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Electrons and the Periodic TableMrs. Freeman
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History• HOW WAS MENDELEEV’S PERIODIC TABLE
ARRANGED? ▫By their chemical properties
• HOW IS THE MODERN PERIODIC TABLE ARRANGED?▫By increasing number of protons and atomic
mass.• WHY DIDN’T MENDELEEV ARRANGE HIS
TABLE THIS WAY?▫Because at the time the number of protons was
not known.
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PERIODS: are a horizontal row of elements.•HOW MANY: 7•VARIATION ACROSS A PERIOD:
Changes from metals to metalloids to nonmetals
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GROUPS AKA FAMILIES: the individual columns of elements.•HOW MANY?
▫18•SIMILARITIES BETWEEN ELEMENTS
IN THE SAME GROUP?▫They have the same number of valence
electrons
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THREE CLASSES OR CATEGORIES OF ELEMENTS ON THE PERIODIC TABLE
METALS NONMETALS METALLOIDS
LOCATION Left side of the stair step line
Right side of the stair step line
Along the stair step line
EXAMPLES AND USES
Zinc-vitamins and certain containers.
Potassium-in bananas for cells to use
Oxygen-gas to breathe
Carbon-foundation for life.
Aluminum- cans, canisters, cars.
Silicon-sealant against water
PROPERTIES Hard, malleable, durable, rust, dense
Not dense, colorless,
Has properties of both metals and non-metals.
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REACTIVITY PATTERN WITHIN A GROUP: increasing reactivity, decreasing melting and boiling point and density generally increases,
•Left side of the table
Metals
•Right side of the table
Nonmetals
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ALKALI METALS
ALKALINE EARTH METALS
BORON FAMILY
CARBON FAMILY
NITROGEN FAMILY
OXYGEN FAMILY
HALOGENS
NOBLE GASES
GROUP # 1 2 13 14 15 16 17 18LIST OF ELEMENTS IN GROUP
HydrogenLithiumSodiumPotassiumRubidiumCesiumFrancium
BerylliumMagnesiumCalciumStrontiumBariumRadium
BoronAluminumGalliumIndiumThallium
CarbonSiliconGermaniumTinLead
NitrogenPhosphorusArsenicAntimonyBismuth
OxygenSulfurSeleniumTelluriumPolonium
FluorineChlorineBromineIodineAstatine
HeliumNeonArgonKryptonXenonRadon
# of valence electrons
1 2 3 4 5 6 7 8
Key Facts
Prop. AndReactivity
Uses
Are very reactive.
Form Ionic CompoundsMetal
Ex. Salt
React with halogens well.
Form ionic compounds.Metal
Ex. Magnesium chloride
Forms covalent compounds
Non-metals
Boron is metalloid.
Forms both covalent and ionic bonds.
2 metals and 2 metalloids
Forms covalent bonds.
Non-metals
Basis for fertilizer
Forms covalent and ionic bonds.
Most abundant elements in earths crust.
All are non-metals.
Form ionic compounds.
Most reactive group.
Inert-do not react
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•THE MOST REACTIVE METALS: ▫Francium, Cesium, and Rubidium (in order
from most reactive to least reactive)•THE MOST REACTIVE NONMETALS:
▫Fluorine, Chlorine, and Bromine (in order from most reactive to least reactive)
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Excited electron-
•an electron in an energy level higher than its ground state (it has absorbed energy)
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Ground state-
•all the electrons have the lowest possible energy.
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Energy Level-
•The possible energies that electrons in an atom can have.
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Sub-level
•Electron orbital designated s, p, d or f. •These sublevels or orbitals have
characteristic shapes which can be used to explain and predict the chemical bonds that atoms can form.
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Orbital-
•the region of space around the nucleus where an electron is likely to be found.
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Energy level/energy shell-
•the possible energies that electrons in an atom can have.
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Three ways to show arrangements of electrons
•Orbital Configuration Notation•Electron Configuration Notation•Electron Dot Notation
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Electron configuration-
•specific distribution of electrons in atomic orbitals of atoms or ions.
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Valence shell-
•the outside energy shell
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Valence electrons-
•an electron that is in the highest energy level of an atom.
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Orbital Configuration Notation•each electron is assigned a space with an
up spin or a down spin.•All up spins must be placed first.•Then place all down spins until all
electrons are used.
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Electron configuration notation:•is just the letters and numbers from the
orbital configuration.•Example: Ar= 1s2 2s2 2p6 3s2 3p6
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Electron dot notation:
•the valence electrons represented by dots around the element symbol.
• -fill in using the house memory trick
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Hund’s Rule
•every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.
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Aufbau Principle:
•is used to determine the electron configuration of an atom, molecule or ion. The principle postulates a hypothetical process in which an atom is "built up" by progressively adding electrons.
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Pauli’s Exclusion Principal
•“no two electrons in the same atom can be in the same quantum state.” [1] This means that no two electrons can have the same set of quantum states of: 1) energy, 2) angular momentum magnitude, 3) angular momentum orientation, and 4) orientation of intrinsic spin.
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Assessment
• LIST THE PERIOD TO WHICH EACH OF THE FOLLOWING BELONGS:▫STRONTIUM:
5 ▫ IRON:
4 ▫RADON:
6 ▫ANTIMONY:
5• HOW MANY ELEMENTS ARE IN PERIOD 4?
▫18 • HOW MANY ELEMENTS ARE IN PERIOD 6?
▫32
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Assessment:
•NAME THE ELEMENT IN GROUP 3 PERIOD 4 ▫Scandium.
•HOW MANY VALENCE ELECTRONS ARE IN AN ATOM OF FLUORINE? ▫7
•TO WHAT GROUP DOES CARBON BELONG ▫14