chemistry Flashcards
1
Q
definition of precise
A
all the answers are close together
2
Q
definition of accuracy
A
all the answers are near the targeted answer
3
Q
kelvin and celsius conversion
A
273.15 + Celsius measurement = Kelvin measurement
4
Q
adding one oxygen makes the name…
A
per____ate
5
Q
removing 1 oxygen makes the name…
A
_____ite
6
Q
removing 2 oxygens makes the name…
A
hypo____ite
7
Q
hydrogen carbonate
A
HCO3 (-1)
8
Q
hydrogen phosphate
A
HPO4 (-2)
9
Q
bisulfite or hydrogen sulfite
A
HSO3(-1)
10
Q
acetate
A
C2H3O2(-)
11
Q
chromate
A
CrO4(-2)
12
Q
peroxide
A
O2(-2)
13
Q
phosphate
A
PO4(-3)
14
Q
borate
A
BO3(3-)
15
Q
carbonate
A
CO3(2-)
16
Q
nitrate
A
NO3(-1)
17
Q
arsenate
A
AsO4(-3)
18
Q
sulfate
A
SO4(-2)
19
Q
selenate
A
SeO4(-2)
20
Q
chlorate
A
ClO3(-)
21
Q
bromate
A
BrO3(-1)
22
Q
iodate
A
IO3(-1)
23
Q
difference between the element, mixture, and compound
A
elements: pure substances made from one type of atom, and cannot be broken down by simple chemical means
mixture: 2+ substances that are mixed together, and ARE NOT chemically bonded
compound: 2+ elements that are mixed together and chemically bonded, and CANNOT be separated and when they are created, it makes a new type of matter
24
Q
difference between heat and temperature
A
heat is total energy of the particles in a substance, but temperature is the actual property that the substance exhibits and measures the energy of the motions of the particles
25
adding a hydrogen to "-ide" makes...
hydro_____ic acid
26
adding a hydrogen to "-ate" makes...
_______ic acid
27
adding a hydrogen to "-ite" makes...
_______ous acid
28
name/describe the states of matter triangle and their phases
solid to liquid = melting
liquid to solid = freezing
solid to gas = sublimation
gas to solid = deposition
liquid to gas = evaporation
gas to liquid = condensation
29
endothermic
absorbing heat
30
exothermic
releasing heat
31
evidences of chemical change
heat, light, color change, smell, bubbles, burning, precipitate (formation of a solid)
32
intensive property vs extensive property
intensive - depends on the identity of the matter (for example, color)
extensive - depends on amount of matter (for example, mass)
33
physical property
observation without changing matter type
34
chemical property
observation when matter changes
35
what are the fundamental chemical laws?(3)
1. law of conservation of mass - mass of reactants is equal to mass of products
2. law of definite proportions:
3. law of multiple proportions:
36
what is the law of conservation of energy?
energy cannot be created or destroyed, only transferred
37
name the properties of each: solid, liquid and gas
solid - volume doesn't expand, cannot be compressed, retain their shape, particles are held in fixed positions with high IMF
liquid- volume doesn't change, weaker forces of attraction / IMF, particles can flow and they take the shape of their container, and cannot be compressed
gas - have no IMF at all, their particles move quickly and freely, can be compressed, has a much greater volume than solids and liquids, and it takes the shape and volume of its container
38
kinetic energy vs potential energy
kinetic energy is the motion of particles
potential energy is the potential for particles to move
39
intermolecular forces vs. intramolecular forces
intermolecular -
intramolecular -
40
3 postulates of kinetic theory?
particles are in constant motion, 2 substances at the same temperature will have the same amount of kinetic energy, and the molecules are incompressible
41
pure substance
all particles are identical
42
what is the molar mass? where can you find it?
molar mass is the mass of one mole of the element on the periodic table, and the number is the one below each element
43
empirical vs. molecular formula
molecular can be reduced, empirical cannot.
44
what is avogadros number? when do you use this?
6.022 x 10^23
used when converting mass to moles to formula units/molecules/particles
45
what are the steps to find percent composition by mass?
46
what are the steps to find percent composition to empirical/molecular formula
47
what is the orders to convert with moles, particles and mass?
48
how to find the molecular formula using given empirical formula and molar mass?
49
cations vs anions
cations = positive charge
anions = negative charge
50
metals vs. nonmetals (which one gains e- and which loses e-?)
metals lose electrons
nonmetals gain electrons
51
what is the octet rule?
52
what are the metal physical properties?
53
what are isotopes?
isotopes are different types of elements, and they have the same atomic # with different molar masses and diff physical properties
54
what does it mean for a substance to be isoelectronic?
electron number is the same
55
what is a valence e-
of electrons in the highest level in that substance
56
what is electronegativity
particle's ability to attract e- from other atoms
57
what is atomic radius? what is the pattern on the periodic table?
atomic radius is the closeness of the electron and neutron
58
what are allotropes
different types of isotopes
59
what is ionization energy
energy needed to ionize a substance (going across it increases and going down it decreases)
60
what is coulumbic attraction?
attraction between oppositely charged particles
61
what Is the difference between mass # and atomic mass
mass # = protons + neutrons
atomic mass = # of protons
62
how to read a isotope symbol?
the top left is mass # and bottom left is atomic mass
63
what does it mean to be: saturated, unsaturated, and supersaturated?
