Brief Timeline of Atomic Theory

Democritus 400BC Greek philosopher

Hard Particle (Cannonball)Theory Proposed that they world was made up of tiny, indivisible particles moving through a void of empty space “atom” comes from the Greek word “atomos”, meaning indivisible (cannot be divided)

John Dalton 1808 AD First modern atomic theory

DaltonsDaltons Atomic Theory 1.All matter is composed of tiny, indivisible particles called atoms 2.All atoms of an element are identical 3.Atoms of different elements are all different 4.Atoms combine in simple ratios to form compounds

J.J. Thomson “Plum Pudding Model” Cathode Ray tube experiment demo

Cathode Ray Tube Thompson showed that cathode rays (electrons) were composed of negatively charged particles that separated from the gas atoms inside the tube Significant because: this meant that atoms are not hard, indivisible particles. Atoms are composed of smaller “subatomic” particles

Thomson’s Plum Pudding Model The atom was a hard sphere that was positively charged with negatively charged electrons that “dotted” the atom like raisins in plum pudding

The discovery of radioactivity Henri Becquerel – 1896 – Discovered that uranium ore released rays that could expose photographic film

The discovery of radioactivity Marie & Pierre Curie – Extracted 2 new elements from uranium (U)ore: radium (Ra) and polonium (Po) Marie Curie

Ernest Rutherford Magnetic Field Experiment Was able to separate radioactive rays into 2 types: alpha (  ) & beta (  ) Determined that  rays were composed of helium nuclei (He +2 charge) Gold Foil Experiment (1911) Lead to discovery of the nucleus, as a positively charged center of atom, containing the mass Most of the atom is negatively charged empty space, electrons are outside the nucleus

Magnetic Field Experiment

Gold Foil ExperimentExperiment

Gold Foil Experiment

Experiment

Gold Foil Experiment

Rutherford’s Atomic Model

Rutherford’s “Nuclear Model” Most of the atom is negatively charged empty space, surrounding a small, positively charged nucleus, containing most of the mass of the atom

Modern Theory of Atomic Structure Developed by Niels Bohr, based on the science of nuclear physics Bohr determined that an element's position on the periodic table was related to its electron configuration.

Electron configuration Electron configuration – shows how many electrons are in each energy level or “ring” Ex: Carbon 2-4

Bohr’s Planetary Atomic Model Niels Bohr (1922) Determined that electrons rotate around the nucleus in discrete paths or rings

Planetary Model of Atomic Structure

Wave-Mechanical Model Current (modern) theory of atomic structure Moseley used x-ray analysis to calculate an integer for each element: these integers are the atomic numbers

Wave-Mechanical Model There is a tiny, dense positively charged nucleus at the center of a huge negatively charged electron cloud

Wave-Mechanical Model

Orbital Region of probability of finding an electron

“The whole point:” The modern model of the atom is the result of many investigations that have been revised over a long period of time by many scientists Atomic theory song

Place the models of atomic structure in order from earliest to the modern theory:

Basic Atomic Structure The nucleus occupies less than 0.01% of the total volume of an atom but accounts for 99.97% of its mass. Thus most of an atom is EMPTY SPACE where the ELECTRONS are found, this is called an ELECTRON CLOUD. One atomic mass unit is 1/12 TH THE MASS OF A CARBON-12 ATOM. This is the standard by which the masses of all other elements are determined. It is abbreviated “u”.

Subatomic Particles

Atomic NumberMass Number Nuclear Charge # of Protons # of Neutrons# of electrons Al Cl 11H11H Pb Use your Periodic Table to complete the following:

The only number that never changes for an element is ATOMIC NUMBER !!

NameSymbol Atomic Number Mass Number Charge # of Protons # of Neutrons# of electrons 19 9 F 0 Helium Nitrogen Cu Atomic Structure 1

Name-massSymbol Atomic Number Mass Number Charge # of Protons # of Neutrons# of electrons Flourine F Helium He Sodium Na Nitrogen N Silicon Si Silicon Si copper Cu Manganese Mn Barium Ba Iodine I Iodine I Atomic Structure 1

Phosphorus C 0 Potassium Fe Mg 0 **Shade the columns representing the nucleons light blue

ISOTOPE Forms of the same element having different mass due to different number of neutrons. Indicated by “element name-mass”

15 8 O 16 8 O Name: _______________ Mass: ________________ Protons: ______________ Neutrons: _____________ Name: _______________ Mass: ________________ Protons: ______________ Neutrons: _____________

Practice: NameSymbolAtomic #Mass ## Protons# Neutrons# Electrons 235 U 238 U Carbon-12 Carbon-13

The mass number on the periodic table indicates the weighted average of all the naturally occurring isotopes of an element To calculate a weighted average: % X mass + % X mass + …..100

Neon is naturally found in nature having 90.51% mass of 20.00u, 0.24% mass of 21.00u and 9.22% mass of 22.00u. Calculate the weighted atomic mass of neon.

