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Inorganic Chemistry > Inorganic Chem Reviewer > Flashcards

Inorganic Chem Reviewer Flashcards

1
Q

One of the fundamental properties of any matter.

A

Density

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2
Q

What is the formula of density?

A

P= m/v

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3
Q

What is the SI unit of density? (Checimal and non-chemical-setup).

A

In chemical setup, g/cm3, non-chemical setup kg/m3

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4
Q

What is the density of 30 C?

A

0.9957g/mL

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5
Q

What is the density of 25 C?

A

0.9970g/mL

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6
Q

What is the density of 4 C?

A

1.0000g/mL

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7
Q

What is the density of 0 C?

A

0.9998g/mL

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8
Q

How is the volume of liquid can be easily determined?

A

It can be determined using calibrated cylinder but in laboratory setting, it can be determined in a graduated cylinder.

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9
Q

Can be determined by direct measurement provided that the solid has a regular geometrical shape, such as a cube or a cylinder.

A

Volumes of Solid

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10
Q

Such as a small rock or a small chunk of metal are determined by liquid volume displacement.

A

Volume of irregularly shaped solids

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11
Q

Closeness of a measurement to its true value.

A

Accuracy

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12
Q

How a measurement or process can repeat the
same value.

A

Precision

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13
Q

What is C?

A

Speed of light (~3.08x108m/s)

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14
Q

What is λ?

A

Wavelength

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15
Q

What is f?

A

Frequency

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16
Q

How is a quantum energy can be released?

A

Whenever an electron decays from a greater amount of energy to a smaller amount of energy.

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17
Q

When are the colors created?

A

When atoms with different energy levels collide.

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18
Q

The first to propose that the outermost electron of an atom.

A

Gilbert N. Lewis

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19
Q

Are responsible for the formation of molecular bonds.

A

Valence electrons

20
Q

Shows how atoms would share electrons to fill eight (8) electrons in its outermost shell to form covalent bonds also known as Octet Rule.

A

Lewis Dot Structure

21
Q

Suggests that electron pairs around an atom will assume a position that minimizes the repulsion between electrons.

A

Valence Shell Electron Pair Repulsion (VSEPR)

22
Q

A process wherein reactants (or starting materials) are converted into products.

A

Chemical reaction

23
Q

Two or more atoms or compounds in this type of reaction combine to form a product.

A

Combination or synthesis.

24
Q

This type of reaction is a breakdown of a compound into simpler compounds or elements.

A

Decomposition

25
Q

This type of reaction is one where a more active element takes the place of another element in a compound.

A

Single replacement or substitution.

26
Q

Two reactants exchange ions to form a new compound. When the reactants are acids and bases, the process is termed neutralization reaction.

A

Double replacement.

27
Q

A specific type of reaction (which can sometimes also fall under the categories given above) where oxygen reacts with a combustible reactant, usually hydrocarbons, to produce carbon dioxide, water, and a huge amount of energy.

A

Combustion reaction

28
Q

Studied the behavior of gases in a systematical and quantitative manner.

A

Robert Boyle

29
Q

Studied the relationship of temperature and volume of gases.

A

Jacques Charles

30
Q

What is the R?

A

0.08206 L∙atm/mol∙K

31
Q

What is m?

A

Mass (g)

32
Q

What is MM?

A

Molar mass (g/mol)

33
Q

Molar weight of unknown mass formula?

A

MM=mRT/PV

34
Q

What are the homogenous mixture?

A

Solution, Colloids, and Suspension Solutions

35
Q

Are stable mixtures with a very large surface area and solute particles ranging from 1 to 1000 nm.

A

Colloids

36
Q

Its ability to scatter light when viewed at a right angle.

A

Tyndall effect

37
Q

Colloidal systems composed of immiscible or partially miscible liquids .

A

Emulsions

38
Q

Are unstable mixture of particles larger than 1000 nm, separating into phases.

A

Suspensions

39
Q

A pure substance has a standard boiling point freezing point and vapor pressure, which may alter in the presence of soluble compounds.

A

Colligative properties of solution

40
Q

Is inversely proportional to the vapor pressure, which means that a decrease (¯) in vapor pressure will result in the rise/increase (+) of boiling point of a liquid.

A

Boiling point

41
Q

Function of the number of particles in solution and the presence of solute lowers the freezing point of pure solvent.

A

Freezing point

42
Q

Pressure that needs to be applied to prevent the flow of pure solvent through a semi-permeable membrane into a solution.

A

Osmotic pressure

43
Q

Constants for water (K) kb

A

Molal boiling

44
Q

point elevation = 0.52°C kf

A

Molal freezing

45
Q

point depression

A

1.86 C

Inorganic Chemistry (1 decks)

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