Chemical Bonding and Structure (1/?)
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- Created on: 13-10-20 11:15
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- Chemical Bonding and Structure
- Ionic Bonding and Structure
- Bonding
- Electrons transferred from one atom to another to form ions
- Total number of electrons still the same
- Positive ions are metallic elements, and negative ions are non-metallic
- Between a metal and non metal
- Number of electrons lost is determined by the electron configuration
- aim for noble gas configuration
- Electrons transferred from one atom to another to form ions
- Ionic Crystals
- electrostatic attraction between ions
- No individual bonds, bonding extends uniformly throughout in all directions
- Physical Porperties
- High melting / boiling point
- solid at room temp.
- strong electrostatic attraction
- lattices with higher ionic charges have higher melting point as electrostatic attraction is stronger
- Low Volatility
- strong electrostatic attraction
- do not conduct in a solid but can in a liquid
- High melting / boiling point
- Bonding
- Covalent Bonding
- Single Covalent Bonds
- Electrons are shared
- Electrostatic attraction between nuclei and shared electrons
- Achieve a full outer shell
- Lewis Structure can be drawn to show electrons and bonds
- As atoms get bigger bond is weaker
- electron pair and nuclei are further away
- Electrons are shared
- Polarity
- Atoms do not attract the electron pair equally
- depends on electronegativity
- noble gases do not have electronegativity values and do not form compounds
- non-metals have a higher electronegativity than metals
- Small electronegativities = covalent. Large electronegativities = ionic
- Unsymmetrical distribution of electron density
- depends on electronegativity
- - shows negative end and + positive end
- Atoms do not attract the electron pair equally
- Multiple Covalent Bonds
- The more electrons shared the stronger and shorter the bond
- Attraction between nuclei and electrons is stronger
- The more electrons shared the stronger and shorter the bond
- Single Covalent Bonds
- Covalent Structures
- The Octet Rule
- Not always the goal when forming a covalent bond
- Elements in period 3 and beyond can expand the octet
- Coordinate Covalent Bonds
- Same qualities as normal bond
- Shown using an arrow
- Lewis Structures
- electron shown as dots and crosses, electron pairs shown as lines
- Most electronegative elements are the outer atoms
- except when hydrogen is present
- Molecules drawn within a bracket with charges in the top right outside
- Resonance Structures
- Bond have equal length
- Actual structure is a hybrid
- Bond have equal length
- Shapes of Molecules
- Use VSEPR theory
- Depends on electron domains in the outer shell
- lone pairs and bonded pairs
- 2 = linear; 3 = trigonal planar; 4 = tetrahedral
- First draw Lewis structure, then count electron domains and consider lone pairs
- Remember 3D
- Block triangles go out of the plane
- Shaded triangles go into the plane
- Remember 3D
- in molecules with more than 1 central atom, central atoms considered separately
- Depends on electron domains in the outer shell
- Use VSEPR theory
- The Octet Rule
- Ionic Bonding and Structure
- Soluble in water
- water is polar and there are ion-dipole attractions
- Physical Porperties
- High melting / boiling point
- solid at room temp.
- strong electrostatic attraction
- lattices with higher ionic charges have higher melting point as electrostatic attraction is stronger
- Low Volatility
- strong electrostatic attraction
- do not conduct in a solid but can in a liquid
- High melting / boiling point
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