Intermolecular Forces And Metallic Bonding Flashcards
True or false? Metallic elements can’t conduct electricity when solid.
False.
What are metals made of?
Positively charged ions
What happens when you heat metal?
It vibrates.
What happens when you hit metal with a hammer?
Dents and changes form.
Most malleable metal?
Ae
What the only metal that’s liquid at room temperature?
Mercury
How can metallic bonding occur?
Positively charged ions are surrounded by a sea of delocalised electrons.
There’s a strong force of attraction between positive nuclei and delocalised electrons.
Scale of strength of types of bonding?
Metallic bonding force is weaker than covalent and ionic bonding force.
Properties of metal?
Conduct electricity
Conduct heat
Ductile
Malleable
What is an electric current?
Flow of charged particles.
Why can electronic conductivity occur?
Metals charged particles which are delocalised Valence electrons are free to move through the 3d lattice of metal ions.
True or false? Connecting a battery across a piece of metal causes electrons to move.
True.
What are the features for how electrons flow?
(-) terminal of a battery = (-) potential = surplus of electrons. (Electrons are negatively charged so move away from (-) potential to a positive potential).
(+) Terminal of a battery = (+) potential = surplus defeciet of electrons.
Electron flow is (-) > (+) terminal (as they are attracted to + charge).
What is thermal conductivity?
Measures substances heat flow when one part of substance is maintained at high temperature.
True or false? As metals temperature increases so does electrons kinetic energy and so does metal ions vibrational energy.
True!
What is thermal conductivity?
Measures substances heat flow when one part of substance bis maintained at a higher temperature.
How is energy conducted through metal?
More energetic electrons in metal collide with slower less energetic ones and speed them up.
How do metals deform?
Metal ions in solid structure slide past each other - happens as sample shape changes because slippage occurs due to internal arrangement of ions and delocalised electrons.
What do intermolecular forces affect?
How substances behave.
What are the three types of intermolecular forces?
London dispersion forces
Dipole-dipole forces
Hydrogen bonding
Details on London dispersion forces.
Weak
Between non-polar covalent molecules
Occurs when molecules electron distribution becomes non-symetrical. One end is more negative and one end is more positive.
Causes temporary diopole
Can disturb electrons in nearby molecule
Repelling electrons and inducing a dipole in that molecule.
Details on permanent dipole - dipole forces.
Permanent forces between polar molecules. That have a permanent positive and negitive charge.
Oppositely charged ends attract each other
Stronger than London dispersion forces but weaker than covalent bonding.
Details on hydrogen bonding.
Strongest form of intermolecular force
Type of dipole - dipole bond
Due to large difference in electronegativity between hydrogen and flourine, oxygen and nitrogen.
Means due to large difference very polar bonds are formed. So molecules have permanent dipoles.
When 2 of these molecules are together attraction between positive end of one and lone pair of electrons on other. This is s hydrogen bond.
