GEN CHEM 2 Flashcards
(70 cards)
1
Q
Forces exist within molecules
A
Intramolecular Forces
2
Q
Forces exist between molecules
A
Intermolecular Forces
3
Q
Types of Intramolecular Forces
A
- Ionic Bond
- Covalent Bond
- Metallic Bond
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
5
Q
- formed between atoms that have similar
electronegativities. - Both atoms have similar affinity for electrons
- Non-metal + Non-metal
A
Covalent Bond
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
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
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
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
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
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
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
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.
14
Q
Bonding forces that influence Chemical Properties
A
Intramolecular Forces
15
Q
Attracting forces that influence Physical Properties
A
Intermolecular Forces
16
Q
Is anything that has
mass and takes up space
A
Matter
17
Q
Will change the visible appearance,
without changing the composition of
the material
Can be irreversible or reversible
A
Physical Change
18
Q
Change from a solid
to a liquid
A
Melting / Fusion
19
Q
Change from liquid to
solid
A
Freezing / Solidification
20
Q
Change from liquid to gas.
A
Evaporation
21
Q
A change from solid
to gas without its
becoming liquid
A
Sublimation
22
Q
When a substance in gas form a changes
states to become a solid
A
Deposition
23
Q
Change from gas to
liquid
A
Condensation
24
Q
A change where a new form of matter
is made
A
Chemical Change
25
SIGNS OF A CHEMICAL CHANGE
Gas production
Precipitate formation
Energy production
Change in temperature
Change in color
Change in chemical or physical property
26
Depends on the amount of matter in a
sample
- Volume, mass, size, weight, length
Extensive Property
27
Depends on the type of matter, not the amount present
- Boiling point, color, temp, luster, hardness
Intensive Property
28
A property that can be observed
and measured without changing the
materials composition
Physical Property
29
Property that can only be observed
by changing the composition of the
material
Chemical Property
30
A physical blend of at least two substances
Mixtures
31
are the mixtures which have the same composition throughout and are also called solutions.
HOMOGENEOUS
32
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.
HETEROGENEOUS
33
Composed of molecules which possess kinetic energy
Matter
34
Shape and volume of gases, liquids, and solids can be explained by the assumptions of the _______?
Kinetic Molecular Theory
35
True or False
A liquid boils when its vapor pressure is equal to the external pressure.
True
(eme lang for review)
36
The normal boiling point of a liquid is the temperature at _____?
1 atm pressure
37
the process when a liquid that is not boiling changes to vapor or gas
Evaporation
38
a good solvent as it dissolves more substances than any other common liquid.
Water
39
Unusual properties of water
- High density
- High boiling point and melting point
- High heat of vaporization
- High surface tension
- High specific heat
40
Solids that contain water molecules as part of their crystalline structure
Hydrates
41
It may have atoms, ions, or molecules as component particles
Matter in the solid phase
42
physical properties of solids are observed when particles gain enough kinetic energy to move from their fixed positions.
Melting and subliming
43
Observed in solids that undergo sublimation
Vapor pressure
44
Bunos infu
Matter in solid phase is either amorphous or crystalline
45
subclassified as: metallic, ionic, molecularly, and covalent network crystals
Crystalline solids
46
The property is shown by solids that can assume more than one stable arrangement of their component or molecules.
Polymorphism
47
It depends on the nature of the substance and on the temperature and pressure of its environment
Phase Changes
48
It shows what phase or phases can be presented for any given pressure-temperature combination
Phase Diagram
49
The intersection of the liquid-vapor, solid-vapor, and soli-liquid curves, which corresponds to an equilibrium among three phases.
Triple point
50
The pressure-temperature combination
Critical Point
51
can be expressed through mass measurement, volume measurement, the number of moles, or a combination of the three.
Concentration of solution
52
It utilizes the mass of the solute and the mass of the solution
Percent by mass
53
it uses the volumes of the solution and the solute
Percent by volume
54
it express concentration in terms of the number of moles of the solute and the solution.
Mole fraction and mole percent
55
An expression of solution concentration in terms of the number of moles per liter of solution
Molarity (M)
56
An expression of solution concentration in terms of the number of moles of solute per 1,00 g or 1kg of solvent
Molality (m)
57
It can be used to determine the concentration of a solution
Titration
58
Additional info
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
Info again mwehehe
The number of moles can be expressed as the product of volume and molar concentration.
60
It is also a solution that are composed of solutes and a solvent
HOMOGENEOUS MIXTURES
61
The component of a solution that exists in greater quantity and which usually dictates the phase of matter of the solution.
Solvent
62
The component of the solution that exists in lesser quantity
Solute
63
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
Solutions
64
The solution that contains ions
Electrolyte Solution
65
The solution that contains molecules as solutes
Non-Electrolyte Solution
66
Infos
- 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
Refers to the maximum quantity of solute that can dissolve in a given quantity of solvent at a given temperature.
Solubility
68
affects the solubility of gases in liquids
Temperature and pressure
69
more info
- Gases dissolve better in lower temperatures and higher pressure
- Most solids dissolve better at higher temperatures, whole pressure has little effect on solubility
70
It involves heat energy absorption and heat energy release
Phase Changes
