Qbank test 1

Question 1

Rate equation

Answer 1

Intermediates are never in the rate law.

Question 2

Common ion effect

Answer 2

Will reduce the solubility of a solid.
Hinders product formation.
(Look up rule later in gen chem notes)

Question 3

Kinetic Energy of a particle/object

Answer 3

KE=1/2m(v^2)

Average KE is only dependent on temp. If molecules are at same temp, they have same KE. (differences in velocity account for mass differences)

Question 4

Gibbs free energy equation

Answer 4

Tells you whether rxn will be spontaneous

G=H - TS

Question 5

Laws of Thermodynamics

Answer 5

(1) Energy is conserved
U=Q-W
(2)Spontaneous rxns create entropy
(3)S=0 when T=0K (absolute zero)

Question 6

Adiabatic system

Answer 6

No heat transfer b/w system and environment.

Question 7

Removing electrons from d orbital

Answer 7

It is easier to remove electrons from the s orbital before removing from the d orbital.

n+l rule*

Question 8

Ideal gas law

Answer 8

PV=nRT

Question 9

Allotrope

Answer 9

Different forms of the SAME element.

If there is any change in the type of atoms “originally” present, it is not an allotrope.

Question 10

Two major factors that affect chemical rxns

Answer 10

Thermodynamics and kinetics.

Need to think about them BOTH when determining why something is happening.

Question 11

Heterogeneous vs homogeneous catalysis

Answer 11

Homo=reactants and catalyst in same state
Gives stable structures despite changes in coord. #

Hetero=reactants and catalyst in different states

Question 12

Zero, First, Second & Third order rate law

Answer 12

Sum of the exponents of the molecules in the rate equation give total order

Question 13

Oxidation rules

Answer 13

(1) Molecules in free form (H2, O2) have 0 oxidation #
(2) Oxidation of a monoatomic ion is its charge
(3) Sum of oxidation #’s in neutral compound is zero
(4) Oxidation # of grp IA=+1 and IIA=+2
(5) Oxidation # of H=+1 unless in binary metal hydride (-H2) where oxidation #= -1
(6) Oxidation # of O= -2; O= -1 in peroxides and O=+1 w/ Fluorine
(7) Oxidation of fluorine is -1; Cl, Br, I = -1 unless w/ F or O

Question 14

Catalysis

Answer 14

Alters the rate of a rxn but NOT it’s equilibrium.

Reduces activation E needed.

Question 15

Aufbau principle

Answer 15

Know how to determine electron configuration.

Fill lowest E orbitals first (build-up)

Question 16

Formal charge

Answer 16

Formal charge=grp# - (lone pairs) - # of bonds

Question 17

Review Titration curves

Answer 17

Equivalence pt=when mols of base equal mols of acid
Buffer regions= areas of small pH change
Polyprotic vs monoprotic (# of pKa’s)

Question 18

Amphoteric species

Answer 18

Compound that can act as an acid or base.

i.e. water

Question 19

Arrhenius acid/base

Answer 19

Acid=donates H+ to solution

Base=donates OH- to solution

Question 20

Bronsted Lowry acid/base

Answer 20

Acid=proton donor

Base=proton acceptor

Question 21

Lewis acid/base

Answer 21

Acid=electron acceptor

Base=electron donor (nucleophiles)

Question 22

Buffers

Answer 22

To prevent extreme pH changes.

Common ion effect

Question 23

Know how to interpret phase diagrams

Answer 23

Regions of solid, liquid, gas.

Critical pt=where phases can no longer be distinguished

Question 24

Hydrogen bonding

Answer 24

-FH, -OH, -NH

Increases melting pt and boiling pt

Question 25

Lattice energy

Answer 25

Generally decreases when either the cation OR anion increases in size.
Will not matter if both cation and anion increase in size at the same time.

Question 26

Types of reactions

Answer 26

Single displacement
Double displacement
Neutralization (acid/base)
Oxidation/reduction
Precipitation
Combustion (oxygen)
Combination
Disproportionation=opposite of combination

Question 27

Graham’s law of diffusion

Answer 27

(v1^2)MM1=(v2^2)MM2

Question 28

Strength of an ionic salt

Answer 28

Made of the most electropositive and electronegative elements (metal & nonmetal)

Question 29

Steps of a Free Radical Reaction

Write it out

Answer 29

3 steps
Initiation (radical formation)
Propagation (rxn can still go on)
Termination (stops rxn from going on)

Question 30

Oxidation vs reduction

Answer 30

Oxidation means becoming positive (losing electrons)

Reduction means becoming negative (gaining electrons)

Question 31

What environment do gases prefer?

Answer 31

Increased volume
Low pressure
Higher temp

Question 32

van der Waals equation

Answer 32

(P+(n^2 x a)/(V^2)) x (V-nb) = nRT

This equation is used when the gas being described is not ideal (high pressure and low temp)

Question 33

Solubility rules

Answer 33

(1) All alkali (IA) salts soluble
(2) All NH4+ salts soluble
(3) All Cl-, Br-, I-soluble EXCEPT Ag+, Pb+, Hg2 2+
(4) All SO4 2- soluble EXCEPT Ca2+, Sr2+, Ba2+, Pb2+
(5) All oxides insoluble EXCEPT CaO, SrO, BaO, alkali
(6) All OH- insoluble EXCEPT Ca2+, Sr2+, Ba2+, alkali
(7) All CO3 2-, PO4 3-, S2-, SO3 2- insoluble EXCEPT alkali, NH4+
(8) All Na+, NO32- salts soluble

Question 34

H+ conc. and pH equation

Answer 34

pH= -log [H+]

Question 35

Osmotic pressure equation

Answer 35

osmotic pressure (pi symbol thing) = MRT

R=0.0821

Question 36

Electrolysis equation

Answer 36

mass of material = it/nF x formula weight of material

n=moles of electrons transferred

Question 37

Avogadro’s volume

Answer 37

at STP = 22.4 L/mol

Question 38

Know how to balance half reactions

Answer 38

Will not always get the reaction in the passage.

This affects the moles of electrons you are dealing with

Question 39

Charge density

Answer 39

First determined by the charge an ion does or does not have.

If two ions have same charge then whichever is smaller (hold electrons more tightly) will have greater charge density.

Question 40

Heating curves

Answer 40

Review them.

Slope=change in T/q

Question 41

Ksp

Answer 41

Increases with increased temperature (generally)

Question 42

STP

Answer 42

1 atm
0 C or 273 K
22.4 L/mol

Question 43

Vibrational frequency of bonds

Answer 43

Depends on the masses of atoms involved (m) and the bond strength (k)

f=(1/2pi) x sqrt(k/m)