The Atom and Periodic Table Physical Science. Element verse Atom ELEMENT – A substance that cannot...
-
Upload
linda-wiggins -
Category
Documents
-
view
223 -
download
0
Transcript of The Atom and Periodic Table Physical Science. Element verse Atom ELEMENT – A substance that cannot...
Element verse Atom
• ELEMENT– A substance that
cannot be broken down into simpler substances
– Ex: Neon, Gold, Helium
• ATOM– Smallest particle
of an element–Counting unit of
elements
History of the Atomic ModelDemocritus
--believed in the atom
John Dalton--made the theory on
atoms
J.J. Thomson--found the electron
Ernest Rutherford--found the nucleus
History of the Atomic Model
Neil Bohr--established energy
levels
Electron Cloud Model--the current model of
the atom
3 Subatomic ParticlesAtoms can be broken into:
• Protons–Positively charged– Symbol = p+
–Mass = 1
• Electrons–Negatively charged– Symbol = e-
– Extremely small mass
• Neutrons– No charged (neutral)– Symbol = n–Mass = 1
Parts of an Atom• Nucleus– Center of the atom– Small, dense,
positively charged– Where Protons and
Neutrons remain
• Energy Levels/Shells/Orbitals– Around the nucleus– Contains the electrons
Atomic Number
• The Identify of the element
• Number of Protons• Top of the Element
Block• SECRET: Also the
number of electrons
Mass Number
• The sum of the Protons and Neutrons
• Bottom Number of the element block
• Round to the Nearest Whole Number
Understanding an Element BlockATOMIC NUMBER
Element Symbol1st letter is upper case2nd letter is lower case
Element Name
Mass NUMBER
How do you Find Items
• Number of Protons = Atomic Number
• Number of Electrons = Number of Protons– (Because Atoms are neutral which means positive equals negative)
• Number of Neutrons = Mass Number subtract Atomic Number
Electron, Protons, Neutrons Example Practice
Name Symbol Atomic Number
Mass Number
Number of Protons
Number of Electrons
Number of Neutrons
NEON
BORON
ISOTOPES• Atoms of the same
element that have the same atomic number but different mass numbers
• # of protons stays the same
• # of neutrons change
How Isotopes are Written
• Elements name/symbol dash mass number• Ex:–Oxygen—16 p+= n =
–Oxygen—17 p+= n =
–O—18 p+= n =
Why is Mass Number a Decimal?• Mass Number is the
weighted average of all the isotopes of an atom
• The isotope whom mass number is closest to the actual mass number is more abundant
The Periodic Table• An arrangement of
elements in columns based on properties that repeat from row to row
• Modern Periodic Table arranged by Henry Moseley– Arranged by increasing
atomic number
Periods• 7 periods• Elements in the
same period have:–Same number of
energy levels or shells or orbitals
Groups• 18 groups• Elements in the
same group have the same:–Properties–Valence Electrons–Oxidation
Numbers
Valence Electrons• Number of electrons on
the outermost (last) energy level
• Code: – 1, 2, 3, 4, 5, 6, 7, 8
• Number next to “A” at the top of the column
Oxidation Number• Number of electrons an
atom will gain or lose to become stable
• Stable = 8 electrons on last shell
• Code:– +1, +2, +3, ±4, -3, -2, -1, 0
• “+” means lose electrons• “—” means gain electrons
Components of Bohr’s Model
Circles• Number of
Circles = Period Number = Number of Energy Level
DOTS• Go on the Last Circle• Number of Dots = Number
of Valence Electrons
• Important Note– First energy level has a max
of 2 electrons– All other energy levels have
a max of 8 electrons
Steps to Draw Bohr’s Model1. Place a dot to be
Nucleus
2. Place circles around Nucleus
3. Place dots on last circle in correct order
EXAMPLEOxygen
Electron Dot Diagrams• Model of an atom
in which each dot represents the valence electrons
• AKA: Lewis Dot Diagrams
Steps to Draw Dot Diagrams1. Identify the number of
valence electrons
2. Write the element’s symbol
3. Place dots around the symbol equal to valence electrons in correct order
ExampleNEON
Classifying Elements• Elements are
classified as metals, nonmetals, or metalloids based on properties and location on the periodic table
Metals• Most elements are them• Good Conductors of
electricity/heat• Solid at room
temperature (except Mercury)
• Ductile: turn into thin wire
• Luster: reflect light
• Malleable: hammer into sheets
• High Melting Point• Left side of the stair step• Francium: Most reactive
metal• High Boiling Point
Nonmetals• Dull• Brittle• Poor Conductors of
electricity/heat• Most are gas at room
temperature• Low Melting Point• Low Boiling Point• Right Side of Stair Step• Fluorine: most reactive
nonmetal
Metalloids• Have BOTH
characteristics of metals and nonmetals
• Found on the stair-step line
• What are the Metalloids–B, Si, Ge, As, Sb, Te, Po,
At
Periodic Trend• Reactivity–As you go left to
right across a period, the less reactive elements become
Alkali Metals• Group IA
• 1 valence electron
• Reactivity increases from top to bottom
• Francium is most reactive metal
Transitional Metals• THE MIDDLE OF THE
PERIODIC TABLE• Groups 3B-12B• Vary in oxidation
numbers• Brightly colored• Likes to combine
with Oxygen
The Halogens• Group VIIA
• 7 valence electrons
• Salt formers
• Reactive with metals
• Fluorine: most reactive nonmetal
Noble Gases• Group VIIIA
• 8 valence electrons
• Stable = not reactive
• Inert Gases
• All Shells are full