Chemistry Flashcards

Question

Transition metals

Answer 1

* High conductivity due to free flowing (loosely bound) outer d electrons * In the presence of ligands (when in a chemical complex) the d orbitals become nondegenerate (different in energy) * Electron transitions between nondegenerate d orbitals gives transition metal complexes vivid colors * Varied oxidation states, always positive

Answer 2

* **Metals**: good conductor of heat and electricity, malleable, ductile, luster, solid at room temp * **Nonmetals**: poor conductor of heat and electricity, solid liq or gas at room temp, brittle if solid and without luster

Answer 3

* **Metals**: good reducing agent, likes to lose electrons to gain a + oxidation state, lower electronegativity, partially positive in covalent bond, forms basic oxides * **Nonmetals**: Likes to gain electrons to form a - oxidation state, good oxidizing agent, higher electronegativity, partially negative in a covalent bond with metal, forms acidic oxides

Answer 4

* s and p block * No free flowing outer d electrons * Valence fills from left to right

Answer 5

* First ionization energy- energy needed to knock of first valence electron * Second ionization energy- energy needed to knock off second valence electron

Answer 6

* Decreases as you go down (increasing radii) * Inceases as you go right (decreasing radii) * Highest peaks (noble gases) * Lowest troughs (alkali metals) * Local maxima for filled subshells and half-filled p subshells * Second ionization energy is always higher than the first

Answer 7

The amount of energy released when something gains an electron. (How easily it can gain an electron)

Answer 8

* Decreases down a group (larger radii) * Increases from L to R * Highest = Halogens * Lowest = noble gases

Answer 9

How much something hordes electron in a covalent bond

Answer 10

* Increases towards the top right * F is most electronegative (N, O, F, Cl, Br are all v electroneg) * Noble gases can be electronegative if they participate in bond formatino (Kr and Xe) * More electroneg atom in covalent bond gets partial negative charge * If electroneg difference is too great- ionic bond will form

Answer 11

* size increases down a column * size decreases as you go across a row

Answer 12

electron transfer completely from one atom to another. Oppositely charged species attract each other via electrostatic interaction.

Answer 13

Electrostatic energy=kq₁q₂/r (Negative because charges are opposite) (Larger indicates stronger bond)

Answer 14

* Lattice energy measures ionic bond strength. * It is the energy required to break the ionic bond. * Larger magnitude = harder to break * Proportional to the electrostatic attraction between ions

Answer 15

F=kq₁q₂/r² * k=9E9 * Like law of gravitation, but G is tiny compared to k

Answer 16

Bond that results from sharing of electrons between two atoms, resulting in the overlap of their electron orbitals.

Answer 17

* σ: single bonds, make up the first bond of double and triple bonds * π: double and triple bonds, make up the second bond in a double bond and both the second and third bond in a triple bond

Answer 18

Total # bonds + unbonded electron pairs

Answer 19

Multiple satisfactory Lewis structures for a molecule. Shifts are fast, spending more time in stable resonance structures.

Answer 20

* Octet rule satisfied in every atom (except Boron group and H) * No formal charges * If there must be formal charge, like charges are apart and unlike charges are close together

Answer 21

Formal charge = (valence electron # in unbonded atom)-(electron # in bonded atom) Formal charge=(valence electron #)-(# dots + lines)

Answer 22

* Acceptor of electron pairs. They don't have lone pairs on central atom.

Answer 23

Lewis bases donate electron pairs. They have lone pairs on their central atom.

