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DAT > General Chemistry > Flashcards

General Chemistry Flashcards

1
Q

What is the formula for density?

A

Density=Mass/Volume

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2
Q

What is the Pauli exclusion principle?

A

No two electrons can have the same quantum numbers (n, l, ml, ms).

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3
Q

What is Hund’s Rule?

A

In order to achieve the lowest energy (most stable), the number of electrons with the same spin is maximized. So, fill up the orbitals with the same spin first.

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4
Q

What does the Valence Shell Electron-Pair Repulsion (VSEPR) theory state?

A

That electron pairs will arrange themselves as far away from each other as possible on an atom.

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5
Q

List characteristics of an ionic bond.

A

Hard, brittle
High melting points
Poor conductors of electricity
Transfer of electrons from metals to nonmetals
Atoms held together via electrostatic forces

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6
Q

List characteristics of a metallic bond.

A

Positively charged ions in sea of electrons
Good conductors of electricity
Ductile and Malleable
Variable hardness and melting points

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7
Q

List characteristics of a covalent bond.

A

Poor conductors of electricity
Polar Covalent bonds have a dipole moment and unequal sharing of bonding electron pair.
Nonpolar covalent bonds have equal sharing of electron pair, same electronegativity, and diatomic molecules.

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8
Q

List characteristics of Molecular bonds, or van der waals forces (London dispersion).

A

Hydrogen bonds
Low melting points
Poor conductors of electricity
High boiling points

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9
Q

Atomic radii increase on the periodic table as you move ____. Why?

A

Down and to the left.
Because as you move down you gain an additional outer principle energy level and as you move right, the additional protons pull the valence electrons closer to the nucleus.

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10
Q

Cations are always ____ than neutral atoms of the same element regarding radii, whereas anions are always ____.

A

Smaller, larger

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11
Q

What is ionization energy and what is its trend on the periodic table?

A

Ionization energy is the energy required to remove an electron from an atom. It increases as you move to the top and to the right.

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12
Q

What is electronegativity and what is its trend on the periodic table?

A

EN is the measure of the ability of an atom to acquire an additional electron. It increases as you move to the top and to the right. Fluorine as the highest EN.

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13
Q

What is electron affinity and what is its trend on the periodic table?

A

Electron affinity is the energy required to add an electron to an atom. It increases as you move up and to the right.

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14
Q

What is the trend of melting points and boiling points on the periodic table?

A

Melting and boiling points tend to decrease from the top to the bottom of a group for metals. Nonmetals show an increase from top to bottom.

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15
Q

What is Avogadro’s number?

A

6.02 x 10^23 atoms = 1 mole

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16
Q

Describe the steps to work an empirical formula problem.

A
  1. assume there are 100 g of sample
  2. convert the grams to moles
  3. divide all by the lowest moles to achieve a ratio
  4. write out the molecular mformula according to the ratio
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17
Q

Combination reaction?

A

A + B -> C

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18
Q

Decomposition reactions?

A

C -> A + B

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19
Q

Single-Replacement Reactions?

A

AB + C -> A + BC

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20
Q

Double-Replacement Reactions?

A

AB + CD -> AD + BC

21
Q

Combustion reactions?

A

Organic substance (C5H12) + O2 -> CO2 + H2O

22
Q

What’s the formula for pressure?

A

Pressure = Force/Area

23
Q

What is STP of the gas laws?

A

Temperature = 0 degrees C or 273 K
Pressure = 1 atmosphere
Volume of 1 mole of gas at STP = 22.4 L

24
Q

Graham’s Law of Effusion?

A

Rate of eff of gas A/ rate of eff of gas B = (density of B/ density of A)^1/2

25
Q

Dalton’s Law of Partial Pressures?

A

Ptotal = P1 + P2 + P3 + …

where PV=nRT

26
Q

What is the formula for Charles’s Law? Boyle’s Law?

A

Charles’s V1/T1 = V2/T2

Boyle’s P1V1 = P2V2

27
Q

What is the difference between homogeneous and heterogeneous reactions?

A

Homogeneous reactions occur in one phase while heterogeneous reactions occur in two or more phases.

28
Q

What is the critical point on a phase diagram?

A

The point where the vapor pressure curve (liquid and gas) ends. Beyond this point, liquids and gases are indistinguishable.

29
Q

What is the triple point on a phase diagram?

A

The point where the curves of all 3 phases intersect. Here, all 3 phases are in equilibrium.

30
Q

What is a saturated solution, an unsaturated solution, and a supersaturated solution.

A

Saturated solutions occur when the max amount of solute that can be dissolved is reached.
Supersaturated solutions occur when there is more than max solute.
Unsaturated solutions occur when max solute has not yet been reached.

31
Q

Describe Raoult’s Law and the lowering of vapor pressure.

A

Raoult’s Law states that
Change of Vapor Pressure = Mol Fraction of solute / vapor pressure of solvent
The more the solute added to a pure solvent, the more vapor pressure above the solvent decreases.

32
Q

Freezing point depression formula?

A

Freezing point depression = Kf * molality

33
Q

Boiling point elevation formula?

A

Boiling point = Kb * molality

34
Q

What is the pH formula?

A

pH = -log [H+]

34
Q

Osmotic pressure formula?

A

Osmotic pressure = Molarity of solutionRT

35
Q

What is the equilibrium constant expression for the auto ionization of water?

A

Kw=[H+][OH-]=1 x 10^-14

36
Q

How does pressure and temperature affect a system in equilibrium?

A

Adding pressure will favor the side with the fewer gas molecules. Adding heat will favor the products in an endothermic rxn and the reactants in an exothermic.

37
Q

What is the Henderson Hasselbach equation?

A

pH = pKa + log [base]/[acid]

When concentrations of the acid and base are the same, pH is equal to pKa.

38
Q

What are oxidizing and reducing agents?

A

Oxidizing agents are reduced and cause something to be oxidized. Reducing agents are oxidized and cause something to be reduced.

39
Q

The anode is the positive electrode and is where ____ occurs while the cathode is the negative electrode and is where ____ occurs.

A

Oxidation, reduction

40
Q

What does faraday’s law state?

A

In an electrolytic cell, the amount of oxidation-reduction reactions occurring is proportional to the amount of current passing through. 96,485 coulombs = 1 mole of electrons = 1 faraday

41
Q

What is electron motive force?

A

In a galvanic cell, it is the driving force that pushes the electrons through the circuit. It is the potential difference between electrodes of the cell.

42
Q

What is standard electron potential E•?

A

It is the emf under standard conditions: Temp = 25 C, Conc. = 1M, Pressure = 1 atm
When values are compared, the higher one is oxidized and the lower is reduced. A positive emf indicates a spontaneous rxn.

43
Q

First Law of thermodynamics?

A

Third Law of thermodynamics?

44
Q

Describe Gibbs free energy and the equation?

A

dG = dH - TdS
if dG is positive, the rxn is spontaneous.
If dG is 0, the rxn is in equilibrium.
If dG is negative, the rxn, is non spontaneous, but the the reverse rxn is spontaneous.

45
Q

What’s the half life formula for a first-order reaction?

A

t1/2 = 0.693/k

46
Q

What’s the half life formula for a second order reaction?

A

t1/2 = 1/k[X] where X is the initial concentration.

47
Q

Neutralization formula?

A

N1 * V1 = N2 * V2

DAT (3 decks)

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