Unit 2 – Electrons and Periodic Behavior
Post on 03-Jan-2016
27 Views
Preview:
DESCRIPTION
Transcript
Unit 2 – Electrons Unit 2 – Electrons and Periodic and Periodic
BehaviorBehavior
Cartoon courtesy of NearingZero.net
Wave-Particle DualityWave-Particle DualityJJ Thomson won the Nobel prize for describing the electron as a particle.
His son, George Thomson won the Nobel prize for describing the wave-like nature of the electron.
The electron
is a particle!
The electron is an energy
wave!
The Wave-like ElectronThe Wave-like Electron
Louis deBroglie
The electron propagates through space as an energy
wave. To understand the atom, one must
understand the behavior of
electromagnetic waves.
…produces all of the colors in a continuous spectrum
Spectroscopic analysis of the visible Spectroscopic analysis of the visible spectrum…spectrum…
This produces bandsof light with definitewavelengths.
Electron Electron transitionstransitionsinvolve jumps of involve jumps of definite amounts definite amounts ofofenergy.energy.
Quantum NumbersQuantum Numbers
Each electron in an atom has a unique set of 4 quantum numbers which describe it.
Principal quantum number Angular momentum quantum number Magnetic quantum number Spin quantum number
Pauli Exclusion PrinciplePauli Exclusion Principle
No two electrons in an atom can have the same four quantum numbers.
Wolfgang Pauli
Principal Quantum NumberPrincipal Quantum NumberGenerally symbolized by n, it denotes the shell (energy level) in which the electron is located.
Number of electrons that can fit in a shell:
2n2
Angular Momentum Angular Momentum Quantum NumberQuantum Number
The angular momentum quantum number,
generally symbolized by l, denotes the orbital (subshell) in which the electron is located.
Magnetic Quantum NumberMagnetic Quantum NumberThe magnetic quantum number, generally symbolized by m, denotes the orientation of the electron’s orbital with respect to the three axes in space.
Assigning the NumbersAssigning the Numbers The three quantum numbers (n, l, and m) are integers. The principal quantum number (n) cannot be zero. n must be 1, 2, 3, etc. The angular momentum quantum number (l) can be any integer between 0 and n - 1. For n = 3, l can be either 0, 1, or 2. The magnetic quantum number (m) can be any integer between -l and +l. For l = 2, m can be either -2, -1, 0, +1, or +2.
Principle, angular momentum, and magnetic quantum Principle, angular momentum, and magnetic quantum numbers: numbers: nn, , ll, and , and mmll
Spin Quantum NumberSpin Quantum NumberSpin quantum number denotes the behavior (direction of spin) of an electron within a magnetic field.
Possibilities for electron spin:
1
2
1
2
Orbital shapes are defined as the surface that contains 90% of the total electron probability.
An orbital is a region within an atom where thereAn orbital is a region within an atom where thereis a probability of finding an electron. This is a is a probability of finding an electron. This is a probability diagram for the s orbital in the probability diagram for the s orbital in the first first energy level…energy level…
Orbitals of the same shape (s, for instance) grow larger as n increases…
Nodes are regions of low probability within an orbital.
Sizes of Sizes of ss orbitals orbitals
The s orbital has a spherical shape centered aroundthe origin of the three axes in space.
s orbital shape
There are three dumbbell-shaped p orbitals in each energy level above n = 1, each assigned to its own axis (x, y and z) in space.
PP orbital shape orbital shape
Things get a bit more complicated with the five d orbitals that are found in the d sublevels beginning with n = 3. To remember the shapes, think of “double dumbells”
…and a “dumbell with a donut”!