Answer 24

* Depends on charge and distance * Greater electronegativity difference = greater charge = greater dipole moment * Greater distance separating charge = greater dipole moment * Things with a dipole moment are polar

Answer 25

Molarity = M = mol/L Molality = m = mol/kg

Answer 26

6.02x10²³

Answer 27

* Oxygen and Ozone * Permanganates- MnO₄^- * Chromates- CrO₄^2-, Dichromates- Cr₂O₇^2- * Peroxides- H₂O₂ * Lewis acids * Stuff with oxygens

Answer 28

* Hydrogen * Metals (ex. K) * Zn/HCl * Sn/HCl * LAH (lithium aluminum hydride) * NaBH₄ (Sodium borohydride) * Lewis Bases * Stuff with lots of hydrogens

Answer 29

When an element in a single oxidation state reacts to form 2 different oxidation states. Disproportionation can occur when a species undergo both oxidation and reduction. ex. 2Cu⁺ → Cu + Cu²⁺

Answer 30

* Analyte (A) = stuff with unknown concentration that you want to find out by titration * Titrant (T) = stuff you add drip by drip to determine how much is needed to complete titration * Standard (S)= something with an accurately known amount or concentration (produces a known amount/conc of I₂) * Intermediate (X)= species that is not present in the net equation of the overall reaction

Answer 31

Equivalence point

Answer 32

0 K = -273 °C

Answer 33

1. Freezing point of water? **0 °C** 2. Room temp? **25 °C** 3. Body Temp? **37 °C** 4. Boiling point of water? **100 °C**

Answer 34

K=C+273 F=1.8C+32

Answer 35

1 atm = 760 mm Hg = 760 torr = 101 kPa

Answer 36

At 0 °C and 1 atm **22.4 L/mol**

Answer 37

* Moves randomly * No intermolecular forces * No molecular volume * Perfectly elastic collisions (conservation of total kinetic energy) * Low P, High T

Answer 38

High P, Low T

Answer 39

P₁V₁/T₁=P₂V₂/T₂

Answer 40

Boyle (Constant T): P₁V₁=P₂V₂ Charles' (Constant P): V₁/T₁=V₂/T₂

Answer 41

* Random molecular motion * No intermolecular forces * Negligible molecular volume * Perfectly elastic collisions (conservation of KE)

Answer 42

Temperature

Answer 43

molecules constantly colliding with the walls of its container.

Answer 44

Random molecular motion- causing a substance to move from an area of higher conc to an area of lower concentration (diffusion down concentration gradient)

Answer 45

Random molecular motion, causing a substance to escape a container through a very small opening.

Answer 46

Rate₁/Rate₂=(M₂/M₁)^½ | (Lighter molecules travel faster)

Answer 47

* b for bounce. repulsion term. Larger b = more reuplsion = greater pressure * a for attraction. Greater a, more attraction, less pressure.

Answer 48

P_i=x_iP_total P_total=ΣP_i

Answer 49

* Weak interaction between a partially positive H and a partially negative atom (F/O/N) * Incrases boiling point

Answer 50

(London dispersion forces) * Only significant for non-polar molecules * Result from induced and instantaneous dipoles

Answer 51

**Induced:** when a polar molecule interacts with a non-polar molecule, then polar molecule induces a dipole in the non-polar molecule **Instantenous:** Non-polar molecules have randomly fluctuating dipoles that tend to align with one another from one instant to the next

Answer 52

* Triple Point: T and P at which all 3 phases of matter coexist at equilibrium * Critical Point: T and P at which liquids and gases become indistinguishable * Critical Temp: T above which you can no longer get a liquid no matter how much pressure you apply

Answer 53

Depends on # of solute particles

Answer 54

(i) Convert concentration to reflect total + particles in solution. (Glucose: i=1, NaCl: i=2)

Answer 55

P = X_solvent·P°_solvent ΔP = X_solute·P°_solvent

Answer 56

ΔT_b = k_b·m·i * k_b = molal boiling point constant * m = molality * i = van't hoff factor

Answer 57

ΔT_f = -k_f·m·i * k_f= molal freezing point constant * m = molality (mol solute/kg solvent) * i = van't hoff factor

Answer 58

Π=MRT\*i * Π = osmotic pressure * M = molarity * R = ideal gas constant * T = temp in K * Determines whether and in what direction osmosis will occur * Solvent goes from low to high Π

Answer 59

Things are mixed at a "semi-molecular level" with solute aggregates that are tiny. Colloids will stay mixed until centrifuged.

