Chapter 2 - Bonding And Structure Flashcards
What’s ionic bonding
(2)
Between ?
Ionic bonding is - electrostatic attraction between OPPOSITELY CHARGED IONS
-non metal & metal
What makes an ionic bond stronger ?
2
- increase in charge
- short radius
Trends in ionic radius as you go down
-charge
-charge density
(3)
- RADIUS INCREASES
- charge is the same
- charge density decreases
What is a covalent bond ?
3
- electrostatic attraction
- between 2 nuclei
- shared PAIR of electrons between them
What the structure of a metal ?
- Giant lattice
- positive ions
- delocalised
What’s the bonding in a metal ?
2
- ELECTROSTATIC ATTRACTION between positively charged ions and seas of delocalised electrons
What’s causes short bond length and greater bond strength ?
4
- shorter BOND LENGTH = stronger
Triple =storter and stronger
-greater electron density
-greater force of attraction to nucleus from bonding pair of electrons
=shorter bond length hence stronger bond strength
How are shapes of molecules decided ?
3
- repulsion between electron pairs
: minimum repulsion
-maximum distance away from each other
What’s electronegativity ?
2
- ability for an atom to attract the electrons in a covalent bond towards itself
How do you know if something is polar ?
2
Electronegativity difference is MORE THAN 0.4
X>0.4
Which intermolecular force is effected by the electronegativity ?
(2)
-PERMANENT DIPOLE DIPOLE
How can a molecule with polar bonds be non -polar?
2
- they cancel out due to symmetrical shape
What are the three intermolecular forces ?
3
- vdw
- permanent dipole dipole
- Hydrogen bonds
What are vdw forces ?
What effects it ?
(4)
- forces between electrons
- more electrons increase vdw
- long straight alkanes = more London forces (large SA in CONTACT WITH MOLECULE)
Permanent dipole dipole definition. ???
1
-intermolecular force between polar substances