atomic structure
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Atomic Structure. Topic 1. Objectives:. To understand how the model of the atom has changed To know the subatomic particles and all their properties To understand electrons and their energies To be able to distinguish between ground, excited state and ion configurations - PowerPoint PPT PresentationTRANSCRIPT
Atomic Structure
Topic 1
Objectives:• To understand how the model of the atom
has changed • To know the subatomic particles and all
their properties• To understand electrons and their
energies• To be able to distinguish between ground,
excited state and ion configurations• To distinguish between different types of
matter
Early Studies of Matter
• The model of the atom is the work of many scientists over a long period of time
• Greeks– Fire, air, water, and earth
• Boyle – 1600s– Gold and silver are elemental
Dalton – 1700s• Atom = basic unit of matter• cannonball• Dalton’s Atomic Theory
• All elements are composed of indivisible atoms• All atoms of a given element are identical• Atoms of different elements are different; (different
masses)• Compounds are formed by the combination of
atoms of different elements
• Not all correct today but the groundwork
Thomson – “Plum Pudding”
• Electron
• Atom has some negative charged particle found within
Rutherford’s Gold Foil Experiment
• Nucleus of atom discovered• Nuclear model• Experiment:
– Alpha particle shot at a piece of gold foil
Results Conclusion
Most particle went through
Some were deflected
Rutherford’s Gold Foil Experiment
Bohr Model
• Planetary model
• Electrons in definite fixed orbits
• How we draw them
Wave-Mechanical Model
• Most modern model of the atom
• Gives electrons properties of both particle and wave
• Electrons with distinct amounts of energy moving in orbitals
• Orbitals = region in which electron is likely to be located
Structure of the Atom
• Positive nucleus and negative electrons in regions called orbitals outside nucleus
Proton Neutron Electron
Charge
Mass
Location
Atomic Number
• Atomic Number is the number of protons
Atomic number = # protons
• Each element has its own atomic number…it identifies what element you have
Complete Chart
Atomic Number 4
# protons 32 80Element symbol Xe
Atom is neutral• Neutral means equal amount of positive
and equal amount of negative
• SOOO…. WHAT 2 SUBATOMIC PARTICLES WILL BE EQUAL IN AN ATOM?
• Remember: APE
Mass Number
• Mass number is the mass of the nucleus (protons + neutrons)
Mass # = #protons + #neutrons
Mass # - #protons = #neutrons
• Notation: C-12 12
6C
Complete Chart
Element symbol
Atomic number
Mass number
# protons
# neutron
C 812 6
17 18
Isotopes
• Isotopes are atoms of the same element that have different numbers of neutrons (giving them different mass numbers)
• Same: #protons (atomic numbers)
• Different: #neutrons (mass numbers)
Atomic Masses
• Average masses of all the naturally occurring isotopes
• Weighted average
Finding Atomic Mass Problems
• Carbon has 2 naturally occurring isotopes. 98.89% of C’s are C-12 with a mass of 12 amu. The remaining 1.108% are C-13 with a mass of 13 amu. What is the atomic mass of carbon?
Isotope Mass Abundance
(decimal or percent key)
Total
for isotope
TOTAL
Atomic Mass
Sample Problem
Element X three isotopes; one that occurs 72.0% with a mass of 84.9 amu, the second that occurs 18.0% with a mass of 87.0 amu, and the last that occurs 10% with a mass of 89.1 amu. Find the average atomic mass of Element X.
SolutionIsotope Mass Abundance Total for
isotope
Electrons, Electrons, Electrons
• Electrons surround the nucleus in regions called orbitals
• Electron Configurations for the atom are on the reference tables– Tells how many electrons are in each energy
level– Last number in electron configuration is
number of valence electrons (outermost electrons)
Sample Questions
• Write the electron configuration of the following atoms:– Sodium– Chlorine– Fe
• Circle the valence electrons in the above atoms
Energy of Electrons
• Each electron has its own distinct amount of energy that corresponds to the energy level that it occupies
– Higher the energy level the higher the electron’s energy
Ground vs. Excited State• Electrons can gain or lose energy making
them move to higher or lower energy levels
• Ground State: electrons in their normal energy levels; stable– Found on the reference table
• Excited State: electron gains energy and moves up to a higher energy level– Start with configuration on table, keep same
number electrons, but change the order
Continued
• Ground Excited; energy is __________
• Excited Ground; energy is __________
• Calcium atom’s electron configuration is…– Ground state:
– Excited state:
Sample Problems
Atom Ground State
Excited State
Cl
K
O
Sample Problems
• Which shows an increase in energy?A - Electron that goes from the 2nd shell to the
3rd shell
B - Electron that goes from the 3rd shell to the 2nd shell
• Which of the above A or B will produce a light spectrum?
Ionic Radii
Types of Matter
• Matter – anything that has mass and takes up space (volume)
• Homogeneous – uniform composition– Can contain more than one type of particle,
but the particles have to be evenly mixed– Sugar water
• Heterogeneous – varying composition– Parts have there own chem and phys
properties– Chocolate chip cookie
Matter
Pure Substance
Mixtures
Compound Element SolutionsAll other heter. mixs
Definitions
• Pure Substances – composition is the same throughout
– Element – substances that cannot be broken down or decomposed into simpler substances by chemical means
– Compounds – two or more elements that are chemically combined in definite proportions by mass
• Law of definite proportions – types of atoms in a compound exist in a fixed ratio
– H2O2 vs. H2O
– H2O: mass ratio of 1:8
• Mixtures – combinations of two or more pure substances that can be separated by physical means (not in “fixed” ratios)
– Heterogeneous mixtures
– Homogenous mixtures = solutions