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Chem 101 ๐Ÿ™ƒ > ๐Ÿ‘จ๐Ÿปโ€๐ŸŽจ > Flashcards

๐Ÿ‘จ๐Ÿปโ€๐ŸŽจ Flashcards

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1
Q

Solubility rules 1

A

(Li+) (Na+)(K+)(Rb+)(Cs+)(NH4)

soluble no exceptions!!!

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2
Q

Solubility rule 2

A

(No3-)(C2H3O2-)(CH3COO-) are all soluble

No exceptions!!!!

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3
Q

Solubility rule 3

A

Cl- Br- I-
Are soluble
Except when bound to
Ag+ Hg2 2+ or Pb 2+

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4
Q

Solubility rule 4

A 
SO4 2- is soluble except when bound to 
Ca 2+
Sr 2+
Ba 2+
Hg2 2+
Pb 2+
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5
Q

Solubility rule 5

A

All other compounds are practically insoluble

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6
Q

Soluble trends

Heat and pressure for solids

A

As heat increase solublilty also increases

Pressure has no particular change

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7
Q

Solubility trends for gases

A

As temp increases solubility decreases!!!!!!

As pressure increases solubility also increases!!!!

Think CO2 in soda pop

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8
Q

Molarity

A

Moles / L of solution

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9
Q

Mass percent

A

g of solute / g of solution x 100%

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10
Q

Dilution or concentration formula

A

M1V1=M2V2

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11
Q

Equilibrium constant expression

A

Keq = [c]^c x [D]^d / [A]^a x [B]^b

Only for aqueous or gases

aA + bB <=> cC + dD

The brackets indicate concentrations molarity

If a given equation is at equilibrium at the same temperature the keq will always be the same

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12
Q

What is a precipitation reaction

A

When two aqueous compounds forma solid

It will occurs if one of the products is a solid or insoluble

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13
Q

Complete ionic equation

A

All ions and soluble things are broken apart into ions

Insoluble things are not!!!!

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14
Q

Spectator ions

A

Ions that donโ€™t change

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15
Q

Net ionic equation

A

Does not contain the spectator ions

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16
Q

Energy

A

The ability to do work

17
Q

Jules to calories ratio

Calorie to kilocalories

A

4.184 Jules for 1 calorie (lower case)

1 Calorie or kilocalorie = 1000 calories

18
Q

System
V
Surrounding

A

The part of the universe being studied (generally the reaction being studied)

V

Everything else

19
Q

Law of the conservation of energy

A

Energy can neither be created or destroyed

20
Q

Heat

A

Is the transfer of energy from one โ€œbodyโ€ to another due to a difference of temperature

21
Q

^H or the change of enthalpy

A

Is equal to heat at a constant pressure

22
Q

Endothermic

V exothermic

A

Endo = +^ = products have more energy then reactants

Exo = -^ = products have less energy then reactants

23
Q

Colisiรณn theory

A

Desired product only forms if effective collision forms

The collisions gives the particles the energy they need to break up and form bonds

24
Q

Increase concentration

A

More collisions

Increase rate of reactions

25
Q

Temp and collisions

A

As temp increases it will increase number of collisions and increase the energy of the reactions

Right shift of the curve

26
Q

Activation energy

A

E(a)
The minimum kinetic energy required by a collision of reactants to create the desired products

Energy of reactants to the top of the hump

27
Q

Catalyst

A

Reduces the height of the hump ( Ea) which speeds up the reaction
(Shifts dotted line to the right)

Is not consumed instead it facilitates the reaction

(HAS NO EFFECT On LE Chatliers )

28
Q

Equilibrium

A

Many (not all) chemical equations are reversible - they can both forward or backwards

The reaction does not stop !!!!!
But when rate forward and backward are equal it has reached equilibrium

Does not have to have the same amount on both sides

๏ฟผ

29
Q

Le chatliers principal

A

Equilibrium can be shifted by changing conditions of the system

If the equilibrium is stressed it will temporarily not be at equilibrium but will the shift to remove the stress so it can regain equilibrium

30
Q

Stresses include

A

Change in concentrations of reactants or products (does not change keq)

Change in pressure

Change in temp ( exothermic written with products, endo written with reactants)

Not no bad (catalyst) ๐Ÿ˜ต

31
Q

How pressure causes a shift

A

Only gas !!!

If increased will shift from high to low to balance

If decreased will shift from low to high to balance

32
Q

Not soluble solubility rules 1 ๐Ÿ˜’

A

Co3 2- is not soluble except when

Bound to NA li k rb cs nh4

33
Q

Saturated
Unsaturated
Supersaturate

A

Saturated is max amount of solute dissolved in solvent

Unsat < max
Super > max

34
Q

Solute vs solvent

A

Solvent major
Solute minor

Types of mixtures
Solid liquid or gas / liquid

Solid / solid

Liquid / liquid

Polar dissolves in polar

Non polar in non polar

35
Q

Dissociation

A

When an ionic compound splits apart into ions in an aqueous solution

36
Q

Hydrated

A

When an ion is completely surrounded by water

37
Q

Electrolyte

A

Any substance that can divide into ions when placed in water

38
Q

Not soluble rule 2

A

Oh is not soluble except when bound to li NA k Rb Cs NH4 Sr Ba

Chem 101 ๐Ÿ™ƒ (6 decks)

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