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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.

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slide2

Ionic – between metal and nonmetal and transfers electrons

  • Covalent – between two nonmetals and shared electrons
slide6

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
slide7

Determine whether these compounds are ionic or covalent.

    • NaCl- ionic
    • CH4 - covalent
    • CaCl2 - ionic
    • NH3 - covalent
    • Al2O3 - ionic
slide8

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__________
slide9

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_______________
slide10

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____
slide12

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______
slide13

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________
slide14

Write the name of each acid. (Hydro- + stem name of element + -ic + acid)

    • HCl____hydrochloric acid________________
    • HF _____hydrofluoric acid_________________
    • HBr_____hydrobromic acid_________
slide15

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
slide16

yields

reactants

product

subscript

coefficient

slide17

Identify the number of atoms in each compound

    • CH4__5___
    • AgNO3__5___
    • Mg(NO3)2__9___
slide18

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
slide19

What doe each of these letters mean after a compound in a chemical equation?

    • s - solid
    • l - liquid
    • g - gas
    • aq - aqueous
slide20

Balance the following chemical equations.

    • _4__ P + __5_ O2 ___ P4O10
    • ___ Mg + _2__ HCl ___ MgCl2 + H2
    • ___ NaS + ___ ZnNO3 ___ NaNO3 + ___ ZnS
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