midterm Flashcards
1
Q
extensive property
A
property that depends on the AMOUNT of matter in a sample
2
Q
intensive property
A
a property that depends on the TYPE of matter in a sample, not the amount
3
Q
intensive property example
A
magnetism, thermal conductivity, electrical conductivity, color, melleability, ductility, condensation, luster, state at room temp., density
4
Q
physical property
A
quality or condition of a substance that can be observed or measured without changing the substances composition
5
Q
gas to liquid
A
condensation
6
Q
liquid to solid
A
freezing
7
Q
gas to solid
A
deposition
8
Q
liquid to gas
A
boiling
9
Q
solid to liquid
A
melting
10
Q
solid to gas
A
sublimation
11
Q
solid
A
a form of matter that has a definite shame and volume. the shape of a solid doesnt depend on the shape of its container
12
Q
particles of a solid
A
packed tightly together often in an orderly arrangement
13
Q
liquid
A
form of matter that has indefinite shape, flows, yet has a fixed volume. liquids volume doesnt change but it takes shape of the container it is in
14
Q
particles of a liquid
A
close together but are free to flow past one another
15
Q
gas
A
a form of matter that takes both shape and volume of its container
16
Q
particles of a gas
A
relatively far apart and can move freely
17
Q
vapor
A
the gaseous state of a substance that is generally a liquid or solid at room temperature
18
Q
endothermic processes include:
A
Fusion, vaporization, and sublimation
19
Q
exothermic processes include:
A
freezing, condensation, and deposition
20
Q
endothermic
A
a process that requires the absorption of heat
21
Q
exothermic
A
a process that requires the releasing of heat
22
Q
increasing the pressure on gas changes the state to a …
A
liquid
23
Q
increasing the pressure on a liquid changes the state to a….
A
solid
24
Q
mixture
A
a physical blend of two or more components
25
heterogenous mixture
a mixture in which the composition is not uniform throughout
26
homogenous mixture
a mixture in which the composition if uniform throughout
27
solution
another name for a homogenous mixture
28
phase
any part of a sample with uniform composition and properties
29
filtration
the process that separates a solid from a liquid in a heterogenous mixture
30
distillation
a process that separates water from other components in tap water
31
element
simplest form of matter that has a unique set of properties ( only one type of atom)
32
compound
a substance that contains two or more elements chemically combined in a fixed proportion
33
can compounds be broken down into simpler substances by chemical means?
yes
34
can elements be broken down into simpler substances by chemical means?
no
35
chemical change
a change that produces matter with a different composition than the original matter
36
chemical property
the ability of a substance to undergo a specific chemical change
37
chemical reaction
when the composition of matter changes
38
possible clues to chemical change include:
transfer in energy, color change, gas production, precipitate
39
precipitate
a solid that forms and settles out of a liquid mixture
40
law of conservation of mass
in any physical change or chemical reaction, mass is conserved. mass is neither created nor destroyed
41
alloy
homogeneous mixture of metals
42
kilo (k)
10^3
43
centi (c)
10^-2
44
milli (m)
10^-3
45
micro (u)
10^-6
46
nano (n)
10^-9
47
1kg =
2.2 lbs
48
1 inch =
2. 54 cm
49
1 ML =
1 cm^3
50
for multiplying and diving sig figs:
round answer to match value with the lowest number of sig figs
51
for adding and subtracting sig figs:
round answer to match value with lowest number of decimal places
52
accepted value
what I SHOULD get for my result
53
experimental value
what I ACTUALLY get
54
error =
what you got - what you should get
55
% error formula
|error| / accepted value x 100%
56
accuracy
how close you are to hitting the target value
57
precision
how repeatable your results are
58
0 degrees C =
273 Kelvins
59
daltons atomic theory
all elements are composed of tiny indivisible particles called atoms, atoms of the same element are identical and the atoms of any one elements are different from those of any other element, atoms of different elements can physically mix together or can chemically combine in simple whole number ratios to form compounds, chemical reactions occur when atoms are separated from each other, joined, or rearranged in a different combination and atoms of one element are never changed into atoms of another element as a result of a chemical reaction
60
JJ thomson
discovered the electron using an electric current through gases at a low pressure which resulted in a cathode ray
61
cathode ray
a glowing beam that showed how elections exist
62
plum pudding model
an atomic model discovered by JJ Thomson, where electrons were stuck into a lump of positive charges and the model was proven wrong by Thomas Rutherford
63
Thomas Rutherford
he tested the plum pudding model by using a gold foil alpha particle experiment and his experimented resulted in the founding of the nucleus in an atom
64
atomic number
number of protons in an atom
65
mass number
number of protons and the number of neutrons in an atom
66
electron symbol, charge, relative mass
e- , 1-, 1/1840
67
proton symbol, charge, relative mass
p+, 1+, 1
68
neutron symbol, charge, relative mass
n0, 0, 1
69
where are protons and neutrons located in an atom?
