Chemistry Spring Final

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97 Terms

1
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ionic bonding is the result of what
electrons being completely transferred
2
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what kind of elements are involved in an ionic bond
one metal and nonmetal that are far apart on the periodic table
3
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covalent bonding is the result of what
electrons being shared
4
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what kind of elements are in a covalent bond
two non metals or one metal and nonmetal that are close to each other on the periodic table
5
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nonpolar covalent bond
electrons are shared equally because the elements have the same electronegatives
6
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polar covalent bond
electrons are shared unequally which creates partially charged poles
7
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why do atoms form bonds
to become stable/ form an octet
8
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what is meant by a stable octet
their ending electron is S2P6
9
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what does is mean if in a covalent bond, there is un-shared pairs
the molecule is polar
10
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what are the characteristics of ionic compounds
high melting point, hard to crush, soluble in water, and good conductors
11
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what are the characteristics of covalent molecules
low melting point, soft(able to crush), slightly insoluble, bad conductors
12
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what are the five kinetic theories of gases
gases have lots of tiny particles that are far apart, collisions between gas particles and the container wall are called elastic collisions, they have kinetic energy because they are always in motion, there is no forces of attraction between gas particles, temp of gas depends on the average kinetic energy of the gas
13
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crystal
a 3D organized pattern of unit cells
14
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lattice
the organized repeating pattern that is in a crystal
15
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solid
definite shape and definite volume
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liquid
definite volume and no shape
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gas
no definite shape or volume
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amorphous
without crystals but not without shape, can hold a shape for a long time
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super cooled liquid
able to hold shape for a long period of time (metastable)
20
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melting
particles change position from solid to a liquid
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melting point
temp at which a solid becomes a liquid (Vapor pressure of a solid = vapor pressure of a liquid)
22
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sublimation
when a solid goes straight to a gas instead of being in the liquid phase first
23
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what are sublimation examples
solid air freshener, moth balls and dry ice
24
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phase diagram
compares temp and pressure, telling you at what temp and pressure your substance is either a solid, liquid or gas
25
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triple point
when a substance can be a solid, liquid or gas at the same temp and pressure
26
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pressure
number of collisions
27
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STP
standard, temp and pressure
28
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what are the values of STP
standard pressure is 101.3 Kpa or 1atm and standard temp is 0 degrees C or 273K for gases
29
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absolute zero
\-273K
30
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daltons law of partial pressure
the total pressure is equal to the sum of partial pressures
31
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boyles law
temp is constant, pressure and volume vary inversely (P⬆️ V⬇️)
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charles law
pressure is constant, volume and temp vary directly (V⬆️T⬆️)
33
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gay-lussac law
volume is constant, pressure and temp vary directly

(P⬆️ T⬆️)
34
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how do you convert celcius to kelvin
add 273
35
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solvent
greater volume, does the dissolving
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solute
less volume, what is being dissolved
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electrolyte
substance that has an electric current
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unsaturated
still has left over space between particles
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saturated
all spaces are filled between particles
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supersaturated
more than the max amount of solute has been dissolved
41
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what are the restrictions for solutes and solvents being able to successfully mix
they both have to be polar or they both have to be nonpolar
42
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miscible
how mixable something is
43
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how do you dissolve a solid in a liquid
heat it, stir it, or increase the surface area(grind solid up)
44
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how do you dissolve a gas in a liquid
increase the pressure and cool it
45
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if 2 moles of a solute are dissolved in 1 liter of solutions what is the morality of the solution
2M
46
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molarity
moles/liters
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molality
moles/kilogram
48
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what are the colligative properties
vapor pressure, boiling point, osmotic pressure, and freezing point
49
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freezing point depression
the LOWERING of the freezing point of a liquid that occurs when substances are dissolved in the liquid
50
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what is an example of freezing point depression
salt on icy roads
51
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arrhenius base
releases hydroxide (OH-)
52
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arrhenius acid
releases hydrogen ions (H+)
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hydroxide ion
OH-
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neutralization
when you mix an acid and a base it makes salt and water
55
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in an acid does hydronium or hydroxide have a higher concentration
hydronium
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in a base does hydronium or hydroxide have a higher concentration
hydroxide
57
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in what substance is the concentration of hydronium and hydroxide equal
water
58
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what is the pH value of an acid
0-6
59
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what is the pH value of a base
8-14
60
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which end of the pH scale represents a strong acid
left
61
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which end of the pH scale represents a strong base
right
62
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indicator
a substance that changes color based on the pH of your solution, tells you the pH is of your solution
63
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titration
controlled addition and measurement of the amt of solution of known concentration required to react completely with a measured amt of another solution with an unknown concentration in order to find the unknown concentration
64
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specific heat
amount of energy required to raise one gram of a substance one degree celsius
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enthalpy change
heat content
66
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â–˛H
change in enthalpy(heat)
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endothermic
reactants gain energy (absorbing the heat)
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exothermic
reactants lose energy (releasing heat)
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how is enthalpy shown for an exothermic reaction
\-â–˛H
70
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how is enthalpy shown for an endothermic reaction
\+â–˛H
71
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the tendency in nature is for a reaction to _____ enthalpy
lose
72
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the tendency in nature for a reaction to _____ entropy
gain
73
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entropy
degree of randomness- amount of disorder
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reaction mechanism
the series of baby steps in a chemical reaction
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activation energy
little bit of energy you have to add to get a reaction started
76
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reaction rate
how long it takes for reaction to take place
77
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catalyst
**a substance that increases the rate of a chemical reaction without itself undergoing any chemical change to itself**
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forward reaction
when the equation looks like reactants → products
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reverse reaction
when the equation looks like reactants
80
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equillibrium
when the rate of the forward reaction equals the rate of the reverse reaction (also called dynamic equillibrium)
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equilibrium constant
Keq
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what does it mean when the Keq value is greater than 1
you will have more products because the forward reaction is favored
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what does it mean when the Keq value is less than 1
you will have more reactants because the reverse reaction is favored
84
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Le Chatelier’s Principle
when you have a system at equilibrium and stress is applied, the equilibrium shifts to release the stress
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what happens when you add a reactant
other reactant is used to make more products
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what happens when you remove a reactant
products are both used to make other reactant
87
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what happens when you add a product
other product is used to make more reactants
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what happens when you remove a product
reactants are used to make more of the other product
89
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hydrochloric acid
HCl
90
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Acetic acid
CH3COOH
91
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carbonic acid
H2CO3
92
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nitric acid
HNO3
93
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phosphoric
H3PO4
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sulfuric
H2SO4
95
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ammonia
NH3
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what is a compound that has hydrogen bonding
H2O(water)
97
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diffusion
scattering of particles from high to low