Intermolecular Forces And Metallic Bonding

Question 1

True or false? Metallic elements can’t conduct electricity when solid.

Answer 1

False.

Question 2

What are metals made of?

Answer 2

Positively charged ions

Question 3

What happens when you heat metal?

Answer 3

It vibrates.

Question 4

What happens when you hit metal with a hammer?

Answer 4

Dents and changes form.

Question 5

Most malleable metal?

Answer 5

Ae

Question 6

What the only metal that’s liquid at room temperature?

Answer 6

Mercury

Question 7

How can metallic bonding occur?

Answer 7

Positively charged ions are surrounded by a sea of delocalised electrons.

There’s a strong force of attraction between positive nuclei and delocalised electrons.

Question 8

Scale of strength of types of bonding?

Answer 8

Metallic bonding force is weaker than covalent and ionic bonding force.

Question 9

Properties of metal?

Answer 9

Conduct electricity
Conduct heat
Ductile
Malleable

Question 10

What is an electric current?

Answer 10

Flow of charged particles.

Question 11

Why can electronic conductivity occur?

Answer 11

Metals charged particles which are delocalised Valence electrons are free to move through the 3d lattice of metal ions.

Question 12

True or false? Connecting a battery across a piece of metal causes electrons to move.

Answer 12

True.

Question 13

What are the features for how electrons flow?

Answer 13

(-) 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).

Question 14

What is thermal conductivity?

Answer 14

Measures substances heat flow when one part of substance is maintained at high temperature.

Question 15

True or false? As metals temperature increases so does electrons kinetic energy and so does metal ions vibrational energy.

Answer 15

True!

Question 16

What is thermal conductivity?

Answer 16

Measures substances heat flow when one part of substance bis maintained at a higher temperature.

Question 17

How is energy conducted through metal?

Answer 17

More energetic electrons in metal collide with slower less energetic ones and speed them up.

Question 18

How do metals deform?

Answer 18

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.

Question 19

What do intermolecular forces affect?

Answer 19

How substances behave.

Question 20

What are the three types of intermolecular forces?

Answer 20

London dispersion forces
Dipole-dipole forces
Hydrogen bonding

Question 21

Details on London dispersion forces.

Answer 21

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.

Question 22

Details on permanent dipole - dipole forces.

Answer 22

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.

Question 23

Details on hydrogen bonding.

Answer 23

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.