General, Organic, and Biological Chemistry: General, Organic, and Biological Chemistry Final Flashcards

Volume

Weight

Potential energy

Kinetic energy

• Freezing water to make ice cubes
• tearing a piece of aluminum foil
• boiling water for soup
• melting gold to make jewelry

Amount of energy needed to raise the temperature of 1 g of the substance by 1 degree Celsius.

Homogenous mixture

Sublimation

Ethyl alcohol

Evaporation

D = Mass/Volume

C = (F - 32)/ 1.8

F = 1.8(C) + 32

K = C + 273.15

2.54 cm

1.06 qt

2.20 lbs

SG = Density/ Density of H2O (1.00g/mL)

Malleable

Ductile

Good conductors of heat and electricity

Atom

A proton has a positive charge and a mass of approximately 1 amu (atomic mass unit)

The mass number corresponds to the mass of the atom, that is obtained by adding the number of protons and neutrons present. The mass numbers appears under the element symbol in the elements table.

Increases going down within a group

The energy needed to remove the least tightly bound electron.

Atoms lose, gain, or share valence electrons to have 8 valence electrons.

Protons

Single covalent bonds do not give all of the atom in the molecule 8 valence electrons.

The greater the electronegativity difference, the more ionic the bond is.

Equal sharing of the bond electrons, arise when the electronegativities of the two atoms are equal

metals; cations

Dispersion forces

Is a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles

The energy that must be removed to turn 1 g of water at 0 degrees Celsius to 1 g of ice at 0 degrees Celsius.

The energy that must be added to turn 1 g of water at 100 degrees Celsius to 1 g of steam at 100 degrees Celsius.

1. Multiply given mass amounts by percentage sample. (mass 13.00 amu) makes up 1.07%. (mass 12.00 amu) makes up 98.93% 13.00(1.07%) = 13.91 12.00(98.93%) = 1187.16
2. Add the totals and divide by 100.
3. Sig Fig is 4 so answer is 12.01 from 1201.07

Energy = SH x mass x temperature change

example: 1.00 cal/g degrees Celsius(100.00 g)(100-25) = 7500 calories about 7.50x10 to the 3rd power

The energy needed to remove the least tightly bound electron from an atom.

Increases across a period and decreases down a group.

The number of each element on the reactant side equals the number of each element on the product side.

Two or more elements or compounds bond to form one product.

A reactant splits into two or more simpler products.

A reacting element switches place with an element in the other reacting compound.

The positive ions in the reacting compounds switch places.

A carbon-containing compound that is the fuel burns in oxygen from the air to produce carbon dioxide, water, and energy in the form of heat or flame.

Loss of electrons.

Gain of electrons.

One mole of any element always contains 6.02 x 10²³ atoms.

Example: Convert 4.00 moles of Fe atoms.

4.00 moles Fe atoms x 6.02 x 10²³ Fe atoms /1 mole Fe atoms = 2.41 x10²⁴ Fe atoms.

Energy is absorbed by the system.

1. Composed of very small particles
2. Gas particles move rapidly
3. Gas particles do not attract or repel one another
4. Gas particles move faster when the temperature increases

The forces of gas particles against the walls of a container.

1 atm = 760 mmHg

The volume of gas decreases when the temperature decreases.

Formula: V1/T1 =V2/T2

The pressure and volume of a gas have an inverse relationship, when temperature is held constant.

Formula: P1V1 = P2V2

The relationship between the pressure and temperature of a fixed mass of gas kept at a constant volume.

Formula: P1/T1 = P2/T2

The volume of a gas is directly related to the number of moles of a gas when pressure and temperature are not changed.

Formula: V1/n1 = V2/n2

22.4 L/mol

All the pressure-volume-temperature relationships for gasses combined to make a single relationship.

Formula: P1V1/T1 = P2V2/T2

The combination of the four properties used in the measurement of a gas-pressure (P), volume (V), temperature (T), and amount (n) to give a single expression.

Formula: PV = nRT

Rearranged, shows the 4 gas properties equal a constant R.

Formula: PV/nT = R

1 atm = 760 torr

1 mole of gas (STP) = 22.4 L

R = (1.00 atm)(22.4)/(1.00 mole)(273 K) = 0.0821 L x atm/ mole x K

Can be solid, liquid, or gas.

oil is nonpolar

The Na+ ions are attracted to the partially negative oxygen atoms of the water molecule.