Answer 60

Mixed at a particle level, will not stay mixed.

Answer 61

P_solute=k[solute] * P_solute= partial pressure of solute at surface * k = constant * [solute] is the solute concentration

Answer 62

Rate = -^ΔReactant/_ΔTime =^ΔProduct/_ΔTime

Answer 63

Single Step: Rate = k[A]^a[B]^b Multi-Step: Rate =k[A]^x[B]^y

Answer 64

k in the rate law is the rate constant The rate constant is an empirically determined value that changes with different reactions and reaction conditions

Answer 65

sum of all exponents of the concentration variables in the rate law

Answer 66

Unimolecular (1st order): r=k[A] Bimolecular (2nd order): r=k[A]², r=k[A][B] Termolecular (3rd order): r=k[A]³, r=k[A]²[B], r=k[A][B][C] Zero Order: r=k

Answer 67

* Slowest step of a multi-step reaction * Rate of the whole rxn = rate of RDS * Rate law corresponds to components of RDS

Answer 68

* What is present at the transition state * Bonds are just beginning to form and break * Peak of energy profile * Can't be isolated

Answer 69

Negative ΔH = exothermic Positive ΔH = endothermic

Answer 70

k=Ae^-Ea/RT * Ea = activation energy * T = temp (K) * A = constant

Answer 71

* Kinetic product: lower activation energy, formed preferentially at a lower T * Thermodynamic product: lower/more favorable ΔG, higher T

Answer 72

ΔG is negative

Answer 73

ΔG = ΔH - TΔS

Answer 74

* Favor: exothermic (-ΔH), increase entropy (+ΔS) * Disfavor: endothermic (+ΔH), decrease in entropy (-ΔS)

Answer 75

lower activation energy

Answer 76

* They speed up a reaction without getting itself used up * Enzymes are biological catalysts * Lower activation energy, speeds up forward and re verse reaction * Alter kinetics, not thermodynamics * Help system achieve equilibrium faster, does not alter position of equilibrium * Increase k, does not alter Keq

Answer 77

* Basis for equilibrium constant * Rate of a reaction depends only on the concentratino of the pertinent substances participating in the reaction * r_forward=r_reverse

Answer 78

* Keq = [C]^c[D]^d/[A]^a[B]^b * ΔG° = -RT ln (Keq)

Answer 79

* \> 1: more products are present * = 1: equilibrium is in the center * \< 1: more reactants are present

Answer 80

* Same as K_eq but can be used at any point, not just at quilibrium * If Q \< Keq, rxn is still moving to the right * If Q = Keq, rxn is at equilibrium * If Q \> Keq, rxn is moving back left

Answer 81

If you knock a system off its equilibrium, it will readjust itself to reachieve equilibrium

Answer 82

ΔG = ΔG° + RT ln Q * ΔG = 0 at equilibrium (Q = Keq) * ΔG° = -RT ln(Keq)

Answer 83

X-, XO-, etc

Answer 84

S₂O₃^2-

Answer 85

HPO₄^2- H₂PO₄^-

Answer 86

C₂O₄^2-

Answer 87

C₂H₃O₂^-

Answer 88

CrO₄^2- Cr₂O₇^2-

Answer 89

* Solvation * Hydration is where water forms a shell around ions in solution * Oxygen atoms surround cations, Hydrogen atoms surround anions

Answer 90

N = molarity of species that matter 1 M HCl = 1 N HCl 1 M H₂SO₄ = 2 N H₂SO₄ 1 M H₃PO₄ = 3 N H₃PO₄

Answer 91

* Solubility product constant, the equilibrium expression * ex. AgCl (s) ↔ Ag+ (aq) + Cl- (aq) * K_sp for AgCl = [Ag+][Cl-] * K_sp value are found in a table * Higher values = more reaction products dominate in a saturated solution

