Chemistry

Question 1

Electron Configuration (Periodic Table)

Answer 1

S,P,D,F

Question 2

Polar Covalent Bond

Answer 2

Bonding electron pair is not equally shared.

Pull toward more electronegative atom

Question 3

Geometry of molecules

Answer 3

Regions of electron density
2=linear, 180
3=bent,120
4=tetrahedral,109.5
5=trigonal bipyrimidal, 90,120,180
6=octahedral, 90,180

Question 4

Intermolecular Forces

Answer 4

Hydrogen bonding
Dipole-Dipole Interactions
Dispersion Forces

Question 5

Hydrogen Bonding

Answer 5

The partial positive charge of hydrogen atom interacts with partial negative charge located on electronegative atoms (F,O,N) of nearby molecules

Question 6

Dipole-Dipole

Answer 6

Polar molecules orient themselves so that the positive region of one molecule is close to the negative region of another molecule

Question 7

Isothermal Process

Answer 7

Temperature of system remains constant

Question 8

Adiabatic Process

Answer 8

No heat exchange occurs

Question 9

Isobaric Process

Answer 9

Pressure of system remains constant

Question 10

Isovolumetric(Isochoric)

Answer 10

Volume remains constant

Question 11

Heat

Answer 11

Transfer of thermal energy from one object to another

Question 12

Endothermic

Answer 12

Reactions that absorb thermal energy

Question 13

Exothermic

Answer 13

Reactions that release thermal energy

Question 14

Enthalpy (H)

Answer 14

Used to express heat changes at constant pressure

Question 15

Standard heat of formation

Answer 15

Delta Hf
The enthalpy change that would occur if one mole of a compound was formed directly from its elements in their standard states

Question 16

Standard heat of reaction

Answer 16

Delta Hrxn
Hypothetical enthalpy change that would occur if the reaction were carried out under standard conditions

=Sum of Delta Hf of products - Sum of Delta Hf reactants

Question 17

Hess’s Law

Answer 17

Enthalpies of reactions are additive

Reverse of any reaction has an enthalpy of same magnitude as forward reaction, but with opposite sign

Question 18

Bond Dissociation Energy

Answer 18

Average of the energy required to break a particular type of bond in one mole of gaseous molecules

Question 19

Bond Enthalpy

Answer 19

Standard heat of reaction can be calculated using bond dissociation energies of particular bonds (given from table)

Delta Hrxn= Sum Delta H bonds broken - Sum Delta H bonds formed

Question 20

Entropy (S)

Answer 20

Measure of distribution of energy throughout a system

Delta S= Delta Ssystem + Delta Ssurroundings

Question 21

Gibbs Free Energy (G)

Answer 21

Combines 2 factors that affect the spontaneity of a reaction. Changes in enthalpy and entropy

Detla G= Delta H-T Delta S

Question 22

If G is negative the reaction is

Answer 22

Spontaneous

Question 23

If G is positive the reaction is

Answer 23

Non-Spontaneous

Question 24

If G=0 the reaction is

Answer 24

At equilibrium and Delta H=T delta S

Question 25

At a moderately high pressure a gasses volume is...

Answer 25

less than would be predicted by ideal gas law due to intermolecular attraction

Question 26

Boyles Law

Answer 26

k=PV or P1V1=P2V2

Question 27

Charles Law

Answer 27

k=V/T or V1/T1=V2/T2

Question 28

Gay-Lussac;s Law

Answer 28

k=P/T or P1/T1=P2/T2

Question 29

Combined Gas Law

Answer 29

P1V1/T1=P2V2/T2

Question 30

Ideal gas law

Answer 30

PV=nRT

Question 31

Arrhenius Definition

Answer 31

An acid is a species that produces excess H+ in an aqueous solution and a base is a species that produces extra OH-

Question 32

Bronsted Lowry Definition

Answer 32

An acid is a species that donates protons while a base is a species that accepts protons

Question 33

Lewis Definition

Answer 33

An acid is an electron pair acceptor and a base is an electron pair donor

Question 34

pH=?

Answer 34

pH=-log[H] = log(1/[H+]

Question 35

pOH=?