Calculate the weighted average atomic mass of the elements below. Show all work, round to the nearest hundredth. a.)99.63% 14 N & 0.37% 10 N b.)69.1% 63 Cu (actual mass of 63.93g) & 30.9% 65 Cu (actual mass of 64.93g) c.)78.9% 24 Mg, 10.00% 25 Mg & 11.01% 26 Mg

You can estimate which isotope is found in the highest abundance as the one with a mass closest to the mass listed on the periodic table Example: Chlorine-35 mass g Chlorine-37 mass g Look on the periodic table for the mass of chlorine ____________________________ The more abundant isotope has a mass closer to the mass given on the periodic table:_____________

Practice: Which isotope of silicon would be found in the highest percentage? Si, mass Si, mass Si, mass Why?

Atomic Structure 2 IsotopicNotation Number of protons Number of neutrons Number of electrons Mass number 1.Oxygen-16O O 2.Oxygen-18 3.Ar S Iron Fe Ne Hydrogen H H3H

2.) Calculate the weighted average of the following naturally occurring isotopes. SHOW ALL WORK! a.) 95.50% 7 Li & 7.50% 6 Li d.) 99.63% 14 N & 0.37% 15 N b.)80.20% 11 B & 19.80% 10 B e.) 78.9% 24 Mg, 10.00% 25 Mg, & 11.01% 26 Mg c.)95.02% 32 S, 0.75% 33 S, & 4.21% 34 Sf.) 92.23% 28 Si, 4.67% 29 Si, & 3.10% 30 Si

Changes in number of subatomic particles Isotopes Change in number of neutrons Same atomic number, different mass Same number protons, different number neutrons Ions Change in number of electrons A ca t ion is positive ion, results from loss of electrons, reducing radius An a n ion is negative ion, results from gain of electrons, increasing radius

IONS A charged part of an atom, resulting from the loss or gain of electrons VALENCE electrons: outermost electrons, the last number in an electron configuration KERNEL electrons: all electrons except valance electrons

Electron configuration Electron configuration – shows how many electrons are in each energy level or “ring” Ex: Carbon 2-4

Electron configuration of sodium:

2 diagrams of atomic structure: Bohr diagramsLewis electron dot diagrams Bohr realized that the rows on the periodic table corresponded to the number of shells of electrons Lewis realized that the groups/families on the periodic table correspond to the number of valence electrons This model shows the nucleus, indicating the number of protons and neutrons, surrounded by rings, representing each energy level This model shows the element symbol surrounded by dots, representing the valence electrons. You must place one dot at each (3, 6,9,12 o’clock) location before “doubling up” (exception: Helium) 18 9 F electron configuration 2-7 F electron configuration 2-7

118 1 Bohr Atomic Structures tables to fill in the electron 4 configurations, as shown, then draw the Bohr Atomic Structure for each element Rules: 1.) Show placement2.) The nucleus is3.) Indicate the number of ALL electronsrepresented by a centerof electrons in each circle showing theenergy level, by writing *use atomic # # of protons & thethe number on each ring OR the entire# of neutrons electron configuration** closest to nucleus is 1 st

2 Main Types of Ions: a n ion A negative ion Ex: Cl -, O -2 ca t ion A positive ion Ex: Na +, Al +3

The octet rule Atoms will gain or lose electrons in order to have a full valence shell of 8 electrons. Exception: Helium can have a maximum of 2 valance electrons

When an atom gains 1 or more electrons It becomes a negative ion and it’s radius increases. A negative ion is an anion.

When an atom loses 1 or more electrons It becomes a positive ion and it’s radius decreases. A positive ion is a cation.

