Hon Chemistry 4-12-21 Chapter 4 Overview

HON CHEMISTRY: God bless as you study for the chapter 4 test! Here’s our overview of the test and look back at some of the “problems” from the chapter.

Have you checked out the Chapter 4 Stuff to Know Sheet? Make sure you give yourself plenty of time to memorize the things you need to memorize so that you can apply them on the test. And practice, practice, practice, the problems and electron configurations. Did I mention that already?

What about applications for discussion? Photoelectric effect, spectroscopy, etc.? Another great idea for studying is to watch the videos that we watched in class, and others – super helpful as you study for the test!! Here are some of them:
Spectrum of the Stars (overivew of the results of the spectroscopy lab you did, shows the connection between our lab on spectroscopy and how we can identify elements), Emission Spectrum of Hydrogen (how we use it to know about the energy levels in an atom), Quantum Mechanics (about the roles of Bohr, Schrodinger, Heisenberg), and also Animated Quantum Mechanics.

God bless you as you study! I’ll be praying for you!!

flickr photo by only alice

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12 thoughts on “Hon Chemistry 4-12-21 Chapter 4 Overview

  1. Q: How does deviant behavior stray from the Aufbau Principal?

    A: While the aufbau principal and in turn aufbau chart give a specific order of how orbitals should fill up, the transition metals decided to be special. The lanthanides and actinides do not go straight into 4f and 5f, but instead, 5d and 6d receive one electron and then 4f or 5f is filled, while the rest of 5d and 6d are filled afterwards.

  2. Q: what makes the Lanthanides and Actinides metals different from other elements and why.

    A: Lanthanides and Actinides have a devient behavior where after putting one electron in the D orbital it will fill up its F orbital then goes back and fill in the rest of its D orbital. This occurs because the element want to have less energy, and putting one electron in the D orbital and filling up the F orbital, then going back and filling up the rest of the D orbital, take less energy then filling up all the D orbital then filling up all the F orbitals.

  3. Q: When a metal is burned in a flame, what determines the color of the flame?

    A: The color of light that is emitted in the flame is determined by the electron configuration of the specific element. When the electrons fall back down to a lower energy level, they emit energy in the form of light. The sum of all of the energy produced by the electrons creates specific colors for each metal. Each element produces a different color because of its unique electron configuration. The colors produced from the metals correspond with the emission spectrum.

  4. Q: Why do different elements give off different colors when their electrons are excited

    A: Every element has a different number of electrons so when electrons are excited and jump energy levels and fall back down they release energy as light which is different for every element

  5. Q: Why do the transition metals display deviant behavior?

    A: The transition metals place one electron in an s orbital and then will fill in the previous d orbitals completely before adding the second electron to that s orbital. They do this because the full d orbitals allow the metal to be more stable than it would be otherwise.

  6. Q: why is helium considered a noble gas despite only having 2 valence electrons

    A: Helium only has 1 energy level and only one orbital, 1s. This orbital can only hold 2 electrons. Because its outermost energy level is filled, it is a noble gas.

  7. Q: Why do elements have different colors when heated?

    A: When electrons take in energy, they go up to a higher energy level. When they fall back down to ground level, the electrons give off that energy in the form of visible light. Since each element has a different number of electrons at different energy levels and orbitals, each one will give off a certain color of light specific to that element.

  8. Q: What causes elements to give off light?

    A: When electricity is shot through the atoms, the electrons jump up to a higher energy level. When they fall back down the release energy in the form of photons, which is light.

  9. Q: What do the spectral lines on emission spectra represent?

    A: They represent the wavelength of light that is given off by electrons falling back down to ground state after being hit with energy. They are all at different wavelengths because each electron releases a different amount of energy in the form of photons when they jump different energy levels and therefore have different wavelengths.

  10. q: when writing the orbital notation of an element in the p block, why do you draw the three up arrows before drawing any down arrows?

    a: according to Hund’s rule, electrons will go into an orbital spinning one direction, before they begin filling it up in the opposite direction. because of this principle, when writing the orbital notation, you must draw the 3 up arrows of a p block before drawing any down arrows, to symbolize the electrons spinning clockwise before counterclockwise.

  11. Q: How is the photoelectric effect work within elevator doors?

    A: Many elevators doors use a beam of light and a photocell, which is a device that converts light energy into electrical energy. When the beam of light strikes the photocell, the photoelectric effect generates and ejects electrons that produce an electric current. When someone puts their foot in the door, the electric current is interrupted, and the doors are signaled to open back up.

  12. Why is it impossible to measure an electron’s location without having some uncertainty?

    This happens because when electrons are detected, photons are used to measure them and since photons have the same energy as electrons, these photons interact with the electrons and knock them off course making it impossible to pinpoint their locations.

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