Flashcards for Ionic

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Flashcards for Ionic Metallic Bonding
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What particle is transferred in ionic bonding?

• Electron

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How do you identify an ionic formula?

• Metal Nonmetal

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How do you identify a covalent formula?

• All Nonmetals

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What do metals do?

• Metals lose electrons form positive ions.

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What do nonmetals do?

• Nonmetals gain electrons form negative ions.

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What are the properties of metals?

1. Luster
2. Good conductors of heat electricity
3. Malleable ductile
4. Low ionization energy low electronegativity
5. High mp, high bp low vapor pressure

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Why do atoms form bonds?

• To get the same electron configuration as the
  nearest noble gas.

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What is a chemical bond?

• Force of attraction that holds 2 atoms together.

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What are the properties of ionic compounds?

1. Hard, brittle
2. High melting point, high boiling point
3. Low vapor pressure
4. Poor conductors of heat
5. Solids do not conduct electricity at all
6. Melts solutions do conduct a current
7. Ions in solution react quickly

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What is the structure of ionic compounds?

• Crystal lattice lattice points are positive
  negative ions.

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Subscripts in formulas

• Tell how many atoms of that element are present.
  
• No subscript means 1.

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Empirical Formula

• Subscripts in chemical formula have smallest
  whole number ratio

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Empirical Formula

• Ionic compounds only have empirical formulas.

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Crystal lattice

• Regular, repeating pattern in 3 dimensions.

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Compounds are electrically

• Neutral.

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Writing formulas from the ions for binary
compounds.

• Write the ions, positive 1st.
• If the superscripts (charges) do NOT add to zero,
  criss-cross.
• Na1 S-2 becomes Na2S

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Molecular Formula

• Gives exact composition of molecule.

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What is the structure of metals.

• Crystal lattice all lattice points are positive
  ions.

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Delocalized electrons

• Valence electrons in metals are free to roam
  throughout the metal.

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Sea of mobile electrons

• Phrase used to describe valence electrons in
  metallic bonding.

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Metallic Bonds

• Formulas have metals only.

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Subscripts in chemical formulas

• Microscopic scale give atomic ratios
• Macroscopic scale give mole ratios

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Lewis Dot Structures for Ionic Compounds

• Have square brackets and charges. Charges add
  up to 0. Positive ion has no dots. Negative ion
  has 8 dots.

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Lewis Dot Structures for NaCl

• NaCl-

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Lewis Dot Structures for NaOH

• NaOH-

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Group 1 metals form

• 1 ions

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Group 2 metals form

• 2 ions

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Group 16 nonmetals form

• -2 ions

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Group 17 nonmetals form

• -1 ions

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Group 18 nonmetals form

• They dont form ions. There the noble gases!

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Binary Compounds

• Composed of 2 elements! (2 uppercase letters)

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Naming Binary Ionic Compounds Stock System

• Name positive ion 1st (metal).
• Name negative ion 2nd (nonmetal). Change ending
  to ide.
• If metal has more than 1 oxidation state, use
  Roman numeral to specify which.

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NaCl

• Binary Ionic Cmpd.
• Na has only 1 oxidation state.
• Sodium Chloride

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FeCl2

• Binary Ionic Cmpd.
• Fe has 2 possible oxidation states.
• Iron (II) chloride

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Fe(NO3)3

• Contains a polyatomic.
• Fe has 2 possible oxidation states.
• Iron (III) Nitrate

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Polyatomic Ion

• A group of covalently bonded atoms that carries a
  charge.
• Can form ionic bonds with other ions.
• Have names.

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NaNO3

• NO3 nitrate ion
• Sodium nitrate

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Cu(NO3)2

• NO3 nitrate ion
• Copper has more than one oxidation state.
• The copper here must have a 2 charge.
• Copper (II) nitrate.

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Cu2SO4

• SO4 sulfate ion
• Copper has more than one oxidation state.
• The copper here must have a 1 charge.
• Copper (I) sulfate.