nucleus
70
where are electrons located in an atom?
outside the nucleus
71
average atomic mass
weighted average of the masses of the different isotopes for an element according to their proportions in nature
72
isotopes
atoms of the same element (with the same amount of protons) with different numbers of neutrons or different masses
73
anion
negatively charged atom, caused when an atom GAINS electrons
74
cation
positively charged atom, caused when an atom LOSES electrons
75
radioisotopes
isotopes of an atom with unstable (radioactive) nuclei
76
stable isotopes
atoms that DO NOT release protons, neutrons, particles, or energy from the nucleus and ARE NOT radio active
77
unstable isotopes
atoms that spontaneously release protons, neutrons, particles or energy from the nucleus
78
alpha radiation
least dangerous radiation, least penetrating (paper can block)
79
beta radiation
middle dangerous (dense wood can block)
80
gamma radiation
most dangerous and most penetrating (walls of lead/concrete can block)
81
alpha radiation symbol, charge, mass #, and identity
4He2, +2, 4, helium nucleus
82
beta radiation symbol, charge, mass #, and identity
0e-1, -1, 0, electron
83
gamma radiation symbol, charge, mass #, and identity
0Y0, 0, 0, photon of light
84
half life
the time it takes for 1/2 of a sample to decompose. it Is a constant value of time for that specific isotope, and it is NOT affected by any environmental conditions life temperature, pressure, or humidity
85
fission
the splitting of a nucleus into smaller fragments, accompanied by the release of neutrons and a large amount of energy
86
fusion
the process of combining nuclei to produce a nucleus of greater mass
87
frequency
the number of wave cycles that pass a point in a unit of time (unit: hz)
88
wavelength
the distance from a point on one wave to the equivalent point on the next wave (unit: m)
89
energy is ___ proportional to frequency
directly
90
wavelength and frequency are ____ proportional
inversely
91
energy is ____ proportional to wavelength
inversely
92
e- can go from a lower to a higher level by _____ energy
absorbing
93
e- can go from a higher to a lower level by ____ energy
releasing
94
quantum
specific amount of energy between energy levels
95
quantum leap/electron transition
electronic transition (e- moving between energy levels)
96
ground state
the lowest possible energy level an electron can be at
97
excited state
an energy level higher than the ground state
98
orbitals
defined regions around the nucleus where e- are likely to be found
99
Aufbau principle
e- fill into orbitals from lowest to highest energy
100
Hunds Rule
e- will fill equal energy orbitals individually before they will pair up
101
Pauli exclusion
2e- in the same orbital must spin opposite of each other and no 2e- can have the same main level, sub level, orbital, and spin
102
column =
group and tells you the number of valence electrons
103
row =
period and tells you the outermost principle energy level containing electrons
104
metals are:
good conductors of heat and electriccurent, have high luster/sheen, solids at room temp, and most are malleable
105
nonmetals are;
not good conductors of heat or electricity (except fro carbon) and generally have properties opposite of metals
106
group 1:
alkali metals
107
group 2:
alkaline earth metals
108
group 17:
hallogens
109
group 18:
noble gases
110
entire d block:
transition metals
111
entire f block:
inner transition metals
112
representative elements:
form many different chemical compounds and are the entire s & p block elements
113
Mendeleevs original table was organized by:
atomic mass and chemical properties
114
elements in same groups have:
similar chemical properties
115
metals are located at
the bottom left of the PT
116
nonmetals are located at
upper right corner of the PT
117
metalloids are located at
border the heavy "stair step" line diving metals from nonmetals
118
atomic radius
half the distance between the nuclei of two atoms of the same element bonded together
119
atomic radius ___ going down a group
increases, because a principle energy level is added with each step
120
atomic radius ____ going across a period
decreases, because the combination of more protons in a nucleus and more electrons in valence level cinches atom in
121
cations are ____ in radius than their neutral atom
smaller
122
anions are ____ in radius than their neutral atom
bigger
123
ionization energy
the amount of energy required to remove the first outermost electron from an energy
124
ionization energy ____ going down a group
decreases, because the outermost electrons are further away from the nucleus
125
ionization energy ____ going across a period
increases because the greater attractive pull on valence electrons because more protons are added to the nucleus
126
Coulombs law
attractive force is directly proportional to an amount of a charge and inversely proportional to the distance between charge
127
force is ___ proportional to magnitude of charge
directly
128
force is ____ proportional to the distance between charges
inversely
129
electronegativity
attraction that an atom has for ANOTHER atoms electrons (same direction of trend as IE)
130
____ is the most electronegative atom
fluorine
131
noble gases ____ have a defined electronegativity
DONT because they aren't reactive so they don't form bonds so they don't need electrons
132
the higher the IE the ____ the electronegativity
higher