CATIONANION Definition positive ionnegative ion Results from Loss of electron(s)Gain of electron(s) Indicated by (+) charge(-) charge What happens to radius??? Gets smallerGets bigger Na Na + Naming “Element name-ion”Change ending of element to “-ide” Lewis Dot Structure [Na] +.. [:. F. :] -

How to predict if an element will form an anion or cation: The “electron clock”: 8/ # valance electrons

Atomic Structure 3: Predicting Ions Element Electron configuration Lewis dot structure of atom Lose or gain electrons? How many electrons lost or gained? Ionic Charge ** Lewis dot structure of ion Radius increase or decrease? F2-7Fgain1Fincrease Mg2-8-2Mglose2+2Mgdecrease O Al N Fr C

**In the “ ionic charge ” column only: shade the cation charges red and the anion charges blue Element Electron configuration Lewis dot structure of atom Lose or gain electrons? How many electrons lost or gained? Ionic Charge ** Lewis dot structure of ion Radius increase or decrease?

# of Protons # of Neutrons # of Electrons Nuclear Charge Bohr Diagram of Atom Lewis Dot of Atom Predict Ionic Charge Lewis Dot of Ion Name of Ion ex Cl Cl Chloride Na Be Zn N S Ne I Ag Ga C Atomic Structure 4

Atomic Spectra

Radiant Energy Energy that travels through space as electromagnetic waves at the speed of light

Electromagnetic Spectrum Includes all types of radiant energy from gamma rays (hi E) to radiowaves (lo E) Visible light is only a small portion of the spectrum

1 photon = 1 quantum Quanta: tiny packets of energy released or absorbed by objects *Einstein and Plank determined that energy is released or absorbed in a continuous flow of small packets or quantum/photons

Release or Absorption of Energy:

Higher energy levels (excited state) Electrons absorb energy when jumping to Electrons release energy when falling to Lower energy levels (ground state)

Bohr used the emission spectrum as proof of planetary model But his model only works for hydrogen because he didn’t account for electrons moving between energy levels

Spectral Lines Characteristic wavelengths ( ) of photons of energy released as electrons fall from hi to lo energy

Spectral lines demo: Salt of Element Color of Flame Strontium Chloride Barium Chloride Copper (II) Chloride Lithium Chloride Potassium Chloride Identity Unknown Element Unknown Mixture

Emission Spectrum:

Each element has it’s own characteristic spectrum:

Compare H & He: hydrogenhelium

Because electrons do move between energy levels, emitting “spectral lines”, we had to change our view of atomic structure:

Excited State Electron Configurations Occurs when elements absorb energy and jump to a higher energy level. ** it will not look like it is written on periodic table, be sure they add to the correct number! Ground state: Excited state : 2-7-2

“Crib Sheet” #p + = atomic number*#n 0 = mass-atomic number #e - = #p + - charge (use the sign of the charge) Isotope: same #p +, different #n o OR same atomic number, different mass To calculate weighted average: (%/100 x atomic mass) + (%/100 X atomic mass) + ….. *Ion: same # p +, different #e - Charge= #p + - #e -

Atomic Structure Review p Br 10. C 11. Sn 12. Zn 13. Cl

Atomic Structure Review p ) =(.925x7) + (.0750x6) = =6.925 =6.93g 17) =(.789x24)+(.10x25)+(.1101x26) = = = 24.30g

Atomic Structure Review p ) ) Na 20.) ) ) 1 23.) Y 24.) Ar 25.) Not possible 27.) as electrons fall from excited state to ground state energy is released as radiant energy (spectral lines). 28.) you can ID the gas element using spectral line analysis. 29.) electrons are negatively charged particles. B has 5 e -, its e - config. is 2-3, with 2 e - in the 1 st energy level and 3 e - in the 2 nd (valence) level

Atomic Structure Review MC?s 1.) 213.) 1 2.) 414.) 4 3.) 115.) 1 4.) 116.) 3 5.) 317.) 4 6.) 118.) 3 7.) 419.) 2 8.) 220.) 2 9.) 421.) 3 10.) 3 11.) 4 12.) 3pg ) 413.) 2 2.) 314.) 4 3.) 215.) 3 4.) 316.) 3 5.) 217.) 2 6.) 318.) 1 7.) 119.) 1 8.) 220.) 4 9.) 321.) 4 10.) 122.) 2 11.) 323.) 3 12.) 1pg 21-22

Atomic Structure Review p ) 19p, 20n, 18e2.) 9p,10n,10e 3.) 5p,6n,2e4.) 15p,16n,18e 5.) 16p,16n,18e6.) 14p,14n,10e 7.) 7p,7n,10e8.) 20p,20n,20e 9.) 37p,48n,36e10.) 53p,75n,54e 11.) 30p,35n,28e12.) 6p,6n,10e