Answer 92

1. MX₂ ↔ M²⁺ + 2X^- 2. K_sp = [M²⁺][X^-]²= [M²⁺][2M²⁺]² = 4[M²⁺]³ 3. Solve for [M²⁺]. Solubility is the same thing as [M²⁺], because you used Q=K_sp for a saturated solution

Answer 93

* AgCl (s) ↔ Ag+ (aq) + Cl- (aq) * If you add Cl^- to the solution above, then less AgCL will dissolve * If you add NaCl to a saturated solution of AgCl, some AgCl would crash out of solution

Answer 94

* Metal⁺ + Lewis base: → Complex ion * M⁺ + L → M-L_n⁺ * K_eq=K_f (formation constant)

Answer 95

* Opposite of common ion effect * AgCl (s) ↔ Ag⁺ (aq) + Cl^- (aq) M⁺ + Cl^- ↔ M-Cl_ncomplex ion. * When complex ion forms, Cl^- is taken out, so more AgCl will dissolve

Answer 96

* Acids are more soluble in bases. * HA → H⁺ + A^- * Putting the above in a base will take out the H+, thus more HA will dissolve

Answer 97

* Bases are more soluble in acids. * B + H⁺ → BH⁺ * Putting this equation in an acid will add more H+, and thus drive more B to dissolve according to Le Chatelier's principle

Answer 98

H-Acid + Base^-↔ Acid^- + H-Base * Acid = proton donor * Base = proton acceptor * Conjugate base = acid after losing proton * Conjugate acid = base after gaining proton

Answer 99

* K_w=[H+][OH-] = 10^-14 * At standard conditions, pure water has [H+]=10^-7M and [OH-]=10^-7

Answer 100

pH = -log[H⁺] pOH = -log[OH^-] * Acidic: pH \< 7 * Neutral: pH = 7 * Basic: pH \> 7 * pH + pOH = 14

Answer 101

* completely dissociate in solution (conj. base anion is highly stable)

Answer 102

They will dissociate less in a solution with a salt.

Answer 103

* CH₃COO^- + H₂O ↔ CH₃COOH + OH^- * For M molar CH₃COO^-, start to abstract protons * [CH₃COO^-]= M-x * [CH₃COOH] = [OH^-] = x * K_b=K_w/K_a = [CH₃COOH][OH-] / [CH₃COO^-] = x²/(M - x) * x is very small: K_b=x²/M (Solve for x) * pOH = -log(x) * pH = 14 - pOH

Answer 104

* H-Acid ↔ H⁺ + Acid^- * K_a=[H⁺][Acid^-]/[HAcid] * Base + H₂O ↔ H-Base⁺ + OH^- * K_b=[HBase⁺][OH^-]/[Base] * K_aK_b=K_w=10^-14 * pK_a=-logK_a * pK_b=-logK_b * pK_a+pK_b=14

Answer 105

* Ka\*Kb=Kw=10^-14 * pKa = -logKa * pKb = -logKb * pKa + pKb = 14

Answer 106

* Solutions that resist changes in pH * Salts of weak acids and bases form buffer systems * Equilibrium between acidic species and a basic species * Acidic species donates protons to resist increase in pH * Basic species accepts protons to resist decreases in pH * Weak acid buffers: buffering capacity at pH = pKa

Answer 107

pH = pKa [Acid] = [conj base]

Answer 108

pH = 14 - pKb [base] = [conj acid]

Answer 109

* Buffers make titration curves "flat" at the region where buffering occurs (point of inflection) * Inflection point at pH = pKa = 14 - pKb * Area around inflection point is the region where the solution has buffering capacity (usually pKa +/- 1)

Answer 110

H-In ↔ H⁺ + In^- * Behave like weak acids/bases * Present in small amount, doesn't affect solution's pH * When solution has a low pH (high [H+]), indicator is mostly H-In (one color) * When solution has a high pH, (low [H+]), indicator is mostly In-, another color

