This chapter is very short and easy.

 

Hardly any solving problems (and the ones that you do solve are super easy)

Just memorize a few things and it will be okay.

 

Key things:

Chromium and Copper take an electron from their 4s orbital to have a more stable P orbital

Electron Configuration only goes up to 30 for SL, so its super easy

 

JJ Tomson discovered the Electron

Rutherford fired alpha particles at a gold foil. Some were reflected, so he found the nucleus. He concluded most of the Atom consists of empty space

 

Subatomic particles:

• Nucleus- protons and neutrons
  • also called nucleons
  • Central, high density, positive charge
• Electrons: equal charge opposite to the proton
  • its weight is called "negligible" (compared to protons and neutrons)

 

Niels Bohr discovered electron orbits

 

• Atomic number (Z)
  • number of protons in the atom (equals the number of electrons in a neutral charged atom)
  • unique identifier of an atom
• Mass number (A)
  • Protons and neutrons in an atom
    • • • • • • •  
• Isotopes: atoms of an element with the same atomic number, but different mass number
  • Same chemical properties but different physical properties
  • Find the relative average mass given the percentages of 2 isotopes
    • ((percentage 1*isotope number) + (percentage 2*isotope number))/(100)
  • Find the abundance of an isotope given the 2 percentage isotopes
    • (a*x)+(b(100-x)) = ram*100
      • A is the mass of the first isotope
      • B is the mass of the second isotope
      • "ram" is Relative Atomic Mass
  • Seperating isotopes (also different physical properties): Melting, boiling point, density, rate of diffusion
• Ions
  • Cation: positively charged atom
  • Anion: negative
• Mass Spectra
  • Continuous spectra: all frequencies
  • Line spectra: selective frequencies
  • Absorption line spectra: all but a few frequencies
  • Form mass spectras
  • Information can be used to find relative atomic mass
• Electromagnetic spectrum
  • Red, orange, yellow, green, blue, violet
  • Red: high wavelength, low energy, low frequency
  • Violet: low wavelength, high energy, high frequency
  • Infared- lower energy than red (you can't see it)
  • Ultraviolet- higher energy than violet
• Hydrogen energy levels
  • Visual light is shown when the electron drops from any energy level to energy level 2.
    • ex: n=3 -> n=2
• Energy levles
  • Electrons can be excited and move up a shell
  • They jump back to their normal shell, emitting light
  • Bigger jump=more energy
  • Energy levels converge the further away they are to the nucleus
  • Infinity: electrons so excited they leave the atom
    • • • • • • •  
• Electron Config
  • Final term of an electron:
    • 1s1-1s2
    • 2p1-2p6
    • 3d1-3d10
    • Row number, block number, and column number in relation to the block
  • In the D row, subtract one. so it starts at 3
  • Electron arrangement:
    • amount of electrons in each layer
      • Boron: 2,3
  • Displayed visually by boxes.
    • S orbitals have one block
    • P orbitals have 3 blocks (six electrons)
  • Aufbah rule:
    • Electron shell filled from the lowest energy level

 

 

 

 

Chem tht:

 

An oxide of copper was reduced in a stream of hydrogen as shown below.

After heating, the stream of hydrogen gas was maintained until the apparatus had cooled.

 

An organic compound, A, containing only the elements carbon, hydrogen and oxygen was analyzed

 

Propane and oxygen react according to the following equation

Calculate the volume of carbon dioxide and water vapour produced and the volume of oxygen remaining....

 

Crocetin consists of the elements carbon, hydrogen and oxygen. Determine the empirical formula of crocetin, ...