Chemistry (Ionic Compounds, Bonds, & Naming)

• :Ionic bonds form due to electrostatic attraction between oppositely charged ions.
• Metals lose electrons to form cations, while non-metals gain electrons to form anions.
• In an ionic bond, electrons are transferred from one atom to another.
• In an ionic bond, electrons are transferred from one atom to another.
• Anions have negative charges because they have gained electrons.
• Cations have positive charges because they have lost electrons.
• A compound is formed when two different elements chemically combine.
• An ion with a positive charge is called a cation
• An ion with a negative charge is called an anion.
• Octet Rule explains that you must have eight valence electrons to form a stable atom.
• Ions with less than four valence electrons loses electrons to form a positive ion
• Ions with more than four valence electrons gain electrons to form a negative ion.
• The name of an anion of a nonmetallic element is not the same as the element and end in -ide.
• An ionic compound is a compound composed of cations and anions.
• Ionic compounds are electrically neutral.
• Covalent bonds occur between two atoms when they share one or more pairs of electrons.
• A formula unit is the lowest whole number ratio of ions in an ionic compound.
• Most ionic compounds are crystallize solids at room temperature.
• A crystal is a substance in which ions are arranged in repeating three dimensional patterns.
• Ionic compounds generally have high melting points due to the strong attractive forces between ions of opposite charges.
• Ionic compounds are highly soluble in water.
• Ionic compounds conduct electric current if they are dissolved in water, or melted into a liquid form; the ions are free to move about in the solution when dissolved.
• What is the formula for Calcium Chloride: CaCl2
• What is the formula for Calcium Phosphate: Ca3(PO4)2
• What is the name of the compound Mg3N2? Magnesium Nitride
• What is the name of the compound CaBr2: Calcium Bromide
• The coordination number of an ion is the number of ions of opposite charge that surround the ion in a crystal.
• Metallic Bonds are bonds formed between two or more cations (metals).
• Valence electrons are de localized so they move around and are shared by ALL atoms.
• Metallic bonds are forces of attraction between the free-floating valence electrons and the positively charged metal ions.
• When a metal is subjected to pressure the metal cations easily slide past one another.

  If a ionic crystal is struck, the blow tends to push the positive ions close together.
• Alloys are mixtures of two or more elements. At least one of which is a metal.
• Alloys are important, because their properties are often superior to those of their component element. The most important alloy is steel.
• Steels have a wide range of useful properties, such as corrosion resistance, ductilty, hardness and toughness.
• Most transition metals and group 4 metals form two or more ions, except: Zn2+, Ag+, Cd2+. they only form one ion.
• The name of metals with two or more positive ions use a Roman numeral to identify ionic charge.
• What is the name of the compound SnO?

  Tin(II) oxide
• What is the name of the compound FeCl2?

  Iron (II) Chloride
• what is the formula of Iron (III) Sulfide?

  Fe2S3
• What is the formula of Copper (II) Oxide?

  CuO