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Introduction to Chemistry for Allied Health Sciences Kirk Hunter Chemical Technology Department Texas State Technical College Waco. Chemical Bonding. Predicting Bond Type. Predicting Bond Type. Metallic character of the atoms Electronegativity. Metallic character of the atoms.

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Introduction to Chemistryfor Allied Health SciencesKirk HunterChemical Technology DepartmentTexas State Technical College Waco

predicting bond type1
Predicting Bond Type
  • Metallic character of the atoms
  • Electronegativity
metallic character of the atoms
Metallic character of the atoms
  • Metal + nonmetal  Ionic Bond
    • NaCl – ionic bond
  • Nonmetal + nonmetal  Covalent Bond
    • CO2 – covalent bond
trends
TRENDS
  • The Periodic Table can be used to predict trends.
    • Atomic radii
    • Metallic character
    • Ionization energy (electron affinity)
trends atomic radii
TRENDSAtomic Radii
  • Increases down a group
  • Increases from right to left
trends1
Trends

Atomic radius increases

example
Example

Which has a larger atomic radius, Na or K?

Answer:

Potassium, K is below sodium, Na in Group IA. Potassium’s atomic radius is larger.

example1
Example

Which has a larger atomic radius, Ca or Ni?

Answer:

Calcium, Ca, is to the left of nickel, Ni in Period 4. Calcium’s atomic radius is larger.

trends metallic character
TRENDSMetallic Character
  • Increases down a group
  • Increases from right to left
trends4
Trends

Metallic character increases

example2
Example

Which has the most metallic character, Sn or Pb?

Answer:

Lead, Pb, is below tin, Sn in Group IVA. Lead has more metallic character.

example3
Example

Which has the most metallic character, Ag or Sr?

Answer:

Strontium, Sr, is to the right of silver, Ag, in Period 5. Stronium has a more metallic character.

trends electronegativity electron affinity
TRENDSElectronegativity(Electron Affinity)
  • Increase – bottom to top of Group
  • Increase – left to right in Period
trends7
Trends

Electronegativity increases (Electron affinity)

example4
Example

Which has a higher ionization energy (electronegativity), Li or Na?

Answer:

Lithium is above sodium in Group IA. Lithium has a higher ionization energy (electronegativity).

example5
Example

Which has a higher ionization energy (electronegativity), N or O?

Answer:

Oxygen is to the right of nitrogen in Period 2. Oxygen has a higher ionization energy (electronegativity).