Chemistry chapter 13 notes

Solution

a homogenous mixture of 2 or more substances

Solute

The substances present in smaller amounts

Solvent

The substance present in the larger amount

For periodic table if element is in black then it should be a solvent!

True

alloy

a mixture of metals

solubility

the maximum amount of solute that dissolves in a specific amount of solvent

Saturated solution

Contains the max amount of a solute that will dissolve in a given solvent at a specific temperature

Unsaturated solution

Contains less solute than the solvent has the capacity to dissolve at a specific temperature

supersaturated solution

contains more solute than is present in a saturated solution at a specific temperature

Water is a universal solvent!

True

Molecular compounds = contains any non-metals!

True

Non-polar covalent bonds

Built between IDENTICAL non metals and electrons are shared EQUALLY

Polar covalent bonds

Built between DIFFERENT non- metals and electrons are shared UNEQUALLY

Two substances with similar intermolecular forces are likely to be soluble in each other!

True

Lewis structure have to follow the octet rule → 8 valence electrons present (there are some exceptions)

True

a non polar will never dissolve in a polar solute

True

Concentration

the amount of solute present in a given quantity of solvent or solution

aqueous solution

a solution where water is the solvent.

mole fraction

moles of A / sum of moles of all components

(M) Molarity

moles of solute / liters of solution

(m) molality

moles of solute / mass of solvent (kg)

Mass / volume percent

% (m/v) = g of solute / mL of solution x 100%

If no solvent is given always assume it is water (aq)

True

Percent by mass formula

%(m/m) = mass of SOLUTE/ mass of solute + mass of solvent x 100%

what units do you multiply / divide by 1000?

L ←→ mL

kg ←→ g

g ←→mg

m ←→ mm

what unit do you multiply / divide by 100

m ←→ cm

what unit do you multiply / divide by 10

cm ←→ mm

If you're going from a larger unit → smaller unit, you multiply! (EX: L → mL)

True

If you're going from a smaller unit → larger unit, you divide! (EX: kg → g)

True

Finding MOLALITY steps

• find the weight of each element

• add all together (equals one mole of the solution)

• divide the given mass by the mass of one mole

• covert mass of the water from kg to g ( divide)

• divide the moles of the solution by the gram of water

How can you tell if an intermolecular force is dipole - dipole?

Hydrogen bonding.

Hydrogen bonding requires a hydrogen atom directly bonded to nitrogen, oxygen, or fluorine.

Solubility decreases with increasing temperature!

True

Solubility increases as the pressure of the gas over the liquid increases!

True

calculating Molarity steps

• find the weight of each element

• add them together

• convenes grams of the solution into moles

• divide the moles by volume in liters