Answer 35

pOH=-log[OH] = log(1/[OH-])

Question 36

Kw=?

Answer 36

Kw=[H+][OH-] = 10^-14

Question 37

pH+pOH=?

Answer 37

pH+pOH= 14

Question 38

Ka=?

Answer 38

[H3O+][A-]/[HA]

Question 39

Kb=?

Answer 39

[B+][OH-]/[BOH]

Question 40

Salt Formation

Answer 40

Acids and bases may react with each other, forming a salt and often water in a neutralization reaction HA+BOH--->BA+H2O

Question 41

Hydrolysis

Answer 41

The reverse reaction where salt ions react with water to give back the acid and the base

Question 42

Amphoteric Species

Answer 42

One that can act either as an acid or base depending on its chemical environment

Question 43

Henderson-Hasselback Equation

Answer 43

pH=pKa+log[conjugate base]/[weak acid] pOH=pKb+log[conjugate acid]/[weak base]

Question 44

Oxidation

Answer 44

Loss of electrons Fewer Bonds to Hydrogen More bonds to heteroatoms (O,N, halogens) Typically goes from OH to O

Question 45

Reduction

Answer 45

Gain of electrons More Bonds to Hydrogen Fewer bonds to heteroatoms Typically goes from O to OH

Question 46

Oxidizing Agent

Answer 46

Causes another atom to undergo oxidation and is itself reduced High affinity for electrons (O2, O3, Cl2)

Question 47

Reducing Agent

Answer 47

Causes another atom to be reduce and is itself oxidized Good reducing agents include sodium, magnesium, aluminum, and zinc Low electronegativities and ionization energies

Question 48

Gibbs free energy in electrolytic cells

Answer 48

Delta G= -nFEcell Ecell=electromotive force

Question 49

Nucleophile

Answer 49

Nucleus Loving | Tend to have lone pairs or pi bonds that can form new bonds to electrophile

Question 50

Electrophile

Answer 50

Electron Loving Tend to have a positive charge or positively polarized atom that accepts an electron pair form a nucleophile

Question 51

Enantiomers

Answer 51

Non-superimposible mirror images Have opposite stereochemistry at every chiral carbon Same chemical and physical properties

Question 52

Diastereomers

Answer 52

Non mirror image stereoisomers | Have different chemical and physical properties

Question 53

Thin Layer Chromatography (Use, Mobile and Stationary Phase)

Answer 53

Identify a sample Mobile Phase: Nonpolar solvent Stationary Phase: Polar solvent

Question 54

Reverse Pahse (Use, Mobile and Stationary)

Answer 54

Identify a sample Mobile Phase: Polar solvent Stationary Phase: Nonpolar solvent

Question 55

Column Chromatography

Answer 55

Separates a sample into components Mobile: Nonpolar solvent Stationary: Polar gel or powder

Question 56

Ion Exchange Chromatography

Answer 56

Separates components by charge Mobile: Nonpolar solvent Stationary: Charged beads in column

Question 57

Size Exclusion Chromatography

Answer 57

Separate Components by size Mobile: Nonpolar solvent Stationary: Polar, porous beads in column

Question 58

Affinity Column

Answer 58

Purify a molecule of interest Mobile: Nonpolar solvent Stationary: Bead coated with antibody or receptor for target molecule

Question 59

Gas Chromatography

Answer 59

Separate vaporizable compounds Mobile: Inert Gas Stationary: Crushed metal or polymer

Question 60

High Performance liquid chromatography (HPLC)

Answer 60

Similar to column but more precise Mobile: Nonpolar solvent Stationary: Small column with concentration gradient

Question 61

IR Spectroscopy

Answer 61

Measures Molecular vibrations of characteristic functional groups

Question 62

Power equation

Answer 62

P=W/delta t Work/ change in time

Question 63

Total Mechanical Energy equation

Answer 63

E=U+K | potential energy+kinetic energy

Question 64

Power by resistors

Answer 64

P=IV V^2/R I^2R

Question 65

Conjugate Acid

Answer 65

Formed when a proton is added to a base | H20-->H3O

Question 66

Conjugate Base

Answer 66

Formed when a proton is removed from an acid | H2PO4-->HPO4