Chem Final

Question 1

First law of thermodynamics

Answer 1

energy cannot be created or destroyed

Question 2

Second law of thermodynamics

Answer 2

the entropy of the universe is increasing

Question 3

Molarity

Answer 3

moles of solute/ L of solution

Question 4

molality

Answer 4

moles of solute/ kg solvent

Question 5

weight percent

Answer 5

(mass of compound x/ total mass) x 100% ( no units)

Question 6

aufbau principle

Answer 6

order filled in (think diagonal)

Question 7

pauli exclusion principal

Answer 7

no 2 electrons can have the same 4 quantum numbers

Question 8

Hunds rule

Answer 8

fill all with spin up before doubling up

Question 9

Pauling scores of fluorine, carbon, and hydrogen

Answer 9

F = 4.0, C = 2.5, H =2.1

Question 10

Combustion

Answer 10

A combustion reaction always has oxygen as one reactant

Question 11

Synthesis

Answer 11

A synthesis reaction is a chemical reaction where two reactants combine to create a new, more complex product.
A + B –> C

Question 12

Decomposition

Answer 12

AB –> A + B

Question 13

Double replacement

Answer 13

those in which two ionic compounds exchange their ions

Question 14

single replacement

Answer 14

a reaction in which one element is substituted for another element in a compound.

Question 15

precipitation

Answer 15

one in which dissolved substances react to form one (or more) solid products

Question 16

Acid- Base

Answer 16

look for a chemical reaction where one reactant (the acid) donates a hydrogen ion (H+) to another reactant (the base), typically forming water (H2O) and a salt as products

Question 17

redox

Answer 17

a chemical reaction that involves the transfer of electrons between two substances

Question 18

Third law of thermodynamics

Answer 18

change in S = 0 at 0 Kelvin for perfect crystalline solid
(the entropy of a system approaches a constant value as the tempreature approches absolute zero)

Question 19

omit solids and liquid when…

Answer 19

calculating q and k

Question 20

Le Chatelier principle

Answer 20

if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish an equilibrium

Question 21

Arrhenius Bronsted-Lowry

Answer 21

acid dissociates to produce hydrogen ions in water. A base produces hydroxide ions in water. In the Bronsted-Lowry theory, an acid is a proton donor. A base is a proton acceptor

Question 22

JJ Thompson

Answer 22

Cathode Ray experiment, discovered the electron, particles in the charged tube bent towards positive charged side

Question 23

Ernest Rutherford

Answer 23

gold foil experiment, fired particles at gold foil, some passed tyhrough other bounced off, conclusion that atoms have mass in the nucleus

Question 24

formal charge

Answer 24

= (# of valence electrons) - ( # of lone electrons) - (# of bonds)

Question 25

Heisenberg Uncertainty Principle

Answer 25

we cannot know the exact position and movement of an electron at any moment

Question 26

probability density function

Answer 26

the square of the wave function represents the probability of locating an e in a given region of an atom

Question 27

Fusion

Answer 27

melting –> solid to liquid

Question 28

Sublimation

Answer 28

solid to gas

Question 29

deposition

Answer 29

gas to solid

Question 30

When determining IMF

Answer 30

1) ionic
2) polar
3) FON
none? –> london dispersion

Question 31

molecular reaction

Answer 31

chemical species written as a whole compund of molecule

Question 32

complete ionic reaction

Answer 32

compounds that can dissociate into ions will do so +aquaese phase compounds dissociate into their component ions

Question 33

Net ionic reaction

Answer 33

cancel out spectator ions (appear in both reactant and product, present in reaction solution and do not participate in rxn)

Question 34

molecular reaction

Answer 34

exact number of each atom

Question 35

Empirical reaction

Answer 35

simplest ratio

Question 36

6 oxidation rules

Answer 36

1) the oxidation number of an element = 0
2) oxidation # of an ion = ions charge
3) oxidation # of Oxygen in compounds = -2
4) oxidation number of Hydrogen in covalent compounds = +1
5) Oxidation of halogens = -1
6) sum of each elements oxidation # = overall charge of molecule

Question 37

auto ionization of water

Answer 37

Kw at 25 C (Kw- 1 x 10^ -14)

Question 38

Enthalpy

Answer 38

(H) total heat of a system ( can be calculated using Hess Law, calorimetry, or bond energies)

Question 39

Entropy

Answer 39

(S) degree of disorder within a system ( can be calculated using products minus reactants formula or change in G formula if given G, H, and T)

Question 40

Buffers are made of

Answer 40

a weak acid and a conjugate base

Question 41

sigma bonds

Answer 41

of bonds

Question 42

pi bonds

Answer 42

double bond (count as one) triple bond (count as two) # of those

Question 43

Molecular rxn

Answer 43

normal equation

Question 44

complete rxn

Answer 44

complete expanded reaction with ions dissociated (aquase state AND strong acids)

Question 45

net ionic rxn

Answer 45

complete rxn

Question 46

Q > K

Answer 46

shift left towards reactants

Question 47

Q < K

Answer 47

shifts right towards products

Question 48

Q = K

Answer 48

equilibrium

Question 49

5% rule

Answer 49

The x term that we dropped must be less than 5%
of the number the assumption was made against

Question 50

equivilance point

Answer 50

the point at which the amount of titrant added is exactly enough to neutralize the analyte

Question 51

amphoteric

Answer 51

acts both as an acid and a base

Question 52

photoelectron effect

Answer 52

phenomenon where electrically charged particles are released from or within materials when it absorbs electromagnetic radiation.