d orbital shapes
Shape of f orbitalsShape of f orbitals
Orbital filling tableOrbital filling table
Electron configuration of the Electron configuration of the elements of the first three elements of the first three
seriesseries
Irregular confirmations of Cr and CuIrregular confirmations of Cr and Cu
Chromium steals a 4s electron to halffill its 3d sublevel
Copper steals a 4s electron to FILL its 3d sublevel
Mendeleev’s Periodic TableMendeleev’s Periodic Table
Dmitri Mendeleev
Modern Russian TableModern Russian Table
Stowe Periodic TableStowe Periodic Table
A Spiral Periodic TableA Spiral Periodic Table
““Mayan” Mayan” Periodic Periodic
TableTable
The Periodic TableThe Periodic Table
Period
Group or family
PeriodGroup or Family
Easily lose valence electron (Reducing agents)
React violently with water Large hydration energy React with halogens to
form salts
The Properties of a Group: The Properties of a Group:
the Alkali Metalsthe Alkali Metals
Properties of MetalsProperties of Metals Metals are good conductors of heat and electricity
Metals are malleable
Metals are ductile
Metals have high tensile strength
Metals have luster
Examples of MetalsExamples of Metals
Potassium, K reacts with water and must be stored in kerosene
Zinc, Zn, is more stable than potassium
Copper, Cu, is a relatively soft metal, and a very good electrical conductor.
Mercury, Hg, is the only metal that exists as a liquid at room temperature
PropertiesProperties of Nonmetalsof Nonmetals
Carbon, the graphite in “pencil lead” is a great example of a nonmetallic element. Nonmetals are poor conductors of heat and electricity Nonmetals tend to be brittle Many nonmetals are gases at room temperature
Examples of NonmetalsExamples of Nonmetals
Sulfur, S, was once known as “brimstone”
Microspheres of phosphorus, P, a reactive nonmetal
Graphite is not the only pure form of carbon, C. Diamond is also carbon; the color comes from impurities caught within the crystal structure
Properties of MetalloidsProperties of Metalloids
Metalloids straddle the border between metals and nonmetals on the periodic table.
They have properties of both metals and nonmetals.Metalloids are more brittle than metals, less brittle than most nonmetallic solids Metalloids are semiconductors of electricity Some metalloids possess metallic luster
Silicon, Si – A MetalloidSilicon, Si – A Metalloid
Silicon has metallic luster Silicon is brittle like a nonmetal Silicon is a semiconductor of electricity
Other metalloids include:
Boron, B Germanium, Ge Arsenic, As Antimony, Sb Tellurium, Te
Half of the distance between nucli in covalently bonded diatomic molecule
"covalent atomic radii"
Periodic Trends in Atomic Radius
Radius decreases across a period Increased effective nuclear charge dueto decreased shielding
Radius increases down a group Addition of principal quantum levels
Determination of Atomic Radius:Determination of Atomic Radius:
Table of Table of Atomic Atomic
RadiiRadii
Increases for successive electrons taken from the same atom
Tends to increase across a period
Electrons in the same quantum level do not shield as effectively as electrons in inner levels
Irregularities at half filled and filled sublevels due to extra repulsion of electrons paired in orbitals, making them easier to remove
Tends to decrease down a groupOuter electrons are farther from thenucleus
Ionization EnergyIonization Energy - the energy required to - the energy required to remove an electron from an atomremove an electron from an atom
Table of 1Table of 1stst Ionization Energies Ionization Energies
Ionization of MagnesiumIonization of Magnesium Mg + 738 kJ Mg+ + e-
Mg+ + 1451 kJ Mg2+ + e-
Mg2+ + 7733 kJ Mg3+ + e-
Another Way to Look at Ionization EnergyAnother Way to Look at Ionization Energy
ElectronegativityElectronegativity
A measure of the ability of an atom in a chemicalcompound to attract electrons
Electronegativities tend to increase across a period
Electronegativities tend to decrease down a group or remain the same
Periodic Table of ElectronegativitiesPeriodic Table of Electronegativities
Summation of Periodic TrendsSummation of Periodic Trends
Ionic RadiiIonic Radii
Cations
Positively charged ions formed when an atom of a metal loses one or more electrons Smaller than the corresponding atom
Anions
Negatively charged ions formed when nonmetallic atoms gain one or more electrons Larger than the corresponding atom
Table Table of Ion of Ion SizesSizes
top related