intermolecular forces part 3

What are intermolecular forces

Is used to describe how molecules react with each others they determine the state of matter and chemical properties

What’s a difference between intermolecular forces and intramolecular forces

Intermolecular forces are weaker

What are London dispersion forces

It’s the weakest force, where the e- is attracted to the others nucleus, and is always present

When does London dispersion occur?

when two nonpolar molecules attract and form a temporary dipole as electron cloud shift due to electrostatic attraction and repulsion

What is electrostatic forces

An attraction or repulsion between charge particles

How does atomic number affect LDF

The higher the atomic number the stronger the force is

What happens when LDF is only present

Substances will have a low MP and BP

In LDF when will substances have a high MP and BP? (Hint:chain)

More charge-more attraction- stronger force-more energy needed-higher MP and BP

And also when theres more e-

What is a dipole dipole interaction?

It occurs when two polar molecules come together, and the opposite partial charges are attracted

How to type or dip forces affect boiling and melting points

Stronger attraction leads to higher melting and boiling plants

what is hydrogen bonding?

It’s a specific strong type of dip dip interaction involving hydrogen

When does hydrogen bonding occur?

Occurs from attraction forces between hydrogen is covalently bonded with very electronegative atoms, nitrogen, oxygen and fluorine

Does hydrogen bonding have a low melting and boiling point or high melting and boiling point

They have a high melting and boiling point due to strong attraction

Why does melting point increase down the halogens?

Larger atomic radius → more electrons → stronger London dispersion forces.

Why does melting point decrease down the alkali metals?

Larger atomic radius → weaker metallic bonding

How can you tell the reactivity of metals?

You can use ionization energy because metals lose electrons to react so the lower the ionization energy, the more reactivity

How to tell the reactivity of nonmetals

You can use electronegativity because nonmetal gain/share electrons to react to the higher, the electronegativity the more reactive it is

the melting temperatures of the noble gases increase going down the periodic table because?

More electrons and stronger london force

the reactivity of the alkali metals increases going down the periodic table because?

The lower the IE the higher the reactivity for metals

the reactivity of the noble gases increases going down the periodic table because?

Larger AR and electrons are easier to remove

The melting temperature of alkali metals decrease going down the periodic table because?

Larger AR causes weaker metallic bonding

the reactivity of the halogens decreases going down the periodic table.

The lower the EN the less reactive it is and vise versa