Strong electrolyte

Multiply the amount of moles by the elements charge

Example: 5.0 moles of Ca²⁺ is 5.0 x 2 = 10 Eq

mass/volume x 100 = Answer%

More solute than the other.

Doing the dissolving.

Being dissolved.

A compound that is dissolved in water mostly a molecules.

The amount of a solute that can be dissolved in a given amount of solvent.

Rapidly dissolving when added to a solvent.

A base is a proton acceptor

A solution that contains all the solute that can dissolve which is the rate at which solute dissolves become equal to the rate at which solids form, also known as recrystallization.

A weak acid/base and its conjugate base/acid salt which reacts with small amounts of an acid or base to maintain pH at a constant value.

1. Solid dissolves
2. Gas formed
3. Precipitate formed
4. Heat released or absorbed
5. Color change

Examples: Changes in size or shape, changes in state, solid -> liquid -> gas

The pressure which is caused by 2 solutions with different solute concentrations separated by a semipermeable membrane.

It also causes water to flow from more concentrated to less concentrated.

Less solute than the other.

The minimum amount of energy required to break the bonds between atoms of reactants.

Is determined by measuring the amount of a reactant used up, or the amount of a product formed, in a certain period of time.

1. Temperature-higher temps. increase in kinetic energy makes the reacting molecules move faster.
2. Concentration of reactants-increases when the concentration of reactants increase.
3. Catalysts-another way to speed up a reaction is to lower the activation energy

The rate of the forward reaction is equal to the rate of the reverse reaction.

No further changes occur in the concentrations of the reactants or products; the forward and reverse reactions continue at equal rates.

Multiplies the concentrations of the products ad divides by the concentrations of the reactants.

A reaction in which all the reactants and products are gases.

When the reactants and products are in 2 or more physical states.

Contains mostly products.

Examples: 2 x 10¹¹, 1.1 x 10⁷, 1.6 x 10²

Contains mostly reactants.

Examples: 1.2 x 10^-2, 2 x 10^-9, 4.7 x 10^-14

States than when a system at equilibrium is disturbed, the system will shift in the direction that will reduce that stress.

• Substances that produces hydrogen ions (H⁺) when they dissolve in water.
• When dissolved in water it produces a hydrogen ion and a simple nonmetal anion.
• Prefix: hydro
• Ending in ide is changed to ic acid
• Polyatomic anion that ends in ite is replaced with ous acid
• Taste sour
• pH less than 7
• Turns blue litmus to red
• Acids neutralize bases producing salt and water
• Proton donors ( Proton H⁺ ion = hydrogen ion)
• Increases H ion concentration in solution
• Are electrolytes

• Are ionic compounds that dissociate into cations and hydroxide ions (OH^-) when dissolved in water
• Taste bitter, chalky
• pH greater than 7
• Turn red litmus blue
• Neutralize acids producing a salt and water
• Proton acceptors (H⁺ = hydrogen ion)
• Increase OH^- ion concentration in solution
• Are electrolytes
• Feel slippery

Consist of molecules or ions related by the loss of one H⁺ by an acid and the gain of one H⁺ by a base.

• Acting as a Bronsted-Lowry acid, HBr loses 1 H⁺ to form Br^-, which is a conjugate base.
• The NH₃, acting as a Bronsted-Lowry base, gains 1 H⁺ to form its conjugate acid NH₄ ⁺.
• The conjugate acid-base pairs are HBr/Br^- and NH₄ ⁺/NH₃

An acid or base separates into ions in water.

Donate hydrogen ions so easily that their dissociation in water is nearly complete.

Dissociates slightly in water, which means only a small percentage of H⁺ is transferred from a weak acid to H₂O, forming only a small amount of H₃O⁺

7

Identify the solution containing an acid or base.

Significant Figures.

Examples:

.010 M HCl (acid H₃O⁺) [H₃O⁺] = 1.0 x 10^-2

0.0100 M NaOH (base OH^-) [OH^-] = 1.0 x 10^-2 pH = 14 14-2 = 12.00

• Protective clothing
• Lead/Concrete shields
• Increase distance from source

OH^-

NH₄ ⁺

NO₃ ^-

NO₂ ^-

ClO₄ ^-

ClO₃ ^-

ClO₂ ^-

ClO^-

CO₃ ^-2

HCO₃ ^-

CN^-

C₂H₃O₂ ^-

SO₄ ^-2

HSO₄ ^-

PO ₄ ^-3

HPO₄ ^-2

H₂ PO₄ ^-2

PO₃ ^-3