KA4- Bonding Flashcards
Diatomic molecules
2 atoms share electrons
2 atoms covalently bonded together
Both atoms have an equal ‘pull’ on the shared electrons
They have the same electronegativity
Pure covalent bond/ non-polar covalent bond
Pure covalent bonding
Occurs in compounds where both atoms have the same electronegativity
Polar covalent bonding (polar molecules)
Atom with slightly higher electronegativity has a slight negative charge and the other has a slight positive charge
Atom with highest electronegativity attracts electrons more strongly than the other atom
Atoms with different electronegativity value form a covalent bond
Polar moles area attracted to other polar molecules by pdp-pdp interactions or brogan bonding
Ionic bonding
Atoms with a large difference in electronegativity
The attraction between the positive ions of one element and the negative ions of the other element
Doesn’t involve the sharing of electron
Occurs where electrons are transferred from one atom to another causing one atom to lose electrons (and become positively charged) and the other atom to gain electrons (and become negatively charged)
Metal+non-metal (metal has a low electronegativity value)
The bonding continuum
To figure out differences in bonding
The one with the greatest difference in electronegativity would usually be the most ionic/ covalent
Ionic bonding features
Conduct electricity when molten or when dissolved in water
Tend to have high melting points as a lot of energy is required to break the strong bonds that exist in the ionic lattice formed by such compounds in the solid state
Usually soluble in water
Held together in the solid state by covalent bonds
Covalent compound properties
Don’t conduct electricity
Smaller molecules have lower melting points and the larger molecules have higher melting points (varied)
Held together in the solid state by ionic bonds
Some held together in the solid state by forces of attraction known as van der Waals’ forces
Main types of van der Wals’ forces
London dispersion forces
Permanent dipole-permanent dipole interactions
Hydrogen bonding
London dispersion forces
Between all molecules and atoms
The only force between non-polar molecules and monatomic elements
The weakest attractive forces
Caused by the uneven distribution of moving electrons
Permanent dipole-permanent dipole interactions
Between polar molecules
Much stronger than London dispersion forces
Hydrogen bonding
Between polar molecules where a H atom is directly bonded to an N, O or F atom
Strongest
London dispersion forces explained
The side of the atom which has an excess of electrons becomes negative, causing the other side of the atom to become positive
The electrons in a neighbouring atom will shift away from an approaching negative causing a positive to appear- known as an induced dipole
Noble gases properties
Held together in the solid state by London dispersion forces
As you descend the noble gases, the melting point increases as it takes more energy to overcome the London dispersion forces between the atoms because of the number of electrons increasing
Permanent dipole-permanent dipole interactions explained
The permanent dipole in one … molecule is attracted to the permanent dipole in a neighbouring … molecule
Non polar molecules
Held together by London dispersion forces