Presentation on theme: "Electrons in Atoms Chapter 5 General Chemistry. Objectives Understand that matter has properties of both particles and waves. Describe the electromagnetic."— Presentation transcript:
Objectives Understand that matter has properties of both particles and waves. Describe the electromagnetic spectrum in terms of wavelength and energy; identify regions of the electromagnetic spectrum.
Objectives Using Bohr’s model of the atom interpret changes (emission/absorption) in electron energies in the hydrogen atom corresponding to emission transitions between quantum levels. Write quantum numbers for electrons in atoms of elements Write the electron configurations for elements.
Review/Link to Previous Learning Atoms are the smallest part of an element that contains the properties of that element Atoms consist of protons, neutrons, and electrons Quantum Mechanics is the currently accepted model of the atom
Parts of EM Spectrum In order of increasing frequency: Radio waves Microwaves and Radar Infrared rays Visible light Ultraviolet rays X rays Gamma rays
Transverse Waves Visible light exhibits properties of wavelike motion. One type of wave is a transverse wave. Transverse waves are like taking a rope and moving it up and down. A transverse wave is a wave that causes the medium to vibrate at right angles to the direction that the wave travels. The particle in the medium travels perpendicular to the motion of the wave.
Solar panel on calculator produced electrical current when light shines on it Photoelectric effect: emission of electrons from a metal caused by light striking the metal Experiments show only certain colors of light (only certain amount of energy) will allow electrical current to flow
Quanta of Energy A quantum is the minimum amount of energy that can be lost or gained by an atom Max Planck proposed relationship between quantum of energy and frequency of radiation (and color of light)
Energy in Quantum of Energy E = h x ν E = Energy (Joules) h = Planck’s Const. (6.63 x 10 -34 Joules x sec) ν = frequency (cycles/sec or Hertz or sec -1 )
Sample Problem Calculate the energy of a photon with a frequency of 2.85 x 10 12 Hz.
Sample Problem Calculate the energy of a photon with a frequency of 2.85 x 10 12 Hz. Answer: 1.89 x 10 -21 J
Study Buddy Review What is the Photoelectric Effect? How is a energy related to the color of light?
Spectra Observations of properties of light emitted by an atom after it absorbs extra energy Continuous spectrum Atomic emission spectrum
Line Spectra 1) For white light (sun or incandescent light bulb), you see continuous spectrum- rainbow of all colors Contains all colors of visible light Example: prism separates white light into rainbow colors. 2) Atomic Emission Spectrum (Line- emission spectrum) contains only certain colors or wavelengths, mostly black unique for each element “fingerprint” Example: pink glow from hydrogen gas tube that can be separated into series of lines
Recall Bohr’s Model of the Atom Thought atom was mostly empty space Nucleus in center is dense, positively charge Electrons move in orbits around the nucleus http://images.search.yahoo.com/search/imag es/
Hydrogen Atom Bohr’s model arose from hydrogen atomic emission spectra. If electrons move in specific orbits, they have a certain fixed amount of energy Observed as discrete bands of color
Why Bands of Color? Electrons can only absorb a certain amount of energy to enter the excited state (next energy level) Like rungs of ladder Can only move to specific orbit, which has a specific energy
Parts of Bohr model Ground state: lowest energy state of an atom Excited state: state in which an atom has a higher potential energy than it has in its ground state
How is Radiation Produced from Atom? When an excited electron falls back from an excited state to its ground state, it emits a photon of radiation. (E= h ν ) Since only specific frequencies of light are emitted from elements, the energy levels in atom are fixed. Electrons exist in only certain energy states.
Only for Hydrogen Bohr’s model of atom was successful only for elements with one electron
Heisenberg Continued building on Bohr model Uncertainty Principle – it is impossible to know both the exact position and the velocity of an electron or other particle simultaneously Act of measuring changes what you are trying to find Thus, no well-defined orbit (like Bohr had proposed) Best we can do is represent PROBABILITY of finding e- within a given space
Schrodinger Erwin Schrodinger developed a mathematical equation that allowed for wavelike behavior of electrons Energy of electrons is quantized
Quantum Mechanical Model of Atom atom is mostly empty space Nucleus in center is dense, positively charge Electrons are around the nucleus e- do not have a precise orbit (electron cloud) e- moves in wavelike motion with quantized amounts of energy
Quantum Numbers Quantum Numbers: specify the properties of atomic orbitals and properties of electrons in orbitals.
Principle Quantum Number (n) n: Principal energy level or energy number n = 1, 2, 3…(as you get farther from nucleus) maximum # of e- in energy level = 2n 2
Angular Momentum (l) l: Shape of orbitals (sublevels) named s, p, d, f s = spherical p = dumbbells d = clover leaf f = butterflies?? each sublevel has slightly different energy
Magnetic (m l ) m l = Orientation of orbital around nucleus s = 1 orbital p = 3 orbitals d = 5 orbitals f = 7 orbitals
Spin m s m s = Magnetic spin Only two directions of spin to create magnetic field Like N and S of magnet
Electron Configurations Electron configuration: Notation describing the most stable arrangement of e- around the nucleus Like writing the address for electrons around nucleus of atom
Three Rules for Electron Configurations 1. The Aufbau Principle e- added one at a time to the lowest energy levels 2. The Pauli Exclusion Principle orbital can hold at most 2 e- must have opposite spin 3. Hund’s Rule (The “bus seat” rule) e- like to be unpaired if possible &e- enter equal energy orbitals until all orbitals contain one e- with parallel spin, then they begin to pair up
Electron Configuration Write the electron configuration for the following: Oxygen Sodium copper