Unit 3 Flashcards
Properties of Electromagnetic Waves
Wavelength
Frequency
Energy
Frequency Measured In
Nu
Electromagnetic Radiation
Form of energy that exhibits wavelike behaviour as it travels through space
Electromagnetic Spectrum
Arrangement of all electromagnetic waves by decreasing wavelength and increasing frequency
Electromagnetic Spectrum Order
Gamma
X-ray
Ultraviolet
Visible light
Infrared
Microwave
TV radio
AM radio
Long radio
Visible Light Amounts
Wavelength 1.0x10^-7 m
Frequency 1.0x10^14 Hz
Energy 1.0x10^-19 J
Quanta
Light does not produce energy continiously, but in packets called quanta
Quantum
Minimum amount of energy lost or gained by an atom due to its energy levels
Quantized Energy
Multiples of quanta
Energy Equation
E=hv
Planck’s Constant
6.626x10^-34 J*s
Photon
Particle of electromagnetic radiation Zero mass
Carrying a quantum of energy
Moves like waves
Line Emission Spectrum
Bands of light
Continiuous Spectra
White light that continuously emits lines of all colors
Line Emission Spectra
Only certain lines of color are seen
Four Arrangements of Electrons
Principle energy level
Sublevel
Orbital
Electrons spin
Sublevel S
Spherical shape
Holds 2 electrons
Sublevel P
Dumbell shape
Three P orbitals in 1 P sublevel
Holds 6 electrons
Sublevel D
Clover shape
Five D orbitals in 1 D sublevel
Holds 10 electrons
Sublevel F
Flower shape
Seven F orbitals in 1 F sublevel
Holds 14 electrons
Orbitals
Different orientations of shapes within a sublevel
Rules to Writing Electron Configurations
Aufbau
Pauli
Hund
Aufbau’s Principle
Electrons will occupy the lowest energy first
Pauli’s Exclusion Principle
A maximum of 2 electrons can fill an orbital if they have opposite spins
Hund’s Rule
Electrons will fill equal level orbitals until each has one before doubling up
All electrons have the same spin in each individually filled orbital
Excpetions
Column 11 and 6
Move S to D to make stable
D Doesn’t Count As
Valence electron
Coefficient on Last Sublevel
Energy level
Highest Sublevel
Block
Isoelectronic Series
Ions with the same electron configuration
Dmitri Mendeleev
Organized periodic table by atomic mass and similar row properties
Henry Moseley
Rearranged elements by increasing atomic number
Periodic Law
Physical and chemical properties of elements are periodic functions of their atomic number
Length of Period
Determined by number of electrons that can occupy the sublevels filled in that row
Elements in Same Group
Share properties
Share same number of valences
Why Same Group Elements Have Similar Properties
Lose or gain same number of electrons when forming ions
Metals
Elements containing atoms that readily lose electrons to form ions
Cations
Chemical Metal Properties
Few electrons in valence level
Loses electrons readily
Positive charge
Forms cations
Physical Metal Properties
Ductile
Malleable
High tensile strength
Good conductors
Luster
Forms alloys
Mostly solid at room temperature
Alkai Metals
Always have one valence electron
Never found purely as too reactive
Alkai Metals IA
Very reactive
Most reactive group of metals
Soft
Silvery
Phenomenon
Alkai metlas plus water
Alkaline Earth Metals IIA
Two valence electrons
Less reactive than alkali
Still not found pure
Alkaline means basic
Transition Metals
D block elements
B groups
Typical metallic properties
Lanthanides
Rare Earth metals
Silver
Tarnish in oxygen
Actinides
Radioactive
Nonmetals
Elements containing atoms that readily gain electrons to form negatuve ions
Anions
Chemical Nonmetal Properties
Almost full or full valence energy level
Tend to gain electrons
Negative charge
Form anions
Physical Nonmetal Properties
Not ductile
Not malleable
Bad conductors
Brittle
Mostly solid
Some are gases at room temperature
Halogens VIIA
Seven valence electrons
Most reactive nonmetals group
Only found in pure form as diatomic
Noble Gases VIIIA
Eight valence electrons
Colorless
Odorless
Chemically unreactive
Only found purely in nature
Metalloids
In between metals and nonmetals
Chemical Metalloid Properties
Form anions or cations depend on environment
Properties of both metals nonmetals
Physical Metalloid Properties
Semiconductors
Some have metallic luster
Semiconductors of electricity
Some are gases at room temperature
Periodic Trends Influenced By
Shielding
Charge on nucleus
Distance of electrons from nucleus
Shielding Cause and Effects
Inner electrons repel outer blocks nuclear effects
Nucleus hold is weak causes electrons to be easier to remove
Atomic Radius Cause and Effects
Increased charge attracts electrons inward
Energy level added makes it further from nucleus
Ionic Radius Cause and Effects
Increased positive charge pulls electrons inward
More electrons than protons increases repulsive forces
Ionization Energy
Energy required to remove an electron from an atom or how easily it becomes a cation
Ionization Energy Cause and Effects
Atomic radius decreases causes valence electron to be closer
Valence electron is closer causes it to be held more tightly
Electronegativity
Measure of the ability of an atom in a chemical compound to attract electrons from another atom or how easily it becomes and anion
Electronegativity Cause and Effects
Positive nuclear charge causes stronger electron pull
Valence electrons further from nucleas causes it to be difficult to pull more in
Nuclear Charge Down The Group and Across The Period
Increases
Periodic Trends
Increasing nuclear charge and number of protons but same energy level
Group Trends
Increasing shielding and number of energy level
Reactivity Cause and Effects
Increase in shielding causes reactivity to decrease
Increase in shielding causes more orbits
More orbits causes less attraction
Valence Electron Pattern
Increase across period
Remain same down a group
Atomic Radius Pattern
Peaks on left and moves down then peaks again
Metals VS Nonmetals Reaction
Lose VS gain electrons
Electron Affinity
The amount of energy released when a neutral gaseous atom gains an electron
Electron Affinity Cause
Greater nuclear charge releases more energy
Smaller valence shells means higher energy release
Three Factors That Affect Electron Affinity
Nuclear charge
Atomic radius
Electron configuration
Electron Affinity Pattern
Increase across period
Decrease down the group
Diatomic Elements
Metallic Character Cause and Effects
Nuclear charge increases from left to right
Electrons are pulled closer inward
Atom has more difficult time losing electrons
Increases metallic character
