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Ionic Bonding Naming and formula writing. Mrs. Kay Chemistry 11 Read pages 158-168. Atoms of different elements have different numbers of electrons Each shell is filled up before electrons move to the next shell found further away from the nucleus

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ionic bonding naming and formula writing

Ionic BondingNaming and formula writing

Mrs. Kay

Chemistry 11

Read pages 158-168

slide2
Atoms of different elements have different numbers of electrons
  • Each shell is filled up before electrons move to the next shell found further away from the nucleus
  • Ex: Sodium has 2 e- on the 1st energy level, 8 e- on the 2nd energy level, and 1 e- on the 3rd energy level.

Sodium has 1 valence electron

valence electrons
Valence electrons
  • Period number indicates the number of electron shells
  • Group number indicates the number of valence electrons (look at the second digit of the group number)
trends
Trends:
  • Elements of the same group have similar chemical properties because they have the same number of electrons in their outer shell or valence shell
  • Group 1 metals reacting with water
reasons for reactions
Reasons for reactions
  • Group 18, the noble gases are the most stable of elements because their valence shell is full with electrons
  • Less energy required to support the atom
  • Other atoms react in attempt to achieve nobel gas configuration, same number of valence electrons as a noble gas.
lewis dot structures
Lewis Dot structures
  • Visual representation of an element and only its valence electrons
  • sodium, Na has 1 valence so it has 1 dot representing that electron. (group 1)
  • Chlorine, Cl has 7 electrons. (group 17)
  • Electrons get placed up along 4 sides of the element before they double up!
ionic bonding
Ionic Bonding
  • attraction between oppositely charged ions formed when metallic ions (+) transfer electron(s) to nonmetallic ions (-)
  • Difference of electronegativity greater than 1.7
  • Ex: NaCl
slide8
Not always 1:1 ratio, sometimes need to use subscript to show the number of atoms

Ex: CaCl2 The 2 is a subscript, it shows that 2 atoms of chlorine bond with one atom of calcium.

Zero Sum Rule: the charges need to add up to zero

simple ionic compounds
Simple Ionic Compounds
  • KBr
  • Name the metal first
    • Potassium
  • Name the non-metal next, end it with –ide
    • Bromine becomes bromide
  • Put together: Potassium bromide
practice
Practice
  • Na2O

Name the metal:

Sodium

Oxide

Name the non-metal:

  • Put them together to get: Sodium Oxide.
  • It takes two Na+ to combine with one O2- to observe the Zero Sum Rule!
slide12
If you’re given the name, can you write the formula?
    • Strontium nitride
    • Strontium is Sr2+
    • Nitride is N3-
    • We must combine them to be equal to zero
      • Need 3 Sr2+ to combine with 2 N3-
    • Answer is Sr3N2
multivalent ionic bonding
Multivalent Ionic bonding
  • Whenever the periodic table of ions has a split cell, we must choose or indicate which charge we are refering to in the chemical equation.
    • Look at Iron
    • There is an option of Fe2+ and Fe3+
    • FeO would be called Iron (II) oxide
      • It takes Fe2+ to balance out charges with O2-
      • We indicate the optional charge with roman numerals; 2= II, 3=III, 4=IV and so on
practice naming
Practice naming
  • FeCl2
  • MnO
  • Fe2O3
  • TiO2
  • Iron (II) chloride
  • Manganese (II) oxide
  • Iron (III) oxide
  • Titanium (IV) oxide
polyatomic ions
Polyatomic ions
  • Ions that are made of multiple atoms covalently bonded together.
  • We treat them like a unit or package
  • When we need more than one, must be put in brackets!!
  • Example: sulphate, SO42-
  • Aluminum sulphate = Al2(SO4)3
    • Because is Al3+ and SO42- must combine to Zero
practice16
Practice
  • NaOH
  • K3PO4
  • CsMnO4
  • Ca(HCO3)2
  • Cu(NO3)2
  • Sodium hydroxide
  • Potassium phosphate
  • Cesium permanganate
  • Calcium hydrogen carbonate
  • Copper (II) nitrate
homework
Homework:
  • Don’t forget to read over the textbook pages for furhter understanding
  • Work on handouts to continue practice with naming and proper formula writing (IUPAC = international naming method, what we learned)
test what you know here http science widener edu svb tutorial namingcsn7 html

Test what you know here:http://science.widener.edu/svb/tutorial/namingcsn7.html