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Chapter 5. Electrons in Atoms. What were early steps in development of atomic theory?. John Dalton – Billiard Ball Theory Atom was indivisible J.J. Thomson – Plum Pudding Model Atom was composed of smaller particles. Rutherford Model. n ucleus contains:
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Chapter 5 Electrons in Atoms
What were early steps in development of atomic theory? • John Dalton – Billiard Ball Theory • Atom was indivisible • J.J. Thomson – Plum Pudding Model • Atom was composed of smaller particles
Rutherford Model • nucleus contains: • all the positive charge & most of mass of atom • nucleus very small: • only 1/10,000th of atomic diameter • electrons occupy most of volume
Later Models • Bohr – Planetary Model • Schrodinger – Wave Mechanical Model
Problems with the Rutherford Model • Why don’t electrons crash into nucleus? • How are electrons arranged? • Why do different elements exhibit different chemical behavior? • How is atomic emission spectra produced?
Atomic Emission Spectra • gas in glass tube & apply voltage across ends • produces light • color of light depends on gas in tube • every element produces its own unique color
emission spectrum of element is set of frequencies (or wavelengths) emitted
Why is emission spectra useful? • use it to determine if given element is present in sample • Neon lights
Bohr Model • Bohr - electrons in atom can have only specific amounts of energy NEW idea! • each specific amount energy is associated with specific orbit • electrons restricted to these orbits • Bohr assigned quantum number (n) to each orbit • the smallest orbit (n= 1) • closest to nucleus • has lowest energy • larger the orbit, more energy it has
E3 n=3 n=3 E2 n=2 E1 n=1 Bohr Diagram • Shows all the electrons in orbits or shells about the nucleus. n=2 n=1
Bohr Model • energy absorbed when electron: • moves to higher orbit (farther from nucleus) • endothermic process • energy released when electron: • drops to lower orbit (closer to nucleus) • exothermic process
energy levels get closer together the farther away they arefrom nucleus Larger orbits can hold more electrons
Orbit Max # of Electrons 1 2 2 8 3 18 4 32 n 2n2 Max Capacity of Bohr Orbits
Electron Transitions • If electron gains (absorbs) specific amount of energy • it can be excited to move to higher energy level • If electron loses specific amount of energy • it drops down to lower energy level
Hydrogen has 1 electron, but it can make many possible electron transitions
Absorption & Emission • cannot easily detect absorption of energy by electron BUT • can easily detect emission of energy by electron • photons (light) given off as excess energy is released
Emitted Light • energy of emitted light (E = h • matches difference in energy between 2 levels • don’t know absolute energy of energy levels, but • observe light emitted due to energy changes
ladder often used as analogy for energy levels of atom How is this one different? Potential Energy
Ground State vs. Excited State • Ground state: • lowest energy state of atom • electrons in lowest possible energy levels • configurations in Reference Tables are ground state • Excited state: • many possible excited states for each atom • one or more electrons excited to higher energy level
Success of Bohr’s Model • Bohr’s model could predict frequencies in emission spectrum of hydrogen • Predicted correct size of H atom • Unfortunately, didn’t work for anything with more than 1 electron
Which principal energy level of an atom contains electron with the lowest energy? • n=1 • n=2 • n=3 • n=4
What is total # of occupied principal energy levels in atom of neon in ground state? • 1 • 2 • 3 • 4
What is total # of fully occupied principal energy levels in atom of nitrogen in ground state? • 1 • 2 • 3 • 4
What is total # of electrons in completely filled fourth principal energy level? • 8 • 10 • 18 • 32
Which atom in ground state has five electrons in its outer level and 10 electrons in its kernel? • C • Cl • Si • P
Which electron configuration represents atom in excited state? a) 2-8-2 • 2-8-1 • 2-8 • 2-7-1
Which electron configuration represents atom of Li in an excited state? • 1-1 • 1-2 • 2-1 • 2-2
The characteristic bright-line spectrum of atom is produced by its • Electrons absorbing energy • Electrons emitting energy • Protons absorbing energy • Protons emitting energy