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GEN CHEM 2 > GEN CHEM 2 > Flashcards

GEN CHEM 2 Flashcards

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1
Q

Forces exist within molecules

A

Intramolecular Forces

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2
Q

Forces exist between molecules

A

Intermolecular Forces

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3
Q

Types of Intramolecular Forces

A
  • Ionic Bond
  • Covalent Bond
  • Metallic Bond
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4
Q
  • A bond that is formed by the complete transfer of valence electron(s) between atoms.
  • a chemical bond that generates two oppositely charged ions.
  • Non-metal + Metal
A

Ionic Bond

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5
Q
  • formed between atoms that have similar
    electronegativities.
  • Both atoms have similar affinity for electrons
  • Non-metal + Non-metal
A

Covalent Bond

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6
Q
  • formed via the attraction of
    the mobile electrons
  • the sea of electrons
  • and the fixed positively charged
    metal ions.
  • Metal + Metal
A

Metallic Bond

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7
Q

Who is the first ferson that introduced intermolecular forces?
He did not develop but he was the first one who postulated the forces.

A

Johannes Diderik van der Waals

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8
Q
  • The strongest intermolecular force.
  • It exists between oppositely charged ions.
  • Ions of like charges repel while opposite charges
    attract.
A

Ion-Ion Forces

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9
Q
  • a force that results from the electrostatic attraction between an ion and a neutral molecule that has a dipole.
  • Occurs between a fully charged ion and
    a partially charged dipole.
A

Ion-Dipole Forces

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10
Q
  • a relatively strong force of attraction between molecules, and considerable energy is required to break its bonds.
  • bonded to either an oxygen, nitrogen, or fluorine atom.
  • Responsible for the unusually high boiling
    point and the melting point of water.
A

Hydrogen Bonding

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11
Q

forces occur when the partially positively charged part of a molecule interacts with the partially negatively charged part of the neighboring molecule.

A

Dipole-Dipole Forces

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12
Q
  • The weakest of the intermolecular forces
  • the attraction between the positively
    charged nucleus of an atom with the negatively charged electron cloud of a nearby atom
  • The more electrons a molecule has, the stronger it gets.
  • This interaction creates an induced dipole.
A

London Dispersion / Van der Waals Forces

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13
Q

How bond strengths affect the Physical Properties of
Substances? (Just some info)

A

+ When the strength of forces decreases, so do the melting points, boiling points, and solubility in water. The vapor pressure and the solubility in nonpolar solvents increase.

+ When the strength of forces increases, it will result in higher melting or boiling points, which require breaking molecules apart. Higher intermolecular forces lead to a higher freezing point.

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14
Q

Bonding forces that influence Chemical Properties

A

Intramolecular Forces

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15
Q

Attracting forces that influence Physical Properties

A

Intermolecular Forces

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16
Q

Is anything that has
mass and takes up space

A

Matter

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17
Q

Will change the visible appearance,
without changing the composition of
the material

Can be irreversible or reversible

A

Physical Change

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18
Q

Change from a solid
to a liquid

A

Melting / Fusion

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19
Q

Change from liquid to
solid

A

Freezing / Solidification

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20
Q

Change from liquid to gas.

A

Evaporation

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21
Q

A change from solid
to gas without its
becoming liquid

A

Sublimation

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22
Q

When a substance in gas form a changes
states to become a solid

A

Deposition

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23
Q

Change from gas to
liquid

A

Condensation

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24
Q

A change where a new form of matter
is made

A

Chemical Change

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25
Q

SIGNS OF A CHEMICAL CHANGE

A

Gas production
Precipitate formation
Energy production
Change in temperature
Change in color
Change in chemical or physical property

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26
Q

Depends on the amount of matter in a
sample
- Volume, mass, size, weight, length

A

Extensive Property

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27
Q

Depends on the type of matter, not the amount present
- Boiling point, color, temp, luster, hardness

A

Intensive Property

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28
Q

A property that can be observed
and measured without changing the
materials composition

A

Physical Property

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29
Q

Property that can only be observed
by changing the composition of the
material

A

Chemical Property

30
Q

A physical blend of at least two substances

A

Mixtures

31
Q

are the mixtures which have the same composition throughout and are also called solutions.

A

HOMOGENEOUS

32
Q

are the mixtures which do not have a uniform composition throughout and sometimes different components can be observed with the naked eye or with a help of a microscope.

