Naming bonds

Metal & non-metal ionic bond 1

Use the criss cross method - exchange the sides of the elements as subscripts

Covalent bond

Use prefixes according to the subscript of the element

Prefixes

Mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca

Groups 1,2,13-18

Have increasing number of valence electrons (1,2,3,4,5,6,7,8) except for helium, having 1 only

Ions

Charged elements (cations and anions)

Molecular formula

Writing the charges as subscripts next to the element

Isomers

Have same chemical properties but different physical characteristics (and same molecular formula’

Crystalline

Highly ordered structures that are repetitive

Amorphous

More random structures that don’t have a sharp melting point

Melting point

The temperature needed for a solid to become liquid

Melting

Solid to liquid

Freezing

Liquid to solid

Condensation

Gas to liquid

Sublimation

Solid to gas

Deposition

Gas to solid

Plasma

The 4th state of matter where a gas is ionized

Helium

A noble gas that doesn’t follow the octet rule

Mixture

A physical combination of two or more substances where each component retains its original properties and can be separated by physical means.

Compounds

elements in a fixed ratio, where the components lose their individual properties and can only be separated by chemical means.

Homogenous mixture

A mixture that’s uniform throughout and you can’t physically distinguish the components

Heterogenous

When you can physically distinguish the components

Alloy and solutions

Homogenous mixtures (metals / one is dissolved)

Suspensions heterogenous

These mixtures have larger particles that will settle out if left undisturbed, such as muddy water or orange juice with pulp

Colloids heterogenous

These mixtures have intermediate-sized particles that do not settle out easily, such as milk

Evaporation

Liquid to gas

Precipitation

Liquids released from clouds

Hydrocarbon molecular formula

CnH2n

Exothermic

When energy is released and the air particles become more compact

Endothermic

When energy is absorbed and particles become more free

What happens to temperature when facing phase change?

It remains constant, heat is the one being transferred

Boiling point

Boiling needs the vapor pressure of the liquid to equal atmospheric pressure, so it happens at a fixed temp and vaporizes. Evaporation can happen below boiling point.

Does potential energy increase in an endothermic process?

Yes, not kinetic energy