttp://www.infoplease.com/ce6/sci/A0805235.htmlhttp://www.chem4kids.com/files/atom_intro.htmlhttp://www.infoplease.com/ce6/sci/A0805227.htmlhttp://www.infoplease.com/ce6/sci/A0833627.htmlhttp://www.infoplease.com/ce6/sci/A0817024.htmlhttp://www.infoplease.com/ce6/sci/A0805235.html -
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Number of proton and nucleon number
The atomic number is also given the more descriptive name of proton number.
The mass number is also called the nucleon number
Isotopes
The number of neutrons in an atom can vary within small limits. For example,
there are three kinds of carbon atom 12C, 13C and 14C. They all have the samenumber of protons, but the number of neutrons varies.
protons neutrons mass number
carbon-12 6 6 12
carbon-13 6 7 13
carbon-14 6 8 14
These different atoms of carbon are called isotopes. Isotopes are atoms which
have the same atomic number but different mass numbers. They have the same
number of protons but different numbers of neutrons.
The arrangement of the electrons
The electrons are found at considerable distances from the nucleus in a series of
levels called energy levels. Each energy level can only hold a certain number of
electrons. The first level (nearest the nucleus) will only hold 2 electrons, the
second holds 8, and the third also seems to be full when it has 8 electrons.
These levels can be thought of as getting progressively further from the nucleus.
Electrons will always go into the lowest possible energy level
For example the arrangement of electron in Sodium,Na atoms:
ENGAGE
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No of proton= atomic number of the atom
No of proton + no of neutrons= mass number of the atom
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You are given the picture as shown below:
1. What do you observe?
2. What is the process occurs during the freezing
and melting the ice cube?
3. How could this happen?
EMPOWER
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Steps1. The Kinetic Theory explains the differences between the three states of matter.
2. The three states of matter are
Solid
Liquid
Gas3. See the video and observe the characteristic of each state of matter to answer the
question
State of matter (video 1)State of matter (video 2)
Result;Video 1
States of matter
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http://opt/scribd/conversion/tmp/scratch5/States%20of%20Matter.flvhttp://opt/scribd/conversion/tmp/scratch5/Chemistry%20Animation%20-%20States%20of%20Matter.flvhttp://opt/scribd/conversion/tmp/scratch5/States%20of%20Matter.flvhttp://opt/scribd/conversion/tmp/scratch5/Chemistry%20Animation%20-%20States%20of%20Matter.flv -
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Solid state
Video 2
The strength of forces that hold atoms at each states
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Compressibility at each states
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Questions
Complete the table below.
SOLID LIQUID GAS
Atomic
structure
Shape
Volume
Particlemovement
Force
Compressibility
Example
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Answer
SOLID LIQUID GAS
Atomicstructure
Shape Fixed shape No fixed shape: follow
the shape of container
No fixed shape: follow
the shape of container
Volume Fixed volume Fixed volume No fixed volume
Particle
movement
Collide only with
near neighbour
Move randomly but
limited
Move rapidly and
randomly
Attractions
Force
Strong
intermolecular forces
Normal intermolecular
forces
No intermolecular
forces
Bonds Strong bonds Weak bonds No bonds
Compressibility Cannot compress;
particle closelypacked and no space
Can be compress; have
space between atoms
Maximum
compression: lot ofempty space between
atoms
Example Sugar, wood Milk, water Oxygen, Nitrogen
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d)
e)
f)
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g)
h)
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