A

HETEROGENEOUS

33
Q

Composed of molecules which possess kinetic energy

A

Matter

34
Q

Shape and volume of gases, liquids, and solids can be explained by the assumptions of the _______?

A

Kinetic Molecular Theory

35
Q

True or False
A liquid boils when its vapor pressure is equal to the external pressure.

A

True
(eme lang for review)

36
Q

The normal boiling point of a liquid is the temperature at _____?

A

1 atm pressure

37
Q

the process when a liquid that is not boiling changes to vapor or gas

A

Evaporation

38
Q

a good solvent as it dissolves more substances than any other common liquid.

A

Water

39
Q

Unusual properties of water

A
  • High density
  • High boiling point and melting point
  • High heat of vaporization
  • High surface tension
  • High specific heat
40
Q

Solids that contain water molecules as part of their crystalline structure

A

Hydrates

41
Q

It may have atoms, ions, or molecules as component particles

A

Matter in the solid phase

42
Q

physical properties of solids are observed when particles gain enough kinetic energy to move from their fixed positions.

A

Melting and subliming

43
Q

Observed in solids that undergo sublimation

A

Vapor pressure

44
Q

Bunos infu

A

Matter in solid phase is either amorphous or crystalline

45
Q

subclassified as: metallic, ionic, molecularly, and covalent network crystals

A

Crystalline solids

46
Q

The property is shown by solids that can assume more than one stable arrangement of their component or molecules.

A

Polymorphism

47
Q

It depends on the nature of the substance and on the temperature and pressure of its environment

A

Phase Changes

48
Q

It shows what phase or phases can be presented for any given pressure-temperature combination

A

Phase Diagram

49
Q

The intersection of the liquid-vapor, solid-vapor, and soli-liquid curves, which corresponds to an equilibrium among three phases.

A

Triple point

50
Q

The pressure-temperature combination

A

Critical Point

51
Q

can be expressed through mass measurement, volume measurement, the number of moles, or a combination of the three.

A

Concentration of solution

52
Q

It utilizes the mass of the solute and the mass of the solution

A

Percent by mass

53
Q

it uses the volumes of the solution and the solute

A

Percent by volume

54
Q

it express concentration in terms of the number of moles of the solute and the solution.

A

Mole fraction and mole percent

55
Q

An expression of solution concentration in terms of the number of moles per liter of solution

A

Molarity (M)

56
Q

An expression of solution concentration in terms of the number of moles of solute per 1,00 g or 1kg of solvent

A

Molality (m)

57
Q

It can be used to determine the concentration of a solution

A

Titration

58
Q

Additional info

A

At the end of the titration, the number of moles of the reactants is equal.
ex: in an acid-base titration, the number of moles of the acid is equal to the number of moles of the base

59
Q

Info again mwehehe

A

The number of moles can be expressed as the product of volume and molar concentration.

60
Q

It is also a solution that are composed of solutes and a solvent

A

HOMOGENEOUS MIXTURES

61
Q

The component of a solution that exists in greater quantity and which usually dictates the phase of matter of the solution.

A

Solvent

62
Q

The component of the solution that exists in lesser quantity

A

Solute

63
Q

Can be classified as gaseous, liquid, or solid solutions.
Can also be classified according to the concentration of their solutes
Can be diluted or concentrated

A

Solutions

64
Q

The solution that contains ions

A

Electrolyte Solution

65
Q

The solution that contains molecules as solutes

A

Non-Electrolyte Solution

66
Q

Infos

A
  • The solution process involves the breakage of solute-solute interactions and the formation of solute-solvent interactions.
  • The particles of the solute, like the particles of the solvent, must overcome the attractive forces among them in order to form the solution.
  • Fo the solute to dissolve in the solvent, the solute particles and solvent particles must exhibit an equal or stronger attraction toward each other. The intermolecular attraction between them must be of a similar type.
67
Q

Refers to the maximum quantity of solute that can dissolve in a given quantity of solvent at a given temperature.

A

Solubility

68
Q

affects the solubility of gases in liquids

A

Temperature and pressure

69
Q

more info

A
  • Gases dissolve better in lower temperatures and higher pressure
  • Most solids dissolve better at higher temperatures, whole pressure has little effect on solubility
70
Q

It involves heat energy absorption and heat energy release

A

Phase Changes

GEN CHEM 2 (1 decks)

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