The Periodic Table Introduction Mendeleev’s Periodic Table Dmitri Mendeleev.
Periodic Table Periodic Table- An arrangement of elements in columns based on properties that repeat...
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Transcript of Periodic Table Periodic Table- An arrangement of elements in columns based on properties that repeat...
Periodic Table- An arrangement of elements in columns based on properties that repeat from row to row.– First organized by Dimitri Mendeleev,
modeled after the card game solitaire– Elements were arranged into rows by
increasing mass– Similar properties were placed in the same
column
Today’s periodic table is arranged by atomic number–The atomic number increases as you move left to right
–PERIOD - rows across–GROUP – columns up & down
Review - ELEMENTS
Can not be chemically broken down into simpler substances
Arranged into 3 groups on table:
metals, metalloids, non- metals
From left to right on the table elements become less like metals
METALS
good conductors of electricity and heat, usually solid at room temperature, malleable, reactive
Blue elements on YOUR table–TRANSITION METALS – special
group of metals found in the middle section of the table, (groups 3-12)
METALLOIDS
Properties are in between the properties of metals and non- metals
All elements that share a border on the “Staircase” on your table
Non- Metals
Poor conductors. Can be solid liquid or gas at room temperature, not reactive
Red elements on YOUR table
Matter
The term matter describes all of the physical substances around us
Matter is anything that has mass and takes up space
The Universe is made up of matter and energy
*Matter is made up of atoms.*An atom is the smallest whole particle of matter. Atoms are the building blocks of matter.* Sub-Atomic particles are the tiny particles that make up an atom.
Atomic Structure
Proton (p+)
Located in the nucleus of the atom
Protons have a positive charge (+)
Much larger and heavier than electrons
Number of protons is different for each element. If the number of protons changes, the element changes.
Atomic Structure
Neutron (n0)
Located in the nucleus of the atom
Neutral particle (has no electrical charge)
Largest particle, a bit bigger than a proton
Atomic Structure
Electron (e-)
Found in a cloud outside the nucleus
Electrons have a negative charge (-)
Smallest particle
Orbit nucleus on energy levels
Atomic Number = number of protons in each atom of any element
All atoms want to balance their protons and electrons to be NEUTRAL (no electrical charge)
In a neutral atom, the # of protons = the # of electrons
Element Atomic # # protons
Hydrogen 1 1
Gold 79 79
Oxygen 8
Iron 26 26
Lead 82
Helium 2
Sodium 11 11
Sulfur 16
Atomic Mass– the sum of the mass of all the protons and neutrons in an atom
-- measured in Atomic Mass Units (amu)
Mass Number – sum of protons and neutrons in the nucleus
--can be used to find the number of neutrons in the nucleus Mass # = atomic # + n or n = mass # - p
ATOMIC NUMBER
the number of (p+) and (e-)
(+) = (-)
ATOMIC MASS
(MASS NUMBER)
PROTONS (+) + NEUTRONS (0)
PROTONS AND NEUTRONS = NUCLEUS
79
Au
19
7
Isotope – when an atom has a different number of neutrons than other atoms of the same element–Example: 2 Oxygen Atoms,
one has 8 neutrons one has 9.
IsotopesThe number of protons for a given atom never changes.
The number of neutrons can change.
Two atoms with different numbers of neutrons are called isotopes
Isotopes have the same atomic #
Isotopes have different atomic Mass #’s
ElectronsElectrons can be found in the electron cloud.
Energy Levels – electrons are located on these levels based on their energy
•The lowest energy level is closest to the nucleus--It holds 2 e-•The 2nd energy level holds 8 e-
•The 3rd energy level holds 8 e-
•ELECTRONS FILL THE LEVELS FROM INSIDE OUT.
Electrons can change levels when energy is added to or removed from the atom–If an e- gains energy it is in
“excited state” and moves out an energy level
–If it loses energy it goes in an energy level
Valence Electrons - Number of electrons in outside row– Identified with a Roman numeral number at
the top of each group– All elements in each group have the same
number– Column VIII (group 18) has 2, 8 or 18 – it
is FILLED!– Transition metals have no specific roman
numeral
2.
The roman numeral columns tell you how many electrons an atom has currently in its outside level.
3.
THE SUBATOMIC PARTICLES ARE:
ELECTRONS (-) NEGATIVE electrical
charge
PROTONS (+) POSITIVE electrical
charge
NEUTRONS (0) NO electrical
charge
5.
79 ATOMIC NUMBER
Au (the number of (p+) and (e-) )
197 (+) = (-)
6. ATOMIC MASS
PROTONS (+) + NEUTRONS (0)
**don’t forget, protons and neutrons are in the nucleus!