Answer 111

* [acid] = [conj base] * [base] = [conj acid] * pH = pK_a * [titrant] = 1/2 [weak acid/base]

Answer 112

* reduction in charge * decreased oxidation number * gain of electrons

Answer 113

* Increase in charge * Increased oxidation number * Losing electrons

Answer 114

* Requires potential/voltage input (battery) * Galvanic cell has either a resistor or voltmeter * potential/voltage inpot + the cell potential must be \> 0 for rxn to occur * Cell potential is negative for electroytic cells * Cell potential is positive for galvanic/voltaic cell

Answer 115

**Anode** is always the place where oxidation happens. **Cathode** is always the place where reduction happens. * An Ox = ANode OXidation* * Red Cat = REDuction CAThode*

Answer 116

**Anode** shoots out electrons, **Cathode** takes in electrons.

Answer 117

* Ions * Conduct electricity by motion of ions * Necessary for a circuit

Answer 118

I=q/t Faraday's constant = coulombs of charge per mol of electron F=q/n

Answer 119

F=q/n F = total charge over total mols of electrons

Answer 120

It = nF | (Combine q = It and q = nF)

Answer 121

Oxidation is **losing** electrons, Reduction is **gaining** electrons. ## Footnote *Oil Rig: Oxidation Is Losing, Reduction is Gaining*

Answer 122

* Oxidation ½ rxn: species loses e^- * Reduction ½ rxn: species gains e^-

Answer 123

* Reduction potential = potential of the reduction half reaction * Oxidation potential = reduction of the oxidation half rection (= neg reduciton potential) * Cell potential = Reduction potential + oxidation Potential * Want to make cell potential positive

Answer 124

1. Isolated system = no exchange of heat, work, or matter with surroundings 2. Closed system = exchange of heat and work, but not matter with surroundings 3. Open system = exchange of heat, work and matter with surroundings

Answer 125

* Path-independent * ΔH (enthalpy), ΔS (entropy), ΔG (free energy change), ΔU (internal energy change) * Also called state quantity, or functions of state

Answer 126

* Endothermic = energy is taken up by rxn (+ ΔH) * Exothermic = energy is released by rxn (- ΔH)

Answer 127

* ΔH_rxn: The change in heat content for any reaction * ΔH_f: The change in heat content in a formation reaction

Answer 128

ΔH_rxn=Δ(ΔH_f)=Σ(ΔH_f)_products-Σ(ΔH_f)_reactants

Answer 129

Energy required to break bonds * ΔH_rxn= (bond dissociation energy for reactants) - (bond dissociation energy of bonds in products)

Answer 130

* Amount of heat required to raise the temperature of something by 1 °C * Molar heat capacity = ^J/_mol °C * Specific heat capacity = ^J/_g °C

Answer 131

1 calorie = 4.2 J 1 Calorie = 1000 calorie

Answer 132

A measurement of "disorder" in J/K * Entropy of gas \> liquid \> crystal states

Answer 133

* Heat flows from hot objects to cold objects to achieve thermal equilibrium

Answer 134

* ΔE = q + w * Energy is conserved * Q is positive when heat is absorbed by system, and negative when heat leaks out of system * W is positive when work is done on the system (compression), negative when work is done by the system (expansion)

Answer 135

Things like to be in a state of higher entropy and disorder ΔS ≥ q / T

Answer 136

increasing

Answer 137

ΔS = q / T (reversible) ΔS \> q / T (irreversible)

Answer 138

1. Heat transfer by direct contact 2. Heat transfer by flowing current. Needs physical flow of matter 3. Heat transfer by electromagnetic radiation. Does not need a medium

Answer 139

Energy input needed to melt something from solid to liquid at constant T

Answer 140

No heat exchange (Q=0, ΔE = W)

Answer 141

No change in temperature. ΔT = 0

Answer 142

W=0, ΔE = q

Answer 143

q=mcΔT (only works if no phase change is involved)

Chemistry Flashcards

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