1
Q
branch of science that deals with the study of the composition, structure, and properties of matter and the changes that matter undergoes
A
chemistry
2
Q
systematic study of God’s universe and how it works
A
science
3
Q
process used to investigate the secrets of nature
A
scientific method
4
Q
specific, empirical description of the way that some aspect of the universe consistently behaves
A
scientific law
5
Q
general explanation of why some part of the universe behaves the way it does
A
theory
6
Q
use of science for man’s benefit and to solve practical problems
A
technology
7
Q
measure of the consistency or reproducibility of a measurement
A
precision
8
Q
closeness of a measurement to the actual, exact value
A
accuracy
9
Q
one billionth, 10^-9
A
nano (n)
10
Q
one millionth, 10^-6
A
micro (µ)
11
Q
one thousandth, 10^-3
A
milli- (m)
12
Q
one hundredth, 10^-2
A
centi (c)
13
Q
one thousand, 10^3
A
kilo (k)
14
Q
one million, 10^6
A
mega (M)
15
Q
coldest possible temperature
A
absolute zero (0 K)
16
Q
energy of motion
A
kinetic energy
17
Q
most common state of matter in the universe
A
plasma
18
Q
developed the atomic theory of matter
A
Dalton
19
Q
negative subatomic particle
A
electron
20
Q
positively charged subatomic particle
A
proton
21
Q
center of an atom
A
nucleus
22
Q
uncharged particle found in an atom
A
neutron
23
Q
designed the planetary model of the atom
A
Rutherford
24
Q
any of several forms of an element that have different mass numbers
A
isotopes
25
the ________ determines the atomic number of an atom, so its identity
number of protons
26
______ measure atomic mass
atomic mass units
27
compound composed of a vast array of ions
ionic compound
28
simplest ratio of atoms in an ionic compound
formula unit
29
prefixes, numbers 1-10
1 = mono
2 = di
3 = tri
4 = tetra
5 = penta
6 = hexa
7 = hepta
8 = octa
9 = nona
10 = deca
30
compounds that are between metals and nonmetals
ionic compounds
31
prefixes are used in ______ compounds
molecular
32
Avogadro's number
6.022 x 10^23
33
Avogadro's number of anything
mole (mol)
34
______ are on the left side of a chemical equation
reactants
35
______ are on the right side of a chemical equation
products
36
A + B -> AB
combination reaction
37
AB -> A + B
decomposition reaction
38
A + BC -> B + AC
single-displacement reaction
39
AB + CD -> AD + CB
double-displacement reaction
40
amount of Torr in 1 atm
760 Torr
41
if pressure is increased by 8 and temperature is constant, then what happens to volume?
volume is divided by 8 (P1V1/T1 = P2V2/T2)
42
temperature must be measured in _____ for the gas laws
Kelvin
43
STP means _______
standard temperature and pressure
44
STP conditions examples
0 C and 1 atm
273.15 K and 100 kPa
45
process of mixing molecules of one substance through another by random molecular motion
diffusion
46
ability to do work and change matter
energy
47
energy of motion
kinetic energy
48
energy associated with the position of an object and the forces acting upon it
potential energy
49
the portion of the universe or the sample of matter being studied
system
50
everything in the universe outside the system
surroundings
51
increases in internal energy mean ΔE is _______ (positive or negative)
positive
52
decreases in internal energy mean ΔE is _______ (positive or negative)
negative
53
SI unit of energy and energy transfer
Joule
54
if heat is a product, the reaction is ________
exothermic (ΔH is negative)
55
if heat is a reactant, the reaction is _______
endothermic (ΔH is positive)
56
enthalpy of formation of an element in its standard state
0
57
heat flows from ____ to ____
hotter to colder
58
specific heat of water
4.18 J/g (degrees C)
59
temperature at which a liquid’s vapor pressure equals the total pressure of all gases present
boiling point
60
combination of temperature and pressure at which all three phases of a substance are in equilibrium
triple point
61
reaction that is able to occur without continuing outside help
spontaneous reaction
62
law stating that the entropy of the universe is always increasing
second law of thermodynamics
63
practical restatement of the law of conservation of energy
first law of thermodynamics
64
periodic back-and-forth motion that transmits energy
wave
65
high point of a wave
crest
66
low point of a wave
trough
67
developed the particle theory of light
Sir Isaac Newton
68
speed of light
3.00 x 10^8 m/s
69
tiny bundles or “packets” of energy that light consists of
photons
70
theory that describes light as having both a wave and particle nature
quantum theory of light
71
lowest energy state of an atom
ground state
72
described atoms as having different energy states
Bohr
73
principle stating that it is impossible to simultaneously determine the momentum and the position of an electron with certainty
(Heisenberg) uncertainty principle
74
regions of space through which an electron moves with probabilities determined using the Schrodinger equation
orbitals
75
number of electrons in each subshell (s, p, d, f)
s = 2
p = 6
d = 10
f = 14
76
when a p, d, or f subshell is being filled, one electron will occupy each orbital in that subshell before pairing begins
Hund's rule
77
outermost electrons, used for bonding
valence electrons
78
states that the physical and chemical properties of the elements are periodic functions of their atomic numbers
periodic law
79
developed the periodic table of the elements
Mendeleev
80
column of the periodic table
group
81
row of the periodic table
period
82
any elements in group 1, 2, or 13-18 of the periodic table
main-group elements
83
principle stating that no two electrons in an atom may have the same set of four quantum numbers
Pauli exclusion principle
84
any elements in groups 3-12 of the periodic table
transition metals
85
number of valence electrons in transition and inner transition metals
2
86
number of valence electrons in main-group elements is determined by _______
the ones place
87
is C^2+ or C larger?
C, because cations (+) are smaller than the normal element
88
is N or N^- larger?
N^- because the anion (-) is larger than the normal element
89
energy required to remove an electron from an atom
ionization energy
90
trend with largest at the bottom left, smallest at top right
atomic radius, metallic character
91
ability of a chemically combined atom to attract electrons to itself
electronegativity
92
largest at top right, smallest at bottom left
electronegativity (doesn't count noble gases), electron affinity, ionization energy
93
says that atoms tend to react in a way that gives them a noble-gas electron configuration
octet rule
94
most atoms try to have this many electrons
8
95
chemical bond that results from the sharing of valence electrons between atoms
covalent bond
96
bonding situation in which electrons are shared by more than two atoms
delocalization
97
electrons that circulate freely throughout a molecule or crystal instead of being bound to a single atom or a pair of atoms
delocalized electrons
98
covalent bond in which electrons are shared unequally between atoms
polar
99
know prefixes, numbers, trends, balancing
study previous quiz flashcards for newest stuff because I don't want to add them
11th Chemistry
flashcards
Decks in class (27)
# Cards
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pages 1-10 quiz35
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11-1636
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test 195
-
mas info90
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40-5023
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ch 415
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test 246
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5.1-5.228
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test 3126
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6.1-236
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test 465
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7.1-255
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7.3-8.229
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9.1-9.237
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MIDTERM99
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9.322
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10.1-10.245
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10.2 - continued42
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test 7105
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11.320
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11.2-350
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12.1-229
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test 8110
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12.4-13.140
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test 9119
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test 1032
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strong acids and bases4
