Chapters 13-18 Flashcards

1
Q

What is it about oxygen that defies explanation using just VSEPR and hybridization theory?

A

The fact that oxygen is paramagnetic.

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2
Q

What makes materials paramagnetic?

A

unpaired electrons in their electron clouds.

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3
Q

What are Michael Faraday’s dates?

A

1791-1867.

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4
Q

Who first discovered that oxygen is attracted to magnetic fields? When?

A

Michael Faraday in 1847.

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5
Q

Who solved the mystery of oxygen’s paramagnetism?

A

Friedrich Hund and Robert Mulliken in 1933. An electron in a molecule could move through larger regions defined by combinations of overlapping atomic orbitals.

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6
Q

Define a chemical reaction.

A

Any process that results in the breaking, formation, or rearrangement of chemical bonds.

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7
Q

Are processes like melting ice or boiling water chemical reactions?

A

No. Just physical changes. The chemical bonds remain the same.

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8
Q

Is radioactive decay a chemical reaction?

A

No– the element’s identity is changed because of nuclear changes, not changes in the chemical bonds.

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9
Q

What are 4 basic types of chemical reactions?

A

Synthesis, Decomposition, Single Displacement and Double Displacement.

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10
Q

What is a synthesis chemical reaction?

A

when 2 or more smaller reagents combine to form a single larger product.

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11
Q

What is a Decomposition chemical reaction?

A

a process in which larger starting materials are broken down into smaller and more numerous products.

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12
Q

What is a Single Displacement chemical reaction?

A

combination of synthesis and decomposition, in which one reactant replaces a part of another molecule, liberating that which it replaced.

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13
Q

What is a Double Displacement chemical reaction?

A

also called metathesis, 2 or more reactants exchange a portion of themselves with one another.

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14
Q

Define Stoichiometry

A

The molar ratios of each reactant and product involved in a given chemical reaction.

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15
Q

When balancing chemical equations, which species should you leave to the last step?

A

The pure elements.

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16
Q

What is a limiting reagent?

A

The reagent we expect to be depleted first in a chemical reaction.

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17
Q

What are James Prescott Joule’s dates?

A

1818-1889.

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18
Q

What was James Joule’s profession?

A

He owned a brewery.

19
Q

What 2 things do engines produce?

A

Heat and work.

20
Q

What did Joule notice about the relationship between heat and work?

A

He noticed that the more heat a device produced, the less work it could do per unit of fuel consumed. Minimizing heat meant maximizing work.

21
Q

What is the definition of a Joule?

A

It is the amount of kinetic energy imparted to an object when 1 newton of force acts on it over a 1-meter distance.

22
Q

What is the definition of a calorie?

A

Equal to 4.17 joules, it is the amount of energy needed to heat 1 gram of water 1 degree centigrade.

23
Q

What is the definition of the British Thermal Unit (BTU)?

A

The amount of heat needed to raise the temperature of 1 pound of water by 1-degree Fahrenheit.

24
Q

What is the first law of thermodynamics?

A

Energy cannot be created or destroyed. It can only be exchanged.

25
Q

What is the definition of enthalpy?

A

When heat is equal to energy in a system performing no work, that heat is given the name enthalpy.

26
Q

What is an exothermic reaction?

A

One which releases heat to its surroundings.

27
Q

What is an endothermic reaction?

A

One which absorbs heat from its surroundings.

28
Q

What is the Specific Heat of a substance?

A

A measure of how much energy is required to heat 1 gram of material by 1-degree centigrade. Denoted by S or c.

29
Q

What is the specific heat of water?

A

4.18 joules per degree centigrade.

30
Q

How do we measure the heat capacity of a sample?

A

multiply the specific heat by the mass of the material.

31
Q

What are Pierre-Eugene-Marcellin Berthelot’s dates?

A

1827-1907.

32
Q

What did Berthelot invent?

A

The bomb calorimeter.

33
Q

What are Germain Hess’s dates?

A

1802-1850

34
Q

What is a state function?

A

properties that are identical for all systems of a particular kind no matter what happened to a system previously.

35
Q

What is Hess’s law?

A

The enthalpy change for a complex process is equal to the sum of the enthalpy changes of the smaller steps making it up, no matter what those smaller steps might be.

36
Q

When did Hess formulate his law?

A

1840

37
Q

The higher the enthalpy, the _____ the bond will be.

A

Stronger

38
Q

What’s the bond enthalpy for a carbon-carbon bond?

A

348 Kj/mol

39
Q

What are Ludwig Boltzmann’s dates?

A

1844-1906.

40
Q

What was a microstate for Boltzmann?

A

a state that considered the position and motion of every atom in a system.

41
Q

What is Boltzmann’s equation?

A

Relates the randomness of a chemical system to the number of microstates accessible to that system: S = Kb*lnW

42
Q

What is the second law of thermodynamics?

A

entropy, or randomness, in a closed system tends to increase unless it is countered by the input of energy from an outside source.

43
Q

What does Boltzmann’s equation and the second law of thermodynamics say about the fate of the universe?

A

that the overall randomness of matter in the universe will constantly increase until it simply can’t any more.