combined ionic metallic and covalent compounds
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Combined Ionic, Metallic and Covalent Compounds

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Combined Ionic, Metallic and Covalent Compounds. Everything together. Properties of Ionic Compounds. Electrons are transferred (Made of Ions) Metal and a Nonmetal present (except NH 4 + may be present) High Melting Points High Boiling Points Normally Solids at Room Temperature

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properties of ionic compounds
Properties of Ionic Compounds
  • Electrons are transferred (Made of Ions)
  • Metal and a Nonmetal present (except NH4+ may be present)
  • High Melting Points
  • High Boiling Points
  • Normally Solids at Room Temperature
  • Conduct electricity when liquid or dissolved
  • Normally dissolve in Water
properties of metallic compounds
Properties of Metallic Compounds
  • WILL NOT dissolve in water
  • Will conduct electricity when solid
  • Malleable and Ductile
  • Most Solids at well above room temperature
  • High Melting and Boiling Points
  • Made of Positive Ions and delocalized electrons
properties of covalent compounds
Properties of Covalent Compounds
  • Electrons are shared (no ions)
  • Only Nonmetals present (NH4+ will be ionic)
  • Low Melting Points
  • Low Boiling Points
  • Normally Gases and Liquids or solids at Room Temp
  • Don’t conduct electricity
  • Normally DON’T dissolve in water
molecules and compounds
Molecules and Compounds
  • MOLECULE: 2 or more atoms COVALENTLY Bonded. (Maybe the same element)
  • COMPOUND: 2 or more DIFFERENT atoms combined
  • MOLECULAR COMPOUND (Both): 2 or more DIFFERENT atoms COVALENTLY bonded.
ionic compounds
IONIC COMPOUNDS
  • A CATION combined with an ANION to form a neutral compound (formula unit)
    • NaCl, CuF2, Ca(NO3)2, (NH4)SO4
  • Normally has a metal and a nonmetal or one or more Polyatomic Ions.
  • Electrons are transferred and opposite charges bring the ions together.
covalent compounds
COVALENT COMPOUNDS
  • NO IONS are present
    • Except Polyatomic Ions themselves are covalent
  • Made up of NONMETALS only
  • Electrons are shared to complete Octets (8 electrons per atom) except H which gets 2 electrons
naming ionic compounds
NAMING IONIC COMPOUNDS
  • Name the Cation first
    • Groups 1, 2, Ag, Cd, Zn, Al and Ammonium get NO ROMAN NUMERIAL
    • All other Metals get a Roman Numerial which is the CHARGE
  • Name the Anion
    • Negative elements end in –ide
    • Polyatomics get their ate or ite
naming covalent compounds
NAMING COVALENT COMPOUNDS
  • Use Prefixes to state the number of each type of element present
  • DON’T use mon on the first element
  • LAST name ends in ide
terms
TERMS
  • ION: An atom or group of atoms that lost or gained electrons and has a charge
  • ANION: A negatively charged atom or group of atoms. Has gained one or more electrons
  • CATION: A positively charged atom or group of atoms. Has lost one or more electrons
more terms
MORE TERMS
  • OCTET RULE: All atoms need 8 valence electrons, Except H, He, Li, Be – 2 only
  • CHEMICAL FORMULA: A representation of a substance using symbols for its constituent elements
  • FORMULA UNIT: The smallest repeating unit of a substance. The molecule for nonionic substances. Also called the Empirical formula
even more terms
EVEN MORE TERMS
  • IONIC BOND: A chemical link between two atoms caused by the electrostatic force between oppositely-charged ions in an ionic compound.
  • COVALENT BOND: a chemical link between two atoms in which electrons are shared between them.
  • POLYATOMIC ION: Two or more nonmetals combined together with a charge (YOU MUST KNOW THE LIST)
again even more
AGAIN EVEN MORE
  • VALENCE ELECTRONS: an electron that is the most likely to be involved in a chemical reaction. They are typically the highest energy s and p electrons.
  • COMPOUNDS: 2 or more DIFFERENT atoms combined
  • MOLECULE: 2 or more atoms COVALENTLY Bonded
  • MONOATOMIC ION: An ion made up of only one type of element.
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