saturated - the maximum amount of solute that can be dissolved has been reached
unsaturated - there is still more solute that is capable of being dissolved
supersaturated - solution has more dissolved solute than required for a saturated solution (imagine reaching the saturated point and then cooling the solution down)
64
what is solubility?
the measure of the maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature
65
what is the difference between miscible and immiscible?
miscible - fully mixed in all proportions
immiscible - mixing polar and non polar together, doesn't mix and separate instead
66
definition of dilute and its equation
low amount of solute - MV = MV
67
what does it mean to be concentrated
large amount of solute
68
diff between colloid and suspension
colloid - particles are large enough to be seen
suspension - larger particles that can settle out over time and aren't fully combined
69
what does "like dissolves like" mean
polar dissolves polar, non polar does not dissolve polar. molecules with similar interactions will dissolve best.
70
what is the difference between molality and molarity?
molality is moles/kg
molarity is moles/Liters
71
what is the solution equation?
solution = solute + solvent (all in grams)
72
what happens to solute when boiling point increases
they are directly related, so when boiling point increases, the solute increases
73
what happens to solute when freezing point increases
freezing point is inversely related, so the solute decreases
74
what is the difference in dissolved particles in ionic compounds compared to covalent ones?
ionic compounds break up the compounds, and covalent ones dont
75
name all the "drill" molecular geometry names and their angles
linear (180)
trigonal planar (120)
bent (120)
tetrahedron (109.5)
trigonal pyramid (107)
bent (105)
trigonal bipyramidal (90)
seesaw (90)
T shaped (90)
linear (180)
octahedral (90)
square pyramidal (90)
square planar (90)
76
polar bonds vs non polar bonds
polar bonds have partial charges and non polar charges dont
77
what are the different types of bonds (hydrogen bonds, dipole dipole, and dispersion) and describe them
hydrogen bonds - strongest bonds, intermolecular force (on the outside of the molecule), uses covalent bonds, only between Hydrogen with O, N or F
dipole dipole interactions - positive and negative charges in dipoles attract each other, only occurs in polar molecules
dispersion forces - all molecules have dispersion forces, the more e- there are, the stronger the dispersion force is.
78
what do the straight lines represent in the graph of temperature's relationship with time/heat (the graph with the AB CD DE EF stuff and phases)
they represent potential energy (BC = fusion) (DE = vaporization)
79
what is the difference between the Arrhenius and Bronsted Lowry acids and bases?
Arrhenius = acids have H+ and Oxygen and are all aqueous, and bases have OH
Bronsted Lowry = acids have H+ and bases have OH-
80
what are conjugate acid and base pairs
conjugate acids received ion and conjugate bases lose an ion
81
acids react with metals to create...
H2 (g) and chloride salt
82
acids react with carbonates/bicarbonates to form...
H2O and CO2
83
bases react with metal ion solutions to form...
H2 (g)
84
what are spectator ions?
spectator ions don't change across a reaction
85
what are acid base indicators
solutions that change colors to indicate the pH of a solution
86
what happens to the substance when they dissolve
they break apart
87
describe the types of ions in basic, acidic, and neutral solutions
basic = hydroxide
acid = Hydrogen
neutral = equal concentration of both
88
what is Le chatelier's principle
when a stress is placed on a system @ equilibrium, the system will shift in order to minimize stress
89
name the five ways to speed up chemical reactions
1) lowering the volume of the vessel
2) speeding up the particles
3) catalysts
4) individual particles instead of groups
5) more particles
90
fill in the blanks: during chemical changes, reactants___________ and products _______
decrease, increase
91
name all of the shifts associated with the following: reactants, products, temperature, volume
reactants - increase = right
decrease = left
products increase = left
decrease = right
temperature = whichever side its on will be what it acts as
volume = volume increases = pressure decrease = shifts to the side with more moles
volume decrease = pressure increase = shifts to side with less moles
92
what are the steps to write and balance half reactions? what are the steps to write and balance in acidic solutions? In basic solutions?
93
what is an antioxidant
94
anode vs cathode
anodes oxidized, lose e-
cathodes reduce and gain e-
95
how do you tell which element is the better oxidizing and reducing agent on the Ered paper?
96
what are the 6 rules of oxidation numbers?
Oxygen is
97
name which types of reactions are always, never, and sometimes redox reactions.
98
heat of fusion
99
surface tension
ability of a substance's surface to resist an outside force
100
viscosity
the substance's resistance to flow
101
boiling point
when the atm (atmospheric pressure) is equal to the vapor pressure
102
vapor pressure
103
name the type of solids and their characteristics
104
what are the rules of polar bonds and non polar bonds
no lone pairs - non polar
one lone pair - polar
two lone pair - polar
all diff - polar
105
stoichiometric mixture
the mixture is mixed in all proportions (balanced equation)
106
how do you read the activity series?
107
what are the difference between metal and nonmetal oxides? which one is basic and which one is acidic?
metal oxides are acidic because they result in H+
nonmetal oxides are basic because they result in OH
108
limiting reactant
reactant that runs out first
109
name all 7 diatomic elements
H, O, F, N,
110
what is precipitation and neutralization in double displacement reactions
111
describe how JJ Thompson discovered cathode rays
