1 / 21

Unit 3 Study Guide

Unit 3 Study Guide. Ionic – between metal and nonmetal and transfers electrons Covalent – between two nonmetals and shared electrons. It fulfills the octet rule. All elements with 8 outer electrons. In an ionic bond, metals lose electrons while nonmetals gain electrons.

halden
Download Presentation

Unit 3 Study Guide

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Unit 3 Study Guide

  2. Ionic – between metal and nonmetal and transfers electrons • Covalent – between two nonmetals and shared electrons

  3. It fulfills the octet rule. All elements with 8 outer electrons

  4. In an ionic bond, metals lose electrons while nonmetals gain electrons

  5. In a covalent bond, nonmetals share electrons

  6. When an atom loses electrons, it becomes a positive charge ion which is called a cation • When an atom gains electrons, it becomes a negative charge ion which is called a anion

  7. Determine whether these compounds are ionic or covalent. • NaCl- ionic • CH4 - covalent • CaCl2 - ionic • NH3 - covalent • Al2O3 - ionic

  8. Name each ionic compound. (Metal name + Nonmetal stem name + -ide ending) • Ex: K3P = potassium + phosph + -ide = potassium phosphide • NaBr__sodium bromide_____________ • CaO__calcium oxide___________________ • Li2S ___lithium sulfide___________________ • LiF__lithium fluoride__________________ • MgO___magnesium oxide__________

  9. Name these ionic compounds containing transition metals. • Pb3P2___lead (II) phosphide___________ • Co3N2___cobalt (II) nitride__________ • CuBr2___copper (II) bromide________________ • FeBr3___iron (III) bromide_________________ • ZnO____zinc (II) oxide_______________

  10. Name each ionic compound containing polyatomic ions. ( Metal name + Polyatomic ion name or Polyatomic ion name + Polyatomic ion name or Polyatomic ion name + Nonmetal name) • Be(OH)2__beryllium hydroxide___________ • CaCO3___calcium carbonate____ • NH4OH ___ammonium hydroxide______ • AlPO4____aluminum phosphate____ • NH4F _____ammonium fluoride____

  11. Write the Greek prefixes for the numbers 1-10.

  12. Name these covalent compounds using prefixes. • ( Prefix + element name + Prefix + stem name + -ide ) • Ex: P2O5 = diphosphoruspentaoxide • SO3___sulfur trioxide__________ • XeF6___xenon hexafluoride___________________ • SiBr4___silicon tetrabromide____________________ • Cl2O7__dichlorineheptaoxide_______ • P4O10_tetraphosphorusdecaoxide______

  13. Write the formulas for the following compounds • aluminum chloride _____AlCl3________________ • calcium carbonate ______CaCO3____________ • beryllium phosphide _____Be3P2_____________ • copper (IV) oxide ______CuO2______________ • magnesium acetate _____Mg(C2H3O2)2________

  14. Write the name of each acid. (Hydro- + stem name of element + -ic + acid) • HCl____hydrochloric acid________________ • HF _____hydrofluoric acid_________________ • HBr_____hydrobromic acid_________

  15. What do subscripts tell you in a chemical formula? How many of each atom there is in a chemical formula • What do coefficients tell you in a chemical formula? How many of each compound there is

  16. yields reactants product subscript coefficient

  17. Identify the number of atoms in each compound • CH4__5___ • AgNO3__5___ • Mg(NO3)2__9___

  18. What does the law of conservation of matter state? Why is it important for a chemical reaction to be balanced? • Matter cannot be created or destroyed in a chemical reaction. The same number of atoms must go in and come out of a chemical reaction

  19. What doe each of these letters mean after a compound in a chemical equation? • s - solid • l - liquid • g - gas • aq - aqueous

  20. Balance the following chemical equations. • _4__ P + __5_ O2 ___ P4O10 • ___ Mg + _2__ HCl ___ MgCl2 + H2 • ___ NaS + ___ ZnNO3 ___ NaNO3 + ___ ZnS

  21. What are the 5 types of chemical reactions? Give an example of each.

More Related