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CHEM 10.01 > Long Test #1 > Flashcards

Long Test #1 Flashcards

(86 cards)

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1
Q

systemic study of everything

A

science

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2
Q

everchanging pool of knowledge

A

science

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3
Q

method of conducting scientific experiments

A

scientific method

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4
Q

educated guess that can be accepted or rejected

A

hypothesis

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5
Q

physical representation of scientific phenomena

A

models

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6
Q

statement generated from multiple observations that explain scientific phenomena

A

laws

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7
Q

tentative explanations to scientific phenomena

A

theories

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8
Q

uses models/theories/laws and relates them to hypothesis

A

data analysis

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9
Q

sciences that deal with the physical world

A

hard sciences

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10
Q

sciences that deal with intangible aspects of nature

A

soft sciences

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11
Q

studies that are inherently true but have no basis in scientific principles

A

pseudoscience

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12
Q

studies that are biased and flawed

A

bad science

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13
Q

science interpreted in lay terms for a general audience

A

pop science

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14
Q

the science of matter

A

chemistry

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15
Q

state with definite volume and shape

A

solid

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16
Q

state with definite volume, indefinite shape

A

liquid

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17
Q

state with indefinite volume and shape

A

gas

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18
Q

distinct form in state of matter; separation in relation to state

A

phase

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19
Q

refers to particle distance of matter

A

state

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20
Q

most basic form of matter, can be found in the periodic table

A

elements

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21
Q

fixed ratio of 2+ elements

A

compounds

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22
Q

combination of substances with a uniform appearance, cannot be separated

A

homogenous mixture

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23
Q

combination of substances with an inconsistent appearance, can be separated

A

heterogenous mixture

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24
Q

properties that don’t change the composition of matter

A

physical

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25
reactions that change composition
chemical
26
unit standard that we use to measure today
International System of Units (SI Units)
27
how close a measurement is to the true value
accuracy
28
how close a measurement is to other data points
precision
29
measurement with some degree of error
uncertainty
30
alternative method of expressing big/small numbers
scientific notation
31
digits that give information on the precision of a unit
significant figures
32
smallest unit of mass
atoms
33
when two elements form a series of compounds, the ratios of the 2nd elements that combine with the first element can be reduced to small whole numbers
law of multiple proportions
34
a specific compound will always contain the exact same ratio (proportion) of elements by mass
law of definite proportions
35
matter cannot be created nor destroyed
law of conservation of mass
36
subatomic particle with a negative charge
electrons
37
subatomic particle with a positive charge
protons
38
subatomic particle with a neutral charge
neutrons
39
the number of protons
atomic number
40
the number of protons and neutrons
atomic mass
41
number of protons minus the number of electrons
charge
42
atoms of an element with a different MASS
isotopes
43
atoms of an element with a different CHARGE
ions
44
ion with more protons
cation
45
ion with more electrons
anion
46
atoms as solid spheres; based on the Ancient Greek notion that atoms are indivisible
Dalton Model
47
plum pudding model; there are smaller particles (electrons) surrounded in a positively charged cloud of space (cathode ray particles)
Thomson Model
48
gold foil experiment suggests that most of the atom is empty space, addition of the nucleus surrounded by electrons in the model
Rutherford Model
49
planetary model; electrons move around nucleus in orbits of fixed sizes, theory of quantized energy (line specrta of hydrogen gas)
Bohr Model
50
electrons don’t move in set paths, but in WAVES, only orbitals can dictate possible locations of an electron (wave-particle duality)
Schrödinger Model
51
organization of the 118 elements
periodic table
52
triadic relationship according to atomic mass
Law of Triads
53
theory that every 8th element has similar properties
law of octaves
54
father of the periodic table
Dmitri Mendeleev
55
underrated periodic table maker
Lothar Meyer
56
columns in a periodic table
groups
57
rows in the periodic table
periods
58
group 1 metals; extremely reactive
alkali metals
59
group 2 metals; reactive but not as much as grp 1
alkaline earth metals
60
top row of the separated elements in the table
lanthanides
61
bottom row of the separated elements in the table
actinides
62
groups 3-12 in the main table
transition metals
63
group 17; chemically reactive nonmetals
halogens
64
last group of stable, nonreactive elements
noble gases
65
good conductors of heat and electricity
metals
66
poor conductors of heat and electricity
nonmetals
67
elements with a mix of metallic and nonmetallic properties
metalloids
68
distance between the nucleus and the farthest electron
atomic radius
69
energy needed to attract an electron
ionization energy
70
tendency to attract electrons
electronegativity
71
state where the atom is at the lowest energy level
ground state
72
when an atom is above ground state
excited state
73
2 electrons
s shell
74
6 electrons
p shell
75
10 electrons
d shell
76
14 electrons
f shell
77
principle that states that electrons fill orbitals with the lowest energy level first
Aufbau Principle
78
outermost shell number (n)
principal quantum number
79
shape of orbital (l)
angular momentum quantum number
80
number of orbitals within a subshell (Ml)
magnetic quantum numbers
81
direction of electron spin
spin quantum number
82
electrons that are in the outermost shell
valence electrons
83
atoms that don’t bond :(
core electrons
84
bonding between a metal and a nonmetal
ionic bonding
85
bonding between nonmetals
covalent bonds
86
sharing of valence electrons amongst positively charged metals
metallic bonding

CHEM 10.01 (4 decks)

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