Chemistry 30s

Card Set Information

Author:
KaZuma_t3
ID:
237141
Filename:
Chemistry 30s
Updated:
2013-09-26 02:16:59
Tags:
Chemistry 30s
Folders:

Description:
Chemistry 30s
Show Answers:

Home > Flashcards > Print Preview

The flashcards below were created by user KaZuma_t3 on FreezingBlue Flashcards. What would you like to do?


  1. Why is Democritus important?
    - proposed that all matter is made up of atoms and empty space
  2. What are Dalton's 4 statements about the atomic theory?
    • - all matter is composed of atoms
    • - all atoms of the same element are identical
    • - atoms of different elements are different
    • - atoms unite in definite ratios to form compounds
  3. Why is Thomson important?
    • - discovered the electron
    • - discovered the charge to mass ratio
    • - established the cottonball model
  4. Why is Chadwick important?
    - discovered the neutron
  5. Why is Rutherford important?
    • - all the mass and positive charge are located in a small nucleus
    • - most of the atom is empty space
    • - negative electrons are scattered throughout this empty space
  6. Why is Milikan important?
    - determined the charge on the atom
  7. Define atom
    - the element is balanced with the same number of protons, electrons, and neutrons
  8. Define ion
    - an element that has gained or lost electrons
  9. Define isotopes
    - a group of the same element with the same number of protons but different masses
  10. Name the Alkali metals
    • - lithium
    • - sodium
    • - potassium
    • - rubidium
    • - cesium
    • - francium
  11. Name the Halogens
    • - flourine
    • - chlorine
    • - bromine
    • - iodine 
    • - astatine
  12. Name the Noble Gases
    • - helium
    • - neon
    • - argon
    • - krypton
    • - xenon 
    • - radon
    • - ununoctium
  13. What are four trends in properties that occur as the atomic number increases in the alkali metals?
    • - they get more reactive
    • - atoms become larger
    • - the outer electron gets farther away from the nucleus
    • - inner electrons shield the outer electrons from the positive nucleus
  14. What are four trends in properties that occur as the atomic number increases in halogens?
    • - they get less reactive
    • - atoms become larger in size
    • - the outer electron gets farther away from the nucleus
    • - inner electrons shield the outer electrons from the positive nucleus
  15. What are four trends in properties that occur as the atomic number increases in the noble gases?
    • - chemically inactive due to their full outer shells
    • - atoms become larger
    • - the outer electron gets farther away from the nucleus
    • - inner electrons shield the outer electrons from the positive nucleus
  16. Why do changes in activity occur as the atomic number increases in alkali metals?
    • - increases in size
    • - increases in shielding 
    • - becomes more reactive
  17. Why do changes in activity occur as the atomic number increases in halogens?
    • - increases in size
    • - increases in shielding
    • - becomes less reactive
  18. Why do changes in activity occur as the atomic number increases in noble gases?
    • - increases in size
    • - increases in shielding
    • - no reactivity due to full outer shells
  19. Why do halogen atoms form diatomic molecules?
    - only two of that element can share an electron
  20. Define orbitals
    - the region of space around a nucleus in which an electron is most likely found
  21. How do orbitals relate to sublevels?
    - each sublevel has a different number of orbitals and therefore a different number of electrons
  22. Define line spectrums
    - when heat is applied to an atom and the light is passed through a prism
  23. Define continuous spectrum
    - when white light is passed through a prism
  24. Define quantum mechanics
    - describes the behaviour of electrons in terms of quantized energy changes
  25. Define principal quantum numbers
    • - the main energy levels in electron configuration 
    • ex the 1 in 1s2

What would you like to do?

Home > Flashcards > Print Preview