Periodic Table of Elements
By: Suad, Khadija & Sahra
Reviewing the Atom...
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The first official discovery of the atom was by Dalton who came up with a atomic theory which stated:
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All elements are composed of tiny indivisible particles
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Atoms of the same element are identical. The atoms of any one element are different
from those of any other element
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Atoms of different elements can physically mix together or can chemically combine in simple wholenumber ratios to form compounds
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Chemical reactions occur when atoms are separated from each other, joined, or rearranged in a different
combination. Atoms of one element, however, are never changed into atoms of another element as a result
of a chemical reaction
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After Dalton a new explosion of studies around this area of chemistry erupted
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Schrodinger devised the quantum mechanical model
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Thomson discovered the electron, as well as isotopes.
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Rutherford discovered that there was a nucleus in atoms
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Bohr proposed that electrons had energy levels and that they revolved around the atomic nucleus but
electrons can jump from one energy level (or orbit) to another.
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Dobereiner organized elements into triads
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Mendeleev was known for creating the first version of the periodic table
Reviewing Atomic Make-up...
The atom is divided up into three parts which vary from element to element. The
neutrons added to the protons is called the mass number.
Protons
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a subatomic particle in an
Neutrons
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a subatomic particle found in
atom's nucleus, with a
the nucleus like proton but
positive electric charge
without an electric charge
Electrons
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negative electric charge
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They also determine an
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atom's atomic number
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Mass is that of 1 mass unit
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a subatomic particle with a
They help determine an
They help determine an
atom's ability to bond and
atom's isotope
location on the periodic table
Mass is that of 1 mass unit
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Mass is 1/1840 relative to the
mass of proton
Organizing the Periodic Table
There are many ways to organize the periodic table;
1. You can divide it up into Metals, Non Metals
and Metalloids (shown below)
2.
You can divide up the elements on the table
by Alkali Metals, Alkaline Earth Metal, Transitional
Metals, Inner Transitional Metals, Halogens, Metals, Non Metals,
Metalloids and Noble gases (shown right)
What Makes NOBLE GASES special
The noble gases are located in the far right of the periodic table and were previously
referred to as the "inert gases" due to the fact that their filled valence shells, making them
extremely unreactive. The elements in this group are helium (He), neon (Ne), argon (Ar),
krypton (Kr), xenon (Xe), and radon (Rn).
The ACTINIDE Period...
They are all radioactive and some are not found in nature. Some of the elements with
higher atomic numbers have only been made in labs. This atoms that are made in lab usually have
short life-spans. The elements from 99-103 are synthetic, and 89-98 are occur naturally from different
circumstances. The elements in this period include actinium (Ac), thorium (Th), protactinium (Pa),
uranium (U), neptunium (Np), plutonium (Pu) americium (Am), curium(Cm), berkelium (Bk),
californium (Ca), einsteinium (Es), fermium (Fm), mendelevium (Md), nobelium (No), lawrencium (Lr).
The LANTHANIDE Period...
Unlike Actinides, all the Lanthanides occur naturally in nature. The elements of this
section of the period table are lanthanum (La), Cerium (Ce), Praseodymium (Pr), Neodymium
(Nd), Promethium (Pm), Samarium (Sm), Europium (Eu), Gadolinium (Gd), Terbium (Tb),
Dysprosium (Dy), Holmium (Ho), Erbium (Er), Thulium (Tm), Ytterbium (Yb), and Lutetium (Lu)
What Make HALOGENS special
The halogens are located on the left of the noble gases on the periodic table. These five toxic,
non-metallic elements make up Group 17 of the periodic table and consist of: fluorine (F), chlorine
(Cl), bromine (Br), iodine (I), and astatine (At). Although astatine is radioactive it is often included in
the halogen group. Because the halogen elements have seven valence electrons, they only require
one additional electron to become “happy” atoms. This characteristic makes them more reactive than
other non-metal groups.
ALKALINE EARTH METAL Family
They are all shiny, silvery-white, somewhat reactive metals and are most likely gonna
lose their two outermost electrons to form cations with a positive charge. The alkaline earth metals
are beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra). They
are in the second group and therefore have 2 valence electrons. All the discovered alkaline earth
metals occur in nature.
ALKALI METALS Family
Alkali metals are among the most reactive metals. This is due in part to their larger atomic radii
and low ionization energies. They tend to donate their electrons in reactions a become positive
cation. The alkali metals include: lithium (Li), sodium (Na), potassium (K), rubidium (RB), cesium
(Cs), and francium (Fr), hydrogen (H)
Metals, Nonmetals & Metalloids
When you divide the Periodic Table into three general groups you come up with
Metals, Nonmetals and Metalloids
Metals
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Makes up 80% of the table. It
Nonmetals
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Is mostly found in the upper-
Metalloids
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The metalloids part of the
includes areas like the
right corner except for
periodic table is the stepping
transition metals and alkali
hydrogen which is on the left.
stair between the metals and
metals
Includes noble gases
nonmetals
Some notable qualities are
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Some notable qualities are
their sheen, conductibility,
that they the are poor
that their ductile and
conductors and most gases
malleable, metals are also
at room temp.
solid at room temp.
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Share qualities of both metals
and nonmetals
Important Terms to Know!
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Octet Rule- That when forming compounds, elements like to have similar electron configurations to
noble gases, which is to have eight electrons in their highest occupied shell
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Valence Electrons- Are the electrons in the highest occupied shell of an atom
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Cations- An ion with a positive charge
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Anion- An ion with a negative charge
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Ion- Is an atom or group of atoms that has a positive or negative charge. This is dependant on if the
electrons in an atom is equal to the protons in an atom
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Ionization Energy- The energy required an electron from an atom
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Electronegativity- Is the ability of an atom of an element to attract electrons when the atom is in a
compound
JOKES/RIDDLES
A. What do you do with a sick chemist?
B. Anyone know any jokes about sodium?
Answers
A.If you can't helium, and you can't curium,
then you might as well barium.
B.NA