matter and chemical change- exam #2

Card Set Information

Author:
aleahmurphy
ID:
211851
Filename:
matter and chemical change- exam #2
Updated:
2013-04-10 01:47:06
Tags:
science
Folders:

Description:
science
Show Answers:

Home > Flashcards > Print Preview

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


  1. Understand compounds. (how many elements and atoms are in a chemical formula)
    • Compounds are made up of elements
    • Ex. Li3N.: elements- lithium, nitrogen. atom- 3 lithium,1 nitrogen
  2. What elements make up common substances like table salt, aspirin, and sugar?
    • Table salt: NaCl
    • Aspirin: CHO
    • Sugar: C6H12O6
  3. What name is given to the #'s 2 and 3 in H2O3?
    co-efficients, written as subscripts
  4. Difference between chemical names, chemical equations, chemical formulas and chemical symbols. examples?
    • chemical name: hydrogen
    • chemical equation: 2H2O -> O2 + 2H2
    • chemical formula: H2O, H2
    • chemical symbol: H
  5. How to write common chemical formula's
    • water: H2O
    • carbon dioxide: Co2
    • table salt: NaCl
    • carbon monoxide: CO
    • glucose: C6H12O6
    • ammonia: NH3
  6. Understand that 2H2O means 2 molecules of water. How would you write 6 molecules of glucose?
    6C6H12O6
  7. When naming Ionic Compounds, does the metal or non-metal get written last? What does the ending change to?
    • metal: first
    • non-metal: last
    • the ending changes to ide
    • Morveau of France created this method*
  8. What does aqueous mean?
    dissolves in water
  9. Be able to draw models of a compound
  10. What is an ion? In order for an atom to become charged positively, will it have to lose or gain electrons? Does "+1" or "-1" have a larger charge?
    • an ion has either lost or gained electrons
    • lose (+1): more positive
    • gain (-1): more negative
  11. Perfect salt crystals have which type of shape?
    cubes
  12. For Ionic compounds, be able to pick out polyatomic ions such as...
    • sulfate: SO4
    • phosphate: PO4
    • carbonate: CO3
  13. Be able to name an ionic compound if given the formula, or write the formula if given the elements or the name.
    metal, non-metal, ide
  14. Be able to name a molecular compound if given the formula, or write the formula if given the elements or name.
    • non-metal, non-metal.
    • mono
    • di
    • tri
    • tetra
    • penta
  15. What is the main difference between copper and copper (II)?
    • copper: it either has a charge of 1 or only 1 charge
    • copper (II): it has a charge of 2 and there's 2 or more charges available
  16. What is the difference between subscript and superscrip?
    • superscript- above
    • subscript- below
  17. Know how to read information off of the periodic table
  18. Be able to predict what the ion charge of an atom will be. HINT: draw out a Bohr model of the atom, then decide if it would be better to lose or gain electrons. If it's going to lose them it will be a "+" ion, and if it needs to gain it will be a "-" ion.
  19. What is the most common element found in a molecular compound?
    hydrogen
  20. Properties of Ionic and Molecular compounds. Be able to identify them based on information given.
  21. Be familiar with the chemical reactions that were demonstrated in class.
    • magnesium ribbon is combined with sulphuric acid: acid eats the ribbon away
    • potassium iodide is combined with lead nitrate: bright yellow, precipitate
    • baking soda is added to vinegar: carbon dioxide bubbles
  22. What three processes is oxygen required for?
    • combustion
    • corrosion
    • cellular respiration
  23. Endothermic vs. Exothermic reactions.
    • endothermic: chemical reaction that absorbs energy. ex. cooking
    • exothermic: chemical reaction that releases energy. ex. burning
  24. Photosynthesis vs. Cellular Respiration ( are they exo. or endo.?)
    • photosynthesis (endothermic): Light A+B -> C+D
    • cellular respiration (exothermic): C+D -> A+B+Chemical Energy
  25. What is another name for chalk?
    Calcium Carbonate: CaCO3
  26. Open systems vs. Closed systems
    • open- things are able to enter and leave
    • closed- absolutely sealed, nothing can enter or leave
  27. What is the Law of Conservation of mass? Understand it and explain it.
    • Conservation of mass- principle that matter is not created or destroyed in a chemical reaction; the mass of the products always equals the mass of the reactants.
    • mass is the same, experiment is changed
  28. The three factors that affect the rate of chemical reactions...
    • concentration
    • temperature
    • surface area
  29. What is a catalyst? What are some types of catalysts?
    • a catalyst speeds up reactions
    • forms of catalysts are heat, electricity
  30. Physics properties
    • ductile- able to be stretched into a long wire
    • malleable- able to be pounded or rolled into a sheet
    • hardness- the ability to be scratched
  31. Chemical properties
  32. Chemical equations
    • Reactants are before the arrow
    • Products are after the arrow
  33. periodic groups (vertical)
    • Halogens: (group 17) most reactive non-metals
    • Non-metals: (solid or gas metals are dull, brittle elements that don't conduct electricity
    • Noble gases: (group 18) most stable and unreactive elements
    • Alkali metals: (group 1)most reactive of the metals
    • Alkaline- earth metals: reactivity is not as strong (group 2)
    • Metals: shiny, malleable, and conduct electricity

What would you like to do?

Home > Flashcards > Print Preview