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Gen Chem Flashcards

1
Q

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A

Arrhenius acids and bases

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2
Q

Electrons fill orbitals starting at lowest possible state before filling higher orbitals

A

Aufbau principle

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3
Q

97bf5b75ad66c80a29e1a0b7710a9fa2.jpg salt in pasta water increases the boiling point of water so that the water boils hotter and pasta cooks faster

A

Boiling point elevation

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4
Q

fce9afb63de87609e1ed73b6c6974920.jpg

A

Bronsted-Lowry acids and bases

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5
Q

ab9458cd3a18aec31f0f7a3329faeb40.jpg

A

Buffers

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6
Q

34c7a5de14c04effe1c85455d751cf52.jpg Pure liquids and solids have concentration=1 Large equilibrium constant – reaction favors products 1788222f251ff1c9c2275e3b452d51b5.jpg

A

Chemical equilibrium constant

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7
Q

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A

Closed system versus isolated system

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8
Q

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A

Dalton’s law of partial pressures

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9
Q

Attraction betwen the negatively charged end of a polar molecule and the positively charged ends of neighboring polar molecules

A

Dipole-dipole forces

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10
Q

Dipole-dipole forces

A

Attraction betwen the negatively charged end of a polar molecule and the positively charged ends of neighboring polar molecules

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11
Q

Attraction between negatively charged electron cloud of one moleculre and the poisivtely charged nuclei of neighboring molecules

A

Dispersion forces

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12
Q

Dispersion forces

A

Attraction between negatively charged electron cloud of one moleculre and the poisivtely charged nuclei of neighboring molecules

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13
Q

856e3c8a4c9bbd6d6a4e8a9e6303265d.jpg 5100d2389ff2c8a69887756bb8f1ab4a.jpg

A

Electrochemical cell potential

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14
Q

Uses electricity to drive non-spontaneous reaction d48496feb7c5b3f5f48c8f8ba43e94e4.jpg

A

Electrolytic cell

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15
Q

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A

Enthalpy

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16
Q

5a65b3934e215adbbccceafab7eb76ef.jpg d4e0e3c321ade86de1986b43bf705a1a.jpg

A

Entropy

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17
Q

198c5f48452eb8eb29c7ec4aa785fbe5.jpg

A

Exothermic and endothermic processes in a calorimeter

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18
Q

aced1ce3c4a1abbb658511b91c052689.jpg

A

First law of thermodynamics

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19
Q

Cations and anions attracted to one another by coulombic interactions

A

Forces holding atoms in ionic solids in place

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20
Q

Delocalised bonding

A

Forces holding atoms in metallic solids in place

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21
Q

Covalent bonds linking every atom to its neighbors

A

Forces holding atoms in network solids in place

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22
Q

dispersion forces dipole-dipole (sometimes) hydrogen bonds

A

Forces holding molecules in place in molecular solids:

23
Q

761c3ae24033c8cbb6ee2ad1668f2cee.jpg Salt lowers freezing point of water

A

Freesing point depression

24
Q

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A

Gibb’s free energy

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Gibbs free energy in electrochemical cell
26
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Graham's law of effusion
27
The position and momentum of a particle cannot both be exactly known at the same time
Heisenberg uncertainty principle
28
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Hess's law
29
When electrons are added to orbitals of equal energy, a single electron enters each orbital before a second electron with opposite spin enters any orbital. Spins remain parallel. Electrons add singly at first and then pair with opposite spins. Ex: 0fd586ba05bdb88340226ff4c9379d5b.jpg
Hund's rule
30
Lone pairs of electrons on an electronegative atom of one molecule are attracted to polar bond to hydrogen in another molecule. Confined to molecules containing O, N, and F.
Hydrogen bonding
31
Hydrogen bonding
Lone pairs of electrons on an electronegative atom of one molecule are attracted to polar bond to hydrogen in another molecule. Confined to molecules containing O, N, and F.
32
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Ideal gas law
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Influence of temperature on spontenaeity
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LeChatelier's Principle
35
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Lewis acids and bases
36
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Molar heat capacity
37
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Molar heats of solution, vaporization, and fusion. Sublimation.
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molarity (M) molality (m) mole fraction (χ) mass percent parts per million (ppm)
39
51a8e0f857348e2b5b038760d7c425f7.jpg increase in pressure due to a solvent crossing a membrane into a more concentrated solution
Osmotic pressure
40
No two electrons in an atom can have the same set of four quantum numbers. Each orbital with quantum numbers (n, l, m) can hold at most two electrons with positive spins
Pauli exclusion principle
41
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Quantum numbers
42
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Raoult's Law
43
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Rate laws for first and second order reactions
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Reaction enthalpies
45
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Reaction entropies
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Real gases
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Redox, cathodes, and anodes
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Second law of thermodynamics
49
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Standard enthalpy of formation 7a8cc3f92ab9be843cdb1e092d87f420.jpg
50
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Standard molar free energy of formation b255a7b0d4636fa25ebf328671d98086.jpg
51
760 mmHg=760torr=101.325kPa=1.01325barr
Units of pressure: 1atm= _____ mmHg = _____ torr =_____ kPa = ______ barr
52
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Water equilibrium constant
53
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What is STP? What is the volume of 1 mol of ideal gas at STP?

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