Physical Science, Advanced

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Physical Science, Advanced

• Instructional Objective1.identify the
  difference between ionic and covalent compounds
• 2.Learn about the bonds

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Ions

• An atom with a charge.
• It can be positive or negative in charge.
• It can be obtain by loosing or gaining electrons.
  (Protons never change)

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Cations

• Are always positive in charge.
• Obtain by loosing electrons.
• Always going to be a metal
• Written using the symbol with a sign
• Ex. Na Proton 11, electron -10
• Roman numerals are used to show the charge of
  certain metals.
• Ex Fe 3 is named as Iron III

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Anions

• Are always negative in charge.
• Obtain by gaining electrons
• Always going to be a nonmetal
• Written using a symbol with a negative sign.
• Ex Cl (Proton -17 ,electron -18)

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What is an oxidation number?

• valence electron electron in the outermost
  energy level of an atom
• oxidation number number of electrons an atom
  gains, loses, or shares when it forms a chemical
  bond

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What is a chemical equation?

• chemical equation
• chemical formula that describe a chemical
  reaction
• coefficient
• number that shows how many molecules of a
  substance are in a chemical reaction
• Used to balance an equation

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Ionic Compound

• Metal and a nonmetal combined.
• Always a cation and anion
• Net charge will be zero.
• Named as metal first ,then the nonmetal that ends
  with ide,ite,ate.
• Ex. Sodium Chloride (Name)
• NaCl (Symbol)
• To write the symbol use the crisscross method to
  cancel the charges.
• Ex

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Metals with multiple ions

• Many transition metals have more than one
  oxidation number.
• It is always indicated with roman Numeral number.
• Ex Copper II
• Copper I
• Chromium II
• Chromium III

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Two types of ionic compounds

• Binary ionic compound
• Contain two elements
• Contain a metal and a nonmetal
• Ex NaCl

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Polyatomic ion

• is a group of atoms that acts as a single
  atom.
• have an overall electrical charge.
• atoms are held together by covalent bonds.
• If there is more than one polyatomic ion in a
  molecule, the polyatomic ion is written in
  parentheses.
• . End with ite or ate
• EX SO32- Sulfite (one less Oxygen than the
  ate) (Charge will be same)
• SO42- Sulfate (Charge will be same)

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3 Exceptions in the polyatomic ions

• Ammonium polyatomic cation that not ending with
  ite or ate ending
• NH4 - Ammonium
• NH3 -Ammonia
• Cyanide CN-
• Hydroxide OH-

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Ionic compound with polyatomic ions

• Contain a metal and a polyatomic ion
• Contain three or more elements
• Or contain a poly atomic cation and a nonmetal
• Or contain two polyatomic ions.
• Ex Na2 SO4 ( 3 elements)
• Ex Ca(SO4)2 (more than one polyatomic ions,
  you must use a parenthesis around it)

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Covalent Compounds (Molecular compounds)

• Always going to be nonmetals combined with
  nonmetals
• Identify or name using prefix for the number of
  atoms.
• Form molecules
• Weaker than ionic compounds

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Prefix for covalent compound

• Mono -1
• Di-2
• Tri-3
• Tetra-4
• Penta-5
• Hexta-6
• Septa-7
• Octa-8
• Nano-9
• Deca-10

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Chemical bonds

• are the force that join two or more atoms.
• A stable compound occurs.
• a net (total) attractive force between the atoms
  .

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Two types of bonds

• Covalent bond one or more pairs of electrons
  are shared by two atoms.
• Ionic bond one or more electrons from one atom
  are removed and attached to another atom.
• resulting in positive and negative ions which
  attract each other.

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Covalent Bonds

• involve the sharing of a pair of valence
  electrons by two atoms

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Ionic Bonds

• one or more atoms lose electrons and other atoms
  gain

                                                      
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Ionization energy

• The amount of energy used to remove an electron
  is known as the ionization energy
• Varies from element to elements
• Energy increases from left to right(less
  reactive)
• Energy decreases from top to bottom(easy to
  remove the electron, so it will be more reactive)
• Ex K is more reactive than Na

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Crystal Lattices

• formed by an ionic compound. the particles are
  arranged in a repeating pattern
• The attractions of the positive and negative ions
  keeps a fixed position in a frame work (lattice)
• ExLiCl

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(metal) (nonmetal)
CHARGE OF ATOM
CHARGE OF ATOM
neutral
neutral
Cl 17
Na 11
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(metal) (nonmetal)
CHARGE OF ATOM
CHARGE OF ATOM
neutral
neutral
Cl 17
Na 11
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(metal) (nonmetal)
CHARGE OF ATOM
CHARGE OF ATOM
neutral
neutral
Cl 17
Na 11
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(metal) (nonmetal)
CHARGE OF ATOM
CHARGE OF ATOM
neutral
neutral
Cl 17
Na 11
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(metal) (nonmetal)
CHARGE OF ATOM
CHARGE OF ATOM
neutral
neutral
Cl 17
Na 11
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(metal) (nonmetal)
CHARGE OF ion
CHARGE OF ion
negative
positive
Ionic Bond
(cation)
(anion)
Cl1- 17
Na 11
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(metal) (nonmetal)
CHARGE OF ion
CHARGE OF ion
positive
negative
Ionic Bond
(cation)
(anion)
Cl 1- 17
Na 1 11
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(metal) (nonmetal)
CHARGE OF ion
CHARGE OF ion
negative
positive
Ionic Bond
(cation)
(anion)
Cl 1- 17
Na 1 11
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(metal) (nonmetal)
CHARGE OF ion
CHARGE OF ion
negative
positive
Ionic Bond
(cation)
(anion)
Cl 1- 17
Na 1 11
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(metal) (nonmetal)
CHARGE OF ion
CHARGE OF ion
negative
positive
Ionic Bond
(cation)
(anion)
Cl 1- 17
Na 1 11
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(metal) (nonmetal)
CHARGE OF ion
CHARGE OF ion
negative
positive
Ionic Bond
(cation)
(anion)
Cl 1- 17
Na 1 11
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(metal) (nonmetal)
CHARGE OF ion
CHARGE OF ion
negative
positive
Ionic Bond
(cation)
(anion)
Cl 1- 17
Na 1 11
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What is a diatomic molecule?

• is made up of two atoms of the same element
• is usually held together by a covalent bond.
• Most gaseous elements form diatomic molecules.

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7 diatomic molecules

• Hydrogen( H2),
• Oxygen ( O2),
• Nitrogen (N2),
• Fluorine (F2),
• Chlorine(Cl2),
• Bromine (Br2)
• Iodine(I2)

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Metallic Bonds

• Is the attraction between a metal cation and the
  shared electrons that surround it
• More valance electrons in a metal-stronger the
  metallic bond